INTRODUCTION
1. ------------- and ---------------- are the fundamental building blocks of matter.
2. What was the major challenge faced by the scientists before 19th century regarding atoms?
CHARGED PARTICLES IN MATTER
3. An atom is ------------ and consists of -------------- particles.
4. The electron was identified by ----------------.
5. Who discovered the presence of new radiations even before the electrons were found?
6. What are canal rays?
7. These rays were ----------------- charged radiations.
8. What is proton? What are its characteristics?
9. Electron is represented as --------- and proton as -------------.
10. What can you say about the mass of electron?
11. What can you say about the mass of proton?
12. Protons and electrons mutually balance their charges. True or False?
THE STRUCTURE OF AN ATOM
13. According to Dalton's theory atom is indivisible and indestructible. True or False?
14. What lead to the failure of Dalton's theory of atom which states that atom is indivisible an indestructible?
15. Who was the first one to propose a model for the structure of an atom?
THOMSON'S MODEL OF AN ATOM
16. Thomson's model of an atom is similar to that of a ---------------.
17. The electrons were like ----------------.
18. How can you connect watermelon and an atom?
19. How are the electrons studded in an atom?
20. What are the proposals of Thomson?
21. What were the drawbacks of Thomson's model?
RUTHERFORD'S MODEL OF AN ATOM
22. Rutherford concentrated more on the arrangement of -------------- in an atom.
23. In his experiment fast moving -------------- were made to fall on a thin gold foil.
24. Why did he select a gold foil? Explain the nature of the gold foil selected.
25. Write a note on the alpha particles used in the experiment.
26. Why didn't he expect large deflections?
27. What were the observations made by Rutherford?
28. What were his words on the observation?
29. Describe a suitable experiment in an open field equivalent to Rutherford's experiment?
30. What were the conclusions made by Rutherford?
31. What are the features of Rutherford's atomic model?
DRAWBACKS OF RUTHERFORD'S MODEL OF THE ATOM
32. The revolution of the electron in a circular orbit is not expected to be -------------.
33. Describe the drawbacks of Rutherford;s model of atom.
BOHR'S MODEL OF THE ATOM
34. What were the postulates of Bohr's model of atom?
NEUTRONS
35. Who discovered neutron?
36. What are the new aspects discovered by J. Chadwick?
37. Neutrons are present in the nucleus of all atoms except ---------------.
38. How can you calculate the mass of an atom?
HOW ARE ELECTRONS DISTRIBUTED IN DIFFERENT ORBITS(SHELLS) ?
39. Who suggested the distribution of electrons into different orbits?
40. What are the rules followed for writing the number of electrons in different energy levels / shells?
41. Have an idea of the fig. 4.4.
VALENCY
42. What are valence electrons?
43. From the Bohr-Bury scheme we know that the outermost shell of an atom can accomodate a maximum of ------------------ electrons.
44. Which atoms show little chemical activity?
45. When can the combining capacity or valence be zero?
46. Define 'comibining capacity'.
47. What is an octet?
48. How is an octet achieved?
49. How can you calculate the valency?
50. What is the different way of calculating valency? Why is this way needed?
51. Go through the table 4.1.
ATOMIC NUMBER AND MASS NUMBER
ATOMIC NUMBER
52. It is the number of ----------- of an atom, which determines its atomic number.
53. Atomic number is denoted by the letter ----------.
54. All atoms of an element have the same atomic number. True or False?
55. Elements are defined by the number of ---------- they possess.
56. Why is Z=1 in a hydrogen atom?
57. Define atomic number.
MASS NUMBER
58. Mass of an atom is practically due to ----------- and -------------- alone.
59. What are nucleons? Why are they called so?
60. The mass of an atom resides in its --------------.
61. Find out the mass of an atom giving an example.
62. Define mass number.
63. How would you represent thbe atomic number, mass number and symbol of an element? Give example.
ISOTOPES
64. Define isototopes. Give example.
65. Define hydrogen atom as an isotope.
66. What are the three isotopes of hydrogen atom?
67. The chemical properties of isotopes are -------------, but their physical properties are ----------------.
68. What are the isotopes of chlorine atom?
69. Describe an experiment to to find out which of the isotope is to be considered for calculating the mass of chlorine atom.
70. How are the special properties of some isotopes useful in different fields?
ISOBARS
71. What are isobars? Explain with example.
1. ------------- and ---------------- are the fundamental building blocks of matter.
