Chemistry 1st Year Chapter 5 Atomic Structure Notes MCQs Bank

chemistry 11th notes chapter 5

1. The shapes of s orbitals is circular and their size:


2. Radius of the third shell of H-atom is:


3. Which of the following has highest ionization energy value?


4. The smallest charge of electricity which has been measured on any particle is:


5. Which one of the following orbital will be first filled:


6. Which of the following orbital is not possible:


7. If “r” is the radius of first orbit, the radius of “nth” orbit of H-atom will be:


8. In which of the following, all have the same number of electrons:


9. The no. of electrons in the M. shell of the element with atomic number 24 is:


10. A fast moving neutron can eject from nitrogen:


11. X-rays were discovered by:


12. When 6d orbital is complete, entering electron goes into:


13. The correct set of four quantum numbers for the valence electron of rubidium (Z = 37) is:


14. The SI unit of wave number is:


15. The mass of an oxygen atom is:


16. The mass of a neutron is:


17. The electron configuration of K(19) is:


18. The radius of first orbit of hydrogen atom is:


19. The ionic specie having more electrons than neutrons is:


20. Which group shows the abnormal behavior in trend of ionization energy in periods?


21. An orbital can accommodate max. of:


22. A nodal plane in an orbital is the plane where the electron density is:


23. Ionization energy depends upon:


24. The mass of a proton is:


25. The ion that is iso-electronic with CI atom is:


26. Angular momentum of an electron:


27. The value of Plank’s constant ’11’ is:


28. Which of the following particles contain 20n, 19p and 18e:


29. How many times the mass of neutrons is greater than the mass of an electron?


30. Identify the correct order of increasing energy:


31. Isotopes differ in:


32. Angle of deflection of cathode rays in electric field was studied by:


33. Colour of fluorescence produced by cathode rays depends upon:


34. Isotopes are:


35. Spin quantum number was given by:


36. The wave number of the light emitted by a certain source is 2 x 10^6 m. The wavelength of this light will be:


37. The correct number of degenerate orbitals:


38. When electron de-excite back into orbit 1, then series obtained is:


39. Balmer series lie in:


40. Charge of electron was measured by:


41. Free neutron change into proton with the emission of:


42. X-rays have same nature as:


43. Positive rays give flash on:


44. An orbital which is spherically symmetrical is:


45. Shapes of p orbitals:


46. The value of elm ratio of electron is C kg⁻¹:


47. The electrons in K-shell of the atom will differ in:


48. Total number of d-electrons in an atom of atomic number 26 is:


49. The place between the two orbitals is called:


50. With the increasing atomic number, ionization energy increases along a period because:


51. Quantum number values for 2p orbitals are:


52. 2nd ionization energy of Mg is higher than the first because:


53. Plank’s equation is:


54. The number of d-electrons in Fe+2 (Z=26) is not equal to:


55. Millikan used in his atomizer:


56. The orbital which is spherically symmetrical is:


57. Which of the following particles would on losing an electron has its outermost p-orbital as half-filled?


58. This represents a/an:


59. Greater shielding effect corresponds to ionization energy value:


60. The elm value for the positive rays is maximum for:


61. The value of Rhdberg constant is:


62. The maximum number of electrons in a sub-shell with! = 3 is:


63. Pressure in gas discharge tube was kept:


Short Questions

1. According to de-Broglie’s idea only microscopic particles have the waves.How waves were measured?
2. Calculate mass of an electron from its e/m value.
3. Calculate the number of electrons in s,p,d and f- sub shells from the formula and write separately.
4. Cathode rays are material in nature justify it.
5. Define atomic number?Write the electronic configuration of oxygen?
6. Define Hund’s rule?
7. Define Zeeman’s effect and Stark’s effect.
8. Differentiate between line spectrum and continuous spectrum.
9. Do you think that the size of Li⁺² is even smaller than He⁺?justify with calculations.
10. Energy of an electron is inversely proportional to ‘N₂’ but energy of higher orbits are always greater than those of the lower orbits.Why?
11. Give any two properties of Neutron.
12. Give properties of positive rays.
13. Give reason for the production of positive rays.
14. Heisenberg’s uncertainty principle has no relation with Bohr’s atomic model.justify it?
15. How Bohr’s model justifies the H-spectra?
16. How did Rutherford’s model of an atom first of all proved the existence of nucleus of the atom?
17. How do you come to know that velocities of electrons in higher orbits are less than those in lower orbits of hydrogen atom?
18. How do you justify that of orbit in H-atom is directly proportional to the square of number of orbit?
19. How do you justify that radius of orbit in H-atom is inversely proportional to the number of protons in the nucleus?
20. How do you justify that the distances between adjacent orbits of H atom go on increasing from lower to the higher orbits?
21. How does Bohr introduce the Planck’s quantum theory in his model?Give its two postulates?
22. How does Bohr’s equation give us the wave number of photon which is emitted or absorbed during jumping of electron between two orbits?
23. How is atomic emission spectrum obtained?
24. How neutron was discovered by Chadwick. Give nuclear equation involved.
25. How the bending of the cathode rays in the electric and magnetic fields shows that they are negatively charged?
26. How the idea of dual nature of matter was deduced from the dual nature of light?
27. How the idea of the proton can be verified by taking H₂ gas in the discharge tube?
28. How the slow neutrons prove to be more effective than the fast neutrons?
29. How various experiments conducted in the cathode ray tube show that cathode rays are material particles with the negative charge on them?
30. Hydrogen atom and He⁺ are monoelectronic system but the size of He⁺ is much smaller than H.Why?
31. Indicate the limiting line of Balmer series?
32. Justify that distance gaps between different orbitals go on increasing from the lower to higher orbit.
33. Justify that the distance gaps between different orbits go on increasing from the lower to the higher orbits?
34. State Heisenberg’s uncertainty principle and give its equation.
35. State Pauli’s exclusion principle and Hund’s rule.
36. State Pauli’s exclusion principle.
37. State spin Quantum number briefly.
38. The e/m values of positive rays for different gases are different but those for cathode rays the e/m values are same.justify it?
39. The e/m values of positive rays obtained from hydrogen gas is 1836 times less than that of cathode rays.Justify it?
40. The energy associated with the violet is greater than the red color in the visible region of spectra.Why?
41. The energy difference between adjacent levels goes on decreasing sharply.Why?
42. The magnetic quantum number gives us the orientation of orbital in space.Justify it?
43. The x-rays produced in a discharge tube experiment are characteristic of the target metal.How?
44. What are defects of Bohr’s atomic model?
45. What are the basis of Schrodinger wave equation?
46. What are the defects (draw backs) in the Rutherford’s atomic model?
47. What are the defects of Rutherford’s atomic model?
48. What is difference between continuous spectrum and line spectrum?
49. What is Ha – line in hydrogen spectrum?
50. What is Hund’s rule?
51. What is line spectra of hydrogen and how it differs from continuous spectrum?
52. What is Moseley’s Law?
53. What is orbital? Discuss the shape of p-orbitals.
54. What is Plank’s quantum theory?
55. What is Starch effect?
56. What is the function of azimuthal quantum number?
57. What is the function of principal quantum number?
58. What is Zeeman effect?
59. What will be the position of electron in an atom when (n+I) value is same for two sub-shells?
60. Which observations tell the presence of cathode rays in the discharge tube?
61. Whichever gas is used in the discharge tube the nature of the cathode rays remains the same.Why?
62. Why does the fine structure of H-atom in its spectrum finds no explanation from Bohr’s model?
63. Why e/m of cathode rays is just equal to that of electron?
64. Why e/m value of the cathode rays is just equal to that of electron?
65. Why is it necessary to decrease the pressure in the discharge tube to get the cathode rays?
66. Why it is important (necessary) to decrease the pressure in the discharge tube to get the cathode rays?
67. Why the anode rays depend upon the nature of the gas?
68. Why the cathode rays are produced in the discharge tube by applying a high voltage?
69. Why the photographic plate is dark and a few bright lines are there in the line emission spectra of hydrogen?
70. Why the photographic plate is white and few dark lines are there in the line absorption spectra of a substance?
71. Why the positive rays are als⁰Called canal rays?Give its reason?
72. Write down any two postulates of Plank’s Quantum theory.
73. Write down electronic configuration of Cr (24).
74. Write down electronic configuration of Fe (26) and Br (35).
75. Write down electronic configuration of P (31) and Cu (29).
76. Write the nuclear reaction for the decay of neutron.
77. Write two points in importance of Moseley’s law.

Long Questions

1. Define orbital. Discuss shapes of its two types.
2. Give defects of Bohr’s atomic model.
3. Derive the formula for calculating the energy of an electron in nth orbit using Bohr’s model.
4. Describe Millikan’s oil drop method for the measurement of charge on electron.
5. Discuss magnetic and spin quantum numbers.
6. Write down the properties of cathode rays.
7. Define Quantum numbers. Discuss briefly Azimuthal quantum number.
8. How did Rutherford discover the nucleus of atom?
9. Write down four properties of Neutron.
10. Describe J.J Thomson’s experiment for determining e/m value of electron.
11. Discuss the properties of cathode rays.
12. Describe the discovery and properties of neutron in Chadwick experiment.
13. How the e/m value of electron was measured?
14. Write defects in Rutherford’s model of atom. How Bohr removed them?
15. Write three points of Plank’s quantum theory. Define frequency and wavelength.
16. Derive radius of revolving electron in nth orbit of an atom.
17. Give postulates of Bohr atomic model.
18. Describe atomic emission and atomic absorption spectrum with diagram.
19. What is spectrum? Differentiate between continuous and line spectrum.
20. What are X rays? How they are produced?
21. What are quantum numbers? Discuss their significance.
22. Explain Pauli’s exclusion principle and Hund’s rule.

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