Question:
Consider the dipole moments of $NH_3$ and $NF_3$.Which of the following is correct ?
Consider the dipole moments of $NH_3$ and $NF_3$.Which of the following is correct ?
Updated On: Jul 6, 2022
- Dipole moment of $NH_3$ is equal to that of $NH_3$
- Dipole moment of $NH_3$ is equal in magnitude but opposite in sign to that of $NH_3$
- Dipole moment of $NH_3$ is more than that of $NH_3$
- Dipole moment of $NH_3$ is more than that of $NF_3$
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The Correct Option is D
Solution and Explanation
Both $NH_3$ and $NF_3$ have pyramidal structures Electronegativity of N, H and F is in the order F > N > H.
Due to lone pair and polarity of N-H and N-F bonds the dipole moment of $NH_3$ is much more than that of $NF_3$
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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