Ch.11 - Liquids, Solids & Intermolecular ForcesWorksheetSee 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

Dipole moments or polarity happen in molecules when there is an unequal sharing of electrons. 

Molecular Polarity

Both a molecule's shape and bond polarity can affect its overall polarity. 

Concept #1: Understanding Molecular Polarity 

When the central element has no lone pairs and has the same surrounding elements then usually the molecule is nonpolar. 

Practice: Determine if carbon dioxide, CO2, is polar or nonpolar.

When the central element has lone pairs then we must use element dipole arrows and lone pair dipole arrows to determine polarity. 

Practice: Determine if xenon tetrafluoride is polar or nonpolar.

Concept #2: Some molecular shapes are seen as perfect and will always lead to a non-polar molecule overall. 

Example #1: Determine if silicon tetrachloride, SiCl4, is polar or nonpolar. 

Example #2: Determine if phosphorus trihydride, PH3, is polar or nonpolar. 

Practice: Determine if the following compound is polar or nonpolar. SiBr42-

Practice: Determine if the following compound is polar or nonpolar. H2S

Practice: Determine if the following compound is polar or nonpolar. PCl2F3

Practice: Determine if the following compound is polar or nonpolar. IF2-

Additional Problems
Classify the molecule AsCl3. 1. polar molecule with polar bonds 2. polar molecule with nonpolar bonds 3. nonpolar molecule with nonpolar bonds 4. nonpolar molecule with polar bonds
Of the molecules drawn below, which is non-polar? If they are all polar, then do not circle a structure. 
The molecules below are described as either polar or non-polar. Which one is incorrectly described? (a) OCN− - Polar (b) CH2Cl2 - Non-polar (c) CO2 - Non-polar (d) NH3 - Polar (e) SO2 - Polar
Complete this sentence:  The PCl 5 molecule has             A)      nonpolar bonds, and is a nonpolar molecule.             B)      nonpolar bonds, but is a polar molecule.             C)      polar bonds, and is a polar molecule.             D)      coordinate covalent bonds             E)      polar bonds, but is a nonpolar molecule.
Explain why CO2 is nonpolar, but OCS is polar?
Select the molecule that is the most polar a. PCI5 b. BrCl5 c. XeF4 d. CCl4 e. XeF2
Predict which of the following molecules is non-polar. a) HBr b) CF4 c) H2S d) NI3 e) CHCl3
Which molecule below is nonpolar?  a) SF4 b) OF2 c) PH3 d) CBrCl3 e) XeCl4
Which statement best describes the polarity of CF 2I2 a) the molecule is nonpolar because the dipoles of the C—I bonds cancel each other b) the molecule is nonpolar because the dipoles of the C—F bonds cancel each other c) depending on the arrangement of the surrounding atoms, the molecule could be polar or nonpolar d) the molecule is always polar e) the molecule is always nonpolar
Which of these is nonpolar?
Which of the following species is nonpolar? 1. SCl2 2. ClO3- 3. IF2- 4. IF5
Which of the following statements about SO 32- is true? 1. The bonds are polar and the ion is polar. 2. The bonds are polar and the ion is nonpolar. 3. The bonds are nonpolar and the ion is polar. 4. The bonds are nonpolar and the ion is nonpolar.
Which of the following statements about SF5 – is true? 1. The ion has polar bonds and the ion is polar. 2. The ion has polar bonds but the ion is nonpolar.  3. The ion has nonpolar bonds and the ion is nonpolar.  4. The ion has nonpolar bonds but the ion is polar. 
Which molecule below is nonpolar? a. SF4 b. OF2 c. PH3 d. CBrCl3 e. XeCl4
Which statement best describes the polarity of CF 2l2? a. the molecule is nonpolar because the dipoles of the C-l bonds cancel each other. b. the molecule is nonpolar because the dipoles of the C-F bonds cancel each other c. depending on the arrangement of the surrounding atoms, the molecule could be polar or nonpolar d. the molecule is always polar e. the molecule is always nonpolar
