Ch.10 - Molecular Shapes & Valence Bond TheoryWorksheetSee 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

Whenever we draw a molecule we must take into account two different systems of geometrical shape. 

Electronic Geometry

Concept #1: Understanding Electronic Geometry 

The electronic geometry of a compound treats surrounding elements and lone pairs on the central element as the same.

Example #1: Draw each of the following compounds and determine their electronic geometries.

PH3

Example #2: Draw each of the following compounds and determine their electronic geometries.

BeCl2

Practice: Draw the following compound and determine its electronic geometry. SBr4

Practice: Draw the following compound and determine its electronic geometry. IF3

Practice: Draw the following compound and determine its electronic geometry. H2S

Practice: Draw the following compound and determine its electronic geometry. PO3 -

Molecular Geometry

Concept #2: Understanding Molecular Geometry 

The molecular geometry of a compound treats surrounding elements and lone pairs on the central as different. 

Example #3: Draw each of the following compounds and determine their molecular geometries. 

PH2   

Example #4: Draw each of the following compounds and determine their   molecular geometries. 

XeCl2

Practice: Draw the following compound and determine its molecular geometry. OBr2

Practice: Draw the following compound and determine its molecular geometry. SO 2 -

Additional Problems
Which of the following is best described as T-shaped? a) NH3 b) BCl3 c) XeF3+ d) NO3− e) SO32−
Choose the best Lewis structure for ICl5 .
Please read each question carefully.
Classify these structures according to their valence shell electron pair repulsion geometry. You can use the answers more than once. ____ XY2                           A. octahedral ____ XY2Z                         B. trigonal bipyramidal ____ XY3Z2                       C. tetrahedal ____ XY2Z2                       D. linear                                          E. trigonal planar
If one atom is replaced with a lone pair of electrons from which of the fundamental basic geometries below could you create a molecule having a triangular pyramidal shape? a. linear b. trigonal planar c. octahedral d. tetrahedral e. trigonal bipyramidal
Classify these structures according to their molecular geometry = shape. You can use the answers more than once. ___ XY5            A. octahedral ___ XY3Z2        B. bent (~120°)  ___ XY2Z3        C. trigonal bipyramidal ___ XY2Z2        D. square pyramidal ___ XY4Z2        E. trigonal pyramidal                         F. square planar                         G. linear                         H. bent (~109.5°)                          I. T-shaped                         J. trigonal planar                         K. tetrahedral
What is the electron geometry and molecular geometry if a central atom has four total electron groups with two being bond pairs and two being lone pairs? a. trigonal pyramidal , seesaw b. tetrahedral , trigonal planar c. tetrahedral , bent d. trigonal planar, trigonal planar e. trigonal pyramidal , linear 
What is the expected molecular geometry of IBr 4 +? a. see saw b. trigonal planar c. octahedral d. tetrahedral e. trigonal bipyramidal 
Which is not a possible shape for molecules with trigonal bipyramidal electron group arrangements? (a) Trigonal planar (b) Linear (c) See-saw (d) T-shaped (e) All the above shapes are possible.
What is the electronic geometry around nitrogen in the molecule CH 3CH2NH2? 1. square planar 2. trigonal planar 3. tetrahedral 4. bent 5. linear 6. trigonal pyramidal
What is the molecular geometry of SbCl 52- ? Antimony (Sb) can be an exception to the octet rule, accepting up to twelve electrons. 1. trigonal bipyramidal 2. square planar 3. square pyramidal 4. octahedral 5. seesaw
Give the number of lone pairs around the central atom and the geometry of the ion SeO42–.             A)      0 lone pairs, square planar             B)      1 lone pair, square pyramidal             C)      1 lone pair, distorted tetrahedron (seesaw)             D)      0 lone pairs, tetrahedral             E)      2 lone pairs, square planar
Which one of the following molecules has tetrahedral geometry?  A)  XeF4         B)  BF 3         C)  AsF 5         D) NH 3          E)  CF 4
What type of molecular structure does the XeOF 2 molecule have? (Xe is the central atom) a) trigonal pyramidal b) tetrahedral c) T-shaped d) trigonal planar e) octahedral
Predict the molecular geometry and polarity of the SO 2 molecule.             A)      linear, polar                                           D)      bent, nonpolar             B)      bent, polar                                             E)      None of the above.             C)      linear, nonpolar           
Select the correct molecular structure for SO 3 from the choices below: a) T-shaped b) trigonal planar c) tetrahedral d) octahedral e) trigonal bipyramid
The predicted geometry of ICl3 would be 1. trigonal pyramidal. 2. linear. 3. trigonal bipyramidal. 4. T-shaped. 5. trigonal planar.
Which of the following is best described as T - shaped? a) NH3 b) BCl3 c) XeF3 +  d) NO3 −  e) SO3 2−
What is the molecular geometry of ICl 4-? T-shaped Trigonal bipyramidal Seesaw Tetrahedral Square planar
What are the electron group geometries of the labeled carbon and oxygen atoms in aspartic acid? a) trigonal pyramidal and bent b) trigonal pyramidal and tetrahedral c) trigonal planar and tetrahedral d) tetrahedral and bent e) trigonal planar and bent
Use VSEPR theory to predict the electron domain geometry of CS 2. a) bent b) linear c) trigonal planar d) tetrahedral e) octahedral
What are the molecular geometries of the labeled carbon and nitrogen atoms in caffeine? a) trigonal pyramidal and tetrahedral b) trigonal pyramidal and trigonal planar c) trigonal planar and tetrahedral d) trigonal planar and trigonal pyramidal e) Tetrahedral and tetrahedral
What is the molecular geometry around a central atom that has three bonding pairs and one lone electron-pair? a) bent b) linear c) trigonal-planar d) trigonal-pyramidal e) trigonal-bipyramidal
Determine the electron geometry (eg) and molecular geometry (mg) of BrF 3. a) eg=trigonal planar, mg=trigonal planar b) eg=trigonal bipyramidal, mg=T-shape c) eg=trigonal planar, mg=bent d) eg=trigonal bipyramidal. mg=see-saw e) eg=tetrahedral, mg=trigonal pyramidal
The molecule of the type ML4 consists of four single bonds and no lone pairs. What structure is it expected to assume? A) square planar B) trigonal planar C) trigonal pyramidal D) tetrahedral
The shape that most closely describes the NF3, molecule is a) octahedral. b) trigonal planar. c) trigonal pyramidal. d) tetrahedral.
When drawing a compound you have to take into account two different systems of geometrical shape. With the MOLECULAR geometry you treat lone pairs (nonbonding electrons) and surrounding elements as different.   With the ELECTRONIC geometry you treat lone pairs (nonbonding electrons) and surrounding elements as the same. They are both treated as X.  
In which pair are the molecules geometricaly similar? a) SO2 and CO2 b) PH3 and BF3 c) CO2 and OF2 d) SO2 and O3
Which is planar? a) NH3 b) SO32- c) CO32- d) CCl4
Which is linear? a) H2S b) NH3 c) NO2 d) CO2
Consider the given Lewis structure for BrF5. What is the predicted shape for the molecule as a whole? a) square pyramidal b) trigonal bipyramidal c) trigonal pyramidal  d) octahedral
What is the shape of the XeF4, molecule? a) square planar b) trigonal bipyramidal c) tetrahedral d) trigonal pyramidal
Use VSEPR theory to predict the geometry of the PCl 3 molecule.
NH3 (pyramidal geometry) reacts with BF3 (planar geometry) to form the addition compound, H3NBF3. What is the geometry around the nitrogen and boron centers in the addition compound? a) Both centers are tetrahedral. b) Nitrogen is tetrahedral; boron is linear.  c) Nitrogen is pyramidal; boron is planar. d) Nitrogen is planar; boron is pyramidal. 
Identify the number of electron groups in XeF2 a.  2             b.  3                 c.  4                 d.  5                 e.  6
