Classification of Elements and Periodicity in Properties Mock Test – Class 11 Chemistry

1. The oxidizing power of halogens generally follows the order

2. The sequence in the long-form table represents the

3. The row in the table that needs correction is

4. A statement says, “Because fluorine is the most electronegative element, it should show positive oxidation states with oxygen.” The best correction is that fluorine

5. The statement “classification only reduces memory load; it does not help in prediction” is best evaluated as

6. Consider the statements about oxidation state and ion charge.
I. Oxidation state may equal ion charge in simple ionic compounds.
II. Oxidation state is always the actual charge on an atom in every covalent molecule.
III. Fluorine is assigned in its compounds.
IV. Noble gases are usually assigned in the elementary periodic discussion.
The supported statements are

7. Consider the two configuration patterns below.
Case 1:
Case 2:
The most suitable comparison is

8. A configuration ending in is associated with an element from the inner-transition region. The block classification is mainly connected with filling of the

9. Use the arrangement described below: Element boxes are placed in rows and columns. Moving left to right along a row increases stepwise, while moving downward in one column keeps elements in the same family. This description identifies

10. Group elements commonly show oxidation state because their valence-shell configuration is generally

11. A student compares , , and and expects a perfectly smooth increase in first ionization enthalpy. The best correction is that

12. For -block elements, the maximum positive oxidation state is often related to

13. A period element has configuration ending . Its classification is best described as

14. Down a group, electron gain enthalpy generally becomes less negative because

15. Metalloids are commonly found along the zig-zag boundary between metals and non-metals. A suitable example set is

16. A short note says: “Element belongs to group . It forms a hydride and an oxide in which can show .” The note most strongly illustrates that

17. The oxide is best described as

18. A set of elements forms oxides with similar formula patterns and also shows related chemical behaviour. In Mendeleev's classification, this evidence would mainly support

19. A metal has successive ionization enthalpies in the pattern: is low, is much higher, and later values are still higher. This pattern most strongly suggests that the atom has

20. A table contains four statements about Mendeleev's merits. Identify the statement that does not represent a merit.

21. The best combined statement about electron gain enthalpy is that it

22. A group element forms a simple hydride with hydrogen as . The formula that satisfies charge balance is

23. Assertion: is smaller than , although both have electrons.
Reason: has a greater nuclear charge than , so it pulls the same number of electrons more strongly.

24. An element has valence-shell configuration . For a representative element, its group and period are respectively

25. The best reason Mendeleev's table was called a natural classification is that it

26. In the modern periodic table, the period number of an element is related to the

27. The anomalous behaviour of many second-period elements compared with heavier members of their groups is mainly due to their

28. For many non-metal atoms, the first electron gain enthalpy is negative because

29. A neutral element has the outer electronic pattern . Its block is

30. Nitrogen has a much less negative first electron gain enthalpy than expected for its position because nitrogen has

31. An element forms the oxide , and oxygen has oxidation state . The oxidation state of is

32. A set of elements contains , , , , , and . A meaningful first grouping would place

33. A claim says, “The absence of -orbitals in period elements only affects rare compounds and has no link with periodic behaviour.” The best evaluation is that the claim is

34. The row that best distinguishes a periodic pattern from a non-periodic listing is

35. For noble gases, first electron gain enthalpy is positive or unfavourable mainly because the incoming electron must enter

36. Valency is best described as the

37. The best comparison of electronegativity and metallic character across a period is that

38. A passage from a historical classification note says that some elements were placed below chemically similar elements even when strict atomic-mass order became slightly disturbed.

This note most strongly reflects

39. A record of period lengths is given below.

The row that needs correction is

40. The strong metallic character of -block elements is closely related to their

41. The best statement about oxidation states across the representative -block is that

42. A representative -block element has the valence-shell configuration . This pattern is characteristic of

43. A student checks , , and as a triad using approximate atomic masses , , and . The best interpretation is

44. The table gives descriptions of periodic-table regions.

The row that needs correction is

45. Use the following arrangement for main-group elements across a period.

The position expected to have simple valency because it needs two electrons to complete an octet is

46. The row that contains a mismatched family name is

47. A claim states, “All elements with must be placed in group .” The claim fails for

48. For a representative element with outer configuration , the most suitable group placement is

49. A claim says, “Down a group, the increasing nuclear charge should always make atoms smaller.” The best correction is that

50. Use the arrangement described below: period begins with filling , continues through , and ends with . The maximum number of elements in this period is