Ch.9 - Bonding & Molecular StructureWorksheetSee all chapters
All Chapters
Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
Ch.7 - Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
Ch.9 - Bonding & Molecular Structure
Ch.10 - Molecular Shapes & Valence Bond Theory
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch. 17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds
Sections
Chemical Bonds
Lattice Energy
Lattice Energy Application
Born Haber Cycle
Dipole Moment
Lewis Dot Structure
Octet Rule
Formal Charge
Resonance Structures
Additional Practice
Bond Energy
Jules Bruno

A Lewis Dot structure, named after Gilbert N. Lewis, is the structural representation of a molecule that involves the use of valence electrons by the involved atoms in the creation of covalent bonds. 

Lewis Dot Diagrams 

Before we can start drawing Lewis electron dot structures we have to figure out how to depict the valence electrons of individual atoms. 

Lewis-Dot-Diagrams-C-N-O-F-Gilbert-N-LewisLewis Dot Diagrams (C, N, O, F)

From these Lewis electron-dot symbols, the element symbol represents the nucleus and inner electrons, and the surrounding dots represent the valence electrons. 

Basics of Lewis Dot Diagrams

It’s easy to write the Lewis symbol for any Main-Group element and since Lewis dot structures involve non-metals we won’t have to worry about transition metals. 

1) Remember that Group Number equals Valence Electron Number. 

2) Place one dot at a time on the four sides starting from the top of the element and moving clockwise. 

3) Keep adding dots, pairing them up until you have reached the number of total valence electrons for that element. 

PRACTICE 1: Determine the electron dot diagram for the following atom. 

Phosphorus (P)

STEP 1: Find the group number for the phosphorus atom and begin to fill in its valence electrons. 

Since phosphorus is in Group 5A it will have 5 valence electrons. 

Lewis-Dot-Digram-PhosphorusLewis Dot Diagram (Phosphorus)

PRACTICE 2: Determine the electron dot diagram for the following ion. 

Calcium ion (Ca2+

STEP 1: When it comes to finding the electron dot diagram of an ion you should first find it for its neutral form. 

Since the calcium atom is in Group 2A it will have 2 valence electrons. 

Lewis-Dot-Diagram-CalciumLewis Dot Diagram (Calcium)

STEP 2: Find the electron dot diagram of the cation. The 2+ charge means calcium has lost 2 valence electrons. For ions we place the element in brackets and its charge on the top right. 

Lewis-Dot-Diagram-Calcium-IonLewis Dot Diagram (Calcium Ion)

PRACTICE 3: Determine the electron dot diagram for the following ion. 

Oxide ion (O2–

STEP 1: Like we did before we again find the electron dot diagram of the neutral atom. 

Since the oxygen atom is in Group 6A it will have 6 valence electrons. 

Lewis-Dot-Diagram-OxygenLewis Dot Diagram (Oxygen)

STEP 2: Find the electron dot diagram of the anion. Again place the charge on the top right corner and brackets around the ion. The 2– charge means calcium has gained 2 valence electrons

Lewis-Dot-Diagram-Oxide-IonLewis Dot Diagram (Oxide Ion)

Drawing Lewis Dot Structures 

Lewis Dot Structures are important within chemistry because not only do they provide the structural representation of a compound, but also help to explain the reactivity, polarity and overall stability of compounds. 

When it comes to drawing lewis dot structures just follow these provided steps: 

Rule 1: When drawing the structure the least electronegative element goes in the center. Recall that electronegativity increases going from left to right across a period and going from bottom to top of any group. 

Periodic-Trend-ElectronegativityPeriodic Trend (Electronegativity)

Hydrogen and Flourine never go in the center and they only make single bonds

Rule 2: The number of valence electrons an element has is equal to its group number. 

Group-Number-Valence-Electrons-vsepr-basicsGroup Number & Valence Electrons

Rule 3: Carbon is in Group 4A, has 4 valence electrons, and must make 4 bonds. It can accomplish this through a combination of single bonds, double bonds or triple bond. 

Bonding-Patterns-Carbon-double-bonds-triple-bonds-single-bonds-sigma-bonds-pi-bonds-bond-length-bond-strengthCarbon Bonding Patterns

In rare occasions carbon can make 3 bonds when it is positively or negatively charged. 

Bonding-Patterns-Carbon-RareRare Carbon Bonding Patterns

Rule 4: Nitrogen is located in Group 5A and has 5 valence electrons. Since it is 3 spaces away from being a noble gas on the periodic table then it ideally wants to make 3 bonds. 

Bonding-Patterns-NitrogenNitrogen Bonding Patterns

Nitrogen can also create 2 or 4 bonds if necessary. 

Bonding-Patterns-Nitrogen-RareRare Nitrogen Bonding Patterns

Nitrogen tends to create only 2 bonds when it gains an electron and 4 bonds when it loses an electron. Also the addition of an electron gives nitrogen a negative charge, while the loss of an electron gives it a positive charge. 

Rule 5: Oxygen is located in Group 6A and has 6 valence electrons. Since it is 2 spaces away from being a noble gas on the periodic table then it ideally wants to make 2 bonds. 

Bonding-Patterns-OxygenOxygen Bonding Patterns

Oxygen can also create 1 or 3 bonds if necessary. 

Bonding-Patterns-Oxygen-RareRare Oxygen Bonding Patterns

Oxygen tends to create a single bond when it gains an electron and 3 bonds when it loses an electron. Also the addition of an electron gives oxygen a negative charge, while the loss of an electron gives it a positive charge. 

Rule 6: When halogens, the elements in Group 7A, are surrounding elements they only make single bonds. 

Bonding-Patterns-Halogens-LEDS-bf3-brf3-bcl3-brf5-bef2-becl2-bh3-br2Halogen Bonding Patterns

Expanded Valence Shell Theory 

Based on this theory, nonmetals starting from Period 3 and lower can have more than eight electrons around them when they are the central element. They accomplish these expanded octets by using the d-orbitals within their third shell. 

Expanded-Octet-nonmetalsExpanded Octets (Nonmetals)

Two examples of these expanded octets  can be seen with the bonding patterns of sulfur (S) and arsenic (As). 

Bonding-Patterns-S-AsBonding Patterns (S, As)

Formal Charge 

Whenever we draw a Lewis Dot Structure we can use the formal charge formula to check to see if you drew our compound correctly. 

Basics of Formal Charge

  1. The only allowable formal charges for an element can be either -1, 0, +1
  2. If you add up all the formula charges in your compound that will equal the overall charge of the compound.

Formal Charge = Group Number – (Bonds of Element + Nonbonding electrons of Element)

Formal-Charge-ThiocyanateFormal Charge (Thiocyanate Ion)

Lewis Structures Practice

With the rules for drawing Lewis dot structures under our belts, it’s time to start drawing. 

PRACTICE 1: Draw the following Lewis dot structure for CH­2Cl2

STEP 1: Determine the group number and from it the number of valence electrons for each element. 

Lewis-Dot-Diagrams-C-H-ClLewis Dot Diagrams (C, H, Cl)

STEP 2: Place the least electronegative element as the central element and remember that hydrogen can never go in the center. Lewis-Dot-Diagrams-CLewis Dot Digram (Carbon)

STEP 3: Start adding the surrounding elements to your central element. Hydrogen can only make single bonds because it has only 1 valence electron. 

Carbon & Hydrogen Bonding (CH2)

STEP 4: Halogens, like chlorine, only make single bonds when they are not a central element. 

Lewis Dot Structure (CH2Cl2)

PRACTICE 2: Draw the following Lewis dot structure for C3H8.

STEP 1: Draw the Lewis dot diagrams for the elements involved. 

Lewis-Dot-Diagrams-C-HLewis Dot Diagrams (C, H)

STEP 2: Place the least electronegative element as the central element (hydrogen is an exception). 

Central-CarbonsCentral Carbon Atoms

STEP 3: Add the surrounding hydrogens to the carbon atoms. Keep in mind that carbon atoms want to make 4 bonds and hydrogen atoms want to make 1 bond. 

Lewis-Dot-Structure-C3H8Lewis Dot Structure (C3H8)

PRACTICE 3: Draw the following Lewis dot structure for CH3SH.

Drawing more complex Lewis dot structures can sometimes be a situation of trial and error in terms of drawing them.

STEP 1: Draw the Lewis dot diagrams for the elements involved. 

Lewis-Dot-Diagrams-C-H-SLewis Dot Diagrams (C, H, S)

STEP 2: Place the least electronegative element as the central element. 

Lewis-Dot-Diagrams-Carbon-CentralCentral Element (Carbon)

STEP 3: Add the 3 hydrogen atoms around the carbon atom. 

Lewis-Dot-Structure-Ch3Carbon & Hydrogen Bonding (CH3)

STEP 4: Since carbon wants to make 4 bonds, attach the sulfur atom to the carbon atom by a single bond. 

Carbon, Hydrogen, Sulfur Bonding (CH3S)

STEP 4: Single bond the hydrogen atom to the sulfur atom to complete the Lewis dot structure. 

Lewis-Dot-Structure-CH3SHLewis Dot Structure (CH3SH)

PRACTICE 4: Draw the following Lewis dot structure for CH2O.

STEP 1: Draw the Lewis dot diagrams for the elements involved. 

Lewis-Dot-Diagrams-c-h-oLewis Dot Diagrams (C, H, O)

STEP 2: Place the least electronegative element as the central element. 

Lewis-Dot-Diagrams-Central-carbonLewis Dot Diagram (Central Carbon)

STEP 3: Add the 2 hydrogen atoms around the carbon atom. 

Carbon & Hydrogen Bonding (CH2)

STEP 4: Since carbon wants to make 4 bonds, it would have to form a double bond with the oxygen atom. 

Lewis-Dot-Structure-CH2O-lone-pair-shapes-polarity-atoms-molecule-valence-electrons-elecrtons-skeleton-trial-and-errorLewis Dot Structure (CH2O)

More than just Shapes

Learning how to draw Lewis dot structures and polyatomic ions will be essential in understanding several related concepts such as resonance structuresmolecular geometry, electronic geometryhybridization, polarity, and the intermolecular forces


Jules Bruno

Jules felt a void in his life after his English degree from Duke, so he started tutoring in 2007 and got a B.S. in Chemistry from FIU. He’s exceptionally skilled at making concepts dead simple and helping students in covalent bonds of knowledge.


