Molecular and Ionic Bonding

O₃ (ozone)

CH₄ (methane)

Cl₂ (chlorine gas)

NH₃ (ammonia)

O₃

CO

CO₂

NH⁴+

Does the presence of a carbonyl group affect the solubility of aldehydes versus ketones in water?

What is the difference in boiling points between ethylene glycol and butan-2-ol?

How do pH changes affect the rate of hydrolysis of acetyl chloride in water?

How does the heat of hydrogenation vary among 1,3-butadiene, cyclopentadiene, and 1,3-cyclohexadiene?

\# valence electrons - (# of lone electrons - # of bonds)

\# valence electrons - (# of bonds - # of lone electrons)

\# valence electrons + (# of lone electrons + # of bonds)

\# valence electrons - (# of lone electrons + # of bonds)

Resonance occurs when there is no possible Lewis structure representation for a given molecule.

If there are multiple ways to represent a molecule with a Lewis structure.

If there is only one way to represent it using a Lewis structure.

If all atoms within a compound have zero formal charge.

Ozone (O3)

Water (H2O)

Sodium Chloride (NaCl)

Methane (CH4)

The structures where sulfur has a formal charge of zero and each oxygen atom carries a -0.5 charge through delocalized electrons.

Structures where one oxygen atom holds a -1 charge while others are neutral emphasizing localized double bonds.

A single structure where sulfur has a +2 formal charge distributing electron density unevenly across oxygens.

Any structure where each oxygen atom has a -1 formal charge disregarding sulfur’s valence shell expansion ability.

H₂O

None of these have resonance structures

CCl₄

CO₃²-

-1

Zero

+1

+2

One triple bond, one lone pair on sulfur

One double bond, one single bond, and a lone pair on sulfur

Two double bonds to sulfur

Two single bonds to sulfur