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| Chemistry 9th Chapter 3 Periodic Table and Periodicity of Properties Questions Bank |
Chapter 3 Periodic Table and Periodicity of Properties MCQs Questions Bank
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1. ______ period is the shortest period of long form of periodic table.
2. 17th group elements are known as:
3. 17th group elements contain electrons in their outer most shell:
4. 4th and 5th periods of the long form of periodic table are called
5. Actinides belong to period:
6. All transition elements are:
7. All transition elements belong to:
8. Along the period, which one of the following decreases:
9. Atomic number of actinium is:
10. Atomic number of lanthanum is:
11. Atomic size of Lithium is:
12. Electronegativity of oxygen is:
13. Elements are arranged in order of:
14. Elements are classified into four blocks depending upon:
15. Elements of a period show properties:
16. Elements of groups 13 to 18 have their valence electrons in subshell:
17. Elements with atomic No.90 to 103 are called:
18. Elements with atomic No. 58 to 71 are called:
19. Fifth period of periodic table has _____ elements.
20. How many blocks are there in the modern periodic table?
21. How many electrons are present in the valence shell of group 1 elements?
22. How many elements are present in 1st period?
23. How many elements are present in 6th period?
24. How many elements are present in 7th period?
25. How many elements are present in each 2nd & 3rd period?
26. How many elements are present in each 4th & 5th period?
27. How many elements were present in Mendeleev’s periodic table?
28. How many groups are present in the modern periodic table?
29. How many periods are present in the modern periodic table?
30. Hydrogen is placed with _______ in the periodic table.
31. In modern periodic table the elements in a group do not have continuously increasing:
32. Ionization energy of sodium is:
33. Lanthanides belong to period:
34. Long form of periodic table consists of :
35. Modern periodic table is based upon:
36. Mark the incorrect statement about ionization energy:
37. Mendeleev’s Periodic Table was based upon the:
38. Moseley arranged the elements in his periodic table on the basis of:
39. Nobel gases are present in group:
40. Normal elements belong to:
41. Number of elements in each normal period are:
42. One atmospheric pressure is equal to how many Pascal:
43. Point out the incorrect statement about electron affinity:
44. Point out the incorrect statement about ionization energy.
45. Second and third periods are called:
46. The amount of energy given out when an electron is added to an atom is called:
47. The atomic mass of strontium element is:
48. The atomic number of ‘Argon’ is:
49. The atomic radii of elements in Periodic table:
50. The atomic radii of the elements in periodic table:
51. The concept of triads was presented by:
52. The d-block elements are called _____ elements.
53. The distance between the Nuclei of two carbon atoms in its elemental form is:
54. The distance between the nuclei of two carbon atoms is:
55. The electronegativity of carbon is:
56. The electronegativity of carbon is:
57. The electronic configuration of phosphorus is:
58. The elements of a group show properties:
59. The elements of group ______ are called s-block elements.
60. The elements of group 1 and 2 are placed in which block:
61. The elements of group 17 have the electronic configuration:
62. The elements of group 3 to 12 are called:
63. The first ionization energy of sodium atom is:
64. The group 1 and 2 and 13 to 17 contain the elements:
65. The horizontal lines present in the periodic table are called:
66. The ionization energy of alkali metals _____ from top to bottom in a group.
67. The ionization energy of elements increases from left to right in a period because:
68. The minimum amount of energy which is required to remove an electron from the gaseous state of an atom is called:
69. The property of an atom in a molecule to attract the shared pair of electrons towards itself is called:
70. The shielding effect across the period:
71. The shortest period of periodic table is:
72. The unit of ionization energy is:
73. The value of electronegativity of chlorine is:
74. The vertical columns present in the periodic table are called:
75. There are _____ elements in the second period of long form of periodic table.
76. Total number of elements in normal periods are:
77. Transition elements are:
78. Unit of atomic size is:
79. When an electron is added in the valence shell than:
80. When we move from left to right in a period, atomic number:
81. When we move from left to right in a period, atomic size:
82. When we move from left to right in a period, ionization energy:
83. When we move from left to right in a period, shielding effect:
84. When we move from top to bottom in a group, atomic size:
85. When we move from top to bottom in a group, shielding effect:
86. Which element is present in 2nd period?
87. Which of the following decreases along a period?
88. Which of the following elements is present in 1st period?
89. Which of the following elements is present in group I?
90. Which of the following has the highest electron affinity?
91. Which of the following obeys duplet rule?
92. Which one of the following halogen has highest electronegativity?
93. Which one of the following halogen has lowest electronegativity?
94. Which one of the following halogens has highest electronegativity?
95. Which one of the following halogens has lowest electronegativity?
96. Which period of the modern periodic table is considered as incomplete period?
97. Who arranged the elements in the groups of three?
98. Who determined the correct atomic masses of elements in 1860?
99. Who discovered atomic number?/ Who introduced the modern periodic table?
100. Who presented the law of octaves?
101. With the increase of atomic number, the number of electrons in an atom also:
Short Questions
1. Electronegativity value can predict the nature of a chemical bond. Comment.
2. Define shielding effect.
3. State the modern periodic law.
4. How many elements are there in first period? Mention their symbols.
5. State the trend of electronegativity in period and give reasoning.
6. Why does the size of atoms increase from top to bottom in a periodic table?
7. Why chlorine accept only one electron?
8. What is the reason of arranging the elements in a group?
