Question Set A

Tamilnadu 12th Standard Chemistry p - Block Elements - II Important Questions Study Material - QB365

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Questions:

Multiple Choice Question

97 x 1 = 97

Choose the correct statement.

(a)

Square planar complexes are more stable than octahedral complexes

(b)

The spin only magnetic moment of [Cu(Cl)₄]^2- is BM and it has square planar structure.

(c)

Crystal field splitting energy \(\left( { \Delta }_{ 0 } \right) \) [FeF₆]^4- is higher than the \((\Delta _{ 0 })\) of [Fe(CN)₆]^4-

(d)

crystal field stabilization energy of [V(H₂O)₆]²⁺ is higher than the crystal field stabilization of [Ti(H₂O)₆]²⁺

Fac-mer isomerism is shown by _______.

(a)

[CO(en)₃]³⁺

(b)

[Co(NH₃)₄(Cl)₂]⁺

(c)

[Co(NH₃)₃(Cl)₃]

(d)

[Co(NH₃)₅Cl]SO₄

Which of the following is paramagnetic in nature?

(a)

[Zn(NH₃)₄]²⁺

(b)

[Co(NH₃)₆]³⁺

(c)

[Ni(H₂O)₆]²⁺

(d)

[Ni(CN)₄]^2-

Formula of tris(ethane-1, 2-diamine)iron(II)phosphate _______.

(a)

[Fe(CH₃-CH(NH₂)₂)₃](PO₄)₃

(b)

[Fe(H₂N-CH₂-CH₂-NH₂)₃](PO₄)

(c)

[Fe(H₂N-CH₂-CH₂-NH₂)₃](PO₄)₂

(d)

[Fe(H₂N-CH₂-CH₂-NH₂)₃]₃(PO₄)₂

A complex in which the oxidation number of the metal is zero is_______.

(a)

K₄[Fe(CN)₆]

(b)

[Fe(CN)₃(NH₃)₃]

(c)

[Fe(CO)₅]

(d)

both (b) and (c)

Which one of the following complexes is not expected to exhibit isomerism?

(a)

[Ni(NH₃)₄(H₂O)₂]²⁺

(b)

[Pt(NH₃)₂Cl₂]

(c)

[Co(NH₃)₅SO₄]Cl

(d)

[FeCl₆]^3-

Which kind of isomerism is possible for a complex [Co(NH₃)₄Br₂]CI?

(a)

geometrical and ionization

(b)

geometrical and optical

(c)

optical and ionization

(d)

geometrical only

Which one of the following pairs represents linkage isomers?

(a)

[Cu(NH₃)₄][PtCl₄] and [Pt(NH₃)₄][CuCl₄]

(b)

[Co(NH₃)₅(NO₃)]SO₄ and [Co(NH₃)₅(ONO)]

(c)

[Co(NH₃)₄(NCS)₂]Cl and [Co(NH₃)₄(SCN)₂]Cl

(d)

both (b) and (c)

How many geometrical isomers are possible for [Pt(Py)(NH₃)(Br)(Cl)]?

(a)

(b)

(c)

(d)

10.

Which type of isomerism is exhibited by [Pt(NH₃)₂Cl₂]?

(a)

Coordination isomerism

(b)

Linkage isomerism

(c)

Optical isomerism

(d)

Geometrical isomerism

11.

Which one of the following will give a pair of enantiomorphs?

(a)

[Cr(NH₃)₆][Co(CN)₆]

(b)

[Co(en)₂Cl₂]Cl

(c)

[Pt(NH₃)₄][PtCl₄]

(d)

[Co(NH₃)₄Cl₂]NO₂

12.

In which of the following coordination entities the magnitude of Δ₀ will be maximum?

(a)

[Co(CN)₆]^3-

(b)

[Co(C₂O₄)₃]^3-

(c)

[Co(H₂O)₆]³⁺

(d)

[Co(NH₃)₆]³⁺

13.

Crystal field stabilization energy for high spin d⁵ octahedral complex is _______.

(a)

-0.6\({ \Delta }_{ 0 }\)

(b)

(c)

2(P-\({ \Delta }_{ 0 }\))

(d)

2(P+\({ \Delta }_{ 0 }\))

14.

