QuestionA student proposes the following Lewis structure for the water molecule.
Assign a formal charge to each atom in the student's Lewis structure.
\begin{tabular}{|c|c|}
\hline atom & formal charge \\
\hline left H & \\
\hline & \\
\hline right H & \\
\hline
\end{tabular}
Studdy Solution
STEP 1
1. The Lewis structure provided is for a water molecule, .
2. The formal charge formula is: .
3. Hydrogen typically has 1 valence electron, and oxygen typically has 6 valence electrons.
STEP 2
1. Identify the valence electrons for each atom.
2. Count the non-bonding and bonding electrons for each atom.
3. Calculate the formal charge for each atom using the formula.
STEP 3
Identify the valence electrons: - Hydrogen (H) has 1 valence electron. - Oxygen (O) has 6 valence electrons.
STEP 4
Count the non-bonding and bonding electrons: - Each hydrogen atom is involved in 1 bond, contributing 2 bonding electrons. - Oxygen is involved in 2 bonds (4 bonding electrons) and has 4 non-bonding electrons (2 lone pairs).
STEP 5
Calculate the formal charge for each atom:
- **Left H:**
$ \text{Formal Charge} = 1 - 0 - \frac{1}{2}(2) = 0
\]
- **O:**
$ \text{Formal Charge} = 6 - 4 - \frac{1}{2}(4) = 0
\]
- **Right H:**
$ \text{Formal Charge} = 1 - 0 - \frac{1}{2}(2) = 0
\]
The formal charges for each atom are:
\begin{tabular}{|c|c|}
\hline atom & formal charge \\
\hline left H & \\
\hline & \\
\hline right H & \\
\hline
\end{tabular}
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