Question: Label each bond in the following compounds as ionic or covalent.

$$\begin{gathered} a\mathit{.}\mathit{}{F}_{\mathit{2}} \\ b\mathit{.}\mathit{}LiBr \\ c\mathit{.}\mathit{}C{H}_{\mathit{3}}C{H}_{\mathit{3}} \\ d\mathit{.}\mathit{}NaN{H}_{\mathit{2}} \\ e\mathit{.}\mathit{}NaOC{H}_{\mathit{2}} \end{gathered}$$

The atoms in a covalent bond have electrostatic attraction, and the reacting atoms are neutral. These bonds have low polarity and are weak. The covalent bond formation is shown below:

Representation of a covalent bond formation

The atoms in an ionic bond possess electron pairs, and the reacting atoms carry a specific electric charge, that is, either positive or negative.These bonds have high polarity and are strong. The ionic bond formation is shown below:

Representation of an ionic bond formation

The bonds are classified as ionic or covalent based on atomic charges. Two neutral atoms will form a covalent bond, whereas two charged species will form an ionic bond.

The fluorine-fluorine bond in is covalent. The lithium-bromine bond in is ionic because of the presence of lithium ion and bromide ion . All the carbon-hydrogen bonds in are covalent.

The two nitrogen-hydrogen bonds in are covalent, but the bond between sodium and nitrogen is ionic due to positive and negative charges on sodium and nitrogen, respectively.

The three carbon-hydrogen bonds and one carbon-oxygen in are covalent, whereas the sodium-oxygen bond is ionic due to charges on the atoms.