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ATOMIC STRUCTURE.

1. The proton and neutron together called as

2. Charge on proton is , electron is and neutron is .

3. Electron was discovered by

4. First model of atom was proposed by

5. According to Thomson electrons are present in

6. Thomson's model of atom failed to explain

7. Rutherford proposed the model of atom based on his experiment.

8. Rutherford 's model of atom is also known as9. According to Rutherford, atoms are in shape.

10. Most of the mass of the atom is present in its

11. According to Rutherford, the two forces acting on the electron are and forces.

12. Quantum theory of radiation is proposed by13. According to Quantum theory electromagnetic radiation is in the form of packets called .

14. Quantum principle is

15. In the formula E = hv 'h ' is

16. Planck based on his theory explained the radiation of

17. Value of Planck 's constant is

18. Bohr proposed a model of atom based on

19. According to Bohr's model, electrons revolve in20. The energy of a stationary orbit which is near to the nucleus is

21. Electron jumps from energy level to energy level.

22. When electron jumps form higher energy level to lower energy level the difference in the energy

levels is radiated as

23. Angular momentum of electron is equal to

24. In the formula mvr = nh /2 n 'n' is known as

25. Splitting of spectral lines in the presence of magnetic field is known as

26. Bohr's model is applicable only for the atoms of

27. Elliptical orbits are introduced by

28. The angular momentum of an electron revolving in elliptical orbit is

29 . According to Sommerfeld stationary orbits are furthe r divided into .30. Dual nature of electron was explained by .

31. De broglie explained based on the dual nature of electron.

32. Wave equation of electron was proposed by

33. Derivations of wave equation lead to

34. Stationary orbits are denoted by

35. Sub stationary orbits are also known as

36. The number of sub stationary orbits present in a stationary orbit depends on value.

37. Number of sub stationary orbits in M orbit are

38. Principle quantum number was proposed by

39. 'n ' value of N shell is

40. The quantum number which gives the size and energy of an orbit is41. No. of sub stationary orbit in a stationary orbit is

42. Azimuthal quantum number was proposed by

43 . Azimuthal quantum number is also known as

44. For a given value of n, the maximum value of l is

45. Shape of sub stationary shell can be determined by using

46. When l = 0, the shape of the orbit is

47. Magnetic quantum number was proposed by .

48. 'm ' value depends on

49. For a given 'l ' value, 'm ' can have values.

50. The boundaries of 'm ' values for a given 'l ' value are

51. Orbitals having same energy are called

52. The orientation of orbitals in the presence of magnetic field can be determined by

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53. The shell having least energy is - .

54. Sub shells present in L- shell are

55. Maximum value of l when n=5 is

56. f- orbital is present in shell.

57. No. of sub shells present in L shell are

58. Spin quantum number was proposed by

59. Spin of electrons takes the values as

60. No. of electrons present in a sub shell are

61. The region in space where there is finite probability of finding electron is called

62. Shape of s- orbital is63. Type of orbital present in K- shell is

64. Type of orbital present in L- shell are

65. Type of orbital present in M-shell are

66. Type of orbital present in N- shell are '

67. The n+l value of 3 s orbital is .

68. The region in space where the probability of find ing electron is zero is called

69. P-orbitals will start in shell.

70. Shape of P-orbital is

71. 'd'-orbi tal will start from

72. The number of d- orbitals present in n = 3 is .

73. The orbital with least energy is74. Among 3 s, 3p the orbital having least energy is .

75. has given a diagram to know the order of energy levels of orbitals.

76. A systematic representation of the occupation of electrons in the orbitals is known as

77. According to principle electron occupies the orbital having lowest energy.

78. Aufbau principle in terms of quantum numbers, the incoming electron occupies an orbital whose

n+l value is

79. The 'l ' value of s-orbital is

80. The 'l ' value of p-orbital is .

81. The 'l ' value of d-orbital is

82. The 'l ' value of f-orbital is

83. rule states that electron pairing takes place only after al the available degenerate

orbitals are occupied by one electron each.84. principle states that no two electrons will have all four quantum numbers same.

85. Electronic configuration of Si (Z = 14 ) is

86. Electronic configuration of Zn (Z=30) is

87. Electronic configuration of K (Z=19) is

88. Electronic configuration of Cr (Z=24) is

89. The distance between nucleus and valency orbital is known as

90. Units of atomic radius A0.

91. 1 A0

= cm.

92. Atomic radius depends on

93. The minimum energy required to remove an electron from the outer most orbital of an atom in

gaseous state is known as94. Units of Ionization Energy are

95. As nuclear charge increases the I.E.

96. As the ion charge increases the I.E. .

97. I.E. with increase in atomic size.

98. The energy released when an electron is added to a neutral gaseous atom in its lowest nergy state

is known as

99. Electron affinity is measured in

100. Among 3p, 4s, 3d and 4p the orbital having least energy is

101. After filling the 3d orbital electron enters into orbital.

102. Valence electronic configuration of Cu is

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MATCHING

GROUP:A GROUP:B

1. Neils Bohr. ( D ) A) Elliptical orbits.

2. Sommerfeld ( A ) B) Spin Quantum number.

3. Uhlenbeck & Goudsmith ( B ) C) Dual nature of electron.

4. Lande ( E ) D) Stationary orbits

5. Louis De - Broglie ( C ) E) Magnetic Quantum Number.

F) Wave Equation.

G) Planetary model.

GROUP:A GROUP:B

1. Principle Quantum number ( D ) A) Sommerfeld

2. Wave equation ( E ) B) Rutherford.

3. Quantum theory of radiation ( C ) C) Max planck

4. Planetary model of atom ( B ) D) Neils Bohr.

5. Azimuthal quantum number ( A ) E) Erwin schrodinger

F) Louis De-broglie

G) J.J.Thomson

GROUP:A GROUP:B

( A ) A)1. K - Shell ( A ) A) n = 1

2. L - Shell ( D ) B) n = 3.

3. M - Shell ( B ) C) f - orbital.

4. N - Shell ( C ) D) n = 2.

5. O - Shell ( E ) E) s,p,d,f,and g orbitals.

GROUP:A GROUP:B

1. Ar ( C ) A)

2. Al ( E ) B)

3. Mg ( B ) C)

4. Ca ( F ) D)

5. Ne ( A ) E)

F)

G)

