Classification of Elements and Periodicity — JEE Main PYQs

The correct set that contains all kinds (basic, acidic, amphoteric and neutral) of oxides is :

Given below are two statements :

Statement I : The second ionization enthalpy of B, Al and Ga is in the order of B > Al > Ga.

Statement II : The correct order in terms of first ionization enthalpy is Si < Ge < Pb < Sn.

In the light of the above statements, choose the correct answer from the options given below :

A monoatomic anion ($\mathrm{A^-}$) has 45 neutrons and 36 electrons. Atomic mass, group in the periodic table and physical state at room temperature of the element (A) respectively are

The $1^{\text{st}}$ ionization enthalpy for Mg is +737 kJ/mol. The most probable estimated value of $2^{\text{nd}}$ ionization enthalpy of Mg is ________.

Given below are two statements:

Statement I: The correct order of electronegativity of fluorine, oxygen and nitrogen is F > O > N.

Statement II: The oxidation state of oxygen in $\mathrm{OF_2}$ is +2 and in $\mathrm{Na_2O}$ is $-2$.

In the light of the above statements, choose the correct answer from the options given below

Given below are two statements :

Statement I : The number of pairs among $\mathrm{[Al_2O_3,\ Cr_2O_3]}$, $\mathrm{[Cl_2O_7,\ Mn_2O_7]}$, $\mathrm{[Na_2O,\ V_2O_3]}$ and $\mathrm{[CO,\ N_2O]}$ that contain oxides of same nature (acidic, basic, neutral or amphoteric) is 4.

Statement II : Among $\mathrm{Na_2O}$, $\mathrm{Al_2O_3}$, $\mathrm{CO}$ and $\mathrm{Cl_2O_7}$, the most basic and acidic oxides are $\mathrm{Na_2O}$ and $\mathrm{Cl_2O_7}$, respectively.

In the light of the above statements, choose the correct answer from the options given below :

First and second ionization enthalpies of lithium are 520 kJ mol$^{-1}$ and 7297 kJ mol$^{-1}$ respectively. Energy required to convert 3.5 mg lithium (g) into $\mathrm{Li^{2+}(g)}$ [$\mathrm{Li(g) \rightarrow Li^{2+}(g)}$] is ________ kJ mol$^{-1}$. (nearest integer)

[Molar mass of Li = 7 g mol$^{-1}$]

In a period, the first ionisation enthalpy of the element at extreme left and the negative electron gain enthalpy of the extreme right element, except noble gases, are respectively.

Match List - I with List - II.

	List - I (Electronic configuration of neutral atom (where n = 2))		List - II (1$^{st}$ Ionization Energy (kJ mol$^{-1}$))
A.	$ns^2$	I.	2080
B.	$ns^2np^1$	II.	899
C.	$ns^2np^3$	III.	800
D.	$ns^2np^6$	IV.	1402

Choose the correct answer from the options given below :

The property/properties that show irregularity in first four elements of group-17 is/are :

(A) Covalent radius (B) Electron affinity (C) Ionic radius (D) First ionization energy

Choose the correct answer from the options given below :

Electronic configuration of four elements A, B, C and D are given below :

(A) $\mathrm{1s^2 2s^2 2p^3}$ \quad (B) $\mathrm{1s^2 2s^2 2p^4}$ \quad (C) $\mathrm{1s^2 2s^2 2p^5}$ \quad (D) $\mathrm{1s^2 2s^2 2p^2}$

Which of the following is the correct order of increasing electronegativity (Pauling's scale) ?

Which of the following statements are correct ?

A. The process of adding an electron to a neutral gaseous atom is always exothermic. B. The process of removing an electron from an isolated gaseous atom is always endothermic. C. The 1$^{st}$ ionization energy of boron is less than that of beryllium. D. The electronegativity of C is 2.5 in $\mathrm{CH_4}$ and $\mathrm{CCl_4}$ E. Li is the most electropositive among elements of group I.

Choose the correct answer from the options given below:

Match the LIST-I with LIST-II

LIST-I (Family)	LIST-II (Symbol of Element)
A. Pnictogen (group 15)	I. Ts
B. Chalcogen	II. Og
C. Halogen	III. Lv
D. Noble gas	IV. Mc

Choose the correct answer from the options given below:

Given below are two statements :

Statement (I) : The first ionisation enthalpy of group 14 elements is higher than the corresponding elements of group 13.

Statement (II) : Melting points and boiling points of group 13 elements are in general much higher than those of corresponding elements of group 14.

In the light of the above statements, choose the most appropriate answer from the options given below :

Choose the incorrect trend in the atomic radii ($r$) of the elements.

The atomic number of the element from the following with lowest $1^{st}$ ionisation enthalpy is :

Which of the following electronegativity order is incorrect ?

Match List-I with List-II.

