M.C.Qs on Atomic Structure ......... Unit # 5

Unit # 5…….. M.C.Qs  on Atomic Structure

1.      A compound material which emits faint visible light by absorbing radiant energy is called:
(a)
Fluorescent
(b)
Cathode
(c)
Anode
(d)
None of the above

2.      Cathode rays experiment shows the presence of:
(a)
Electrons  
(b)
Protons
(c)
Neutrons
(d)
Nucleus

3.      The e/m ratio of cathode rays (electrons) is:
(a)
 1.7588x1011C/kg
(b)
1.7588x108 C/g
(c)
 all of the above
(d)
None of the above

4.      The charge on an electron is:  
(a)
 1.6022x10-19  C
(b)
1.6022x10-18 C
(c)
 1.6022x10-29 C
(d)
1.6022x10-21 C

5.      The mass of an electron is:
(a)
 9.1096x10-19 kg
(b)
9.1096x10-31 kg
(c)
 9.1096x10-20  kg
(d)
9.1096x10-30 kg

6.      Which particle has a mass of 1/1836 times that of hydrogen?
(a)
Electrons  
(b)
Protons
(c)
Neutrons
(d)
Positron

7.      Which particle has a mass of 1836 times that of electron?
(a)
β-particles
(b)
Protons
(c)
Neutrons
(d)
Positron

8.      The e/m ratio for positive (anode) rays is ……………..of nature of gas used
(a)
Dependent         
(b)
Independent
(c)
none of the above
(d)
all of the above

9.      Which gas has a highest value of e/m ratio?
(a)
Hydrogen 
(b)
helium
(c)
nitrogen
(d)
oxygen

10.    The e/m ratio of cathode rays is always ……….. anode rays.
(a)
less than 
(b)
greater than
(c)
Equal to
(d)
none of the above

11.    The spontaneous emission of nuclear radiations from radioactive elements is called
(a)
Radioactivity
(b)
Fission
(c)
Cleavage
(d)
Ionization

12.    These are helium nuclei with double positive charge and atomic mass of 4 amu
(a)
alpha rays
(b)
B-rays
(c)
Gamma rays
(d)
X-rays

13.    Alpha rays consist of:
(a)
Stream of hydrogen
(b)
Stream of Helium
(c)
stream of electron only
(d)
Stream of neutron only

14.    The fast moving electrons like the cathode rays are called
(a)
alpha rays
(b)
beta-rays
(c)
gamma rays
(d)
X-rays

15.    Which rays are electromagnetic radiations traveling with velocity of light?
(a)
alpha rays
(b)
beta-rays
(c)
gamma rays
(d)
X-rays

16.    The wavelength of gamma rays is …………than most of the X-rays:
(a)
Shorter
(b)
Larger
(c)
Equal
(d)
all of the above

17.    Which radioactive rays have greater penetrating power?
(a)
alpha rays
(b)
beta-rays
(c)
gamma rays
(d)
none of the above

18.    Gamma rays are emitted as
(a)
Protons     
(b)
Electrons
(c)
Neutrons
(d)
Photons

19.    The phenomenon of emission of radioactive radiations from nuclei of lighter isotopes of a stable element due to bombardment of fast moving sub atomic particles is called
(a)
Radioactivity      
(b)
 natural radioactivity
(c)
artificial radioactivity
(d)
 Cleavage

19.    Which order is correct?
(a)
electron<proton<neutron
(b)
proton<electron<neutron
(c)
neutron<electron<proton
(b)
proton<neutron<electron

20.    Alpha particle consists of: 
(a)
2 protons and one neutrons
(b)
2 electrons and 2 neutrons
(c)
2 protons and 2 neutrons
(b)
2 protons and 3 neutrons

21.    The e/m ratio of positive rays is always:
(a)
Much smaller than cathode rays.
(b)
Much greater than cathode rays.
(c)
equal to cathode rays
(b)
Unpredictable

22.    Photons of red color are:
(a)
More energetic than that of violet colour
(b)
less energetic than that of violet color
(c)
equal energetic than that of violet colour
(b)
none of the above