Additional Problems
Write Lewis dot structures for the following molecule (note: you must indicate the total number of valence electrons in the molecule and show all bonding pairs and lone pairs in the structure).  AsCl3                      
Chemists use Lewis dot structures primarily to help visualize: (A) protons in ionically bonded compounds (B) protons in covalently bonded compounds (C) electrons in ionically bonded compounds (D) electrons in covalently bonded compounds (E) pretty pictures
How many dots should be included in the Lewis structure of SeCl  42+? (A) 32 (B) 34 (C) 36 (D) 100 (E) 102
How many valence electrons would be drawn in the Lewis structure of SiCl 4? (A) 32 (B) 82 (C) 5 (D) 160 (E) 28
Which of the following is the correct Lewis structure for CS 2?
In the nitrite ion, how many total valence electrons are used for all three atoms? HINT: nitrite ion, not nitrate ion. a. 16 valence electrons are used b. 26 valence electrons are used c. 18 valence electrons are used d. 25 valence electrons are used e. 17 valence electrons are used
How many valence electrons are represented in the Lewis electron-dot structure for SO2? a) 6 b) 8 c) 18 d) 32
In the Lewis structure for ICI2-,how many lone pairs of electrons are on the central iodine atom.
Choose the best Lewis structure for ICI5.
Draw the best dot structure you can for HNNH, where the atoms are connected as written. 
Write the Lewis Dot structures for the following molecule (note: the first atom is the central atom).  Be sure to give the total number of valence electrons and show all bonding and lone pair electrons.  CH2Cl2                        
How many "dots" would be drawn in the Lewis structure of KrF 22+? (A) 14 (B) 12 (C) 20 (D) 22 (E) 24
Which of the following is the correct Lewis formula for formaldehyde (CH  2O)?
The Ti2+ ion is isoelectronic with the Ca atom.Calculate the number of unpaired electrons for Ti2+.
You may want to reference (Pages 315 - 319)Section 8.5 while completing this problem.How many nonbonding electron pairs are there in the Lewis structure of the peroxide ion, O22-?
You may want to reference (Pages 322 - 325)Section 8.7 while completing this problem.In which of these molecules or ions is there only one lone pair of electrons on the central sulfur atom?
A common form of elemental phosphorus is the tetrahedral P4 molecule, where all four phosphorus atoms are equivalent: . At room temperature phosphorus is a solid.Are there any lone pairs of electrons in the P4 molecule?
Ortho-dichlorobenzene, C6H4Cl2, is obtained when two of the adjacent hydrogen atoms in benzene are replaced with Cl atoms. A skeleton of the molecule is shown here. Complete a Lewis structure for the molecule using bonds and electron pairs as needed.
A carbene is a compound that has a carbon bonded to two atoms and a lone pair remaining on the carbon. Many carbenes are very reactive.Draw the Lewis structure for the simplest carbene, H2C.
The Ti2+ ion is isoelectronic with the Ca atom.Calculate the number of unpaired electrons for Ca.
The molecule shown below is called furan. It is represented in typical shorthand way for organic molecules, with hydrogen atoms not shown. How many valence electrons are there in the molecule?
You may want to reference (Pages 387 - 387) Section 9.3 while completing this problem.Identify which electrons from the electron configuration are included in the Lewis symbol.
Consider the Lewis structure shown below. How many electrons are in the pi system of the species?
You may want to reference (Pages 300 - 301) Section 8.1 while completing this problem.True or false: An element’s number of valence electrons is the same as its atomic number.
You may want to reference (Pages 300 - 301) Section 8.1 while completing this problem.How many valence electrons does a nitrogen atom possess?
Consider the element silicon, Si. You may want to reference (Pages 300 - 301) Section 8.1 while completing this problem.Which subshells hold the valence electrons?
Consider the element silicon, Si. You may want to reference (Pages 300 - 301) Section 8.1 while completing this problem.How many valence electrons does a silicon atom have?
Propylene, C3 H6, is a gas that is used to form the important polymer called polypropylene. Its Lewis structure is shown in the diagram. the figure What is the total number of valence electrons in the propylene molecule?
Propylene, C3 H6, is a gas that is used to form the important polymer called polypropylene. Its Lewis structure is shown in the diagram. the figure How many valence electrons remain in nonbonding pairs in the molecule?
Ethyl acetate, C4H8O2, is a fragrant substance used both as a solvent and as an aroma enhancer. Its Lewis structure is . You may want to reference (Pages 362 - 368) Section 9.6 while completing this problem.What is the total number of valence electrons in ethyl acetate?
Ethyl acetate, C4H8O2, is a fragrant substance used both as a solvent and as an aroma enhancer. Its Lewis structure is . You may want to reference (Pages 362 - 368) Section 9.6 while completing this problem.How many valence electrons remain in nonbonding pairs in the molecule?
How do you determine the number of electrons in the Lewis structure of a molecule?
How do you determine the number of electrons in the Lewis structure of a polyatomic ion?
Which electrons from the electron configuration are included in the Lewis structure.
Using Lewis symbols and Lewis structures, diagram the formation of SiCl4 from Si and Cl atoms, showing valence-shell electrons.How many valence electrons does Si have initially?
Using Lewis symbols and Lewis structures, diagram the formation of SiCl4 from Si and Cl atoms, showing valence-shell electrons.How many valence electrons does each Cl have initially?
Using Lewis symbols and Lewis structures, diagram the formation of SiCl4 from Si and Cl atoms, showing valence-shell electrons.How many valence electrons surround the Si in the SiCl4 molecule?
Using Lewis symbols and Lewis structures, diagram the formation of SiCl4 from Si and Cl atoms, showing valence-shell electrons.How many valence electrons surround each Cl in the SiCl4 molecule?
Use Lewis symbols and Lewis structures to diagram the formation of PF3 from P and F atoms, showing valence-shell electrons.How many valence electrons does P have initially?
Use Lewis symbols and Lewis structures to diagram the formation of PF3 from P and F atoms, showing valence-shell electrons.How many valence electrons does each F have initially?
Use Lewis symbols and Lewis structures to diagram the formation of PF3 from P and F atoms, showing valence-shell electrons.How many valence electrons surround the P in the PF3 molecule?
Use Lewis symbols and Lewis structures to diagram the formation of PF3 from P and F atoms, showing valence-shell electrons.How many valence electrons surround each F in the PF3 molecule?
You may want to reference(Pages 309 - 315)Section 8.4 while completing this problem.How many bonding electrons are between the two oxygen atoms in hydrogen peroxide, H2O2?
You may want to reference (Pages 315 - 319)Section 8.5 while completing this problem.Draw the Lewis structure(s) for the molecule with the chemical formula C2H3N, where the N is connected to only one other atom. How many double bonds are there in the correct Lewis structure?
The C-O bond length in carbon monoxide, CO, is 1.13, whereas the C-O bond length in CO2 is 1.24.Without drawing a Lewis structure, do you think that CO contains a single, double, or triple bond?
A common form of elemental phosphorus is the tetrahedral P4 molecule, where all four phosphorus atoms are equivalent: . At room temperature phosphorus is a solid.How many P - P bonds are there in the molecule?
The lactic acid molecule, CH3CH (OH) COOH, gives sour milk its unpleasant, sour taste. You may want to reference (Pages 338 - 393) Chapter 9 while completing this problem.How many sigma bonds are in the molecule?
The compound with the following Lewis structure is acetylsalicylic acid, better known as aspirin: . You may want to reference (Pages 362 - 368) Section 9.6 while completing this problem.How many sigma bonds are in the molecule?
From their Lewis structures, determine the number of sigma and pi bonds in each of the following molecules or ions.formaldehyde, H2 CO;
From their Lewis structures, determine the number of sigma and pi bonds in each of the following molecules or ions.formic acid, HCO(OH), which has one H and two O atoms attached to C.
Buckminsterfullerene, C60 The molecule has a highly symmetric structure in which the 60 carbon atoms sit at the vertices of a truncated icosahedron. The bottom view shows only the bonds between carbon atoms.How many bonds does each carbon atom in C60 make?
Using Lewis symbols and Lewis structures, diagram the formation of SiCl4 from Si and Cl atoms, showing valence-shell electrons.How many bonding pairs of electrons are in the SiCl4 molecule?
Use Lewis symbols and Lewis structures to diagram the formation of PF3 from P and F atoms, showing valence-shell electrons.How many bonding pairs of electrons are in the PF3 molecule?
Ammonium chloride, NH4Cl, is a very soluble salt in water.Is there an N-Cl bond in solid ammonium chloride?
You may want to reference (Pages 300 - 301) Section 8.1 while completing this problem.Both Ti and Hf behave as though they possess the same number of valence electrons. Which of the subshells in the electron configuration of Hf behave as valence orbitals?
The molecule shown below is called furan. It is represented in typical shorthand way for organic molecules, with hydrogen atoms not shown. What is the molecular formula for furan?
The molecule shown below is called furan. It is represented in typical shorthand way for organic molecules, with hydrogen atoms not shown. How many electrons are in the pi system of the molecule?
Are all these Lewis symbols for Cl correct?
You may want to reference (Pages 361 - 368)Section 9.6 while completing this problem.How many electrons are in the O3 system of the ozone molecule, m O_3?
You may want to reference (Pages 320 - 322) Section 8.6 while completing this problem.With what allotrope of oxygen is NO2- isoelectronic?
Consider the molecule PF4 Cl.Draw a Lewis structure for the molecule.
The organic molecules shown beloware derivatives of benzene in which additional six-membered rings are "fused" at the edges of the hexagons. The compounds are shown in the usual abbreviated method for organic molecules.Using the Lewis structure for naphthalene and the average bond enthalpies in Table 8.4 in the textbook, estimate the heat of combustion of naphthalene, in kJ/mol.
