1. A Review of General Chemistry

Refer to the following Lewis structures.

(a)

(b)

Predict the hybridization of all non-hydrogen atoms.

Refer to the following Lewis structures.

(a)

(b)

If an atom is sp² hybridized, how many sp²-hybridized orbitals does it use for bonding? How many p orbitals?

Refer to the following Lewis structures.

(c)

(d)

If an atom is sp² hybridized, how many sp²-hybridized orbitals does it use for bonding? How many p orbitals?

Hydrogen forms bonds without hybridizing. Why?

The C―H σ bond length in ethane is 1.09 Å. The C―H σ bond in ethene is 1.07 Å. Explain.

In propene, the indicated C―C bond length is 1.51 Å. In the allyl cation, the indicated C―C bond length is 1.41 Å. Explain.

What is the hybridization of carbon in each of the following molecules?

(a)

What is the hybridization of carbon in each of the following molecules?

(d)

Draw the molecular orbital picture for propane. Your picture should clearly show the shape and hybridization of the carbons. Label all σ bonds.

Predict the shape and hybridization of the indicated atoms.

What orbitals are used to form the carbon–carbon s bond between the highlighted carbons?

g.

h.

i.

What orbitals contain the electrons represented as lone pairs in the structures of quinoline, indole, imidazole?

What orbital do the lone-pair electrons occupy in each of the following compounds?

a.

b.

c.

In addition to radicals, anions, and cations, a fourth class of reactive intermediates is carbenes. A neutral species, the simplest carbene has a molecular formula of CH₂.

(b) What are the hybridization and shape of the central carbon of CH₂?

Predict the hybridization of the indicated atoms.

(b)