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NEET Practice Questions (MCQs) with Answers & Solutions

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Which of the following will have the largest value of $K_{s p}$

$B e S O_{4}$

$M g S O_{4}$

$C a S O_{4}$

$B a S O_{4}$

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Explanation

(A). Because it is most soluble in water and solubility decreases as

$B e S O_{4}$ > $M g S O_{4}$ > $C a S O_{4}$ > $B a S O_{4}$

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What are $α$ , $β$ and $γ$ in the following equation

$α K_{4} [F e {(C N)}_{6}] + β K_{2} C O_{3} + γ S \overset{h e a t}{\to}$ Products ?

the products are Fe, $C O_{2},$ KCNO and KSCN.

1, 2, 3

2, 1, 5

1, 1, 5

2, 2, 3

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Explanation

(C). $K_{4} [F e {(C N)}_{6}] + K_{2} C O_{3} + 5 S \to F e + C O_{2} + K C N O + 5 K C N S$

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The correct order of increasing ionic character is –

$B e C l_{2} < M g C l_{2} < C a C l_{2} < B a C l_{2}$

$B e C l_{2} < M g C l_{2} < B a C l_{2} < C a C l_{2}$

$B e C l_{2} < B a C l_{2} < M g C l < C a C l_{2}$

$B a C l_{2} < C a C l_{2} < M g C l_{2} < B e C l_{2}$

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Explanation

(A). The ionic character of the halides increases on moving down the group.

$B e C l_{2} < M g C l_{2} < C a C l_{2} < B a C l_{2}$

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Sodium metal cannot be stored under-

Benzene

Kerosene

Alcohol

Toluene

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Explanation

(C). Na reacts with alcohol

$N a + C_{2} H_{5} O H \to C_{2} H_{5} O N a + \frac{1}{2} H_{2}$

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$B e F_{2}$ is soluble in water whereas fluorides of other alkaline earth metals are insoluble because of–

Ionisation nature of $B e F_{2}$

Covalent nature of $B e F_{2}$

Greater hydration energy of $B e^{2 +}$ ion as compared to its lattice energy

None of these

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Explanation

(C). An ionic compound is soluble in water if its hydration energy > lattice energy.

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Sodium looses its lustre on exposure to air due to formation of-

$N a_{2} O,$ NaOH and $N a_{2} C O_{3}$

$N a_{2} O$ and NaOH

$N a_{2} O$ and $N a_{2} C O_{3}$

NaOH and $N a_{2} C O_{3}$

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Explanation

(A). In air, a layer of $N a_{2} O$ , NaOH and $N a_{2} C O_{3}$ is formed on its surface which loses its lustre.

$4 N a + O_{2} \to 2 N a_{2} O \overset{2 H_{2} O}{\to} 4 N a O H \overset{2 C O_{2}}{\to} 2 N a_{2} C O_{3} + 2 H_{2} O$

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Sodium oxide reacts with water violently forming NaOH. On heating above 400ºC, it produces

Monoxide and peroxide

Monoxide and metallic sodium

Peroxide and metallic sodium

Monoxide and oxygen

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Explanation

$2 N a_{2} O \overset{400 ° C}{\to} N a_{2} O_{2} + 2 N a$

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Alkaline earth metals form hydrated crystalline solids such as $M g C l_{2} . 6 H_{2} O, C a C l_{2} . 6 H_{2} O$ . This is due to-

Smaller ionic size

Increased charge on ions

Higher hydration enthalpies

High oxidation potential

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Explanation

(C). The hydration energy of the ions of alkaline earth metals ( $M^{2 +}$ ) is nearly 4 or 5 times greater than that of alkali metals because of their small size and increased charge.

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Which of the following properties of alkali metals increases in magnitude as the atomic number increases –

Ionic radius

Electronegativity

Melting point

First ionisation energy

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Explanation

(A). Ionic radius increases as the atomic number of alkali metal increases.

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Which of the following statements is correct.

Alkali metals are less electropositive than alkaline earth metals

The alkaline earth metals are more denser and harder than alkali metals

The alkali metals are denser and harder than alkaline earth metals

The first IP of alkali metals is more than that of alkaline earth metals

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Explanation

(B). Because of small size, they are more closely packed in the crystal lattice. So they have comparatively stronger metallic bonds and so more denser and harder than alkali metals.

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