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

11th Standard

    Reg.No. :
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Chemistry

Time : 00:45:00 Hrs
Total Marks : 100
    100 x 1 = 100
  1. The oxidation state of a element in its uncombined state is

    (a)

    zero

    (b)

    +1

    (c)

    -1

    (d)

    none

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

    (a)

    redox

    (b)

    reduction

    (c)

    oxidation

    (d)

    decomposition

  3. The oxidation number of hydrogen in LiH is _____________

    (a)

    +1

    (b)

    -1

    (c)

    +2

    (d)

    -2

  4. The oxidation number of Cr in Cr2O72- __________ is

    (a)

    +6

    (b)

    -6

    (c)

    +7

    (d)

    -7

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

    (a)

    CrO2Cl2

    (b)

    MnO2

    (c)

    [Fe(CN)6]3-

    (d)

    MnO

  6. 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)

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

    (a)

    Solids

    (b)

    Liquid

    (c)

    Gases

    (d)

    None of these

  8. 12 g of carbon-12 contains_____carbon atoms

    (a)

    6.022 x 1023

    (b)

    6

    (c)

    12

    (d)

    12.022 x 10-23 kg

  9. 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

  10. 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

  11. 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

  12. 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

  13. 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

  14. Identify the compound formed during the rusting of iron

    (a)

    Fe2O3

    (b)

    Fe2O3.xH2O

    (c)

    FeO.xH2O

    (d)

    FeO

  15. The molar mass of Na2SO4 is.....

    (a)

    129

    (b)

    142

    (c)

    110

    (d)

    70

  16. Which of the following pairs of d-orbitals will have electron density along the axes ?

    (a)

    dz2, dxz

    (b)

    dxz, dyZ

    (c)

     dz2, dx2-y2

    (d)

    dxy ,dx2-y2

  17. Shape of an orbital is given by

    (a)

    Principal quantum number

    (b)

    Spin quantum number

    (c)

    Azimuthal quantum number

    (d)

    Magnetic quantum number

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

    (a)

    N3+

    (b)

    Fe2+

    (c)

    Zn+

    (d)

    Cu+

  19. 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

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

    (a)

    6, 13

    (b)

    6, 7

    (c)

    13,6

    (d)

    7,6

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

    (a)

    Carbon

    (b)

    Nitrogen

    (c)

    Oxygen

    (d)

    Fluorine

  22. Neutrons was discovered by

    (a)

    Rutherford

    (b)

    Chadwick

    (c)

    Bohr

    (d)

    Thomson

  23. If En = -313.6/n2,If the value of Ei = -34.84 to which value 'n' corresponds

    (a)

    4

    (b)

    3

    (c)

    2

    (d)

    1

  24. 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)

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

  25. 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

  26. 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

  27. 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

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

    (a)

    3

    (b)

    7

    (c)

    5

    (d)

    9

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

    (a)

    (b)

    (c)

    (d)

  30. 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

  31. Identify the quantum number for 4dx2-y2.electron.

    (a)

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

    (b)

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

    (c)

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

    (d)

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

  32. The value of n, I, m and s of 8th 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)

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

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

    (a)

    0.529 \(\mathring{A}\)

    (b)

    0.0753\(\mathring{A}\)

    (c)

    0.7053\(\mathring{A}\)

    (d)

    0.0529\(\mathring{A}\)

  34. What are the values of n, I, m and s for 3px electron?

    (a)

    3,2,1,0

    (b)

    3,1,-1,+1/2

    (c)

    3,2,+1,-1/2

    (d)

    3,0,0,+1/2

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

    (a)

    Berzelius

    (b)

    Dobereiner

    (c)

    Lavoisier

    (d)

    John Dalton

  36. Which of the following is Dobereiner's triad?

    (a)

    Ne,Ca,Na

    (b)

    H2, N2, O2

    (c)

    Li, Na, K

    (d)

    Na, Br, K

  37. The atomic weight of Au is ______

    (a)

    195

    (b)

    197

    (c)

    198

    (d)