How do you determine how many dots to put around the Lewis symbol of an element?
Describe the octet rule in Lewis theory.
The partial Lewis structure that follows is for a hydrocarbon molecule. In the full Lewis structure, each carbon atom satisfies the octet rule, and there are no unshared electron pairs in the molecule. The carbon-carbon bonds are labeled 1, 2, and 3. How many hydrogen atoms are in the molecule?
How do you draw an ionic Lewis structure?
How can Lewis structures be used to determine the formula of ionic compounds? Give an example.
Look at the Lewis structure for HF. Where are the nonbonding electrons?
Within a covalent Lewis structure, what is the difference between lone pair and bonding pair electrons?
How does the Lewis model for covalent bonding account for why certain combinations of atoms are stable while others are not?
What is the basic procedure for writing a covalent Lewis structure?
The substances NaF and CaO are isoelectronic (have the same number of valence electrons).What are the charges on each of the cations in each compound?
The substances NaF and CaO are isoelectronic (have the same number of valence electrons).What are the charges of each of the anions in each compound?
Barium azide is 62.04% Ba and 37.96% N. Each azide ion has a net charge of -1.Determine the chemical formula of the azide ion.
The ionic compound CaO crystallizes with the same structure as sodium chloride. In this structure, how many O2− are in contact with each Ca2+ ion (Hint: Remember the pattern of ions shown in the figure repeats over and over again in all three directions.)
Consider the Lewis structure for the polyatomic oxyanion shown here, where X is an element from the third period (Na-Ar). By changing the overall charge, n, from 1- to 2- to 3- we get three different polyatomic ions. For each of these ions identify the central atom, X. Arrange your answers in order increasing n.
Although I3- is known, F3- is not.Another classmate says F3-– does not exist because F is too small to make bonds to more than one atom. Is this classmate possibly correct?
Atoms follow the octet rule by gaining, losing, or sharing electrons until they are surrounded by eight valence electrons. Use the elements shown below as a guide to predict how electrons will fill the valence shells of the following elements. Potassium
Atoms follow the octet rule by gaining, losing, or sharing electrons until they are surrounded by eight valence electrons. Use the elements shown below as a guide to predict how electrons will fill the valence shells of the following elements. Calcium
You may want to reference (Pages 300 - 301) Section 8.1 while completing this problem. For each of these Lewis symbols, indicate the group in the periodic table in which the element X belongs.
Atoms follow the octet rule by gaining, losing, or sharing electrons until they are surrounded by eight valence electrons. Use the elements shown below as a guide to predict how electrons will fill the valence shells of the following elements. Bromine
You may want to reference (Pages 300 - 301) Section 8.1 while completing this problem. For each of these Lewis symbols, indicate the group in the periodic table in which the element X belongs.
The structure of borazine, B3N3H6, is a six-membered ring of alternating B and N atoms. There is one H atom bonded to each B and to each N atom. The molecule is planar.How many electrons are in the pi system of borazine?
Atoms follow the octet rule by gaining, losing, or sharing electrons until they are surrounded by eight valence electrons. Use the elements shown below as a guide to predict how electrons will fill the valence shells of the following elements. Krypton
You may want to reference (Pages 300 - 301) Section 8.1 while completing this problem. For each of these Lewis symbols, indicate the group in the periodic table in which the element X belongs.
You may want to reference (Pages 300 - 301) Section 8.1 while completing this problem.Which of the subshells in the electron configuration of Hf behave as core orbitals?
You may want to reference (Pages 300 - 301) Section 8.1 while completing this problem. Write the Lewis symbol for atoms of each of the following elements. To add an element not available in the menu, start by adding any element. Then, double click on the element you wish to change and using the keyboard type the element you wish to add.Al
You may want to reference (Pages 300 - 301) Section 8.1 while completing this problem. Write the Lewis symbol for atoms of each of the following elements. To add an element not available in the menu, start by adding any element. Then, double click on the element you wish to change and using the keyboard type the element you wish to add.Br
For COF2 draw an appropriate Lewis structure (carbon is the central atom).
For S2 Cl2 draw an appropriate Lewis structure (ClSSCl).
What is the Lewis symbol for each of the following atoms or ions? You may want to reference(Pages 300 - 301)Section 8.1 while completing this problem.Ca
For SF4 draw an appropriate Lewis structure.
What is the Lewis symbol for each of the following atoms or ions? You may want to reference(Pages 300 - 301)Section 8.1 while completing this problem.P
What is the Lewis symbol for each of the following atoms or ions? You may want to reference(Pages 300 - 301)Section 8.1 while completing this problem.Mg2+
What is the Lewis symbol for each of the following atoms or ions? You may want to reference(Pages 300 - 301)Section 8.1 while completing this problem.S2-
Methyl isocyanate, CH3NCO, was made infamous in 1984 when an accidental leakage of this compound from a storage tank in Bhopal, India, resulted in the deaths of about 3,800 people and severe and lasting injury to many thousands more.Draw a Lewis structure for methyl isocyanate.
For IF5 draw an appropriate Lewis structure.
For CH2 CHCH3 draw an appropriate Lewis structure.
You may want to reference (Pages 387 - 387) Section 9.3 while completing this problem.Draw the Lewis symbol for Ne.
Write an appropriate Lewis structure for each of the following compounds.BI3
For CH3SH draw an appropriate Lewis structure.
Write an appropriate Lewis structure for each of the following compounds.HCFO
Draw the Lewis structure of ClF3.
Hydrazine (NH2 NH2 ), hydrogen peroxide (HOOH), and water (H2 O) all have exceptionally high surface tensions in comparison with other substances of comparable molecular weights.Draw the Lewis structure for hydrazine (NH2 NH2).
Write an appropriate Lewis structure for each of the following compounds.PBr3
Hydrazine (NH2 NH2 ), hydrogen peroxide (HOOH), and water (H2 O) all have exceptionally high surface tensions in comparison with other substances of comparable molecular weights.Draw the Lewis structure for hydrogen peroxide (HOOH).
Hydrazine (NH2 NH2 ), hydrogen peroxide (HOOH), and water (H2 O) all have exceptionally high surface tensions in comparison with other substances of comparable molecular weights.Draw the Lewis structure for water (H2 O)
Draw the Lewis structure of SF4.
You may want to reference (Pages 388 - 393) Section 9.4 while completing this problem. Identify the correct Lewis symbol for the ions in each ionic compound.SrO
Make a sketch of BrF5.
You may want to reference (Pages 388 - 393) Section 9.4 while completing this problem. Identify the correct Lewis symbol for the ions in each ionic compound.CaI2
Make a sketch of SCl6.
You may want to reference (Pages 388 - 393) Section 9.4 while completing this problem. Identify the correct Lewis symbol for the ions in each ionic compound.RbF
Make a sketch of PF5.
Make a sketch of IF4 + .
You may want to reference (Pages 400 - 402) Section 9.7 while completing this problem.Draw the Lewis structure for BrF.
Construct a Lewis structure for O2 in which each atom achieves an octet of electrons.
You may want to reference(Pages 309 - 315)Section 8.4 while completing this problem.Construct a Lewis structure for hydrogen peroxide, H2O2, in which each atom achieves a stable noble-gas electron configuration.
You may want to reference (Pages 400 - 402) Section 9.7 while completing this problem.Draw the Lewis structure for CO.
You may want to reference(Pages 319 - 322)Section 8.6 while completing this problem.Complete the Lewis dot structure for H2CO (in which both H atoms are bonded to C).
You may want to reference(Pages 319 - 322)Section 8.6 while completing this problem.Complete the Lewis dot structure for H2O2.
You may want to reference(Pages 319 - 322)Section 8.6 while completing this problem.Complete the Lewis dot structure for C2F6 (which contains a C - C bond).
You may want to reference(Pages 319 - 322)Section 8.6 while completing this problem.Complete the Lewis dot structure for AsO33-.
You may want to reference(Pages 319 - 322)Section 8.6 while completing this problem.Complete the Lewis dot structure for H2SO3 (in which H is bonded to O).
You may want to reference(Pages 319 - 322)Section 8.6 while completing this problem.Complete the Lewis dot structure for NH2Cl.
Draw the Lewis structure for each organic compound from its condensed structural formula.C3H8
Draw the Lewis structure for each organic compound from its condensed structural formula.CH3OCH3
You may want to reference (Pages 316 - 319) Section 8.5 while completing this problem.Write a Lewis structure for the phosphorus trifluoride molecule, PF3.
Draw the Lewis structure for each organic compound from its condensed structural formula.CH3COCH3
Draw the Lewis structure for each organic compound from its condensed structural formula.CH3COOH
Draw the Lewis structure for each organic compound from its condensed structural formula.CH3CHO
Draw the Lewis structure for each organic compound from its condensed structural formula.C2H4
Draw the Lewis structure for each organic compound from its condensed structural formula.CH3NH2
Draw the Lewis structure for each organic compound from its condensed structural formula.HCHO
In the formate ion, pandoc: Error at "source" (line 1, column 13): unexpected " " expecting "{" or "" { m HCO_2}^ - , the carbon atom is the central atom with the other three atoms attached to it.Draw a Lewis structure for the formate ion.
Draw the Lewis structure for each organic compound from its condensed structural formula.CH3CH2OH
Draw the Lewis structure for each organic compound from its condensed structural formula.HCOOH
The compound C3H4 has two double bonds.Draw its Lewis structure.
Draw a Lewis structure for HCSNH2. (The carbon and nitrogen atoms are bonded together and the sulfur atom is bonded to the carbon atom.)
