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According to Fajans rule covalent bond is favoured by:
According to Fajans rule covalent bond is favoured by:
Updated On: Jun 17, 2022
- small cation and large anion
- small cation and small anion
- large cation and large anion
- large cation and small anion
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The Correct Option is A
Solution and Explanation
According to Fajans rule : (i) The cations with smaller size have higher polarising power. (ii)The anions with large size have high polarisability. (iii)There should be high charge on cation or theanionorboth. (iv) Cations with pseudo inert gas configuration $ (n{{s}^{2}}{{p}^{6}}{{d}^{10}}) $ or with inert pair configuration $ {{d}^{10}}(n+1){{s}^{2}}, $ have high polarising power, while cations with noble gas configuration $ (n{{s}^{2}}{{p}^{6}}) $ have low polarising power.
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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.
- Ionic Bonds - Ionic bonding is a type of chemical bonding which involves a transfer of electrons from one atom or molecule to another.
- 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
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