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Classification of Elements and Periodicity in Properties

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Q 1. The element {tex} Z = 114 {/tex} has been discovered recently. It will belong to which of the following family/group and electronic configuration?

Carbon family, [Rn] 5{tex} f ^ { 14 } .6 d ^ { 10 } 7 s ^ { 2 } 7 p ^ { 2 } {/tex}

B

Oxygen family, [Rn] 5{tex} f ^ { 14 } \ 6 d ^ { 10 } \ 7 s^ { 2 }\ 7 p ^ { 4 } {/tex}

C

Nitrogen family, [Rn] 5{tex} f ^ { 1 4 } 6 d ^ { 10 } 7 s ^ { 2 } 7 p ^ { 6 } {/tex}

D

Halogen family, [Rn] 5{tex} f ^ { \prime 4 } 6 d ^ { 10 } 7 s ^ { 2 } 7 p ^ { 5 } {/tex}

Explanation

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Q 2. In which of the following options the order of arrangement does not agree with the variation of property indicated against it?

{tex} \mathrm { I } < \mathrm { Br } < \mathrm { Cl } < \mathrm { F } {/tex} (increasing electron gain enthalpy)

B

{tex} \mathrm {Li} < \mathrm N a < \mathrm K < \mathrm {Rb} {/tex} (increasing metallic radius)

C

{tex} \mathrm { Al } ^ { 3 + } < \mathrm { Mg } ^ { 2 + } < \mathrm { Na } ^ { + } < \mathrm { F } {/tex} (increasing ionic size)

D

None of these

Explanation

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Q 3. The species {tex} \mathrm{Ar, K }^ { + }{/tex}and {tex}\mathrm{ C a} ^ { 2 + } {/tex} contain the same number of electrons. In which order do their radii increase?

{tex} \mathrm { Ca } ^ { 2 + } < \mathrm { K } ^ { + } < \mathrm { Ar } {/tex}

B

{tex} \mathrm { K } ^ { + } < \mathrm { Ar } < \mathrm { Ca } ^ { 2 + } {/tex}

C

{tex} \mathrm { Ar } < \mathrm { K } ^ { + } < \mathrm { Ca } ^ { 2 + } {/tex}

D

{tex} \mathrm { Ca } ^ { 2 + } < \mathrm { Ar } < \mathrm { K } ^ { + } {/tex}

Explanation

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Q 4. Which of the following orders of ionic radii is correctly represented?

A

{tex} \mathrm { H^- } > \mathrm { H } ^ { + } > \mathrm { H } {/tex}

B

{tex} \mathrm { Na } ^ { + } > \mathrm { F } > \mathrm { O } ^ { 2 - } {/tex}

C

{tex} \mathrm { F } ^ { - } > \mathrm { O } ^ { 2 - } > \mathrm { Na } ^ { + } {/tex}

None of the above

Explanation



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Q 5. Which one of the following arrangements represents the correct order of least negative to most negative electron gain enthalpy for {tex} \mathrm { C } , \mathrm { Ca } , \mathrm { Al } , \mathrm { F } {/tex} and {tex} \mathrm { O } ? {/tex}

A

{tex} \mathrm{Al} < \mathrm {Ca} < \mathrm O < \mathrm C < \mathrm F {/tex}

B

{tex} \mathrm { Al } < \mathrm { O } < \mathrm { C } < \mathrm { Ca } < \mathrm { F } {/tex}

C

{tex} \mathrm C < \mathrm F < \mathrm O < \mathrm {Al} <\mathrm {Ca} {/tex}

{tex} \mathrm { Ca } < \mathrm { Al } < \mathrm { C } < \mathrm { O } < \mathrm { F } {/tex}

Explanation

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Q 6. What is the value of electron gain enthalpy of {tex} \mathrm { Na } ^ { + } {/tex} if {tex} \mathrm{I E} _ { 1 } {/tex} of {tex} \mathrm { Na } = 5.1 \mathrm { eV } ? {/tex}

{tex} - 5.1 \mathrm { eV } {/tex}

B

{tex} - 10.2 \mathrm { eV } {/tex}

C

{tex} + 2.55 \mathrm { eV } {/tex}

D

{tex} + 10.2 \mathrm { eV } {/tex}

Explanation

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Q 7. The correct order of the decreasing ionic radii among the following isoelectronic species is

A

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

B

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

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

D

{tex} \mathrm{K ^ { + }} >\mathrm {C a ^ { 2 + }} > \mathrm {Cl^-} >\mathrm {S ^ { 2 - }} {/tex}

Explanation

In iso-electronic species, if a positive charge is more then they will have a very less ionic radius. Because here protons are more than electrons and protons attract electrons to come close to the nucleus. But in anionic iso-electronic species, electrons are more than protons. Protons which are in less number can't attract all the electrons to come closer. So, ionic radius increases in the case of anionic species, if negative charge increases.

