provide Lewis structure, molecular geometry and hybridization for. CH4. BH3. PF5. XeF2. SF6. NO^- 2. CO^2- 3. CN^- . I^- 3. SF^- 5. NH^+ 4.
The Correct Answer and Explanation is :
Lewis Structures, Molecular Geometry, and Hybridization of Given Molecules/Ions
- CH₄ (Methane)
- Lewis Structure: Carbon in the center with four single bonds to hydrogen atoms.
- Molecular Geometry: Tetrahedral
- Hybridization: sp³
- BH₃ (Borane)
- Lewis Structure: Boron in the center with three single bonds to hydrogen.
- Molecular Geometry: Trigonal planar
- Hybridization: sp²
- PF₅ (Phosphorus Pentafluoride)
- Lewis Structure: Phosphorus in the center with five single bonds to fluorine.
- Molecular Geometry: Trigonal bipyramidal
- Hybridization: sp³d
- XeF₂ (Xenon Difluoride)
- Lewis Structure: Xenon in the center with two single bonds to fluorine and three lone pairs.
- Molecular Geometry: Linear
- Hybridization: sp³d
- SF₆ (Sulfur Hexafluoride)
- Lewis Structure: Sulfur in the center with six single bonds to fluorine.
- Molecular Geometry: Octahedral
- Hybridization: sp³d²
- NO₂⁻ (Nitrite Ion)
- Lewis Structure: Nitrogen in the center, one oxygen with a double bond, one with a single bond and a negative charge.
- Molecular Geometry: Bent
- Hybridization: sp²
- CO₃²⁻ (Carbonate Ion)
- Lewis Structure: Carbon in the center with three oxygen atoms (one with a double bond, two with single bonds and negative charges).
- Molecular Geometry: Trigonal planar
- Hybridization: sp²
- CN⁻ (Cyanide Ion)
- Lewis Structure: Carbon triple-bonded to nitrogen, with a negative charge on carbon.
- Molecular Geometry: Linear
- Hybridization: sp
- I₃⁻ (Triiodide Ion)
- Lewis Structure: Central iodine with two single bonds to two outer iodines, with three lone pairs.
- Molecular Geometry: Linear
- Hybridization: sp³d
- SF₅⁻ (Pentafluorosulfate Ion)
- Lewis Structure: Sulfur in the center with five single bonds to fluorine and one lone pair.
- Molecular Geometry: Square pyramidal
- Hybridization: sp³d²
- NH₄⁺ (Ammonium Ion)
- Lewis Structure: Nitrogen in the center with four single bonds to hydrogen, with a positive charge.
- Molecular Geometry: Tetrahedral
- Hybridization: sp³
Explanation (300 Words)
The Lewis structure of a molecule or ion represents its valence electrons and helps predict bonding. To determine molecular geometry, we use the VSEPR (Valence Shell Electron Pair Repulsion) theory, which states that electron pairs around a central atom repel each other and arrange themselves to minimize repulsion.
For CH₄, NH₄⁺, and SF₆, all bonding pairs contribute to symmetrical shapes like tetrahedral and octahedral. BH₃, CO₃²⁻, and PF₅ have trigonal geometries, while NO₂⁻ and SF₅⁻ exhibit bent and square pyramidal shapes, respectively, due to lone pair repulsions.
Hybridization helps explain orbital mixing in bonding. Carbon in CH₄ undergoes sp³ hybridization, forming four equivalent sigma bonds. In contrast, CO₃²⁻ has sp² hybridization with resonance among oxygen atoms. Linear molecules like XeF₂, CN⁻, and I₃⁻ exhibit sp or sp³d hybridization, where lone pairs influence shape.
Expanded octets occur in elements like phosphorus (PF₅) and sulfur (SF₆, SF₅⁻), using d-orbitals for additional bonding. Ions like NH₄⁺ carry formal charges, affecting structure and bond angles.
Understanding these concepts helps predict reactivity, polarity, and molecular behavior in chemistry.