PERIODIC TABLE & PROPERTIES OF ELEMENTS SOLVED MCQs

Periodic Table in Chemistry and Its Properties

1. Who is credited with the creation of the periodic table?

a. Dmitri Mendeleev

b. Antoine Lavoisier

c. Marie Curie

d. Robert Boyle

2. How are elements arranged on the modern periodic table?

a. Alphabetically

b. By atomic mass

c. By atomic number

d. Randomly

3. Which group of elements is known for their high reactivity and tendency to lose electrons?

a. Noble Gases

b. Alkali Metals

c. Halogens

d. Transition Metals

4. How many elements are there in the modern periodic table?

a. 92

b. 108

c. 118

d. 120

5. Which of the following elements is a metalloid?

a. Sodium

b. Silicon

c. Fluorine

d. Iodine

6. In which period do transition elements mostly appear?

a. 2nd period

b. 3rd period

c. 4th period

d. 5th period

7. Which group of elements is characterized by their low reactivity and full outer electron shells?

a. Alkali Metals

b. Noble Gases

c. Halogens

d. Transition Metals

8. What is the primary characteristic of transition elements?

a. High reactivity

b. Multiple oxidation states

c. Non-metallic properties

d. Low melting points

9. Which of the following is a non-metal?

a. Iron

b. Oxygen

c. Sodium

d. Calcium

10. How many metalloids are generally recognized in the periodic table?

a. 5

b. 7

c. 8

d. 10

11. What is the atomic number of carbon?

a. 6

b. 12

c. 14

d. 16

12. Which of the following elements is a noble gas?

a. Oxygen

b. Helium

c. Sodium

d. Chlorine

13. What is the symbol for gold?

a. Au

b. Ag

c. Fe

d. Pb

14. How many electrons does an oxygen atom have?

a. 6

b. 8

c. 16

d. 18

15. Which group does helium belong to in the periodic table?

a. Alkali metals

b. Noble gases

c. Halogens

d. Transition metals

16. What is the atomic mass of hydrogen?

a. 1

b. 2

c. 3

d. 4

17. Which period is potassium (K) located in?

a. 1st period

b. 2nd period

c. 3rd period

d. 4th period

18. What is the most abundant element in the Earth's crust?

a. Oxygen

b. Silicon

c. Carbon

d. Aluminum

19. What is the chemical symbol for lead?

a. Pd

b. Pb

c. Pt

d. Li

20. How many elements are in the first period of the periodic table?

a. 2

b. 4

c. 6

d. 8

21. What is the period number of an element located in Group 17 of the periodic table?

a. 1

b. 2

c. 3

d. 4

22. Elements in the same period of the periodic table have the same number of:

a. Protons

b. Neutrons

c. Electrons

d. Isotopes

23. Which period of the periodic table contains the most elements?

a. 1

b. 2

c. 3

d. 4

24. The number of valence electrons in an element from period 3 is:

a. 2

b. 5

c. 8

d. 18

25. As you move from left to right across a period, the atomic size generally:

a. Increases

b. Decreases

c. Remains constant

d. Becomes unpredictable

26. Which element in period 7 has the highest atomic number?

a. Francium (Fr)

b. Uranium (U)

c. Osmium (Os)

d. Hassium (Hs)

27. The element located at the beginning of a period typically has the lowest:

a. Atomic number

b. Atomic mass

c. Electronegativity

d. Ionization energy

28. In which period does the transition metals block appear?

a. 2

b. 3

c. 4

d. 5

29. Elements in the same period share similarities in their:

a. Chemical properties

b. Physical states

c. Radioactive decay

d. Half-life

30. The period number of an element can be determined by its:

a. Atomic number

b. Atomic mass

c. Number of isotopes

d. Electronegativity

31. Which of the following factors generally increases ionization energy across a period in the periodic table?

a) Atomic radius

b) Nuclear charge

c) Electron shielding

d) All of the above

32. In which group of the periodic table do elements typically have the lowest ionization energy?

a) Alkali metals

b) Halogens

c) Noble gases

d) Transition metals

33. What happens to ionization energy as you move from left to right across a period?

a) It increases

b) It decreases

c) It remains constant

d) It fluctuates

34. Which of the following elements is likely to have the highest ionization energy?

a) Sodium (Na)

b) Phosphorus (P)

c) Chlorine (Cl)

d) Aluminum (Al)

35. What is the relationship between ionization energy and atomic size?

a) Inversely proportional

b) Directly proportional

c) No correlation

d) Exponential

36. What is electron affinity?

a) The ability of an atom to lose electrons

b) The energy released when an electron is added to a neutral atom

c) The tendency of an atom to gain protons

d) The ability of an atom to form bonds

37. Which group of elements generally has the highest electron affinity?

a) Alkali metals

b) Noble gases

c) Halogens

d) Alkaline earth metals

38. What happens to electron affinity as you move across a period from left to right in the periodic table?

a) Increases

b) Decreases

c) Remains constant

d) Varies unpredictably

39. Which element has the highest electron affinity among the following?

a) Oxygen

b) Fluorine

c) Nitrogen

d) Carbon

40. True or False: Noble gases generally have positive electron affinities.

a. False

b. True

41. Which factor contributes to the increase in electron affinity across a period?

a) Increased atomic size

b) Decreased nuclear charge

c) Increased effective nuclear charge

d) Enhanced metallic character

42. Which element is likely to have the least negative electron affinity?

a) Chlorine

b) Oxygen

c) Neon

d) Sodium

43. What is electronegativity?

a. The ability of an atom to lose electrons

b. The ability of an atom to attract electrons

c. The ability of an atom to conduct electricity

d. The ability of an atom to gain protons

44. Which element has the highest electronegativity?

a. Sodium (Na)

b. Fluorine (F)

c. Carbon (C)

d. Potassium (K)

45. How does electronegativity change across a period in the periodic table?

a. It increases

b. It decreases

c. It remains constant

d. It fluctuates randomly

46. Which group of elements generally has higher electronegativity?

a. Alkali metals

b. Halogens

c. Noble gases

d. Transition metals

47. In the periodic table, electronegativity generally decreases down a group. What is the primary reason for this trend?

a. Increased atomic size

b. Decreased atomic size

c. Increased number of protons

d. Decreased number of protons

48. What is the shielding effect in the periodic table?

a. The ability of an atom's outer electrons to shield its nucleus from the influence of nearby atoms.

b. The tendency of electrons to repel each other in the same energy level.

c. The shielding of the nucleus from external magnetic fields.

d. All of them

49. Which factor contributes to increased shielding effect in an atom?

a. Increased nuclear charge.

b. Increased distance from the nucleus.

c. Increased number of electrons in inner energy levels.

d. None of them

50. How does the shielding effect influence atomic size?

a. Higher shielding leads to larger atomic size.

b. Higher shielding leads to smaller atomic size.

c. Shielding has no effect on atomic size.

d. All of them

51. In a period (row) of the periodic table, how does the shielding effect change?

a. It increases.

b. It decreases.

c. It remains constant.

d. None of them

52. Which element in a group (column) of the periodic table has the highest shielding effect?

a. The topmost element.

b. The middle element.

c. The bottommost element.

d. All of them

Further Chemistry Related Solved MCQs as Suggestrd Reading

Chemistry & its Branches Solved MCQs

Fundamentals of Chemistry Solved MCQs

Fundamentals of Chemistry Short Notes

Matter in Chemistry Solved MCQs

Chemical Bonding Solved MCQs

Acids, Bases & Salts Solved MCQs

General Chemistry Solved MCQs

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