1
MCQ (Single Correct Answer)

JEE Main 2016 (Online) 10th April Morning Slot

The following statements concern elements in the periodic table. Which of the following is true ?
A
All the elements in Group 17 are gases.
B
The Group 13 elements are all metals.
C
Elements of Group 16 have lower ionization enthalpy values compared to those of Group 15 in the corresponding periods.
D
For Group 15 elements, the stability of + 5 oxidation state increases down the group.
2
MCQ (Single Correct Answer)

JEE Main 2017 (Online) 8th April Morning Slot

Consider the following ionization enthalpies of two elements 'A' and 'B' .

Element Ionization enthalpy (kJ/mol)
1st 2nd 3rd
A 899 1757 14847
B 737 1450 7731


Which of the following statements is correct ?
A
Both ‘A’ and ‘B’ belong to group-1where ‘B’ comes below ‘A’.
B
Both ‘A’ and ‘B’ belong to group-1 where ‘A’ comes below ‘B’.
C
Both ‘A’ and ‘B’ belong to group-2 where ‘B’ comes below ‘A’.
D
Both ‘A’ and ‘B’ belong to group-2 where ‘A’ comes below ‘B’.

Explanation

From the table you can see ionization enthalpy of A is greater than B in all the cases.

So, B comes below A in the group as in a group from top to bottom ionization enthalpy decreases.

After 1st ionization enthalpy each element become cation by removing a electron. In A+ and B+, after removing one electron from each element, effective nuclear charge increases as per-electron attraction increase by the neuclers. So, the removal of next electron will be more difficult, therefore more energy is required for 2nd ionization energy. From the table you can see 2nd ionization energy is more than first ionization energy for both elements.

But you can see 3rd ionization enthalpy is so much higher than 2nd ionization enthalpy. It means after 2nd ionization enthalpy outermost shell is empty and in 3rd ionization enthalpy from a new shell electron is removed, as the new shell is closer to the neucleus so the attraction by the nucleus to the electrons of this shell is more and to remove a electron from this shell you have to provide very high energy, that is why 3rd ionization enthalpy is so high.

If A and B are from group 1 then after 1st ionization enthalpy outermost shell will be empty and 2nd electron will be removed from inner shell, so 2nd ionization will be so high. But from table you can see 2nd ionization energy is around double of 1st ionization energy, it is not so much high than 1st onization energy. So A and B can't be from group 1.

A and B are from group 2 as in group 2 element, outermost shell has 2 electron and after 2nd ionization enthalpy outermost shell will be empty and in 3rd ionization enethalpy, third electron will removed from innershell so 3rd ionization enthalpy will be very high.
3
MCQ (Single Correct Answer)

JEE Main 2017 (Online) 9th April Morning Slot

The electronic configuration with the highest ionization enthalpy is :
A
[Ne] 3s2 3p1
B
[Ne] 3s2 3p2
C
[Ne] 3s2 3p3
D
[Ar] 3d10 4s2 4p3

Explanation

In option (D) electron is removed from 4p subshell for 1st ionization enthalpy, but in all other options electron is removed from 3p subshell. As 3p subshell is closer to nucleus than 4p, then attraction to the electrons in 3p subshell is more compared to the electrons in 4p subhell. That is why removal of electrons from 4p subshell is easy compared to 3p subshell. So among all the options, option (D) will have least ionization enthalpy.

Among (A), (B), (C) options, (C) has half filled 3p subshell so it is more stable compare to the others and you have to provide more energy to remove electrons from stable 3p subshell. That is why electron configuration [Ne] 3s2 3p3 has highest ionization enthalpy.
4
MCQ (Single Correct Answer)

JEE Main 2018 (Online) 15th April Morning Slot

For Na+, Mg2+, F- and O2-; the correct order of increasing ionic radii is :
A
O2- < F- < Na+ < Mg2+
B
Na+ < Mg2+ < F- < O2-
C
Mg2+ < Na+ < F- < O2-
D
Mg2+ < O2- < Na+ < F-

Explanation

Here all of them are isoelectric. For isoelectric anion size is more than cation. Among two anions which anion has more negative charge will have more radius and among two cation which cation has less positive charge will have more radius.

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