Chemistry Objective Questions and Answers: Classification Of Elements and Periodicity In Properties
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Multiple Choice Questions
(a) 50
(b) 46
(c) 64
(d) 36
Show Answer & Explanation
Answer: (b) 46
Explanation:
1. Difference = 2.0: 16 x 2 + 3.5 x 4 = 32 + 14 = 46 percent.
Teacher's Note:
1. Use Hannay-Smith's formula.
(a) Mn
(b) Sc
(c) Cr
(d) Ti
Show Answer & Explanation
Answer: (c) Cr
Explanation:
1. Cr+ is 3d5 (half-filled), so removing a 3d electron is difficult: IE2 of Cr = 1591 kJ/mol, the highest.
Teacher's Note:
1. Half-filled subshells are very stable.
(a) Al3+ < Mg2+ < Na+ < F- (increasing ionic size)
(b) B < C < N < O (increasing first ionisation energy)
(c) I < Br < F < Cl (increasing electron gain enthalpy, magnitude)
(d) Li < Na < K < Rb (increasing metallic radius)
Show Answer & Explanation
Answer: (b) B < C < N < O (increasing first ionisation energy)
Explanation:
1. IE1: B 801, C 1086, N 1402, O 1314: O is lower than N.
2. So the order B < C < N < O is incorrect.
Teacher's Note:
1. N has a stable half-filled 2p3.
(a) 4f4 5d4 6s2
(b) 4f7 5d1 6s2
(c) 4f3 5d5 6s2
(d) 4f8 5d0 6s2
Show Answer & Explanation
Answer: (b) 4f7 5d1 6s2
Explanation:
1. Gd uses the extra stability of half-filled 4f7: [Xe] 4f7 5d1 6s2.
Teacher's Note:
1. An exception to the aufbau order.
(a) I > Br > Cl > F
(b) F > Cl > Br > I
(c) Cl > F > Br > I
(d) Br > Cl > I > F
Show Answer & Explanation
Answer: (c) Cl > F > Br > I
Explanation:
1. Magnitudes: Cl 349, F 328, Br 325, I 295 kJ/mol.
Teacher's Note:
1. F is anomalous due to its small size.
(a) Al(OH)3, LiOH
(b) Be(OH)2, Mg(OH)2
(c) B(OH)3, Be(OH)2
(d) Be(OH)2, Zn(OH)2
Show Answer & Explanation
Answer: (d) Be(OH)2, Zn(OH)2
Explanation:
1. Be(OH)2 and Zn(OH)2 react with both acids and bases. LiOH and Mg(OH)2 are basic; B(OH)3 is acidic.
Teacher's Note:
1. Be-Al diagonal relationship.
(a) Electrons get repelled
(b) Electrons get attracted
(c) Gain of electrons
(d) Loss of protons
Show Answer & Explanation
Answer: (b) Electrons get attracted
Explanation:
1. It is the ability of an atom in a bond to attract the shared pair.
Teacher's Note:
1. It is not the same as electron affinity.
(a) Directly proportional to the square of effective nuclear charge
(b) Inversely proportional to effective nuclear charge
(c) Inversely proportional to the square of effective nuclear charge
(d) Directly proportional to effective nuclear charge
Show Answer & Explanation
Answer: (b) Inversely proportional to effective nuclear charge
Explanation:
1. For isoelectronic ions, radius is inversely proportional to effective nuclear charge.
Teacher's Note:
1. Greater Zeff pulls electrons in more.
(a) F < Cl < O < S
(b) S < O < Cl < F
(c) O < S < F < Cl
(d) Cl < F < S < O
Show Answer & Explanation
Answer: (c) O < S < F < Cl
Explanation:
1. Magnitudes: O 141 < S 200 < F 328 < Cl 349.
Teacher's Note:
1. Second period elements O and F fall below their congeners S and Cl.
(a) Elements having high IP also have high EA
(b) 2nd IP of noble gas is less than 1st IP
(c) IP of Be is more than B
(d) 2nd IP of N is more than 2nd IP of O
Show Answer & Explanation
Answer: (c) IP of Be is more than B
Explanation:
1. IE1: Be 899 > B 801.
2. (d): IE2 of O (3388) is higher than IE2 of N (2856), so (d) is wrong. Noble gases have IE2 greater than IE1.
