Question 2 1 Pts Determine The Number Of Valence Electrons For CH2Cl2 And Draw The Lewis Structure. Based On Your Structure, The Electron Geometry Of This Molecule Is Select) The Molecular Geometry Is Select] Bond Angles Are [Select And The Hybridization At The Centralis Sp3
The Correct Answer and Explanation is:
To answer this question about CH₂Cl₂ (dichloromethane), we need to:
1. Determine the number of valence electrons:
We sum the valence electrons of each atom:
- Carbon (C): 4 valence electrons
- Hydrogen (H): 1 valence electron × 2 = 2
- Chlorine (Cl): 7 valence electrons × 2 = 14
Total = 4 (C) + 2 (H) + 14 (Cl) = 20 valence electrons
2. Draw the Lewis structure:
- Carbon (C) is the central atom because it can form 4 bonds.
- Attach two H atoms and two Cl atoms to the central C with single bonds.
- This uses 4 bonds × 2 electrons = 8 electrons.
- Remaining 20 – 8 = 12 electrons go on the Cl atoms to complete their octets (6 electrons per Cl atom as lone pairs).
- Hydrogen atoms already have 2 electrons each, so no lone pairs are needed.
Structure:
H
|
Cl–C–H
|
Cl
Carbon has four single bonds — two to hydrogen and two to chlorine.
3. Electron Geometry:
- The central carbon has four regions of electron density (4 single bonds).
- According to VSEPR theory, four bonding groups with no lone pairs form a tetrahedral electron geometry.
4. Molecular Geometry:
- Since all four regions are bonding pairs (no lone pairs), the molecular geometry is also tetrahedral.
5. Bond Angles:
- In a tetrahedral geometry, the bond angles are approximately 109.5°.
6. Hybridization:
- Carbon forms four sigma (σ) bonds → it uses sp³ hybrid orbitals.
- So, the hybridization at the central atom (C) is sp³.
✅ Final Answers:
- Valence electrons: 20
- Electron geometry: Tetrahedral
- Molecular geometry: Tetrahedral
- Bond angles: 109.5°
- Hybridization: sp³
This analysis follows the VSEPR model, ensuring correct geometry and hybridization. CH₂Cl₂ is a polar molecule due to the difference in electronegativity between hydrogen and chlorine, and the asymmetrical shape leads to a net dipole moment.