Molecule AE Lewis Structure EC Hyb’d about X Electronic Geometry Molecular Geometry 3-D P or NP PC13 PC15 C2H4Cl2(1, 1) C2H4Cl2(1, 2) C2H2Cl2(1,1) C2H2Cl2 (1,2-cis) C2H2Cl2 (1,2-trans)
The Correct Answer and Explanation is:
1. PCl3 (Phosphorus Trichloride)
- Lewis Structure: Phosphorus (P) is in the center with three chlorine (Cl) atoms surrounding it. Each Cl atom is single-bonded to P. Phosphorus has one lone pair of electrons.
- Hybridization: sp3
- Electronic Geometry: Tetrahedral
- Molecular Geometry: Trigonal Pyramidal (due to one lone pair)
- Polarity: Polar. The lone pair on phosphorus creates an asymmetry in the electron cloud, leading to a net dipole.
2. PCl5 (Phosphorus Pentachloride)
- Lewis Structure: Phosphorus is the central atom with five chlorine atoms attached via single bonds. No lone pairs on phosphorus.
- Hybridization: sp3d
- Electronic Geometry: Trigonal Bipyramidal
- Molecular Geometry: Trigonal Bipyramidal
- Polarity: Nonpolar. The symmetry of the five chlorine atoms around phosphorus cancels out any dipoles.
3. C2H4Cl2 (1, 1-Dichloroethene)
- Lewis Structure: Each carbon is double-bonded to the other and each is single-bonded to a hydrogen and a chlorine. The chlorine atoms are on the same carbon.
- Hybridization: sp2
- Electronic Geometry: Trigonal Planar (around each carbon)
- Molecular Geometry: Planar, with each carbon in a trigonal planar arrangement.
- Polarity: Polar. The chlorines on the same carbon create a dipole moment, resulting in an overall polar molecule.
4. C2H4Cl2 (1, 2-Dichloroethene)
- Lewis Structure: Similar to 1, 1-Dichloroethene, but the chlorines are on different carbons.
- Hybridization: sp2
- Electronic Geometry: Trigonal Planar (around each carbon)
- Molecular Geometry: Planar. Each carbon is sp2 hybridized, with a trigonal planar geometry.
- Polarity: Polar. The chlorines on opposite sides create a net dipole moment, making the molecule polar.
5. C2H2Cl2 (1, 1-Dichloroethene)
- Lewis Structure: Each carbon is triple-bonded to the other and single-bonded to a hydrogen and a chlorine. Both chlorines are on the same carbon.
- Hybridization: sp
- Electronic Geometry: Linear (around each carbon)
- Molecular Geometry: Linear
- Polarity: Polar. The two chlorines on the same carbon result in an overall dipole moment.
6. C2H2Cl2 (1, 2-Dichloroethene, Cis form)
- Lewis Structure: Same as 1, 2-Dichloroethene, but the chlorines are on the same side of the double bond.
- Hybridization: sp2
- Electronic Geometry: Trigonal Planar (around each carbon)
- Molecular Geometry: Planar. Each carbon is sp2 hybridized with trigonal planar geometry.
- Polarity: Polar. The chlorines being on the same side result in a net dipole moment.
7. C2H2Cl2 (1, 2-Dichloroethene, Trans form)
- Lewis Structure: Same as 1, 2-Dichloroethene, but the chlorines are on opposite sides of the double bond.
- Hybridization: sp2
- Electronic Geometry: Trigonal Planar (around each carbon)
- Molecular Geometry: Planar. Each carbon is sp2 hybridized, with a trigonal planar geometry.
- Polarity: Nonpolar. The opposing directions of the dipoles cancel out, making the molecule nonpolar.
These are the main structures, hybridizations, geometries, and polarities for each molecule based on their respective bonding.