Which compound would be expected to have the largest dipole moment? a) CO2 (linear) b) SO2 (bent) c) BF3 (trigonal planar) d) CF4 (tetrahedral)
Knowing that F is more electronegative than either B or P, what conclusion can be drawn from the fact that BF3 has no dipole moment, but PF3 does? a) BF3 is not spherically symmetrical, but PF3 is. b) The BF3 molecule must be trigonal planar. c) The BF3 molecule must be linear.  d) The atomic radius of P is larger than the atomic radius of B.
What is the molecular shape of the XeF 5+ ion? 1. tetrahedral 2. square pyramidal 3. trigonal bipyramidal 4. trigonal pyramidal 5. octahedral
Dot structures are given below for several compounds containing iodine (lone pairs are shown only for the central atom). Draw the structure and name the molecular geometry from the following list: linear, bent, T-shaped, see-saw, trigonal pyramidal, trigonal planar, trigonal bipyramidal, square planar, square pyramidal, tetrahedral, octahedral. 
Dot structures are given below for several compounds containing iodine (lone pairs are shown only for the central atom). Draw the structure and name the molecular geometry from the following list: linear, bent, T-shaped, see-saw, trigonal pyramidal, trigonal planar, trigonal bipyramidal, square planar, square pyramidal, tetrahedral, octahedral. 
Choose the correct description for SiOH 2. NOTE: Si is the CENTRAL atom and all the other atoms are attached to Si.  1. polar, pyramidal 2. polar, trigonal planar 3. non-polar, T-shaped 4. polar, T-shaped 5. polar, tetrahedral 6. non-polar, pyramidal 7. non-polar, tetrahedral 8. non-polar, trigonal planar
The molecular geometry of ICl2− is 1. trigonal planar. 2. octahedral. 3. trigonal bipyramidal. 4. tetrahedral. 5. linear.
Which of the following has a trigonal planar geometry? 1. FNO2 (N is central) 2. SO3 2– 3. BrO3 –  4. CH3 –
Which of the following molecules has a nonlinear structure? a) XeF2 b) BeCl2 c) SeO2 d) CO2 e) N2O (central atom is N)
What is the molecular geometry of SeF5 - ? 1. see-saw 2. square pyramidal 3. octahedral 4. trigonal bipyramidal
What type of molecular structure does the XeOF 2 molecule have? (Xe is the central atom) a). trigonal pyramidal b) tetrahedral c) T-shaped d) trigonal planar e) octahedral
Consider the polyatomic ion PCl 4- and its three dimensional structure. What is the electronic geometry and the molecular geometry for this ion? 1. tetrahedral; tetrahedral 2. trigonal bypyramidal; tetrahedral 3. octahedral; square planar 4. octahedral; square pyramidal 5. trigonal bipyramidal; T-shaped 6. trigonal bipyramidal; seesaw
What are the electronic and molecular geometries of the molecule BrF 5? 1. octahedral, trigonal bipyramidal 2. trigonal bipyramidal, square pyramidal 3. ocahedral, square pyramidal 4. trigonal bipyramidal, trigonal bipyramdal 5. octahedral, octahedral
Which of the following has a trigonal bipyramidal structure? a) PCl5 b) IF5 c) NH3 d) I3− e) Two of these four molecules
Tetrahedral shape of CCl4.In the space-filling model, what determines the relative sizes of the spheres?
An AB4 molecule has no lone pairs of electrons on the A atom. What is its molecular geometry?
Derivatives of the tetrahedral molecular shape. In going from the tetrahedral shape to the bent shape, does it matter which two of the atoms we choose to remove?
Determine the molecular geometry around the carbon atom in COF2, using VSEPR theory.
Determine the molecular geometry around the sulfur atom in S2Cl2, using VSEPR theory.
Determine the molecular geometry around the sulfur atom in SF4, using VSEPR theory.
Determine the molecular geometry for ClF3.
How does a trigonal pyramid differ from a tetrahedron so far as molecular geometry is concerned?
Determine the molecular geometry around the iodine atom in IF5, using VSEPR theory.
Determine the molecular geometry around each carbon atom located at the ends of the molecule CH2CHCH3, using VSEPR theory.
Determine the molecular geometry for SF4.
Determine the molecular geometry around the carbon and the sulfur atoms in CH3SH, using VSEPR theory.
This figure shows ball-and-stick drawings of three possible shapes of an AF3 molecule. Which of the following elements will lead to an AF3 molecule with the shape in (ii): Li, B, N, Al, P, Cl?
Determine the molecular geometry of BrF5.
Determine the molecular geometry of SCl6.
Determine the molecular geometry of PF5.
In a trigonal-bipyramidal geometry, there are two types of positions for the outer atoms.What is the bond angle formed by an axial atom, the central atom, and any equatorial atom?
Consider the molecule PF4 Cl.Predict the molecular geometry of PF4 Cl.
Consider the molecule PF4 Cl.Would you expect the molecule to distort from its ideal electron domain geometry?
The Lewis structure for allene is shown in the diagram. Is the molecule planar?
Why is molecular geometry important?
Azo dyes are organic dyes that are used for many applications, such as the coloring of fabrics. Many azo dyes are derivatives of the organic substance azobenzene, C12 H10 N2. A closely related substance is hydrazobenzene, C12 H12 N2. The Lewis structures of these two substances are showin in the diagram. (Recall the shorthand notation used for organic molecules.)All the atoms of azobenzene lie in one plane, whereas those of hydrazobenzene do not. Is this observation consistent with the statement in part F?
How do you apply VSEPR theory to predict the shape of a molecule with more than one interior atom?
An AB5 molecule adopts the geometry shown below. What is the name of this geometry?
An AB5 molecule adopts the geometry shown below. Suppose the atoms B are halogen atoms. Of which group in the periodic table is atom A a member?
What is the molecular geometry about nitrogen in CH3NH2?
Each of the following ball-and-stick models shows wrong electron and molecular geometry of a generic molecule.Provide the correct molecular geometry for (a), given the number of lone pairs and bonding groups on the central atom.
Each of the following ball-and-stick models shows wrong electron and molecular geometry of a generic molecule.Provide the correct molecular geometry for (b), given the number of lone pairs and bonding groups on the central atom.
Each of the following ball-and-stick models shows wrong electron and molecular geometry of a generic molecule.Provide the correct molecular geometry for (c), given the number of lone pairs and bonding groups on the central atom.
Determine the molecular geometry of CS2.
Determine the molecular geometry of CO2.
Determine the molecular geometry of CCl4.
Which geometry would you expect in the series BH4-, CH4, NH4+?
The PH3 molecule is polar. Does this offer experimental proof that the molecule cannot be planar? Explain.
Acetone, (CH3 )2 CO, is widely used as an industrial solvent.Predict the geometry around the central carbon atom.
Acetone, (CH3 )2 CO, is widely used as an industrial solvent.Predict the geometry around the terminal C atoms.
Predict the molecular geometry for the following molecule:
Predict the molecular geometry for the following molecule:
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.Would you expect the molecule to be planar for both Lewis structures?
Give the electron-domain and molecular geometries of a molecule that has the following electron domains on its central atom.
Give the electron-domain and molecular geometries of a molecule that has the following electron domains on its central atom.four bonding domains and two nonbonding domains
Imagine that a molecule with six electron groups is confined to two dimensions and therefore has a hexagonal planar electron geometry. If two of the six groups are lone pairs, where are they located?
Give the electron-domain and molecular geometries for the following molecules and ions.HCN
Give the electron-domain and molecular geometries for the following molecules and ions.HCN
Give the electron-domain and molecular geometries for the following molecules and ions.SO32-
Give the electron-domain and molecular geometries for the following molecules and ions.SO32-
Give the electron-domain and molecular geometries for the following molecules and ions.SF4
Give the electron-domain and molecular geometries for the following molecules and ions.SF4