9. What difference of electronegativity between bonding atoms results in formation of ionic bond and covalent bond?
10. Why is the second ionization energy of an element higher than the first one?
11. Define electron affinity.
12. Why the ionization energy of sodium is less than that of magnesium?
13. Why were the elements arranged in periodic table according to their atomic number?
14. Why electron affinity increases in a period and decreases in a group?
15. State any four properties of long form of periodic table.
16. What are periods and groups of periodic table?
17. Define electronegativity.
18. What is the difference between Mendeleev’s periodic table and modern periodic table?
19. Write down the names and symbols of alkali metals.
20. Define atomic radius.
21. Give the trend of atomic size in periodic table.
22. Describe the trend of ionization energy in periodic table.
23. Why elements are arranged in periodic table?
24. Write electronegativity of nitrogen and oxygen.
25. Which elements are called lanthanides and actinides?
26. Why are noble gases not reactive?
27. Why electron affinity increases decreases in a group?
28. Define ionization energy.
29. Why does ionization energy increases in a period from left to right?
30. How are elements arranged in modern periodic table?
31. Why does Cesium (atomic no.55) require little energy to release its one electron present in the outermost shell?
32. Which element has the highest electronegativity?
33. Why the trend of electron affinity and electronegativity is same in a period?
34. Why does the bigger size atoms have more shielding effect?
35. How does shielding effect decrease the forces of electrostatic attractions between nucleus and outer most electrons?
36. What is shielding effect?
37. Why is it difficult to remove an electron from halogens?
38. Why the ionization energy of sodium is less than that of magnesium?
39. What is the trend of ionization energy in a group?
40. Why the 2nd ionization energy of an elements is higher than first one?
41. Define ionization energy.
42. Why the size of atoms decreases in a period?
43. Define atomic radius? Write its units.
44. Define electronegativity. Write the electronegativity of Nitrogen and oxygen.
45. Why does electron affinity increase in a period?
46. Why does electron affinity decrease in a group?
47. What is the trend of electron affinity in groups and periods in the periodic table?
48. Define electron affinity. Write down its unit.
49. Give the trend of ionization energy in a period.
50. Why does ionization energy decrease from top to bottom in any group?
51. Why does atomic radius of elements increase down the group?
52. Write down the trends of atomic size in groups and periods in the periodic table.
53. Give the trend of ionization energy in periodic table.
54. Why does the size of atom not decrease regularly in a period?
55. Why does shielding effect of electrons make cation formation easy?
56. Why are noble gases not reactive?
57. Write down the names of elements of group 1 with their symbols?
58. Why the elements are called s or p block elements?
59. What do you mean by periodic function?
60. What is the reason of arranging elements in a group?
61. Why the improvement in Mendeleev's periodic table was made?
62. How many periods are considered normal periods?
63. How many elements are in 3rd period, write their names and symbols?
64. From which period actinides series starts?
65. From which element lanthanide series starts?
66. How many elements are placed in 4th period?
67. How many elements are in first period and what are their names and symbols?
68. In which pattern modern periodic table was arranged?
69. How the properties of elements repeat after regular intervals?
70. Why and how elements are arranged in 4th Period?
71. Write the names or symbols of any four elements of Nobel Gases.
72. Write down the names of any four elements of group 17.
73. What are the elements arranged in group 3 to 12 called?
74. Define actinides. To which period do they belong?
75. Define lanthanides. To which period do they belong?
76. Who were Alchemists?
77. Define transition elements.
78. Define normal or representative elements.
79. How are elements arranged into four blocks?
80. How many blocks are present in Modern Periodic table?
81. How many groups and periods are present in Modern periodic table?
82. What do you mean by group number and period number?
83. Write down significance of atomic number.
84. Describe Modern periodic law.
85. Define periodic table.
86. What do you mean by groups and periods in the Periodic Table?
87. What is the difference between Mendeleev’s periodic law and modern periodic law?
88. How is periodicity of properties dependent upon the number of protons in an atom?
89. Why and how elements are arranged in a period?
90. State Mendeleev's periodic law.
91. What do you mean by a group in a periodic table?
92. Who introduced the name Periodic Table?
93. How Newlands arranged the elements? Define law of octaves.
94. What was the contribution of Dobereiner towards classification of elements?
95. Write down drawbacks of Mendeleev’s periodic table.
96. Describe drawbacks of Newlands octaves.
Long Questions
1. Define atomic radius. Give its trends in periods and groups of periodic table.
2. Define electron affinity, why it increases in a period and decreases in a group in the Periodic Table.
3. Define groups and explain them in periodic table.
4. Define ionization. Explain its trend along the periodic table.
5. Define periods and explain all periods of periodic table.
6. Define shielding effect and describe its trend in groups and periods.
7. Describe the salient features of modern periodic table.
8. Describe the trends of electronegativity in a period and in a group.
9. Discuss in detail the periods in Periodic Table?
10. Discuss the important features of modern Periodic Table.
11. Explain the contributions of Mendeleev for the arrangement of elements in his Periodic Table.
12. Justify the statement, bigger size atoms have more shielding effect thus low ionization energy.
13. Show why in a 'period’ the size of an atom decreases if one moves from left to right.
14. What do you mean by blocks in a periodic table and why elements were placed in blocks?
15. What is ionization energy? Describe its trend in the Periodic Table?
16. Why and how elements are arranged in a Periodic Table?