The second ionization enthalpy of calcium is more than that of the first and yet calcium form ${C a C l}_{2}$ not CaCl. Why ?

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Solution

The higher enthalpy of lattice formation by $C a^{2 +}$ ions more than compensates the higher ionization enthalpy of calcium.

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How would you explain the fact that the first ionization enthalpy of sodium is lower than that of magnesium but its second ionization enthalpy is higher than that of magnesium?

Q. Why first ionization enthalpy of nitrogen is more than oxygen?

Q. Third ionization enthalpy of

C a

is much more greater than that of its second ionisation enthalpy because:

The standard enthalpy of formation

△ H_{f}^{\circ}

, of hypothetical CaCl(s) theoretically found to be

- 188 k J m o l^{- 1}

and that of

C a C l_{2} (s)

- 795 k J m o l^{- 1}

Which of the following compounds is more stable?

Q. Why is the second ionization enthalpy of group 1 elements higher than group 2 elements?

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The second ionization enthalpy of calcium is more than that of the first and yet calcium form CaCl2 not CaCl. Why ?

The higher enthalpy of lattice formation by Ca2+ ions more than compensates the higher ionization enthalpy of calcium.

The second ionization enthalpy of calcium is more than that of the first and yet calcium form ${C a C l}_{2}$ not CaCl. Why ?

The higher enthalpy of lattice formation by $C a^{2 +}$ ions more than compensates the higher ionization enthalpy of calcium.