I\'m trying to draw this Lewis structure but I\'m not sure what I\'m doing wrong
ID: 762749 • Letter: I
Question
I'm trying to draw this Lewis structure but I'm not sure what I'm doing wrong
Determine the formal charge on the nitrogen atom in the following structure. If the atom is formally neutral, indicate a charge of zero Draw an alternative Lewis structure for the compound given in part (a). Show the unshared pairs and nonzero formal charges in your structure. Don't use radicals. Formal charge is the difference between the number of valence electrons in an isolated atom and the number of valence electrons assigned to the atom in a Lewis structure. The number of valence electrons in a single atom equals the element's group number in the periodic table. If the number of the electrons assigned to the atom in a Lewis structure is more than the group number, then the atom has a negative formal charqe; if less, then it is positive. To find the number of valence electrons assigned to an atom, you need to count all of its nonbonding electrons (the ones in unshared pairs) and half of its bonding electrons. Nitrogen is in the group 5A and thus has 5 valence electrons in a neutral atom. In the given structure, nitroqen is shown with a valence-electron count of 4, so it is electron deficient. An alternative Lewis structure will have the same sigma-bond connectivity. Only the electrons from pi bonds and lone pairs may be moved.Explanation / Answer
formal charge on N = 5-(8/2) = +1
CH2(+)-N(:)H2 is lewis structure . +ve sign on Carbon