Which of the following conversions involves change in both shape and hybridisation?
- $NH _{3} \rightarrow NH _{4}^{+}$
- $CH _{4} \rightarrow C _{2} H _{6}$
- $H _{2} O \rightarrow H _{3} O ^{+}$
- $BF _{3} \rightarrow BF _{4}^{-}$
The Correct Option is D
Solution and Explanation
\(BF _{3}\) combines with \(F ^{-}\) ion to form \(BF _{4}^{-}\).
The shape of the \(BF _{3}\) molecule is a planar triangle with bond angles of \(120^{\circ}\) and \(s p^{2}\) hybridisation.
The shape of the \(BF _{4}^{-1}\) molecule is a tetrahedral with bond angles of \(108^{\circ}\) and \(s p^{3}\) hybridisation.
So, the correct option is (D): \(BF _{3} \rightarrow BF _{4}^{-}\)
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Concepts Used:
Chemical Bonding and Molecular Structure
Such a group of atoms is called a molecule. Obviously, there must be some force that holds these constituent atoms together in the molecules. The attractive force which holds various constituents (atoms, ions, etc.) together in different chemical species is called a chemical bond.
Types of Chemical Bonds:
There are 4 types of chemical bonds which are formed by atoms or molecules to yield compounds.
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- Covalent Bonds - Compounds that contain carbon commonly exhibit this type of chemical bonding.
- Hydrogen Bonds - It is a type of polar covalent bonding between oxygen and hydrogen wherein the hydrogen develops a partial positive charge
- Polar Bonds - In Polar Covalent chemical bonding, electrons are shared unequally since the more electronegative atom pulls the electron pair closer to itself and away from the less electronegative atom.
Factors Affecting Bond Enthalpy in Chemical Bonding:
- Size of the Atom
- Multiplicity of Bonds
- Number of Lone Pair of Electrons Present
- Bond Angle