Chemistry NCERT Exemplar Solutions Class 12th Chapter Seven

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NO₃⁻ + 3Fe₂⁺ + 4H⁺→ NO⁺ + 3Fe₃⁺ + 2H₂O

[Fe (H₂O)₆]²⁺ + NO → [Fe (H₂O)₅ (NO)]²⁺ + H₂O ( brown ring )

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A is PCl₅ (yellowish white powder)

P₄ + 10Cl₂→4PCl₅

B is PCl₃ (colourless oily liquid)

Hydrolysis of the following product

PCl₃+3H₂O→H3PO₃+3HCl

PCl₅+4H₂O→H3PO₄+5HCl

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Six F atoms can be accommodated around sulphur due to fluorine's tiny size, however the chloride ion is comparably bigger, resulting in interatomic repulsion.

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Oxygen is more electronegative than sulphur, the bond angle of H₂O is greater, and the bod pair electron of an OH bond will be closer to oxygen, causing bond-pair repulsion between bond pairs of two OH bonds

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Chlorine has vacant d-orbitals, which become excited upon bonding when electrons from the 3p-orbital are promoted to the 3d-orbital, giving it a covalency of three.

Due to the lack of unoccupied d-orbitals in the second energy shell, fluorine cannot expand its octet. As a result, it can only have one covalency.

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NO₂ exists as a monomer with one unpaired electron in the gaseous state, but it dimerises to N₂O₄ in the solid state, leaving no unpaired electron, making the solid form diamagnetic.

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Three P—Cl bonds are arranged in one plane at a 1200 angle. These bonds are known as equatorial bonds because they are formed between two points. The remaining two P—Cl bonds, one above the equatorial plane and the other below it, form  90° angle with the plane. Axial bonds are the name for these types of bonds. Because axial bond pairs are subjected to greater repulsive interaction than equatorial bond pairs, axial bonds are slightly longer and hence slightly weaker than equatorial bonds, making the PCl₅ molecule more reactive.

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PH₃ is insoluble in water and cannot create hydrogen bonds with it, it forms bubbles, whereas NH₃ dissolves because it is soluble in water and can form hydrogen bonds with it.

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