Identify the correct Lewis structure  of CH3− . Ensure that all charges and lone pairs are shown.Group of answer choices

The Lewis structure for CH3- (methyl anion) is drawn step by step as follows:

1. Count the total number of valence electrons. Carbon has 4, each hydrogen has 1, and there is an extra 1 from the negative charge. So, total valence electrons = 4+(3*1)+1 = 8.

2. Draw a skeleton structure of the molecule. Carbon is less electronegative than hydrogen, so it is the central atom. Draw a single bond (two electrons) between the carbon and each hydrogen atom.

3. Subtract the electrons used in step 2 from the total valence electrons. 8 - 6 = 2. These remaining electrons are lone pairs.

4. Place the remaining electrons on the central atom. Carbon now has a lone pair of electrons.

5. Check the formal charges. Each hydrogen atom has a formal charge of 0. Carbon has 4 valence electrons in its free state, but now it has 5 (3 from the bonds with hydrogen and 2 from the lone pair), so its formal charge is -1. This matches with the overall charge of the molecule.

So, the Lewis structure of CH3- is H3C:− where ":" represents the lone pair of electrons and "−" represents the negative charge.