Which of the following shows these molecules in order from the most polar to least polar? a. CH4 > CF2Cl2 > CCl4 CCl2H2 b. CH4 > CF2H2 > CF2Cl2 > CCl4 > CCl2H2 c. CF2Cl2 > CF2H2 > CCl2H2 > CH4 = CCl4 d. CF2H2 > CCl2H2 > CF2Cl2 > CH4 = CCl4 e. CF2Cl2 > CF2H2 > CCl4 > CCl2H2 > CH4
Which of the following statements about polar molecules is  false? a. A molecule with polar bonds can be nonpolar. b. A molecule with polar bonds can be polar. c. A molecule with only nonpolar bonds can be polar. d. A molecule with 120° bond angles can be polar. e. A molecule with 180° bond angles can be polar.
Which one of the following is a nonpolar molecule with polar covalent bonds? a. NH3 b. H2Se c. SOBr2 (S is central atom) d. BeCl2 e. HCl
Which of the following isomers of PF 2Cl3 are polar? a) only I b) only II c) only III d) II and III e) I, II, and III
Choose the compound below that contains at least one polar covalent bond, but is nonpolar. A) SCl2 B) CF2Cl2 C) BCl3 D) GeH2Br2 E) All of the above are nonpolar and contain a polar covalent bond.
Which of the following statements concerning polar molecules is false? a. There must be at least one polar bond or one unshared pair of electrons on the central atom. b. If there are more than one polar bond, they must not be symmetrically arranged so that their polarities cancel. c. If there are more than one unshared pair of electrons on the central atom, they must not be symmetrically arranged so that their polarities cancel. d. There must be an odd number of polar bonds so that their polarities not cancel. e. A molecule with symmetrically arranged polar bonds can be polar if the central atom is bonded to atoms of different elements.
Consider four molecules I) CHCl3 II) CH4 III) CH3Cl IV) CCl4 Which of these exhibit permanent dipole-dipole interactions? 1. I, III, and IV only 2. III only 3. None of these 4. I only 5. I and III only
You may want to reference (Pages 352 - 354) Section 9.3 while completing this problem.Is the molecule BF3 polar or nonpolar?
Why is polarity important?
Fill in the following chart. If the molecule column is blank, find an example that fulfills the conditions of the rest of the row. # Molecule Electron-domain Geometry Hybridization of Central Atom Dipole moment? Yes or No. 1 CO2 2 sp3 yes 3 sp3 no 4 trigonal planar no 5 SF4 6 octahedral no 7 sp2 yes 8 trigonal bipyramidal no 9 XeF2 Complete the first row of the table.
Fill in the following chart. If the molecule column is blank, find an example that fulfills the conditions of the rest of the row. # Molecule Electron-domain Geometry Hybridization of Central Atom Dipole moment? Yes or No. 1 CO2 2 sp3 yes 3 sp3 no 4 trigonal planar no 5 SF4 6 octahedral no 7 sp2 yes 8 trigonal bipyramidal no 9 XeF2 Complete the fifth row of the table.
Fill in the following chart. If the molecule column is blank, find an example that fulfills the conditions of the rest of the row. # Molecule Electron-domain Geometry Hybridization of Central Atom Dipole moment? Yes or No. 1 CO2 2 sp3 yes 3 sp3 no 4 trigonal planar no 5 SF4 6 octahedral no 7 sp2 yes 8 trigonal bipyramidal no 9 XeF2 Complete the sixth row of the table.
Fill in the following chart. If the molecule column is blank, find an example that fulfills the conditions of the rest of the row. # Molecule Electron-domain Geometry Hybridization of Central Atom Dipole moment? Yes or No. 1 CO2 2 sp3 yes 3 sp3 no 4 trigonal planar no 5 SF4 6 octahedral no 7 sp2 yes 8 trigonal bipyramidal no 9 XeF2 Complete the fourth row of the table.
Fill in the following chart. If the molecule column is blank, find an example that fulfills the conditions of the rest of the row. # Molecule Electron-domain Geometry Hybridization of Central Atom Dipole moment? Yes or No. 1 CO2 2 sp3 yes 3 sp3 no 4 trigonal planar no 5 SF4 6 octahedral no 7 sp2 yes 8 trigonal bipyramidal no 9 XeF2 Complete the eighth row of the table.
Fill in the following chart. If the molecule column is blank, find an example that fulfills the conditions of the rest of the row. # Molecule Electron-domain Geometry Hybridization of Central Atom Dipole moment? Yes or No. 1 CO2 2 sp3 yes 3 sp3 no 4 trigonal planar no 5 SF4 6 octahedral no 7 sp2 yes 8 trigonal bipyramidal no 9 XeF2 Complete the ninth row of the table.