A magnetic moment of 1.73BM will be shown by one among the following.

(a)

TiCl₄

(b)

[CoCl₆]^4-

(c)

[Cu(NH₃)₄]²⁺

(d)

[Ni(CN)₄]^2-

15.

IUPAC name of the complex K₃[Al(C₂O₄)₃] is _______.

(a)

potassium trioxalatoaluminium (III)

(b)

possium trioxalatoaluminate (II)

(c)

potassium trisoxalatoaluminate (III)

(d)

potassium trioxalatoaluminate (III)

16.

As per IUPAC guidelines, the name of the complex [Co(en)₂(ONO)Cl]Cl is _______.

(a)

chloro bis ethylenediamine nitrocobalt(III) chloride

(b)

chloridobis(ethane-1, 2-diamine)nitro K-O Cobaltate(III) chloride

(c)

chloridobis(ethane-1, 2-diammine)nitrito K-O Cobalt(II) chloride

(d)

chloridobis(ethane-1, 2-diamine)nitrito K-O Cobalt(III) chloride

17.

Oxidation state of Iron and the charge on the ligand NO in [Fe(H₂O)₅NO]SO₄ are_______.

(a)

+2 and 0 respectively

(b)

+3 and 0 respectively

(c)

+3 and -1 respectively

(d)

+1 and +1 respectively

18.

A complex has a molecular formula MSO₄Cl.6H₂O. The aqueous solution of it gives white precipitate with Barium chloride solution and no precipitate is obtained when it is treated with silver nitrate solution. If the secondary valence of the metal is six, which one of the following correctly represents the complex?

(a)

[M(H₂O)₄Cl]SO₄.2H₂O

(b)

[M(H₂O)₆]SO₄

(c)

[M(H₂O)₅Cl]SO₄.H₂O

(d)

[M(H₂O)₃Cl]SO₄.3H₂O

19.

An excess of silver nitrate is added to 100ml of a 0.01M solution of Pentaaquachlorochromium (III)chloride. The number of moles of AgCl precipitated would be _______.

(a)

0.02

(b)

0.002

(c)

0.01

(d)

0.2

20.

The sum of primary valence and secondary valence of the metal M in the complex [M(en)₂(Ox)]Cl is________.

(a)

(b)

(c)

-3

(d)

21.

Which one of the following is not correct?

(a)

La(OH)₃ is less basic than Lu(OH)₃

(b)

In lanthanoid series ionic radius of Ln³⁺ ions decreases

(c)

La is actually an element of transition metal series rather than lanthanide series

(d)

Atomic radii of Zr and Hf are same because of lanthanide contract

22.

The actinoid elements which show the highest oxidation state of +7 are _______.

(a)

Np, Pu, Am

(b)

U, Fm, Th

(c)

U, Th, Md

(d)

Es, No, Lr

23.

The most common oxidation state of actinoids is _______.

(a)

(b)

(c)

(d)

24.

Which of the following oxidation states is most common among the lanthanoids?

(a)

(b)

(c)

(d)

25.

Which of the following lanthanoid ions is diamagnetic?

(a)

Eu²⁺

(b)

Yb²⁺

(c)

Ce²⁺

(d)

Sm²⁺

26.

Which one of the following statements related to lanthanons is incorrect?

(a)

Europium shows +2 oxidation state

(b)

The basicity decreases as the ionic radius decreases from Pr to Lu.

(c)

All the lanthanons are much more reactive than aluminium

(d)

Ce⁴⁺ solutions are widely used as oxidising agents in volumetric analysis.

27.

The number of moles of acidified KMnO₄required to oxidize 1 mole of ferrous oxalate(FeC₂O₄) is _______.

(a)

(b)

(c)

0.6

(d)

1.5

28.

How many moles of I₂ are liberated when 1 mole of potassium dichromate react with potassium iodide?

(a)

(b)

(c)

(d)

29.

Permanganate ion changes to ________ in acidic medium.

(a)

MnO₄²⁻

(b)

Mn²⁺

(c)

Mn³⁺

(d)

MnO₂

30.

Which of the following statements is not true?