Teacher's Note:
1. Be has the filled 2s2.
(a) Atomic radius: Li < Be < B
(b) Ionisation potential: Li < Be < B
(c) Electron affinity: Li < Be < B
(d) Electronegativity: Li < Be < B
Show Answer & Explanation
Answer: (d) Electronegativity: Li < Be < B
Explanation:
1. EN (Pauling): Li 1.0 < Be 1.5 < B 2.0.
2. Radius decreases and IE of Be is higher than B, EA of Be is lower than Li (near zero).
Teacher's Note:
1. Use data values for each property.
Assertion–Reason Questions
Assertion (A): The ionisation potential of F is greater than the electron affinity of F.
Reason (R): F is a highly electronegative element.
(a) Both A and R are true, and R is the correct explanation of A.
(b) Both A and R are true, but R is not the correct explanation of A.
(c) A is true, but R is false.
(d) A is false, but R is true.
Show Answer & Explanation
Answer: (b) Both A and R are true, but R is not the correct explanation of A.
Explanation:
1. IP(F) = 1681 kJ/mol and EA(F) = 328 kJ/mol, so A is true.
2. R is true, but electronegativity alone is not the reason for the IP-EA comparison (IP is always bigger than EA in magnitude).
Teacher's Note:
1. Compare numerical values first.
2. Do not link the statements by superficial similarity.
Assertion (A): The properties of beryllium are similar to those of aluminium.
Reason (R): Both elements belong to the same group.
(a) Both A and R are true, and R is the correct explanation of A.
(b) Both A and R are true, but R is not the correct explanation of A.
(c) A is true, but R is false.
(d) A is false, but R is true.
Show Answer & Explanation
Answer: (c) A is true, but R is false.
Explanation:
1. Be and Al show a diagonal relationship because of similar charge/size ratio, so A is true.
2. Be is in group 2 and Al in group 13: R is false.
Teacher's Note:
1. Diagonal pairs: Li-Mg, Be-Al, B-Si.
Assertion (A): The size of an anion is larger than its parent atom.
Reason (R): The effective nuclear charge (Zeff) of an anion is greater than that of its parent atom.
(a) Both A and R are true, and R is the correct explanation of A.
(b) Both A and R are true, but R is not the correct explanation of A.
(c) A is true, but R is false.
(d) A is false, but R is true.
Show Answer & Explanation
Answer: (c) A is true, but R is false.
Explanation:
1. Extra electrons repel each other and Zeff per electron decreases, so the anion is larger (A true).
2. R is false: the Zeff of an anion is smaller than that of its parent atom.
Teacher's Note:
1. Same nuclear charge, more electrons.
Assertion (A): A stable electronic configuration does not affect electronegativity.
Reason (R): Electronegativity is the tendency of an atom to attract shared electrons, not to gain electrons.
(a) Both A and R are true, and R is the correct explanation of A.
(b) Both A and R are true, but R is not the correct explanation of A.
(c) A is true, but R is false.
(d) A is false, but R is true.
Show Answer & Explanation
Answer: (a) Both A and R are true, and R is the correct explanation of A.
Explanation:
1. EN is about shared pairs in a bond, not about electron gain, so the stability of the isolated atom (as in EA) does not matter.
2. R explains A.
Teacher's Note:
1. EA depends on stability of the configuration; EN does not.
Assertion (A): The atomic radii of inert gases are the largest in their period.
Reason (R): The effective nuclear charge of inert gases is minimum.
(a) Both A and R are true, and R is the correct explanation of A.
(b) Both A and R are true, but R is not the correct explanation of A.
(c) A is true, but R is false.
(d) A is false, but R is true.
Show Answer & Explanation
Answer: (c) A is true, but R is false.
