List of top Chemistry Questions on Periodic properties asked in JEE Main

Consider the following elements In, Tl, Al, Pb, and Ge. The most stable oxidation states of elements with highest and lowest first ionisation enthalpies, respectively, are:

The electron affinity values are negative for:
A. Be → Be⁻
B. N → N⁻
C. O → O²⁻
D. Na → Na⁻
E. Al → Al⁻
Choose the most appropriate answer from the options given below:

Given below are two statements:
Statement (I): \( \text{SiO}_2 \) and \( \text{GeO}_2 \) are acidic while \( \text{SnO} \) and \( \text{PbO} \) are amphoteric in nature.
Statement (II): Allotropic forms of carbon are due to property of catenation and \( p\pi-d\pi \) bond formation.
In the light of the above statements, choose the most appropriate answer from the options given below:

Match List I with List II

List-I	List-II
A. Melting point [K]	I. Tl > In > Ga > Al > B
B. Ionic Radius [M3/pm]	II. B > Tl > Al ≈ Ga ≈ In
C. ΔiH1 [kJ mol-1]	III. Tl > In > Al > Ga > B
D. Atomic Radius [pm]	IV. B > Al > Tl > In > Ga

Choose the correct answer from the options given below:

The transition metal having highest \(3^\text{rd}\) ionisation enthalpy is:

Given below are two statements :
Statement I: In group 13, the stability of +1 oxidation state increases down the group.
Statement II: The atomic size of gallium is greater than that of aluminium. In the light of the above statements.
Choose the most appropriate answer from the options given below:

Match List - I with List - II.

Choose the correct answer from the options given below.

The number of element from the following that do not belong to lanthanoids is :
Eu, Cm, Er, Tb, Yb and Lu

Match List-I with List-II.

List-I (Elements)	List-II (Properties in their respective groups)
(A) Cl,S	(I) Elements with highest electronegativity
(B) Ge, As	(II) Elements with largest atomic size
(C) Fr, Ra	(III) Elements which show properties of both metals and non metal
(D) F, O	(IV) Elements with highest negative electron gain enthalpy

Choose the correct answer from the options given below:

Identify the incorrect statements about group 15 elements:
(A) Dinitrogen is a diatomic gas which acts like an inert gas at room temperature.
(B) The common oxidation states of these elements are −3, +3 and +5.
(C) Nitrogen has unique ability to form p$\pi$-p$\pi$ multiple bonds.
(D) The stability of +5 oxidation states increases down the group.
(E) Nitrogen shows a maximum covalency of 6.
Choose the correct answer from the options given below.

The statement(s) that are correct about the species O 2^– , F ^– , Na⁺ and Mg²⁺.
(A) All are isoelectronic
(B) All have the same nuclear charge
(C) O2^– has the largest ionic radii
(D) Mg²⁺ has the smallest ionic radii
Choose the most appropriate answer from the options given below :

Lowest oxidation number of an atom in a compound \( A_2B \) is -2. The number of electrons in its valence shell is:

In case of isoelectronic species the size of F^– , Ne and Na⁺ is affected by:

Anomalous behaviour of oxygen is due to its

Given below are two statements:
Statement I: Fluorine has most negative electron gain enthalpy in its group.
Statement II: Oxygen has least negative electron gain enthalpy in its group.
In the light of the above statements, choose the most appropriate from the options given below.

The element having the highest first ionization enthalpy is

The ionic radii of $K^+$, $Na^+$, $Al^{3+}$ and $Mg^{2+}$ are in the order :

The CORRECT order of first ionisation enthalpy is :