Understanding Bond Polarity and Dipole Moments

What type of bond is formed when the electronegativity difference between two atoms exceeds 2.0?

• Hydrogen bond

• Metallic bond

• Ionic bond

• Covalent bond

Which type of bond is characterized by an electronegativity difference between 0.4 and 2.0?

• Pure covalent bond

• Metallic bond

• Ionic bond

• Polar covalent bond

What is a limitation of using electronegativity difference to measure bond polarity?

• It does not consider bond length

• It is only applicable to ionic bonds

• It has an arbitrary reference point

• It is an absolute scale

What is the formula for calculating the dipole moment?

• mu = Q * R

• mu = Q + R

• mu = Q / R

• mu = Q - R

What is the elementary charge of a proton?

• 0 coulombs

• -1.6 x 10^-19 coulombs

• 1.6 x 10^-19 coulombs

• 3.2 x 10^-19 coulombs

What is the approximate dipole moment of a completely ionic bond with a bond length of 130 picometers?

• 9.4 Debye

• 6.2 Debye

• 12.4 Debye

• 3.0 Debye

What is the unit conversion factor from coulombs times meters to Debye?

• 1 Debye = 3.34 x 10^-32 coulombs times meters

• 1 Debye = 3.34 x 10^-34 coulombs times meters

• 1 Debye = 3.34 x 10^-30 coulombs times meters

• 1 Debye = 3.34 x 10^-28 coulombs times meters

How is percent ionic character calculated?

• Measured dipole divided by bond length

• Measured dipole divided by dipole moment if completely transferred, times 100%

• Measured dipole times bond length

• Measured dipole minus dipole moment if completely transferred, times 100%

What is the measured dipole moment of a diatomic molecule with a bond length of 130 picometers?

• 12.0 Debye

• 6.2 Debye

• 3.0 Debye

• 9.0 Debye

What is the percent ionic character of a bond with a measured dipole moment of 3.0 Debye and a completely transferred dipole moment of 6.2 Debye?

• 24%

• 36%

• 48%

• 60%