Understanding Resonance in Chemistry

What is the formal charge on the oxygen atom that is doubly bonded to carbon in the acetate ion's Lewis structure?

• -2

• 0

• -1

• +1

How are resonance structures typically represented in chemical diagrams?

• With a single-headed arrow

• With a double-headed arrow

• With a dashed line

• With a solid line

What is the real structure of a molecule with resonance forms?

• It is none of the resonance forms

• It is the average of the resonance forms

• It is a hybrid of the resonance forms

• It is exactly one of the resonance forms

What is the difference between resonance and equilibrium arrows?

• Resonance arrows indicate a dynamic process

• Equilibrium arrows indicate a static process

• Resonance arrows show a hybrid structure

• Equilibrium arrows show a hybrid structure

Which type of electrons are involved in forming pi bonds?

• Sigma electrons

• Pi electrons

• Valence electrons

• Core electrons

What is a necessary condition for a molecule to have more than one resonance form?

• It must have a positive charge

• It must have an equal number of atoms

• It must have a triple bond

• It must have a pi bond and non-bonding electrons

What must resonance forms adhere to in order to be considered legitimate?

• They must have an equal number of bonds

• They must be legitimate Lewis structures

• They must have the same formal charges

• They must have identical bond lengths

In the example of the conjugate base of acetone, why is one resonance form a larger contributor?

• Because it has more bonds

• Because it is more symmetrical

• Because the negative charge is on a more electronegative atom

• Because it has a higher energy

Why might resonance forms not contribute equally to the real structure?

• Because they have different energies

• Because they have different numbers of atoms

• Because they have different charges

• Because they have different bond angles

What is a common feature of non-equivalent resonance forms?

• They have different energies

• They have different bond lengths

• They have different atoms

• They have the same formal charges