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1 month ago

Draw a lewis structure for hccl3. Show all unshared pairs and the formal charges

Chemistry

1 answer:

eduard [2.7K]1 month ago

6 0

Explanation:

Lewis-dot structure: It illustrates how the atoms in a molecule are bonded together and indicates the presence of unpaired electrons in the molecule.

The molecule in question is, $HCCl_3$

Carbon possesses '4' valence electrons, hydrogen has '1' valence electron, and chlorine contains '7' valence electrons.

Consequently, the cumulative count of valence electrons in $HCCl_3$ = 1(1) + 1(4) + 3(7) = 26

Based on the electron-dot structure, there are 8 bonding electrons and 18 non-bonding electrons.

The electron-dot representation for $HCCl_3$ is depicted below.

Next, we need to assess the formal charges on carbon, hydrogen, and chlorine.

The formula for calculating formal charge:

$\text{Formal charge}=\text{Valence electrons}-\text{Non-bonding electrons}-\frac{\text{Bonding electrons}}{2}$

$\text{Formal charge on carbon}=4-0-\frac{8}{2}=0$

$\text{Formal charge on hydrogen}=1-0-\frac{2}{2}=0$

$\text{Formal charge on chlorine}=7-0-\frac{2}{2}=0$

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