Question

on a sheet of paper, draw the lewis structure for the following compound. please use the periodic table if needed. nh₃ sample answer: h - n - h | h check all features below that you included in your lewis structure. correct number of n and h atoms n as the central atom line (single bond) between n and all three h atoms two dots (electrons) associated with the n atom no other lines or dots

Explanation:

• Correct number of \(N\) and \(H\) atoms: In \(NH_3\), there is 1 \(N\) atom and 3 \(H\) atoms as per the formula.
• \(N\) as the central atom: \(N\) is more electronegative than \(H\) and can form more bonds (has more valence electrons to share in bonding), so it is the central atom.
• Line (single bond) between \(N\) and all three \(H\) atoms: \(N\) has 5 valence electrons (\(2s^22p^3\)) and \(H\) has 1 valence electron (\(1s^1\)). Each \(H\) shares 1 electron with \(N\) to form a single covalent bond (\(N - H\)), and there are three such bonds in \(NH_3\).
• Two dots (electrons) associated with the \(N\) atom: After forming three \(N - H\) bonds (using 3 of its 5 valence electrons), \(N\) has a lone pair (2 electrons) left, which is represented as two dots on the \(N\) atom in the Lewis structure.
• No other lines or dots: All valence electrons are accounted for (3 in \(N - H\) bonds and 2 as a lone pair on \(N\)), so there are no extra bonds or non - bonding electrons to represent.

Answer:

All the checkboxes (correct number of \(N\) and \(H\) atoms, \(N\) as the central atom, line (single bond) between \(N\) and all three \(H\) atoms, two dots (electrons) associated with the \(N\) atom, no other lines or dots) should be checked.