AP Chemistry Unit 2

What is the hybridization of carbon in C₂H₂?

• sp³

• sp

• sp²

The Lewis structure of the CO₃^2- ion is

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NGSS.HS-PS1-1

NGSS.HS-PS1-2

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

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NGSS.HS-PS1-3

The ion NO- has _____ valence electrons.

• 10

• 12

• 14

• 15

• 16

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NGSS.HS-PS1-1

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

• 0

• +1

• +2

• +3

• -1

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NGSS.HS-PS1-1

 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^-

The elements C and Se have the same electronegativity value, 2.55. Which of the following claims about the compound that forms from C and Se is most likely to be true?

• The carbon-to-selenium bond is unstable.

• The carbon-to-selenium bond is nonpolar covalent.

• The compound has the empirical formula CSe.

• A molecule of the compound will have a partial negative charge on the carbon atom.

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NGSS.HS-PS1-1

NGSS.HS-PS1-2

Which of the following Lewis diagrams best represents the bonding in the N₂O molecule, considering formal charges?

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NGSS.HS-PS1-1

NGSS.HS-PS1-2