Hybridisation

Carbanion and Hybridization

The given carbanion, , has a negative charge on the carbon that is part of the triple bond (C≡C). The carbon atoms involved in the triple bond (≡) typically undergo sp hybridization to form the bonding orbitals. In this case:

• sp Hybridization: The carbon with the negative charge (C⁻) is sp-hybridized because of the triple bond. In sp hybridization, one s orbital and one p orbital mix to form two sp hybrid orbitals.
• Lone Pair: The electron pair that gives the carbanion's negative charge is present in one of these sp hybrid orbitals, where it is not involved in the bonding of the triple bond but resides as a lone pair on the negatively charged carbon.
• Lone Pair Location: Thus, the lone pair in the carbanion is located in an sp hybrid orbital.

Conclusion:

The lone pair of electrons in the carbanion resides in an sp hybrid orbital due to the nature of the triple bond and sp hybridization of the carbon atoms involved.

Hybridization and Geometry of

is a compound where xenon is bonded to four fluorine atoms through four sigma bonds, and xenon has two lone pairs. The formula for the compound is , where represents the central atom (xenon), represents the bonding atoms (fluorine), and represents the lone pairs on the central atom (xenon).

Explanation:

• Bonds: Xenon forms four sigma bonds with four fluorine atoms, and it has two lone pairs of electrons.
• Hybridization: The hybridization of xenon is , which accounts for six regions of electron density (four bonds and two lone pairs).
• Geometry: The molecular geometry of is octahedral because it involves six regions of electron density (including the lone pairs).
• Shape: The shape of the molecule is square planar because the two lone pairs occupy two opposite positions, leaving the fluorine atoms in a square arrangement around the xenon atom.

Conclusion:

In , xenon undergoes hybridization, resulting in an octahedral geometry with a square planar shape.

To determine which of the given molecules is non-polar, we must consider the molecular geometry and the electronegativity differences between the atoms involved in each molecule. A molecule is non-polar if the dipole moments of the bonds cancel each other out due to symmetrical arrangement.

1. : This molecule has a tetrahedral geometry. The different atoms (P, O, and Cl) have different electronegativities, which leads to dipole moments that do not cancel each other out. Therefore, is polar.
2. : Also known as formaldehyde, it has a trigonal planar geometry with carbon in the center. The difference in electronegativity between C and O, and C and H, results in dipole moments that do not cancel each other. Thus, is polar.
3. : This molecule has a trigonal bipyramidal geometry. Despite differing electronegativities between Sb and Cl, the molecule's symmetrical geometry allows the dipole moments to cancel out completely. Therefore, is non-polar.
4. : This molecule is bent, similar to the structure of water, and as such, has an overall dipole moment due to the differing electronegativities of N and O. Hence, is polar.

Based on the above analysis, the correct answer is , as the molecular geometry ensures that the dipole moments cancel, resulting in a non-polar molecule.