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

What hybridization do you expect for the atom indicated in red in each of the following species? (a) CH3CO2-

Which of the following statements about molecular orbitals and hybrid orbitals are true?

a. Molecular orbitals and hybrid orbitals are both created by mathematically mixing the wave functions of atomic orbitals.

b. Molecular orbitals are made by combining atomic orbitals from different atoms.

c. Hybrid orbitals and molecular orbitals are different names for the same things.

d. A hybrid orbital can hold more electrons than can a molecular orbital.

Consider the H₂⁺ ion. (a) Sketch the molecular orbitals of the ion and draw its energy-level diagram.

Consider the H₂⁺ ion. (b) How many electrons are there in the H₂⁺ ion?

Consider the H₂⁺ ion. (c) Write the electron configuration of the ion in terms of its MOs. (d) What is the bond order in H₂⁺?

Consider the H₂⁺ ion. (e) Suppose that the ion is excited by light so that an electron moves from a lower-energy to a higher-energy MO. Would you expect the excited-state H₂⁺ ion to be stable or to fall apart?

Consider the H2+ ion. f. Which of the following statements about part (e) is correct: i. The light excites an electron from a bonding orbital to an antibonding orbital, ii. The bond order of the ion does not change when an electron is excited, or iii. In the excited state there are more bonding electrons than antibonding electrons?