Which of the following is an incorrect statement?
- Hydrogen bonding is stronger than dispersion forces
- Sigma bonds are stronger than $\pi$-bonds
- lonic bonding is non-directional :
- $\sigma$-electrons are referred to as mobile electrons
The Correct Option is D
Solution and Explanation
To determine which of the given statements is incorrect, we must analyze each option based on our knowledge of chemical bonding concepts:
- Hydrogen bonding is stronger than dispersion forces:
Hydrogen bonds are a type of dipole-dipole attraction that occurs when hydrogen is bonded to a highly electronegative atom such as nitrogen, oxygen, or fluorine, making it capable of strong intermolecular forces. On the other hand, dispersion forces (London dispersion forces) are the weakest intermolecular forces caused by temporary dipoles. Thus, hydrogen bonding is indeed stronger than dispersion forces. This statement is correct.
- Sigma bonds are stronger than $\pi$-bonds:
A sigma bond (\(\sigma\)) is formed by the head-on overlap of atomic orbitals and is generally stronger than a pi bond (\(\pi\)), which is formed by the side-to-side overlap of atomic orbitals. Sigma bonds are more stable due to this head-on overlap being more effective than the side overlap of pi bonds. Therefore, this statement is correct.
- Ionic bonding is non-directional:
Ionic bonds form due to the electrostatic attraction between ions of opposite charges. Since the force is equal in all directions, ionic bonding is indeed non-directional. Therefore, this statement is also correct.
- $\sigma$-electrons are referred to as mobile electrons:
Sigma (\(\sigma\)) bonds involve localized electrons in a specific bond between two atoms, meaning they are not free to move. On the contrary, mobile electrons are typically found in delocalized pi bonds or metallic bonding where electrons can move freely, contributing to electrical conductivity. Hence, this statement is incorrect.
Therefore, the incorrect statement among the given options is: $\sigma$-electrons are referred to as mobile electrons.
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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.