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.
12 months agoReport content
Answer
Full Solution Locked
Sign in to view the complete step-by-step solution and unlock all study resources.
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.
Need Help with Homework?
Stuck on a difficult problem? We've got you covered:
- Post your question or upload an image
- Get instant step-by-step solutions
- Learn from our AI and community of students