23.    The frequency of X-rays is:
(a)
very small
(b)
very high
(c)
intermediate      
(d)
all of the above

24.    Moseley showed that frequency of X-rays is directly proportional to:
(a)
 atomic number
(b)
mass number
(c)
 Number of neutrons
(d)
none of the above

25.    Moseley found that the wavelength of X-rays emitted ……. regularly with increasing atomic no:
(a)
 increase
(b)
Decrease
(c)
 both a and b
(d)
none of the above

26.    The energy of photon is directly proportional to
(a)
 frequency of light
(b)
Wavelength
(c)
 all of the above
(d)
none of the above

27.    The energy of photon is inversely proportional to
(a)
 frequency of light
(b)
wavelength
(c)
 speed of light
(d)
none of the above

28.    The spectrum of sun or of incandescent solids (electric light) is:
(a)
 line spectrum
(b)
 continuous spectrum
(c)
 both a and b
(d)
 none of the above

29.    Light of a single wavelength is called
(a)
 Monochromatic
(b)
 Dichromatic
(c)
 Polychromatic
(d)
 All of above
30.    It is called fingerprint of element
(a)
 line spectrum
(b)
 continuous spectrum
(c)
 absorption spectrum
(d)
 all of the above

31.    Violet colour has a wavelength of
(a)
 4000-4200 A°
(b)
 4200-4600 A°
(c)
 4600-5000 A°
(d)
 none of above

32.    Indigo color has a wavelength of
(a)
 6300-7500 A°
(b)
 4600-5100A°
(c)
 4200-4600 A°
(d)
 5100-5800 A°

33.    Blue color has a wavelength of:
(a)
 6300-7500 A°
(b)
 6000-6300 A°
(c)
 5800-6000 A°
(d)
 4600-5100 A°

34.    Green color has a wavelength of
(a)
 4000-4200 A°
(b)
 4200-4600 A°
(c)
 4600-5100 A°
(d)
 5100-5800 A°

35.    Yellow color has a wavelength of
(a)
 5800-6000 A°
(b)
 4000-4200 A°
(c)
 4200-4600 A°
(d)
 4600-5100 A°

36.    The color with wave length 600-630 nm (6000-6300A0) is:
(a)
 Red
(b)
 Green        
(c)
 Yellow
(d)
 Orange

37.    1A is equal to:
(a)
 10-10 m
(b)
 10-8cm
(c)
 10-1nm or 102 pm
(d)
 All of the above

38.    10A° is equal to:
(a)
 10-9m
(b)
 10-7cm
(c)
 1nm 
(d)
 All of the above

39.    The value of plank’s constant is:
(a)
 6.625x10-34 J-S
(b)
 6.625x10-32 J-S
(c)
 6.625x10-36 J-S
(d)
 6.625x10-28 J-S

40.    It is a distance between two successive crest or trough:
(a)
 Frequency
(b)
 Wavelength
(c)
 Amplitude  
(d)
 Wave number

41.    The no of waves per unit distance is called:
(a)
 Wave frequency
(b)
 Wavelength
(c)
 Amplitude
(d)
 wave number

42.    The inverse of wavelength is called:
(a)
 Wave frequency
(b)
 Time period
(c)
 Amplitude
(d)
 Wave number

43.    Rutherford’s alpha particle scattering experiment showed for the first time that the atom has:
(a)
 Electrons
(b)
 Protons
(c)
 Neutrons     
(d)
 A  nucleus

44.    An instrument that measures the intensity and frequency of emitted or absorbed photon radiation is called:
(a)
 Spectrometer
(b)
 Hydrometer
(c)
 Barometer
(d)
 Calorimeter
45.    The numerical value of Bohr’s radius
(a)
 5.29x10-11m
(b)
 5.29x10-9 cm
(c)
 0.529A°     
(d)
 All of the above

46.    Bohr’s theory does not explain the spectra of:
(a)
 Hydrogen
(b)
 single electron system
(c)
 multi electron system
(d)
 none of the above

47.    Lyman series lies in:
(a)
 Visible region (l = 4000-8000A°).
(b)
 Ultraviolet region (l = 2000-5000A°).
(c)
 Infra red region (l = 9000-10000A°).
(d)
 Far-infra red region (l >10000A°).

48.    Balmer series lies in
(a)
 visible region
(b)
 ultra violet region
(c)
 infra red region
(d)
 none of the above

49.    Paschen series lies in
(a)
 visible region
(b)
ultra violet region
(c)
 infra red region
(d)
none of the above

50.    Lyman series is formed when electrons jump from any higher orbit to ……. orbit
(a)
 1
(b)
 2
(c)
 3
(d)
 4

51.    Balmer series is formed when electrons jump from any higher orbit to ____orbit
(a)
 1
(b)
 2
(c)
 3
(d)
 4

52.    paschen series is formed when electrons jump from any higher orbit to………..orbit.
(a)
 1
(b)
 2
(c)
 3
(d)
 4

53.    Bracket series is formed when electron jumps from any higher orbit to……….orbit
(a)
1
(b)
 2
(c)
3
(d)
 4

54.    pfund series is formed when electron jumps from any higher orbit to _____ orbit
(a)
 1
(b)
 5
(c)
 3
(d)
 4

55.    This quantum number tells the size of orbit and energy of electron:
(a)
 n       
(b)
 l
(c)
 m
(d)
 ms

56.    This quantum number shows the shape of an orbital
(a)
 n       
(b)
 l
(c)
 m
(d)
 ms

57.    This quantum number shows the orientation of an orbit
(a)
 n       
(b)
 l
(c)
 m
(d)
 ms

58.    This quantum number specifies the spin of electron in an orbit
(a)
 n       
(b)
 l
(c)
 m
(d)
 ms

59.    Principle quantum number (n) specifies:
(a)
 size of orbit        
(b)
 energy of electron
(c)
 maximum shell capacity
(d)
 all of the above

60.    For energy level n=3 the no of possible sub-shells are
(a)
 1       
(b)
 3
(c)
 4
(d)
 9

61.    If the value of l=0 the orbital is spherical in shape and is called
(a)
 s       
(b)
 p
(c)
 d
(d)
 f

62.    If the value of l=1 the orbital is dumbbell in shape and is called
(a)
 s       
(b)
 p
(c)
 d
(d)
 f

63.    If the value of l=2 the orbital is called
(a)
 s       
(b)
 p
(c)
 d
(d)
 f

64.    No two electrons in an atom has same set of quantum no. this is called
(a)
 Auf-Bau principle
(b)
 Pauli’s principle
(c)
 Uncertainty principle
(d)
 Hund’s rule         

65.    Which of the following principle limits the maximum no of electrons in an orbital of two?
(a)
 Auf-Bau principle
(b)
 Pauli’s principle
(c)
 (n + l)rule
(d)
 Hund’s rule         

66.    The electrons are added in an orbital in the order of increasing orbital energy. This is called
(a)
 Auf-Bau principle
(b)
 Pauli’s principle
(c)
 (n + l)rule
(d)
 Hund’s rule         

67.    In degenerate orbital, electrons would tend to go in separate orbital with same spin.         This is the statement of:
(a)
 Auf-Bau principle
(b)
 Pauli’s principle
(c)
 (n + l)rule
(d)
 Hund’s rule         

68.    Which rule violated in the configuration N = 1s2, 2s2 2px2 2py1
(a)
 Auf-Bau principle
(b)
 Pauli’s principle
(c)
 (n + l)rule
(d)
 Hund’s rule         

69.    When 3d orbital is complete, the newly entering electron goes into
(a)
 4f
(b)
 4p
(c)
 4s
(d)
 4d

70.    The inter nuclear distances between two carbon atoms in diamond is 1.54A than the radius of carbon atom would be:
(a)
 0.77A°
(b)
 0.077A°
(c)
 1.77A°
(d)
 none of the above

71.    Atomic radii decrease along a period due to:
(a)
 increase in nuclear charge
(b)
 decrease in force of attraction on valence electron
(c)
 decrease in nuclear charge
(d)
 none of the above

72.    Atomic radii ……….. in a group from top to bottom:
(a)
 Increase
(b)
 Decrease
(c)
 remains same
(d)
 none of the above

