Understanding Polarity and Dipole Moments

What determines whether a bond is ionic, polar covalent, or nonpolar covalent?

• The temperature at which the bond forms

• The number of atoms in the molecule

• The difference in electronegativity between the atoms

• The size of the atoms involved

Which of the following bonds is considered nonpolar covalent?

• Carbon-carbon

• Carbon-nitrogen

• Sodium-chlorine

• Carbon-oxygen

A carbon-hydrogen bond is classified as:

• Ionic

• Polar covalent

• Nonpolar covalent

• Metallic

Which bond is right at the cusp of being polar?

• Carbon-nitrogen

• Sodium-chlorine

• Carbon-carbon

• Carbon-fluorine

What is the electronegativity difference for a carbon-fluorine bond?

• 2.0

• 1.5

• 1.0

• 0.5

Which of the following is an example of an ionic bond?

• Carbon-carbon

• Carbon-hydrogen

• Carbon-nitrogen

• Sodium-chlorine

What is the dipole moment a product of?

• The difference in atomic radii

• The sum of the atomic masses

• The product of partial charges and distance of separation

• The sum of electronegativities

Which molecule has a dipole moment of zero due to its symmetrical structure?

• Trichloromethane

• Carbon tetrachloride

• Dichloromethane

• Chloromethane

How does the dipole moment of a carbon-oxygen double bond compare to a single bond?

• It is smaller

• It is the same

• It is larger

• It is zero

Why are pi electrons more polarizable than sigma electrons?

• They are less stable

• They have higher energy

• They are more spread out

• They are closer to the nucleus