Fill in the following chart. If the molecule column is blank, find an example that fulfills the conditions of the rest of the row. # Molecule Electron-domain Geometry Hybridization of Central Atom Dipole moment? Yes or No. 1 CO2 2 sp3 yes 3 sp3 no 4 trigonal planar no 5 SF4 6 octahedral no 7 sp2 yes 8 trigonal bipyramidal no 9 XeF2 Complete the third row of the table.
Fill in the following chart. If the molecule column is blank, find an example that fulfills the conditions of the rest of the row. # Molecule Electron-domain Geometry Hybridization of Central Atom Dipole moment? Yes or No. 1 CO2 2 sp3 yes 3 sp3 no 4 trigonal planar no 5 SF4 6 octahedral no 7 sp2 yes 8 trigonal bipyramidal no 9 XeF2 Complete the seventh row of the table.
Determine whether each molecule is polar or nonpolar.SCl4
Determine whether each molecule is polar or nonpolar.BrF5
In which direction does the net dipole point in SCl2?
Predict whether each of the following molecules is polar or nonpolar IF, CS2, SO3, PCl3, SF6, IF5.
Classify CS2 as polar or nonpolar.
What is the distinction between a bond dipole and a molecular dipole moment?
Acetone, (CH3 )2 CO, is widely used as an industrial solvent.Is the acetone molecule polar or nonpolar?
How do you determine whether a molecule is polar?
Determine whether the molecule SF4 is polar.
Determine whether the molecule IF5 is polar.
Determine whether the molecule CH2 CHCH3 is polar.
Is XeF2 polar or nonpolar?
Which of the molecules below will be polar?CS2, BF3, SO2, CH3Bra. CH3Br onlyb. CS2 onlyc. Both BF3 and CH3Brd. Both SO2 and CH3Br
Are SO3,XeF2,IF2- polar or nonpolar? How it is polar or nonpolar? Add formal charges and bond dipoles to all lewis dot structures. According to Vallence bond theory , what is the hybridization of all atoms in SO 3? Describe the orbitals that overlap to form all bonds in SO3.
Specify the polarity of the bonds and the overall polarity of the molecule.# of Polar Bonds _____________Polar molecule (yes/no) _______________ 
Specify the polarity of the bonds and the overall polarity of the molecule.# of Polar Bonds _____________Polar molecule (yes/no) _______________
Which of the following molecules is non-polar? A) XeF4 B) H2O C) PH3 D) O3 E) H2O2
Choose from the compound below that contains at least one polar covalent bond, but is non-polar.a. HCNb. CF4c. SeBr4d. ICl3e. Both B and C are non-polar and contain a polar covalent bond
Consider the following moleculesI. BCl3        II. CHBr3 (C is the central atom)      III. Cl2        IV. XeBr2          V. COThese molecules have a zero net dipole moment (nonplolar)III, VIII, IV, VI, III, IVI, III, IV, VINone of them 
Which statement best describes the polarity of CF 2Cl2?a. Always polar.b. Always nonpolar.c. Depending on the arrangement of outer atoms, this molecule could be polar or nonpolar.
Which statement best describes the polarity of SF 4Cl2?a. Always polar.b. Always nonpolar.c. Depending on the arrangement of outer atoms, this molecule could be polar or nonpolar.
Which one of the following molecules is polar? a) PBr5 b) CCl4 c) BrF5 d) XeF2  e) XeF4
How many of the following molecules are polar?a. BrCl3b. CS2c. SiF4d. SO3
Identify whether each molecule given below is polar or nonpolar.SiH3Br, SBr2, BrF3, BF3 
There are 3 Lewis structures for C2H2Cl2 draw all three and indicate whether each is non-polar or polar.Explain why one of these structures is non-polar and the other 2 are polar.
Which statement is true about the polarity of HCN, which has a structure of H-C≡N:?(Hint: The electronegativities of H, C, and N are 2.1, 2.5, and 3.0, respectively.)a. The carbon-nitrogen bond in HCN is a polar-covalent bondb. Both bonds in HCN are nonpolar covalent bondsc. The total molecular dipole moment in HCN points towards the H atomd. Statements a and c are correcte. Statements b and c are correct