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Q 8. Which of the following represents the correct order of increasing electron gain enthalpy with negative sign for the elements {tex} \mathrm { O } , \mathrm { S } , \mathrm { F } {/tex} and {tex} \mathrm { Cl } {/tex} ?

A

{tex} \mathrm { Cl } < \mathrm { F } < \mathrm { O } < \mathrm { S } {/tex}

{tex} \mathrm { O } < \mathrm { S } < \mathrm { F } < \mathrm { Cl } {/tex}

C

{tex} \mathrm { F } < \mathrm { S } < \mathrm { O } < \mathrm { Cl } {/tex}

D

{tex} \mathrm { S } < \mathrm { O } < \mathrm { Cl } < \mathrm { F } {/tex}

Explanation

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Q 9. Among the elements {tex} \mathrm { Ca } , \mathrm { Mg } , \mathrm { P } {/tex} and {tex} \mathrm { Cl } , {/tex} the order of increasing atomic radii is

A

{tex} \mathrm { Mg } < \mathrm { Ca } < \mathrm { Cl } < \mathrm { P } {/tex}

{tex} \mathrm { Cl } < \mathrm { P } < \mathrm { Mg } < \mathrm { Ca } {/tex}

C

{tex} \mathrm { P } < \mathrm { Cl } < \mathrm { Ca } < \mathrm { Mg } {/tex}

D

{tex} \mathrm { Ca } < \mathrm { Mg } < \mathrm { P } < \mathrm { Cl } {/tex}

Explanation

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Q 10. Among the following which one has the highest cation to anion size ratio?

A

{tex} \mathrm { CsI } {/tex}

{tex} \mathrm { CsF } {/tex}

C

{tex} \mathrm {LiF}{/tex}

D

{tex} \mathrm { NaF } {/tex}

Explanation

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Q 11. Which one of the following arrangements does not give the correct picture of the trends indicated against it?

{tex} \mathrm { F } _ { 2 } > \mathrm { Cl } _ { 2 } > \mathrm { Br } _ { 2 } > \mathrm { I } _ { 2 } : {/tex} Bond dissociation energy

B

{tex} \mathrm { F } _ { 2 } > \mathrm { Cl } _ { 2 } > \mathrm { Br } _ { 2 } > \mathrm { I } _ { 2 } : {/tex} Electronegativity

C

{tex} \mathrm { F } _ { 2 } > \mathrm { Cl } _ { 2 } > \mathrm { Br } _ { 2 } > \mathrm { I } _ { 2 } : {/tex} Oxidizing power

D

{tex} \mathrm { Cl } _ { 2 } > \mathrm { F } _ { 2 } > \mathrm { Br } _ { 2 } > \mathrm { I } _ { 2 } : {/tex} Electron gain enthalpy

Explanation



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Q 12. Identify the correct order of the size of the following:

{tex} \mathrm { Ca } ^ { 2 + } < \mathrm { K } ^ { + } < \mathrm { Ar } < \mathrm { Cl } ^ { - } < \mathrm { S } ^ { 2 - } {/tex}

B

{tex} \mathrm { Ar } < \mathrm { Ca } ^ { 2 + } < \mathrm { K } ^ { + } < \mathrm { Cl } ^ { - } < \mathrm { S } ^ { 2 - } {/tex}

C

{tex} \mathrm { Ca } ^ { 2 + } < \mathrm { Ar } < \mathrm { K } ^ { + } < \mathrm { Cl } ^ { - } < \mathrm { S } ^ { 2- } {/tex}

D

{tex} \mathrm { Ca } ^ { 2 + } < \mathrm { K } ^ { + } < \mathrm { Ar } < \mathrm { S } ^ { 2 - } < \mathrm { Cl } ^ { - } {/tex}

Explanation

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Q 13. With which of the following electronic configuration an atom has the lowest ionisation enthalpy?

A

1{tex} s ^ { 2 } 2 s ^ { 2 } 2 p ^ { 3 } {/tex}

1{tex} s ^ { 2 } 2 s ^ { 2 } 2 p ^ { 5 } 3 s ^ { 1 } {/tex}

C

1{tex} s ^ { 2 } 2 s ^ { 2 } 2 p ^ { 6 } {/tex}

D

1{tex} s ^ { 2 } 2 s ^ { 2 } 2 p ^ { 5 } {/tex}

Explanation

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Q 14. Which one of the following ionic species has the greatest proton affinity to form stable compound?

{tex} \mathrm { NH } _ { 2 }^- {/tex}

B

{tex}\mathrm F^- {/tex}

C

{tex}\mathrm {I^-}{/tex}

D

{tex} \mathrm { HS^- } {/tex}

Explanation

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Q 15. Which one of the following orders is not in accordance with the property stated against it?

