Question:
The bond lengths and bond angles in the molecules of methane, ammonia and water are given below .This variation in bond angle is a result of
(i) the increasing repulsion between hydrogen atoms as the bond length decreases
(ii) the number of non-bonding electron pairs in the molecule
(iii) a non-bonding electron pair having a greater repulsive force than a bonding electron pair
The bond lengths and bond angles in the molecules of methane, ammonia and water are given below .This variation in bond angle is a result of
(i) the increasing repulsion between hydrogen atoms as the bond length decreases
(ii) the number of non-bonding electron pairs in the molecule
(iii) a non-bonding electron pair having a greater repulsive force than a bonding electron pair
Updated On: Jun 6, 2022
- (i), (ii) and (iii) are correct
- (i) and (ii) only are correct
- (ii) and (iii) only are correct
- (i) only is correct
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The Correct Option is C
Solution and Explanation
The variation in bond angle in methane, ammonia and water is a result of the number of non-bonding pairs in the molecules and a lone pair (non-bonding electron pair) have greater repulsion force than bonding pair.
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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