Draw the lewis dot structure for CH 2Cl2. Is this molecule polar?
How would you describe the molecular polarity of SeCl 6?Nonpolar, because Se-Cl is a nonpolar bond and there is no lone pair on SeNonpolar, because Se-Cl is a polar bond but the geometry is symmetricPolar, because Se-Cl is a polar bond although the geometry is symmetricPolar, because Se-Cl is a polar bond and there is a lone pair on SePolar, because Se-Cl is a nonpolar bond but there is a lone pair on Se
There are 3 different possible isomers of a dibromoethene molecule, C 2H2Br2. One of them has no net dipole moment, but the other two do. Draw Lewis structures for each of these isomers. Include H atoms.Nonpolar C2H2Br2 (one isomer)Polar C2H2Br2 (two isomers)
How many of the following molecules are polar?CF4             PCl  3            H 2S            ICl 5a. 0b. 1c. 2d. 3e. 4
BrCl5 (bromine pentachloride) is sometimes called a polar molecule, sometimes called nonpolar. Which one is it REALLY and WHY?
There are 3 Lewis structures for [ NO3]- draw all three and compare polarity of the 3.
Water is known as a polar molecule because (check all apply)a. The oxygen and hydrogen atoms have the same electronegativity.b. The hydrogen atom attracts electrons much more strongly than the oxygen atom.c. Water has two hydrogen atoms covalently bonded to a single oxygen atom.d. The oxygen atom has a greater attraction for electrons than the hydrogen atom does.e. Water dipole moment is equal to zero.f. The electrons of the covalent bond are not shared equally between the hydrogen and oxygen atoms.
Is O3 polar or non-polar?
For the molecules below, provide the Lewis dot structure, draw the three dimensional dash-wedge structure, and comment on the polarity of the molecule.a. Nitrous acid, HNO2b. Polypropylene, CH3CHCH2c. Percholorethylene, CCl2CCl2d. Sulfonyl fluoride, SO2F2
How do you determine if a molecule is polar or nonpolar?
Is ClF3 polar or non polar?
Which of the following molecules is nonpolar? a. NH3 b. OF2 c. CH3Cl d. H2O e. BeCl2   
Predict which molecules are polar. Select all that apply. a) AsF3 b) IOF5 c) CF4 d) CH2Cl2
Predict whether each of the following molecules is polar or nonpolar. XeF4, NH3, CH3Br, CCl4, SF4, GaH3
Explain how a molecule that contains polar bonds can be nonpolar.
The molecule O=C=S is linear and has a Lewis structure analogous to that of CO2. Would you expect this molecule to be nonpolar?
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. (b) Which of the five fluorine-containing molecules have no dipole moment?
Explain why CO2 and CCl4 are both nonpolar even though they contain polar bonds.
What is the sum of the two red vectors at the top of the left figure?
Identify the molecules with polar bonds and the polar molecules. a. CCl4  b. CH3Cl c. H2O d. CO2 e. O2
Classify these molecules as polar or nonpolar. CH3Cl CCl4 HF BCl3 H2O H2
Predict whether each of the following molecules is polar or non-polar: IF, CS2, SO3, PCl3, SF6, IF5
Which of the following molecules is not necessarily polar?a. SeF4b. SO2c. CH2Cl2d. PH3e. Cl2XeF2
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. Do you predict that the molecule will have a dipole moment?
A useful solvent that will dissolve salts as well as organic compounds is the compound acetonitrile, H3CCN. It is present in paint strippers.(a) Write the Lewis structure for acetonitrile, and indicate the direction of the dipole moment in the molecule.
As a general rule, MXn molecules (where M represents a central atom and X represents terminal atoms; n = 2 – 5) are polar if there is one or more lone pairs of electrons on M. NH3 (M = N, X = H, n = 3) is an example. There are two molecular structures with lone pairs that are exceptions to this rule. What are they?
The following molecules have the same molecular formula (C3H8O), but different chemical structures.propanolethyl methyl etherWhich molecule do you expect to have a larger dipole moment?
Which of the following molecules have net dipole moments? For the molecules that are polar, indicate the polarity of each bond and the direction of the net dipole moment of the molecule.a. CH2Cl2, CHCl3, CCl4
Which of the following molecules have net dipole moments? For the molecules that are polar, indicate the polarity of each bond and the direction of the net dipole moment of the molecule.b. CO2, N2O
Which of the following molecules have net dipole moments? For the molecules that are polar, indicate the polarity of each bond and the direction of the net dipole moment of the molecule.c. PH3, NH3
Determine whether each molecule is polar or nonpolar.SCl2
You may want to reference(Pages 352 - 354)Section 9.3 while completing this problem.Predict whether each of the following molecules is polar or nonpolar: (a) CCl4, (b) NH3, (c) SF4, (d) XeF4, (e) CH3Br, (f) GaH3.
Dichloroethylene (C2H2Cl2) has three forms (isomers), each of which is a different substance. How many isomers of dichloroethylene have a zero dipole moment?
You may want to reference (Pages 352 - 354) Section 9.3 while completing this problem.Consider a molecule with formula AX3. Supposing the A–X bond is polar, how would you expect the dipole moment of the AX3 molecule to change as the X–A–X bond angle increases from 100˚ to 120˚?
The O-H bond lengths in the water molecule (H2O) are 0.96 Å, and the H–O–H angle is 104.5˚. The dipole moment of the water molecule is 1.85 D. In what directions do the bond dipoles of the O–H bonds point? In what direction does the dipole moment vector of the water molecule point?
The molecule shown here is difluoromethane (CH2F2), which is used as a refrigerant called R-32.Would the molecule have a nonzero dipole moment?
The molecule shown here is difluoromethane (CH2F2), which is used as a refrigerant called R-32.If the molecule is polar, which of the following describes the direction of the overall dipole moment vector in the molecule:(i) from the carbon atom toward a fluorine atom(ii) from the carbon atom to a point midway between the fluorine atoms(iii) from the carbon atom to a point midway between the hydrogen atoms(iv) from the carbon atom toward a hydrogen atom?
The Lewis structure for allene is shown in the diagram.Does it have a nonzero dipole moment?
Which of these AF3 molecules will have a nonzero dipole moment?
Which of the following AF4 molecules will have a zero dipole moment?
You may want to reference (Pages 352 - 354) Section 9.3 while completing this problem.Dichlorobenzene, C6H4Cl2, exists in three forms (isomers), called ortho, meta, and para:Which of these has a nonzero dipole moment?
The four bonds of carbon tetrachloride (CCl4) are polar, but the molecule is nonpolar because the bond polarity is canceled by the symmetric tetrahedral shape. When other atoms substitute for some of the Cl atoms, the symmetry is broken and the molecule becomes polar. Rank the following molecules from the least polar to the most polar:CH2Br2, CF2Cl2, CH2F2, CH2Cl2, CBr4, CF2Br2
There are three possible structures for PCl2F3 with phosphorus as the central atom. Draw them and discuss how measurements of dipole moments could help distinguish among them.
What would you expect for the magnitude and direction of the bond dipoles in this series: BH4–, CH4, NH4+?
Identify whether each molecule given below is polar or nonpolar.a. PF3b. SBr2c. CHCl3d. CS2
Determine whether each molecule given below is polar or nonpolar.a. CF4b. NF3c. OF2d. H2S
Determine whether each molecule is polar or nonpolar.a. SiCl4b. CF2Cl2c. SeF6d. IF5
Use the simulation (http://openstaxcollege.org/l/16MolecPolarity) to perform the following exercises for a real molecule. You may need to rotate the molecules in three dimensions to see certain dipoles.(a) Sketch the bond dipoles and molecular dipole (if any) for O3. Explain your observations.
Use the simulation (http://openstaxcollege.org/l/16MolecPolarity) to perform the following exercises for a real molecule. You may need to rotate the molecules in three dimensions to see certain dipoles.(c) Predict whether there should be a molecular dipole for NH3 and, if so, in which direction it will point. Check the molecular dipole box to test your hypothesis.
