Question

which of the lewis structures in the image is correct?

Explanation:

Step1: Analyze option A

Carbon has 4 valence electrons. In option A, carbon forms 3 single bonds (with 3 H atoms), which accounts for 3 electrons, and there are 2 non - bonding electrons (a lone pair). But carbon should have 4 bonds (either single, double, or triple) to complete its octet. So, option A is incorrect.

Step2: Analyze option B

Oxygen has 6 valence electrons. In option B, oxygen forms 2 single bonds (with 2 H atoms), which accounts for 2 electrons. But the way the non - bonding electrons are represented is wrong. There should be 4 non - bonding electrons (2 lone pairs) around oxygen, not the way shown in option B. So, option B is incorrect.

Step3: Analyze option C

Oxygen has 6 valence electrons. In option C, oxygen forms 2 single bonds (with 2 H atoms), which accounts for 2 electrons. And there are 4 non - bonding electrons (2 lone pairs) around oxygen, which correctly represents the valence electron distribution of oxygen in a water - like structure (if we consider a simple O - H bond situation).

Step4: Analyze option D

Nitrogen has 5 valence electrons. In option D, nitrogen forms 4 single bonds (with 4 H atoms). But nitrogen can only form 3 single bonds (or equivalent in terms of bond order) to complete its octet (3 single bonds give 6 electrons from bonds and 2 non - bonding electrons for a total of 8, but here 4 single bonds would over - fill the valence shell in a wrong way). So, option D is incorrect.

Answer:

C.