AP Chemistry Unit 2.2 & 2.5 Practice

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 ability of an atom in a molecule to attract electrons is best quantified by the ______.

• electronegativity

• paramagnetism

• diamagnetism

• electron change-to-mass ratio

• first ionization energy

Which atom can accommodate an octet of electrons, but doesn't necessarily have to accommodate an octet?

• N

• C

• H

• O

• B

Tags

NGSS.HS-PS1-1

As the number of covalent bonds between two atoms increases, the distance between the atoms ______ and the strength of the bond between them ______.

• increases, increases

• decreases, decreases

• increases, decreases

• decreases, increases

• is unpredictable

Which of these bonds takes the most energy to break?

• single

• double

• triple

• quadruple

Tags

NGSS.HS-PS1-4

Potassium iodide, KI,has the following bonding:

• ionic

• metallic

• nonpolar covalent

• polar covalent

Tags

NGSS.HS-PS1-2

The electronegativity of C is 2.5, F is 4.0.  predict the character of a C-F bond.

• polar covalent
• nonpolar covalent
• ionic
• metallic

The following molecules all contain polar bonds however only one is a polar molecule.  Which one?

• CCl₄
• CO₂
• NH₃
• CH₄

 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 

Tags

NGSS.HS-PS1-1