(a)

on passing H₂S, through acidified K₂Cr₂O₇ solution, a milky colour is observed

(b)

Na₂Cr₂O₇ is preferred over K₂Cr₂O₇ in volumetric analysis

(c)

K₂Cr₂O₇ solution in acidic medium is orange in colour

(d)

K₂Cr₂O₇ solution becomes yellow on increasing the P^H beyond 7

31.

In acid medium, potassium permanganate oxidizes oxalic acid to _______.

(a)

oxalate

(b)

Carbon dioxide

(c)

acetate

(d)

acetic acid

32.

The correct order of increasing oxidizing power in the series _______.

(a)

VO₂⁺ < Cr₂O₇^2- < MnO₄^-

(b)

Cr₂O₇^2- < VO₂⁺ < MnO₄^-

(c)

Cr₂O₇^2- < MnO₄^- < VO₂⁺

(d)

MnO₄^- < Cr₂O₇^2- < VO₂⁺

33.

The catalytic behaviour of transition metals and their compounds is ascribed mainly due to _______.

(a)

their magnetic behaviour

(b)

their unfilled d orbitals

(c)

their ability to adopt variable oxidation states

(d)

their chemical reactivity

34.

The magnetic moment of Mn²⁺ ion is _______.

(a)

5.92BM

(b)

2.80BM

(c)

8.95BM

(d)

3.90BM

35.

Which one of the following ions has the same number of unpaired electrons as present in V³⁺?

(a)

Ti³⁺

(b)

Fe³⁺

(c)

Ni²⁺

(d)

Cr³⁺

36.

Among the transition metals of 3d series, the one that has highest negative \(\left( \frac { M^{ 2+ } }{ M } \right) \) standard electrode potential is _______.

(a)

(b)

(c)

(d)

37.

Which of the following d block element has half filled penultimate d sub shell as well as half filled valence sub shell?

(a)

(b)

(c)

(d)

none of these

38.

Sc (Z = 21) is a transition element but Zinc (z = 30) is not because _______.

(a)

both Sc³⁺ and Zn²⁺ ions are colourless and form white compounds

(b)

In case of Sc, 3d orbital are partially filled but in Zn these are completely filled

(c)

last electron as assumed to be added to 4s level in case of zinc

(d)

both Sc and Zn do not exhibit variable oxidation states

39.

The stability of +1 oxidation state increases in the sequence ________.

(a)

Al < Ga < In < Tl

(b)

Tl < In < Ga < Al

(c)

In < Tl < Ga < Al

(d)

Ga< In < Al < Tl

40.

The compound that is used in nuclear reactors as protective shields and control rods is _________.

(a)

Metal borides

(b)

metal oxides

(c)

Metal carbonates

(d)

metal carbide

41.

Duralumin is an alloy of ______.

(a)

Cu, Mn

(b)

Cu, Al, Mg

(c)

Al, Mn

(d)

Al, Cu, Mn, Mg

42.

Column-I		Column-II
A	Borazole	1	B(OH)₃
B	Boric acid	2	B₃N₃H₆
C	Quartz	3	Na₂[B₄O₅(OH)₄]8H₂O
D	Borax	4	SiO₂

(a)

A	B	C	D
2	1	4	3

(b)

A	B	C	D
1	2	4	3

(c)

A	B	C	D
1	2	4	3

(d)

None of these

43.

Which of the following statements is not correct?

(a)

Beryl is a cyclic silicate

(b)

Mg₂SiO₄ is an orthosilicate

(c)

SiO₄⁴⁻is the basic structural unit of silicates

(d)

Feldspar is not aluminosilicate

44.

The geometry at which carbon atom in diamond are bonded to each other is _______.

(a)

Tetrahedral

(b)

hexagonal

(c)

Octahedral

(d)

none of these

45.

Which of the following is not sp² hybridised?

(a)

Graphite

(b)

graphene

(c)

Fullerene

(d)

dry ice

46.

Which of these is not a monomer for a high molecular mass silicone polymer?

(a)

Me₃SiCl

(b)

PhSiCl₃

(c)

MeSiCl₃

(d)

Me₂SiCl₂

47.

When copper is heated with conc HNO₃ it produces ________.

