Question

question 11 (5 points)
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in this molecule, whats the formal charge on the central o atom?
a) -1
b) -2
c) 0
d) +1

Explanation:

Step1: Recall the formula for formal charge

The formula for formal charge \(FC\) is \(FC = V - N - \frac{B}{2}\), where \(V\) is the number of valence electrons of the atom in its free state, \(N\) is the number of non - bonding electrons (lone pair electrons), and \(B\) is the number of bonding electrons.
For oxygen in \(H_2O\), \(V = 6\) (oxygen has 6 valence electrons in its free state).

Step2: Determine \(N\) and \(B\)

In \(H_2O\), the central oxygen atom has 4 non - bonding electrons (\(N = 4\)) and 4 bonding electrons (\(B=4\), since there are 2 \(O - H\) bonds and each bond has 2 electrons).

Step3: Calculate the formal charge

Substitute the values into the formula: \(FC=6 - 4-\frac{4}{2}\)

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Answer:

C. 0