Give the electron-domain and molecular geometries for the following molecules and ions.PF6-
Give the electron-domain and molecular geometries for the following molecules and ions.PF6-
Give the electron-domain and molecular geometries for the following molecules and ions.NH3Cl+
Give the electron-domain and molecular geometries for the following molecules and ions.NH3Cl+
Give the electron-domain and molecular geometries for the following molecules and ions.N3-
Give the electron-domain and molecular geometries for the following molecules and ions.N3-
This figure shows ball-and-stick drawings of three possible shapes of an AF3 molecule. Name one of the possible elements A those are expected to lead to the AF3 structure shown in (iii).
The compound C3H4 has two double bonds.Describe its bonding and geometry, using a valence bond approach.
How would we modify the figure if we were looking at PH3 rather than NH3?
The ion CH5+, can form under very special high-energy conditions in the vapor phase in a mass spectrometer.Predict the geometry for CH5+.
Draw the Lewis structure for acetamide (CH3CONH2), an organic compound, and determine the geometry about each interior atom. Experiments show that the geometry about the nitrogen atom in acetamide is nearly planar. What resonance structure can account for the planar geometry about the nitrogen atom?In resonance structure that would have a trigonal pyramidal molecular geometry around the nitrogen determine the electron geometry about each interior atom.
Draw the Lewis structure for acetamide (CH3CONH2), an organic compound, and determine the geometry about each interior atom. Experiments show that the geometry about the nitrogen atom in acetamide is nearly planar. What resonance structure can account for the planar geometry about the nitrogen atom?In resonance structure that would have a planar molecular geometry around the nitrogen determine the electron geometry about each interior atom.
The molecule H2S4 has a linear arrangement of its atoms. Number all sulfur atoms along the chain from 1 to 4.Find the oxidation number of each sulfur in the molecule from the first to the fourth.
Consider the molecule PF4 Cl.If so, how would it distort?
In addition to tetrahedral, another common shape for AB4 molecules is square planar. All five atoms lie in the same plane, with the B atoms at the corners of a square and the A atom at the center of the square. Which shape in the figure below could lead to a square-planar shape upon removal of one or more atoms?
What is the geometry of the HCN molecule?
According to VSEPR theory, what determines the geometry of a molecule?
Identify the five basic electron geometries and state the number of electron groups corresponding to each.
Explain the difference between electron geometry and molecular geometry.
Give the correct electron and molecular geometry that corresponds to each set of electron groups around the central atom of a molecule.four electron groups overall; three bonding groups and one lone pair
Give the correct electron and molecular geometry that corresponds to each set of electron groups around the central atom of a molecule.four electron groups overall; two bonding groups and two lone pairs
Give the correct electron and molecular geometry that corresponds to each set of electron groups around the central atom of a molecule.five electron groups overall; four bonding groups and one lone pair
Give the correct electron and molecular geometry that corresponds to each set of electron groups around the central atom of a molecule.five electron groups overall; three bonding groups and two lone pairs
Give the correct electron and molecular geometry that corresponds to each set of electron groups around the central atom of a molecule.five electron groups overall; two bonding groups and three lone pairs
Give the correct electron and molecular geometry that corresponds to each set of electron groups around the central atom of a molecule.six electron groups overall; five bonding groups and one lone pair
Give the correct electron and molecular geometry that corresponds to each set of electron groups around the central atom of a molecule.six electron groups overall; four bonding groups and two lone pairs
At least two different numbers of electron groups can result in a linear molecule. What are they?
In which of these molecules or ions does the presence of nonbonding electron pairs produce an effect on molecular shape, assuming they are all in the gaseous state?
An AB2 molecule is described as linear, and the A-B bond length is known.Does this information completely describe the geometry of the molecule?
In many reactions the addition of AlCl3 produces the same effect as the addition of H+.Determine AlCl3 structure using the VSEPR method.
Give the electron-domain and molecular geometries of a molecule that has the following electron domains on its central atom.four bonding domains and no nonbonding domains,
Give the electron-domain and molecular geometries of a molecule that has the following electron domains on its central atom.three bonding domains and two nonbonding domains,
Give the electron-domain and molecular geometries of a molecule that has the following electron domains on its central atom.five bonding domains and one nonbonding domain.
An AB4 molecule has one lone pair of electrons on the A atom (in addition to the four B atoms). What is the electron-domain geometry around the A atom?
This figure shows ball-and-stick drawings of three possible shapes of an AF3 molecule. For each shape, give the electron-domain geometry on which the molecular geometry is based.
This figure shows ball-and-stick drawings of three possible shapes of an AF3 molecule. For each shape, how many nonbonding electron domains are there on atom A?
Use VSEPR to predict the geometry (including bond angles) about each interior atom of methyl azide (CH3N3), and make a sketch of the molecule. Would you expect the bond angle between the two interior nitrogen atoms to be the same or different? Would you expect the two nitrogen-nitrogen bond lengths to be the same or different?Determine the electron geometry about each interior atom for all resonance structures.
For each molecule, indicate how many different electron-domain geometries are consistent with the molecular geometry shown.
For each molecule, indicate how many different electron-domain geometries are consistent with the molecular geometry shown.
For each molecule, indicate how many different electron-domain geometries are consistent with the molecular geometry shown.
For each molecule, indicate how many different electron-domain geometries are consistent with the molecular geometry shown.
For each molecule, indicate how many different electron-domain geometries are consistent with the molecular geometry shown.
For each molecule, indicate how many different electron-domain geometries are consistent with the molecular geometry shown.
Relative volumes occupied by bonding and nonbonding electron domains.Why is the volume occupied by the nonbonding electron pair domain larger than the volume occupied by the bonding domain?
Consider the molecule PF4 Cl.Predict its electron-domain geometry.
Consider the molecule PF4 Cl.Which would you expect to take up more space, a P-F bond or a P-Cl bond?
In determining electron geometry, why do we consider only the electron groups on the central atom? In other words, why don’t we consider electron groups on terminal atoms? Explain.
Suppose a particular AB3 molecule has the resonance structure How many electron domains are there around the A atom?
The anion (v) is called "BARF" by chemists, as its common abbreviation sounds similar to this word. What is the central atom and the number of electron-pair domains around the central atom in each of these anions?
An AB3 molecule is described as having a trigonal-bipyramidal electron-domain geometry.How many nonbonding domains are on atom A?
What constitutes an electron group?
Name the five basic electron geometries.
An AB5 molecule adopts the geometry shown below. Do you think there are any nonbonding electron pairs on atom A?
A molecule with the formula AB3 has a trigonal pyramidal geometry.How many electron groups are on the central atom (A)?
