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

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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

Account for the difference in the shape and color of the potential maps for ammonia and the ammonium ion in Section 1.11.

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If the dipole moment of CH₃F is 1.847 D and the dipole moment of CD₃F is 1.858 D, which is more electronegative: hydrogen or deuterium?

Which of the following has a polar covalent bond?

CH₃NH₂ CH₃CH₃ CH₃F CH₃OH

Which of the following has a bond closest to the ionic end of the bond spectrum?

CH₃NH₂ CH₃CH₃ CH₃F CH₃OH

What is the hybridization of all the atoms (other than hydrogen) in each of the following?

What are the bond angles around each atom?

c. ^-CH₃

d. ⋅CH₃