	List-I		List-II
(A)	$\mathrm{Al^{3+}} < \mathrm{Mg^{2+}} < \mathrm{Na^{+}} < \mathrm{F^{-}}$	(I)	Ionisation Enthalpy
(B)	B < C < O < N	(II)	Metallic character
(C)	B < Al < Mg < K	(III)	Electronegativity
(D)	Si < P < S < Cl	(IV)	Ionic radii

Choose the correct answer from the options given below :

Given below are two statements :

Statement (I) : An element in the extreme left of the periodic table forms acidic oxides.

Statement (II) : Acid is formed during the reaction between water and oxide of a reactive element present in the extreme right of the periodic table.

In the light of the above statements, choose the correct answer from the options given below :

The element, which does not occur in the same period as the other elements (modern periodic table):

Given below are two statements about X-ray spectra of elements :

Statement (I) : A plot of $\sqrt{\nu}$ ($\nu =$ frequency of X-rays emitted) vs atomic mass is a straight line.

Statement (II) : $\nu$ ($\nu =$ frequency of X-rays emitted) vs atomic number is a straight line.

In the light of the above statements, choose the correct answer from the options given below :

Which of the following statements are NOT true about the periodic table?

A. The properties of elements are function of atomic weights.

B. The properties of elements are function of atomic numbers.

C. Elements having similar outer electronic configurations are arranged in same period.

D. The position of an element indicates the quantum numbers of the last filled orbital.

E. The number of elements present in a period is equal to the number of atomic orbitals present in the energy level that is being filled.

Choose the correct answer from the options given below:

Given below are two statements :

Statement (I): The first ionization energy of Pb is greater than that of Sn.

Statement (II): The first ionization energy of Ge is greater than that of Si.

In the light of the above statements, choose the correct answer from the options given below :

The five successive ionization energies of an element are respectively 800, 2427, 3658, 25024 and $32824\ \mathrm{kJ/mol}$. Using the above values, predict the group in which it is present :

The incorrect decreasing order of atomic radii is

Given below are two statements :

Statement (I) : According to the Law of Octaves, the elements were arranged in the increasing order of their atomic number.

Statement (II) : Meyer observed a periodically repeated pattern upon plotting physical properties of certain elements against their respective atomic numbers.

In the light of the above statements, choose the correct answer from the options given below :

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

Number of elements from the following that CANNOT form compounds with valencies which match with their respective group valencies is _________. B, C, N, S, O, F, P, Al, Si

Given below are two statements :

Statement I : The correct order of first ionization enthalpy values of Li, Na, F and Cl is Na < Li < Cl < F.

Statement II : The correct order of negative electron gain enthalpy values of Li, Na, F and Cl is Na < Li < F < Cl

In the light of the above statements, choose the correct answer from the options given below :

The correct order of the first ionization enthalpy is

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 :

Given below are two statements :

Statement I : The metallic radius of Na is $1.86 \mathrm{~\mathring{A}}$ and the ionic radius of $\mathrm{Na^+}$ is lesser than $1.86 \mathrm{~\mathring{A}}$.

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 :

The electron affinity value are negative for

A. $\mathrm{Be \rightarrow Be^-}$ B. $\mathrm{N \rightarrow N^-}$ C. $\mathrm{O \rightarrow O^{2-}}$ D. $\mathrm{Na \rightarrow Na^-}$ E. $\mathrm{Al \rightarrow Al^-}$

Choose the most appropriate answer from the options given below :

Match List - I with List - II.

List - I (Alkali Metal)	List - II (Emission Wavelength in nm)
(A) Li	(I) 589.2
(B) Na	(II) 455.5
(C) Rb	(III) 670.8
(D) Cs	(IV) 780.0

Choose the correct answer from the options given below :

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:

Match List I with List II

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

Choose the correct answer from the options given below:

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

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 ionisation enthalpy and higher electronegativity than the metals.

In the light of the above statements, choose the most appropriate answer from the options given below :

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 :

Given below are two statements : one is labelled as Assertion A and the other is labelled as Reason R :

Assertion A : The first ionisation 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 :

Given below are two statements : one is labelled as Assertion (A) and the other is labelled as Reason (R).

Assertion (A) : There is a considerable increase in covalent radius from N to P. However from As to Bi only a small increase in covalent radius is observed.

Reason (R) : Covalent and ionic radii in a particular oxidation state increases down the group.

In the light of the above statements, choose the most appropriate 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 ________.

Given below are two statements:

Statement - I: Along the period, the chemical reactivity of the elements 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:

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:

Consider the following elements.

$$\text{Group} \downarrow \quad \begin{matrix} \mathrm{A'} & \mathrm{B'} \\ \mathrm{C'} & \mathrm{D'} \end{matrix} \quad \rightarrow \text{Period}$$

(A′ and B′ lie in the same period with B′ to the right of A′; C′ and D′ lie in the next period directly below A′ and B′ respectively.)

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′⁺

Choose the correct answer from the options given below :