The figure that follows contains ball-and-stick drawings of three possible shapes of an AF4 molecule. (a) For each shape, give the electron-domain geometry on which the molecular geometry is based. ii.

The figure that follows contains ball-and-stick drawings of three possible shapes of an AF4 molecule. (a) For each shape, give the electron-domain geometry on which the molecular geometry is based. iii.

The figure that follows contains ball-and-stick drawings of three possible shapes of an AF4 molecule. (a) For each shape, give the electron-domain geometry on which the molecular geometry is based. i.

The figure that follows contains ball-and-stick drawings of three possible shapes of an AF4 molecule. (c) Which of the following elements will lead to an AF4 molecule with the shape in (iii): Be, C, S, Se, Si, Xe? i.

ii.

iii.

Give the approximate values for the indicated bond angles in the following molecules: (a)

Give the approximate values for the indicated bond angles in the following molecules: (c)

Give the approximate values for the indicated bond angles in the following molecules: (a)

Give the approximate values for the indicated bond angles in the following molecules: (d)

Ammonia, NH3, reacts with incredibly strong bases to produce the amide ion, NH2-. Ammonia can also react with acids to produce the ammonium ion, NH4+. (a) Which species (amide ion, ammonia, or ammonium ion) has the largest H¬N¬H bond angle? (b) Which species has the smallest H¬N¬H bond angle?

Consider the following XF₄ ions: PF₄^-, BrF₄^-, ClF₄⁺, and AlF₄^-. (a) Which of the ions have more than an octet of electrons around the central atom?

Consider the following XF4 ions: PF4-, BrF4-, ClF4+, and AlF4-. (c) Which of the ions will have an octahedral electron-domain geometry?

Which of the following statements are true?

i. The overall dipole moment of a molecule is the vector sum of its individual bond dipoles.

ii. If atoms A and B in an AB𝑛 molecule have different electronegativities, then the AB𝑛 molecule must have a nonzero dipole moment.

iii. The bond dipoles in a tetrahedral AB4 molecule cancel one another.

a. Does SCl2 have a nonzero dipole moment?

(b) It turns out that ozone, O₃, has a small dipole moment. How is this possible, given that all the atoms are the same?

(c) Does the molecule BF₂Cl have a dipole moment?

a. Consider the AF3 molecules in Exercise 9.27. Which of these will have a nonzero dipole moment?

Predict whether each of the following molecules is polar or nonpolar: (a) IF, (b) CS2, (c) SO3, (d) PCl3, (e) SF6, (f) IF5.

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. (b) Which of these isomers has a zero dipole moment?

Dichloroethylene (C₂H₂Cl₂) has three forms (isomers), each of which is a different substance. (c) How many isomeric forms can chloroethylene, C2H3Cl, have? Would they be expected to have dipole moments?

Dichlorobenzene, C₆H₄Cl₂, exists in three forms (isomers) called ortho, meta, and para:

Which of these has a nonzero dipole moment?

Draw sketches illustrating the overlap between the following orbitals on two atoms: (a) the 2s orbital on each atom

Draw sketches illustrating the overlap between the following orbitals on two atoms: (b) the 2p_z orbital on each atom (assume both atoms are on the z-axis) (c) the 2s orbital on one atom and the 2p_z orbital on the other atom.

For each statement, indicate whether it is true or false. (d) Nonbonding electron pairs cannot occupy a hybrid orbital.

Consider the molecule BF₃. (c) What hybrid orbitals should be constructed on the B atom to make the B–F bonds in BF₃?

Consider the SCl2 molecule. (c) What hybrid orbitals should be constructed on the S atom to make the S-Cl bonds in SCl2?

Consider the SCl2 molecule.(d) What valence orbitals, if any, remain unhybridized on the S atom in SCl2?