X CHEMISTRY

UNIT-I

ATOMIC STRUCTURE

1. The _______________ principle states that no two electrons in an atom can have all the four quantum numbers the same.

2. Atomic sizes are expressed in _______________units.

3. Ionisation potential can be determined from _______________ experiment.

4. As nuclear chare increases, ionisation potential _______________.

5. Neutrons and protons are known as _______________.

6. Atomic spectra displays fine structures due to splitting of _______________lines.

7. Units of I.P. are _______________.

8. An a particle consists of _______________and _______________.

9. Chadwick discovered _______________.

10. The ellipticity of Sommerfield’s orbit is given by the ratio _______________.

11. Bohr’s theory of atom is based on _______________.

12. As the ‘n’ value increases _______________ of orbit energy increases.

13. Electron affinity is the highest for _______________ in halogen.

14. As the charge on the ion increases, the ionization energy _______________.

15. Each stationary level state is divided into _______________ states or sub-levels.

16. The number of electrons present in L shell of atom with atomic number 11 are______.

17. The number of ‘p’ electrons present in phosphorous atom are _______________.

18. The ratio of protons and neutrons in C12 is = _______________.

19. The number of unpaired electrons present in an oxygen atom = _______________.

20. The orbital which does not lie along the axis is _______________.

21. The atomic number of the element which can be come negative ion by accepting an electron is_______________.

22. Bohr’s theory can explain _______________.

23. The element atomic number__________ can loose electrons and can become cation.

24. The (n+l) volume for a 3f electron is _______________.

25. Number of electrons in the penultimate shell of strontium atom are_______________.

26. Hydrogen atom gets stability by achieving the configuration of _______________.

27. An electron spinning in clock wise direction is represented as _______________.

28. Atomic number of Magnesium is _______________.

29. 3d10, 4s1 is the valence electronic configuration of _______________.

30. Among 3p, 4s, 3d and 4p, orbit having least energy is _______________.
31. Bohr’s theory is valid for _______________.

32. The maximum value of l and n=5 is _______________.

33. f orbitals are present in _______________.

34. The number of sub-shells present in L shell is _______________.

35. Atoms are made up of sub atomic particles such as _______________ and _____________.

36. According to Bohr’s model electrons revolve only in specified paths called ____________.

37. The principle quantum number gives the size and _______________ of stationary orbit. 38. The shape of the 1s orbital is _______________.

39. _______________ discovered electrons in 1903.

40. Existence of only certain values for a property is known as _______________.

41. ‘h’ is called _______________ constant.

42. In Bohr’s model of atom _______________ and ______________of electron are quantized.

43. If an electron moves from lower energy level to higher energy level, it ______________ energy.

44. Bohr’s model successfully explains the atomic spectrum of hydrogen and other single electron species like _______________ etc.

45. In 1930 _______________ proposed the particle and wave nature (dual nature) of electron.

46. The number of orbitals present in a given stationary orbit are _______________.

47. The number of subshells present in L shell are _______________.

48. The filling up of electrons into orbitals is governed by ________, _______ and ______ principal.

49. _______________ rule states that electron pairing takes place only after all the available degenerated orbitals are occupied by one electron each.

50. Number of electrons can be accommodated in 1s orbital are _______________.

51. One Angstrom unit is equal _______________.

52. Energy of an electron is specified by _______________.

53. Ionisation energy is expressed in units of _________ or _______________ or __________.

54. As the charge on the ion increases, ionization energy _______________.

55. J.J.Thomson discovered _______________.

56. Bohr’s theory is valid for _______________.

57. Number of electrons in ‘d’ sub-level is _______________.

58. Total number of orbitals in the nth shell is _______________.

59. The names s, p, d and f are given to represent in atom are _______________.

60. Angular momentum of electrons in atom is _______________.

X CHEMISTRY

UNIT-I

ATOMIC STRUCTURE (Key )

(1) Pauli’s (2) Angstrom (3) discharge tube (4) increases (5) nucleons (6) spectral (7) ev or K.J. mol-1 or K.Cal mol-1 (8) two protons, two neutrons (9) neutrons (10) n/k (11) Planck’s quantum (12) energy (13) chlorine (14) increases (15) sub stationary (16) 8 (17) 9 (18) 6/6 (19) 2 (20) dxy (21) 17 (22) Li++ (23) 9 (24) 6 (25) 18 (26) Helium (27)? (28) 12 (29) Cu (30) 3p. (31) any atom or ion having one electron (32) 4 (33) N-shell (34) 2 (35) electrons, protons and neutrons (36) stationary orbit (37) energy (38) spherical (39) J.J.Thomosn (40) quantization (41) Planck’s (42) angular momentum , energy (43) stationary orbits (44) He+, Li+2 (45) Louis de Brogile (46) n2 (47) 2 (48) Aufbau, Hund’s Pauli’s (49) Hund’s (50) 2 (51) 10-8 cm (52) principal quantum number (53) ) Energy Volts or K.Joules. mole-1 or K.Cal mole-1 (54) increase (55) electrons (56) an atom or ion having one electron (57) 10 (58) n2 (59) sub levels (60) quantized.