11th Public Exam March 2019 Important Creative One Mark Test 1

Download Tamil Nadu 11th Standard Chemistry question papers, model tests, one-mark questions, important questions, and public exam papers in PDF format. Free study materials and answer keys for TN State Board students.

Questions:

Multiple Choice Question

99 x 1 = 99

Cause of eutrophication is ____________

(a)

Increase of oxygen in water bodies

(b)

Increase in number of aquatic organisms

(c)

Nutrient enrichment of water bodies

(d)

All ofthese

For the homogeneous gas reaction at 600K \(4NH_{ 3\left( g \right) }+5{ O }_{ 2\left( g \right) }\rightleftharpoons 4NO_{ \left( g \right) }+6{ H }_{ 2 }{ O }_{ \left( g \right) }\) The unit of equilibrium constant K" is

(a)

(mol dm^-3)^-1

(b)

(mol dm^-3)

(c)

(mol dm^-3)¹⁰

(d)

(mol dm-³)⁹

For the system \(3A+2B\rightleftharpoons C\) , the expression for equilibrium constant K is __________

(a)

\(\cfrac { \left[ 3A \right] \times \left[ 2B \right] }{ \left[ C \right] } \)

(b)

\(\cfrac { { \left[ A \right] }^{ 3 }\times \left[ B \right] }{ \left[ C \right] } \)

(c)

\(\cfrac { \left[ C \right] }{ { \left[ A \right] }^{ 3 }\times { \left[ B \right] }^{ 2 } } \)

(d)

\(\cfrac { \left[ C \right] }{ { \left[ 3A \right] }\times { \left[ 2B \right] } } \)

For the reaction,\(CaC{ O }_{ 3\left( s \right) }\rightleftharpoons { CaO }_{ \left( s \right) }+{ CO }_{ 2\left( g \right) }\) K_p is equal to __________

(a)

K_c

(b)

K_cRT

(c)

K_c(RT)²

(d)

K_c(RT)^-

Chloropicrin is prepared by adding nitric acid to______________,

(a)

CCl₄

(b)

CH₃CI

(c)

CH₃CI₃

(d)

None

Which among the following cannot be formed?

(a)

H₂

(b)

He₂

(c)

N₂

(d)

O₂

Identify the pair of species that possess same bond order.

(a)

\(O_{ 2 }^{ 2- }\), B₂

(b)

NO, CO

(c)

N₂,O₂

(d)

He₂, H₂

Le-Chatelier's principle is not applicable to _____________

(a)

\({ F }e_{ \left( g \right) }+{ S }_{ \left( s \right) }\rightleftharpoons { FeS }_{ \left( s \right) }\)

(b)

\({ H }_{ 2\left( g \right) }+{ I }_{ 2\left( g \right) }\rightleftharpoons { 2HI }_{ \left( g \right) }\)

(c)

\(x = {-b \pm \sqrt{b^2-4ac} \over 2a}\)

(d)

\({ N }_{ 2\left( g \right) }+3H_{ 2\left( g \right) }\rightleftharpoons { 2NN }_{ 3\left( g \right) }\)

The correct order of increasing bond angles in the following triatomic species is ____________

(a)

\({ NO }_{ 2 }^{ + }\)< NO₂ <\({ NO }_{ 2 }^{ - }\)

(b)

\({ NO }_{ 2 }^{ - }\)< NO₂ <\({ NO }_{ 2 }^{ + }\)

(c)

\({ NO }_{ 2 }^{ - }\)<\({ NO }_{ 2 }^{ + }\)< NO₂

(d)

\({ NO }_{ 2 }^{ + }\)< \({ NO }_{ 2 }^{ - }\)2

10.

Which among the following molecule obeys octet rule?

(a)

(b)

NO₂

(c)

N₂O₃

(d)

ClO₂

11.

Which of the following molecule has no dative bond?

(a)

(b)

\({ SO }_{ 4 }^{ 2- }\)

(c)

\({ CO }_{ 3 }^{ 2- }\)

(d)

None of these

12.

