JEE Chemistry S Block Elements MCQs Set 22

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Chapter-wise Objective Questions: S Block Elements

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Multiple Choice Questions

Question 1: Which of the following are correct orders of first ionisation energy? (1) K < Na < Li (2) Be > Mg > Ca (3) B > C > N (4) Ge > Si > C
(a) (2) and (3) only
(b) (3) and (4) only
(c) (1) and (2) only
(d) (1) and (4) only
Show Answer & Explanation

Answer: (c) (1) and (2) only

Explanation:
1. (1), (2) follow the decrease down a group. The correct orders are N > C > B and C > Si > Ge for (3), (4), so those are wrong.

Teacher's Note:
1. IE falls down a group and rises across a period with exceptions.
2. N has a half-filled p subshell.

Question 2: The hydration energy of Mg\(^{2+}\) is higher than that of
(a) Al\(^{3+}\) and Ca\(^{2+}\)
(b) Al\(^{3+}\) and Na\(^+\)
(c) Ca\(^{2+}\) and Na\(^+\)
(d) Al\(^{3+}\) only
Show Answer & Explanation

Answer: (c) Ca\(^{2+}\) and Na\(^+\)

Explanation:
1. Hydration energy rises with charge density. Mg2+ is smaller than Ca2+ and carries twice the charge of Na+, so its hydration energy is larger than both, but Al3+ is smaller and more highly charged.

Teacher's Note:
1. Compare charge/radius.
2. Hydration energy: Al3+ > Mg2+ > Ca2+ > Na+.

Question 3: Which of the following statements are incorrect? (1) The atomic radius of Na is greater than that of Mg. (2) The metallic bond in Mg is stronger than in Na. (3) K has higher melting and boiling points than Na. (4) Mg and Ca both impart characteristic colours to a flame.
(a) (3) and (4)
(b) (1) and (2)
(c) (2) and (3)
(d) (1) and (4)
Show Answer & Explanation

Answer: (a) (3) and (4)

Explanation:
1. K melts at 336 K and Na at 371 K, so (3) is wrong. Mg gives no flame colour, so (4) is wrong. (1) and (2) are right.

Teacher's Note:
1. Metallic bonding weakens down the group.
2. Be and Mg give no colour.

Question 4: Which of the following statements are true? (1) Hydration enthalpy of alkali metal ions is less than that of alkaline earth ions of the same period. (2) Alkaline earth ions have a much larger charge to radius ratio. (3) Heats of hydration of dipositive alkaline earth ions decrease with increasing ionic size.
(a) (1) and (2) only
(b) (2) and (3) only
(c) (1) and (3) only
(d) (1), (2) and (3)
Show Answer & Explanation

Answer: (d) (1), (2) and (3)

Explanation:
1. All three follow from hydration enthalpy increasing with charge density.

Teacher's Note:
1. Higher charge and smaller size increase hydration.
2. Be2+ is hydrated most strongly.

Question 5: Which of the following statements are correct? (1) Milk of lime is a suspension of Ca(OH)\(_2\) in water. (2) Lime water is a clear solution of Ca(OH)\(_2\). (3) Baryta water is a clear solution of Ba(OH)\(_2\). (4) Nitrolim is a mixture of CaCN\(_2\) and carbon.
(a) (1), (2) and (3) only
(b) All four
(c) (2), (3) and (4) only
(d) (1) and (4) only
Show Answer & Explanation

Answer: (b) All four

Explanation:
1. Each is the standard definition.

Teacher's Note:
1. Learn the common names.
2. Nitrolim is a fertiliser.

Question 6: Which statements are correct? (1) Stability of peroxides and superoxides of alkali metals increases as cation size increases. (2) This is due to stabilisation of large anions by large cations through lattice energy. (3) The low solubility of LiF is due to high lattice energy, and of CsI due to low hydration energy. (4) NaOH is not deliquescent.
(a) (1), (2) and (4)
(b) (1), (2) and (3)
(c) (2), (3) and (4)
(d) (1) and (4) only
Show Answer & Explanation

Answer: (b) (1), (2) and (3)

Explanation:
1. NaOH is strongly deliquescent, so (4) is wrong. The first three are correct.

Teacher's Note:
1. Remember the lattice energy argument.
2. Large cation-large anion pairs pack well.

Question 7: Sodium bicarbonate can react with which of the following? (1) Na\(_2\)CO\(_3\) (2) NaOH (3) NaH (4) HCl
(a) (1), (2) and (3)
(b) (1) and (4)
(c) (2) and (4) only
(d) (2), (3) and (4)
Show Answer & Explanation

Answer: (d) (2), (3) and (4)

Explanation:
1. NaHCO3 is acidic towards NaOH and NaH (giving Na2CO3 with H2O or H2) and reacts with HCl. It does not react with Na2CO3.

