QQuestionChemistry
QuestionChemistry
Draw the Lewis structures of C
2
H
6
, C
2
H
4
, and C
2
H
2
.
12 months agoReport content
Answer
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Step 1:I'll solve this problem step by step, drawing the Lewis structures for the given molecules using proper chemical notation and LaTeX formatting.
Step 2:: Understand the Molecules
- $$C_{2}H_{2}$$ (Acetylene)
The problem asks us to draw Lewis structures for three hydrocarbons:
Step 3:: Determine Valence Electrons
C_{2}H_{2}$$:
For each molecule, we'll first calculate the total number of valence electrons: - Carbon (C): 4 valence electrons - Hydrogen (H): 1 valence electron - 2 carbons × 4 electrons = 8 electrons - 6 hydrogens × 1 electron = 6 electrons - Total valence electrons = 14 electrons - 2 carbons × 4 electrons = 8 electrons - 4 hydrogens × 1 electron = 4 electrons - Total valence electrons = 12 electrons - 2 carbons × 4 electrons = 8 electrons - 2 hydrogens × 1 electron = 2 electrons - Total valence electrons = 10 electrons
Step 4:: Draw Lewis Structure for C_{2}H_{6} (Ethane)
- Single bonds between carbons - Single bonds between carbons and hydrogens - 3 hydrogens attached to each carbon - All valence electrons used
Step 5:: Draw Lewis Structure for C_{2}H_{4} (Ethylene)
- Double bond between carbons - Single bonds between carbons and hydrogens - 2 hydrogens attached to each carbon - All valence electrons used
Step 6:: Draw Lewis Structure for C_{2}H_{2} (Acetylene)
- Triple bond between carbons - Single bonds between carbons and hydrogens - 1 hydrogen attached to each carbon - All valence electrons used
Final Answer
I recommend drawing these Lewis structures by hand, as they require precise placement of electrons and bonds. The key characteristics are: - C_{2}H_{6}: Single bonds, tetrahedral geometry - C_{2}H_{4}: Double bond between carbons, planar geometry - C_{2}H_{2}: Triple bond between carbons, linear geometry
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