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What is the formal charge on atom N in the following Lewis structure?

A. 2
B. 1
C. 0
D. -1
E. -2

Sagot :

GinnyAnsweridn
To determine the formal charge on the nitrogen (N) atom in the given Lewis structure, we will follow these steps:

1. Determine the number of valence electrons for the nitrogen atom. Nitrogen is in Group 15 of the periodic table and has 5 valence electrons.

2. Identify the number of non-bonded (lone pair) electrons on the nitrogen atom in the Lewis structure. Let's assume from the given Lewis structure that there are 2 non-bonded electrons on the nitrogen atom.

3. Count the number of bonds the nitrogen atom is involved in. Each bond is considered as a pair of electrons shared between the nitrogen atom and another atom. Let's assume that the nitrogen atom is involved in 3 bonds.

4. Calculate the formal charge using the formula:

[tex]\[ \text{Formal Charge} = \text{Number of Valence Electrons} - (\text{Number of Non-Bonded Electrons} + \text{Number of Bonds}) \][/tex]

- Number of Valence Electrons: 5
- Number of Non-Bonded Electrons: 2
- Number of Bonds: 3

5. Substitute the values into the formula:

[tex]\[ \text{Formal Charge} = 5 - (2 + 3) \][/tex]

[tex]\[ \text{Formal Charge} = 5 - 5 \][/tex]

[tex]\[ \text{Formal Charge} = 0 \][/tex]

So, the formal charge on the nitrogen atom in the given Lewis structure is 0.

The correct answer is:
c. 0
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