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Classification of Elements and Periodicity in Properties

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Q 1. Which of the following metals give inflammable gas with both acid and base?

A

{tex} \mathrm { Na } {/tex} and {tex} \mathrm { Zn } {/tex}

B

{tex} \mathrm { Mg } {/tex} and {tex} \mathrm { Al } {/tex}

C

{tex} \mathrm { Mg } {/tex} and {tex} \mathrm { Be } {/tex}

{tex} \mathrm { Zn } {/tex} and {tex} \mathrm { Al } {/tex}

Explanation

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Q 2. Which of the following have an incorrect order of ionization energy:

A

{tex} \mathrm { Pb } ( \mathrm { IE } ) > \mathrm { Sn } ( \mathrm { IE } ) {/tex}

B

{tex} \mathrm { Na } ^ { + } ( \mathrm { IE } ) > \mathrm { Mg } ^ { + } ( \mathrm { IE } ) {/tex}

{tex} \mathrm { Li } ^ { + } ( \mathrm { IE } ) < \mathrm { O } ^ { + } ( \mathrm { IE } ) {/tex}

D

{tex} \mathrm { Be } ^ { + } ( \mathrm { IE } ) < \mathrm { C } ^ { + } ( \mathrm { IE } ) {/tex}

Explanation



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Q 3. Which set of ions have same magnetic moment?

A

{tex} \mathrm { Co } ^ { + 2 } , \mathrm { Cr } ^ { + 3 } , \mathrm { V } ^ { + 3 } {/tex}

{tex} \mathrm { Mn } ^ { + 2 } , \mathrm { Fe } ^ { + 3 } , \mathrm { Cr } ^ { + } {/tex}

C

{tex} \mathrm { Ni } ^ { + 2 } , \mathrm { Mn } ^ { + 2 } , \mathrm { Co } ^ { + 2 } {/tex}

D

{tex} \mathrm { Fe } ^ { + 2 } , \mathrm { Mn } ^ { + 2 } , \mathrm { Co } ^ { + 2 } {/tex}

Explanation



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Q 4. The correct order of acidic strength of the following is:

{tex} \mathrm { SO } _ { 2 } > \mathrm { P } _ { 2 } \mathrm { O } _ { 3 } > \mathrm { SiO } _ { 2 } > \mathrm { Al } _ { 2 } \mathrm { O } _ { 3 } {/tex}

B

{tex} \mathrm { P } _ { 2 } \mathrm { O } _ { 3 } > \mathrm { SO } _ { 2 } > \mathrm { SiO } _ { 2 } > \mathrm { Al } _ { 2 } \mathrm { O } _ { 3 } {/tex}

C

{tex} \mathrm { P } _ { 2 } \mathrm { O } _ { 3 } > \mathrm { Al } _ { 2 } \mathrm { O } _ { 3 } > \mathrm { SO } _ { 2 } > \mathrm { SiO } _ { 2 } {/tex}

D

{tex} \mathrm { Al } _ { 2 } \mathrm { O } _ { 3 } > \mathrm { SiO } _ { 2 } > \mathrm { P } _ { 2 } \mathrm { O } _ { 3 } > \mathrm { SO } _ { 2 } {/tex}

Explanation



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Q 5. The value of {tex} \mathrm { IE } _ { 1 } , \mathrm { IE } _ { 2 } , \mathrm { IE } _ { 3 } , {/tex} and {tex} \mathrm { IE } _ { 4 } {/tex} of an atom are {tex} 7.5 \mathrm { eV } , 25.6 \mathrm { eV } , 48.6 \mathrm { eV } {/tex} and 170.6{tex} \mathrm { eV } {/tex} respectively.
The electronic configuration of the atom will be:

A

1{tex} \mathrm { s } ^ { 2 } 2 \mathrm { s } ^ { 2 } 2 \mathrm { p } ^ { 6 } 3 \mathrm { s } ^ { 1 } {/tex}