The following figures show several molecular geometries.Give the number of total electron groups, the number of bonding groups, and the number of lone pairs for (a) geometry.
The following figures show several molecular geometries.Give the number of total electron groups, the number of bonding groups, and the number of lone pairs for (b) geometry.
The following figures show several molecular geometries.Give the number of total electron groups, the number of bonding groups, and the number of lone pairs for (c) geometry.
An AB2 molecule is described as linear, and the A-B bond length is known.Can you tell how many nonbonding pairs of electrons are around the A atom from this information?
How many nonbonding electron pairs are there in each of the following molecules?(CH3) 2S
How many nonbonding electron pairs are there in each of the following molecules?HCN
How many nonbonding electron pairs are there in each of the following molecules?H2C2
How many nonbonding electron pairs are there in each of the following molecules?CH3F
Which of these molecules are linear? Check all that apply.a. SF2b. XeF2c. BeCl2d. NO2-
Consider nitrous acid, HNO2 (HONO).(b) What are the electron pair and molecular geometries of the internal oxygen and nitrogen atoms in the HNO2 molecule?
What is the molecular shape of sulfur dioxide, SO 2, (i.e., what is the atom geometry around the central atom)? A) linear B) trigonal planar C) bent D) trigonal pyramidal
What is the molecular Geometry of NO 2?
Why does NO3- have a molecular geometry shape of trigonal planar?? Isn't it true that in order to be  trigonal planar there should be 4 bonded pairs and 0 lone pairs?
a) Select all of the equatorial atoms on the structure below.  b) What is the shape of this molecule?
White phosphorous is composed of molecules of P4 in which each P atom is connected to three other P atoms in the shape of a tetrahedron. Does it obey the octet rule?1. No2. Yes3. Unable to determine
What is the molecular geometry of NH 3? a. Trigonal planar b. Tetrahedral c. Triangular pyramid d. Bent
What is the electronic geometry of H 2O?
What is the molecular geometry of PCl 3?
Draw the Lewis electron-dot structures for the 3 isomers of C 2H2Cl2. Use models to deduce the shape and polarity of each isomer.
According to VSEPR theory, the geometry of the PH 3 molecule is best described as: linear, trigonal planar, tetrahedral, bent, or trigonal pyramidal.
Predict the shape of:a. SF5+b. NO3-c. SO42-d. O3e. N2O
The molecular geometry of the SF2 molecule is a) linear. b) bent. c) trigonal planar. d) tetrahedral. e) octahedral.
Determine the molecular geometry, or shape, of ClO 2 A) octahedral B) tetrahedral C) trigonal bipyramidal D) trigonal planar E) t-shaped F) bent
The molecular geometry of the CH 3+ ion is best described as _______________ .
What is the electron geometry of NF 3?  
Determine the molecular geometry of ClF3.
Consider the following moleculesi) BrF3, ii) SO42-, iii) ClO2, and iv) SO2,A) Draw ONE appropriate Lewis structure for each of the four chemical species listed above.B) What are the electron domain geometries surrounding the central atoms?
Determine the molecular geometry of BrF2-. 
Which of the following statements is  incorrect?Ionic bonding results from the transfer of electrons from one atom to another.Dipole moments result from the unequal distribution of electron in a molecule.The electrons in a polar bond are found nearer to the more electronegative element.A molecule with very polar bonds can be nonpolarLinear molecules cannot have a net dipole moment 
Determine the molecular geometry of ClF4-.
Determine molecular geometry of BrF5.
Draw the Lewis structure for CCl 4. What is the molecular geometry of this compound? Is the molecule polar or nonpolar?
What is the molecular shape of the XeF5+ ion? 1. tetrahedral 2. square pyramidal  3. trigonal bipyramidal 4. trigonal pyramidal 5. octahedral
Predict the molecular shape of methane, the carbonate ion, carbon dioxide, and the sulfite ion.
After drawing the Lewis structure determine what the molecular geometry of PCl 3 is  a) trigonal bipyramidal b) square planar c) trigonal planar d) V-shaped e) trigonal pyramidal
How many outer atoms and lone pairs are present in a molecule with a square pyramidal shape?
What is the electron pair geometry and Molecular geometry of SCl 2?  
What is the molecular geometry of a molecule with: i) 4 outer atoms and 1 lone pair on the central atom? ii) 2 outer atoms and 2 lone pairs on the central atom? iii) 4 outer atoms and 2 lone pairs on the central atom?
Draw the lewis structure of Cl2O2 based on this structure Cl-Cl with the 2 Oxygen's branching off of the Chlorine. Do not add formal charges. Then, what is the geometry about the central chlorine atom?
What is the molecular geometry of H3O+, hydronium ion?
Draw the Lewis structure of chlorous acid (HClO 2).The result is that around Cl there are ___ (a number) bonding groups and ___ lone pair(s) of electrons. The number and types of structural groups aroud Cl corresponds to the shape called _____ (one 4-letter word). The number and types of structural groups aroud Cl leads to the conclusion that the bonding groups are arranged around Cl in a(n) _____ (a 10 letter word) arrangement. 
The central atom of a molecule has three lone pairs and is bonded to each of two other atoms with a single bond. What is the molecular geometry (shape) of the molecule? a) Linear b) Trigonal planar c) Trigonal bipyramidal d) Octahedral e) Square Planar
For the molecule CO2a) Draw the Lewis structure.b) Determine the geometry.c) Determine whether the compound is polar or non-polar.
According to the VSEPR theory, the shape of the SO 3 molecule is a. trigonal planar b. pyramidal c. square planar d. tetrahedral e. distorted tetrahedron (seesaw)
The molecular shapes of XeF4, BrF5, SF4 and ClO3− are respectively described as:a. octahedral; T-shaped; square planar; T-shapedb. see-saw; square planar; T-shaped; tetrahedralc. tetrahedral; see-saw; tetrahedral; octahedrald. square planar; square pyramidal; see-saw; trigonal pyramidal e. see-saw; octahedral; T-shaped; square planar
a. Predict the molecular geometry of ClNO.b. Enter the molecular geometry of ClNO.
a) Select all of the equatorial atoms on the structure below. b) What is the shape of this molecule?
What is the correct  electron geometry of SeF4? a. tetrahedral b. square pyramid c. triangular bipyramid d. see saw e. t-shaped
Consider the polar chemical species XeO2Cl22- . A) Draw the Lewis electron dot diagram. B) Draw a diagram, show and state the geometry around the central atom.
What is the electron-domain (charge-cloud) geometry of ICl 5? Enter the electron-domain geometry of the molecule.
Which of these molecules are linear? Check all that apply. a) NO2- b) XeF2 c) BeCl2 d) SF2
What is the molecular shape of C2H2? What is the geometry of electron pairs around its central atom?
Draw the Lewis structure of H2O. Include any nonbonding electron pairs. Include all lone pairs of electrons.What is the electronic geometry of H2O?What is the electronic geometry of ClF3?What is the electronic geometry of BBr3?
For which of the following compounds is the molecular geometry and electron geometry the same? A. NBr3 B. ICI5 C. NH4+ D. BrF2- E. XeF2
For the following molecules or ions, draw a VSEPR picture showing the approximate geometry and the positions of all bonded pairs and lone pairs. Also name the shape of the structure (considering only the position of the nuclei and not the lone pairs) and the hybridization scheme used by the central atom in its bonding.
Dot structures are given below for several compounds containing iodine (lone pairs are shown only for the central atom). Draw the structure and name the molecular geometry from the following list: linear, bent, T-shaped, see-saw, trigonal pyramidal, trigonal planar, trigonal bipyramidal, square planar, square pyramidal, tetrahedral, octahedral. 
The electronic arrangement is the same as the molecular shape when A. the molecule is not polar. B. the number of bonding orbitals equals the number of anti-bonding orbitals. C. there are no lone pairs of electrons on the central atom. D. the atoms are joined by sigma bonds. E. there are more shared electrons than non-shared electrons.