You may want to reference (Pages 426 - 461) Chapter 10 while completing this problem.Draw the structures of two different compounds that have the composition CH3NO2. All three H atoms must remain bonded to the C atom and both O atoms must remain bonded to the N atom.
A major challenge in implementing the “hydrogen economy” is finding a safe, lightweight, and compact way of storing hydrogen for use as a fuel. The hydrides of light metals are attractive for hydrogen storage because they can store a high weight percentage of hydrogen in a small volume. For example NaAlH4, can release 5.6% of its mass as H2 upon decomposing to NaH(s), Al(s), and H2(g). NaAlH4 possesses both covalent bonds, which hold polyatomic anions together, and ionic bonds.Based on electronegativity differences, predict the identity of the polyatomic anion.
You may want to reference (Pages 388 - 393) Section 9.4 while completing this problem.Use the Lewis model to predict the formula for the compound that forms between magnesium and nitrogen.
In the vapor phase, BeCl2 exists as a discrete molecule.Draw the Lewis structure of this molecule, using only single bonds.
A compound composed of only carbon and hydrogen is 7.743% hydrogen by mass. Propose a Lewis structure for the lightest of the possible compounds.
You may want to reference (Pages 400 - 402) Section 9.7 while completing this problem.Draw the Lewis structure for H2CO.
Draw four possible Lewis structures of the molecule xenon trioxide, XeO3, one each with zero, one, two, or three Xe - O double bonds.
A compound composed of only carbon and chlorine is 85.5% chlorine by mass and its molar mass is 165.82 g/mol. Propose a Lewis structure for the compound.
You may want to reference (Pages 408 - 411) Section 9.9 while completing this problem.Write the Lewis structure for XeF4.
Acetylene (C2H2) and nitrogen (N2) both contain a triple bond, but they differ greatly in their chemical properties.Write the Lewis structure for C2H2.
A 0.167-g sample of an unknown acid requires 27.8 mL of 0.100 M NaOH to titrate to the equivalence point. Elemental analysis of the acid gives the following percentages by mass: 40.00% C; 6.71% H; 53.29% O.Draw the Lewis structure.
The following table presents the solubilities of several gases in water at 25 oC under a total pressure of gas and water vapor of 1 atm. Gas Solubility (m M) CH4 (methane) 1.3 C2H6 (ethane) 1.8 C2H4 (ethylene) 4.7 N2 0.6 O2 1.2 NO 1.9 H2S 99 SO2 1476 You may want to reference (Pages 524 - 567) Chapter 13 while completing this problem.Draw the structures for the three hydrocarbons methane, ethane, and ethylene.
Acetylene (C2H2) and nitrogen (N2) both contain a triple bond, but they differ greatly in their chemical properties.Write the Lewis structure for N2.
You may want to reference (Pages 448 - 460) Section 10.7 while completing this problem.Draw the Lewis structure for XeF4.
A common form of elemental phosphorus is the tetrahedral P4 molecule, where all four phosphorus atoms are equivalent: . At room temperature phosphorus is a solid.Draw a Lewis structure for a linear P4 molecule that satisfies the octet rule.
A compound has the formula C8H8 and does not contain any double or triple bonds. All the carbon atoms are chemically identical and all the hydrogen atoms are chemically identical. Draw a Lewis structure for this molecule.
You may want to reference (Pages 323 - 325) Section 8.7 while completing this problem. Draw the Lewis structures for each of the following ions or molecules.PH3
You may want to reference (Pages 323 - 325) Section 8.7 while completing this problem. Draw the Lewis structures for each of the following ions or molecules.AlH3
You may want to reference (Pages 448 - 460) Section 10.7 while completing this problem.Draw the Lewis structure for HCN.
You may want to reference (Pages 323 - 325) Section 8.7 while completing this problem. Draw the Lewis structures for each of the following ions or molecules.CH2Cl2
The NOx waste stream from automobile exhaust includes species such as NO and NO2. Catalysts that convert these species to N2 are desirable to reduce air pollution.Draw the Lewis dot structure of NO.
You may want to reference (Pages 323 - 325) Section 8.7 while completing this problem. Draw the Lewis structures for each of the following ions or molecules.[SnF6]2-
The NOx waste stream from automobile exhaust includes species such as NO and NO2. Catalysts that convert these species to N2 are desirable to reduce air pollution.Draw the Lewis dot structure of NO2.
The NOx waste stream from automobile exhaust includes species such as NO and NO2. Catalysts that convert these species to N2 are desirable to reduce air pollution.Draw the Lewis dot structure of N2.
Draw the Lewis structures for each of the following molecules or ions. You may want to reference(Pages 322 - 325)Section 8.7 while completing this problem.NO
Dichloroethylene (C2 H2 Cl2 ) has three forms (isomers), each of which is a different substance.Draw Lewis structures of the three isomers, all of which have a carbon–carbon double bond.
Draw the Lewis structures for each of the following molecules or ions. You may want to reference(Pages 322 - 325)Section 8.7 while completing this problem.BF3
Draw the Lewis structures for each of the following molecules or ions. You may want to reference(Pages 322 - 325)Section 8.7 while completing this problem.OPBr3 (where P is the central atom)
Draw the Lewis structures for each of the following molecules or ions. You may want to reference(Pages 322 - 325)Section 8.7 while completing this problem.XeF4
The nitrogen atoms in N2 participate in multiple bonding, whereas those in hydrazine, N2H4, do not. You may want to reference (Pages 361 - 368)Section 9.6 while completing this problem.Complete Lewis structures for both molecules. You may draw them in any order.
The lactic acid molecule, CH3CH (OH) COOH, gives sour milk its unpleasant, sour taste. You may want to reference (Pages 338 - 393) Chapter 9 while completing this problem.Draw the Lewis structure for the molecule, assuming that carbon always forms four bonds in its stable compounds.
You may want to reference (Pages 362 - 368) Section 9.6 while completing this problem.Write a single Lewis structure for SO3.
Carbon monoxide, CO, is isoelectronic to N2.Draw a Lewis structure for CO that satisfies the octet rule.
Draw the Lewis structure for ethane (C2H6).
Draw the Lewis dot symbol for Li.
Draw the Lewis dot symbol for Be.
Draw the Lewis dot symbol for B.
Draw the Lewis dot symbol for C.
Draw the Lewis dot symbol for N.
Draw the Lewis structure for acetylene (C2H2).
Draw the Lewis dot symbol for O.
Draw the Lewis dot symbol for F.
Draw the Lewis structure for ethylene (C2H4).
Draw the Lewis dot symbol for Ne.
Draft a list of step-by-step instructions for writing the correct Lewis dot structure for any molecule or polyatomic ion.
Draw the Lewis structure for N2H4.
Write Lewis structure of N2H4.
Draw the Lewis structure for CCl4.
Draw the Lewis structure for CO32-.
Write Lewis structure of N2H2.
Draw the Lewis structure for NH4+.
Draw the Lewis dot symbol for the atom Al.
Write Lewis structure of N2.
Draw the Lewis dot symbol for the atom O.
There are many Lewis structures you could draw for sulfuric acid, H2SO4 (each H is bonded to an O).What Lewis structure(s) would you draw to satisfy the octet rule?
You may want to reference (Pages 316 - 319) Section 8.5 while completing this problem.Draw the Lewis structure for SiH4.
You may want to reference (Pages 316 - 319) Section 8.5 while completing this problem.Draw the Lewis structure for CO.
You may want to reference (Pages 316 - 319) Section 8.5 while completing this problem.Draw the Lewis structure for SF2.
You may want to reference (Pages 316 - 319) Section 8.5 while completing this problem.Draw the Lewis structure for H2 SO4 (H is bonded to O).
You may want to reference (Pages 316 - 319) Section 8.5 while completing this problem.Draw the Lewis structure for NH2 OH.
Draw the Lewis dot structure for CS2.
Draw the Lewis dot structure for NCl3.
Draw the Lewis dot structure for CF4.
Draw the Lewis dot structure for CH2F2.
You may want to reference (Pages 439 - 440) Section 10.4 while completing this problem.Draw the Lewis structure of N2.
You may want to reference (Pages 439 - 440) Section 10.4 while completing this problem.Draw the Lewis structure of N2H2 (whose skeletal structure is HNNH).
Draw the Lewis structure for CO2.
You may want to reference (Pages 439 - 440) Section 10.4 while completing this problem.Draw the Lewis structure of N2H4 (whose skeletal structure is H2NNH2).
Draw the Lewis structure for CCl4.
Triazine, C3 H3 N3, is like benzene except that in triazine every other C-H group is replaced by a nitrogen atom. Draw the Lewis structure for the triazine molecule.
You may want to reference (Pages 326 - 327) Section 8.8 while completing this problem.Draw the Lewis structure for hydrogen peroxide, H2O2.
Using Lewis symbols, diagram the reaction between magnesium and oxygen atoms to give the ionic substance MgO .
Use Lewis theory to determine the formula for the compound that forms between:Sr and Se
Use Lewis theory to determine the formula for the compound that forms between:Ba and Cl
The compound chloral hydrate, known in detective stories as knockout drops, is composed of 14.52% C, 1.83% H, 64.30% Cl, and 19.35% O by mass and has a molar mass of 165.4 g/mol.Draw the Lewis structure of the molecule, assuming that the Cl atoms bond to a single C atom and that there is a C-C bond and two C-O bonds in the compound.
Use Lewis theory to determine the formula for the compound that forms between:Na and S
Use Lewis theory to determine the formula for the compound that forms between:Al and O
Acetone, (CH3 )2 CO, is widely used as an industrial solvent.Draw the Lewis structure for the acetone molecule.
Draw covalent Lewis structures of the following elements (or families of elements).hydrogen, H2
Draw covalent Lewis structures of the following elements (or families of elements).the halogens, X2
Draw covalent Lewis structures of the following elements (or families of elements).oxygen, O2
Draw covalent Lewis structures of the following elements (or families of elements).nitrogen, N2
Use covalent Lewis structures to explain why the compound that forms between nitrogen and hydrogen has the formula NH3. Show why NH2 and NH4 are not stable.
You may want to reference (Pages 320 - 322) Section 8.6 while completing this problem.Write a Lewis structure that obeys the octet rule for SOCl2 (S is the central atom) and assign formal charges to each atom.
Write the Lewis symbol for N.
You may want to reference (Pages 320 - 322) Section 8.6 while completing this problem.Write a Lewis structure that obeys the octet rule for HClO2 (H is bonded to O) and assign formal charges to each atom.      