73.    Cations are………… in size than their parent atom:
(a)
 Smaller
(b)
 Larger
(c)
 remains same
(d)
 none of the above

74.    Which one is larger in size than its parent atom?
(a)
 Cl+    
(b)
 Cl
(c)
 Cl
(d)
 none of the above
75.    Anions are………… in size than its parent atom
(a)
 Smaller
(b)
 Larger
(c)
 Equal
(d)
 none of the above

80.    Na+, Mg2+ and Al3+ are called:
(a)
 Iso-electric ions
(b)
 compound ions
(c)
 Anions
(d)
 none of the above

81.    which one is larger in size?
(a)
 Na+
(b)
 Mg2+ 
(c)
 Al3+
(d)
 all are equal in size

82.    The energy required for the removal of least tightly bounded electron from the valence shell        of its isolated atom is called
(a)
 ionization energy
(b)
 ionization potential      
(c)
 I.P.
(d)
 all of the above

83.    The 2nd and 3rd I.P. is always ………. than 1st I.P.
(a)
 Smaller
(b)
 greater      
(c)
 Equal
(d)
 both a and b

84.    It is easier to remove electron from which one of the following
(a)
 Na+
(b)
 Mg+
(c)
 Al3+
(d)
 Ca+

85.    It is difficult to remove electron from which one of the following
(a)
 Ca
(b)
 Mg
(c)
 Al2+
(d)
 Na

86.    Bigger size atoms possess:
(a)
 high I.P.
(b)
 Low I.P.
(c)
 both a and b
(d)
 None of the above

87.    I.P. ………………. from top to bottom in a group
(a)
 Increase    
(b)
 Decrease  
(c)
 Same
(d)
 none of the above

88.    I.P. ………… from left to right in a period
(a)
 Increase    
(b)
 Decrease
(c)
 Same
(d)
 none of the above

89.    The I.P. is inversely proportional to
(a)
 Nuclear energy
(b)
 Shielding effect
(c)
 Both a and b
(d)
 None of the above

90.    The energy released when an electron is added in an lowest energy state of a neutral   isolated gaseous atom to form an anion is called
(a)
 Electron affinity
(b)
 Ionization potential
(c)
 Electronegativity
(d)
 Electropositivity

91.    The formation of a bivalent anion from a univalent anion is always …………:
(a)
 Exothermic
(b)
 Endothermic
(c)
 both a and b
(d)
 None of the above

92.    High values of electron affinity shows that element are
(a)
 oxidizing agent
(b)
 Reducing agent
(c)
 electron donor agents
(d)
 None of the above

93.    The measure of the ability of an atom to attract an electron pair to itself in a chemical   bond is called
(a)
 Electron affinity
(b)
 Ionization potential
(c)
 Electronegativity
(d)
 Electropositivity

94.    The average ionization energy and electron affinity is called
(a)
 electron affinity
(b)
 ionization potential
(c)
 Electronegativity
(d)
 Electropositivity

95.    it is the most electronegative element:
(a)
 F
(b)
 O
(c)
 Cl
(d)
 N

96.    Cations are ________electronegative than their parent atom
(a)
 Less
(b)
 More
(c)
 Equal
(d)
 None of the above

97.    Anions are …………….electronegative than their parent atom
(a)
 Less
(b)
 More
(c)
 Equal
(d)
 None of the above

98.    Electronegativity . ……………in a group from top to bottom
(a)
 Increase
(b)
 Decrease
(c)
 both a and b
(d)
 none of the above

99.    Electronegativity . …………… in a period from left to right
(a)
 Increase
(b)
 Decrease
(c)
 both a and b
(d)
 none of the above

100. If ΔE.N. between two bounded atoms is greater than 1.7 then the bond in between them will be
(a)
 Covalent   
(b)
 Dative
(c)
 Ionic
(d)
 None of the above

101. If the ΔE.N. between two bounded atom is less than 1.7, than the bond in between them will be
(a)
 Covalent   
(b)
 Dative
(c)
 Ionic
(d)
 None of the above

102. Which one is more polar than other?
(a)
 HF
(b)
 NH3
(c)
 H2O
(d)
 CH4

103. Which one is more electronegative than the other?
(a)
 Li+
(b)
 F
(c)
 Cs    
(d)
 O2─

NOTE: nitrogen has 0 electron affinities because it has half-filled valence shell which makes it stable thereby reducing the tendency to accept electron.























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