Determine whether the molecule COF2 is polar.
Determine whether the molecule CH3SH is polar.
Which of the molecules have net dipole moments (are polar)?a. SeO3b. SeO2c. PCl3d. SCl2e. SiF4
Consider the molecules SCl 2, F2, CS2, CF4, and BrCl.(b) Which molecules have a dipole moment?
Consider the molecules BF3, PF3, BrF3, SF4, and SF6.(b) Which molecules have a dipole moment?
Which molecule in each pair has the greater dipole moment? Give the reason for your choice.(a) SO2 or SO3
Which molecule is polar?a) SF2b) BH3c) PF5d) CS2
Which molecule in each pair has the greater dipole moment? Give the reason for your choice.(b) ICl or IF
Which molecule in each pair has the greater dipole moment? Give the reason for your choice.(c) SiF4 or SF4
Which molecule in each pair has the greater dipole moment? Give the reason for your choice.(d) H2O or H2S
Indicate whether CF4 is polar.
Which molecule in each pair has the greater dipole moment? Give the reason for your choice.(a) ClO2 or SO2
Which molecule in each pair has the greater dipole moment? Give the reason for your choice.(b) HBr or HCl
Which molecule in each pair has the greater dipole moment? Give the reason for your choice.(c) BeCl2 or SCl2 
Which molecule in each pair has the greater dipole moment? Give the reason for your choice.(d) AsF3 or AsF5
There are three different dichloroethylenes (molecular formula C2H2Cl2), which we can designate X, Y, and Z. Compound X has no dipole moment, but compound Z does. Compounds X and Z each combine with hydrogen to give the same product:C2H2Cl2 (X or Z) + H2 ⟶ ClCH2—CH2ClWhat are the structures of X, Y, and Z? Would you expect compound Y to have a dipole moment?
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).(b) Predict the direction of the molecular polarity, if any, of each form.
When SO3 gains two electrons, SO32− forms.(b) Does molecular polarity change during this reaction?
A molecule of formula AY3 is found experimentally to be polar. Which molecular shapes are possible and which are impossible for AY3?
Consider the following molecular shapes:(b) Which, if any, is polar?
Is the compound NH 2- polar or non polar? Why or why not?
Which of the molecules have net dipole moments (are polar)?a. XeCl2b. ICl3c. TeF4d. PCl5e. ICl5 f. XeCl4 g. SeCl6
Draw the structure of a molecule with the formula C4H6Cl2 that has a dipole moment of 0.
Which has no dipole moment?A. CO2 B. NH3 C. H2O D. HF E. None of the above
POLAR OR NON-POLAR? WHY? (a) Phosphate, PO43- (b) Potassium lon (c) Nitrous oxide (d) Magnesium ion (e) Nitrogen, N2
Which statement for NH3 and NF3 is false? Electronegativities: N = 3.0, H = 2.1, F = 4.0.a. The NF3 molecule is more polar than the NH 3 molecule. b. The bond angles in NF3 are smaller than those in NH3.c. The bond dipoles in NF3 are directed toward the more electronegative fluorine atoms.d. Both molecules have one unshared pair of electrons in the outer shell of nitrogen.e. Both are sp3 hybridized at nitrogen. f. The bond dipoles in NF3 oppose the effect of the unshared pair of electrons. g. The nitrogen atom can be described as utilizing sp3 hybrid orbitals in the nitrogen trifluoride molecule. h. The bond dipoles of NF3 are directed toward fluorine, whereas those in NH 3 are directed toward nitrogen.
Decide whether each molecule or polyatomic ion is polar or nonpolar. If the molecule or polyatomic ion is polar, write the chemical symbol of the atom closest to the negative side. For example, if the molecule were HCl and you decided the hydrogen atom was closest to the negative side of the molecule, you'd enter "H" in the last column of the table. 
Would the following structures be polar or nonpolar? (Not applicable if the structure is an ion. Pick "ionic" in that case).NO2+SCN-CS2
Which statement best describes the polarity of SCl 4F2? a. The molecule is always polar. b. The molecule is always nonpolar. c. Depending on the arrangement of outer atoms, this molecule could be polar or nonpolar.
