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Mathematics

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