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Consider the following elements.

Which of the following is/are true about \( A', B', C' \) and \( D' \)?
\((A)\) Order of atomic radii: \( B' < A' < D' < C' \)
\((B)\) Order of metallic character: \( B' < A' < D' < C' \)

\((C)\) Size of the element: \( D' < C' < B' < A' \)

\((D)\) Order of ionic radii: \( B'^{+} < A'^{+} < D'^{+} < C'^{+} \)

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 decreases across a period.
Reason R : The increasing nuclear charge outweighs the shielding across the period.
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:

Arrange the following elements in the increasing order of number of unpaired electrons in it.
(A) Sc (B) Cr (C) V (D) Ti (E) Mn
Choose the correct answer from the options given below:

The correct statements from the following are:
(A) The decreasing order of atomic radii of group \( 13 \) elements is \( \mathrm{Tl > In > Ga > Al > B} \).
(B) Down the group \( 13 \) electronegativity decreases from top to bottom.
(C) \( \mathrm{Al} \) dissolves in dil. \( \mathrm{HCl} \) and Liberates \( \mathrm{H_2} \) but conc. \( \mathrm{HNO_3} \) renders \( \mathrm{Al} \) passive by forming a protective oxide layer on the surface.
(D) All elements of group \( 13 \) exhibits highly stable \( +1 \) oxidation state.
(E) Hybridization of \( \mathrm{Al} \) in \( [\mathrm{Al(H_2O)_6}]^{3+} \) ion is \( \mathrm{sp^3 d^2} \).
Choose the correct answer from the options given below:

The correct sequence of electron gain enthalpy of the elements listed below is
A. Ar
B. Br
C. F
D. S
Choose the most appropriate from the options given below:

In case of isoelectronic species the size of \( \text{F}^- \), \( \text{Ne} \) and \( \text{Na}^+ \) is affected by:

Match List-I with List-II.

Choose the correct answer from the options given below:

If IUPAC name of an element is "Unununnium" then the element belongs to \( n \)th group of Periodic table. The value of \( n \) is ___________.

10.

Given below are two statements:
Statement I: The metallic radius of \( \mathrm{Na} \) is \( 1.86 \, A^\circ \) and the ionic radius of \( \mathrm{Na^+} \) is lesser than \( 1.86 \, A^\circ \).
Statement II: Ions are always smaller in size than the corresponding elements.
In the light of the above statements, choose the correct answer from the options given below:

11.

Given below are two statements:
Statement (I): Both metals and non-metals exist in p and d-block elements.
Statement (II): Non-metals have higher ionization enthalpy and higher electronegativity than the metals.
In the light of the above statements, choose the most appropriate answer from the options given below:

12.

Element not showing variable oxidation state is :

13.

Given below are two statements :
Statement (I) : The \( 4f \) and \( 5f \) - series of elements are placed separately in the Periodic table to preserve the principle of classification.
Statement (II) : \( s \)-block elements can be found in pure form in nature.
In the light of the above statements, choose the most appropriate answer from the options given below :

14.

The correct order of first ionization enthalpy values of the following elements is:
\( (A) \) \( \mathrm{O} \)
\( (B) \) \( \mathrm{N} \)
\( (C) \) \( \mathrm{Be} \)
\( (D) \) \( \mathrm{F} \)
\( (E) \) \( \mathrm{B} \)
Choose the correct answer from the options given below:

15.

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 statement, choose the most appropriate answer from the options given below:

16.

Given below are two statements:
Statement-I: Along the period, the chemical reactivity of the element gradually increases from group \( 1 \) to group \( 18 \).
Statement-II: The nature of oxides formed by group \( 1 \) elements is basic while that of group \( 17 \) elements is acidic.
In the light of the above statements, choose the most appropriate from the options given below:

17.

Match List I with List II

List-I (Element)	List-II (Electronic Configuration)
(A) N	I. \( [\mathrm{Ar}]\,3 d^{10}\,4s^{2}\,4p^{5} \)
(B) S	II. \( [\mathrm{Ne}]\,3s^{2}\,3p^{4} \)
(C) Br	III. \( [\mathrm{He}]\,2s^{2}\,2p^{3} \)
(D) Kr	IV. \( [\mathrm{Ar}]\,3d^{10}\,4s^{2}\,4p^{6} \)

18.

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

19.

The electron affinity value are negative for:
A. \( \mathrm{Be \to Be^-} \)
B. \( \mathrm{N \to N^-} \)
C. \( \mathrm{O \to O^{2-}} \)
D. \( \mathrm{Na \to Na^-} \)
E. \( \mathrm{Al \to Al^-} \)
Choose the most appropriate answer from the options given below:

20.

Given below are two statements:
Statement I: The correct order of first ionization enthalpy values of Li, Na, F and Cl is \( \mathrm{Na} < \mathrm{Li} < \mathrm{Cl} < \mathrm{F} \).
Statement II: The correct order of negative electron gain enthalpy values of Li, Na, F and Cl is \( \mathrm{Na} < \mathrm{Li} < \mathrm{F} < \mathrm{Cl} \).
In the light of the above statements, choose the correct answer from the options given below:

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JEE Main 2024 29th Jan Evening Shift

The element having the highest first ionization enthalpy is:

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