1. A Review of General Chemistry

Write Lewis structures for the following molecular formulas. Circle any lone pairs (pairs of nonbonding electrons) in the structures.

i. C₃H₆ (one double bond)

j. C₃H₄ (two double bonds)

k. C₃H₄ (one triple bond)

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

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

(g)

(h)

Which atom in each pair would you expect to be the central atom in a Lewis structure?

(b) C vs. O

How many valence electrons does each of the following contribute to a Lewis structure?

(l) ―1 charge

Draw Lewis structures for the following compounds.

e. dimethylamine, CH₃NHCH₃

f. diethyl ether, CH₃CH₂OCH₂CH₃

g. 1-chloropropane,CH₃CH₂CH₂Cl

Draw Lewis structures for the following compounds and ions, showing appropriate ­formal charges.

(i) (CH₃)₂O—BF₃

(j) [HONH₃]⁺

(k) KOC(CH₃)₃

(l) [H₂C=OH]⁺

How many valence electrons does each of the following contribute to a Lewis structure?

(g) S

Given the atoms involved and the number of valence electrons remaining, complete the Lewis structure by placing bonds between atoms such that each has a full octet.

(d)

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

Draw the Lewis structure for each of the following:

f. NaOH