QQuestionChemistry
QuestionChemistry
Below is the Lewis structure of the chloroform molecule.
Count the number of bonding pairs and the number of lone pairs around the carbon atom.
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Answer
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Step 1:I'll solve this step-by-step while following the precise LaTeX and formatting guidelines:
Step 2:: Analyze the Lewis Structure
In the Lewis structure of chloroform ($$CHCl_{3}$$), we need to carefully count the bonding and lone pairs around the central carbon atom.
Step 3:: Count Bonding Pairs
- Carbon forms single bonds with:
Step 4:
One hydrogen (H)
Step 5:
\text{Bonding Pairs} = 4
Three chlorine (Cl) atoms - Total bonding pairs = 4 single bonds
Step 6:: Count Lone Pairs
\text{Lone Pairs} = 0
- Carbon has no lone pairs in this molecule
Final Answer
- Bonding Pairs: 4 - Lone Pairs: 0 Key Insight: In chloroform, the carbon atom uses all of its valence electrons in single bonds, leaving no lone pairs around the central carbon atom.
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