1. A Review of General Chemistry

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

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.

(a)

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

(j) Al

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

(c) B

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

(g) S

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

(i) Cl

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

(l) ―1 charge

Show how the Lewis dot structure for each of the following atoms would overlap to form a single bond.

(b) C and O

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

(b) C vs. O

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

(d) C vs. N

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

(f) C vs. F

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)

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.

(e)

Draw the Lewis structure for the following molecular formulas.

(l) SO₄^2-

In addition to radicals, anions, and cations, a fourth class of reactive intermediates is carbenes. A neutral species, the simplest carbene has a molecular formula of CH₂.

(a) Draw the Lewis structure of CH₂.