What is the effect of resonance on bond length and bond strength?
Resonance leads to bond lengths that are intermediate between single and double bonds, and bond strength that is greater than a single bond but less than a double bond.
What is the effect of a large formal charge on the stability of a Lewis structure?
A large formal charge generally decreases the stability of a Lewis structure.
What happens if you don't draw all resonance structures on the AP exam?
You may lose points, as it indicates an incomplete understanding of resonance.
What is the effect of minimizing formal charges on the stability of a Lewis structure?
Minimizing formal charges generally increases the stability of a Lewis structure.
What happens if you place a negative formal charge on a less electronegative atom?
The Lewis structure becomes less stable.
Label the resonance structures of the nitrate ion ($NO_3^-$).
1: Nitrogen atom, 2: Oxygen atoms, 3: Single bond, 4: Double bond, 5: Lone pairs, 6: Negative charge
Label the key components in the formal charge calculation diagram for SCN-.
1: Sulfur (S), 2: Carbon (C), 3: Nitrogen (N), 4: Single bond, 5: Triple bond, 6: Lone pairs
Label the structure of the phosphate ion ($PO_4^{3-}$) before optimization.
1: Phosphorus atom, 2: Oxygen atoms, 3: Single bonds, 4: Lone pairs, 5: +1 Formal Charge on P, 6: -1 Formal Charge on O
Label the structure of the phosphate ion ($PO_4^{3-}$) after optimization.
1: Phosphorus atom, 2: Oxygen atoms, 3: Single bonds, 4: Double bond, 5: Lone pairs, 6: Formal charge of 0 on P and one O, -1 on the other three O
Label the completed Lewis structure diagram for $S_2Cl_2$.
1: Sulfur (S) atoms, 2: Chlorine (Cl) atoms, 3: Single bonds, 4: Lone pairs on S, 5: Lone pairs on Cl
What are the key differences between resonance structures and isomers?
Resonance Structures: Represent different ways of drawing the *same* molecule, differ only in electron arrangement. | Isomers: Are *different* molecules with the same molecular formula, but different arrangements of atoms.
How do formal charge and oxidation number differ?
Formal Charge: Assumes equal sharing of electrons in a bond. | Oxidation Number: Assumes the more electronegative atom gets all the shared electrons.