The most stable carbocation is ____________

(a)

\(C{ H }_{ 3 }-\overset { + }{ C } { H }_{ 2 }\)

(b)

\(C{ H }_{ 3 }-\overset { + }{ C } H-C{ H }_{ 3 }\)

(c)

\(C{ H }_{ 2 }=CH-\overset { + }{ C } { H }_{ 2 }\)

(d)

\(\overset { + }{ C } { H }_{ 3 }\)

13.

In which of the following compound has only one type of hybridised carbon atom?

(a)

(b)

(c)

(d)

All of these

14.

The relationship between the values of osmotic pressure of 0.1 M solutions. of KNO₃ (P₁) and CH₃COOH(P₂) is ___________

(a)

P₁ > P₂

(b)

P₂ > P₁

(c)

P₁ = P₂

(d)

\(\frac { { P }_{ 1 } }{ { P }_{ 1 }+{ P }_{ 2 } } =\frac { { P }_{ 2 } }{ { P }_{ 1 }+2{ P }_{ 2 } } \)

15.

Two liquids having vapour pressures \({ p }_{ 1 }^{ 0 }\) and \({ p }_{ 2 }^{ 0 }\) in pure state in the ratio of 2 : 1 are mixed in the molar ratio of 1 : 2. The ratio of their moles in the vapour state would be __________

(a)

1: 1

(b)

1: 2

(c)

2: 1

(d)

3: 2

16.

Which of the following has maximum freezing point?

(a)

Pure H₂0

(b)

0.1 M NaCl (aq)

(c)

0.01 M NaCl (aq)

(d)

0.5 M NaCl (aq)

17.

For associative solutes ____________

(a)

i < 1 and a < 1

(b)

i > 1 and a >. 1

(c)

i < 1 and a < 1

(d)

i > 1 and a < 1

18.

In a binary solution __________

(a)

solvent may be liquid

(b)

solvent may be solid

(c)

solute may be gas

(d)

any of these

19.

Mathematically, the third law of thermodynamics is expressed as _______

(a)

\(\overset{\lim}{T\rightarrow 0}{ S=0 } \)

(b)

\(\overset{\lim}{T\rightarrow \infty} {S=1 } \).

(c)

ΔU = q + w

(d)

G = H - TS

20.

The order of screening effect of electron of s, p, d and f orbits of a given shell of an atom on its outershell electrons is ___________

(a)

s > p > d> f

(b)

f>d>p>s

(c)

P>d>s>f

(d)

f>p>s>d

21.

Which of the following is not a peroxide?

(a)

KO₂

(b)

CrO₅

(c)

Na₂O₂

(d)

BaO₂

22.

The molar mass of Na₂SO₄ is ___________.

(a)

129

(b)

142

(c)

110

(d)

23.

Identify the compound formed during the rusting of iron

(a)

Fe₂O₃

(b)

Fe₂O₃.xH₂O

(c)

FeO.xH₂O

(d)

FeO

24.

Which is used to treat upset stomach and eczema?

(a)

MgSO₄·7H₂O

(b)

FeSO₄·7H₂O

(c)

CaSO₄.2H₂O

(d)

2CaSO₄.H₂O

25.

The value of Avogadro Number N is equal to ___________.

(a)

2.24 x 10^-2L

(b)

22400 cm^-3

(c)

6.023 x 10^-23

(d)

6.023 x 10²³

26.

Which of the following pair is not diagonally related?

(a)

Li, Mg

(b)

Li, Na

(c)

Be, Al

(d)

B, Si

27.

Which one of the following is not an isoelectronic ion?

(a)

Al³⁺

(b)

N^3-

(c)

Mg²⁺

(d)

K⁺

28.

Which one of the following is used to build the beam pipe in accelerators?

(a)

(b)

(c)

(d)

29.

Which of the following can effectively remove all types of hardness of water?

(a)

Soap

(b)

Slaked lime

(c)

Washing soda

(d)

Zeolite

30.

Which of the following ions are more responsible for transmission of nerve signal?

(a)

Li⁺

(b)

RB⁺

(c)

Cs⁺

(d)

K⁺

31.

The second ionization enthalpy of alkali metals is ________

(a)

Zero

(b)

low

(c)

high

(d)

very low

32.

