JEE Chemistry Classification of Elements and Periodicity in Properties MCQs Set 22

Chemistry Objective Questions and Answers: Classification Of Elements and Periodicity In Properties

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Multiple Choice Questions

Question 1: An element has the outermost electron configuration 5f2 6d1 7s2. It belongs to the
(a) s-block
(b) transition series
(c) actinoid series
(d) lanthanoid series
Show Answer & Explanation

Answer: (c) actinoid series

Explanation:
1. The 5f subshell is being filled, which defines the actinoids.

Teacher's Note:
1. Last electron enters 5f.
2. Lanthanoids fill 4f.

Question 2: Which oxyacid of chlorine shows the +5 oxidation state?
(a) Chloric acid (HClO3)
(b) Chlorous acid
(c) Perchloric acid
(d) Hypochlorous acid
Show Answer & Explanation

Answer: (a) Chloric acid (HClO3)

Explanation:
1. In HClO3: +1 + x - 6 = 0, so x = +5.
2. HOCl is +1, HClO2 is +3 and HClO4 is +7.

Teacher's Note:
1. Calculate oxidation number from the formula.
2. Chloric acid = +5.

Question 3: Which element does not show a positive oxidation state?
(a) Chlorine
(b) Fluorine
(c) Oxygen
(d) Iodine
Show Answer & Explanation

Answer: (b) Fluorine

Explanation:
1. Fluorine is the most electronegative element and always shows -1.
2. Oxygen is +2 in OF2.

Teacher's Note:
1. No element can pull electrons from fluorine.
2. Cl and I show positive states.

Question 4: The atom of an element X contains 27 electrons. X is expected to be
(a) an s-block element
(b) diamagnetic and belongs to the d-block
(c) a non-metal of the p-block
(d) paramagnetic and belongs to the d-block
Show Answer & Explanation

Answer: (d) paramagnetic and belongs to the d-block

Explanation:
1. Z = 27 is cobalt: [Ar] 3d7 4s2.
2. It has three unpaired electrons, so it is paramagnetic.

Teacher's Note:
1. Count unpaired electrons.
2. Co is a d-block metal.

Question 5: The group of the periodic table in which the elements exist in all three physical states at room temperature is
(a) group 1
(b) group 17 (halogens)
(c) group 14
(d) group 15
Show Answer & Explanation

Answer: (b) group 17 (halogens)

Explanation:
1. Fluorine and chlorine are gases, bromine is a liquid and iodine is a solid.

Teacher's Note:
1. Halogens are gas, liquid and solid.
2. Alkali metals are all solids.

Question 6: The element with Z = 83 belongs to which block?
(a) s-block
(b) f-block
(c) p-block
(d) d-block
Show Answer & Explanation

Answer: (c) p-block

Explanation:
1. Z = 83 is bismuth: [Xe] 4f14 5d10 6s2 6p3.

Teacher's Note:
1. The last electron enters 6p.
2. Bi is in group 15.

Question 7: Which of the following has the highest electron affinity?
(a) Br
(b) F
(c) Cl
(d) I
Show Answer & Explanation

Answer: (c) Cl

Explanation:
1. Cl has the highest electron gain enthalpy of all the elements (-349 kJ/mol).

Teacher's Note:
1. F is lower due to repulsion.
2. Cl > F > Br > I.

Question 8: The group of the long form of the periodic table that contains three elements together in each period is
(a) zero group
(b) group VIII (groups 8, 9, 10)
(c) group III
(d) group IV
Show Answer & Explanation

Answer: (b) group VIII (groups 8, 9, 10)

Explanation:
1. The VIII group contains triads: Fe, Co, Ni; Ru, Rh, Pd; Os, Ir, Pt.

Teacher's Note:
1. Triads occur in group VIII.
2. Other groups have one element per period.

Question 9: The atom with the largest electron affinity among Na, Cl, I and P is
(a) Cl
(b) I
(c) P
(d) Na
Show Answer & Explanation

Answer: (a) Cl

Explanation:
1. Cl -349 kJ/mol, I -295, P -72, Na -53.

Teacher's Note:
1. Halogens have the highest values.
2. Cl is the highest.

Question 10: The correct order of increasing atomic radius of Li, Be, B and Na is
(a) B < Be < Li < Na
(b) Li < Be < B < Na
(c) Be < Li < B < Na
(d) Be < B < Li < Na
Show Answer & Explanation

Answer: (a) B < Be < Li < Na

Explanation:
1. Radii (pm): B 88, Be 111, Li 152, Na 186.

Teacher's Note:
1. Period 2 radii fall from Li to B.
2. Na is in period 3.

