AP Chemistry Bonding and Molecular Shapes

The Lewis structure of the CO₃^2- ion is

• 
• 
• 
• 
• 

Tags

NGSS.HS-PS1-2

In the nitrite ion (NO₂^-), __________.

• both bonds are single bonds

• both bonds are double bonds

• both bonds are the same because of resonance

• there are 20 valence electrons

• there is one single and one double bond

Tags

NGSS.HS-PS1-2

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

Of the possible bonds between carbon atoms (single, double, and triple), _____.

• a triple bond is longer than a single bond

• a double bond is stronger than a triple bond

• a single bond is stronger than a triple bond

• a double bond is longer than a triple bond

• a single bond is stronger than a double bond

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

Tags

NGSS.HS-PS1-2

NGSS.HS-PS1-1

The ion NO- has _____ valence electrons.

• 10

• 12

• 14

• 15

• 16

Tags

NGSS.HS-PS1-2

NGSS.HS-PS1-1

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

• 0

• +1

• +2

• +3

• -1

Tags

NGSS.HS-PS1-2

In the Lewis structure of ClF, the formal charge on Cl is _______ and the formal charge on F is _______.

• 0,0

• -1, -1

• 0, -1

• -1, 0

• +1, -1

In the resonance form of ozone shown, the formal charge on the central oxygen atom is _______.

• 0

• +1

• -1

• +2

• -2

Tags

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