Identify the correct orders against the property mentioned
A. H₂O > NH₃ > CHCl₃ – dipole moment
B. XeF₄ > XeO₃ > XeF₂ – number of lone pairs on central atom
C. O–H > C–H > N–O – bond length
D. N₂ > O₂ > H₂ – bond enthalpy
Choose the correct answer from the options given below:

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  1. A, D only 
  2. B, D only 
  3. A, C only 
  4. B, C only

Answer (Detailed Solution Below)

Option 1 : A, D only 
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Detailed Solution

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CONCEPT:

Dipole Moment, Lone Pairs, Bond Length, and Bond Enthalpy

  • Dipole Moment: The dipole moment depends on the electronegativity difference between bonded atoms and the molecular geometry.
  • Lone Pairs on the Central Atom: The number of lone pairs can be determined using the molecular structure and valence electrons of the central atom.
  • Bond Length: Bond length is inversely proportional to bond strength and directly related to the size of the atoms involved in the bond.
  • Bond Enthalpy: Bond enthalpy is the energy required to break a bond. Triple bonds are stronger than double bonds, which are stronger than single bonds.

EXPLANATION:

  • H₂O > NH₃ > CHCl₃ – Dipole Moment
    • H₂O has the highest dipole moment due to its bent shape and high electronegativity difference.
    • NH₃ has a lower dipole moment than H₂O, as it is pyramidal and less polar.
    • CHCl₃ has the lowest dipole moment because its geometry partially cancels out dipoles.
    • This order is correct.
  • XeF₄ > XeO₃ > XeF₂ – Number of Lone Pairs on Central Atom
    • XeF₄: Xenon has 4 bonds and 2 lone pairs.
    • XeO₃: Xenon has 3 bonds and 1 lone pair.
    • XeF₂: Xenon has 2 bonds and 3 lone pairs.
    • The correct order of lone pairs is XeF₂ > XeF₄ > XeO₃, so this option is incorrect.
  • O–H > C–H > N–O – Bond Length
    • O–H has the shortest bond length due to high bond strength and small atomic size.
    • C–H is longer than O–H but shorter than N–O.
    • N–O has the longest bond length due to weaker bond strength and larger atomic size.
    • This order is correct.
  • N₂ > O₂ > H₂ – Bond Enthalpy
    • N₂ has the highest bond enthalpy due to the strong triple bond.
    • O₂ has a lower bond enthalpy than N₂ due to its double bond.
    • H₂ has the lowest bond enthalpy due to its single bond.
    • This order is correct.

Therefore, the correct answer is A, D only.

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