(a)

Cu(NO₃)₂, NO and NO₂

(b)

Cu(NO₃)₂ and N₂O

(c)

Cu(NO₃)₂ and NO₂

(d)

Cu(NO₃)₂ and NO

48.

Among the following the correct order of acidity is ________.

(a)

HClO₂ < HClO < HClO₃ < HClO₄

(b)

HClO₄ < HClO₂ < HClO < HClO₃

(c)

HClO₃ < HClO₄ < HClO₂ < HClO

(d)

HClO < HClO₂ < HClO₃ < HClO₄

49.

Which one of the following orders is correct for the bond dissociation enthalpy of halogen molecules?

(a)

Br₂ > I₂ > F₂ > Cl₂

(b)

F₂ > Cl₂ > Br₂ > l₂

(c)

I₂ > Br₂ > Cl₂ > F₂

(d)

Cl₂ > Br₂ > F₂ > I₂

50.

Which of the following is strongest acid among all?

(a)

(b)

(c)

HBr

(d)

HCl

51.

XeF₆ on complete hydrolysis produces________.

(a)

XeOF₄

(b)

XeO₂F₂

(c)

XeO₃

(d)

XeO₂

52.

Most easily liquefiable gas is _______.

(a)

(b)

(c)

(d)

53.

Which one of the following compounds is not formed?

(a)

XeOF₄

(b)

XeO₃

(c)

XeF₂

(d)

NeF₂

54.

The correct order of the thermal stability of hydrogen halide is_______.

(a)

HI > HBr > HCl > HF

(b)

HF > HCl > HBr > HI

(c)

HCl > HF > HBr > HI

(d)

HI > HCl > HF > HBr

55.

Among the following, which is the strongest oxidizing agent?

(a)

Cl₂

(b)

F₂

(c)

Br₂

(d)

l₂

56.

The molarity of given orthophosphoric acid solution is 2M. Its normality is _______.

(a)

(b)

(c)

(d)

none of these

57.

The basicity of pyrophosphorous acid ( H₄P₂O₅) is _______.

(a)

(b)

(c)

(d)

58.

P₄O₆ reacts with cold water to give _______.

(a)

H₃PO₃

(b)

H₄P₂O₇

(c)

HPO₃

(d)

H₃PO₄

59.

On hydrolysis, PCl₃ gives________.

(a)

H₃PO₃

(b)

PH₃

(c)

H₃PO₄

(d)

POCl₃

60.

Solid (A) reacts with strong aqueous NaOH liberating a foul smelling gas(B) which spontaneously burn in air giving smoky rings. A and B are respectively_________.

(a)

P₄(red) & PH₃

(b)

P₄(white) & PH₃

(c)

S₈ & H₂S

(d)

P₄(white) & H₂S

61.

An element belongs to group 15 and 3^rdperiod of the periodic table, its electronic configuration would be_______.

(a)

1s² 2s² 2p⁴

(b)

1s² 2s² 2p³

(c)

1s² 2s² 2p⁶ 3s² 3p²

(d)

1s² 2s² 2p⁶ 3s² 3p³

62.

Which is true regarding nitrogen?

(a)

least electronegative element

(b)

has low ionisation enthalpy than oxygen

(c)

d- orbitals available

(d)

ability to form pπ-pπ bonds with itself

63.

In which of the following, NH₃ is not used?

(a)

Nessler's reagent

(b)

Reagent for the analysis of IV group basic radical

(c)

Reagent for the analysis of III group basic radical

(d)

Tollen's reagent

64.

The repeating unit in silicone is_______.

(a)

SiO₂

(b)

(c)

(d)

65.

The basic structural unit of silicates is _______.

(a)

\(\left( SiO_{ 3 } \right) ^{ 2- }\)

(b)

\(\left( SiO_{ 4 } \right) ^{ 2- }\)

(c)

\(\left( Sio \right) ^{ - }\)

(d)

\(\left( SiO_{ 4 } \right) ^{ 4- }\)

66.

Oxidation state of carbon in its hydrides _______.

(a)

(b)

-4

(c)

(d)

67.

Carbon atoms in fullerene with formula C₆₀have _______hybridisation.

(a)

sp³ hybridised

(b)

sp hybridised

(c)

sp² hybridised

(d)

partially sp² and partially sp³ hybridised

68.

The element that does not show catenation among the following p-block elements is ________.

(a)

Carbon

(b)

silicon

(c)

Lead

(d)

germanium

69.

In diborane, the number of electrons that accounts for banana bonds is ________.

(a)

six

(b)

two

(c)

four

(d)

three

70.

Which of the following metals has the largest abundance in the earth’s crust?

(a)

Aluminium

(b)

Calcium

(c)

Magnesium

(d)

Sodium

71.

Which among the following is not a borane?

(a)

B₂H₆

(b)

B₃H₆

(c)

B₄H₁₀

(d)

none of these

72.

Boric acid is an acid because its molecule________.

(a)

contains replaceable H⁺ ion

(b)

gives up a proton

(c)

combines with proton to form water molecule

(d)

accepts OH^- from water, releasing proton.

73.

An aqueous solution of borax is________.

(a)

neutral

(b)

acidic

(c)

basic

(d)

amphoteric

74.

Which of the following is not true with respect to Ellingham diagram?

(a)

Free energy changes follow a straight line. Deviation occurs when there is a phase change.

(b)

The graph for the formation of CO₂ is a straight line almost parallel to free energy axis.

(c)

Negative slope of CO shows that it becomes more stable with increase in temperature.

(d)

Positive slope of metal oxides shows that their stabilities decrease with increase in temperature.

75.

Which of the following reduction is not thermodynamically feasible?

(a)

\({ Cr }_{ 2 }{ O }_{ 3 }+2Al\longrightarrow { Al }_{ 2 }{ O }_{ 3 }+2Cr\)

(b)

\(\mathrm{Al}_2 \mathrm{O}_3+2 \mathrm{Cr} \longrightarrow \mathrm{Cr}_2 \mathrm{O}_3+2 \mathrm{Al}\)

(c)

\(3Ti{ O }_{ 2 }+4Al\longrightarrow 2A{ l }_{ 2 }{ O }_{ 3 }+3Ti\)

(d)

none of these

76.

In the Ellingham diagram, for the formation of carbon monoxide________.

(a)

\(\left( \cfrac { \Delta { S }^{ 0 } }{ \Delta T } \right) \) is negative

(b)

\(\left( \cfrac { \Delta { G }^{ 0 } }{ \Delta T } \right) \) is positive

(c)

\(\left( \cfrac { \Delta { G }^{ 0 } }{ \Delta T } \right) \) is negative

(d)

initially \(\left( \cfrac { \Delta T }{ \Delta { G }^{ 0 } } \right) \) is positive, after 700^oC,\(\left( \cfrac { \Delta { G }^{ 0 } }{ \Delta T } \right) \) is negative

77.

Which of the following plot gives Ellingham diagram

(a)

\(\Delta S \ \text{Vs} \ T\)

(b)

\(\Delta { G }^{ 0 }\ \text{Vs} \ T\)

(c)

\(\Delta { G }^{ 0 }\ \text{Vs} \ \frac { 1 }{ T } \)

(d)

\(\Delta { G }^{ 0 }\ \text{Vs} \ { T }^{ 2 }\)

78.

In the electrolytic refining of copper, which one of the following is used as anode?

(a)

Pure copper

(b)

Impure copper

(c)

Carbon rod

(d)

Platinum electrode

79.

The incorrect statement among the following is______.

(a)

Nickel is refined by Mond’s process

(b)

Titanium is refined by Van Arkel’s process

(c)

Zinc blende is concentrated by froth floatation

(d)

In the metallurgy of gold, the metal is leached with dilute sodium chloride solution

80.

Which of the following is used for concentrating ore in metallurgy?

(a)

Leaching

(b)

Roasting

(c)

Froth floatation

(d)

Both (a) and (c)

81.

The following set of reactions are used in refining Zirconium
\(Zr \text{(impure)}+2I_{ 2 }\overset { 523k }{ \longrightarrow } ZrI_{ 4 }\)
\({ ZrI }_{ 4 }\overset { 1800K }{ \longrightarrow } Zr \text{(pure)}+{ 2I }_{ 2 }\)This method is known as ______.

