Each pair of structures represents two valid resonance structures. Use the arrow-pushing formalism to justify the formation of the one on the left from the one on the right.

(b)

Draw the resonance structure that would result from the indicated movement of electrons.

(a)

For each of the molecules shown, do the following:

(i) Identify all pushable pairs.

(ii) Identify all places where electrons can be pushed.

(iii) Draw one valid resonance structure.

(a)

i) Which of the following resonance structures represents the 'actual' structure of the molecule shown? (ii) Which contributes more to the resonance hybrid? (iii) Why?

(a)

(b)

(c)

To which atom of formaldehyde would you expect H⁺ to add?

Which atoms in the enol ether would you expect to react with Br⁺ ?

Assign the hybridization of the nitrogen in each resonance structure of acetamide.

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?

(j) Al

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.

(a)

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)

By moving an electron pair, draw a better Lewis structure that minimizes formal charges.

(a)

By moving an electron pair, draw a better Lewis structure that minimizes formal charges.

(b)

Draw the Lewis structure for the following molecular formulas.

(j) H₂SO₄

Draw the Lewis structure for the following molecular formulas.

(l) SO₄^2-

Draw the Lewis structure for the following molecular formulas.

(u) NH₄⁺

Draw the Lewis structure for the following molecular formulas.

(v) CH₅N

In the following molecules, identify all pushable electron pairs.

(a)

Two resonance structures are shown for each molecule. Use the arrow-pushing formalism to represent the electron flow from the structure on the left to the one on the right.

(b)

Two resonance structures are shown for each molecule. Use the arrow-pushing formalism to represent the electron flow from the structure on the left to the one on the right.

(d)

Two resonance structures are shown for each molecule. Use the arrow-pushing formalism to represent the electron flow from the structure on the left to the one on the right.

(e)

Two resonance structures are shown for each molecule. Use the arrow-pushing formalism to represent the electron flow from the structure on the left to the one on the right.

(f)