write the resonance desription for the following

A. ClNO2
B. NO-2

Lewis dot structures are quite difficult (actually almost impossible unless VERY simple) to do on these boards. You can try to describe what you have and we can help that way, perhaps.

i don't know what the resonance description is so i don't have anything yet

A. Resonance description for ClNO2:

In ClNO2, the chlorine atom is bonded to the nitrogen atom, which is in turn bonded to an oxygen atom. The resonance description of ClNO2 involves delocalizing the electrons within the molecule.

Step 1: Start by drawing the Lewis structure for ClNO2, with the atoms and their connections.

Cl
|
O = N - O

Step 2: Identify the lone pairs of electrons on the atoms. In ClNO2, the oxygen atoms each have two lone pairs, and the nitrogen atom has one lone pair.

Cl
|
O = N - O
|
(LP)

Step 3: In the resonance description, you can imagine the movement of electrons. The lone pairs on the oxygen atoms can be moved towards the nitrogen atom, forming double bonds and creating a new resonance structure.

O - Cl
|
O = N
|
O

Step 4: In the next resonance structure, you can move the double bond from the nitrogen atom to the chlorine atom.

O
|
O = Cl
|
N
|
O

Step 5: The final resonance structure is obtained by moving the double bond from the chlorine atom to the oxygen atom.

O
|
O = N
|
Cl
|
O

Overall, ClNO2 has multiple resonance structures, indicating electron delocalization within the molecule.

B. Resonance description for NO-2:

In NO-2, the nitrogen atom is negatively charged (NO2-). The resonance description of NO-2 involves the delocalization of the negative charge and the movement of electrons.

Step 1: Start by drawing the Lewis structure for NO-2, with the atoms and their connections.

O
||
O - N

Step 2: Identify the lone pairs of electrons on the atoms. In NO-2, the nitrogen atom has one lone pair.

O
||
O - N
|
(LP)

Step 3: In the resonance description, the lone pair on the nitrogen atom can be moved to form a double bond with one of the oxygen atoms, creating a new resonance structure.

O - N
|
O

Step 4: In the next resonance structure, you can move the double bond from the nitrogen atom to the other oxygen atom.

O
|
O = N

Step 5: The final resonance structure is obtained by moving the double bond from the nitrogen atom to the oxygen atom on the opposite side.

O
|
N = O

Overall, NO-2 (or NO2-) has multiple resonance structures, indicating electron delocalization within the molecule.

To describe the resonance for ClNO2 and NO-2, we need to consider the Lewis structures and the movement of electrons in these molecules.

A. ClNO2:
To represent the resonance in ClNO2, we start by drawing the Lewis structure:

ClNO2: Cl-N=O

Now, let's examine the movement of electrons. The nitrogen atom (N) can form a double bond with either the chlorine atom (Cl) or one of the oxygen atoms (O). This means that we can represent two resonance structures:

Resonance Structure 1:
Cl-N=O

Resonance Structure 2:
Cl=N-O

In the resonance hybrid, the actual structure of ClNO2 is a combination representing the average of these resonance structures. The double bond characters are delocalized, giving partial double bond character to the Cl-N and N-O bonds.

B. NO-2:
For NO-2, we'll start with the Lewis structure:

NO-2: N=O

In this case, the nitrogen atom (N) has a lone pair of electrons, and the oxygen (O) has an extra electron. This excess electron enters a pi (π) bond, resulting in the formation of a double bond between N and O:

Resonance Structure:
N≡O⁻

In the resonance hybrid, the actual structure of NO-2 is a combination representing the average of this resonance structure and the original Lewis structure. The double bond character is delocalized, giving partial double bond character to the N-O bond.