Exam-Style Mock Test | Chapter: Classification Of Elements

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Quiz: Classification of Elements and Periodicity in Properties – Progressive Test
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1 / 50

1. Assertion: Actinoids are generally treated with awareness that many of them are radioactive.
Reason: Actinoids belong to the period inner-transition series associated mainly with filling.

a) Assertion is true, but Reason is false

b) Both Assertion and Reason are true, but Reason does not explain Assertion

c) Assertion is false, but Reason is true

d) Both Assertion and Reason are true, and Reason explains Assertion

2 / 50

2. The main reason for classifying elements is to make the study of elements more systematic by grouping them according to similarities and trends. What does this achieve most directly?

a) It helps compare elements and predict properties more easily

b) It removes the need to know any chemical properties

c) It makes all elements show identical behaviour

d) It arranges elements only in alphabetical order

3 / 50

3. 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

a) I, II, III, and IV

b) II and IV only

c) I, II, and III only

d) I and IV only

4 / 50

4. A compound is an acidic oxide, and oxygen is assigned oxidation state . The oxidation state of is

5 / 50

5. The high reactivity of alkali metals is best connected with their

a) strong tendency to gain seven electrons

b) complete valence-shell configuration

c) low first ionization enthalpy and easy loss of the outer electron

d) high first ionization enthalpy and strong attraction for valence electrons

6 / 50

6. 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

a) rows as blocks and columns as atomic numbers

b) rows as periods and columns as groups

c) rows as groups and columns as periods

d) rows as atomic masses and columns as symbols

7 / 50

7. A claim states, “Second-period elements cannot show group similarity because they behave anomalously.” The best evaluation is that the claim is

a) correct, because second-period elements have no valence electrons

b) too extreme, because they show group similarity but may differ in specific properties due to small size and absence of -orbitals

c) correct, because group number has no relation to valence configuration

d) too extreme only because all second-period elements are metals

8 / 50

8. Mendeleev's approach was stronger than a simple increasing-mass list because it

a) arranged elements only by their physical states

b) ignored chemical properties to keep the numbers neat

c) removed the idea of families from classification

d) used property patterns to judge the most suitable positions

9 / 50

9. Match the cause in Column I with the consequence in Column II.

Column I	Column II
P. Small atomic size	1. Stronger polarizing power or high charge density in some cases
Q. High electronegativity	2. Stronger attraction for bonding electrons
R. Absence of -orbitals	3. Restricted expansion of covalency
S. Similar diagonal charge/radius ratio	4. Partial similarity between diagonal pairs

a) P-1, Q-3, R-2, S-4

b) P-2, Q-1, R-3, S-4

c) P-1, Q-2, R-3, S-4

d) P-4, Q-2, R-1, S-3

10 / 50

10. A data card for magnesium gives the symbol , atomic number , and atomic mass about . For placing magnesium in the modern periodic table, the most fundamental entry is

b) the English name magnesium

c) the two-letter symbol

11 / 50

11. In the modern view, is placed before because

a) and are isotopes

b) has no electrons

c) has atomic number and has atomic number

d) has a smaller atomic mass than

12 / 50

12. The table shows some claims about Newlands' law of octaves. Identify the row that needs correction.

Row	Claim
P	Elements were arranged in increasing order of atomic mass.
Q	Every eighth element was expected to show similarity with the first.
R	The law worked well for all elements including very heavy elements.
S	The law used an analogy with musical notes.

a) Row S

b) Row R

c) Row Q

d) Row P

13 / 50

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

a) has no valence electrons

b) is smaller and more electronegative than oxygen

c) belongs to period , where -orbital involvement is possible in elementary bonding descriptions

d) has fewer shells than oxygen

14 / 50

14. A pair of isotopes has the same but different mass numbers. The modern periodic law places them in the same position because

a) their atomic numbers and ordinary electronic configurations are the same

b) their atomic masses are exactly equal

c) isotopes are always placed in different groups

d) neutron number decides group number directly

15 / 50

15. 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.

