Given below are two statements:
Statement I: The second ionization enthalpy of B, Al and Ga is in the order of $B > Al > Ga$ .
Statement II: The correct order in terms of first ionization enthalpy is $Si < Ge < Pb < Sn$ .
In the light of the above statements, choose the correct answer from the options given below:

Question

Given below are two statements:
Statement I: The second ionization enthalpy of B, Al and Ga is in the order of

B > Al > Ga

.
Statement II: The correct order in terms of first ionization enthalpy is

Si < Ge < Pb < Sn

.
In the light of the above statements, choose the correct answer from the options given below:

Quantrex Academy · Accepted Answer

Correct answer: B. Both Statement I and Statement II are false

Statement I: The second ionization enthalpy of Ga is higher than that of Al. This is due to the poor shielding effect of the ten

3d

electrons in Ga, which increases the effective nuclear charge and holds the valence electrons more tightly. The correct order of second ionization enthalpy is

B > Ga > Al

. Thus, Statement I is false.

Statement II: The first ionization enthalpy generally decreases down the group. However, Pb has a slightly higher ionization enthalpy than Sn due to the poor shielding of

4f

and

5d

electrons (lanthanoid contraction). The correct order of first ionization enthalpy for Group 14 elements is

Sn < Pb < Ge < Si < C

. Thus, Statement II is false.

Both Statement I and Statement II are false.

Answer: Both Statement I and Statement II are false

Given below are two statements: Statement I: The second ionization...

Options

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