31. The quantum numbers describe the space around the nucleus where the electrons are found and also their energies. These are called ____________.

32. Principal quantum number was introduced by ___________.

33. Principle quantum number was denoted by the letter ‘____’

34. The principal quantum number is related to the _______ and _________ of the main shell.

35. ‘n’ has positive integer values of ____________

36. As ‘n’ increases, the shells become _________ and the electrons in those shells are farther from the nucleus.

37. An increase in ‘n’ also means higher energy. n = 1, 2, 3 … are often represented by the letters __________ For each ‘n’ value there is one main shell.

38. Each shell or orbit has definite energy. These orbits are called ___________.

39. Stationary orbits are denoted by the letters ____________ .etc.

40. The angular-momentum quantum number (l) was proposed by ___________.

41. ‘l’ has integer values from 0 to n-1 for each value of ‘n’. Each ‘l’ value represents one ___________.

42. Each value of ‘l’ is related to the shape of a particular __________ in the space around the nucleus.

43. The value of ‘l’ for a particular sub-shell is generally designated by the letters _________

44. When n = 1, there is only one sub-shell with l= 0. This is designated as ‘____’ orbital.

45. When n = 2, there are two sub-shells, with l= 0, the ‘2s’ sub-shell and with l= 1, the ‘_____’ sub-shell.

46. The magnetic quantum number (ml) quantum number was proposed by ________.

47. Orbitals in the sub-shell belonging to the same shell possess ___________.

48. S-orbital is __________in shape, p-orbital is ____________ and d-orbital are double dumbbell shape.

49. Each sub-shell holds a maximum of _______ as many electrons as the number of orbital’s in the sub-shell.

50. The maximum number of electrons that can occupy various sub-shells is given by the formula _______.

51. The total number of electrons that can occupy various shell or orbit was given by the formula _________.

52. Spin Quantum Number (ms) was introduced by _________ and _________.

53. According to Pauli Exclusion Principle no two electrons of the same atom can have the entire four quantum numbers _________.

54. According to Aufbau principle, the electron enter into _________ orbital’s first.

55. According to ________ rule, the electron pairing takes place all the available degenerate orbitals are completely filled by one electron in each.The clock wise and anti-clock wise spin of the electron was represented by +1/2 and -1/2.

56. Electrons with paired spins are denoted by ‘_____’.

57. The maximum number of electrons in any shell is ‘______’, where ‘n’ is the principal quantum number.

58. The maximum number of electrons in a sub-shell (s, p, d or f) is equal to ________.

59. Electrons are assigned to orbitals in order of increasing value of _______.

60. Spectrum is a group of _____________ or _____________.