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The group \( 14 \) elements A and B have the first ionization enthalpy values of \( 708 \) and \( 715 \, \text{kJ mol}^{-1} \) respectively. The above values are lowest among their group members. The nature of their ions \( A^{2+} \) and \( B^{4+} \) respectively is:

A group \( 15 \) element forms \( d\pi - d\pi \) bond with transition metals. It also forms hydride, which is a strongest base among the hydrides of other group members that form \( d\pi - d\pi \) bond. The atomic number of the element is __________.

Given below are two statements:
Statement (I) : The metallic radius of Al is less than that of Ga.
Statement (II) : The ionic radius of \( \text{Al}^{3+} \) is less than that of \( \text{Ga}^{3+} \).
In the light of the above statements, choose the most appropriate answer from the options given below:

Which of the following happens when \( \mathrm{NH_4OH} \) is added gradually to the solution containing \( 1 \, \text{M} \) \( A^{2+} \) and \( 1 \, \text{M} \) \( B^{3+} \) ions? Given: \( K_{sp}[A(OH)_2] = 9 \times 10^{-10} \) and \( K_{sp}[B(OH)_3] = 27 \times 10^{-18} \) at \( 298 \, \text{K} \).

First ionization enthalpy values of first \( 4 \) group \( 15 \) elements are given below: Choose the correct value for the element that is a main component of apatite family:

Consider the following elements \( \mathrm{In} \), \( \mathrm{Tl} \), \( \mathrm{Al} \), \( \mathrm{Pb} \), \( \mathrm{Sn} \) and \( \mathrm{Ge} \).
The most stable oxidation states of elements with highest and lowest first ionisation enthalpies, respectively, are:

Given below are two statements:
Statement I : \( \mathrm{H_2Se} \) is more acidic than \( \mathrm{H_2Te} \).
Statement II : \( \mathrm{H_2Se} \) has higher bond enthalpy for dissociation than \( \mathrm{H_2Te} \).
In the light of the above statements, choose the correct answer from the options given below:

The correct statements from the following are:
(A) \( \mathrm{Tl^{3+}} \) is a powerful oxidising agent
(B) \( \mathrm{Al^{3+}} \) does not get reduced easily
(C) Both \( \mathrm{Al^{3+}} \) and \( \mathrm{Tl^{3+}} \) are very stable in solution
(D) \( \mathrm{Tl^{+}} \) is more stable than \( \mathrm{Tl^{3+}} \)
(E) \( \mathrm{Al^{3+}} \) and \( \mathrm{Tl^{+}} \) are highly stable
Choose the correct answer from the options given below:

Given below are the atomic number of some group \( 14 \) elements. The atomic number of the element with lowest melting point is:

Given below are the pairs of group \( 13 \) elements showing their relation in terms of atomic radius. (\( \mathrm{B} < \mathrm{Al} \)), (\( \mathrm{Al} < \mathrm{Ga} \)), (\( \mathrm{Ga} < \mathrm{In} \)) and (\( \mathrm{In} < \mathrm{Tl} \)) Identify the elements present in the incorrect pair and in that pair find out the element \( (X) \) that has higher ionic radius \( (M^{3+}) \) than the other one. The atomic number of the element \( (X) \) is:

Given below are two statements:
Statement I : The \( \mathrm{N{-}N} \) single bond is weaker and longer than that of \( \mathrm{P{-}P} \) single bond.
Statement II : Compounds of group \( 15 \) elements in \( +3 \) oxidation states readily undergo disproportionation reactions.
In the light of the above statements, choose the correct answer from the options given below:

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JEE Main 2025 23rd Jan Evening Shift

Given below are the atomic number of some group \( 14 \) elements. The atomic number of the element with lowest melting point is: