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?

Indicate the hybridization of the central atom in b. AlCl₄^–

Indicate the hybridization of the central atom in d. GeH4.

What is the hybridization of the central atom in a. SiCl4?

What is the hybridization of the central atom in c. SO3?

What is the hybridization of the central atom in d. TeCl2?

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)

Which of the following statements are true? c. A 𝜋 bond is made from the sideways overlap of two p orbitals.

Which of the following statements are true? d. A 𝜋 bond has two regions of overlap on opposite sides of the internuclear axis.

(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?

(b) What is the hybridization of the carbon atoms in each molecule?

Propylene, C₃H₆, is a gas that is used to form the important polymer called polypropylene. Its Lewis structure is (a) What is the total number of valence electrons in the propylene molecule?

Ethyl acetate, C₄H₈O₂, is a fragrant substance used both as a solvent and as an aroma enhancer. Its Lewis structure is

a. What is the hybridization at each of the carbon atoms of the molecule?

Ethyl acetate, C₄H₈O₂, is a fragrant substance used both as a solvent and as an aroma enhancer. Its Lewis structure is

(c) How many of the valence electrons are used to make s bonds in the molecule?

Ethyl acetate, C₄H₈O₂, is a fragrant substance used both as a solvent and as an aroma enhancer. Its Lewis structure is

(e) How many valence electrons remain in nonbonding pairs in the molecule?

Glycine, the simplest amino acid, has the following Lewis structure:

a. What are the approximate bond angles about each of the two carbon atoms, and what are the hybridizations of the orbitals on each of them?

Glycine, the simplest amino acid, has the following Lewis structure:

b. What are the hybridizations of the orbitals on the two oxygens and the nitrogen atom, and what are the approximate bond angles at the nitrogen?

Glycine, the simplest amino acid, has the following Lewis structure:

c. What is the total number of 𝜎 bonds in the entire molecule, and what is the total number of 𝜋 bonds?

d. Would you expect SO3 to exhibit delocalized 𝜋 bonding?

In the formate ion, HCO₂^-, the carbon atom is the central atom with the other three atoms attached to it. (c) Are there multiple equivalent resonance structures for the ion?

In the formate ion, HCO₂^-, the carbon atom is the central atom with the other three atoms attached to it. (d) How many electrons are in the p system of the ion? 

Consider the following Lewis structure:

a. Does the Lewis structure depict a neutral molecule or an ion? If it is an ion, what is the charge on the ion?

Predict the molecular geometry of each of the following molecules: (b) H O C O C O O H