Identify the resonance structure that will be produced given the molecule shown and the electron flow indicated.

(a)

Identify the resonance structure that will be produced given the molecule shown and the electron flow indicated.

(c)

Refer to the following Lewis structures.

(a)

(b)

Predict the hybridization of all non-hydrogen atoms.

Predict the hybridization of all non-hydrogen atoms.

(c)

(d)

Predict the hybridization of all non-hydrogen atoms.

(e)

(f)

(g)

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?

Connect the atoms using the indicated hybrid orbitals.

(b) C (sp²) with C (sp²)

For the following partial structures, the bond is shown. Add the indicated number of bonds, being sure to specify the orientation (that is, x, y, or z axis) of the p orbitals used.

(c)

For the following partial structures, the σ bond is shown. Add the indicated number of π bonds, being sure to specify the orientation (that is, x, y, or z axis) of the p orbitals used.

(e)

Given the Lewis structures, indicate the direction of the dipole moment, if there is one.

(a)

Given the Lewis structures, indicate the direction of the dipole moment, if there is one.

(b)

Given the Lewis structures, indicate the direction of the dipole moment, if there is one.

(e)

Carbon dioxide (CO₂) has no dipole moment (μ = 0 D). The related molecule sulfur dioxide (SO₂) does have a dipole moment (μ = 1.6 D) Explain this observation.

There is free rotation around the C―C bond in ethane. There is an extremely high barrier to rotation around the C=C bond in in ethene. Explain.

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.

Looking ahead in Chapter 4, we explain that molecules like CH₃⁺ are Lewis acids or electron pair acceptors. Into which orbital would the new electron pair go?

In comparison to CH₃⁺ in Assessment 2.82, the related molecule H₃O⁺ is not a Lewis acid at oxygen. Why?

The C―N bond in the following amide is much stronger than the C―N bond in the amine. Explain.

Looking ahead in Chapter 3, we describe how the formal charge on an atom can be used to predict the number of lone pairs. Given the charge, or lack of charge, on each atom, fill in the electron pairs.

(a)

Looking ahead in Chapter 3, we describe how the formal charge on an atom can be used to predict the number of lone pairs. Given the charge, or lack of charge, on each atom, fill in the electron pairs.

(c)

In Chapter 4, we explain that molecules like CH₃^- are Lewis bases or electron pair donors. What makes it a Lewis base?

In comparison to CH₃^- in Assessment 2.86, the related molecule BH₄^- is itself not a Lewis base at boron. Why?