QQuestionChemistry
QuestionChemistry
"Below is the Lewis structure of the acetylene (C₂H₂) molecule:
H:C:::C:H
Count the number of bonding pairs and the number of lone pairs around the left hydrogen atom in this molecule."
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Answer
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Step 1:I'll solve this problem step by step, carefully following the LaTeX formatting guidelines:
Step 2:: Analyze the Lewis Structure
The given Lewis structure shows acetylene ($$\mathrm{C}_{2}\mathrm{H}_{2}$$) with a triple bond between the carbon atoms and single bonds to the hydrogen atoms.
Step 3:: Examine the Left Hydrogen Atom
Looking at the left hydrogen atom (H), we can see that it is directly bonded to a carbon atom with a single bond.
Step 4:: Count Bonding Pairs
- Number of bonding pairs = $$1
- The hydrogen atom forms one single bond with the carbon atom
Step 5:: Count Lone Pairs
- Number of lone pairs = $$0
- The hydrogen atom does not have any lone pairs
Final Answer
- Bonding pairs: 1 - Lone pairs: 0 Key Insight: In the Lewis structure of acetylene, each hydrogen atom forms a single bond with a carbon atom and has no lone pairs of electrons.
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