Write the Lewis symbol for each atom or ion.Al
You may want to reference (Pages 320 - 322) Section 8.6 while completing this problem.Write a Lewis structure that obeys the octet rule for OCS and assign formal charges to each atom.
Write a Lewis structure for each molecule.SF2
Write the Lewis symbol for each atom or ion.Cl
Write a Lewis structure for each molecule.SiH4
Write a Lewis structure for each molecule.HCOOH (both O bonded to C)
Select the Lewis symbols for the ions in each ionic compound.NaF
Ammonia reacts with boron trifluoride to form a stable compound.Draw the Lewis structure of the ammonia-boron trifluoride reaction product.
Write a Lewis structure for each molecule.CH3SH (C and S central)
Select the Lewis symbols for the ions in each ionic compound.CaO
Select the Lewis symbols for the ions in each ionic compound.SrBr2
Although I3- is known, F3- is not.Draw the Lewis structure for I3- (It is linear, not a triangle).
Draw the Lewis structure for CO.
Ammonium chloride, NH4Cl, is a very soluble salt in water.Draw the Lewis structures of the ammonium and chloride ions.
The structure of borazine, B3N3H6, is a six-membered ring of alternating B and N atoms. There is one H atom bonded to each B and to each N atom. The molecule is planar.Write a Lewis structure for borazine in which the octet rule is satisfied for every atom.
Write a Lewis structure for each molecule or ion.H3COCH3
Draw the dominant Lewis structures for these chlorine-oxygen molecules/ions.ClO
Write a Lewis structure for each molecule or ion.CN-
Draw the dominant Lewis structures for these chlorine-oxygen molecules/ions.ClO-
Write a Lewis structure for each molecule or ion.NO2-
Draw the dominant Lewis structures for these chlorine-oxygen molecules/ions.ClO2-
Write a Lewis structure for each molecule or ion.ClO-
Draw the dominant Lewis structures for these chlorine-oxygen molecules/ions.ClO3-
Draw the dominant Lewis structures for these chlorine-oxygen molecules/ions.ClO4-
Draw lewis structure for XeF2O. 
The Lewis electron dot structure of SO4 2- shows how many lone pairs are present in the structure. Which of the following answers is correct?a) 0b) 1c) 4d) 12e) none of the given answers
What is the total number of valence electrons in the Lewis structure of CH  2ClCH2Cl?a. 14b. 12c. 18d. 10e. 26
Select the element whose Lewis symbol is correct.  
Select the molecule which has one lone pair on the central atoma. NH2 -b. H2Oc. CH4d. H3O+e. BeCl2
In the Lewis structures of N2H2a. There is a nitrogen-nitrogen triple bondb. There is a nitrogen- nitrogen single bondc. Each nitrogen has two nonbonding electron pairs (lone-pairs)d. Each nitrogen has one nonbonding electron pair (lone-pair)e. Each hydrogen has one nonbonding electron pair (lone pair) 
The number of lone electron pairs in the N 2 molecule is ___.A)  1   B)  3   C)  2   D)  4   E)  5
 Give Lewis structures for the following molecules or ions.a) HCFO    b) CH3CH2OCH3
Which of the following species will have a Lewis structure most like that of the hydronium ion , H3O+ ?a. NO3 - b. NH3c. SO3 d. CO3 2- e. H2CO
Draw the Lewis Structure H3COH.
Which of the following is a possible valid Lewis structure for the compound which has the molecular formula C2H6O? a. 1 and 2b. 2c. 3d. 2 ande. 1,2 and 3
How many lone pairs are on the central atom in BCl 3? Express your answer numerically as an integer.     How many lone pairs are on the central atom of BrF 3? Express your answer numerically as an integer.
Draw the Lewis structures of N 2H4, N2H2, and N2.
Draw the Lewis structure of ammonia, NH3. In the Lewis structure 1) Nitrogen has a lone pair of electrons 2) Nitrogen has three bonding pairs of electrons 3) Each hydrogen has a bonding pair of electrons 4) all of the above
How many valence electrons are in an atom of phosphorus and an atom of selenium?(A) Phosphorus has 3; selenium has 4(B) Phosphorus has 5; selenium has 1(C) Phosphorus has 5; selenium has 6(D) Phosphorus has 15; selenium has 34(E) Phosphorus has 3; selenium has 6
For neutral molecules, which statements about covalent Lewis structures are true? Hydrogen atoms are often the central atom of a Lewis structure. Each atom of a Lewis structure must have eight electrons.For a neutral molecule, the number of electrons in the Lewis structure is the sum of the valence electrons for the atoms.Electrons of covalent compounds may be shared between atoms.
In the Lewis dot structure of the molecule ClF 3, how many unbonded electron pairs are found around the central atom?1. 12. 33. 24. 05. 4
Which one of the following Lewis structures is definitely incorrect? 
Draw the Lewis structure for formic acid (HCOOH).
Draw the Lewis dot structure for NH 2Cl.
Add lone pairs to these Lewis structures of polyhalide ions. ClF2– ClF2+ ClF4–
In the Lewis structure for formic acid, HCOOH, how many bonding pairs and lone pairs of electrons are present? a) 4 bonding, 2 lone b) 4 bonding, 5 lone c) 5 bonding, 0 lone d) 5 bonding, 4 lone
Draw the Lewis electron-dot structure for H 2S.
Draw the Lewis Dot Structure for NH+4, NH2- and Mg2+.
Draw Lewis structures for molecular formula C3H8O (Three Isomers).
Draw the main Lewis structure of NOF. Draw nonbonding electrons using the dot notation, and bonding electrons as a bond.
Which molecule does not contain a double bond?a) HNOb) C2H2c) H2COd) C2H4e) S2
Draw the Lewis Dot structure of PF6-.
Each of the following structures is invalid. Identify the error in each case.
Draw the Lewis Dot structure for BrO2-.  
How many covalent bonds does carbon form in neutral compounds?
How many covalent bonds does oxygen form in electrically neutral compounds?
Determine the number of valence electrons for each of the following four elements.GaPbClN
How many covalent bonds does nitrogen form in electrically neutral compounds?
How many covalent bonds does hydrogen form in electrically neutral compounds?
Draw a Lewis dot structure for BCl 3 with any lone pairs.
Draw the Lewis structure for HBr.
Which of the following are possible Lewis structures for C 2H6O? A. 1 only B. 2 only C. 3 only D. 1 and 2 E. 2 and 3
Which of the following are valid ionic Lewis structures? Drag each item to the appropriate bins.
Draw the Lewis structure of PH 3.
Construct the Lewis structure for the covalent compound silicon dioxide (SiO 2).
Choose the best Lewis structure for SF4.
Draw the Lewis structure for the sulfite ion, SO 3 2−. Which of the statements below is true for the Lewis structure of the sulfite ion?a) There must be a double bond between the sulfur atom and one of the oxygen atoms to ensure that all atoms have an octet (eight electrons).b) There are no lone pairs of electrons on the sulfur atom.c) There is one lone pair of electrons on the sulfur atom.d) There are double bonds between the sulfur atom and each of the three oxygen atoms.
How many valence electrons must be accounted for in the Lewis structure of chloroethane (C2H5Cl)?
Draw the lewis structure for the formaldehyde molecule, H 2CO.
Draw the lewis structures for each of the following molecules or ions. a. NO b. AlH3 c. ICl2- d. OPBr3e. XeF4
what is the lewis structure for HOFO?
Draw a Lewis structure for C2H3Cl. Show all unshared electron pairs.
Draw the main Lewis structure of NOF. Draw nonbonding electrons using the dot notation and bonding electrons as a bond.   Determine the number of bonding electrons and the number of nonbonding electrons in the structure of BeF2. 
Which of the following are possible Lewis structures for C2H6O? a. (1) and (2) b. (1) and (3) c. (2) and (3) d. (1) or (2) or (3) - only one structure is possible e. (1), (2), and (3) - all three structures are possible
The central atom in HNO3 is surrounded by a. two single bonds and one double bond. b. four single bonds and no double bonds. c. three single bonds and one double bond. d. three single bonds and one triple bond. e. three double bonds and one single bond.
Draw the Lewis structure of O 2. How many pairs of bonding and non-bonding valence electrons are in this molecule? A) 3 pairs of bonding electrons, 3 pairs of non-bonding electrons B) 4 pairs of bonding valence electrons, 2 pairs of non-bonding valence electrons C) 4 pairs of bonding valence electrons, 4 pairs of non-bonding valence electrons D) 2 pairs of bonding valence electrons, 4 pairs of non-bonding valence electrons
How many valence electrons does an atom of arsenic have? a) 3 b) 33 c) 15 d) 5 e) 8
The central atom in SOCl2 is a sulfur atom. Fill in the blanks in the statement below:The sulfur-oxygen bond is a ________ and there are _________ around the oxygen.a. single bond and two lone pairs of electrons.b. single bond and three lone pairs of electrons.c. double bond and two lone pairs of electrons.d. double bond and three lone pairs of electrons.e. triple bond and one lone pair of electrons.
The complete Lewis structure of the structure below will havea) at least one lone pair on each atom.b) at least one double bond.c) both polar and nonpolar bonds.d) resonance forms.
One atom of silicon can properly be combined in a compound with a. two atoms of oxygen. b. one atom of chlorine. c. four atoms of calcium. d. three atoms of hydrogen.
Choose a Lewis structure for BF3.
The molar mass of a hydrocarbon compound was found to be 30.069 g/mol. What is the molecular formula?
Diborane, the simplest known member of the series of boron hydrides, is comprised of:(a) 1 boron-boron bond, and 6 terminal hydrogens(b) 1 BF3 − ion and 1 BF3 + ion(c) No boron-boron bond, 1 bridging hydrogen, 4 terminal hydrogens, and an ionic H(d) No boron-boron bond, 2 bridging hydrogens and 4 terminal hydrogens(e) No boron-boron bond, 4 bridging hydrogens and 2 terminal hydrogens
Draw the Lewis dot structure for AlCl 3.
Draw the Lewis dot structure for the following:CaO, SrBr2, K2O
Write the electron dot structure for SBr2.
Draw the electron-dot structure for CHClO. Note: Carbon is the central atom and all three atoms (H, Cl, O) are attached to the carbon.  
Which element is most likely to form a triple bond?a) Pbb) Fc) Nd) S
What is the Lewis dot structure of XeF 2O? Draw all lone pairs.
How do you draw a Lewis Structure for SiCl 2Br2?
Add lone pairs to these Lewis structures of interhalogen compounds.
Draw the Lewis structure for the following molecule: OPBr 3. 
Draw Lewis structures for the following xenon compounds. Show all lone pairs.  
Draw a Lewis structure for each of the following molecules. Include all lone pairs of electrons. NF3        HBr        SBr2     CCl4  
Draw a Lewis structure of CH 3NH2.
Choose a likely identity for X,Y, and Z in these structures.