a) Assertion is false, but Reason is true

b) Both Assertion and Reason are true, but Reason does not explain Assertion

c) Both Assertion and Reason are true, and Reason explains Assertion

d) Assertion is true, but Reason is false

16 / 50

16. A period oxide sequence is written as , , , , , , and . The general change in acidic character along this sequence is

a) decreases from left to right

b) remains exactly zero for every oxide

c) increases from left to right

d) changes only with atomic mass and not with element character

17 / 50

17. A group of representative elements forms hydrides of the type and oxides of the type . This formula pattern most strongly suggests that the elements belong to

a) group

b) group

c) group

d) group

18 / 50

18. For a neutral atom with atomic number , this number is central to periodic classification because it fixes

a) the physical state of the element under all conditions

b) the average atomic mass exactly

c) only the number of neutrons

d) the number of protons and, for the neutral atom, the number of electrons

19 / 50

19. Consider the statements about metals, non-metals, and metalloids in the periodic table.
I. Metals occupy much of the left and central part of the table.
II. Non-metals are concentrated mainly toward the upper right.
III. Metalloids commonly lie along a zig-zag boundary.
IV. All elements in the -block are metals.
The supported statements are

a) I, II, III, and IV

b) II and IV only

c) I, II, and III only

d) I and IV only

20 / 50

20. The oxide is best described as

a) amphoteric

b) a noble gas oxide with no acid-base behaviour

c) strongly acidic only

d) strongly basic only

21 / 50

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

Row	Periodic situation	Likely bonding tendency
P	Group metal with group non-metal	High ionic character
Q	Two similar non-metals from the right side	Covalent character
R	Large electronegativity difference	High ionic character
S	Very small electronegativity difference	Compulsory full ionic transfer in every case

The row that needs correction is

a) Row R

b) Row S

c) Row P

d) Row Q

22 / 50

22. A mixed trend comparison gives four statements.
I. is larger than .
II. has higher first ionization enthalpy than .
III. is more electronegative than .
IV. is more strongly basic than .
The supported statements are

a) I, II, III, and IV

b) I and IV only

c) I, II, and III only

d) II and IV only

23 / 50

23. A graph is described as follows.

The x-axis shows increasing atomic number . The y-axis shows a property that rises and falls in a repeating pattern as new periods begin and end.

The graph description is best interpreted as showing

a) random variation unrelated to classification

b) equality of atomic masses in each group

c) a fixed value of every chemical property

d) periodic variation of a property with atomic number

24 / 50

24. Consider the statements about Newlands' law of octaves.
I. It used increasing atomic mass as the arranging basis.
II. It succeeded mainly for lighter elements.
III. It deliberately left gaps for undiscovered elements and predicted their properties.
IV. It sometimes placed dissimilar elements together.
The supported statements are

a) I, II, III, and IV

b) II and III only

c) I and III only

d) I, II, and IV only

25 / 50

25. The row that best explains why carbon commonly forms strong multiple bonds compared with silicon is

Row	Explanation
P	Carbon has compact -orbitals that overlap effectively.
Q	Carbon has -orbitals available for multiple bonding.
R	Silicon and carbon have identical atomic sizes.
S	Silicon has no valence-shell orbitals.

a) Row P

b) Row R

c) Row S

d) Row Q

26 / 50

26. A data set shows that atomic radius generally decreases from to , then becomes large again at . This pattern is best described as

a) alphabetical variation with element name

b) periodic variation with atomic number

c) random variation with no chemical meaning

d) isotope variation within one element

27 / 50

27. The family name chalcogens is commonly associated with

a) group

b) group

c) group

d) group

28 / 50

28. A configuration note mentions filling along with outer electrons. The safest classification is

a) -block representative element

b) -block transition element

c) -block inner-transition element

d) -block representative element

29 / 50

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

a) the lowest effective nuclear charge in the period

b) a closed valence shell and small size at the end of the period

c) only one loosely held -electron

d) no electrons around the nucleus

30 / 50

30. A note says: “The unknown element below boron should resemble boron in some group properties but should not be identical to boron.” This statement is chemically sound because elements in a group

a) cannot be used for predicting unknown elements

b) always have the same atomic mass

c) must have identical physical and chemical properties

d) share related valence behaviour but differ in size and other properties

31 / 50

31. Match the period with its usual number of elements in the long-form periodic table.

Column I	Column II
P. Period	1.
Q. Period	2.
R. Period	3.
S. Period	4.

