Which out of NH3 and NF3 has higher dipole moment and why?
Solution and Explanation
In both molecules i.e., \(NH_3\) and \(NF_3\), the central atom \((N)\) has a lone pair electron and there are three bond pairs. Hence, both molecules have a pyramidal shape. Since fluorine is more electronegative than hydrogen, it is expected that the net dipole moment of \(NF_3\) is greater than \(NH_3\). However, the net dipole moment of \(NH_3\) \((1.46 \;D)\) is greater than that of \(NF_3\) \((0.24 \;D)\).
This can be explained on the basis of the directions of the dipole moments of each individual bond in NF3 and NH3. These directions can be shown as:
Thus, the resultant moment of the \(N-H\) bonds add up to the bond moment of the lone pair (the two being in the same direction), whereas that of the three \(N - F\) bonds partly cancels the moment of the lone pair.
Hence, the net dipole moment of \(NF_3\) is less than that of \(NH_3\).
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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