resonance hybrid sturture of C2H5N?
- electron1Lv 76 months ago
Each hydrogen atom makes a single bond. Each carbon atom will make four bonds. The nitrogen atom will make three bonds. In this problem, a double bond must exist between two atoms. A double bond can exist between the two carbon atoms. Or a double bond must be between a carbon atom and the nitrogen atom. As you look at the resonance hybrid structures that pisgahchemist drew, you can that first structure has a double bond between the second carbon atom and the nitrogen atom. For the second carbon atom to have four bonds, the first carbon atom must be bonded to three hydrogen atoms. As you look at the second resonance hybrid, you can see that the first carbon atom is only bonded to hydrogen atoms. But the nitrogen atom is bonded to two hydrogen atoms. During this resonance process, the position of the hydrogen atoms changed. For the number of hydrogen atoms that are bonded to a carbon or nitrogen atom, the oxidation number of each of these elements must change. I guess that we could call this an oxidation – reduction reaction. I hope some of this is helpful for you.
- pisgahchemistLv 76 months ago
CH3−CH=NH <−> CH2=CH−NH2
Is this an example of resonance or isomerism?
- klyposLv 66 months ago
CH2=CH-NH2 The nitrogen is trigonal and the lone pairs can enter into conjugation with the C=C across the C-N bond. Just draw it and add dotted lines as appropriate.