In carbon-containing compounds, carbon usually forms1. four bonds, nitrogen and oxygen usually form two bonds, and hydrogen only forms one bond.2. three bonds, nitrogen and oxygen usually form two bonds, and hydrogen only forms one bond.3. four bonds, nitrogen usually forms three bonds, oxygen usually forms two bonds, and hydrogen only forms one bond.4. four bonds, nitrogen usually forms five bonds, oxygen usually forms six bonds, and hydrogen only forms one bond.
Draw the Lewis structure of chloroform, CHCl 3.
Write a Lewis structure for each molecule. Include all lone pairs of electrons. CH2O   C2Cl4   CH3NH2      CFCl3 (C central)
How many valence electrons does a neutral oxygen atom have? How many bonds can a neutral oxygen participate in? How many lone pair electrons does a neutral oxygen in a compound normally have? a) 2, 1, 6 b) 2, 2, 4 c) 2, 3, 2 d) 2, 4, 0 e) 4, 1, 6 f) 4, 2, 4 g) 4, 3, 2 h) 4, 4, 0 i) 6, 1, 6 j) 6, 2, 4 k) 6, 3, 2 l) 6, 4, 0
What is the lewis dot structure NH4Cl
In the Lewis Dot Structure of nitrogen trichloride, NCl 3, how many shared valence electrons are around the central atom?
The Lewis structure for N2H2 (HHNH) shows1. two single bonds, one double bond and two unshared pairs2. three single bonds and four unshared pairs3. three single bonds and two unshared pairs4. two single bonds, one double bond and dour unshared pairs
Draw the Lewis structure for HCN. Include lone pairs.
Which of the following Lewis structures is incorrect?
Draw the Lewis structure for Si, Cl 2, Br2.
Which of the following has NO unshared pairs of electrons on the central atom?1. BrO3 -2. IF2 +3. FNO2 (N is central)4. SF5 -
For the compound below, state why it is wrong and write a version that is correct. 
Draw the Lewis structure for IBr.
Sodium acetate, CH3CO2Na, contains both ionic and covalent bonds.Draw the Lewis structure of this compound.
Draw the Lewis structure of xenon difluoride and give the number of lone pairs of electrons around the central atom.1. 42. 53. 24. 35. 1
Part A:Consider the partial oxidation of ethane as shown in the following reaction: C2H6(g) + O2(g) → 2CO(g) + 3H2(g) First, write dot structures for C2H6, O2, CO, and H2.        Part B:Was ethane really oxidized in this reaction? Assign oxidation numbers. Was C2H6 oxidized? __________ If so, did oxidation occur at C or H or both? 
The arrangement of atoms in several biologically important molecules is given. Complete the Lewis structures of the molecule by adding multiple bonds and lone pairs. Do not add any more atoms.The amino acid serine:
The arrangement of atoms in several biologically important molecules is given. Complete the Lewis structures of the molecule by adding multiple bonds and lone pairs. Do not add any more atoms.Urea:
Two molecules used in the polymer industry are azodicarbonamide and methyl cyanoacrylate. Their structures areAzodicarbonamide is used in forming polystyrene. When added to the molten plastic, it decomposes to nitrogen, carbon monoxide, and ammonia gases, which are captured as bubbles in the molten polymer. Methyl cyanoacrylate is  super glue. As the glue sets, methyl cyanoacrylate polymerizes across the carbon–carbon double bond. a. Complete the Lewis structures showing all lone pairs of electrons.
The arrangement of atoms in several biologically important molecules is given. Complete the Lewis structures of the molecule by adding multiple bonds and lone pairs. Do not add any more atoms.Pyruvic Acid:
The arrangement of atoms in several biologically important molecules is given. Complete the Lewis structures of the molecule by adding multiple bonds and lone pairs. Do not add any more atoms.Uracil:
The arrangement of atoms in several biologically important molecules is given. Complete the Lewis structures of the molecule by adding multiple bonds and lone pairs. Do not add any more atoms.Carbonic Acid:
Hot and spicy foods contain molecules that stimulate paindetecting nerve endings. Two such molecules are piperine and capsaicin:Piperine is the active compound in white and black pepper, and capsaicin is the active compound in chili peppers. The ring structures in piperine and capsaicin are shorthand notation. Each point where lines meet represents a carbon atom.a. Complete the Lewis structure for piperine and capsaicin, showing all lone pairs of electrons.
The antibiotic thiarubin-A was discovered by studying the feeding habits of wild chimpanzees in Tanzania. The structure for thiarubin-A isa. Complete the Lewis structure, showing all lone pairs of electrons.
Draw the lewis structure of CH 2N2, including formal charges and reasonable resonance structures, if any. 
You may want to reference (Pages 300 - 301) Section 8.1 while completing this problem.An atom has the electron configuration 1s22s22p63s23p3. How many valence electrons does the atom have?
You may want to reference (Pages 448 - 460) Section 10.7 while completing this problem.The valence electron configurations of several atoms are shown. How many bonds can each atom make without hybridization?Be: 2s2
For COF2 draw an appropriate Lewis structure (carbon is the central atom).
Two structures can be drawn for cyanuric acid:a. Are these two structures the same molecule? Explain.
In the Lewis structure shown below, M and X represent various elements in the third period of the periodic table. Write the formula of the compound using the chemical symbols of each element.
In the Lewis structure shown below, M and X represent various elements in the third period of the periodic table. Write the formula of the compound using the chemical symbols of each element.
In the Lewis structure shown below, M and X represent various elements in the third period of the periodic table. Write the formula of the compound using the chemical symbols of each element.
In the Lewis structure shown below, M and X represent various elements in the third period of the periodic table. Write the formula of the compound using the chemical symbols of each element.
For S2Cl2 draw an appropriate Lewis structure (ClSSCl). For SF4 draw an appropriate Lewis structure. Make a sketch of ClF3. Make a sketch of IF2-.  
Draw the Lewis structure for (CH 3)2NH.
Draw the Lewis structure for Cl 2CO.
What is the lewis structure for IBr 2-?
Draw a single Lewis structure for the phosphate ion, assuming that the phosphorus atom can expand its octet, such that the formal charge on each of the atoms is minimized. Include all formal charges and lone-pair electrons.
Draw Lewis structures of CH 3NO2, showing all resonance forms.
What is the lewis structure of XeH 4?
Draw a Lewis structure for CH 4O in which O is bonded to two kinds of atoms.
Draw the lewis dot structure for CH 3CN.
Draw the Lewis structure for each compound.Cl2O7 (no Cl–Cl bond)
Draw a Lewis structure for (a) SiF4
Draw the Lewis structure for each compound.H3PO3 (two O–H bonds)
Draw a Lewis structure for (b) SeCl2
Draw the Lewis structure for each compound.H3AsO4
Write a Lewis structure for H 2CO.
Consider nitrous acid, HNO2 (HONO).(a) Write a Lewis structure.
Use Lewis electron-dot symbols to represent the formation of BrF 3 from bromine and fluorine atoms;
Draw a Lewis structure for (c) COF2 (C is the central atom)
Write a Lewis structure for AsF 3.
Draw a Lewis structure for (a) PH4+ 
Write Lewis structure that obey the octet rule for the following molecules and ions. (In this case the first atom listed is the central atom.)c. ClO2-, SCl2, PCl2-
Use Lewis electron-dot symbols to represent the formation of AlF 3 from aluminum and fluorine atoms.
Draw a Lewis structure for (b) C2F4 
Draw a Lewis structure for (c) SbH3
Write a Lewis structure for ClNO.
Draw a Lewis structure for (a) PF3
Write a Lewis structure for SiCl 4.
Draw a Lewis structure for (b) H2CO3 (both H atoms are attached to O atoms)
Write a Lewis structure for H 3O +.
Draw a Lewis structure for (c) CS2
Draw a Lewis structure for (a) CH4S
Write a Lewis structure for NH 4 +.
Strike-anywhere matches contain a layer of KClO3 and a layer of P4S3. The heat produced by the friction of striking the match causes these two compounds to react vigorously, which sets fire to the wooden stem of the match. KClO3 contains the ClO3− ion. P4S3 is an unusual molecule with the skeletal structure.(a) Write Lewis structures for P4S3 and the ClO3– ion.
Draw a Lewis structure for (b) S2Cl2
Draw a Lewis structure for (c) CHCl3
Write a Lewis structure for BF4 –.
Write a Lewis structure for HCCH.
You may want to reference (Pages 382 - 416) Chapter 9 while completing this problem.Construct or identify an appropriate Lewis structure for each of the following compounds. Make certain to distinguish between ionic and covalent compounds.ClF5
Write a Lewis structure for ClCN.
You may want to reference (Pages 382 - 416) Chapter 9 while completing this problem.Construct or identify an appropriate Lewis structure for each of the following compounds. Make certain to distinguish between ionic and covalent compounds.XeO4
You may want to reference (Pages 382 - 416) Chapter 9 while completing this problem.Construct or identify an appropriate Lewis structure for each of the following compounds. Make certain to distinguish between ionic and covalent compounds.Al2O3
You may want to reference (Pages 382 - 416) Chapter 9 while completing this problem.Construct or identify an appropriate Lewis structure for each of the following compounds. Make certain to distinguish between ionic and covalent compounds.MgI2
You may want to reference (Pages 388 - 393) Section 9.4 while completing this problem.Identify the correct Lewis symbol for the ions in each ionic compound.Li2S
Write a Lewis structure for CO 2 2+.
Lewis structure can be used to understand why some molecule react in certain ways. Write the Lewis structure for the reactant and product in the reaction described below.a. Nitrogen dioxide dimerizes to produce dinitrogen tetroxide.Give a possible explanation for why these two reactions occur.
Write a Lewis structure for ClF 3.
Write a Lewis structure for PCl 5.
Write a Lewis structure for BF 3.
Carbon ring structures are common in organic chemistry. Draw a Lewis structure for each of the following carbon ring structures.C4H8
Lewis structure can be used to understand why some molecule react in certain ways. Write the Lewis structure for the reactant and product in the reaction described below.b. Boron trihydride accepts a pair of electrons from ammonia, forming BH 3NH3.Give a possible explanation for why these two reactions occur.
Carbon ring structures are common in organic chemistry. Draw a Lewis structure for each of the following carbon ring structures.C4H4