1{tex} \mathrm { s } ^ { 2 } 2 \mathrm { s } ^ { 2 } 2 \mathrm { p } ^ { 6 } 3 \mathrm { s } ^ { 2 } 3 \mathrm { p } ^ { 1 } {/tex}

C

1{tex} \mathrm { s } ^ { 2 } 2 \mathrm { s } ^ { 2 } 2 \mathrm { p } ^ { 6 } 3 \mathrm { s } ^ { 2 } 3 \mathrm { p } ^ { 3 } {/tex}

D

1{tex} \mathrm { s } ^ { 2 } 2 \mathrm { s } ^ { 2 } 2 \mathrm { p } ^ { 6 } 3 \mathrm { s } ^ { 2 } {/tex}

Explanation



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Q 6. The correct order increasing radii is:

{tex} \mathrm { Be } ^ { 2 + } , \mathrm { Mg } ^ { 2 + } , \mathrm { Na } ^ { + } {/tex}

B

{tex} \mathrm { K } ^ { + } , \mathrm { Ca } ^ { 2 + } , \mathrm { S } ^ { 2 - } {/tex}

C

{tex} \mathrm { O } ^ { 2 } , \mathrm { F } , \mathrm { N } ^ { 3 } {/tex}

D

{tex} S ^ { 2 - } , O ^ { 2 - } , A s ^ { 3 } {/tex}

Explanation

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Q 7. What will be the distance between {tex} \mathrm { H } {/tex} and {tex} \mathrm { Cl } {/tex} atom in HCl. The radius of hydrogen is 0.37{tex} \mathrm { Å} {/tex} and the radius of chlorine is 1.67{tex} \mathrm { Å } ? {/tex}
(According to the concept of covalent radius)

A

37.3{tex} \mathrm { g } {/tex}

1.96Å

C

2.12{tex} \mathrm { Å} {/tex}

D

1.0{tex}Å{/tex}

Explanation



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Q 8. The electronegativity of the following elements increases in the order:

A

{tex} \mathrm { S } < \mathrm { P } < \mathrm { N } < \mathrm { O } {/tex}

{tex} \mathrm { P } < \mathrm { S } < \mathrm { N } < \mathrm { O } {/tex}

C

{tex} \mathrm { N } < \mathrm { O } < \mathrm { P } < \mathrm { S } {/tex}

D

{tex} \mathrm { N } < \mathrm { P } < \mathrm { S } < \mathrm { O } {/tex}

Explanation



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Q 9. The formation of the oxide ion, {tex} \mathrm { O } ^ { 2 - } ( \mathrm { g } ) , {/tex} from oxygen atom requires first an exothermic and then an endothermic step as shown below:
{tex}\mathrm{O(g)+e^{-}\rightarrow O^{-}(g);\triangle_{eg}H=-141\,kJ mol^{-1}}{/tex}
{tex}\mathrm{O^{-}(g)+e^{-}\rightarrow O^{2-}(g);\triangle_{eg}H=+780\,kJ mol^{-1}}{/tex}
Thus process of formation of {tex} \mathrm { O } ^ { 2 - } {/tex} in gas phase is unfavorable even {tex} \mathrm { O } ^ { 2 - } {/tex} is isoelectronic with neon. It is due to the fact that:

A

Oxygen is more electronegative.

B

Addition of electron in oxygen results in larger size of the ion.

Electron repulsion outweighs the stability gained by achieving noble gas configuration.

D

{tex} \mathrm {O^{2-}} {/tex} ion has comparatively smaller size than oxygen atom.

