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Q 1. Which of the following metals give inflammable gas with both acid and base?
{tex} \mathrm { Na } {/tex} and {tex} \mathrm { Zn } {/tex}
{tex} \mathrm { Mg } {/tex} and {tex} \mathrm { Al } {/tex}
{tex} \mathrm { Mg } {/tex} and {tex} \mathrm { Be } {/tex}
{tex} \mathrm { Zn } {/tex} and {tex} \mathrm { Al } {/tex}
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Q 2. Which of the following have an incorrect order of ionization energy:
{tex} \mathrm { Pb } ( \mathrm { IE } ) > \mathrm { Sn } ( \mathrm { IE } ) {/tex}
{tex} \mathrm { Na } ^ { + } ( \mathrm { IE } ) > \mathrm { Mg } ^ { + } ( \mathrm { IE } ) {/tex}
{tex} \mathrm { Li } ^ { + } ( \mathrm { IE } ) < \mathrm { O } ^ { + } ( \mathrm { IE } ) {/tex}
{tex} \mathrm { Be } ^ { + } ( \mathrm { IE } ) < \mathrm { C } ^ { + } ( \mathrm { IE } ) {/tex}
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Q 3. Which set of ions have same magnetic moment?
{tex} \mathrm { Co } ^ { + 2 } , \mathrm { Cr } ^ { + 3 } , \mathrm { V } ^ { + 3 } {/tex}
{tex} \mathrm { Mn } ^ { + 2 } , \mathrm { Fe } ^ { + 3 } , \mathrm { Cr } ^ { + } {/tex}
{tex} \mathrm { Ni } ^ { + 2 } , \mathrm { Mn } ^ { + 2 } , \mathrm { Co } ^ { + 2 } {/tex}
{tex} \mathrm { Fe } ^ { + 2 } , \mathrm { Mn } ^ { + 2 } , \mathrm { Co } ^ { + 2 } {/tex}
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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}
{tex} \mathrm { P } _ { 2 } \mathrm { O } _ { 3 } > \mathrm { SO } _ { 2 } > \mathrm { SiO } _ { 2 } > \mathrm { Al } _ { 2 } \mathrm { O } _ { 3 } {/tex}
{tex} \mathrm { P } _ { 2 } \mathrm { O } _ { 3 } > \mathrm { Al } _ { 2 } \mathrm { O } _ { 3 } > \mathrm { SO } _ { 2 } > \mathrm { SiO } _ { 2 } {/tex}
{tex} \mathrm { Al } _ { 2 } \mathrm { O } _ { 3 } > \mathrm { SiO } _ { 2 } > \mathrm { P } _ { 2 } \mathrm { O } _ { 3 } > \mathrm { SO } _ { 2 } {/tex}
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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:
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}
1{tex} \mathrm { s } ^ { 2 } 2 \mathrm { s } ^ { 2 } 2 \mathrm { p } ^ { 6 } 3 \mathrm { s } ^ { 2 } 3 \mathrm { p } ^ { 3 } {/tex}
1{tex} \mathrm { s } ^ { 2 } 2 \mathrm { s } ^ { 2 } 2 \mathrm { p } ^ { 6 } 3 \mathrm { s } ^ { 2 } {/tex}
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Q 6. The correct order increasing radii is:
{tex} \mathrm { Be } ^ { 2 + } , \mathrm { Mg } ^ { 2 + } , \mathrm { Na } ^ { + } {/tex}
{tex} \mathrm { K } ^ { + } , \mathrm { Ca } ^ { 2 + } , \mathrm { S } ^ { 2 - } {/tex}
{tex} \mathrm { O } ^ { 2 } , \mathrm { F } , \mathrm { N } ^ { 3 } {/tex}
{tex} S ^ { 2 - } , O ^ { 2 - } , A s ^ { 3 } {/tex}
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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)
37.3{tex} \mathrm { g } {/tex}
1.96Å
2.12{tex} \mathrm { Å} {/tex}
1.0{tex}Å{/tex}
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Q 8. The electronegativity of the following elements increases in the order:
{tex} \mathrm { S } < \mathrm { P } < \mathrm { N } < \mathrm { O } {/tex}
{tex} \mathrm { P } < \mathrm { S } < \mathrm { N } < \mathrm { O } {/tex}
{tex} \mathrm { N } < \mathrm { O } < \mathrm { P } < \mathrm { S } {/tex}
{tex} \mathrm { N } < \mathrm { P } < \mathrm { S } < \mathrm { O } {/tex}
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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:
Oxygen is more electronegative.
Addition of electron in oxygen results in larger size of the ion.
Electron repulsion outweighs the stability gained by achieving noble gas configuration.
{tex} \mathrm {O^{2-}} {/tex} ion has comparatively smaller size than oxygen atom.