    196

  38. 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

  39. The general electronic configuration of d-block element is _____

    (a)

    ns2np6

    (b)

    (n-1) d1-10 ns0-2

    (c)

    (n-1) d1 ns0-2

    (d)

    (n-1) d0-10 ns2

  40. With respect to chlorine, hydrogen will be

    (a)

    Electropositive

    (b)

    Electronegative

    (c)

    Neutral

    (d)

    None of these

  41. Which of the following processes involves absorption of energy?

    (a)

    Cl(g) +e- ⟶ Cl-

    (b)

    O-(g) +e- ⟶ O2-

    (c)

    O(g) +e- ⟶ O(g)-

    (d)

    S(g)+e- ⟶ S-(g)

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

    (a)

    B<P< S<F

    (b)

    B < S < P < F

    (c)

    F < S < P < B

    (d)

    P< S<B <F

  43. Which period contain 32 elements?

    (a)

    Period 1

    (b)

    Period 4

    (c)

    Period 5

    (d)

    Period 6

  44. Which one of the following is not an isoelectronic ion?

    (a)

    Al3+

    (b)

    N3-

    (c)

    Mg2+

    (d)

    K+

  45. Which of the following pair is not diagonally related?

    (a)

    Li, Mg

    (b)

    Li, Na

    (c)

    Be, Al

    (d)

    B, Si

  46. 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

  47. The number of neutrons in  hydrogen atom is ___________.

    (a)

    three

    (b)

    two

    (c)

    one

    (d)

    zero

  48. The half life period of Tritium is ___________

    (a)

    12.33 secs

    (b)

    12.33 mins

    (c)

    12.33 hrs

    (d)

    12.33 years

  49. Ortho and para hydrogen differ in

    (a)

    proton spin

    (b)

    electron spin

    (c)

    nuclear charge

    (d)

    both b and c

  50. FeSO4 contains _________ molecules of water of hydration.

    (a)

    5

    (b)

    7

    (c)

    10

    (d)

    12

  51. H2O2 is a ________ acid.

    (a)

    mono basic

    (b)

    di basic

    (c)

    tri basic

    (d)

    none

  52. The element which does not contain a neutron is

    (a)

    hydrogen

    (b)

    helium

    (c)

    chlorine

    (d)

    none of the above

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

    (a)

    Phosphorous

    (b)

    Radon

    (c)

    Tritium

    (d)

    Deuterium

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

    (a)

    Soap

    (b)

    Slaked lime

    (c)

    Washing soda

    (d)

    Zeolite

  55. 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

  56. Which of the following is used in photoelectric cells?

    (a)

    Na

    (b)

    K

    (c)

    Li

    (d)

    Cs

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

    (a)

    Lithium

    (b)

    Calcium

    (c)

    Caesium

    (d)

    Francium

  58. Identify the most stable hydride among the following

    (a)

    NaH

    (b)

    LiH

    (c)

    KH

    (d)

    CsH

  59. Alkaline earth metals exhibit ______ oxidation state in their compounds

    (a)

    +1

    (b)

    +2

    (c)

    +4

    (d)

    +6

  60. The element that does not answer the flame test is

    (a)

    Ba

    (b)

    Mg

    (c)

    Ca

    (d)

    Sr

  61. Plaster of Paris is______

    (a)

    CaSO4.H2O

    (b)

    CaSO4.1/2H2O

    (c)

    CaSO4.1/4H2O

    (d)

    CaSO4.2H2O

  62. Dead burnt plaster is ________

    (a)

    CaSO4

    (b)

    CaSO4·1/2H20

    (c)

    CaSO4.H2O

    (d)

    CaSO4.2H20

  63. Which is insoluble in water?

    (a)

    CaF2

    (b)

    CaCI

    (c)

    HgCl2

    (d)

    Ca(NO3)2

  64. Quick lime is:

    (a)

    CaCO3

    (b)

    CaO

    (c)

    CaSO4.2H2O

    (d)

