Answer
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Step 1:I'll solve this problem step by step, focusing on drawing the correct Lewis structure for ethene (C^2H4).
Step 2:: Determine the total number of valence electrons
- Total valence electrons: $$(2 \times 4) + (4 \times 1) = 8 + 4 = 12
- Carbon (C) has 4 valence electrons - Hydrogen (H) has 1 valence electron
Step 3:: Arrange the atoms
- Place the two carbon atoms next to each other - Attach two hydrogen atoms to each carbon atom
Step 4:: Connect atoms with single bonds
- First, connect the two carbon atoms with a single bond - This uses 2 electrons
Step 5:: Distribute remaining electrons
- Remaining electrons: $$12 - 2 = 10
- Add single bonds between carbons and hydrogens - This uses 8 more electrons
Step 6:: Check electron distribution
- These 2 electrons form a double bond between the carbon atoms Final Lewis Structure: \begin{array}{c} H-C=C-H \ | \ / | \ H \ H \end{array}
Final Answer
The correct Lewis structure of C^2H^4 shows a double bond between the two carbon atoms, with two hydrogen atoms attached to each carbon.
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