Explanation

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Q 10. In which of the following compounds chromium shows maximum radius:-

A

{tex} \mathrm { K } _ { 2 } \mathrm { Cr } _ { 2 } \mathrm { O } _ { 7 } {/tex}

B

{tex} \mathrm { CrO } _ { 2 } \mathrm { Cl } _ { 2 } {/tex}

C

{tex} \mathrm { Cr } _ { 2 } \left( \mathrm { SO } _ { 4 } \right) _ { 3 } {/tex}

{tex} \mathrm { CrCl } _ { 2 } {/tex}

Explanation

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Q 11. The atomic number of three elements {tex} \mathrm { A } , \mathrm { B } {/tex} and {tex} \mathrm { C } {/tex} are {tex} \mathrm { a } , \mathrm { a } + 1 {/tex} and {tex} \mathrm { a } + 2 , \mathrm { C } {/tex} is an alkali metal. In a compound of {tex} \mathrm { A } {/tex} and {tex} \mathrm { C } , {/tex} the nature of bonding is-

A

Co-ordinate

B

Covalent

Ionic

D

Metallic

Explanation

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Q 12. In which of the following arrangements, the order is NOT according to the property indicated against it?

A

{tex} Li < N a < K < R b {/tex} : Increasing metallic radius

B

{tex}I < \mathrm { Br } < \mathrm { F } < \mathrm { Cl } {/tex} : Increasing electron gain enthalpy (with negative sign)

{tex} \mathrm { B } < \mathrm { C } < \mathrm { N } < \mathrm { O } {/tex} Increasing first ionization enthalpy

D

{tex} \mathrm { Al } ^ { 3 + } < \mathrm { Mg } ^ { 2 + } < \mathrm { Na } ^ { + } < \mathrm { F } ^ { - } {/tex} Increasing ionic size

Explanation




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Q 13. Which of the following oxides is amphoteric in character?

{tex} \mathrm { SnO } _ { 2 } {/tex}

B

{tex} \mathrm { SiO } _ { 2 } {/tex}

C

{tex} \mathrm { CO } _ { 2 } {/tex}

D

{tex} \mathrm { CaO } {/tex}

Explanation







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Q 14. According to the periodic law of elements, the variation in properties of elements is related to their

A

atomic masses

B

nuclear masses

atomic numbers

D

nuclear neutron-proton number ratios.

Explanation


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Q 15. Which one of the following sets of ions represents a collection of isoelectronic species?

{tex} \mathrm { K } ^ { + } , \mathrm { Cl } ^ { - } , \mathrm { Ca } ^ { 2 + } , \mathrm { Sc } ^ { 3 + } {/tex}

B

{tex} \mathrm { Ba } ^ { 2 + } , \mathrm { Sr } ^ { 2 + } , \mathrm { K } ^ { + } , \mathrm { S } ^ { 2 - } {/tex}

C

{tex} \mathrm { N } ^ { 3 - } , \mathrm { O } ^ { 2 - } , \mathrm { F } ^ { - } , \mathrm { S } ^ { 2 - } {/tex}

D

{tex} \mathrm { Li } ^ { + } , \mathrm { Na } ^ { + } , \mathrm { Mg } ^ { 2 + } , \mathrm { Ca } ^ { 2 + } {/tex}

Explanation



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Q 16. Which one of the following sets of ions represents the collection of isoelectronic species?
(Atomic nos.: {tex} \mathrm { F } = 9 , \mathrm { Cl } = 17 , \mathrm { Na } = 11 , \mathrm { Mg } = 12 , {/tex} {tex} \mathrm { Al } = 13 , \mathrm { K } = 19 , \mathrm { Ca } = 20 , \mathrm { Sc } = 21 {/tex})

{tex} \mathrm { K } ^ { + } , \mathrm { Ca } ^ { 2 + } , \mathrm { Sc } ^ { 3 + } , \mathrm { Cl } ^ { - } {/tex}

B

{tex} \mathrm { Na } ^ { + } , \mathrm { Ca } ^ { 2 + } , \mathrm { Sc } ^ { 3 + } , \mathrm { F } ^ { - } {/tex}

C

{tex} \mathrm { K } ^ { + } , \mathrm { Cl } ^ { - } , \mathrm { Mg } ^ { 2 + } , \mathrm { Sc } ^ { 3 + } {/tex}

