Which of the following molecules is non-polar in nature?
- $POCl _{3}$
- $CH _{2} O$
- $SbCl _{5}$
- $NO _{2}$
The Correct Option is C
Solution and Explanation
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.
- $POCl_{3}$: 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, \(POCl_{3}\) is polar.
- $CH_{2}O$: 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, \(CH_{2}O\) is polar.
- $SbCl_{5}$: 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, \(SbCl_{5}\) is non-polar.
- $NO_{2}$: 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, \(NO_{2}\) is polar.
Based on the above analysis, the correct answer is \(SbCl_{5}\), as the molecular geometry ensures that the dipole moments cancel, resulting in a non-polar molecule.
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Concepts Used:
Hybridisation
Hybridization refers to the concept of combining atomic orbitals in order to form new hybrid orbitals that are appropriate to represent their bonding properties. Hybridization influences the bond length and bond strength in organic compounds.
Types of Hybridization:
sp Hybridization
sp hybridization is observed while one s and one p orbital inside the identical principal shell of an atom mix to shape two new equal orbitals. The new orbitals formed are referred to as sp hybridized orbitals.
sp2 Hybridization
sp2 hybridization is observed whilst ones and p orbitals of the same shell of an atom blend to shape three equivalent orbitals. The new orbitals formed are referred to as sp2 hybrid orbitals.
sp3 Hybridization
When one ‘s’ orbital and 3 ‘p’ orbitals belonging to the identical shell of an atom blend together to shape 4 new equal orbitals, the sort of hybridization is referred to as a tetrahedral hybridization or sp3.
sp3d Hybridization
sp3d hybridization involves the joining of 3p orbitals and 1d orbital to form 5 sp3d hybridized orbitals of identical energy. They possess trigonal bipyramidal geometry.
sp3d2 Hybridization
With 1 s three p’s and two d’s, there is a formation of 6 new and identical sp3d2 orbitals.