What is the molecular shape of BrF 3 as predicted by the VSEPR theory? A) Trigonal planar B) Tetrahedral C) Trigonal bipyramidal D) T-shaped
An AB4 molecule has two lone pairs of electrons on the A atom (in addition to the four B atoms). Predict the molecular geometry.
If you react BF3 to make the ion BF32-, is this ion planar?
You may want to reference (Pages 343 - 351) Section 9.2 while completing this problem.Name the proper three-dimensional molecular shapes for each of the following molecules or ions, showing lone pairs as needed: (a) ClO2– (b) SO42– (c) NF3 (d) CCl2Br2 (e) SF42+
Determine the molecular geometry IF2–.
Determine the molecular geometry IBr4–.
Explain why BrF4– is square planar, whereas BF4– is tetrahedral.
Sulfur tetrafluoride (SF4) reacts slowly with O2 to form sulfur tetrafluoride monoxide (OSF4) according to the following unbalanced reaction: SF4(g) + O2(g) → OSF4(g). The O atom and the four F atoms in OSF4 are bonded to a central S atom.Based on the electron-domain geometry there are two possible molecular geometries for this molecule (shown below). For the two possible molecular geometries, state how many fluorines are equatorial and how many are axial.
Amino acids are biological compounds that link together to form proteins, the workhorse molecules in living organisms.Determine the molecular geometry about each interior atom.
Determine the molecular geometry of IF4 + .
The figure  that follows contains ball-and-stick drawings of three possible shapes of an AF4 molecule.Name an element A that is expected to lead to the AF4 structure shown in (i).
The formulas of several chemical substances are given in the table below. For each substance in the table, give its chemical name and predict its molecular structure.
Predict the molecular geometry about nitrogen in the molecule CH3NHCH3.
The following electrostatic potential diagram represent CH4, NH3, or H2O. Label and explain your choice.
What is the molecular geometry of the bromate ion, BrO3–?a. square planarb. trigonal planarc. square pyramidald. tetrahedrale. trigonal pyramidal
You may want to reference (Pages 338 - 393) Chapter 9 while completing this problem.The molecule IF7 has a pentagonal bipyramid structure: five fluorines are equatorial, forming a flat pentagon around the central iodine atom, and the other two fluorines are axial. Predict the molecular geometry of IF6–.
Write Lewis structures and predict the molecular structures of the following. Which of these compounds are polar?a. OCl2, KrF2, BeH2, SO2
Complete the following resonance structures for POCl 3.a. Would you predict the same molecular structure from each resonance structure?
Indicate whether each statment is true or false.Lone pairs of electrons on an atom in a molecule influence the shape of a molecule.
Write Lewis structures and predict the molecular structures of the following. Which of these compounds are polar?b. SO3, NF3, IF3
Write Lewis structures and predict the molecular structures of the following. Which of these compounds are polar?c. CF4, SeF4, KrF4
Write Lewis structures and predict the molecular structures of the following. Which of these compounds are polar?d. IF5, AsF5
The allene molecule has the following Lewis structure:Must all hydrogen atoms lie the same plane? If not, what is their spatial relationship? Explain.
Consider an AB3 molecule in which A and B differ in electronegativity. You are told that the molecule has an overall dipole moment of zero. Which of the following could be the molecular geometry of the molecule?
Determine the molecular geometry of SCl 4.
The structure of TeF 5- isDraw a complete Lewis structure for TeF 5-, and explain the distortion from the ideal square pyramidal structure. (See Exercise 26.)Exercise 26:Two variations of the octahedral geometry (see Table 4‑1) are illustrated below.Which of the compounds/ions Br3-, ClF3, XeF4, SF4, PF5, ClF5, and SF6 have these molecular structures?
Determine the molecular geometry of CBr4.
Determine the molecular geometry of SeF4.
The molecules BF3, CF4, CO2, PF5, and SF6 are all nonpolar, even though they all contain polar bonds. Why?
Identify the molecular geometry of CCl4.
You may want to reference (Pages 439 - 440) Section 10.4 while completing this problem.Predict the molecular geometry of I3–.
A certain AB4 molecule has a "seesaw" shape:.From which of the fundamental geometries shown in Figure 9.3 in the textbook (available from the eText link) could you remove one or more atoms to create a molecule having this seesaw shape?
Which molecule geometry results when a central atom has five total electron groups, with three of those being bonding groups and two being lone pairs?
Exercise 99:Write Lewis structures that obey the octet rule for the following species. Assign the formal charge for each central atom.a. POCl3                            e. SO   2Cl2b. SO42-                             f. XeO   4c. ClO4-                             g. ClO   3-d. PO43-                            h. NO   43-Exercise 100:Write Lewis structures for the species in Exercise 99 that involve minimum formal charges.Refer back to the formal charge Exercises 99 and 100 from Chapter 3. Would you make the same prediction for the molecular structure for each case using the Lewis structure obtained in Exercise 99 as compared with the one obtained in Exercise 100?
Determine the correct molecular geometry (from left to right) about each interior atom in CH3CH2OH.
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.On the basis of formal charges, which is more stable, the linear molecule or the tetrahedral molecule?
Predict the molecular geometry about xenon in XeF4.
a. What is the molecular geometry of PF3? Enter the molecular geometry of the molecule.b. What is the molecular geometry of BeF2? Enter the molecular geometry of the molecule.c. What is the molecular geometry of OF2? Enter the molecular geometry of the molecule.
Predict the molecular geometry about the carbon atom in HCN.
Give the molecular shape of each species:(a) PF5
Give the molecular shape of each species:(b) CCl4
Give the molecular shape of each species:(c) H3O+
Give the molecular shape of each species:(d) ICl3
Give the molecular shape of each species:(e) BeH2
Give the molecular shape of each species:(f) PH2−
Give the molecular shape of each species:(g) GeBr4
Give the molecular shape of each species:(h) CH3−
Give the molecular shape of each species:(i) BCl3
Give the molecular shape of each species:(j) BrF4+
Give the molecular shape of each species:(k) XeO3
An AB3 molecule is described as having a trigonal-bipyramidal electron-domain geometry. Based on the information given, which of the following is the molecular geometry of the molecule: (i) trigonal planar, (ii) trigonal pyramidal, (iii) T-shaped, or (iv) tetrahedral?
Give the molecular shape of each species:(l) TeF4
Consider the following reaction of silicon tetrafluoride:SiF4 + F− ⟶ SiF5−(a) Which depiction below best illustrates the change in molecular shape around Si?
Consider the following reaction of silicon tetrafluoride:SiF4 + F− ⟶ SiF5−(b) Give the name and AXmEn designation of each shape in the depiction below.
The VSEPR model was developed before any xenon compounds had been prepared. Thus, these compounds provided an excellent test of the model’s predictive power. What would you have predicted for the shapes of XeF2, XeF4, and XeF6?
Which of the compounds/ions Br 3-, ClF3, XeF4, SF4, PF5, ClF5, and SF6 have these molecular structures?
Which of the compounds/ions Br 3-, ClF3, XeF4, SF4, PF5, ClF5, and SF6 have these molecular structures?
Chloral, Cl3C—CH=O, reacts with water to form the sedative and hypnotic agent chloral hydrate, Cl3C—CH(OH)2. Draw Lewis structures for these substances, and describe the change in molecular shape, if any, that occurs around each of the carbon atoms during the reaction.
The gas-phase reaction of NO with F2 to form NOF and F has an activation energy of Ea = 6.3 kj/mol and a frequency factor of A = 6.0 x 108 M-1 s - 1. The reaction is believed to be bimolecular:NO(g) + F2 (g) → NOF (g) + F(g).Predict the shape for the NOF molecule.
Predict which molecules, if any, are planar: ethane (C2H6), ethylene (C2H4), and acetylene (C2H2).
