1. A Review of General Chemistry

Draw the Lewis structure for the following ions. Be sure to calculate the formal charge of each atom to confirm that your structure is correct.

(b) H⁺

Draw the Lewis structure for the following ions. Be sure to calculate the formal charge of each atom to confirm that your structure is correct.

(d) AlCl₄^-

Calculate the formal charge of the indicated atoms in the ions shown.

Calculate the formal charge on the non-hydrogen atoms in the molecules shown. Use the arrow-pushing formalism to 'move' an electron pair such that it is shared between two (formerly) charged atoms. Your arrow should account for the formation of the molecule on the right from the molecule on the left.

Looking ahead in Chapter 3, we describe how the formal charge on an atom can be used to predict the number of lone pairs. Given the charge, or lack of charge, on each atom, fill in the electron pairs.

(a)

Based on the formal charge, determine how many lone pairs are on each indicated atom.

(a)

Give each atom the appropriate formal charge:

a.

b.

Draw the missing lone-pair electrons and assign the missing formal charges for the following:

c.

d.

Give each atom the appropriate formal charge:

c.

d.

Draw the missing lone-pair electrons and assign the missing formal charges for the following:

a.

b.

For each of the following compounds and ions,

1. Draw a Lewis structure.

2. Show the kinds of orbitals that overlap to form each bond.

3. Give approximate bond angles around each atom except hydrogen.

d. CH₃–CH=CH₂

e. HC≡C–CHO

f. H₂N–CH₂–CN

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

Draw the Lewis structure for each of the following:

d. ⁺C2H5

Draw the Lewis structure for each of the following:

e. CH₃N⁺H₃

Draw the Lewis structure for the following molecular formulas.

(u) NH₄⁺