1s2

2s2

2p6

1s2

2s2

2p63s

2

1s2

2s2

2p63s

23p

6

1s2 2s2 2p63s2 3p2

1s2

2s2

2p63s

23p

1

1s2

2s2

2p63s

23p

64s

2

1s2

2s2

2p63s

23p

4

ELECTRONIC CONFIGURATION OF SOME ELEMENTS

Element Atomic

number

Electronic configuration

Name of the

element

symbol

Atomic

number Long form Valence

configuration

Hydrogen H 1 1s1

1s1

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Helium He 2 1s21s

2

Lithium Li 3 1s22s' (He) 2s1

Beryllium Be 4 1s22s

2(He) 2s

2

Boron B 5 1s2

2s2

2p' (He) 2s2

2p1

Carbon C 6 1s2 2s2 2p2(He) 2s

22p

2

Nitrogen N 7 1s2 2s2 2p3(He) 2s

22p

3

Oxygen O 8 1s2 2s2 2p4(He) 2s

22p

4

Fluorin F 9 1s22s

22p5 (He) 2s

22p

5

Neon Ne 10 1s22s22p6 (He) 2s

22p

6

Sodium Na 11 1s22s22p6 3s' (Ne)3s1

Magnesium Mg 12 1s22s22p6 3s2(Ne)3s

2

Aluminium Al 13 1s22s

22p

6 3s

23P

1(Ne)3s

23p

1

Silicon Si 14 1s22s22p6 3s2 3p2 (Ne)3s23p

2

Phosphorous P 15 1s22s22p6 3s2 3p3 (Ne)3s23p

3

Sulphur S 16 1s22s22p6 3s2 3p4 (Ne)3s23p

4

Chlorine Cl 17 1s22s22p6 3s2 3p5(Ne)3s

23p

5

Argon Ar 18 1s22s22p6 3s2 3p6 (Ne)3s

23p

6

Potassium K 19 1s22s

22p

6 3s

23p

6 4s

1(Ar) 4s

1

Calcium Ca 20 1s22s

22p

6 3s

23p

6 4s

2

1 c21,2 -. 6 0 2 o-r.6 j 2 oj1

(Ar) 4s2

l A A/I J ™ 1

ScandiumTitanium

ScTi

21

22

1s 2s 2p 3s 3p 4s 3d 1s22s22p6 3s2 3p6 4s23d 2

(Ar)4s 3d(Ar)4s

23d

2

Vanadium V 23 1s22s22p6 3s2 3p6 4s23d 3 (Ar)4s23d

3

Chromium Cr 24 1s22s22p6 3s2 3p6 4s13d 5 (Ar)4s13d

5

Manganese Mn 25 1s22s22p6 3s2 3p6 4s23d 5 (Ar)4s23d

5

Iron Fe 26 1s22s

22p

6 3s

23p

6 4s

23d

6 (Ar)4s

23d

6

Cobalt Co 27 1s22s22p6 3s2 3p6 4s23d 7 (Ar)4s

23d

7

Nickel Ni 28 1s22s22p6 3s2 3p6 4s23d (Ar)4s23d

8

Copper Cu 29 1s22s22p6 3s2 3p6 4s13d 10(Ar)4s

13d

10

Zinc Zn 30 1s22s22p6 3s2 3p6 4s23d 10(Ar)4s

23d

10

ANSWERS

1) Nucleons 2) Positive, Negative, No charge 3) J.J.Thomson 4) J.J. Thomson 5) Nucleus

6) Atomic spectra 7) a - ray scattering experiment 8) Planetary model or Nuclear model

9) Spherical 10) Nucleus 11) Centripetal, Centrifugal 12) Max planck 13) Quanta 14) E = hv

15) Planck 's Constant 16) Black body 17) 6.625 x 10-27

erg sec or 6.625 x 10-34

joule.sec

18) Planck 's Quantum theory 19) Stationary orbit 20) Less 21) Higher, Lower 22) E2 - E1 = hv 23) mvr = nh /2n. 24) Pri nci ple q u a n t u m n u m b e r 25) Zeeman effect

26) Single electron 27) Sommerfield 28) mvr = kh/ 2n 29) Sub stationary orbits 30) Louis De Broglie

31) Quantizationof angular momentum 32) Erwin Schordinger 33) Atomic orbitals 34) Principle

quantum number 35) Atomic orbitals 36) n 37) 3 38) Neils bohr 39) 4 40) Principle quantum number

41) n2

42) Somerfield 43) Angular momentum quantum number 44) n - 1 45) l 46) Circular 47)

Lande 48) l 49) (2l + 1) 50) -l to +l 51) Degenerate orbitals

52) Magnetic quantum number 53) K 54) s and p 55) 4 56) N 57) 2

58) Uhlenbeck and Goudsmith 59) +1/2 or -1/2 60) 2 61) Orbital 62) Spherical 63) s 64) s and p 65)

s, p, and d 66) s,p,d, and f 67) 3 68) Nodal region 69) L 70) Dumbell 71) M 72) 5 73) 1s

74) 3S 75) Moeller 76) Electronic configuration 77) Aufbau 78) n + l 79) 0 80) 1 81) 2 82) 3

83) Hund 's 84) Pauli' s exclusion 85) 1s22s2 2p6 3s2 3p2 (or) (Ne) 3s2 3p2.

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86) 1s22s

22p

63s

23p

64s

23d

10(or) (Ar) 4s

23d

10. 87) 1s

22s

22p

63s

23p

64s

1(or) (Ar) 4s

1.

88) 1s22s

22p

63s

23p

64s

13d

5(or) (Ar) 4s

13d

589) Atomic radius 90) A

091) 10

-8Cm

92) Principle quantum number 93) Ionization energy 94) e.v or K. Cal/mole or K. Joule/mole

95) increases 96) increases 97) Decreases 98) Electron Affinity 99) ev 100) 3p 101) 4p

102) 4s13d

10.

R t Ed ti

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