The phosphorus trihalides (PX3) show the following variation in the bond angle X–P–X: PF3, 96.3˚; PCl3, 100.3˚; , 101.0  ; Pl3{ m Pl_3}, 102.0˚. The trend is generally attributed to the change in the electronegativity of the halogen.Using the VSEPR model, explain the observed trend in X–P–X angle as the electronegativity of X changes. Based on your answer, predict the structure of PBrCl4.
Except for nitrogen, the elements of Group 5A(15) all form pentafluorides, and most form pentachlorides. The chlorine atoms of PCl5 can be replaced with fluorine atoms one at a time to give, successively, PCl4F, PCl3F2, … , PF5. (a) Given the sizes of F and Cl, would you expect the first two F substitutions to be at axial or equatorial positions? Explain. 
A student isolates a product with the molecular shape shown (F is orange).(a) If the species is a neutral compound, can the black sphere represent selenium (Se)? 
A student isolates a product with the molecular shape shown (F is orange).(b) If the species is an anion, can the black sphere represent N?
A student isolates a product with the molecular shape shown (F is orange). (c) If the black sphere represents Br, what is the charge of the species?
Consider the following molecular shapes:(a) Match each shape with one of the following species: XeF3+, SbBr3, GaCl3.
Describe the molecular structure around the indicated atom or atoms:(a) the sulfur atom in sulfuric acid, H2SO4 [(HO)2SO2]
Consider the following molecular shapes:(c) Which has the most valence electrons around the central atom?
Determine the molecular geometry for each molecule.a. PF3b. SBr2c. CHCl3d. CS2
Describe the molecular structure around the indicated atom or atoms:(b) the chlorine atom in chloric acid, HClO3 [HOClO2]
Describe the molecular structure around the indicated atom or atoms:(c) the oxygen atom in hydrogen peroxide, HOOH
Describe the molecular structure around the indicated atom or atoms:(d) the nitrogen atom in nitric acid, HNO3 [HONO2]
Describe the molecular structure around the indicated atom or atoms:(e) the oxygen atom in the OH group in nitric acid, HNO3 [HONO2]
Describe the molecular structure around the indicated atom or atoms:(f) the central oxygen atom in the ozone molecule, O3
Phosphorus pentachloride, a key industrial compound with annual world production of about 2×107 kg, is used to make other compounds. It reacts with sulfur dioxide to produce phosphorus oxychloride (POCl3) and thionyl chloride (SOCl2). Draw a Lewis structure and name the molecular shape of each of these products.
Describe the molecular structure around the indicated atom or atoms:(g) each of the carbon atoms in propyne, CH3CCH
Determine the molecular geometry about each interior carbon atom of this molecule.a. C2H2 (skeletal structure HCCH)b. C2H4 (skeletal structure H2CCH2)c. C2H6 (skeletal structure H3CCH3)
Describe the molecular structure around the indicated atom or atoms:(h) the carbon atom in Freon, CCl2F2
Describe the molecular structure around the indicated atom or atoms:(i) each of the carbon atoms in allene, H2CCCH2
Draw the Lewis structures and predict the shape of each compound or ion:(a) CO2
Draw the Lewis structures and predict the shape of each compound or ion:(b) NO2−
Draw the Lewis structures and predict the shape of each compound or ion:(c) SO3
Determine the molecular geometry about interior carbon atom in CH3OH.
Draw the Lewis structures and predict the shape of each compound or ion:(d) SO32−
Determine the molecular geometry about interior oxygen atom in CH3OH.
Determine the molecular geometry about each interior carbon atom in CH3OCH3.
Determine the molecular geometry about interior oxygen atom in CH3OCH3.
Determine the molecular geometry about interior oxygen atom in H2O2.
Determine the molecular geometry for each molecule.CF4NF3OF2H2S
Draw the Lewis electron dot structures for these molecules, including resonance structures where appropriate:(d) predict the molecular shapes for CS32− and CS2 and explain how you arrived at your predictions
Determine the molecular geometry about each interior nitrogen atom of N2H2.
Determine the molecular geometry about each interior nitrogen atom of N2H4.
Each of the following ball-and-stick models shows the wrong electron and molecular geometry of a generic molecule.Provide the correct molecular geometry for (a), given the number of lone pairs and bonding groups on the central atom.
Each of the following ball-and-stick models shows the wrong electron and molecular geometry of a generic molecule.Provide the correct molecular geometry for (b), given the number of lone pairs and bonding groups on the central atom.
Each of the following ball-and-stick models shows the wrong electron and molecular geometry of a generic molecule.Provide the correct molecular geometry for (c), given the number of lone pairs and bonding groups on the central atom.
The genetic code is based on four different bases with the following structures.Assign a molecular geometry to each interior atom in cytosine.
The genetic code is based on four different bases with the following structures.Assign a molecular geometry to each interior atom in adenine.
Predict the molecular geometry for the following molecule:
The genetic code is based on four different bases with the following structures.Assign a molecular geometry to each interior atom in thymine.
The genetic code is based on four different bases with the following structures.Assign a molecular geometry to each interior atom in guanine.
Consider the following XF4 ions: PF4–, BrF4–, ClF4+, and AlF4–. Which of the ions will exhibit a see-saw molecular geometry?
The NH3 molecule is trigonal pyramidal, while BF3 is trigonal planar. Which of these molecules is flat?
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.(c) Predict the shape of the molecules of the compound.
Which of these molecular shapes do you expect for the SF6 molecule?
Give the electron-domain and molecular geometry of a molecule that has the following electron domains on its central atom: five bonding domains and one nonbonding domain.
You may want to reference (Pages 343 - 351) Section 9.2 while completing this problem.What are the electron-domain and molecular geometries of a molecule that has the following electron domains on its central atom: three bonding domains and no nonbonding domains?
What are the electron-domain and molecular geometries of a molecule that has the following electron domains on its central atom?Select the electron-domain geometry for a molecule with three bonding domains and one nonbonding domain.
What are the electron-domain and molecular geometries of a molecule that has the following electron domains on its central atom?Select the electron-domain geometry for a molecule with two bonding domains and two nonbonding domains.
What are the electron-domain and molecular geometries of a molecule that has the following electron domains on its central atom?Select the molecular geometry for a molecule with three bonding domains and no nonbonding domains.
What are the electron-domain and molecular geometries of a molecule that has the following electron domains on its central atom?Select the molecular geometry for a molecule with three bonding domains and one nonbonding domain.
What are the electron-domain and molecular geometries of a molecule that has the following electron domains on its central atom?Select the molecular geometry for a molecule with two bonding domains and two nonbonding domains.
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.(b) Describe the geometry about the P atoms, the S atom, and the Cl atom in these species.
A certain AB4 molecule has a square-planar molecular geometry. Which of the following statements about the molecule is or are true?The molecule has four electron domains about the central atom A.The B-A-B angles between neighboring B atoms is 90A.The molecule has two nonbonding pairs of electrons on atom A.
Draw the Lewis Structure for KrF2. The central atom has _____ lone pairs. It's geometry is ______.
Sodium azide is a shock-sensitive compound that releases N2 upon physical impact. The compound is used in automobile airbags. The azide ion is N3–.Is it linear or bent?