D

{tex} \mathrm { Na } ^ { + } , \mathrm { Mg } ^ { 2 + } , \mathrm { Al } ^ { 3 + } , \mathrm { Cl } ^ { - } {/tex}

Explanation


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Q 17. The formation of the oxide ion {tex} \mathrm { O } ^ { 2 - } {/tex} {tex}_(g){/tex} requires first an exothermic and then an endothermic step as shown below.
{tex} \mathrm { O } _ { ( g ) } + e ^ { - } = \mathrm { O } ^ { - } _ { ( g ) } ; \Delta H ^ { \circ } = - 142 \mathrm { kJmol } ^ { - 1 } {/tex}
{tex} \mathrm { O } ^ { - } _ { ( g ) } + e ^ { - } = \mathrm { O } ^ { 2 - } _ { ( \mathrm { g } ) } ; \Delta H ^ { \circ } = 844 \mathrm { kJmol } ^ { - 1 } {/tex}
This is because

Oxygen is more electronegative

B

oxygen has high electron affinity

C

{tex}O^-{/tex}ion will tend to resist the addition of another electron

D

{tex}O^-{/tex} ion has comparatively larger size than oxygen atom.

Explanation


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Q 18. Which is the correct order of atomic sizes?
(At. Nos.: {tex} \mathrm { Ce } = 58 , \mathrm { Sn } = 50 , \mathrm { Yb } = 70 \text { and } \mathrm { Lu } = 71 ) {/tex}

{tex} \mathrm { Ce } > \mathrm { Sn } > \mathrm { Yb } > \mathrm { Lu } {/tex}

B

{tex} \mathrm { Sn } > \mathrm { Ce } > \mathrm { Lu } > \mathrm { Yb } {/tex}

C

{tex} \mathrm { Lu } > \mathrm { Yb } > \mathrm { Sn } > \mathrm { Ce } {/tex}

D

{tex} \mathrm { Sn } > \mathrm { Yb } > \mathrm { Ce } > \mathrm { Lu } {/tex}

Explanation


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Q 19. According to Mendeleev's periodic law, physical and chemical properties are function of

A

Atomic number

Atomic weight

C

Atomic volume

D

Number of neutrons

Explanation

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Q 20. Which of the following orbitals has higher screening power?

{tex} 4 s {/tex}

B

{tex} 4 p {/tex}

C

{tex} 4 d {/tex}

D

{tex} 4 f {/tex}

Explanation

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Q 21. Which one of the following order is correct?

A

{tex} \mathrm {I>I^+>I^- } {/tex} (radii)

{tex} \mathrm {I^- >I>I^+ } {/tex} (radii)

C

{tex} \mathrm {I^- >I>I^+ } {/tex} (Ionisation energy)

D

{tex} \mathrm {I^{+5} >I^{+}>I^{+7} } {/tex} (Ionisation energy)

Explanation

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Q 22. An element has electronic configuration {tex} [ \mathrm { Xe } ] 4 f ^ { 7 } , 5 \mathrm { d } ^ { 1 } , 6 \mathrm { s } ^ { 2 } . {/tex} It belongs to which block of the periodic table?

A

{tex} \mathrm {s} {/tex}

B

{tex} \mathrm {p} {/tex}

C

{tex}\mathrm{d} {/tex}

{tex}\mathrm{f} {/tex}

Explanation

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Q 23. The chemistry of Be is very similar to that of aluminium, because

A

They belong to same group

B

They belong to same period

C

Both have nearly the same ionic size

The ratio of their charge to size is nearly the same

Explanation

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Q 24. The first ionization potential of Na is 5. 1 eV . The value of electron gain enthalpy of Na+ will be
[JEE M 2013]

-2.55 eV

B

-5.1 eV

C

-10.2 eV

D

#ERROR!

Explanation

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Q 25. The ionic radii ( in A) of N-3,O2- and F- are respectively :[JEE M 2015]

A

1.71, 1.40 and 1.36

B

1.71, 1.36 and 1.40

C

1.36, 1.40 and 1.71

1.36, 1.71 and 1.40