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

The correct order of C, N, O and F in terms of second ionisation potential is
Given below are two statements:
Statement I: $\mathrm{K>Mg>Al>B}$ is the correct order in terms of metallic character.
Statement II: Atomic radius is always greater than the ionic radius for any element.
In the light of the above statements, choose the correct answer from the options given below:
Given below are two statements:
Statement I: The first ionization enthalpy of Cr is lower than that of Mn.
Statement II: The second and third ionization enthalpies of Cr are higher than those of Mn.
In the light of the above statements, choose the correct answer from the options given below:
Out of \( \mathrm{N, P, S, Cl, F} \), number of valence electrons in the {least metallic element and most metallic element respectively is: }
The correct order of electron gain enthalpy (magnitude only) for group 16 elements is:
Correct order of 2$^{nd}$ ionisation energy is:
The correct order of ionization energy of Cl, S, P, Al, Si is:
Consider the following statements about group 13 elements of the periodic table. (A) Electronegativity decreases down the group.
(B) Size increases down the group.
(C) Ionization energy decreases down the group.
(D) Boiling point of Boron is maximum.
(E) Melting point of Boron is maximum.
Correct order of ionisation enthalpy is:
The correct order of ionisation energy of Cl, S, P, Al, Si is:
In period 4 of the periodic table which elements have the lowest and highest atomic radii respectively?
Given below are two statements: Statement I: The correct order for radius is \( \text{Al}>\text{Mg}>\text{Mg}^{2+}>\text{Al}^{3+} \). Statement II: Atomic size always depends on electronegativity. In the light of the above statements, choose the correct option.
Electronegativity difference between a group 15 element and $\text{P}$ is less than electronegativity difference between another group 15 element and $\text{P}$. Those group 15 elements respectively are :
Which of the following is the correct order with respect to the property indicated?
$K_2Cr_2O_7 + KI \xrightarrow{H^+} I_2 + Cr^{3+}$
Statement-I : Size of $O^{2-}$ is smaller than $F^-$.
Statement-II: Second ionization energy of $\text{Na}$ is greater than second ionization energy of $\text{Mg}$.
Four elements from the second period Boron to Oxygen can have the following IE$_1$ values (in kJ mol$^{-1}$): 1086.5, 800.6, 1313.9, 1402.3. The value of IE$_1$ for Nitrogen is:
Given below are two statements: Statement-I: The correct order for radius is \[ \mathrm{Al > Mg> Mg^{2+} > Al^{3+}} \] Statement-II: Atomic size always depends on electronegativity. In the light of the above statements, choose the correct option.
Choose the incorrect trend in the atomic radii (r) of the elements :
Consider the following statements:
Statement I: $H_2Se$ is more acidic than $H_2Fe$
Statement II: $H_2Se$ has higher bond dissociation enthalpy
In light of the above statements, choose the correct option.
Correct order of electronegativity in below elements:
The correct option with order of melting points of the pairs (Mn, Fe), (Tc, Ru) and (Re, Os) is:
For the reaction, $$ H_2(g) + I_2(g) \rightleftharpoons 2HI(g) $$ Attainment of equilibrium is predicted correctly by: 
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:

For the reaction, $H_2(g) + I_2(g) \rightleftharpoons 2HI(g)$

Attainment of equilibrium is predicted correctly by: 


 
 

An element 'E' has the ionisation enthalpy value of 374 kJ mol\(^{-1}\). 'E' reacts with elements A, B, C, and D with electron gain enthalpy values of \( -328 \), \( -349 \), \( -325 \), and \( -295 \) kJ mol\(^{-1}\), respectively. The correct order of the products EA, EB, EC, and ED in terms of ionic character is: