Ionization potential of ${\rm{Na}}$ would be numerically the same as:

Electron affinity of ${\rm{N}}{{\rm{a}}^ + }$

Electronegativity of ${\rm{N}}{{\rm{a}}^ + }$

Electron affinity of ${\rm{He}}$

Ionization potential of ${\rm{Mg}}$

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JEE • CHEMISTRY • CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

Classification of elements and periodicity in properties practice · Medium

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Showing 1-30 of 227 questions

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1 Medium

1 of 227

Remembering +4 | -1

Among the following elements, the most electronegative is:

View answer and explanation

Correct option: D

Fluorine

Option D (Fluorine) is correct because electronegativity increases across a period and decreases down a group, making Fluorine the most electronegative element among the given options.

2 Medium

2 of 227

Understanding +4 | -1

The correct order of size among

\mathrm{O}, \mathrm{O}^{2-}, \mathrm{F}

and

\mathrm{F}^{-}

is:

View answer and explanation

Correct option: D

\mathrm{O}^{2-}>\mathrm{F}^{-}>\mathrm{O}>\mathrm{F}

Option D (

\mathrm{O}^{2-}>\mathrm{F}^{-}>\mathrm{O}>\mathrm{F}

) is correct because anions are larger than their neutral atoms, and for isoelectronic species, size decreases with increasing nuclear charge.

3 Medium

3 of 227

Analyzing +4 | -1

The electronic configuration of four elements are given below. Which elements does not belong to the same family as others?

View answer and explanation

Correct option: C

[\mathrm{Ne}] 3 s^2 3 p^5

Option C ([Ne] 3s² 3p⁵) is correct because it is the only element with 7 valence electrons, belonging to Group 17, while the others have 2 valence electrons.

4 Medium

4 of 227

Remembering +4 | -1

Which of the following set of oxides are amphoteric

View answer and explanation

Correct option: D

A{l_2}{O_3},ZnO,Sn{O_2},S{b_4}{O_6}

Option D (

A{l_2}{O_3},ZnO,Sn{O_2},S{b_4}{O_6}

) is correct because these oxides exhibit both acidic and basic properties.

5 Medium

5 of 227

Understanding +4 | -1

Arrange the elements

\mathrm{Se}, \mathrm{Cl}

and

\mathrm{S}

in the increasing order of ionisation energy

View answer and explanation

Correct option: B

\mathrm{Se} < \mathrm{S} < \mathrm{Cl}

Option B (

\mathrm{Se} < \mathrm{S} < \mathrm{Cl}

) is correct because ionization energy generally increases across a period and decreases down a group.

6 Medium

6 of 227

Analyzing +4 | -1

The decreasing order of the ionization potential of the following elements is

View answer and explanation

Correct option: B

\mathrm{Ne}>\mathrm{Cl}>\mathrm{P}>\mathrm{S}>\mathrm{Mg}>\mathrm{Al}

Option A (Ne > Cl > P > S > Al > Mg) is correct because it accurately reflects the general trend of ionization potential, considering exceptions due to electronic configurations.

7 Medium

7 of 227

Understanding +4 | -1

Select the ion of largest size in gas phase among the given species

View answer and explanation

Correct option: D

{N}^{3-}

Option D (

{N}^{3-}

) is correct because for isoelectronic species, the size increases with increasing negative charge.

8 Medium

8 of 227

Remembering +4 | -1

The pair of amphoteric oxides among the following is

View answer and explanation

Correct option: C

{ZnO}, {Al}_2 {O}_3

Option C (

{ZnO}, {Al}_2 {O}_3

) is correct because both zinc oxide and aluminum oxide can act as both acids and bases.

9 Medium

9 of 227

Understanding +4 | -1

The correct order of electron affinities is:

View answer and explanation

Correct option: A

Cl > Si > Na > Ar

Option A is correct because electron affinity generally increases across a period and decreases down a group, with noble gases having very low electron affinities.

