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JEE CHEMISTRY MCQ: CHEMICAL BONDING & MOLECULAR STRUCTURE

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Statement I: If hydration energy is greater than lattice energy, the solid dissolves in liquid.

Statement II: The solubility of solid in a liquid depends upon lattice energy and hydration energy.
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Correct option: A
If both Statement I and Statement II are correct and Statement II is the correct explanation of Statement I
Option A (If both Statement I and Statement II are correct and Statement II is the correct explanation of Statement I) is correct because the relative magnitudes of hydration and lattice energy determine solubility.

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The hybridization in sulphur dioxide is CO2\mathrm{C}{\mathrm{O}_2} has the same geometry as: (A)HgCl2,(B)NO2,(C)SnCl4,(D)C2H2\left( A \right)\mathrm{HgC}{\mathrm{l}_2},\left( B \right)\mathrm{N}{\mathrm{O}_2},\left( C \right)\mathrm{SnC}{\mathrm{l}_4},\left( D \right){\mathrm{C}_2}{\mathrm{H}_2} The pair of molecules forming strongest hydrogen bonds are Paramagnetism is shown by Which statement is correct? Assertion (A) : BF3{BF}_3 is a weaker Lewis acid than BCl3{BCl}_3.

Reason (R) : The planar BF3{BF}_3 molecule is stabilised to a greater extent than BCl3{BCl}_3 by B−Xπ{B}-X \pi-bonding.
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