Classify each of the following bonds as nonpolar covalent,...

Classify each of the following bonds as nonpolar covalent, polar covalent, or ionic on the basis of electronegativity differences.
a. $\mathrm{C}-\mathrm{O}$
b. $\mathrm{Na}-\mathrm{Cl}$
c. $\mathrm{C}-\mathrm{I}$
d. $\mathrm{Ca}-\mathrm{S}$

Key Concepts

Electronegativity Difference

The electronegativity difference between two bonded atoms is the basis for classifying the bond as nonpolar covalent, polar covalent, or ionic. Small differences usually lead to nonpolar covalent bonds, moderate differences create polar covalent bonds, and large differences result in ionic bonds.

Ionic Bond

Ionic bonds are formed when there is a very large difference in electronegativity between atoms, typically between a metal and a non-metal. In these bonds, one atom donates one or more electrons to the other, resulting in the formation of oppositely charged ions that are held together by strong electrostatic forces.

Electronegativity

Electronegativity is a measure of how strongly an atom attracts electrons in a chemical bond. It plays a crucial role in determining how electrons are shared between atoms, influencing the type of bond that forms. Higher differences in electronegativity between bonded atoms typically lead to a greater imbalance in electron sharing.

Nonpolar Covalent Bond

Nonpolar covalent bonds occur when two atoms share electrons almost equally, typically because the atoms have identical or very similar electronegativities. This equal sharing minimizes the formation of partial charges and results in a bond with no significant dipole moment.

Polar Covalent Bond

Polar covalent bonds form when two atoms share electrons unequally due to a moderate difference in electronegativity. This unequal sharing creates a dipole, where one atom acquires a partial negative charge and the other a partial positive charge, leading to an overall polar molecule.

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