a) P-4, Q-2, R-3, S-1

b) P-1, Q-2, R-3, S-4

c) P-2, Q-1, R-3, S-4

d) P-1, Q-3, R-2, S-4

32 / 50

32. A compact family-description card says: “Group elements generally form ions; group elements commonly form ions.” The difference is mainly due to

a) group having one valence electron and group having seven valence electrons

b) group being part of the -block

c) both groups having identical valence-shell configurations

d) group having a complete octet in the neutral atom

33 / 50

33. The table gives successive ionization enthalpies for three elements in arbitrary units.

Element
P
Q
R

The element most likely having two valence electrons is

a) P and R only

b) R

c) P

d) Q

34 / 50

34. Diagonal relationship refers to similarity between certain elements that are

a) in the same isotope series

b) always in the same vertical group only

c) diagonally adjacent in the periodic table, especially between period and period

d) arranged alphabetically beside each other

35 / 50

35. The row with the most suitable block assignment is

Row	Configuration ending	Assigned block
P		-block
Q		-block
R		-block
S		-block

a) Row R

b) Row P

c) Row Q

d) Row S

36 / 50

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

a) period

b) period

c) period

d) period

37 / 50

37. For the configuration , the claim “it is in group because the shell number is ” is best evaluated as

a) weak only because krypton has no electrons

b) strong, because period number and group number are always identical

c) strong, because all atoms are noble gases

d) weak, because gives the period while gives group

38 / 50

38. Assertion: Elements with valence-shell configurations and are placed in the same group.
Reason: Both have the same highest principal quantum number .

a) Both Assertion and Reason are true, but Reason does not explain Assertion

b) Assertion is true, but Reason is false

c) Both Assertion and Reason are true, and Reason explains Assertion

d) Assertion is false, but Reason is true

39 / 50

39. A record of period lengths is given below.

Period	Number of elements
P	First period:
Q	Second period:
R	Third period:
S	Fourth period:

The row that needs correction is

a) Row S

b) Row P

c) Row R

d) Row Q

40 / 50

40. 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

a) I, II, III, and IV

b) I and III only

c) II and III only

d) I, II, and IV only

41 / 50

41. The oxidation state of phosphorus in , taking chlorine as , is

42 / 50

42. 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.

a) Assertion is false, but Reason is true

b) Both Assertion and Reason are true, but Reason does not explain Assertion

c) Both Assertion and Reason are true, and Reason explains Assertion

d) Assertion is true, but Reason is false

43 / 50

43. A graph is described below.

On the x-axis, elements are arranged in increasing atomic number. The y-axis shows a property that decreases across one period, then rises sharply at the beginning of the next period, and again decreases across that period.

This graph most likely represents a periodic trend because

a) the graph proves that atomic number is unrelated to properties

b) the x-axis should have been alphabetical order

c) the property has the same value for all elements

d) the property repeats a pattern after a new shell begins

44 / 50

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

a) -block, because is written at the end

b) -block, because -subshell elements are always inner transition elements

c) -block, because all elements after group are -block

d) -block, because the differentiating electron belongs to a subshell

45 / 50

45. Consider the statements about hydrides and oxides as periodic indicators.
I. Hydride formulae can reflect valency patterns.
II. Oxide formulae can help infer oxidation state.
III. Similar oxide and hydride formulae were useful in Mendeleev's grouping.
IV. Hydride formulae always prove that two elements are isotopes.
The supported statements are

a) I and IV only

b) I, II, and III only

c) II and IV only

d) I, II, III, and IV

46 / 50

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

Row	Valence-shell configuration	Family or group idea
P		group , halogen family
Q		group , halogen family
R		group , boron family
S		group , noble gases

a) Row Q

b) Row R

c) Row P

d) Row S

47 / 50

47. A limitation of Newlands' law becomes clear when it is applied to elements heavier than calcium because

a) the octave pattern no longer works regularly

b) atomic mass stops increasing after

c) every heavier element forms a Dobereiner triad

d) all heavier elements become noble gases

48 / 50

48. 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

a) four valence electrons and can be considered from electron-sharing or electron-accounting viewpoints

b) no valence electrons

c) a complete shell in every neutral atom

d) the same atomic mass as noble gases

49 / 50

49. 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

a) arranging them only by the length of their names

b) separating them because similar formulae are irrelevant

c) assigning them all the same atomic mass

d) placing the elements in the same chemical family

50 / 50

50. Use the short passage below.

Element is very small, has no available -orbitals in its valence shell, and forms compounds in which its covalency does not exceed . Its heavier group member can form compounds with higher covalency under suitable conditions.

The most suitable inference is that is likely a

a) period inner-transition element

b) group noble gas only

c) period transition metal

d) second-period element

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