Question 11: The ion that has 18 electrons in its outermost shell is
(a) Al3+ (Z = 13)
(b) Th4+ (Z = 90)
(c) Cu+ (Z = 29)
(d) K+ (Z = 19)
Show Answer & Explanation

Answer: (c) Cu+ (Z = 29)

Explanation:
1. Cu+ = [Ar] 3d10, so its outermost occupied shell (n = 3) has 18 electrons.
2. Al3+ has 8 (n = 2), K+ has 8 and Th4+ has 8 in the sixth shell.

Teacher's Note:
1. Count electrons in the highest occupied shell.
2. Pseudo-noble gas configuration.

Question 12: The correct order of increasing first ionisation energy is
(a) K < Ca < P < F < Ne
(b) Ca < K < Ne < P < F
(c) Ne < F < P < Ca < K
(d) F < Ca < Ne < P < K
Show Answer & Explanation

Answer: (a) K < Ca < P < F < Ne

Explanation:
1. IE1 (kJ/mol): K 419, Ca 590, P 1012, F 1681, Ne 2081.

Teacher's Note:
1. Metals have low IE.
2. Noble gases are highest.

Question 13: Which group has the species correctly listed in decreasing order of radius?
(a) Cu2+, Cu+, Cu
(b) B, Be, Li
(c) F-, Br-, I
(d) V, V2+, V3+
Show Answer & Explanation

Answer: (d) V, V2+, V3+

Explanation:
1. Removing electrons shrinks the species, so V > V2+ > V3+.
2. The other sets are not in decreasing order.

Teacher's Note:
1. Cations are smaller than atoms.
2. Higher charge means smaller size.

Question 14: Among S, I, Ba and Al, the element with the lowest electronegativity is
(a) I
(b) S
(c) Al
(d) Ba
Show Answer & Explanation

Answer: (d) Ba

Explanation:
1. Pauling values: Ba 0.89, Al 1.61, S 2.58, I 2.66.

Teacher's Note:
1. Alkaline earth metals have low EN.
2. Ba is the most metallic of these.

Question 15: An atom has 11 electrons in its 5f subshell (as in einsteinium). The number of unpaired electrons in that subshell is
(a) 4
(b) 3
(c) 11
(d) 7
Show Answer & Explanation

Answer: (b) 3

Explanation:
1. The 7 orbitals take 7 electrons singly, and the remaining 4 pair up, leaving 7 - 4 = 3 unpaired electrons.

Teacher's Note:
1. Hund's rule: fill singly first.
2. Unpaired = 14 - number of electrons for more than half-filled.

Question 16: The first four ionisation energies of a metal are 191, 587, 872 and 5962 kcal/mol. The number of valence electrons is
(a) 5
(b) 2
(c) 1
(d) 3
Show Answer & Explanation

Answer: (d) 3

Explanation:
1. The big jump after the third value shows that the fourth electron comes from the core.

Teacher's Note:
1. Look for the largest jump.
2. It comes after the last valence electron.

Question 17: Which species has the largest size among O2-, Na+, F- and Al3+?
(a) O2-
(b) F-
(c) Na+
(d) Al3+
Show Answer & Explanation

Answer: (a) O2-

Explanation:
1. All are isoelectronic; O2- has the lowest nuclear charge, so it is the largest.

Teacher's Note:
1. Anions are larger than cations of the same electron count.
2. Lower Z means bigger.

Question 18: Among N3-, F-, Na+ and Mg2+, which will have the smallest and which the largest ionic radius?
(a) N3- smallest and Na+ largest
(b) Mg2+ smallest and Na+ largest
(c) F- smallest and N3- largest
(d) Mg2+ smallest and N3- largest
Show Answer & Explanation

Answer: (d) Mg2+ smallest and N3- largest

Explanation:
1. All have 10 electrons.
2. Mg2+ has the highest nuclear charge (smallest) and N3- the lowest (largest).

Teacher's Note:
1. Isoelectronic: size is inverse to Z.
2. Order: N > F > Na > Mg.

Question 19: Which set does NOT show correct matching according to the modern periodic table?
(a) Fe2+ = [Ar]3d6; the element belongs to group 8
(b) Sc3+ = [Ne]3s23p6; the element belongs to group 18
(c) Cr = [Ar]3d54s1; the element belongs to group 6
(d) Cu = [Ar]3d104s1; the element belongs to group 11
Show Answer & Explanation

Answer: (b) Sc3+ = [Ne]3s23p6; the element belongs to group 18

Explanation:
1. Sc3+ has the argon configuration but the element Sc has Z = 21 and belongs to group 3.
2. The group is decided by the neutral atom, not by the ion.