2. What was the major challenge faced by the scientists before 19th century regarding atoms?
CHARGED PARTICLES IN MATTER
3. An atom is ------------ and consists of -------------- particles.
4. The electron was identified by ----------------.
5. Who discovered the presence of new radiations even before the electrons were found?
6. What are canal rays?
7. These rays were ----------------- charged radiations.
8. What is proton? What are its characteristics?
9. Electron is represented as --------- and proton as -------------.
10. What can you say about the mass of electron?
11. What can you say about the mass of proton?
12. Protons and electrons mutually balance their charges. True or False?
THE STRUCTURE OF AN ATOM
13. According to Dalton's theory atom is indivisible and indestructible. True or False?
14. What lead to the failure of Dalton's theory of atom which states that atom is indivisible an indestructible?
15. Who was the first one to propose a model for the structure of an atom?
THOMSON'S MODEL OF AN ATOM
16. Thomson's model of an atom is similar to that of a ---------------.
17. The electrons were like ----------------.
18. How can you connect watermelon and an atom?
19. How are the electrons studded in an atom?
20. What are the proposals of Thomson?
21. What were the drawbacks of Thomson's model?
RUTHERFORD'S MODEL OF AN ATOM
22. Rutherford concentrated more on the arrangement of -------------- in an atom.
23. In his experiment fast moving -------------- were made to fall on a thin gold foil.
24. Why did he select a gold foil? Explain the nature of the gold foil selected.
25. Write a note on the alpha particles used in the experiment.
26. Why didn't he expect large deflections?
27. What were the observations made by Rutherford?
28. What were his words on the observation?
29. Describe a suitable experiment in an open field equivalent to Rutherford's experiment?
30. What were the conclusions made by Rutherford?
31. What are the features of Rutherford's atomic model?
DRAWBACKS OF RUTHERFORD'S MODEL OF THE ATOM
32. The revolution of the electron in a circular orbit is not expected to be -------------.
33. Describe the drawbacks of Rutherford;s model of atom.
BOHR'S MODEL OF THE ATOM
34. What were the postulates of Bohr's model of atom?
NEUTRONS
35. Who discovered neutron?
36. What are the new aspects discovered by J. Chadwick?
37. Neutrons are present in the nucleus of all atoms except ---------------.
38. How can you calculate the mass of an atom?
HOW ARE ELECTRONS DISTRIBUTED IN DIFFERENT ORBITS(SHELLS) ?
39. Who suggested the distribution of electrons into different orbits?
40. What are the rules followed for writing the number of electrons in different energy levels / shells?
41. Have an idea of the fig. 4.4.
VALENCY
42. What are valence electrons?
43. From the Bohr-Bury scheme we know that the outermost shell of an atom can accomodate a maximum of ------------------ electrons.
44. Which atoms show little chemical activity?
45. When can the combining capacity or valence be zero?
46. Define 'comibining capacity'.
47. What is an octet?
48. How is an octet achieved?
49. How can you calculate the valency?
50. What is the different way of calculating valency? Why is this way needed?
51. Go through the table 4.1.
ATOMIC NUMBER AND MASS NUMBER
ATOMIC NUMBER
52. It is the number of ----------- of an atom, which determines its atomic number.
53. Atomic number is denoted by the letter ----------.
54. All atoms of an element have the same atomic number. True or False?
55. Elements are defined by the number of ---------- they possess.
56. Why is Z=1 in a hydrogen atom?
57. Define atomic number.
MASS NUMBER
58. Mass of an atom is practically due to ----------- and -------------- alone.
59. What are nucleons? Why are they called so?
60. The mass of an atom resides in its --------------.
61. Find out the mass of an atom giving an example.
62. Define mass number.
63. How would you represent thbe atomic number, mass number and symbol of an element? Give example.
ISOTOPES
64. Define isototopes. Give example.
65. Define hydrogen atom as an isotope.
66. What are the three isotopes of hydrogen atom?
67. The chemical properties of isotopes are -------------, but their physical properties are ----------------.
68. What are the isotopes of chlorine atom?
69. Describe an experiment to to find out which of the isotope is to be considered for calculating the mass of chlorine atom.
70. How are the special properties of some isotopes useful in different fields?
ISOBARS
71. What are isobars? Explain with example.
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