(a)

Liquation

(b)

Van Arkel process

(c)

Zone refining

(d)

Mond’s process

82.

Considering Ellingham diagram, which of the following metals can be used to reduce alumina?

(a)

(b)

(c)

(d)

83.

Extraction of gold and silver involves leaching with cyanide ion. silver is later recovered by_______.

(a)

Distillation

(b)

Zone refining

(c)

Displacement with zinc

(d)

liquation

84.

Zinc is obtained from ZnO by________.

(a)

Carbon reduction

(b)

Reduction using silver

(c)

Electrochemical process

(d)

Acid leaching

85.

In the extraction of aluminium from alumina by electrolysis, cryolite is added to_______.

(a)

Lower the melting point of alumina

(b)

Remove impurities from alumina

(c)

Decrease the electrical conductivity

(d)

Increase the rate of reduction

86.

Which one of the following ores is best concentrated by froth – floatation method?

(a)

Magnetite

(b)

Haematite

(c)

Galena

(d)

Cassiterite

87.

Flux is a substance which is used to convert_______.

(a)

Mineral into silicate

(b)

Infusible impurities to soluble impurities

(c)

Soluble impurities to infusible impurities

(d)

All of these

88.

Electrochemical process is used to extract_______.

(a)

Iron

(b)

Lead

(c)

Sodium

(d)

silver

89.

Which one of the following is not feasible

(a)

Zn_(s) + Cu²⁺_(aq) \(\rightarrow\) Cu_(s) + Zn²⁺_(aq)

(b)

Cu_(s)+ Zn²⁺_(aq)\(\rightarrow\) Zn_(s) + Cu²⁺_(aq)

(c)

Cu_(s) + 2Ag⁺_(ag)\(\rightarrow\) 2Ag_(s) + Cu²⁺_(aq)

(d)

Fe_(s) + Cu²⁺_(aq) \(\rightarrow\) Cu_(s)+ Fe²⁺_(aq)

90.

Wolframite ore is separated from tinstone by the process of________.

(a)

Smelting

(b)

Calcination

(c)

Roasting

(d)

Electromagnetic separation

91.

Match items in column - I with the items of column – II and assign the correct code.

Column-I		Column-II
A.	Cyanide process	(i)	Ultrapure Ge
B	Froth floatation process	(ii)	Dressing of ZnS
C	Electrolytic reduction	(iii)	Extraction of Al
D	Zone refining	(iv)	Extraction of Au
		(v)	Purification of Ni

(a)

A	B	C	D
(i)	(ii)	(iii)	(iv)

(b)

A	B	C	D
(iii)	(iv)	(v)	(i)

(c)

A	B	C	D
(iv)	(ii)	(iii)	(i)

(d)

A	B	C	D
(ii)	(iii)	(i)	(v)

92.

Which of the following statements, about the advantage of roasting of sulphide ore before reduction is not true?

(a)

\(\Delta { G }_{ f }^{ 0 }\) of sulphide is greater than those for CS₂ and H₂S

(b)

\(\Delta { G }_{ r }^{ 0 }\) is negative for roasting of sulphide ore to oxide

(c)

Roasting of the sulphide to its oxide is thermodynamically feasible

(d)

Carbon and hydrogen are suitable reducing agents for metal sulphides

93.

Which of the metal is extracted by Hall-Heroult process?

(a)

(b)

(c)

(d)

94.

The metal oxide which cannot be reduced to metal by carbon is ________.

(a)

PbO

(b)

Al₂O₃

(c)

ZnO

(d)

FeO

95.

Which one of the following reaction represents calcinations?

(a)

\(2Zn+{ O }_{ 2 }\rightarrow 2ZnO\)

(b)

\(2ZnS+3O_{ 2 }\rightarrow 2ZnO+2SO_{ 2 }\)

(c)

\(MgCO_{ 3 }\rightarrow MgO+CO_{ 2 }\)

(d)

Both (a) and (c)

96.

Roasting of sulphide ore gives the gas (A).(A) is a colourless gas. Aqueous solution of (A) is acidic. The gas (A) is______.

