Q. The enthalpy change of solution involves release or absorption of energy by adding 1 mole of ionic solid in sufficient

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Q. Lattice energy is inversely proportional to sum of radii of

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Q. After ionic salts come in contact with water, they form bonds called

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Q. The energy released by gaseous ions when dissolving in water is called enthalpy change of

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Q. Lead carbonate (PbCO₃) only dissolves 0.00017g in dm³ of water, hence it is regarded as

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Q. Increase in radius of metal ion will decrease its

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Q. When ionic solid dissolves in water

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Q. Strong acids completely ionize in

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Q. Water may act as

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Q. Water has very low extent of

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Q. In compost, the reaction takes place among

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Q. The value of ionic product of water is

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Q. On ionizing, water molecules (H₂O) the products include

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Q. The lattice energy is always

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Q. When ions of opposite charges come together to form a crystal lattice is called

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Q. Under standard conditions the energy with enthalpy change when 1 mole of an ionic compound is formed from its gaseous ions is

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Q. Many ionic compounds have some covalent ability due to

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Q. The ionic radius of cation will be smaller and more efficient in polarizing

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Q. The degree of polarization depends on

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Q. Group II nitrates decompose to give off

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