{tex} \mathrm { F } _ { 2 } > \mathrm { Cl } _ { 2 } > \mathrm { Br } _ { 2 } > \mathrm { I } _ { 2 } : {/tex} Bond dissociation energy

B

{tex} \mathrm { F } _ { 2 } > \mathrm { Cl } _ { 2 }^{} > { \mathrm { Br } } _ { 2 } > \mathrm { I } _ { 2 } : {/tex} Oxidising power

C

{tex} \mathrm { HI } > \mathrm { HBr } > \mathrm { HCl } > \mathrm { HF } {/tex} : Acidic property in water

D

{tex} \mathrm { F } _ { 2 } > \mathrm { Cl } _ { 2 } > \mathrm { Br } _ { 2 } > \mathrm { I } _ { 2 } : {/tex} Electronegativity

Explanation

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Q 16. Which one of the following arrangements represents the correct order of electron gain enthalpy (with negative sign) of the given atomic species?

A

{tex} \mathrm { S } < \mathrm { O } < \mathrm { Cl } < \mathrm { F } {/tex}

B

{tex} \mathrm { Cl } < \mathrm { F } < \mathrm { S } < \mathrm { O } {/tex}

C

{tex} \mathrm { F } < \mathrm { Cl } < \mathrm { O } < \mathrm { S } {/tex}

{tex} \mathrm { O } < \mathrm { S } < \mathrm { F } < \mathrm { Cl } {/tex}

Explanation

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Q 17. Ionic radii are

inversely proportional to effective nuclear charge

B

inversely proportional to square of effective nuclear charge

C

directly proportional to effective nuclear charge

D

directly proportional to square of effective nuclear charge.

Explanation

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Q 18. The ions {tex} \mathrm { O } ^ { 2 - } , \mathrm { F } ^ { - } , \mathrm { Na } ^ { + } , \mathrm { Mg } ^ { 2 + } {/tex} and {tex} \mathrm { Al } ^ { 3 + } {/tex} are isoelectronic. Their ionic radii show

A

a significant increase from {tex} \mathrm { O } ^ { 2 - } {/tex} to {tex} \mathrm { A } \mathrm { l } ^ { 3 + } {/tex}

a significant decrease from {tex} \mathrm { O } ^ { 2 - } {/tex} to {tex} \mathrm { Al } ^ { 3 + } {/tex}

C

an increase from {tex} \mathrm { O } ^ { 2 - } {/tex} to {tex} \mathrm { F } ^ { - } {/tex} and then decrease from {tex} \mathrm { Na } ^ { + } {/tex} to {tex} \mathrm { Al } ^ { 3 + } {/tex}

D

a decrease from {tex} \mathrm { O } ^ { 2 - } {/tex} to {tex} \mathrm { F^- } {/tex} and then increase from {tex} \mathrm { Na } ^ { + } {/tex} to {tex} \mathrm { Al } ^ { 3 + } {/tex} .

Explanation

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Q 19. Which statement is wrong?

Bond energy of {tex} \mathrm { F } _ { 2 } > \mathrm { Cl } _ { 2 } {/tex}

B

Electronegativity of {tex} \mathrm { F } > \mathrm { Cl } {/tex}

C

{tex} \mathrm { F } {/tex} is more oxidising than {tex} \mathrm { Cl } {/tex}

D

Electron affinity of {tex} \mathrm { Cl } > \mathrm { F } {/tex}

Explanation

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Q 20. Which of the following elements has the maximum electron affinity?

A

{tex} \mathrm I {/tex}

B

{tex} \mathrm {Br} {/tex}

{tex}\mathrm {Cl} {/tex}

D

{tex} \mathrm {F} {/tex}

Explanation

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Q 21. The first ionization potentials {tex} ( \mathrm { eV } ) {/tex} of {tex} \mathrm { Be } {/tex} and {tex} \mathrm { B } {/tex} respectively are

A

{tex} 8.29,8.29 {/tex}

B

{tex} 9.32,9.32 {/tex}

C

{tex} 8.29,9.32 {/tex}

{tex} 9.32,8.29 {/tex}

Explanation


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Q 22. Which one of the following is correct order of the size of iodine species?

A

{tex} I ^ { + } > I ^ { - } > I {/tex}

{tex} I ^ { - } > I > I ^ { + } {/tex}

C

{tex} I > I^- > I^+ {/tex}

D

{tex} I > I ^ { + } > I^- {/tex}

Explanation

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Q 23. Which of the following ion is the largest in size?

A

{tex} \mathrm {K^+} {/tex}

B

{tex} \mathrm { Ca } ^ { 2 + } {/tex}

C

{tex} \mathrm { Cl^- } {/tex}

{tex} \mathrm { S } ^ { 2- } {/tex}

Explanation

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Q 24. Which of the following has the smallest size?

{tex} \mathrm { Al } ^ { 3+ } {/tex}

B

{tex}\mathrm F^-{/tex}

C

{tex} \mathrm { Na^+ } {/tex}

D

{tex} \mathrm { Mg } ^ { 2+ } {/tex}

Explanation