(a)

CO₂

(b)

SO₃

(c)

SO₂

(d)

H₂S

97.

Bauxite has the composition ______.

(a)

Al₂O₃

(b)

Al₂O₃.nH₂O

(c)

Fe₂O₃.2H₂O

(d)

None of these

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Multiple Choice Question

97 x 1 = 97

(d)
crystal field stabilization energy of [V(H₂O)₆]²⁺ is higher than the crystal field stabilization of [Ti(H₂O)₆]²⁺

a) Zn²⁺ (d¹⁰ ⇒ diamagnetic)
b) Co³⁺ (d⁶ Low spain ⇒ t_2g⁶ e⁰_g ; diamagnetic)
c) Ni²⁺ (d⁸ Low spain ⇒ t_2g⁶ e²_g ; paramagnetic)
d) [Ni(CN)₄]²⁺ (dsp² ; square planar, diamagnetic)

[Fe(H₂N-CH₂-CH₂-NH₂)₃]₃(PO₄)₂
[Fe(en)₃]²⁺(\(PO_{4}^{3-}\))

a) Fe²⁺ b) Fe³⁺ c) Fe⁰

Option (a) and (b) -geometrical isomerism is possible
Option (c) - ionization isomerism is possible
Option (d) - no possibility to show either constitutional isomerism or stereo isomerism

For [MA₄B₂]⁴⁺ complexes - geometrical isomerism is possible
{[Co(NH₃)₄Br₂]CI,[Co(NH₃)₄Br CI]Br} - ionisation isomers

(a) coordination isomers
(b) no isomerism ( different molecular formula)
(c)⬅NCS; ⬅SCN coordinating atom differs : linkage isomers

Three isomers. If we consider any one of the ligands as reference (say Py), the arrangement of other three ligands (NH₃, Br^- and Cl^-) with respect to (Py) gives three geometrical isomers.

10.

11.

Complexes given in other options (a), (c) and (d) have symmetry elements and hence they are optically inactive.

12.

In all the complexes, the central metal ion is Co³⁺, among the given ligands CN^- is the strongest ligand, which causes large crystal
field splitting i.e maximum Δ₀

13.

The electronic configuration t_2g³, e²_g
[ 3 x (-0.4)+ 2(0.6)]Δ₀
[-1.2 + 1.2] Δ₀ = 0

14.

Ti⁴⁺ (d⁰ ⇒ 0BM)
Co²⁺ (d⁷ spain free ⇒ t_2g⁵, e²_g;n = 3; μ = 3.9BM)
Cu²⁺ (d⁹ Low spain ⇒ t_2g⁶, e³_g; n = 1; μ = 1.732BM)
Ni²⁺ (d⁸ Low spain ⇒ t_2g⁶, e²_g;n = 2; μ = 2.44 BM)

15.

(d)
potassium trioxalatoaluminate (III)

16.

(d)
chloridobis(ethane-1, 2-diamine)nitrito K-O Cobalt(III) chloride

17.

[\( \overset{+}{Fe}\)(H₂O)₅\( \overset{+}{NO}\)]²⁺ SO^2-₄
+1 and +1 respectively

18.

Molecular formula: MSO₄Cl.6H₂O
Formation of white precipitate with Barium chloride indicates that SO^2-₄ ions are outside the coordination sphere, and no precipitate with AgNO₃ solution indicates that the Cl^- ions are inside the coordination sphere. Since the coordination number of M is 6.Cl^- and 5 H₂O are ligands, remaining 1 H₂O molecular and SO^2-₄ are in the outer coordination sphere.

19.

The complex is [M(H₂O)₅Cl]Cl₂
1000 ml of 1 M solution of the complex gives 2 moles of Cl^- ions 1000 ml of 0.01 M solution of the complex will give
\(\frac{100 ml \times 0.01M \times 2Cl^-}{1000 ml \times 1M}\)
= 0.002 moles of Cl^- ions

20.

In the complex [M(en)₂(Ox)]Cl For the central metal ion M3+
The primary valence is = +3
The secondary valence = 6
sum of primary valence and secondary valence = 3 + 6 = 9

21.

(a)
La(OH)₃ is less basic than Lu(OH)₃

22.

