Question:
$H_2O$ has a net dipole moment while $BeF_2$ has zero dipole moment because
$H_2O$ has a net dipole moment while $BeF_2$ has zero dipole moment because
Updated On: Apr 8, 2024
- $H_2O$ molecule is linear while $BeF_2$ is bent
- $BeF_2$ molecule is linear while $H_2O$ is bent
- fluorine has more electronegativity than oxygen
- beryllium has more electronegativity than oxygen
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The Correct Option is B
Solution and Explanation
$H_2O$ have bent structure in which the two $O-H $ bonds are oriented at an angle of 104.5$^{\circ}$, so water have a net dipole moment whereas $BeF_2$ have linear geometry, so the dipole moment of one bond is cancelled by another bond, so it have zero dipole moment.
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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