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Metals generally melt at very high temperature. Amongst the following, the metal with the highest melting point will be:

Element "E" belongs to the period \( 4 \) and group \( 16 \) of the periodic table. The valance shell electron configuration of the element, which is just above "E" in the group is:

The IUPAC nomenclature of an element with electronic configuration \( [\mathrm{Rn}]5f^{14}6d^{1}7s^{2} \) is :

Match List-I with List-II

Choose the correct answer from the options given below.

The correct order of increasing ionic radii is

Given two statements below:
Statement I: In \( \mathrm{Cl_2} \) molecule the covalent radius is double of the atomic radius of chlorine.
Statement II: Radius of anionic species is always greater than their parent atomic radius.
Choose the most appropriate answer from options given below:

Outermost electronic configurations of four elements A, B, C, D are given below:
(A) \( 3s^2 \) (B) \( 3s^2 3p^1 \) (C) \( 3s^2 3p^3 \) (D) \( 3s^2 3p^4 \)
The correct order of first ionization enthalpy for them is:

The correct order of electron gain enthalpies of \( \mathrm{Cl} \), \( \mathrm{F} \), \( \mathrm{Te} \) and \( \mathrm{Po} \) is

The first ionization enthalpy of \( \mathrm{Na} \), \( \mathrm{Mg} \) an \( \mathrm{Si} \), respectively, are: \( 496 \) and \( 737 \) and \( 786 \) \( \mathrm{kJ \, mol^{-1}} \). The first ionization enthalpy (\( \mathrm{kJ \, mol^{-1}} \)) of \( \mathrm{Al} \) is:

The correct decreasing order of metallic character is:

The incorrect statement is:

The electronic configuration of Pt (atomic number \( 78 \)) is:

The metal that has very low melting point and its periodic position is closer to a metalloid is:

The first ionization enthalpies of \( \mathrm{Be} \), \( \mathrm{B} \), \( \mathrm{N} \) and \( \mathrm{O} \) follow the order.

Given below are two statements. One is labelled as Assertion A and the other is labelled as Reason R.
Assertion A: The first ionization enthalpy for oxygen is lower than that of nitrogen.
Reason R: The four electrons in \( 2p \) orbitals of oxygen experience more electron-electron repulsion.
In the light of the above statements, choose the correct answer from the options given below:

Given below are the oxides:
\( \mathrm{Na}_{2}\mathrm{O}, \ \mathrm{As}_{2}\mathrm{O}_{3}, \ \mathrm{N}_{2}\mathrm{O}, \ \mathrm{NO} \) and \( \mathrm{Cl}_{2}\mathrm{O}_{7} \)
Number of amphoteric oxides is:

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JEE Main 2022 27th July Evening Shift

Outermost electronic configurations of four elements A, B, C, D are given below:
(A) \( 3s^2 \) (B) \( 3s^2 3p^1 \) (C) \( 3s^2 3p^3 \) (D) \( 3s^2 3p^4 \)
The correct order of first ionization enthalpy for them is: