Question

question 13 (5 points)
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in this molecule, whats the formal charge on the central o atom?
a) 0
b) -2
c) -1
d) +1

Explanation:

Step1: Recall formal charge formula

The formula for formal charge (\(FC\)) is \(FC = V - N - \frac{B}{2}\), where \(V\) is the number of valence electrons in the neutral atom, \(N\) is the number of non - bonding (lone pair) electrons, and \(B\) is the number of bonding electrons.

For oxygen (\(O\)), the number of valence electrons \(V = 6\) (since oxygen is in group 16 of the periodic table).

Step2: Determine \(N\) and \(B\) for the central \(O\) in \(H_2O\)

From the Lewis structure of \(H_2O\) (the given structure), the central \(O\) has 4 non - bonding (lone pair) electrons (\(N = 4\)) and 4 bonding electrons (since there are 2 single bonds, each single bond has 2 electrons, so \(B=4\)).

Step3: Calculate the formal charge

Substitute the values into the formula:
\(FC=6 - 4-\frac{4}{2}\)
First, calculate \(\frac{4}{2}=2\). Then, \(6 - 4-2=0\).

Answer:

A) 0