Carbon ring structures are common in organic chemistry. Draw a Lewis structure for each of the following carbon ring structures.C6H12
Write a Lewis structure for PF 6–.
Carbon ring structures are common in organic chemistry. Draw a Lewis structure for each of the following carbon ring structures.C6H6
Molten beryllium chloride reacts with chloride ion from molten NaCl to form the BeCl 42− ion, in which the Be atom attains an octet. Show the net ionic reaction with Lewis structures.
Write a Lewis structure for SeF 6.
Cryolite (Na3AlF6) is an indispensable component in the electrochemical production of aluminum. Draw a Lewis structure for the AlF63− ion.
Write a Lewis structure for XeF 4.
Write a Lewis structure for SeCl 3+.
Write a Lewis structure for Cl 2BBCl2 (contains a B–B bond).
 Write a Lewis structure for PO 43−.
 Write a Lewis structure for ICl 4−.
 Write a Lewis structure for SO 32−.
 Write a Lewis structure for HONO.
You may want to reference (Pages 382 - 416) Chapter 9 while completing this problem.Free radicals are important in many environmentally significant reactions (see the Chemistry in the Environment box on free radicals in Chapter 9 in the textbook). For example, photochemical smog (smog that results from the action of sunlight on air pollutants) forms in part by these two steps:NO2 + UV light → NO + OO + O2 → O3The product of this reaction, ozone, is a pollutant in the lower atmosphere. (Upper atmospheric ozone is a natural part of the atmosphere that protects life on Earth from ultraviolet light.) Ozone is an eye and lung irritant and also accelerates the weathering of rubber products. Construct the Lewis structure of NO2.
 Write a Lewis structure for SbH 3.
You may want to reference (Pages 382 - 416) Chapter 9 while completing this problem.Free radicals are important in many environmentally significant reactions (see the Chemistry in the Environment box on free radicals in Chapter 9 in the textbook). For example, photochemical smog (smog that results from the action of sunlight on air pollutants) forms in part by these two steps:NO2 + UV light → NO + OO + O2 → O3The product of this reaction, ozone, is a pollutant in the lower atmosphere. (Upper atmospheric ozone is a natural part of the atmosphere that protects life on Earth from ultraviolet light.) Ozone is an eye and lung irritant and also accelerates the weathering of rubber products. Construct the Lewis structure of O2 .
You may want to reference (Pages 382 - 416) Chapter 9 while completing this problem.Free radicals are important in many environmentally significant reactions (see the Chemistry in the Environment box on free radicals in Chapter 9 in the textbook). For example, photochemical smog (smog that results from the action of sunlight on air pollutants) forms in part by these two steps:NO2 + UV light → NO + OO + O2 → O3The product of this reaction, ozone, is a pollutant in the lower atmosphere. (Upper atmospheric ozone is a natural part of the atmosphere that protects life on Earth from ultraviolet light.) Ozone is an eye and lung irritant and also accelerates the weathering of rubber products. Construct the Lewis structure of O3 .
 Write a Lewis structure for XeF 2.
Draw a Lewis electron-dot symbol for the following atom:Rb
Draw a Lewis electron-dot symbol for the following atom:Si
 Write a Lewis structure for Se 8 (a cyclic molecule with a ring of eight Se atoms).
Draw a Lewis electron-dot symbol for the following atom:I
Draw a Lew is electron-dot symbol for the following atom:Ba
Methanol, H3COH, is used as the fuel in some race cars. Ethanol, C 2H5OH, is used extensively as motor fuel in Brazil. Both methanol and ethanol produce CO2 and H2O when they burn. Write the chemical equations for these combustion reactions using Lewis structures instead of chemical formulas.
Draw a Lewis electron-dot symbol for the following atom:Kr
Draw a Lewis is electron-dot symbol for the following atom:Br
Write Lewis structure and predict whether the following is polar or nonpolar.a. HOCN (exists as HOOCN)
Many planets in our solar system contain organic chemicals including methane (CH 4) and traces of ethylene (C2H4), ethane (C2H6), propyne (H3CCCH), and diacetylene (HCCCCH). Write the Lewis structures for each of these molecules.
Draw a Lewis electron-dot symbol for the following:Sr
Write Lewis structure and predict whether the following is polar or nonpolar.b. COS
Draw a Lewis electron-dot symbol for the following:P
Write Lewis structure and predict whether the following is polar or nonpolar.c. XeF2
Carbon tetrachloride was formerly used in fire extinguishers for electrical fires. It is no longer used for this purpose because of the formation of the toxic gas phosgene, Cl2CO. Write the Lewis structures for carbon tetrachloride and phosgene.
Draw a Lewis electron-dot symbol for the following:S
Write Lewis structure and predict whether the following is polar or nonpolar.d. CF2Cl2
Identify the atom that correspond to the following electron configuration. Then, write the Lewis symbol for the common ion formed from each atom: 1s22s22p5.
Draw a Lewis electron-dot symbol for the following:As
Write Lewis structure and predict whether the following is polar or nonpolar.e. SeF6
Draw a Lewis electron-dot symbol for the following:Se
Write Lewis structure and predict whether the following is polar or nonpolar.f. H2CO (C is the central atom.)
Identify the atom that correspond to the following electron configuration. Then, write the Lewis symbol for the common ion formed from each atom: 1s22s22p63s2.
Draw a Lewis electron-dot symbol for the following:Ga
Identify the atom that correspond to the following electron configuration. Then, write the Lewis symbol for the common ion formed from each atom: 1s22s22p63s23p64s23d10.
Use condensed electron configurations and Lewis electrondot symbols to depict the ions formed from the following atoms, and predict the formula of their compound:Ba and Cl
Use condensed electron configurations and Lewis electrondot symbols to depict the ions formed from the following atoms, and predict the formula of their compound:Sr and O
Identify the atom that correspond to the following electron configuration. Then, write the Lewis symbol for the common ion formed from each atom: 1s22s22p63s23p64s23d104p4.
Use condensed electron configurations and Lewis electrondot symbols to depict the ions formed from the following atoms, and predict the formula of their compound:Al and F
Borazine (B3N3H6) has often been called “inorganic” benzene. Write Lewis structures for borazine. Borazine contains a sixmembered ring of alternating boron and nitrogen atoms with one hydrogen bonded to each boron and nitrogen.
Identify the atom that correspond to the following electron configuration. Then, write the Lewis symbol for the common ion formed from each atom: 1s22s22p63s23p64s23d104p1.
Use condensed electron configurations and Lewis electrondot symbols to depict the ions formed from the following atoms, and predict the formula of their compound:Rb and O
Use condensed electron configurations and Lewis electrondot symbols to depict the ions formed from the following atoms, and predict the formula of their compound:Cs and S
Use condensed electron configurations and Lewis electrondot symbols to depict the ions formed from the following atoms, and predict the formula of their compound:O and Ga
Use condensed electron configurations and Lewis electrondot symbols to depict the ions formed from the following atoms, and predict the formula of their compound:N and Mg
Use condensed electron configurations and Lewis electrondot symbols to depict the ions formed from the following atoms, and predict the formula of their compound:Br and Li
Draw a Lewis structure for each species:(a) PF5
Draw a Lewis structure for each species:(b) CCl4
Draw a Lewis structure for each species:(c) H3O+
Draw a Lewis structure for each species:(d) ICl3
Draw a Lewis structure for each species:(e) BeH2
Draw a Lewis structure for each species:(f) PH2−
Draw a Lewis structure for each species:(g) GeBr4
Draw a Lewis structure for each species:(h) CH3−
A compound with a molar mass of about 28 g/mol contains 85.7% carbon and 14.3% hydrogen by mass. Write the Lewis structure for a molecule of the compound.
Draw a Lewis structure for each species:(i) BCl3
Draw a Lewis structure for each species:(j) BrF4+
Draw a Lewis structure for each species:(k) XeO3
A compound with a molar mass of about 42 g/mol contains 85.7% carbon and 14.3% hydrogen by mass. Write the Lewis structure for a molecule of the compound.
Draw a Lewis structure for each species:(l) TeF4
Two arrangements of atoms are possible for a compound with a molar mass of about 45 g/mol that contains 52.2% C, 13.1% H, and 34.7% O by mass. Write the Lewis structures for the two molecules.
Hydrazine, N2H4, and carbon disulfide, CS2, react to form a cyclic molecule (below). Draw Lewis structures for N2H4 and CS2.
Sulfuric acid is the industrial chemical produced in greatest quantity worldwide. About 90 billion pounds are produced each year in the United States alone. Write the Lewis structure for sulfuric acid, H2SO4, which has two oxygen atoms and two OH groups bonded to the sulfur.
Write the Lewis symbol for As 3–.
A gaseous compound has a composition by mass of 24.8% carbon, 2.08% hydrogen, and 73.1% chlorine. At STP, the gas has a density of 4.3 g/L. Draw a Lewis structure that fits these facts. Would another structure be equally satisfactory? Explain.
Use Lewis structures to determine which two of the following are unstable: (a) SF2 (b) SF3 (c) SF4 (d) SF5 (e) SF6
Write the Lewis symbol for I –.
Write the Lewis symbol for Be 2+.
Write the Lewis symbol for O 2–.
Write the Lewis symbol for Ga 3+.
Write the Lewis symbol for Li +.
Write the Lewis symbol for N 3–.
Make a sketch of the following molecule: C2H2 (skeletal structure HCCH).
Make a sketch of the following molecule: C2H4 (skeletal structure H2CCH2).
Many monatomic ions are found in seawater, including the ions formed from the following elements. Write the Lewis symbol for the monatomic ion formed from Cl.
Make a sketch of the following molecule: C2H6 (skeletal structure H3CCH3).
Many monatomic ions are found in seawater, including the ions formed from the following elements. Write the Lewis symbol for the monatomic ion formed from Na.
Many monatomic ions are found in seawater, including the ions formed from the following elements. Write the Lewis symbol for the monatomic ion formed from Mg.
Many monatomic ions are found in seawater, including the ions formed from the following elements. Write the Lewis symbol for the monatomic ion formed from Ca.