10 Medium

10 of 227

Analyzing +4 | -1

The five successive ionisation enthalpies of an element are

\mathrm{800, 2427, 3658, 25024 \,\,and\,\, 32824\,\, kJ \,mo}{\mathrm{l}^{ - 1}}.

The number of valence electrons in the element is

View answer and explanation

Correct option: A

Option A (3) is correct because there is a significant jump in ionization enthalpy after the third ionization, indicating that the element has 3 valence electrons.

11 Medium

11 of 227

Analyzing +4 | -1

Assertion :The

1^{\text {st}}

IP of

\mathrm{Be}

is greater than that of

\mathrm{B}

.

Reason : 2p orbital is lower in energy than 2s.

View answer and explanation

Correct option: C

If Assertion is True but the Reason is False

Option C is correct. The first ionization potential (IP) of Be is greater than that of B because Be has a stable, fully filled 2s orbital, while B has a partially filled 2p orbital. The reason is false because 2s orbital is lower in energy than 2p.

12 Medium

12 of 227

Analyzing +4 | -1

In which of the following have higher difference in the value of IInd and IIIrd I.P.

View answer and explanation

Correct option: C

1{s}^2 2 {s}^2 2 {p}^6 3 {s}^1

Option C (

1{s}^2 2 {s}^2 2 {p}^6 3 {s}^1

) is correct because removing the second electron from

Na^+

requires breaking the stable noble gas configuration, leading to a large jump in ionization potential.

13 Medium

13 of 227

Analyzing +4 | -1

Which of the following statements is/are wrong?

View answer and explanation

Correct option: B

All isoelectronic ions belong to same period of the periodic table.

The correct answer is B (All isoelectronic ions belong to same period of the periodic table.) because isoelectronic ions can belong to different periods depending on their charge and electronic configuration.

14 Medium

14 of 227

Understanding +4 | -1

The element with atomic number 35 belongs to :

View answer and explanation

Correct option: C

p-block

Option C (p-block) is correct because the element with atomic number 35 (Bromine) has its last electron entering the p-orbital.

15 Medium

15 of 227

Understanding +4 | -1

Correct order of

{Z}_{\text {eff }}

for species

\mathrm{Na}^{+}, {Mg}^{2+}, {Al}^{3+}

View answer and explanation

Correct option: B

{Na}^{+} < {Mg}^{2+} < {Al}^{3+}

Option B (

{Na}^{+} < {Mg}^{2+} < {Al}^{3+}

) is correct because for isoelectronic species, the effective nuclear charge increases with increasing nuclear charge, leading to a smaller ionic radius and greater effective nuclear charge.

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16 Medium

16 of 227

Understanding +4 | -1

For general ionic compounds, choose the correct characteristics

View answer and explanation

Correct option: A

Cations derived from metallic elements and anions from non‐metallic elements

Option A (Cations derived from metallic elements and anions from non‐metallic elements) is correct because ionic compounds typically consist of cations formed from metals (which lose electrons) and anions formed from non-metals (which gain electrons).

17 Medium

17 of 227

Understanding +4 | -1

Ionization potential of

\mathrm{Na}

would be numerically the same as:

View answer and explanation

Correct option: A

Electron affinity of

\mathrm{N}{\mathrm{a}^ + }

Option A is correct because the electron affinity of Na+ is the energy released when an electron is added, which is numerically equal to the ionization energy of Na.

18 Medium

18 of 227

Understanding +4 | -1

Which of the following elements has maximum tendency to release electrons

View answer and explanation

Correct option: B

Option B (Be) is correct because among the given elements, Be is a metal and has the lowest ionization energy, thus the highest tendency to release electrons.

19 Medium

19 of 227

Understanding +4 | -1

In periodic table, the metallic character …… with increase in atomic no.

View answer and explanation

Correct option: A

Decrease in period and increases in a group

Option A (Decrease in period and increases in a group) is correct because metallic character decreases across a period and increases down a group due to changes in ionization energy and effective nuclear charge.

20 Medium

20 of 227

Remembering +4 | -1

Which of the following period contain most of the manmade radioactive elements?

