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

1. The process representing first ionization enthalpy is

2. Use the simplified sequence below in the spirit of Newlands' law of octaves.

If is taken as position , the element expected to resemble it by this counting rule would be at

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

4. Read the case below and answer the question.

This case best illustrates Mendeleev's

5. The strongest overall evaluation of Dobereiner's triads is that they

6. Consider the statements about common group names.
I. Group is called the boron family.
II. Group is called the carbon family.
III. Group is called the halogen family.
IV. Group is called the alkaline earth metal family.
The supported statements are

7. Use the family map below.

A member of the nitrogen family is expected to have the valence pattern

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

9. Rare earth elements were difficult to place in Mendeleev's table mainly because

10. The table gives oxide-character assignments.

The row that needs correction is

11. A compound has formula , and hydrogen is assigned when bonded to a non-metal. The oxidation state of is

12. A configuration ends in . Without identifying the element by name, its period can be determined as

13. First ionization enthalpy of an element is the enthalpy change required to remove

14. Down a group, atomic size generally increases even though nuclear charge increases. The main reason is that

15. The usual unit used for molar ionization enthalpy is

16. The second ionization enthalpy of sodium is much larger than its first ionization enthalpy because after the first ionization sodium has

17. 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

18. Down a group, electronegativity generally decreases because

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

20. The maximum covalency of second-period elements is limited to mainly because they have

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

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

23. The older group notation is less preferred in modern use mainly because

24. The following graph is described for elements of one period.

The best interpretation of this graph is that

25. Helium is placed in group even though its electronic configuration is , not . The best reason is that helium

26. The table gives qualitative data for halogens.

The row-wise trend is best explained by

27. Chlorine has a more negative first electron gain enthalpy than fluorine because

28. Consider the statements about Mendeleev's table.
I. It arranged elements mainly according to increasing atomic mass.
II. It used chemical properties such as oxide and hydride formulae.
III. It had no ability to predict undiscovered elements.
IV. It helped form natural families of elements.
The supported statements are

29. Consider the statements about Moseley's contribution.
I. It supported atomic number as the fundamental basis of classification.
II. It helped explain anomalous pairs such as -.
III. It showed that atomic mass and atomic number are always identical.
IV. It linked periodic order with nuclear charge.
The supported statements are

30. A short note says: “Element lies near the left side of a period, while element lies near the right side before the noble gas. In a bond, pulls the shared electron pair more strongly.” The note is mainly using

31. Consider the statements below.
I. Elements in the same period must have identical chemical properties.
II. Elements in the same group often have similar valence-shell patterns.
III. The periodic table is only a storage chart and cannot help predict properties.
The supported statement set is

32. A neutral atom has the electronic distribution . Its period number is

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

34. A graph is described below.

This graph most likely represents a periodic trend because

35. Which description gives the meaning of atomic number ?

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

37. A claim says, “Valency and number of valence electrons are always identical.” The best evaluation is that the claim is

38. A final synthesis card lists these clues for an unknown neutral element: , oxide formula , amphoteric oxide behaviour, and valence-shell configuration ending in . The element is best placed as

39. A molecule has a bond between and . Chlorine is more electronegative than hydrogen. The bond polarity is best described as

40. Electron gain enthalpy is the enthalpy change when

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

42. has greater first ionization enthalpy than , even though is to the right of . The best explanation is that the electron removed from is from

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

44. Valency is best described as the

45. The table shows hydride formula patterns for representative groups. Select the row that needs correction.

46. In the long-form periodic table, atomic number generally increases

47. A record of period lengths is given below.

The row that needs correction is

48. A claim states, “A negative ion is always smaller than a positive ion because the negative sign pulls electrons inward.” The best correction is that

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

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