You may want to reference (Pages 382 - 416) Chapter 9 while completing this problem.Draw the Lewis structure for urea, H2NCONH2, the compound primarily responsible for the smell of urine. (The central carbon atom is bonded to both nitrogen atoms and to the oxygen atom.)
Many monatomic ions are found in seawater, including the ions formed from the following elements. Write the Lewis symbol for the monatomic ion formed from K.
Sketch the following molecule: CH3OH (skeletal structure H3COH).
Many monatomic ions are found in seawater, including the ions formed from the following elements. Write the Lewis symbol for the monatomic ion formed from Br.
Sketch the following molecule: CH3OCH3 (skeletal structure H3COCH3).
Sketch the following molecule: H2O2 (skeletal structure HOOH).
Many monatomic ions are found in seawater, including the ions formed from the following elements. Write the Lewis symbol for the monatomic ion formed from Sr.
Many monatomic ions are found in seawater, including the ions formed from the following elements. Write the Lewis symbol for the monatomic ion formed from F.
Write the Lewis symbols of the ions in MgS and the Lewis symbols of the atom from which it is formed.
You may want to reference (Pages 439 - 440) Section 10.4 while completing this problem.Sketch the following molecule: CH3NH2 (whose skeletal structure is H3CNH2).
You may want to reference (Pages 439 - 440) Section 10.4 while completing this problem.Sketch the following molecule: CH3CO2CH3 (whose skeletal structure is H3CCOOCH3, with both O atoms attached to the second C).
Write the Lewis symbols of the ions in Al 2O3 and the Lewis symbols of the atom from which it is formed.
You may want to reference (Pages 439 - 440) Section 10.4 while completing this problem.Sketch the following molecule: NH2CO2H (whose skeletal structure is H2NCOOH, with both O atoms attached to C).
Write the Lewis symbols of the ions in GaCl  3 and the Lewis symbols of the atom from which it is formed.
Write the Lewis symbols of the ions in K 2O and the Lewis symbols of the atom from which it is formed.
What is the molecular structure of the stable form of FNO2? (N is the central atom.)
A compound with a molar mass of about 42 g/mol contains 85.7% carbon and 14.3% hydrogen. What is its molecular structure?
Write the Lewis symbols of the ions in Li 3N and the Lewis symbols of the atom from which it is formed.
CH3F is a polar molecule, even though the tetrahedral geometry often leads to nonpolar molecules. Draw the Lewis structure of CH3F.
Write Lewis structure that obey the octet rule (duet rule for H) for the following molecule. Carbon is the central atom in CH4, nitrogen is the central atom in NH 3, and oxygen is the central atom in H2O.a. F2
Write the Lewis symbols of the ions in KF and the Lewis symbols of the atom from which it is formed.
Write Lewis structure that obey the octet rule (duet rule for H) for the following molecule. Carbon is the central atom in CH4, nitrogen is the central atom in NH 3, and oxygen is the central atom in H2O.b. O2
Draw the Lewis structure for the CCl4.  
Write Lewis structure that obey the octet rule (duet rule for H) for the following molecule. Carbon is the central atom in CH4, nitrogen is the central atom in NH 3, and oxygen is the central atom in H2O.c. CO
Write the Lewis structure for the NH3.
Write the Lewis structure for the OF2.
Write Lewis structure that obey the octet rule (duet rule for H) for the following molecule. Carbon is the central atom in CH4, nitrogen is the central atom in NH 3, and oxygen is the central atom in H2O.d. CH4
Write the Lewis structure for the CO2.
Write Lewis structure that obey the octet rule (duet rule for H) for the following molecule. Carbon is the central atom in CH4, nitrogen is the central atom in NH 3, and oxygen is the central atom in H2O.e. NH3
Draw the Lewis structure for the SO32-.
Write Lewis structure that obey the octet rule (duet rule for H) for the following molecule. Carbon is the central atom in CH4, nitrogen is the central atom in NH 3, and oxygen is the central atom in H2O.f. H2O
Draw the Lewis structure for the PF6-.
Write Lewis structure that obey the octet rule (duet rule for H) for the following molecule. Carbon is the central atom in CH4, nitrogen is the central atom in NH 3, and oxygen is the central atom in H2O.g. HF
Write Lewis structure that obey the octet rule (duet rule for H) for the following molecule.a. H2COCarbon is the central atom in this molecule.
Draw the Lewis structure for the BrF3.
Write the Lewis structure for the diatomic molecule P 2 , an unstable form of phosphorus found in high temperature phosphorus vapor.
Draw the Lewis structure for the HCN.
Write Lewis structure that obey the octet rule (duet rule for H) for the following molecule.b. CO2Carbon is the central atom in this molecule.
Write a Lewis structure for H 2.
Draw the Lewis structure for the N2H2 (skeletal structure HNNH).
Draw the Lewis structure for the N2H4 (skeletal structure H2NNH2).
Write a Lewis structure for HBr.
You may want to reference (Pages 400 - 402) Section 9.7 while completing this problem.Construct a Lewis structure for each of the following molecules.PH3
You may want to reference (Pages 400 - 402) Section 9.7 while completing this problem.Construct a Lewis structure for each of the following molecules.SCl2
Draw the Lewis structure for the CH3NH2 (skeletal structure H3CNH2).
Write a Lewis structure for PCl 3.
You may want to reference (Pages 400 - 402) Section 9.7 while completing this problem.Construct a Lewis structure for each of the following molecules.HI
Write a Lewis structure for SF 2.
You may want to reference (Pages 400 - 402) Section 9.7 while completing this problem.Construct a Lewis structure for each of the following molecules.CH4
Draw the Lewis structure for the C2H2 (skeletal structure HCCH).
Draw the Lewis structure for the C2H4 (skeletal structure H2CCH2).
Write Lewis structure that obey the octet rule (duet rule for H) for the following molecule.c. HCNCarbon is the central atom in this molecule.
Write a Lewis structure for H 2CCH2.
Draw the Lewis structure for the C2H6 (skeletal structure H3CCH3).
Write Lewis structure that obey the octet rule for the following molecule.a. CCl4In this case, the atom listed first is the central atom.
Write a Lewis structure for HNNH.
You may want to reference (Pages 400 - 402) Section 9.7 while completing this problem.Construct a Lewis structure for each molecule: CH2O
You may want to reference (Pages 400 - 402) Section 9.7 while completing this problem.Construct a Lewis structure for each molecule: C2Cl4
Select the Lewis symbols for the ions in each ionic compound.K2O
Write Lewis structure that obey the octet rule for the following molecule.b. NCl3In this case, the atom listed first is the central atom.
You may want to reference (Pages 400 - 402) Section 9.7 while completing this problem.Construct a Lewis structure for each molecule: CH3NH2
Write Lewis structure that obey the octet rule for the following molecule.c. SeCl2In this case, the atom listed first is the central atom.
You may want to reference (Pages 400 - 402) Section 9.7 while completing this problem.Construct a Lewis structure for each molecule: CFCl3 (C central)
Write Lewis structure that obey the octet rule for the following molecule.d. IClIn this case, the atom listed first is the central atom.
Write a Lewis structure for H 2CNH.
You may want to reference (Pages 400 - 402) Section 9.7 while completing this problem.Construct a Lewis structure for each molecule or ion: CI4
You may want to reference (Pages 400 - 402) Section 9.7 while completing this problem.Construct a Lewis structure for each molecule or ion: N2O
You may want to reference (Pages 400 - 402) Section 9.7 while completing this problem.Construct a Lewis structure for each molecule or ion: SiH4
Write a Lewis structure for NO –.
You may want to reference (Pages 400 - 402) Section 9.7 while completing this problem.Construct a Lewis structure for each molecule or ion: Cl2CO
Write a Lewis structure for N 2.
For many years after they were discovered, it was believed that the noble gases could not form compounds. Now we know that belief to be incorrect. A mixture of xenon and fluorine gases, confined in a quartz bulb and placed on a windowsill, is found to slowly produce a white solid. Analysis of the compound indicates that it contains 77.55% Xe and 22.45% F by mass.(b) Write a Lewis structure for the compound.
Write Lewis structure that obey the octet rule for the following molecules and ions. (In this case the first atom listed is the central atom.)a. POCl3, SO42-, XeO4, PO43-, ClO4-
Write a Lewis structure for CO.
Write a Lewis structure for CN –.
Amino acids are the building blocks of proteins. The simplest amino acid is glycine (H2NCH2COOH). Draw a Lewis structure for glycine.
Write a Lewis structure for O 2.
Formic acid is responsible for the sting of ant bites. By mass, formic acid is 26.10% C, 4.38% H, and 69.52% O. The molar mass of formic acid is 46.02 g/mol. Draw its Lewis structure.
Write Lewis structure that obey the octet rule for the following molecules and ions. (In this case the first atom listed is the central atom.)b. NF3, SO32-, PO33-, ClO3-
Draw Lewis structures of the following diatomic molecules and ions. Add formal charges (minimized), if any, to the atoms.
Identify the central atom in each of the following molecules: 
Be sure to answer all parts.Draw the Lewis structure (including all lone pair electrons) with the lowest formal charges and determine the charge of each atom in IF5. What are the formal charges of I and F of IF 5? 
This symbol could represent which of the following elements? 
Using the standard number of expected covalent bonds, predict the formula of carbon bonding to chlorine.
What is the Lewis symbol for the element Nitrogen?
How many lone pairs are on the central atom in BCl 3? Express your answer numerically as an integer.
Given the skeleton structure shown below, what is(are) the correct Lewis electron dot structure(s)? For this question, neglect the formal charges on each atom. 
Given the skeleton structure shown below, what is(are) the correct Lewis electron dot structure(s)? For this question, neglect the formal charges on each atom.
Click the "draw structure" button to launch the drawing utility. Draw the Lewis structure for NF3. 
Given the skeleton structure shown below, what is(are) the correct Lewis electron dot structure(s)? For this question, neglect the formal charges on each atom. 
Draw a Lewis structure for H3O+, Show all unshared electrons and the formal charges. If any. Assume that bonding follows the octel rule.