The general electronic configuration of alkali metals is ____________

(a)

[noble gas] ns²

(b)

[noble gas] ns¹

(c)

ns² np⁶

(d)

ns² (n-1)d^1-10

33.

What are the values of n, I, m and s for 3p_x electron?

(a)

3,2,1,0

(b)

3,1,-1,+1/2

(c)

3,2,+1,-1/2

(d)

3,0,0,+1/2

34.

Which period contain 32 elements?

(a)

Period 1

(b)

Period 4

(c)

Period 5

(d)

Period 6

35.

The Bohr's radius of Li²⁺ of 2^nd orbit is ________________

(a)

0.529 \(\mathring{A}\)

(b)

0.0753\(\mathring{A}\)

(c)

0.7053\(\mathring{A}\)

(d)

0.0529\(\mathring{A}\)

36.

The value of n, I, m and s of 8^th electron in an oxygen atom are respectively____________.

(a)

\(1,0,0,+\frac{1}{2}\)

(b)

\(2,1,+1,-\frac{1}{2}\)

(c)

\(2,1,-1,-\frac{1}{2}\)

(d)

\(2,1,0,+\frac{1}{2}\)

37.

Identify the quantum number for 4d_x²-y².electron ____________

(a)

\(4,2,-2,+\frac{1}{2}\)

(b)

\(4,0,0,+\frac{1}{2}\)

(c)

\(4,3,2,+\frac{1}{2}\)

(d)

\(4,3,2,-\frac{1}{2}\)

38.

Which of the following is used in illumination of wrist watches?

(a)

Phosphorous

(b)

Radon

(c)

Tritium

(d)

Deuterium

39.

For the reaction, X₂ O₄(l) \(\rightarrow\) 2 XO₂ (g), \(\Delta\)U=2.1 Kcal, \(\Delta\)S = 20 cal K^-1 at 300 K. Hence,\(\Delta\)G is:

(a)

2.7 Kcal

(b)

-2.7 Kcal

(c)

9.3 K.=cal

(d)

-9.3 Kcal

40.

Enthalpy change for the reaction, 4H (g) \(\rightarrow\) 2H₂ (g) is - 869.6 kJ. The dissociation energy of H - H bond is _________

(a)

-217.4 kJ

(b)

-434.8 kJ

(c)

- 896.6 kJ

(d)

+ 434.8 kJ

41.

10g of hydrogen and 64g of oxygen were filled in a steel vessel and exploded. The amount of water produced in this reaction will be ________

(a)

3mol

(b)

4mol

(c)

1mol

(d)

2mol

42.

Which of the following has the largest wavelength, provided all have equal velocity?

(a)

carbon di oxide molecule

(b)

electron

(c)

ammonia molecule

(d)

proton

43.

The orbital diagram in which both the Pauli's exclusion principle and Hund's rule are violated is __________

(a)

(b)

(c)

(d)

44.

The increasing order of the first ionisation enthalpy of the elements B, P, Sand F (lowest first) is __________

(a)

(b)

B < S < P < F

(c)

F < S < P < B

(d)

P< S

45.

For a principle quantum number n = 4, the total number of orbitals having l = 3 is:

(a)

(b)

(c)

(d)

46.

Which of the following will have highest \(\Delta\)H_vap value?

(a)

Acetone

(b)

Ethanol

(c)

Carbon tetrachloride

(d)

Chloroform

47.

The velocity of light is 3 x 10⁸ ms^-1. The wave length of violet radiation is 400 nm. The wavelength in frequency (Hz) is:

(a)

7.5 x 10¹⁴ Hz

(b)

7.5 x 10¹⁵ Hz

(c)

7.5 x 10¹³ Hz

(d)

7.5 x 10¹⁶ Hz

48.

Maximum deviations from ideal gas is expected from ___________

(a)

H₂(g)

(b)

N₂(g)

(c)

CH₄(g)

(d)

NH₃(g)

49.

Quick lime is ________

(a)

CaCO₃

(b)

CaO

(c)

CaSO₄.2H₂O

(d)

Ca(OH)₂

50.

The element which does not contain a neutron is _____________

(a)

hydrogen

(b)

helium

(c)

chlorine

(d)

none of the above

51.

