What is the Lewis structure, electron pair geometry, molecular geometry, polarity, formal charge (on each element), and hybridization of the following molecules? a. HCFO b. XeO
c. PO
(has more than one structure)
The Correct Answer and Explanation is:
Let’s go through each molecule one by one: HCFO, XeO, and PO, including Lewis structure, electron pair geometry, molecular geometry, polarity, formal charges, hybridization, and an explanation.
a. HCFO (Fluoroformaldehyde)
Lewis Structure:
H–C(=O)–F
O is double bonded to C, F and H are single bonded.
Electron Pair Geometry (EPG): Trigonal planar (around carbon)
Molecular Geometry (MG): Trigonal planar
Polarity: Polar (dipole from O and F)
Hybridization: sp² (carbon)
Formal Charges:
- H: 0
- C: 0
- O: 0
- F: 0
Explanation:
Carbon forms 3 sigma bonds: one with H, one with F, and one double bond (1 sigma + 1 pi) with oxygen. This suggests sp² hybridization, leading to a trigonal planar shape around carbon. Due to the electronegativity differences between O and F, the molecule is polar.
b. XeO (Xenon Monoxide)
Lewis Structure:
Xe=O
(Xe has one double bond with O and two lone pairs)
EPG: Tetrahedral (due to 2 lone pairs + 2 bonding domains)
MG: Bent
Polarity: Polar
Hybridization: sp³ (Xe)
Formal Charges:
- Xe: 0
- O: 0
Explanation:
Xenon, although a noble gas, can expand its octet. With one double bond to oxygen and two lone pairs, the geometry is bent. The polarity arises from the oxygen’s higher electronegativity.
c. PO (Phosphorus Monoxide)
Lewis Structures (Resonance):
- P≡O (triple bond)
- P=O with a formal charge separation: P⁺–O⁻
EPG: Linear
MG: Linear
Polarity: Polar
Hybridization: sp (P and O)
Formal Charges:
- In P≡O: P = 0, O = 0
- In P⁺–O⁻: P = +1, O = –1
Explanation:
PO is a diatomic molecule, usually with multiple bonding (triple or double). Resonance suggests a mix between P≡O and P⁺–O⁻. The molecule is polar and linear, and both atoms are sp hybridized. The formal charge separation stabilizes the molecule despite its small size.
Conclusion (Summary):
Each molecule shows different hybridizations (sp, sp², sp³), geometries, and formal charge distributions. Polarity is a common feature due to high electronegativity atoms (O, F). Lewis structures help predict geometry and bonding, with formal charges validating the most stable resonance structures.