Explain why the HOH molecule is bent, whereas the HBeH molecule is linear.
What feature of a Lewis structure can be used to tell if a molecule’s (or ion’s) electron-pair geometry and molecular structure will be identical?
Explain the difference between electron-pair geometry and molecular structure.
Predict the electron pair geometry and the molecular structure of each of the following molecules or ions:(a) SF6
Predict the electron pair geometry and the molecular structure of each of the following molecules or ions:(b) PCl5
Predict the electron pair geometry and the molecular structure of each of the following molecules or ions:(c) BeH2
Predict the electron pair geometry and the molecular structure of each of the following molecules or ions:(d) CH3+
Identify the electron pair geometry and the molecular structure of each of the following molecules or ions:(a) IF6+
Identify the electron pair geometry and the molecular structure of each of the following molecules or ions:(b) CF4
Identify the electron pair geometry and the molecular structure of each of the following molecules or ions:(c) BF3
Identify the electron pair geometry and the molecular structure of each of the following molecules or ions:(d) SiF5−
a. Draw the electron-dot structure for CHClO. Draw the molecule by placing the atoms on the grid and connecting them with bonds. Include all lone pairs of electrons.b. What is the electron-domain (charge-cloud) geometry of ClF5? Enter the electron-domain geometry of the molecule.c. What is the molecular geometry of ClF5? Enter the molecular geometry of the molecule.d. ignoring lone-pair effects, what is the smallest bond angle in ClF5? Express your answer as an integer.
Identify the electron pair geometry and the molecular structure of each of the following molecules or ions:(e) BeCl2
What are the electron-pair geometry and the molecular structure of each of the following molecules or ions?(a) ClF5
What are the electron-pair geometry and the molecular structure of each of the following molecules or ions?(b) ClO2−
What are the electron-pair geometry and the molecular structure of each of the following molecules or ions?(c) TeCl42−
What are the electron-pair geometry and the molecular structure of each of the following molecules or ions?(d) PCl3
What are the electron-pair geometry and the molecular structure of each of the following molecules or ions?(f) PH2−
What are the electron-pair geometry and the molecular structure of each of the following molecules or ions?(f) PH2−
Predict the electron pair geometry and the molecular structure of each of the following ions:(a) H3O+
Predict the electron pair geometry and the molecular structure of each of the following ions:(b) PCl4−
Predict the electron pair geometry and the molecular structure of each of the following ions:(c) SnCl3−
Predict the geometry of each interior atom in acetic acid.
Predict the electron pair geometry and the molecular structure of each of the following ions:(d) BrCl4−
Predict the electron pair geometry and the molecular structure of each of the following ions:(e) ICl3
Predict the electron pair geometry and the molecular structure of each of the following ions:(f) XeF4
Predict the electron pair geometry and the molecular structure of each of the following ions:(g) SF2
Identify the electron pair geometry and the molecular structure of each of the following molecules:(a) ClNO (N is the central atom)
Identify the electron pair geometry and the molecular structure of each of the following molecules:(b) CS2
Identify the electron pair geometry and the molecular structure of each of the following molecules:(c) Cl2CO (C is the central atom)
Identify the electron pair geometry and the molecular structure of each of the following molecules:(d) Cl2SO (S is the central atom)
Identify the electron pair geometry and the molecular structure of each of the following molecules:(e) SO2F2 (S is the central atom)
Both aluminum and iodine form chlorides, Al 2Cl6 and I2Cl6, with “bridging” Cl atoms. The Lewis structures are(b) Which of these molecules has a planar shape? Explain.
Identify the electron pair geometry and the molecular structure of each of the following molecules:(f) XeO2F2 (Xe is the central atom)
Identify the electron pair geometry and the molecular structure of each of the following molecules:(g) ClOF2+ (Cl is the central atom)
Predict the electron pair geometry and the molecular structure of each of the following:(a) IOF5 (I is the central atom)
Predict the electron pair geometry and the molecular structure of each of the following:(b) POCl3 (P is the central atom)
Predict the electron pair geometry and the molecular structure of each of the following:(c) Cl2SeO (Se is the central atom)
Predict the electron pair geometry and the molecular structure of each of the following:(d) ClSO+ (S is the central atom)
Predict the electron pair geometry and the molecular structure of each of the following:(e) F2SO (S is the central atom)
Predict the electron pair geometry and the molecular structure of each of the following:(f) NO2−
Predict the electron pair geometry and the molecular structure of each of the following:(g) SiO44−
The molecule called diazene has the formula N2H2 and the Lewis structure.Do you expect diazene to be a linear molecule (all four atoms on the same line)?
The molecule called diazene has the formula N2H2 and the Lewis structure.Do you expect the molecule to be planar (all four atoms in the same plane)?
A compound composed of 2.1% H, 29.8% N, and 68.1% O has a molar mass of approximately 50 g/mol. What is the geometry of the molecule?
At least two different numbers of electron groups can result in a linear molecule. What are they? What are the numbers of bonding groups and lone pairs in each case? Provide an example of a linear molecule in each case.
A molecule with the formula AB2, in which A and B represent different atoms, could have one of three different shapes. Sketch and name the three different shapes that this molecule might have. Give an example of a molecule or ion for each shape.
A molecule with the formula AB3, in which A and B represent different atoms, could have one of three different shapes. Sketch and name the three different shapes that this molecule might have. Give an example of a molecule or ion that has each shape.
Identify the geometry about interior atoms in CH3 NH2.
Identify the geometry about interior atoms in CH3 CO2 CH3.
Identify the geometry about interior atoms in NH2 CO2 H.
Acetylsalicylic acid (aspirin), the most widely used medicine in the world, has the Lewis structure shown. How many C atoms have a trigonal planar shape around them? A tetrahedral shape?
What do each of the following sets of compounds/ions have in common?a. SO3, NO3-, CO32-
What do each of the following sets of compounds/ions have in common?b. O3, SO2, NO2-
You may want to reference (Pages 343 - 351) Section 9.2 while completing this problem.Draw the Lewis structure for AsF3. Predict the electron-domain and molecular geometry.
You may want to reference (Pages 343 - 351) Section 9.2 while completing this problem.Draw the Lewis structure for CH3+. Predict the electron-domain and molecular geometry.
You may want to reference (Pages 343 - 351) Section 9.2 while completing this problem.Draw the Lewis structure for BrF3. Predict the electron-domain and molecular geometry.
You may want to reference (Pages 343 - 351) Section 9.2 while completing this problem.Draw the Lewis structure for ClO3–. Predict the electron-domain and molecular geometry.
You may want to reference (Pages 343 - 351) Section 9.2 while completing this problem.Draw the Lewis structure for XeF2. Predict the electron-domain and molecular geometry.
You may want to reference (Pages 343 - 351) Section 9.2 while completing this problem.Draw the Lewis structure for BrO2–. Predict the electron-domain and molecular geometry.
Which of the following characteristics does not apply to PF3?a.contains polar bondsb.has three σ bondsd.trigonal planard.one lone pair of electrons on phosphoruse. polar molecule
Consider the following XF4 ions: PF4–, BrF4–, ClF4+, and AlF4–. For which of the ions will the electron-domain and molecular geometries be the same?