Teacher's Note:
1. NaHCO3 + NaOH gives Na2CO3 + H2O.
2. NaH + NaHCO3 gives Na2CO3 + H2.

Question 8: Which of the following sulphates are readily soluble in water? (1) MgSO\(_4\) (2) SrSO\(_4\) (3) BeSO\(_4\) (4) BaSO\(_4\)
(a) (1) and (3)
(b) (2) and (4)
(c) (1) and (2)
(d) (3) and (4)
Show Answer & Explanation

Answer: (a) (1) and (3)

Explanation:
1. Solubility of group 2 sulphates decreases down the group because lattice energy falls less than hydration energy. BeSO4 and MgSO4 are soluble.

Teacher's Note:
1. BaSO4 is the least soluble sulphate known.
2. Hydration energy dominates for Be and Mg.

Question 9: Nitrates that give the metal oxide on heating not above 500 \(^\circ\)C are those of
(a) Na and Li
(b) Na and Mg
(c) Li and Mg
(d) Na only
Show Answer & Explanation

Answer: (c) Li and Mg

Explanation:
1. LiNO3 and Mg(NO3)2 decompose to oxide + NO2 + O2, while NaNO3 gives the nitrite.

Teacher's Note:
1. Li behaves like Mg.
2. Sodium nitrate gives NaNO2 + O2.

Question 10: A substance P when heated in a dry tube gives a colourless odourless gas that rekindles a glowing splinter. P may be
(a) K2SO3 or CaCO3
(b) KClO3 or CaCO3
(c) NaNO3 or K2SO3
(d) KClO3 or NaNO3
Show Answer & Explanation

Answer: (d) KClO3 or NaNO3

Explanation:
1. The gas is O2. KClO3 gives KCl + O2 and NaNO3 gives NaNO2 + O2. CaCO3 gives CO2.

Teacher's Note:
1. A glowing splinter relights in oxygen.
2. K2SO3 gives K2SO4 and K2S.

Question 11: Ammoniated solutions of alkali metals are reducing agents because of the
(a) solvated cation
(b) solvated unpaired electron
(c) liberation of hydrogen gas
(d) solvated cation and solvated electron both
Show Answer & Explanation

Answer: (b) solvated unpaired electron

Explanation:
1. The ammoniated electron [e(NH3)y]- is a powerful electron donor.

Teacher's Note:
1. It is responsible for blue colour and reducing power.
2. The cation is not a reductant.

Question 12: Highly pure dilute solution of sodium in liquid ammonia: which statements are correct? (1) shows blue colour (2) conducts electricity (3) produces sodium amide (4) produces hydrogen gas
(a) (1) and (2) only
(b) (1), (2) and (3)
(c) (3) and (4)
(d) (1), (2) and (4)
Show Answer & Explanation

Answer: (a) (1) and (2) only

Explanation:
1. Pure solutions are stable and blue with ammoniated electrons which conduct. Amide and H2 form slowly only on standing or with a catalyst.

Teacher's Note:
1. Traces of Fe or air cause decomposition.
2. The blue solution is not stable to catalysts.

Question 13: Sodium nitrate decomposes above 800 \(^\circ\)C to give
(a) NaNO2 and O2
(b) N2O only
(c) N2, O2 and Na2O
(d) NO2 and Na2O
Show Answer & Explanation

Answer: (c) N2, O2 and Na2O

Explanation:
1. Below 800 C it gives NaNO2 + O2. Above 800 C the nitrite decomposes further: \( \ce{4NaNO3 -> 2Na2O + 2N2 + 5O2} \).

Teacher's Note:
1. Higher temperature, more complete decomposition.
2. Na2O is a basic oxide residue.

Question 14: Which is/are formed on burning sodium in excess of air?
(a) only NaO2
(b) only NaOH
(c) Na2O2 with a little Na2O
(d) only Na2O
Show Answer & Explanation

Answer: (c) Na2O2 with a little Na2O

Explanation:
1. Sodium gives mainly the peroxide, with a small amount of the oxide.

Teacher's Note:
1. Li gives Li2O, K gives KO2.
2. NaOH forms later from moisture.

Question 15: Statement-1: Alkali metals dissolve in liquid ammonia to give blue solutions. Statement-2: Alkali metals in liquid ammonia give solvated species of the type [M(NH\(_3\))\(_n\)]\(^+\). Choose the correct option.
(a) Both statements are true but Statement-2 is not the correct explanation of Statement-1
(b) Both are true and Statement-2 explains Statement-1
(c) Statement-1 is true and Statement-2 is false
(d) Statement-1 is false and Statement-2 is true
Show Answer & Explanation

Answer: (a) Both statements are true but Statement-2 is not the correct explanation of Statement-1

Explanation:
1. The blue colour is due to the ammoniated electron, not the ammoniated cation.

