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

1. The row in the table that needs correction is

2. A graph of first ionization enthalpy against atomic number shows low points near alkali metals and high points near noble gases. This pattern occurs because

3. The anomalous order - in Mendeleev's table is best understood as a case where

4. A predicted element is placed below silicon in Mendeleev's table and is expected to form an oxide similar in type to silicon oxide. This reasoning uses

5. A student says, “Electronegativity is just electron gain enthalpy with a different name.” The best correction is that electronegativity is

6. Mendeleev could correct some doubtful atomic masses because

7. A graph is described below.

The downward slope is best explained by

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

9. A claim says, “Diagonal relationship is just the same as group similarity.” The best correction is that diagonal relationship

10. A proposed group of three elements satisfies the arithmetic mean relation exactly, but the three elements have very different chemical properties. For Dobereiner's triad idea, this group should be

11. The usual unit used for molar ionization enthalpy is

12. A graph of first electron gain enthalpy across a period is described below.

The sharp rise for the noble gas is best explained by

13. In the long-form periodic table, the -block begins after the -block in a period and generally covers

14. 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

15. A short passage describes an element family.

This family is

16. An element has the configuration ending . The safest block assignment is

17. The row with the most suitable -block family identification is

18. A graph compares two properties across period . Curve decreases from to , while curve increases over the same range. The most suitable pair is

19. Arrange the halogens , , , and in decreasing electronegativity.

20. The statement “same group means same valence-shell pattern” is most reliable for

21. 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.

22. A graph is described below.

For the same movement down the group, the metallic reactivity curve would generally

23. A period inner-transition series is mainly associated with filling of the

24. When a period element forms strong multiple bonds with another small atom, while its heavier group member forms weaker multiple bonds less readily, the difference is mainly due to

25. A neutral atom has the shell distribution . The period number and valence-electron count are respectively

26. A period contains a left-side metal, a middle boundary element, and an upper-right non-metal. The middle boundary element is most likely to show

27. Across a period from left to right, first ionization enthalpy generally increases because

28. Periodicity in properties means that

29. An unfamiliar element is placed below a known element in the same group. The most reasonable first prediction is that the unfamiliar element will

30. The modern IUPAC group numbering system labels the vertical columns of the periodic table as

31. Select the option that gives a valid example of a Dobereiner triad.

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

33. Moving from to across period , the broad change in character is

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

35. The most suitable order of acidic character among the period oxides listed is

36. A bond between two elements changes from mostly ionic to more covalent as the electronegativity difference between the bonded atoms

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

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

39. The notation in the general -block configuration means that for a period transition element, the subshell involved is

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

41. Down group , metallic character generally increases because

42. Coloured ions and catalytic behaviour are often associated with transition elements. At the Class classification level, these features are introduced as consequences linked with

43. The most complete reasoning chain for predicting that is acidic rather than basic is

44. The pair of general formulae and for a group of elements would suggest, in Mendeleev's style of reasoning, that the elements commonly show

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

46. Consider the statements about periodic properties.
I. Periodic properties show regular trends when elements are arranged by increasing .
II. Periodicity is mainly related to recurring valence-shell configurations.
III. Periodic properties imply that all elements in a group have exactly the same size.
IV. Atomic size, ionization enthalpy, and electronegativity can show periodic trends.
The supported statements are

47. Match the terms in Column I with their correct meanings in Column II.

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

49. Newlands arranged elements in increasing order of atomic mass and observed that the properties of every eighth element were similar to those of the first. This observation is known as

50. The row that contains a mismatched common oxidation-state idea is