How many of the following molecules are polar? Hint: All of the bonds in these molecules are polar except for the C=S bond.PCl5     OCS     SeCl 2A) 2B) 3C) 1D) 0
Which choice best describes the polarity of ICl 5?a. The molecule is polar and has polar bonds.b. The molecule is nonpolar and has polar bonds.c. The molecule is polar and has nonpolar bonds.d. The molecule is nonpolar and has nonpolar bonds.
Does BeCl2 have a dipole moment?
Is the Cl2BBCl2 molecule polar or nonpolar?
Determine the electron geometry (eg), molecular geometry(mg) and polarity of XeO 3.a. eg = tetrahedral, mg = trigonal pyramidal, polarb. eg = trigonal bipyramidal, mg = trigonal planar, nonpolarc. eg = trigonal planar, mg = trigonal pyramidal, polard. eg = trigonal planar, mg = trigonal planar, nonpolare. eg = octahedral, mg = tetrahedral, nonpolar
Which of the following compounds are polar:a. CBr4, XeF2, SCl4, BrF3, CH3OHb. XeF2, SCl4, BrF3, CH3OH onlyc. BrF3, CH3OH only d. SCl4, BrF3, CH3OH only
Which of the following molecules has a net dipole moment (i.e. is polar)?A. KrF2     B. CCl4      C. CO2      D. BeCl2     E. SF2
Which of the following molecules is polar?a. BF3b. CCI4c. CO2d. NO2e. SF6
Of the molecules PF3 and PCl3, which has bonds that are more polar?
Which of these molecules are polar? Check all that apply
Identify the following bonds as polar or nonpolarO-H, C-F, N-C, I-Br, C-C
Classify these molecules as polar or nonpolar. 
Is CS2 polar or nonpolar?
Is the CH4 a polar or non-polar bond? What about the molecule as a whole? Is that molecule CH4 a polar or non-polar?
The molecules BF3, CF4, CO2, PF5, and SF6 are all nonpolar, even though they all contain polar bonds. Why?
Choose the pair of substances that are most likely to form a homogeneous solution. a. Nal and C6H14 b. KCI and Hg c. NH3 and CH3OH d. F2 and PF3 e. C3H8 and C2H5OH
At standard temperature and pressure the molar volumes of Cl2 and NH3 gases are 22.06 and 22.40 L, respectively.Given the different molecular weights, dipole moments, and molecular shapes, why are their molar volumes nearly the same?
CH3 F is a polar molecule, even though the tetrahedral geometry often leads to nonpolar molecules.Explain why the molecule CH3 F is polar.
Determine whether each molecule given below is polar or nonpolar:NF3, XeF2, H2S, and CF4.
Describe the molecular dipole of OCl2.
Choose the pair of substances that are most likely to form a homogeneous solution. LiBr and C5H12 C6H14 and C10H20 I2 and CH3OH N2O4 and NH4Cl None of the pairs above will form a homogeneous solution.
Which of these molecules would you expect to be polar: Cl 2, ICl, BF3, SO2?a. ICl and SO2b. Cl2 and BF3c. ICl and BF3d. BF3 and SO2
Determine whether the molecule S2 Cl2 is polar.
Which formula represents a nonpolar molecule?a. NH3b. H2Sc. CH4d. HCl
State whether each is polar or nonpolar.a. BeF2 b. SF6 c. FCN 
Is BeCl2 polar or nonpolar?
Is ICl4- polar or nonpolar?
Is HBr a polar or non polar molecule?
Consider the molecule IF3.i) What is the electron domain geometry and the molecular geometry of IF 3?ii) Is IF3 polar or nonpolar?
a) PF3Cl2 is a nonpolar molecule. Based on this information, determine the F−P−F bond angle, the Cl−P−Cl bond angle, and the F−P−Cl bond angle. b) Which statement best describes the polarity of CF2Cl2?a. The molecule is always polar.b. The molecule is always nonpolar.c. Depending on the arrangement of outer atoms, this molecule could be polar or nonpolar.
Is H2O polar or nonpolar?
Explain whether Cl2XeF2 is necessarily polar?
Is SCl4 polar or non polar?
Determine whether each molecule is polar or nonpolar. Drag the appropriate items to their respective bins.
Determine whether each molecule given below is polar or nonpolar.CF4, PBr5, XeF2, SF6   
Is XeF4 polar or nonpolar? Explain your answer.
Rank the following molecules from the least polar to the most polar:CH2Br2, CF2Cl2, CH2F2, CH2Cl2, CBr4, CF2Br2.
Why is CCl4 non-polar and SF4 polar?