Compounds of Xenon have one electron pair on central atom :
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Lone pairs are calculated using the formula: Lone pairs = Valence electrons on Xe −Bonding electrons (shared) − Extra electrons
- XeO3
- XeOF2
- XeF4
- XeF5-
The Correct Option is A
Solution and Explanation
Analysis of Lone Pairs on Xenon (Xe):
Using VSEPR theory, the number of lone pairs on the central atom Xenon (Xe) is calculated for each species:
- XeF5+: Xenon has 8 valence electrons. It forms 5 bonds with fluorine, and 1 electron is removed due to the positive charge.
Lone pairs = \(8 - 5 - 1 = 2\) (not a single lone pair). - XeO3: Xenon forms 3 bonds with oxygen atoms.
Lone pairs = \(8 - 6 = 2\) (not a single lone pair). - XeO2F2: Xenon forms 4 bonds (2 with oxygen and 2 with fluorine).
Lone pairs = \(8 - 4 = 1\) (single lone pair). - XeF5−: Xenon forms 5 bonds with fluorine atoms. One extra electron is added due to the negative charge.
Lone pairs = \(8 - 5 + 1 = 2\) (not a single lone pair). - XeO3F2: Xenon forms 5 bonds (3 with oxygen and 2 with fluorine).
Lone pairs = \(8 - 5 = 1\) (single lone pair). - XeOF4: Xenon forms 5 bonds (1 with oxygen and 4 with fluorine).
Lone pairs = \(8 - 5 = 1\) (single lone pair). - XeF4: Xenon forms 4 bonds with fluorine atoms.
Lone pairs = \(8 - 4 = 2\) (not a single lone pair).
Species with a single lone pair: XeO2F2, XeO3F2, XeOF4, XeF5.
Total number of such species: 4.
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Identify the correct orders against the property mentioned:
A. H$_2$O $>$ NH$_3$ $>$ CHCl$_3$ - dipole moment
B. XeF$_4$ $>$ XeO$_3$ $>$ XeF$_2$ - number of lone pairs on central atom
C. O–H $>$ C–H $>$ N–O - bond length
D. N$_2$>O$_2$>H$_2$ - bond enthalpy
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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