Question

which of the lewis structures in the image is correct?

Explanation:

• For structure A (methane, \(CH_4\)): Carbon should have 4 valence electrons. In a correct Lewis structure of \(CH_4\), carbon forms 4 single bonds (each bond represents 2 electrons). But in structure A, there are only 3 pairs of non - bonding electrons shown incorrectly around carbon.
• For structure B (\(H_2O\)): Oxygen should have 6 valence electrons. In \(H_2O\), oxygen forms 2 single bonds with hydrogen and has 2 pairs of non - bonding electrons. Structure B shows the electrons in a wrong distribution (with unpaired electrons on oxygen and hydrogen which is not correct as hydrogen has 1 valence electron and forms a single bond, and oxygen should have paired non - bonding electrons).
• For structure C (\(H_2O\)): Oxygen has 6 valence electrons. In \(H_2O\), oxygen forms 2 single bonds (each bond has 2 electrons) with hydrogen and has 2 pairs (4 electrons) of non - bonding electrons. This structure correctly represents the electron distribution around oxygen (2 bonding pairs and 2 non - bonding pairs).
• For structure D (\(NH_3\)): Nitrogen should have 5 valence electrons. In \(NH_3\), nitrogen forms 3 single bonds with hydrogen and has 1 pair of non - bonding electrons. Structure D does not show the non - bonding pair of electrons on nitrogen.

Answer:

C.