AP Chemistry Unit 2 Review

Count the number of sigma and pi bonds in this molecule:

• 13 sigma, 1 pi

• 14 sigma, 2 pi

• 1 sigma, 14 pi

• 2 sigma, 13 pi

What is the hybridization of carbon in C₂H₂?

• sp³

• sp

• sp²

The Lewis structure of the CO₃^2- ion is

• 
• 
• 
• 
• 

Tags

NGSS.HS-PS1-3

The Lewis structure of N₂H₂ shows __________.

• a nitrogen-nitrogen triple bond

• a nitrogen-nitrogen single bond

• each nitrogen has one lone pair

• each nitrogen has two lone pairs

• each hydrogen has one lone pair

The ion NO- has _____ valence electrons.

• 10

• 12

• 14

• 15

• 16

Tags

NGSS.HS-PS1-1

The formal charge on carbon in the molecule shown is _______.

• 0

• +1

• +2

• +3

• -1

Potassium iodide, KI,has the following bonding:

• ionic

• metallic

• nonpolar covalent

• polar covalent

Tags

NGSS.HS-PS1-1

NGSS.HS-PS1-2

NGSS.HS-PS1-3

 A lone pair is defined as

• A pair of bonding electrons

• One non-bonding electron

• A pair of non-bonding electrons

• A pair of electrons on the central atom

How are compounds with metallic bonds similar to ionic compounds? 

• Both tend to have double and triple bonds

• Both tend to have low boiling points 

• Both tend to have poor conductivity

• Both tend to have high melting points 

The melting point of MgO is higher than that of NaF. Which of the following best explains this observation?

• O^2- is more negatively charged than F-

• Mg²⁺ is more positively charged than Na+

• The O^2- ion is smaller than the F^- ion

• Mg²⁺ is more positively charged than Na⁺ and O^2- is more negatively charged than F^-