Here's a detailed question bank based on Chapter 3 of the BISE, Gujranwala curriculum. I’ve organized it with an appropriate mix of easy, moderate, and tough questions according to the structure you requested.
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### **Short Questions (120 Questions)**
**Easy (36 Questions)**
1. What is Dobereiner’s Triads?
2. Define Newlands' Octaves.
3. What was Mendeleev’s contribution to the periodic table?
4. State Mendeleev's Periodic Law.
5. What is the Modern Periodic Law?
6. How is the modern periodic table arranged?
7. What is meant by a "period" in the periodic table?
8. How many periods are in the modern periodic table?
9. Define "group" in the periodic table.
10. How many groups are in the modern periodic table?
11. Define atomic size.
12. What is atomic radius?
13. What is ionization energy?
14. Define electron affinity.
15. What is electronegativity?
16. Describe the shielding effect.
17. Name the scientist who introduced the concept of atomic number.
18. How does atomic size change across a period?
19. What happens to atomic radius down a group?
20. How does ionization energy vary in a group?
21. How does electron affinity change across a period?
22. What is the general trend of electronegativity across a period?
23. What is the highest electronegative element?
24. Which element has the lowest ionization energy?
25. Name the three types of elements found in the periodic table.
26. Which period contains only two elements?
27. What are noble gases?
28. How many elements are in Period 3?
29. Name the most reactive group of nonmetals.
30. State the element with the smallest atomic radius.
31. Which element has the highest first ionization energy?
32. How many elements are in Group 18?
33. Why are noble gases inert?
34. What does "periodicity of properties" mean?
35. How does atomic size change down a group?
36. Which scientist is known as the "Father of the Modern Periodic Table"?
**Moderate (48 Questions)**
1. Describe Dobereiner's contribution to the periodic table.
2. Explain Newlands’ Law of Octaves with an example.
3. How did Mendeleev arrange the elements in his periodic table?
4. How does Mendeleev's periodic table differ from the modern periodic table?
5. Describe one limitation of Mendeleev's periodic table.
6. What are the main features of the modern periodic table?
7. Define the term "periodicity."
8. How does the periodic table organize elements with similar properties?
9. Differentiate between periods and groups in the periodic table.
10. What pattern does the atomic radius follow within a period?
11. How does shielding effect influence atomic size?
12. Why does atomic size increase down a group?
13. Explain the trend in ionization energy across a period.
14. What factors affect electron affinity?
15. Why does electron affinity generally increase across a period?
16. How does shielding effect change down a group?
17. Explain the concept of atomic size in terms of atomic radius.
18. What is the trend in ionization energy across a group?
19. How does electronegativity change down a group?
20. Why do alkali metals have low ionization energies?
21. Explain the relationship between atomic radius and ionization energy.
22. How does electron affinity vary in Group 17?
23. What is meant by "shielding effect" and how does it occur?
24. Differentiate between atomic size and atomic radius.
25. Describe the general trend of atomic size in periods.
26. Explain the reason for increasing atomic size in a group.
27. Why do noble gases have zero electron affinity?
28. How does atomic size relate to periodic trends?
29. What is the effect of increased nuclear charge on atomic radius?
30. Explain the trend of electron affinity in a period.
31. Describe why fluorine has high electronegativity.
32. Why do noble gases show no electronegativity values?
33. Explain why halogens have high electron affinities.
34. How is shielding effect observed in a period?
35. Why does atomic radius decrease from left to right in a period?
36. How does shielding affect ionization energy in a group?
37. Describe why metals generally have low ionization energies.
38. What is the periodic trend in electron affinity from left to right?
39. Why do alkali metals have the largest atomic sizes in their periods?
40. How does atomic number influence periodic trends?
41. Why do halogens have high electronegativity values?
42. Define periodicity and explain its importance.
43. Describe one example of a periodic property.
44. Explain why atomic radius decreases across a period.
45. How do electron affinities differ between metals and nonmetals?
46. Explain how atomic radius affects ionization energy.
47. Why is atomic radius important in the periodic table?
48. Describe the general trend of ionization energy down a group.
**Tough (36 Questions)**
1. Explain the significance of Dobereiner's Triads in early chemistry.
2. Describe the main limitation of Newlands' Octaves.
3. How did Mendeleev handle gaps in his periodic table?
4. Explain the concept of groups and periods in terms of electronic configuration.
5. How is atomic radius measured, and why is it important?
6. Explain the trend of ionization energy in d-block elements.
7. How do electron affinities help in predicting chemical reactivity?
8. Discuss the relationship between atomic size and chemical properties.
9. How do transition elements fit into the modern periodic table?
10. Explain why ionization energy generally increases across a period.
11. Describe the effect of shielding in transition metals.
12. Why is electron affinity low in noble gases?
13. What factors determine the trend of electronegativity across a period?
14. Why do d-block elements show variable oxidation states?
15. Explain why ionization energy trends differ in groups and periods.
16. Discuss why lanthanides have low electronegativity.
17. How does atomic size relate to reactivity in alkali metals?
18. Explain how periodicity is used in predicting element properties.
19. Why do s-block elements show low ionization energies?
20. What is the significance of periodicity in modern chemistry?
21. Discuss the factors that affect electron affinity in a period.
22. Explain why elements in Group 1 are more reactive than those in Group 2.
23. How do atomic radius and ionization energy relate to periodic trends?
24. Describe the trend of atomic radius in p-block elements.
25. Why do transition metals have high melting points?
26. Explain the shielding effect’s role in atomic radius variations.
27. How does nuclear charge impact electronegativity?
28. Describe the periodic trend in electron affinity within a group.
29. Explain how atomic radius varies in noble gases.
30. Discuss how shielding effect impacts chemical reactivity.
31. Why does ionization energy increase significantly after removing one electron?
32. How is periodicity essential to predicting unknown elements?
33. Explain why metallic character decreases across a period.
34. Describe the relationship between electron affinity and reactivity.
35. Why do some elements have negative electron affinity?
36. Explain why noble gases have stable configurations.
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### **Long Questions (10 Questions)**
**Easy (3 Questions)**
1. Discuss the historical development of the periodic table and the main contributions of Dobereiner, Newlands, and Mendeleev.
2. Explain the periodic law, modern periodic law, and how it led to the creation of the modern periodic table.
3. Describe the main features of the modern periodic table, including periods and groups.
**Moderate (4 Questions)**
1. Explain the trends of atomic radius and ionization energy across a period and down a group with examples.
2. Describe the shielding effect and its impact on atomic size, ionization energy, and electron affinity.
3. Discuss the importance of electron affinity and electronegativity and how they change across periods and down groups.
4. Explain the factors that affect ionization energy in detail and describe its periodic trends with examples.
**Tough (3 Questions)**
1. Discuss the relationship between atomic radius, ionization energy, and reactivity across a period and down a group.
2. Explain the trends of electron affinity and electronegativity, providing examples to illustrate the variations within groups and periods.
3. Discuss the role of shielding effect and nuclear charge in determining the periodic trends of elements in the periodic table.