View answer and explanation

Correct option: A

Seventh

Option A (Seventh) is correct because the seventh period contains most of the man-made radioactive elements, including transuranic elements.

21 Medium

21 of 227

Understanding +4 | -1

Assertion : Ionic bonds are formed between metal and non-metals.

Reason : In ionic bonds electrons are shared oxygen.

View answer and explanation

Correct option: C

If Assertion is True but the Reason is False

Option C (If Assertion is True but the Reason is False) is correct because ionic bonds are formed between metals and non-metals, but electrons are transferred, not shared.

22 Medium

22 of 227

Understanding +4 | -1

Outermost configuration of most electronegative element of the periodic table is

View answer and explanation

Correct option: B

2{s^2}2{p^5}

Option B is correct because Fluorine is the most electronegative element, and its outermost electronic configuration is

2s^22p^5

23 Medium

23 of 227

Analyzing +4 | -1

Assertion : Second IP of oxygen is greater than that of fluorine

Reason : Oxygen aquires stable half filled electronic configuration after loosing one electron

View answer and explanation

Correct option: A

If both Assertion & Reason are True & the Reason is correct explanation of the Assertion

Option A is correct because both the assertion and reason are true, and the reason correctly explains why the second ionization potential of oxygen is greater than that of fluorine.

24 Medium

24 of 227

Understanding +4 | -1

Which of the following statements is wrong?

View answer and explanation

Correct option: D

Non-metals are more than metals.

Option D is correct because metals are more abundant than non-metals in the periodic table.

25 Medium

25 of 227

Analyzing +4 | -1

Which of the following relation is correct?

View answer and explanation

Correct option: A

{\mathrm{I}^{\mathrm{st}}}\mathrm{\;IE\;of\;C} > {\mathrm{I}^{\mathrm{st}}}\mathrm{\;IE\;of\;B}

The correct answer is A (

{\mathrm{I}^{\mathrm{st}}}\mathrm{\;IE\;of\;C} > {\mathrm{I}^{\mathrm{st}}}\mathrm{\;IE\;of\;B}

) because carbon has a more stable electronic configuration than boron, leading to a higher ionization energy.

26 Medium

26 of 227

Analyzing +4 | -1

Assertion(A) Electron gain enthalpy of oxygen is less than that of fluorine but greater than that of nitrogen.

Reason(R) Ionisation enthalpy is as follows:

{N}>{O}>{F}

View answer and explanation

Correct option: C

If (A) is correct and (R) is incorrect.

The correct answer is C (If (A) is correct and (R) is incorrect) because electron gain enthalpy of oxygen is less negative than fluorine but more negative than nitrogen, and the ionization enthalpy order is incorrect.

27 Medium

27 of 227

Understanding +4 | -1

The element with the electronic configuration as

\left[ {\mathrm{Ar}} \right]3{d^{10}}4{s^2}4{p^3}

represents a

View answer and explanation

Correct option: C

Metalloid

Option C is correct because the element with the given electronic configuration ([Ar]3d¹⁰ 4s² 4p³) is Arsenic (As), which is a metalloid.

28 Medium

28 of 227

Remembering +4 | -1

Which of the following relationship proposed graphically by Lothar Meyer?

View answer and explanation

Correct option: B

Physical properties vs atomic weight

The correct answer is B (Physical properties vs atomic weight) because Lothar Meyer plotted physical properties against atomic weight to observe periodic patterns.

29 Medium

29 of 227

Remembering +4 | -1

Alkaline earth metals form ions of the formula:

View answer and explanation

Correct option: A

{M^{2 + }}

Option A (

{M^{2 + }}

) is correct because alkaline earth metals have two valence electrons which they lose to form +2 ions.

30 Medium

30 of 227

Understanding +4 | -1

Among the elements Ca, Mg, P and Cl, the order of increasing atomic radii is

View answer and explanation

Correct option: D

Cl < P < Mg < Ca

Option D (Cl < P < Mg < Ca) is correct because atomic radius increases down a group and decreases across a period.

Revision notes and key takeaways

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Key Takeaways

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