For each compound, state whether its bonding is covalent, ionic, or a mixture of covalent and ionic.

a. NaCl

b. NaOH

c. CH₃Li

d. CH₂Cl₂

e. NaOCH₃

f. HCO₂Na

g. CF₄

Both PCl₃ and PCl₅ are stable compounds. Draw Lewis structures for these two compounds.

Draw a Lewis Structure for each species.

a. N₂H₄

b. N₂H₂

c. (CH₃)₂NH₂Cl

d. CH₃CN

Draw a Lewis Structure for each species.

e. CH₃CHO

f. CH₃S(O)CH₃

g. H₂SO₄

h. CH₃NCO

Draw a Lewis Structure for each species.

i. CH₃OSO₂OCH₃

j. CH₃C(NH)CH₃

k. (CH₃)₃CNO

Draw a Lewis structure for each compound. Include all nonbonding pairs of electrons.

a. CH₃COCH₂CHCHCOOH

b. NCCH₂COCH₂CHO

Draw a line-angle formula for each compound.

a. CH₃COCH₂CHCHCOOH

b. NCCH₂COCH₂CHO

Draw a line-angle formula for each compound.

c. CH₂CHCH(OH)CH₂CO₂H

d. CH₂CHC(CH₃)CHCOOCH₃

Draw Lewis structures for

a. two compounds of formula C₄H₁₀

b. two compounds of formula C₂H₆O

Draw a complete structural formula and a condensed structural formula for

a. three compounds of formula C₃H₈O

Draw a complete structural formula and a condensed structural formula for

b. five compounds of formula C₃H₆O

Some of the following molecular formulas correspond to stable compounds. When possible, draw a stable structure for each formula. Propose a general rule for the numbers of hydrogen atoms in stable hydrocarbons.

Draw complete Lewis structures, including lone pairs, for the following compounds.

(a)

(b)

(c)

Draw complete Lewis structures, including lone pairs, for the following compounds.

(g)

(h)

Give the molecular formula of each compound shown

(a)

(b)

(c)

Give the molecular formula of each compound shown

(d)

(e)

(f)

Give the molecular formula of each compound shown

(g)

(h)

1. From what you remember of electronegativities, show the direction of the dipole moments of the following bonds.

2. In each case, predict whether the dipole moment is relatively large (electronegativity difference >0.5) or small.

a. C—Cl

b. C—H

c. C—Li

d. C—N

e. C—O

For each of the following structures,

1. Draw a Lewis structure; fill in any nonbonding electrons.

2. Calculate the formal charge on each atom other than hydrogen

d. [(CH₃)₃O]⁺

e. CH₃NC

f. (CH₃)₄NBr

Determine whether the following pairs of structures are actually different compounds or simply resonance forms of the same compounds.

a.

b.

c.

d.

Determine whether the following pairs of structures are actually different compounds or simply resonance forms of the same compounds.

e.

f.

g.

h.

Determine whether the following pairs of structures are actually different compounds or simply resonance forms of the same compounds.

i.

j.

k.

l.

Draw the important resonance forms to show the delocalization of charges in the following ions. In each case, indicate the major resonance form(s).

(j)

(k)

In the following sets of resonance forms, label the major and minor contributors and state which structures would be of equal energy. Add any missing important resonance forms.

(d)

(e)

For each of these ions, draw the important resonance forms and predict which resonance form is likely to be the major contributor.

(a)

For each of these ions, draw the important resonance forms and predict which resonance form is likely to be the major contributor.

(b)

For each of these ions, draw the important resonance forms and predict which resonance form is likely to be the major contributor.

(c)

For each pair of ions, determine which ion is more stable. Use resonance forms to explain your answers.

(e)

(f)

Use resonance structures to identify the areas of high and low electron density in the following compounds:

(a)

(b)

(c)

Use resonance structures to identify the areas of high and low electron density in the following compounds:

g.

h.