The SI unit of entropy is ______

(a)

(b)

JK^-1

(c)

KJ K^-1

(d)

KJ / mole

52.

Which is insoluble in water?

(a)

CaF₂

(b)

CaCl2

(c)

HgCl₂

(d)

Ca(NO₃)₂

53.

Dead burnt plaster is ________

(a)

CaSO₄

(b)

CaSO₄·1/2H₂0

(c)

CaSO₄.H₂O

(d)

CaSO₄.2H₂O

54.

Internal energy is denoted by the symbol_______

(a)

(b)

(c)

(d)

55.

A fundamental goal of thermodynamics is the prediction of __________ of the process.

(a)

reversibility

(b)

rate

(c)

spontaneity

(d)

none of these

56.

Plaster of Paris is______

(a)

CaSO₄.H₂O

(b)

CaSO₄.1/2H₂O

(c)

CaSO₄.1/4H₂O

(d)

CaSO₄.2H₂O

57.

Give an example of molecule in which the ratio of the molecular formula is six times the empirical formula.

(a)

C₆H₁₂O₆

(b)

CH₂O

(c)

CH₄

(d)

NA₂CO₃

58.

Which of the following processes involves absorption of energy?

(a)

Cl_(g) +e^- ⟶ Cl^-

(b)

O^-_(g) +e^- ⟶ O^2-

(c)

O_(g) +e^- ⟶ O_(g)^-

(d)

S_(g)+e^- ⟶ S^-_(g)

59.

With respect to chlorine, hydrogen will be __________

(a)

Electropositive

(b)

Electronegative

(c)

Neutral

(d)

None of these

60.

The element that does not answer the flame test is _________

(a)

(b)

(c)

(d)

61.

H₂O₂ is a ________ acid.

(a)

monobasic

(b)

dibasic

(c)

tribasic

(d)

none

62.

Alkaline earth metals exhibit ______ oxidation state in their compounds

(a)

(b)

(c)

(d)

63.

What is the correct increasing order of liquefiability of the gases?

(a)

H₂ < CO₂ < CH₄ < N₂

(b)

H₂ < N₂ < CH₄ < CO₂

(c)

CO₂ < CH₄ < H₂ < N₂

(d)

CO₂ < CH₄ < N₂ < H₂

64.

The empirical formula and molecular mass of a compound are CH₂O and 180g respectively. What will be the molecular formula of the compound?

(a)

C₉H₁₉0

(b)

CH₂O

(c)

C₆H₁₂O₆

(d)

C₂H₄O₂

65.

Identify the most stable hydride among the following ____________

(a)

NaH

(b)

LiH

(c)

(d)

CsH

66.

One mole of Sulphuric acid contains _______oxygen atoms

(a)

4 x 10²³

(b)

4 x 6.023 x 10^-23

(c)

4 x 6.023 x 10²³

(d)

4 x 6.023 x 10³²

67.

12 g of carbon-12 contains_____carbon atoms

(a)

6.022\(\times\)10²³

(b)

(c)

(d)

12.022\(\times\)10^-23 kg

68.

What will be the wavelength of a ball of mass 0.1 kg moving with a velocity of 10ms^-1?

(a)

6.62 \(\times\) 10^-34m

(b)

6.626 \(\times\) 10³⁴m

(c)

6.626 \(\times\) 10^-34m

(d)

6.626 \(\times\) 10³⁴m

69.

Maximum number of electrons in a subshell of an atom is determined by the following

(a)

2l + 1

(b)

4l - 2

(c)

2n²

(d)

4l + 2

70.

The energy of electron in an atom is given by En =

(a)

\(\frac { 4{ \pi }^{ 2 }{ me }^{ 4 } }{ { n }^{ 2 }h^{ 2 } } \)

(b)

\(\frac { 2{ \pi }^{ 2 }{ me }^{ 4 } }{ { n }^{ 2 }h^{ 2 } } \)

(c)

\(\frac { 2{ \pi }^{ 2 }{ me }^{ 4 } }{ { n }^{ 2 }h^{ 2 } } \)

(d)

\(\frac { 2{ \pi }{ me }^{ 4 } }{ { n }^{ 2 }h^{ 2 } } \)

71.

