Answer :

Sure! Let's solve the problem step-by-step to find the formal charge of nitrogen in [tex]\(NH_3\)[/tex] (ammonia).

First, let's recall the formula for calculating the formal charge (FC):

[tex]\[ \text{Formal charge} = \text{Valence electrons} - (\text{Non-bonding electrons} + \text{Number of bonds}) \][/tex]

Now, we'll apply this formula to nitrogen in [tex]\(NH_3\)[/tex]:

1. Valence electrons for nitrogen (N):
Nitrogen is in Group 15 of the periodic table, so it has 5 valence electrons.

2. Non-bonding electrons on nitrogen (N):
In [tex]\(NH_3\)[/tex], nitrogen has one lone pair of electrons. One lone pair consists of 2 electrons.

3. Number of bonds nitrogen (N) forms:
In [tex]\(NH_3\)[/tex], nitrogen forms 3 single bonds with hydrogen atoms.

Let’s substitute these values into the formal charge formula:

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

Now, calculate the values inside the parentheses:
[tex]\[ 2 + 3 = 5 \][/tex]

Finally, subtract this result from the number of valence electrons:
[tex]\[ 5 - 5 = 0 \][/tex]

So, the formal charge of nitrogen in [tex]\(NH_3\)[/tex] is [tex]\(0\)[/tex].

Therefore, the correct answer is:
[tex]\[ \boxed{0} \][/tex]

This means the correct option is:
[tex]\[ \text{b. 0} \][/tex]

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Rewritten by : Barada