Two important industrial chemicals, ethene, C2H4, and propene, C3H6, are produced by the steam (or thermal) cracking process:2C3H8(g) ⟶ C2H4(g) + C3H6(g) + CH4(g) + H2(g)For each of the four carbon compounds, do the following:(b) Predict the geometry about the carbon atom.
Give the electron-domain and molecular geometry of a molecule that has the following electron domains on its central atom: four bonding domains and no nonbonding domains.
Give the electron-domain and molecular geometry of a molecule that has the following electron domains on its central atom: three bonding domains and two nonbonding domains.
a. What is the electron-domain (charge-cloud) geometry of IF5? Enter the electron-domain geometry of the molecule.b. What is the molecular geometry of IF5? Enter the molecular geometry of the molecule.
Which of the following molecules is not planar? a. NCCN b. H2CCH2 c. SO3 d. SeF4 e. XeF2Cl2
Part A: What is the molecular geometry of NF3? Part B: What is the molecular geometry of HCN? Part C: What is the molecular geometry of SCl2?
Sulfur tetrafluoride (SF4) reacts slowly with O2 to form sulfur tetrafluoride monoxide (OSF4) according to the following unbalanced reaction: SF4(g) + O2(g) → OSF4(g). The O atom and the four F atoms in OSF4 are bonded to a central S atom.Determine the electron-domain geometry of OSF4.
This figure shows ball-and-stick drawings of three possible shapes of an AF3 molecule.For each shape, give the electron-domain geometry on which the molecular geometry is based.
This figure shows ball-and-stick drawings of three possible shapes of an AF3 molecule.For each shape, how many nonbonding electron domains are there on atom A?
The figure  that follows contains ball-and-stick drawings of three possible shapes of an AF4 molecule.For each shape, how many nonbonding electron domains are there on atom A?
The figure  that follows contains ball-and-stick drawings of three possible shapes of an AF4 molecule.For shape (i) give the electron-domain geometry on which the molecular geometry is based.
Amino acids are biological compounds that link together to form proteins, the workhorse molecules in living organisms.Determine the electron geometry about each interior atom.
The figure  that follows contains ball-and-stick drawings of three possible shapes of an AF4 molecule.For shape (ii) give the electron-domain geometry on which the molecular geometry is based.
The figure  that follows contains ball-and-stick drawings of three possible shapes of an AF4 molecule.For shape (iii) give the electron-domain geometry on which the molecular geometry is based.
The following electrostatic potential diagram represent CH4, NH3, or H2O. Label and explain your choice.
What is the electronic geometry of SCl4? Enter the electronic geometry of the molecule.
The following electrostatic potential diagram represent CH4, NH3, or H2O. Label and explain your choice.
Predict the electron-domain geometry around the central Xe atom in XeF2, XeF4, and XeF6.
Use VSEPR theory to predict the electron geometry about xenon in XeF4.
Use VSEPR theory to predict the electron geometry about the carbon atom in HCN.
The anion (v) is called "BARF" by chemists, as its common abbreviation sounds similar to this word.What is the electron-domain geometry around the central Cl in ClO4–?
You may want to reference (Pages 343 - 351) Section 9.2 while completing this problem.Would you expect the nonbonding electron-pair domain in NH3 to be greater or less in size than the corresponding one in PH3?
Determine the electron geometry for each molecule.a. PF3b. SBr2c. CHCl3d. CS2
A molecule with the formula AB3 has a trigonal planar geometry. How many electron groups are on the central atom?
The following figures show several molecular geometries.Give the number of total electron groups, the number of bonding groups, and the number of lone pairs for the geometry depicted in (a).
The following figures show several molecular geometries.Give the number of total electron groups, the number of bonding groups, and the number of lone pairs for the geometry depicted in (b).
The following figures show several molecular geometries.Give the number of total electron groups, the number of bonding groups, and the number of lone pairs for the geometry depicted in (c).
Determine the electron geometry for each molecule.CF4NF3OF2H2S
The genetic code is based on four different bases with the following structures.Assign an electron geometry to each interior atom in cytosine.
Consider the following XF4 ions: PF4–, BrF4–, ClF4+, and AlF4–. Which of the ions will have an octahedral electron-domain geometry?
The genetic code is based on four different bases with the following structures.Assign an electron geometry to each interior atom in adenine.
The genetic code is based on four different bases with the following structures.Assign an electron geometry to each interior atom in thymine.
The genetic code is based on four different bases with the following structures.Assign an electron geometry to each interior atom in guanine.
Describe the characteristic electron-domain geometry of each of the following numbers of electron domains about a central atom.
Match each two-dimensional structure to its correct three-dimensional description. Drag the appropriate items to their respective bins.
A 0.02847 g sample of gas occupies 10.0-mL at 292.0 K and 1.10 atm. Upon further analysis, the compound is found to be 38.734% C and 61.266% F. What is the molecular formula of the compound? Draw the Lewis structure of the compound. Identify the geometry around each carbon atom.
Molecular geometry of IF2-1 and lewis structure?
What is the electron-domain (charge-cloud) geometry of BrF5?
a) Select all of the equatorial atoms on the structure below. You may need to rotate the molecule to see all the atoms.b) What is the shape of this molecule?
Which geometrical shape is associated with the carbon atoms in alkanes?
What shape would you expect for XeF4?
What would you expect to be the electron-group arrangement around atom A in the following case? Give the ideal bond angle. Electron-group arrangement:a. trigonal bipyramidalb. square planarc. trigonal planarIdeal bond angle:  ____    ° 
The shape of the carbon dioxide molecule isa. tetrahedral b. triangular c. pyramidal d. linear
When SO3 gains two electrons, SO32− forms. (a) Which depiction best illustrates the change in molecular shape around S?
What shape would you expect for XeF4?What are the expected bond angles in ICl 4+? Check all that apply.a) 90°b) 109.5°c) 120°d) 180°
The molecule shown here is difluoromethane (CH2F2), which is used as a refrigerant called R-32.Based on the structure, how many electron domains surround the C atom in this molecule?
What is the electron-domain (charge-cloud) geometry of BrI 5?
Which of these molecules are linear? Check all that apply.a) XeF2b) BeCl2c) SF2d) NO2- 
Why must all six atoms in C2H4 lie in the same plane?
The figure that follows contains ball-and-stick drawings of three possible shapes of an AF4 molecule.Which of the following elements will lead to an AF4 molecule with the shape in (iii): Be, C, S, Se, Si, Xe?
The N2O molecule is linear and polar.a. On the basis of this experimental evidence, which arrangement, NNO or NON, is correct? Explain your answer.
The molecular geometry of PF3 is best described asA) trigonal planarB) trigonal pyramidalC) T-shapedD) tetrahedralE) the correct geometry is not listed
Dinitrogen difluoride, N2F2, is the only stable, simple inorganic molecule with an N=N bond. It occurs in two forms: cis (both F atoms on the same side of the N=N bond) and  trans (the F atoms on opposite sides of the N=N bond).(a) Draw the molecular shapes of the two forms of N 2F2.
In CIF3, the electron pairs are arranged about the chlorine atom ina. an octahedron.b. a square plane. c. a trigonal pyramid.d. a tetrahedron. e. a trigonal bipyramid. 
Determine the molecular geometry of PF5. 
What is the molecular geometry of SF2?a. Upside downb. Bentc. Tetrahedrald. Linear
Determine the molecular geometry of SCl 6.
What is the electronic geometry of  BI3?
1) Draw the lewis Dot Structures for CS 2 and SCl4    2) Using VSEPR rules, predict the geometry of the two molecules in question 1