Question

Write the C.S.S and draw the resonance hybrid of each of the following:

Answer 1

Hint: Let us first discuss resonance hybrid structures. In any given molecule or ion or atom which exhibits resonance, there exist a few resonance forms that can be understood as the average of two or more resonance structures that define the given species. They are represented as separate structures from the other resonance structures by using double-headed arrows.

Complete step by step answer:
Resonance structures are two or more Lewis structures that describe the delocalization of electrons in a molecule or polyatomic ions. Resonance in chemistry describes the bonding in particular molecules or ions by merging many contributing forms, referred to as canonical structures or resonance structures as per the theory of valence bonding into a hybrid resonance or structures.
The delocalization of electrons takes place by fractional bonds and formal charges in a resonance hybrid. Not all resonance structures are equivalent and we need to determine which one is best describing the actual bonding. To predict which resonance structures are favored, we use formal charges.
Let us look at the carbocation which is given, the lone pair electrons can undergoes;

Note: Out of the two resonance structures of the emulate ion that we have drawn above, the one which places the positive charge on the carbon is the least stable and more reactive. This is because the positive charge will be destabilized more by the greater due to incomplete octane of the carbon atom. But in the next structure octane of carbon is complete which stabilizes that structure more than before.