The general electronic configuration of d-block element is _____

(a)

ns²np⁶

(b)

(n-1) d^1-10 ns^0-2

(c)

(n-1) d¹ ns^0-2

(d)

(n-1) d^0-10 ns²

72.

If E_n = -313.6/n2,If the value of E_i = -34.84 to which value 'n' corresponds __________

(a)

(b)

(c)

(d)

73.

Compression factor Z is given by _____________

(a)

PV/nRT

(b)

P/nRT

(c)

PV/R

(d)

PV/T

74.

FeSO₄ contains _________ molecules of water of hydration.

(a)

(b)

(c)

(d)

75.

Neutron was discovered by ________

(a)

Rutherford

(b)

Chadwick

(c)

Bohr

(d)

Thomson

76.

Name the element whose isotope has mass number 14 and 8 neutrons.

(a)

Carbon

(b)

Nitrogen

(c)

Oxygen

(d)

Fluorine

77.

How many neutrons and protons respectively are present in the ₆C¹³ nuclei?

(a)

6, 13

(b)

6, 7

(c)

13,6

(d)

7,6

78.

In Rutherford's gold foil experiment, a thin gold foil was bombarded with a stream of fast moving ___________

(a)

B particles

(b)

\(\alpha\)-particles

(c)

\(\gamma\) particles

(d)

\(\delta\) particles

79.

Which of the following metals is most commonly used in photochemical cells?

(a)

Lithium

(b)

Calcium

(c)

Caesium

(d)

Francium

80.

The absolute zero is _____________

(a)

-273^oC

(b)

273^oC

(c)

(d)

both a and c

81.

Find the incorrect statement.

(a)

Smallest atom of periodic table is He

(b)

p-block elements are metals, nonmetals and metalloids

(c)

Noble gases have 8 valence electrons except He

(d)

Valence electron and valency is same for group I

82.

Which of the following is used in photoelectric cells?

(a)

(b)

(c)

(d)

83.

Value of gas constant R is ____________

(a)

0.082dm³atm

(b)

0.987 cal mol^-1 K^-1

(c)

8.3 J mol^-1 K^-1

(d)

8 er mol^-1 K^-1

84.

The characteristic feature of orderly arrangement of molecules belongs to ______________.

(a)

Solids

(b)

Liquid

(c)

Gases

(d)

None of these

85.

The atomic weight of Au is ______

(a)

195

(b)

197

(c)

198

(d)

196

86.

The elements that belong to group 1 of the periodic table are called as _________

(a)

alkali metals

(b)

alkaline earth metals

(c)

chalcogens

(d)

rare gases

87.

Ortho and para hydrogen differ in _____________

(a)

proton spin

(b)

electron spin

(c)

nuclear charge

(d)

both b and c

88.

Which of the following is Dobereiner's triad?

(a)

Ne,Ca,Na

(b)

H₂, N₂, O₂

(c)

Li, Na, K

(d)

Na, Br, K

89.

The first list of 23 chemical elements was published by _____ in the year 1789.

(a)

Berzelius

(b)

Dobereiner

(c)

Lavoisier

(d)

John Dalton

90.

The half life period of Tritium is ___________

(a)

12.33 secs

(b)

12.33 mins

(c)

12.33 hrs

(d)

12.33 years

91.

The number of neutrons in hydrogen atom is ___________.

(a)

three

(b)

two

(c)

one

(d)

zero

92.

Identify the redox reaction taking place in a beaker.

(a)

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

(b)

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

(c)

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

(d)

2Ag_(s) + cu²⁺_(aq) \(\longrightarrow\) 2Ag⁺_aq + Cu_(s)

93.

Maximum oxidation state is present in the central metal atom of which compound

(a)

CrO₂Cl₂

(b)

MnO₂

(c)

[Fe(CN)₆]^3-

(d)

MnO

94.

Which of the following has maximum number of unpaired d-electrons?

(a)

N³⁺

(b)

Fe²⁺

(c)

Zn⁺

(d)

Cu⁺

95.