    Ca(OH)2

  65. The general electronic configuration of alkali metals is ____________

    (a)

    [noble gas] ns2

    (b)

    [noble gas] ns1

    (c)

    ns2 np6

    (d)

    ns2 (n-1)d1-10

  66. The second ionization enthalpy of alkali metals is ________

    (a)

    Zero

    (b)

    low

    (c)

    high

    (d)

    very low

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

    (a)

    Li+

    (b)

    RB+

    (c)

    Cs+

    (d)

    K+

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

    (a)

    Be

    (b)

    Ca

    (c)

    Mg

    (d)

    Sr

  69. Which is used to treat upset stomach and eczema?

    (a)

    MgSO4·7H2O

    (b)

    FeSO4·7H2O

    (c)

    CaSO4.2H2O

    (d)

    2CaSO4.H2O

  70. Which of the following is not a peroxide?

    (a)

    KO2

    (b)

    CrO5

    (c)

    Na2O2

    (d)

    BaO2

  71. 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

  72. The absolute zero is _____________

    (a)

    -273oC

    (b)

    273oC

    (c)

    OK

    (d)

    both a and c

  73. Compression factor Z is given by _____________

    (a)

    PV/nRT

    (b)

    P/nRT

    (c)

    PV/R

    (d)

    PV/T

  74. What is the correct increasing order of liquefiability of the gas?

    (a)

    H2 < CO2 < CH4 < N2

    (b)

    H2 < N2 < CH4 < CO2

    (c)

    CO2 < CH4 < H2 < N2

    (d)

    CO2 < CH4 < N2 < H2

  75. Maximum deviations from ideal gas is expected from:

    (a)

    H2(g)

    (b)

    N2(g)

    (c)

    CH4(g)

    (d)

    NH3(g)

  76. A fundamental goal of thermodynamics is the prediction of ------ of the process.

    (a)

    reversibility

    (b)

    rate

    (c)

    spontaneity

    (d)

    none of these

  77. Internal energy is denoted by the symbol------

    (a)

    H

    (b)

    S

    (c)

    G

    (d)

    U

  78. The SI unit of entropy is ______

    (a)

    JK

    (b)

    JK-1

    (c)

    KJ K-1

    (d)

    KJ / mole

  79. Which of the following will have highest \(\Delta\)Hvap value?

    (a)

    Acetone

    (b)

    Ethanol

    (c)

    Carbon tetrachloride

    (d)

    Chloroform

  80. 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

  81. 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

  82. 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

  83. 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)

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

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

    (a)

    Kc

    (b)

    KcRT

    (c)

    Kc(RT)2

    (d)

    Kc(RT)-

  85. 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)

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

  86. 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 equilibrium Kc has the unit.

    (a)

    (mol dm-3)-1

    (b)

    (mol dm-3)1

    (c)

    (mol dm-3)10

    (d)

    (mol dm-3)9

  87. In a binary solution

    (a)

    solvent may be liquid

    (b)

    solvent may be solid

    (c)

    solute may be gas

    (d)

    any of these

  88. 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

  89. 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)

  90. 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

  91. 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)

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

  92. Which of the following molecule has no dative bond?

    (a)

    CO

    (b)

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

    (c)

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

    (d)

    None of these

  93. Which among the following molecule obeys octet rule?

    (a)

    NO

    (b)

    NO2

    (c)

    N2O3

    (d)

    ClO2

  94. 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)

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

  95. Identify the pair of species that possess same bond order.

    (a)

    \(O_{ 2 }^{ 2- }\), B2

    (b)

    NO, CO

    (c)

    N2,O2

    (d)

    He2, H2

  96. Which among the following cannot be formed?

    (a)

    H2

    (b)

    He2

    (c)

    N2

    (d)

    O2

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

    (a)

    (b)

    (c)

    (d)

    All of these

  98. 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)

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

  99. Chloropicrin is prepared by adding nitric acid to______________,

    (a)

    CCl4

    (b)

    CH3CI

    (c)

    CH3CI3

    (d)

    None

  100. 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

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