Teacher's Note:
1. Both statements are true on their own.
2. Colour comes from the electron.

Question 16: Solution of K\(_2\)O in water is basic because it contains a significant concentration of
(a) \( \ce{O2^{2-}} \)
(b) \( \ce{O^{2-}} \)
(c) \( \ce{OH^-} \)
(d) \( \ce{K^+} \)
Show Answer & Explanation

Answer: (c) \( \ce{OH^-} \)

Explanation:
1. \( \ce{K2O + H2O -> 2KOH} \). O2- is a very strong base and cannot exist in water.

Teacher's Note:
1. Oxide ion reacts completely with water.
2. The OH- gives the basic solution.

Question 17: Which oxide is formed when potassium is burnt in excess of air?
(a) \( \ce{KO2} \)
(b) \( \ce{KO3} \)
(c) \( \ce{K2O} \)
(d) \( \ce{K2O2} \)
Show Answer & Explanation

Answer: (a) \( \ce{KO2} \)

Explanation:
1. K forms the superoxide as the main product.

Teacher's Note:
1. Larger cations stabilise larger anions.
2. Li gives Li2O, Na gives Na2O2.

Question 18: Sodium hydroxide is prepared on a commercial scale by
(a) Dow's process
(b) Solvay process
(c) Hall-Heroult process
(d) the Castner-Kellner cell
Show Answer & Explanation

Answer: (d) the Castner-Kellner cell

Explanation:
1. Electrolysis of brine with a mercury cathode (Castner-Kellner) gives NaOH.

Teacher's Note:
1. Solvay gives Na2CO3.
2. Hall-Heroult is for aluminium.

Question 19: Which gives sodium hydroxide along with hydrogen gas on reaction with water?
(a) Sodium oxide
(b) Sodium amalgam
(c) Sodium peroxide
(d) Sodium carbonate
Show Answer & Explanation

Answer: (b) Sodium amalgam

Explanation:
1. \( \ce{2Na(Hg) + 2H2O -> 2NaOH + H2 + Hg} \).

Teacher's Note:
1. Na2O gives only NaOH; Na2O2 gives NaOH and H2O2.
2. The carbonate does not react.

Question 20: Which of the following can exist in aqueous solution?
(a) \( \ce{Na2O} \)
(b) \( \ce{K2CO3} \)
(c) \( \ce{Na2O2} \)
(d) \( \ce{KO2} \)
Show Answer & Explanation

Answer: (b) \( \ce{K2CO3} \)

Explanation:
1. Oxides, peroxides and superoxides react with water. K2CO3 simply dissolves.

Teacher's Note:
1. The others hydrolyse completely.
2. Choose a stable salt.

Question 21: Which of these salts are made of isoelectronic cation and anion? (I) NaCl (II) BaCl\(_2\) (III) MgF\(_2\) (IV) CaS
(a) I and II
(b) II and III
(c) None of these
(d) III and IV
Show Answer & Explanation

Answer: (d) III and IV

Explanation:
1. MgF2: Mg2+ and F- both have 10 electrons. CaS: Ca2+ and S2- both have 18. NaCl has 10 and 18, BaCl2 has 54 and 18.

Teacher's Note:
1. Count electrons in each ion.
2. Isoelectronic means equal electron count.

Question 22: Which of the following liberates H\(_2\) with cold water?
(a) \( \ce{NaH} \)
(b) \( \ce{H2O2} \)
(c) \( \ce{NaOH} \)
(d) \( \ce{Mg} \)
Show Answer & Explanation

Answer: (a) \( \ce{NaH} \)

Explanation:
1. \( \ce{NaH + H2O -> NaOH + H2} \). Mg reacts only with hot water or steam.

Teacher's Note:
1. Ionic hydrides contain H-.
2. H2O2 does not give H2.

Question 23: When ionic nitrides react with water, the products are
(a) an acidic solution and hydrogen
(b) an acidic solution and ammonia
(c) a basic solution and ammonia gas
(d) a basic solution and hydrogen
Show Answer & Explanation

Answer: (c) a basic solution and ammonia gas

Explanation:
1. \( \ce{N^{3-} + 3H2O -> NH3 + 3OH^-} \).

Teacher's Note:
1. Nitride ion is a strong base.
2. Li3N and Mg3N2 behave this way.

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Multiple Choice Questions (MCQs) for JEE Chemistry S Block Elements

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