The oxidation number of Cr in Cr₂O₇^2- _______ is

(a)

(b)

-6

(c)

(d)

-7

96.

Shape of an orbital is given by ____________

(a)

Principal quantum number

(b)

Spin quantum number

(c)

Azimuthal quantum number

(d)

Magnetic quantum number

97.

The oxidation number of hydrogen in LiH is _________

(a)

(b)

-1

(c)

(d)

-2

98.

Fe2 + \(\longrightarrow\) Fe³⁺ + e^- is a ________ reaction.

(a)

redox

(b)

reduction

(c)

oxidation

(d)

decomposition

99.

The oxidation state of a element in its uncombined state is

(a)

zero

(b)

(c)

-1

(d)

none

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Answers Key:

Multiple Choice Question

99 x 1 = 99

(b)
(mol dm^-3)

(b)
K_cRT

(b)
He₂

(a)
\(O_{ 2 }^{ 2- }\), B₂

(a)
\({ F }e_{ \left( g \right) }+{ S }_{ \left( s \right) }\rightleftharpoons { FeS }_{ \left( s \right) }\)

(b)
\({ NO }_{ 2 }^{ - }\)< NO₂ <\({ NO }_{ 2 }^{ + }\)

10.

11.

12.

13.

14.

(a)
P₁ > P₂

15.

(a)
1: 1

16.

(a)
Pure H₂0

17.

(a)
i < 1 and a < 1

18.

(d)
any of these

19.

(a)
\(\overset{\lim}{T\rightarrow 0}{ S=0 } \)

20.

(a)
s > p > d> f

21.

(a)
KO₂

22.

(b)
142

23.

(b)
Fe₂O₃.xH₂O

24.

25.

(d)
6.023 x 10²³

26.

(b)
Li, Na

27.

(d)
K⁺

28.

(a)
Be

29.

(a)
Soap

30.

(d)
K⁺

31.

32.

33.

(b)
3,1,-1,+1/2

34.

(d)
Period 6

35.

36.

(b)
\(2,1,+1,-\frac{1}{2}\)

37.

(a)
\(4,2,-2,+\frac{1}{2}\)

38.

39.

(b)
-2.7 Kcal

40.

(d)
+ 434.8 kJ

41.

(b)
4mol

42.

(b)
electron

43.

44.

(b)
B < S < P < F

45.

(b)
7

46.

47.

(a)
7.5 x 10¹⁴ Hz

48.

(d)
NH₃(g)

49.

(b)
CaO

50.

(a)
hydrogen

51.

(b)
JK^-1

52.

(a)
CaF₂

53.

(a)
CaSO₄

54.

(d)
U

55.

56.

(b)
CaSO₄.1/2H₂O

57.

(a)
C₆H₁₂O₆

58.

(b)
O^-_(g) +e^- ⟶ O^2-

59.

(a)
Electropositive

60.

(b)
Mg

61.

(b)
dibasic

62.

(b)
+2

63.

(b)
H₂ < N₂ < CH₄ < CO₂

64.

65.

(b)
LiH

66.

67.

(a)
6.022\(\times\)10²³

68.

(a)
6.62 \(\times\) 10^-34m

69.

(d)
4l + 2

70.

71.

(b)
(n-1) d^1-10 ns^0-2

72.

(b)
3

73.

(a)
PV/nRT

74.

(b)
7

75.

(b)
Chadwick

76.

(a)
Carbon

77.

(d)
7,6

78.

(b)
\(\alpha\)-particles

79.

80.

(d)
both a and c

81.

(a)
Smallest atom of periodic table is He

82.

(d)
Cs

83.

84.

(a)
Solids

85.

(b)
197

86.

(a)
alkali metals

87.

(a)
proton spin

88.

89.

90.

(d)
12.33 years

91.

(d)
zero

92.

(d)
2Ag_(s) + cu²⁺_(aq) \(\longrightarrow\) 2Ag⁺_aq + Cu_(s)

93.

(a)
CrO₂Cl₂

94.

(b)
Fe²⁺

95.

(a)
+6

96.

97.

(b)
-1

98.

99.

(a)
zero

11th Standard Chemistry Public Exam March 2019 Important Creative One Mark Test 1

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