Explanation:
1. Noble gas radii are van der Waals radii and are larger than covalent radii of neighbours, so A is accepted as true.
2. R is false: Zeff of the noble gas is maximum in its period.
Teacher's Note:
1. Do not confuse van der Waals and covalent radii.
Assertion (A): The second ionisation potential of oxygen is greater than that of fluorine.
Reason (R): Oxygen acquires a stable half-filled electronic configuration after losing one electron.
(a) Both A and R are true, and R is the correct explanation of A.
(b) Both A and R are true, but R is not the correct explanation of A.
(c) A is true, but R is false.
(d) A is false, but R is true.
Show Answer & Explanation
Answer: (a) Both A and R are true, and R is the correct explanation of A.
Explanation:
1. O+ is 2p3 (half-filled) and extra stable, which makes the removal of the second electron hard; F+ is 2p4.
2. R explains A.
Teacher's Note:
1. Half-filled subshells raise the next ionisation energy.
Assertion (A): Alkali metals have the least first ionisation potential in their respective periods.
Reason (R): Alkali metals have only one electron in the valence shell.
(a) Both A and R are true, and R is the correct explanation of A.
(b) Both A and R are true, but R is not the correct explanation of A.
(c) A is true, but R is false.
(d) A is false, but R is true.
Show Answer & Explanation
Answer: (b) Both A and R are true, but R is not the correct explanation of A.
Explanation:
1. A is true. R is true, but the low IE is due to large size and small Zeff; having one electron alone is not the explanation.
Teacher's Note:
1. The ns1 electron is far from the nucleus and well shielded.
Assertion (A): The atomic size of Na is larger than that of Mg.
Reason (R): The number of shells in Na is more than that of Mg.
(a) Both A and R are true, and R is the correct explanation of A.
(b) Both A and R are true, but R is not the correct explanation of A.
(c) A is true, but R is false.
(d) A is false, but R is true.
Show Answer & Explanation
Answer: (c) A is true, but R is false.
Explanation:
1. Na (186 pm) is larger than Mg (160 pm) because of a lower nuclear charge: A is true.
2. Both are in period 3 with three shells, so R is false.
Teacher's Note:
1. Zeff increases from Na to Mg.
Assertion (A): The second ionisation potential of alkali metals is the maximum in the period.
Reason (R): Alkali metals have the smallest atomic size in the period.
(a) Both A and R are true, and R is the correct explanation of A.
(b) Both A and R are true, but R is not the correct explanation of A.
(c) A is true, but R is false.
(d) A is false, but R is true.
Show Answer & Explanation
Answer: (c) A is true, but R is false.
Explanation:
1. M+ has a noble gas configuration, so IE2 is very high: A is true.
2. R is false: alkali metals have the largest atomic size in the period.
Teacher's Note:
1. IE2 of alkali metals is huge because of the core electron.
Assertion (A): Atomic size along a period decreases.
Reason (R): The effective nuclear charge in a period decreases.
(a) Both A and R are true, and R is the correct explanation of A.
(b) Both A and R are true, but R is not the correct explanation of A.
(c) A is true, but R is false.
(d) A is false, but R is true.
Show Answer & Explanation
Answer: (c) A is true, but R is false.
Explanation:
1. A is true; R is false: Zeff increases across the period, which causes the decrease in size.
Teacher's Note:
1. Zeff increases left to right.
Assertion (A): The atomic sizes of Cs and Fr are almost similar.
Reason (R): Cs and Fr belong to the same group.
(a) Both A and R are true, and R is the correct explanation of A.
(b) Both A and R are true, but R is not the correct explanation of A.
(c) A is true, but R is false.
(d) A is false, but R is true.
Show Answer & Explanation
Answer: (b) Both A and R are true, but R is not the correct explanation of A.
Explanation:
1. Cs (265 pm) and Fr (about 270 pm) are very nearly equal: A is true.
2. R is true but being in the same group does not explain the similarity of sizes; relativistic effects and filled f-orbital shielding do.
Teacher's Note:
1. Same group does not imply equal size.
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