Formula: AsF_(5) 5+(7**5) Lewis structure 5+35 =>40 Molecular Shape Drawing Electronic groups: 5 sigma bonded pair Electronic Shape: Molecular Shape: Ideal Bond Angle: Hybridization: sp^(3)d 10. Formula: SF_(4) Molecular Shape Drawing Electronic groups: Electronic Shape: Molecular Shape: Ideal Bond Angle: Hybridization: 8 9.Formula:AsFs 6 + (+ 5) Lewis structure 5+35 0h= Molecular Shape Drawing As .F Electronic groups: 5 sigma boned pair Electronic Shape: Molecular Shape: Ideal Bond Angle: HybridizationS’ 10.Formula:SF4 6+Lewis structure 0G 5 6+28 =734 Molecular Shape Drawing S F F :F :F. Electronic groups: Electronic Shape: Molecular Shape: Ideal Bond Angle: Hybridization:
The Correct Answer and Explanation is:
Let’s break down the given formulas and their corresponding characteristics:
1. AsF₅⁺
- Lewis Structure: In AsF₅⁺, arsenic (As) is the central atom, surrounded by five fluorine atoms. The positive charge indicates that one electron has been lost from the arsenic atom. The Lewis structure shows As forming five bonds with five F atoms, and arsenic has an expanded octet.
- Electronic Groups: 5 sigma bonded pairs (one for each As-F bond).
- Electronic Shape: Trigonal bipyramidal.
- Molecular Shape: Trigonal bipyramidal.
- Ideal Bond Angle: 90° (between axial and equatorial positions), 120° (between equatorial positions).
- Hybridization: sp³d (because there are five bonding regions around arsenic).
2. SF₄
- Lewis Structure: In SF₄, sulfur (S) is the central atom, bonded to four fluorine (F) atoms. One lone pair is present on the sulfur atom.
- Electronic Groups: 5 (4 sigma bonds + 1 lone pair).
- Electronic Shape: Trigonal bipyramidal (due to five regions of electron density).
- Molecular Shape: See-saw (the lone pair repels one of the equatorial bonds, creating a distorted shape).
- Ideal Bond Angle: The angles between the fluorine atoms will be less than the ideal 90° and 120° due to the lone pair.
- Hybridization: sp³d (because there are five regions of electron density).
3. AsF₆⁺
- Lewis Structure: In AsF₆⁺, arsenic (As) is at the center, bonded to six fluorine (F) atoms, with no lone pairs on arsenic. The positive charge suggests arsenic has lost an electron.
- Electronic Groups: 6 sigma bonds (one for each As-F bond).
- Electronic Shape: Octahedral (due to six regions of electron density).
- Molecular Shape: Octahedral.
- Ideal Bond Angle: 90° (between all positions).
- Hybridization: sp³d² (since there are six regions of electron density).
4. SF₄ (Again)
- The structure and properties for SF₄ have already been described above. Repeating the answer for clarification:
- Lewis Structure: Similar to the first description, sulfur is bonded to four fluorine atoms, with one lone pair.
- Electronic Shape: Trigonal bipyramidal.
- Molecular Shape: See-saw.
- Hybridization: sp³d.
Explanation:
- Hybridization is determined by the number of electron pairs (both bonding and lone pairs) around the central atom. In these molecules, the hybridization depends on how many regions of electron density surround the central atom (this could be bonding pairs or lone pairs).
- Molecular Shape is the 3D arrangement of atoms (not electron clouds) in space. Lone pairs tend to repel bonds, which is why molecular shapes might differ from electronic shapes. For example, SF₄ has a see-saw shape due to the lone pair, while AsF₅⁺ and AsF₆⁺ retain their ideal geometries since no lone pairs are involved.
These structures are prime examples of molecules that involve expanded octets, where elements in the third period or beyond (such as arsenic and sulfur) can accommodate more than eight electrons in their valence shell.