Teacher's Note:
1. Group number comes from the atom's configuration.
2. d + s electrons give the group for d-block elements.

Question 20: Which pair of ions cannot exist together in aqueous solution?
(a) Mg2+ and Br-
(b) Pb2+ and F-
(c) Na+ and Cl-
(d) Tl3+ and I-
Show Answer & Explanation

Answer: (d) Tl3+ and I-

Explanation:
1. Tl3+ is a strong oxidant (inert pair effect) and oxidises I- to I2, being reduced to Tl+.

Teacher's Note:
1. Inert pair effect makes Tl(III) oxidising.
2. TlI3 actually contains Tl+ and I3-.

Question 21: Consider the statements: (I) Across the transition series from Cr to Cu the atomic radius changes little. (II) The rate of decrease in size across the lanthanoid series is less than across the first transition series. Which is correct?
(a) Both (I) and (II)
(b) Only (I)
(c) Only (II)
(d) Neither (I) nor (II)
Show Answer & Explanation

Answer: (a) Both (I) and (II)

Explanation:
1. In a transition series the added electrons enter the inner d subshell and screen the nuclear charge, so Zeff changes very little.
2. Across the 4f series the increase in Zeff is gradual, so the contraction per element is small.

Teacher's Note:
1. Inner subshell filling gives small radius change.
2. Lanthanoid contraction is gradual.

Question 22: Which statement is true?
(a) A larger IE and electron affinity give smaller Mulliken electronegativity
(b) A larger ionisation enthalpy makes cation formation easier
(c) A larger electron gain enthalpy (more negative) makes anion formation easier
(d) A larger Zeff means a larger atomic size
Show Answer & Explanation

Answer: (c) A larger electron gain enthalpy (more negative) makes anion formation easier

Explanation:
1. Mulliken's EN is proportional to (IE + EA)/2, so it rises with both.
2. A larger Zeff shrinks the atom, and a large IE makes cation formation harder.

Teacher's Note:
1. Easy anion formation needs a large negative egH.
2. Larger Zeff means smaller size.

Question 23: Which statements are correct for d-block elements? (i) their general configuration is (n-1)d1-10ns0-2; (ii) they exhibit variable valency; (iii) the last electron enters the (n-1)d subshell; (iv) they are placed in periods 3 to 6
(a) (i), (ii) and (iii) only
(b) (i), (ii) and (iv) only
(c) All four
(d) (ii), (iii) and (iv) only
Show Answer & Explanation

Answer: (a) (i), (ii) and (iii) only

Explanation:
1. (i), (ii) and (iii) are standard properties of d-block elements.
2. The d-block occupies periods 4 to 7 (3d, 4d, 5d, 6d), not 3 to 6.

Teacher's Note:
1. d-block begins in period 4 with Sc.
2. 3d is filled in period 4.

Question 24: Poor shielding of nuclear charge by d and f electrons is responsible for which of these facts? (i) the radius of Nb (4d) is comparable to that of Ta (5d); (ii) the first IE of Cu is less than that of Zn; (iii) the egH of S is more negative than that of O; (iv) the IE of Au is higher than that of Ag
(a) (ii) and (iii) only
(b) (i) and (ii) only
(c) (iii) and (iv) only
(d) (i) and (iv) only
Show Answer & Explanation

Answer: (d) (i) and (iv) only

Explanation:
1. Poor shielding by 4f electrons causes the lanthanoid contraction, so Nb and Ta have similar radii and Au has a higher IE than Ag.
2. The Cu/Zn and S/O differences have other causes.

Teacher's Note:
1. d and f shielding is poor.
2. Effect shows up in 5d series.

Question 25: Which of the following elements has only one non-zero oxidation state? (i) Be, (ii) O, (iii) F, (iv) N
(a) F and N only
(b) Be and O only
(c) Be and F only
(d) O and N only
Show Answer & Explanation

Answer: (c) Be and F only

Explanation:
1. Be shows only +2 and F shows only -1.
2. O shows -2, -1, +2 and N shows -3 to +5.

Teacher's Note:
1. Count the oxidation states.
2. F has no positive state.

Question 26: Which of these are endothermic steps? (i) S-(g) + e- gives S2-(g); (ii) Ne(g) + e- gives Ne-(g); (iii) N(g) + e- gives N-(g); (iv) Al2+(g) gives Al3+(g) + e-
(a) All four
(b) (i) and (iv) only
(c) (i) and (ii) only
(d) (ii) and (iii) only
Show Answer & Explanation

Answer: (a) All four

Explanation:
1. Second egH is positive; noble gases and N have positive egH; and every ionisation step is endothermic.

Teacher's Note:
1. Positive egH means endothermic.
2. Ionisation is always endothermic.

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