Question:
The shape of $XeO_2F_2$ molecule is
The shape of $XeO_2F_2$ molecule is
Updated On: Jun 14, 2022
- trigonal bipyramidal
- square planar
- tetrahedral
- see-saw
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The Correct Option is D
Solution and Explanation
In $XeO_2F_2$, the bonding arrangement around the central
atom Xe is
$4s $ bonds + 1.01/7=5
Hybridisation of Xe = $sp^3d$
$sp^3$d-hybridisation corresponds to trigonal bipyramidal
geometry.
Also, in trigonal bipyramidal geometry, lone pairs remain
present on equatorial positions in order to give less
electronic repulsion.
NOTE According to Bent's rule, the more electronegative atoms must
be present on axial position. Hence, F are kept on axial
positions.
atom Xe is
$4s $ bonds + 1.01/7=5
Hybridisation of Xe = $sp^3d$
$sp^3$d-hybridisation corresponds to trigonal bipyramidal
geometry.
Also, in trigonal bipyramidal geometry, lone pairs remain
present on equatorial positions in order to give less
electronic repulsion.
NOTE According to Bent's rule, the more electronegative atoms must
be present on axial position. Hence, F are kept on axial
positions.
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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