Which of the following has

a. the most polar bond?

b. the least polar bond?

NaI LiBr Cl₂ KCl

Use the symbols δ⁺ and δ⁻ to show the direction of the polarity of the indicated bond in each of the following compounds:

c. H₃C—NH₂

d. H₃C—Cl

Use the symbols δ⁺ and δ⁻ to show the direction of the polarity of the indicated bond in each of the following compounds:

e. HO—Br

f. H₃C—Li

Use the symbols δ⁺ and δ⁻ to show the direction of the polarity of the indicated bond in each of the following compounds:

g. I—Cl

h. H₂N—OH

Explain why HCl has a smaller dipole moment than HF, even though the H—Cl bond is longer than the H—F bond.

After examining the potential maps for LiH, HF, and H₂, answer the following questions:

<IMAGE>

a. Which compounds are polar?

b. Why does LiH have the largest hydrogen?

c. Which compound has the hydrogen that would be most apt to attract a negatively charged molecule?

Draw the Lewis structure for each of the following:

f. NaOH

Draw two Lewis structures for C₂H₆O.

Draw three Lewis structures for C₃H₈O.

Draw the lone-pair electrons that are not shown in the following condensed structures:

a. CH₃CH₂NH₂

b. CH₃NHCH₃

c. CH₃CH₂OH

Draw condensed structures for the compounds represented by the following models (black = C, gray = H, red = O, blue = N, and green = Cl):

a. <IMAGE>

b. <IMAGE>

Draw condensed structures for the compounds represented by the following models (black = C, gray = H, red = O, blue = N, and green = Cl):

c. <IMAGE>

d. <IMAGE>

Change the following condensed structures to Kekulé structures:

a. CH₃NH(CH₂)₂CH₃

b. (CH₃)₂CHCl

Explain why a σ bond formed by overlap of an s orbital with an sp³ orbital of carbon is stronger than a σ bond formed by overlap of an s orbital with a p orbital of carbon.

Put a number in each of the blanks:

a. ___ s orbital and ___ p orbitals form ____ sp³ orbitals.

b. ___ s orbital and ___ p orbitals form ____ sp² orbitals.

c. ___ s orbital and ___ p orbitals form ____ sp orbitals.

For each of the given species:

a. Draw its Lewis structure.

b. Describe the orbitals used by each carbon atom in bonding and indicate the approximate bond angles.

3. CCl₄

For each of the given species:

a. Draw its Lewis structure.

b. Describe the orbitals used by each carbon atom in bonding and indicate the approximate bond angles.

2. HCN

For each of the given species:

a. Draw its Lewis structure.

b. Describe the orbitals used by each carbon atom in bonding and indicate the approximate bond angles.

1. H₂CO₂

For each of the given species:

a. Draw its Lewis structure.

b. Describe the orbitals used by each carbon atom in bonding and indicate the approximate bond angles.

4. H₂CO₃

Predict the approximate bond angles in

a. the methyl cation.

b. the methyl radical.

c. the methyl anion.

According to the potential map for the ammonium ion <IMAGE>, which atom has the greatest electron density?

Describe the orbitals used in bonding and the bond angles in the following compounds:

a. CH₃O^-

Describe the orbitals used in bonding and the bond angles in the following compounds:

c. H₂CO

Describe the orbitals used in bonding and the bond angles in the following compounds:

d. N₂

Describe the orbitals used in bonding and the bond angles in the following compounds:

e. BF₃

What is the hybridization of each of the C, N, and O atoms in the following compounds:

Predict the approximate bond angles for

c. the H—C—N bond angle in (CH₃)₂NH.

d. the H—C—O bond angle in CH₃OCH₃

Which of the following molecules would you expect to have a dipole moment of zero?

a. CH₃CH₃

b. H₂C═O

c. CH₂Cl₂

Which of the following molecules would you expect to have a dipole moment of zero?

d. NH₃

e. H₂C═CH₂

f. H₂C═CHBr

Which of the following molecules would you expect to have a dipole moment of zero?

g. BeCl₂

h. BF₃