Question:
The electronegativity difference between N and F is greater than that between N and H yet the dipole moment of NH3 (1.5 D) is larger than that of NF3 (0.2 D). This is because:
The electronegativity difference between N and F is greater than that between N and H yet the dipole moment of NH3 (1.5 D) is larger than that of NF3 (0.2 D). This is because:
Updated On: Oct 20, 2023
- in NH3 as well as in NF3 the atomic dipole and bond dipole are in the same direction
- in NH3 the atomic dipole and bond dipole are in the same direction whereas in NF3 these are in opposite directions
- in NH3 as well as NF3 the atomic dipole and bond dipole are in opposite directions
- in NH3 the atomic dipole and bond dipole are in the opposite directions whereas in NF3 these are in the same directions
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The Correct Option is B
Solution and Explanation
Despite the fact that the electronegativity difference between nitrogen (N) and fluorine (F) is larger than that between nitrogen (N) and hydrogen (H), the dipole moment of NH3 (1.5 D) exceeds that of NF3 (0.2 D). This discrepancy arises because in NH3, the atomic dipole moments and bond dipole moments align in the same direction, while in NF3, they are oriented in opposite directions.
So, the correct option is (B): in NH3 the atomic dipole and bond dipole are in the same direction whereas in NF3 these are in opposite directions.
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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