Draw the lewis structure of CH2Cl2. include all lone pairs
The Correct Answer and Explanation is:
Lewis Structure of CH₂Cl₂ (Dichloromethane)
Here’s the Lewis structure of CH₂Cl₂:
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Cl — C — H
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Cl
Now, let’s include all lone pairs:
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:Cl:— C — H
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:Cl:
- Carbon (C) has 4 valence electrons and forms 4 bonds: two single bonds with hydrogen atoms and two single bonds with chlorine atoms.
- Each Hydrogen (H) has 1 valence electron and forms 1 single bond (no lone pairs).
- Each Chlorine (Cl) has 7 valence electrons. In the molecule, each chlorine shares one electron with carbon (a single bond), and retains 3 lone pairs.
Explanation
The Lewis structure of CH₂Cl₂ (dichloromethane) helps us understand how atoms are bonded and where electrons are located within the molecule. First, we count the total number of valence electrons:
- Carbon (C): 4 valence electrons
- Hydrogen (H): 1 × 2 = 2 valence electrons
- Chlorine (Cl): 7 × 2 = 14 valence electrons
- Total = 4 + 2 + 14 = 20 valence electrons
Next, we arrange the atoms. Since carbon is the central atom (it’s the least electronegative among non-hydrogen atoms and can form 4 bonds), it connects to 2 hydrogen atoms and 2 chlorine atoms.
We form single bonds (each 2 electrons) between carbon and each of the other atoms:
- 4 single bonds = 4 × 2 = 8 electrons used
Now we distribute the remaining electrons (20 – 8 = 12 electrons) as lone pairs:
- Hydrogen atoms have no lone pairs (only 1 bond each)
- Chlorine atoms need 3 lone pairs each to complete their octets (6 electrons per Cl)
- So: 2 Cl × 6 = 12 electrons used as lone pairs
Carbon has 4 bonds (8 shared electrons), so it obeys the octet rule. Each chlorine atom has a complete octet (1 bond + 3 lone pairs = 8 electrons). Hydrogens have 2 electrons each, fulfilling their duet requirement.
This structure reflects the correct bonding and lone pairs for each atom, making it the valid Lewis structure for CH₂Cl₂.
