Question

an incomplete lewis structure is shown below. the structure only shows the atoms and how they are connected. the molecule has a net charge of +1. complete the lewis structure giving all atoms full octets. if there is more than one way to do this, draw resonance structures showing all possibilities. if not, just draw one lewis structure. be sure to write in any non - zero formal charges.

Explanation:

Step1: Determine valence electrons

Carbon has 4 valence electrons, hydrogen has 1, oxygen has 6 and nitrogen has 5. The total number of valence - electrons without considering the charge is \(2\times4 + 7\times1+6 + 5=26\). Since the molecule has a net charge of + 1, the actual number of valence electrons is \(26 - 1=25\).

Step2: Satisfy octet rule for carbon

The two carbon atoms already have some bonds. The left - hand carbon has 4 bonds (satisfies octet). The right - hand carbon is bonded to 3 atoms and needs one more pair of electrons.

Step3: Satisfy octet rule for oxygen

Oxygen is bonded to one atom (carbon) and has one bond to hydrogen. It needs 3 lone pairs of electrons to complete its octet.

Step4: Satisfy octet rule for nitrogen

Nitrogen is bonded to 3 hydrogen atoms and one carbon atom. It has a full octet. But to account for the positive charge, we can consider the formal charge. The formal charge on nitrogen is \(FC = 5-(2 + 3)=0\). To get a + 1 charge on the molecule, we can assume that the positive charge is on the oxygen atom. The formal charge on oxygen is \(FC=6-(6 + 1)= - 1\), but if we consider the positive charge of the whole molecule, we can represent the oxygen with a positive charge when it has 3 bonds and 2 lone pairs.
The Lewis structure will have the oxygen atom with a positive charge, 3 bonds (one to carbon, one to hydrogen and one lone pair) and 2 lone pairs, the left - hand carbon with 4 single bonds, the right - hand carbon with 4 single bonds, and nitrogen with 3 single bonds to hydrogen and one single bond to carbon.

Answer:

The oxygen atom will have a positive charge, 3 bonds (C - O, O - H) and 2 lone pairs. The left - hand carbon has 4 single bonds (3 to H and 1 to C), the right - hand carbon has 4 single bonds (1 to C, 1 to N, 1 to O, 1 to H), and nitrogen has 3 single bonds to hydrogen and 1 single bond to carbon.