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Q 10. In which of the following compounds chromium shows maximum radius:-
{tex} \mathrm { K } _ { 2 } \mathrm { Cr } _ { 2 } \mathrm { O } _ { 7 } {/tex}
{tex} \mathrm { CrO } _ { 2 } \mathrm { Cl } _ { 2 } {/tex}
{tex} \mathrm { Cr } _ { 2 } \left( \mathrm { SO } _ { 4 } \right) _ { 3 } {/tex}
{tex} \mathrm { CrCl } _ { 2 } {/tex}
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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-
Co-ordinate
Covalent
Ionic
Metallic
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Q 12. In which of the following arrangements, the order is NOT according to the property indicated against it?
{tex} Li < N a < K < R b {/tex} : Increasing metallic radius
{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
{tex} \mathrm { Al } ^ { 3 + } < \mathrm { Mg } ^ { 2 + } < \mathrm { Na } ^ { + } < \mathrm { F } ^ { - } {/tex} Increasing ionic size
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Q 13. Which of the following oxides is amphoteric in character?
{tex} \mathrm { SnO } _ { 2 } {/tex}
{tex} \mathrm { SiO } _ { 2 } {/tex}
{tex} \mathrm { CO } _ { 2 } {/tex}
{tex} \mathrm { CaO } {/tex}
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Q 14. According to the periodic law of elements, the variation in properties of elements is related to their
atomic masses
nuclear masses
atomic numbers
nuclear neutron-proton number ratios.
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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}
{tex} \mathrm { Ba } ^ { 2 + } , \mathrm { Sr } ^ { 2 + } , \mathrm { K } ^ { + } , \mathrm { S } ^ { 2 - } {/tex}
{tex} \mathrm { N } ^ { 3 - } , \mathrm { O } ^ { 2 - } , \mathrm { F } ^ { - } , \mathrm { S } ^ { 2 - } {/tex}
{tex} \mathrm { Li } ^ { + } , \mathrm { Na } ^ { + } , \mathrm { Mg } ^ { 2 + } , \mathrm { Ca } ^ { 2 + } {/tex}
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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}
{tex} \mathrm { Na } ^ { + } , \mathrm { Ca } ^ { 2 + } , \mathrm { Sc } ^ { 3 + } , \mathrm { F } ^ { - } {/tex}
{tex} \mathrm { K } ^ { + } , \mathrm { Cl } ^ { - } , \mathrm { Mg } ^ { 2 + } , \mathrm { Sc } ^ { 3 + } {/tex}
{tex} \mathrm { Na } ^ { + } , \mathrm { Mg } ^ { 2 + } , \mathrm { Al } ^ { 3 + } , \mathrm { Cl } ^ { - } {/tex}
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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
oxygen has high electron affinity
{tex}O^-{/tex}ion will tend to resist the addition of another electron
{tex}O^-{/tex} ion has comparatively larger size than oxygen atom.
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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}
{tex} \mathrm { Sn } > \mathrm { Ce } > \mathrm { Lu } > \mathrm { Yb } {/tex}
{tex} \mathrm { Lu } > \mathrm { Yb } > \mathrm { Sn } > \mathrm { Ce } {/tex}
{tex} \mathrm { Sn } > \mathrm { Yb } > \mathrm { Ce } > \mathrm { Lu } {/tex}
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Q 19. According to Mendeleev's periodic law, physical and chemical properties are function of
Atomic number
Atomic weight
Atomic volume
Number of neutrons
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Q 20. Which of the following orbitals has higher screening power?
{tex} 4 s {/tex}
{tex} 4 p {/tex}
{tex} 4 d {/tex}
{tex} 4 f {/tex}
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Q 21. Which one of the following order is correct?
{tex} \mathrm {I>I^+>I^- } {/tex} (radii)
{tex} \mathrm {I^- >I>I^+ } {/tex} (radii)
{tex} \mathrm {I^- >I>I^+ } {/tex} (Ionisation energy)
{tex} \mathrm {I^{+5} >I^{+}>I^{+7} } {/tex} (Ionisation energy)
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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?
{tex} \mathrm {s} {/tex}
{tex} \mathrm {p} {/tex}
{tex}\mathrm{d} {/tex}
{tex}\mathrm{f} {/tex}
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Q 23. The chemistry of Be is very similar to that of aluminium, because
They belong to same group
They belong to same period
Both have nearly the same ionic size
The ratio of their charge to size is nearly the same
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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
-5.1 eV
-10.2 eV
#ERROR!
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Q 25. The ionic radii ( in A) of N-3,O2- and F- are respectively :[JEE M 2015]
1.71, 1.40 and 1.36
1.71, 1.36 and 1.40
1.36, 1.40 and 1.71
1.36, 1.71 and 1.40