(a)
Np, Pu, Am

23.

(b)
+3

24.

(d)
+3

25.

Yb²⁺ - 4f¹⁴ - no unpaired electrons - diamagnetic

26.

As we move from La to Lu, their metallic behaviour because almost similar to that of aluminium.

27.

+7 +2+3 2+ 3+ 4+
MnO₄^- + FeC₂O₄ ⟶ Mn²⁺ + Fe³⁺ + 2CO₂
5e^-acception 3e^- release
5 moles of FeC₂O₄ \(\equiv\) 3 moles of KMnO₄
1 mole of FeC₂O₄ \(\equiv\) (3/5) moles of KMnO₄
1 mole of FeC₂O₄ \(\equiv\) 0.6 moles of KMnO₄

28.

29.

MnO^-₄ + 8H⁺ + 5e^-→ Mn²⁺ + 4H₂O

30.

(b)
Na₂Cr₂O₇ is preferred over K₂Cr₂O₇ in volumetric analysis

31.

(b)
Carbon dioxide

32.

+5 +6 +7
VO₂⁺ < Cr₂O₇^2- < MnO₄^-
Greater the oxidation state, higher is the oxidising power.

33.

34.

Mn²⁺ ⇒ 3d⁵ contains 5 unpaired electrons
n = 5,
\( \sqrt{n(n+ 2)} \) BM
\(= \sqrt{5(5+ 2)} = \sqrt{35} = 5.92 BM\)

35.

36.

(a)
Ti

37.

Cr ⇒ [Ar]3d⁵4s¹

38.

(b)
In case of Sc, 3d orbital are partially filled but in Zn these are completely filled

39.

(a)
Al < Ga < In < Tl

40.

(a)
Metal borides

41.

(d)
Al, Cu, Mn, Mg

42.

(a)

A B C D

2 1 4 3

43.

(d)
Feldspar is not aluminosilicate

44.

(a)
Tetrahedral

45.

(d)
dry ice

46.

(a)
Me₃SiCl

47.

48.

(d)
HClO < HClO₂ < HClO₃ < HClO₄

49.

(d)
Cl₂ > Br₂ > F₂ > I₂

50.

(a)
HI

51.

52.

(d)
Kr

53.

(d)
NeF₂

54.

(b)
HF > HCl > HBr > HI

55.

(b)
F₂

56.

(a)
6N

57.

(b)
2

58.

(a)
H₃PO₃

59.

(a)
H₃PO₃

60.

(b)
P₄(white) & PH₃

61.

(d)
1s² 2s² 2p⁶ 3s² 3p³

62.

(d)
ability to form pπ-pπ bonds with itself

63.

(a)
Nessler's reagent

64.

65.

(d)
\(\left( SiO_{ 4 } \right) ^{ 4- }\)

66.

(a)
+4

67.

68.

69.

70.

(a)
Aluminium

71.

(b)
B₃H₆

72.

(d)
accepts OH^- from water, releasing proton.

73.

74.

(b)
The graph for the formation of CO₂ is a straight line almost parallel to free energy axis.

75.

(b)
\(\mathrm{Al}_2 \mathrm{O}_3+2 \mathrm{Cr} \longrightarrow \mathrm{Cr}_2 \mathrm{O}_3+2 \mathrm{Al}\)

76.

77.

(b)
\(\Delta { G }^{ 0 }\ \text{Vs} \ T\)

78.

(b)
Impure copper

79.

(d)
In the metallurgy of gold, the metal is leached with dilute sodium chloride solution

80.

(d)
Both (a) and (c)

81.

(b)
Van Arkel process

82.

83.

84.

(a)
Carbon reduction

85.

(a)
Lower the melting point of alumina

86.

87.

(b)
Infusible impurities to soluble impurities

88.

89.

(b)
Cu_(s)+ Zn²⁺_(aq)\(\rightarrow\) Zn_(s) + Cu²⁺_(aq)

90.

(d)
Electromagnetic separation

91.

92.

(d)
Carbon and hydrogen are suitable reducing agents for metal sulphides

93.

(a)
Al

94.

(b)
Al₂O₃

95.

96.

97.

(b)
Al₂O₃.nH₂O

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