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

1. The species can exist, but -type expansion is not expected for boron. The best reason is that boron

2. Down group , the reducing character generally increases because

3. The table compares oxide behaviour across a period.

The row that needs correction is

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

5. A third-period element such as sulfur can show higher covalency than oxygen in suitable compounds. The most suitable explanation is that sulfur

6. Group and group elements are placed in the -block because their valence-shell configurations are generally

7. A group element forms an oxide with oxygen in its usual oxidation state . The expected formula of the oxide is

8. A graph is described as follows.

The graph description is best interpreted as showing

9. In Newlands' arrangement, the word octave was used because the pattern was compared with

10. Select the pair that is matched with the correct role in periodic-table vocabulary.

11. The table gives valence-shell data for some representative elements.

The row that needs correction is

12. The statement “periodic properties repeat, so every repeated property value must be numerically identical” is

13. The correct order of atomic radii for the second-period elements , , , and is generally

14. The molecule is possible in the usual Class periodicity discussion, but is not similarly expected. This contrast mainly illustrates

15. Compare two neutral atoms: one has and electronic distribution , while the other has and distribution . Their related behaviour in modern classification is best linked to

16. The long-form modern periodic table contains

17. The change from to across period is best described as a movement from

18. The table connects periodic position with likely bonding character.

The row that needs correction is

19. Moving from left to right across a typical period, the broad change in element character is usually

20. Consider the statements below.
I. Mendeleev left gaps for undiscovered elements.
II. He predicted properties of elements such as eka-aluminium and eka-silicon.
III. He placed noble gases by removing all alkali metals.
IV. He used chemical properties to support placement decisions.
The supported statements are

21. A claim says, “The -block is written below the table because its elements do not follow atomic number order.” The best evaluation is that the claim is

22. A period element has oxide , hydride , and a common negative oxidation state in its hydride. The element most likely belongs to

23. The recurrence of after completion of an inert-gas configuration explains why elements such as , , and are placed together. The recurring feature is

24. The table compares possible bases for arranging elements. The row most closely matching Mendeleev's original classification is

25. Arrange the isoelectronic species , , , , and in decreasing ionic radius.

26. The table compares species with their electron counts.

The smallest species in the table is

27. The order of increasing reactivity among the alkali metals , , and is

28. The table gives four statements about -block elements. Select the statement that best fits the transition-element idea.

29. For a period inner-transition element, the subshell associated with the rule is

30. A halogen displacement record says that can oxidize to , but cannot oxidize to . This record supports the conclusion that

31. Consider the statements about representative elements.
I. Group elements generally have valence-shell configuration.
II. Group elements generally have valence-shell configuration.
III. Group elements generally have valence-shell configuration.
IV. Group elements always have , including helium.
The supported statements are

32. A simplified periodic-table layout is described as follows: seven horizontal rows are present, eighteen vertical columns are used, and two series are shown separately below the main body. This layout corresponds to

33. The passage below describes two elements.

The shared chemical tendency is best explained by

34. The row in the table that best represents a valid modern-periodic-law link is

35. A temporary systematic name begins with roots corresponding to the digits , , and . Using the roots and , the root sequence is

36. Consider the statements about blocks.
I. -block elements generally belong to groups and .
II. -block elements generally occupy groups to .
III. -block elements are associated with groups to .
IV. -block elements are the same as the halogen family.
The supported statements are

37. Group elements are often discussed with possible oxidation states and . The reason this group can show both signs in simple periodic discussion is that its atoms have

38. 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

39. 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.

40. Consider the statements about electronegativity.
I. It is the tendency of a bonded atom to attract the shared electron pair.
II. It is dimensionless on the Pauling scale.
III. It generally increases down a group.
IV. It can help predict bond polarity.
The supported statements are

41. The row in the table that needs correction is

42. Assertion: The maximum covalency of oxygen is lower than that of sulfur in common basic-level periodicity discussions.
Reason: Oxygen is a second-period element without valence -orbitals, while sulfur is a third-period element.

43. The highest first ionization enthalpy in a period is generally shown by a noble gas because it has

44. A periodic-property graph has radius maxima at group positions and ionization-enthalpy maxima near group positions. The two maxima appear in different places because

45. The vertical set containing elements such as , , and is best described as a

46. Assertion: Noble gases are often excluded or treated specially in electronegativity comparisons.
Reason: Electronegativity is defined for atoms in bonds, and noble gases form few ordinary bonds under normal conditions.

47. The row with the correct radius description is

48. A periodic-table note gives these formula patterns: group , ; group , ; group , . The decrease in the number of hydrogen atoms from group to group is mainly due to

49. A simple symbolic way to express effective nuclear charge is , where represents shielding. If two atoms have the same but one has greater shielding, its will be

50. The oxide is best described as