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Problem 41
Predict whether each of the following molecules is polar or nonpolar: (a) IF, (b) CS2, (c) SO3, (d) PCl3, (e) SF6, (f) IF5.
Problem 42
Predict whether each of the following molecules is polar or nonpolar: (a) CCl4, (b) NH3, (c) SF4, (d) XeF4, (e) CH3Br, (f) GaH3.
Problem 43b
Dichloroethylene (C2H2Cl2) has three forms (isomers), each of which is a different substance. (b) Which of these isomers has a zero dipole moment?
Problem 43c
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?
Problem 44
Dihydroxybenzene, C6H6O2, exists in three forms (isomers) called ortho, meta, and para:
Which of these has a nonzero dipole moment?
- For each statement, indicate whether it is true or false. (a) In order to make a covalent bond, the orbitals on each atom in the bond must overlap. (b) A p orbital on one atom cannot make a bond to an s orbital on another atom.
Problem 45
Problem 46a
Draw sketches illustrating the overlap between the following orbitals on two atoms: (a) the 2s orbital on each atom
Problem 46b,c
Draw sketches illustrating the overlap between the following orbitals on two atoms: (b) the 2pz orbital on each atom (assume both atoms are on the z-axis) (c) the 2s orbital on one atom and the 2pz orbital on the other atom.
Problem 47d
For each statement, indicate whether it is true or false. (d) Nonbonding electron pairs cannot occupy a hybrid orbital.
- How would you expect the extent of overlap of the bonding atomic orbitals to vary in the series IF, ICl, IBr, and I2? Explain your answer.
Problem 48
Problem 49a,b
Consider the molecule BF3. (a) What is the electron configuration of an isolated B atom? (b) What is the electron configuration of an isolated F atom?
Problem 49c
Consider the molecule BF3. (c) What hybrid orbitals should be constructed on the B atom to make the B–F bonds in BF3?
Problem 50c
Consider the SCl2 molecule. (c) What hybrid orbitals should be constructed on the S atom to make the S-Cl bonds in SCl2?
Problem 50d
Consider the SCl2 molecule.(d) What valence orbitals, if any, remain unhybridized on the S atom in SCl2?
Problem 51a,b
Indicate the hybridization of the central atom in (a) H2S (b) SeF6
Problem 51c,d
Indicate the hybridization of the central atom in (c) P1OH23 (d) AlI3.
Problem 52a,b
What is the hybridization of the central atom in (a) PBr5? (b) CH2O?
Problem 52c
What is the hybridization of the central atom in (c) O3?
Problem 52d
What is the hybridization of the central atom in (d) NO2?
Problem 53
Shown here are three pairs of hybrid orbitals, with each set at a characteristic angle. For each pair, determine the type of hybridization, if any, that could lead to hybrid orbitals at the specified angle. (a)
(b)
(c)
- (c) Write the formulas for the analogous species of the elements of period 3;
Problem 54
Problem 54a
(a) Which geometry and central atom hybridization would you expect in the series BH4-, CH4, NH4+?
Problem 54b
(b) What would you expect for the magnitude and direction of the bond dipoles in this series?
Problem 55a,b
(a) Draw a picture showing how two p orbitals on two different atoms can be combined to make a σ bond. (b) Sketch a π bond that is constructed from p orbitals.
Problem 55c
(c) Which is generally stronger, a s bond or a p bond? Explain.
Problem 55d
(d) Can two s orbitals combine to form a p bond? Explain.
- (a) If the valence atomic orbitals of an atom are sp hybridized, how many unhybridized p orbitals remain in the valence shell? How many p bonds can the atom form?
Problem 56
Problem 56b
(b) Imagine that you could hold two atoms that are bonded together, twist them, and not change the bond length. Would it be easier to twist (rotate) around a single s bond or around a double 1s plus p2 bond, or would they be the same?
Problem 57a
(a) Draw Lewis structures for chloromethane (CH3Cl), chloroethene (C2H3Cl), and chloroethyne (C2HCl).
Problem 57b
(b) What is the hybridization of the carbon atoms in each molecule?