Given below are two statements:
Statement I: The second ionisation enthalpy of Na is larger than the corresponding ionisation enthalpy of Mg .
Statement II: The ionic radius of 
is larger than that of 
.
In the light of the above statements, choose the correct answer from the options given below
Text Solution
Verified by ExpertsD
Statement I examines second ionization enthalpy:
loses its first electron to achieve a stable noble gas configuration. The second ionization would break into the 2 p core, requiring enormous energy.
loses its second electron from the 3s orbital, which is less stable.
Thus, IE 2 of Na is much larger than 
of Mg .
Statement I is TRUE.
Statement II compares 
and 
:
both are isoelectronic with 10 electrons.
has 8 protons while 
has 9 protons.
The lower nuclear charge in 
results in weaker electrostatic attraction, making the ionic radius of 
larger than 
.
Statement II is TRUE.
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