Bond Polarity (DP IB Chemistry: HL)

• When two atoms in a covalent bond have the same electronegativity the covalent bond is nonpolar

The two chlorine atoms have identical electronegativities so the bonding electrons are shared equally between the two atoms

• When two atoms in a covalent bond have different electronegativities the covalent bond is polar and the electrons will be drawn towards the more electronegative atom
• As a result of this:
  • The negative charge centre and positive charge centre do not coincide with each other
  • This means that the electron distribution is asymmetric
  • The less electronegative atom gets a partial charge of δ+ (delta positive)
  • The more electronegative atom gets a partial charge of δ- (delta negative)

• The greater the difference in electronegativity the more polar the bond becomes

Cl has a greater electronegativity than H causing the electrons to be more attracted towards the Cl atom which becomes delta negative and the H delta positive

Dipole moment

• The dipole moment is a measure of how polar a bond is
• The direction of the dipole moment is shown by the following sign in which the arrow points to the partially negatively charged end of the dipole:

The sign shows the direction of the dipole moment and the arrow points to the delta negative end of the dipole

Answer:

The correct option is B.

• • You have to calculate the difference in electronegativity for the bonds and then rank them from smallest to largest:

NO  (3.4 - 3.0 = 0.4)

OF₂ (4.0 - 3.4 = 0.6)

CO   (3.4 - 2.6 = 0.8)

CF₄  (4.0 - 2.6 = 1.4)