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When a standard solution of NaOH is left in air for a few hours :

a precipitate will form

strength of solution will decrease

the strength of solution will increase

the concentration of $N a^{+} .$ ion in solution will remains same

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Explanation

(b) NaOH being deliquescent absorb water from atmosphere therefore strength of solution will decrease.

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$C a C l_{2}$ is preffered over NaCl for clearing ice on roads particularly in very cold countries. This is because:

$C a C l_{2}$ is less soluble in $H_{2} O$ than NaCl

$C a C l_{2}$ is hygroscopic but NaCl is not

Eutectic mixture of $C a C l_{2} / H_{2} O$ freezes at $- 55 ° C$ while that of $N a C l / H_{2} O$ freezes at $- 18 ° C$

NaCl makes the road slippery but $C a C l_{2}$ does not

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Explanation

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Which of the following statement is false?

The milk of magnesia used as antacidis chemically $M g O + M g C l_{2}$

Stability of alkali metal peroxides increases with increase in atomic number

Hydration energy of AgF is higher than its lattice energy

Anhydrous $M g C l_{2}$ cannot be prepared contains by direct heating of $M g C l_{2} 6 H_{2} O$

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Explanation

(a) Milk of magnesia of MgO + $H_{2} O .$

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Calcium imide on hydrolysis gives gas (B) which on oxidation by bleaching powder gives gas (C). Gas (C) on reaction with magnesium give compound (D) which on hydrolysis gives again gas (B)> Identify (B), (C) and (D).

$N H_{3}, N_{2}, M g_{3} N_{2}$

$N_{2}, N H_{3}, M g N H$

$N_{2}, N_{2} O_{5}, M g {(N O_{3})}_{2}$

$N H_{3}, N O_{2}, M g {(N O_{2})}_{2}$

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Explanation

(a) $C a (N H) + 2 H_{2} O \to C a {(O H)}_{2} + \underset{(B)}{N H_{3} (g)}$

$\underset{(B)}{2 N H_{3}} + 3 C a O C l_{2} \to \underset{(C)}{N_{2} (g)} + 3 C a C l_{2} + 3 H_{2} O$

$\underset{(C)}{N_{2} (g)} + 3 M g \to \underset{(D)}{M g_{3} N_{2}}$

$\underset{(D)}{M g_{2} N_{2}} + 6 H_{2} O \to 3 M g {(O H)}_{2} + \underset{(B)}{2 N H 3}$

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Which of the following order is correct?

$K^{+} < C a^{2 +} < p^{3 -} < S^{2 -} : I o n i c s i z e$

$N a_{(a q .)}^{+} > K_{(a q .)}^{+} > R b_{(a q .)}^{+} > C s_{(a q .)}^{+} : E l e c t r i c a l c o n d u c \tan c e$

$A l_{(a q .)}^{3 +} > M g_{(a q .)}^{2 +} > N a_{(a q .)}^{+} : H y d r a t e d s i z e$

$I_{(a q .)}^{-} < B r_{(a q .)}^{-} < C l_{(a q .)}^{-} < F_{(a q .)}^{-} : I o n i c m o b i l i t y$

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Explanation

(c)

(a) $C a^{2 +} < K^{+} < S^{2 -} < p^{3 -} : I o n i c s i z e$

(b) $N a_{(a q .)}^{+} < K_{(a q .)}^{+} < R b_{(a q .)}^{+} < C s_{(a q .)}^{+} : E l e c t r i c a l c o n d u c \tan c e$

(d) $I_{(a q .)}^{-} < B r_{(a q .)}^{-} < C l_{(a q .)}^{-} > F_{(a q .)}^{-} : I o n i c m o b i l i t y$

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For the alkali metals, which of the following increase with increasing atomic number?

First ionization energy

Electronegativity

Hydration energy of the univalent ion

Atomic radius

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Explanation

for any group, top to bottom size increase.

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Compound having lowest melting point:

LiCl

CsCl

RbCl

KCl

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Which of the following statements is true for all the alkali metals?

Their nitrate decomposes on heating to give the corresponding nitrites and oxygen.

Their chlorides are deliquescent and crystallize as hydrates.

They react with water to form hydroxide and hydrogen.

They really react with halogens to form ionic halides. $M^{+} X^{-} .$

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Explanation

(C)

(A) $4 {LiNO}_{3} \overset{}{\to} 2 {Li}_{2} O + 4 {NO}_{2} + O_{2}$

$2 {NaNO}_{3} \overset{}{\to} 2 {NaNO}_{2} + O_{2}$ (similar decomposition with the nitrates of K, Rb, and Cs)

(B) Only LiCl is deliquescent and crystallises as a hydrate $LiCl . 2 H_{2} O$

(D) Halides of Li are covalent in nature.

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Sodium and potassium react with water much more vigorously than lithium because :

Sodium and potassium have high values of hydration energy as compared to that of lithium.

Sodium and Potassium have a higher melting point than that of lithium.

Sodium and potassium have a lower melting point than that of lithium.

Sodium and potassium have lower hydration energy than that of lithium.

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Explanation

(C)

When sodium and potassium react with water, the heat evolved causes them to melt, giving a

larger area of contact with water, lithium, on the other hand, does not melt under these conditions

and thus reacts more slowly.

$\underset{Melting point (° C) 180}{Li} \underset{98}{Na} \underset{64 .}{K}$

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Which of the following statements is not true about the dilute solutions of alkali metals in liquid ammonia?

They are deep blue coloured solutions.

They are highly conducting in nature.

They are diamagnetic in nature.

Ammoniated cations and ammoniated anions are formed in a solution.

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Explanation

(C)

$M + (x + y) {NH}_{3} \overset{}{\to} {[M {({NH}_{3})}_{x}]}^{+} + {[e {({NH}_{3})}_{y}]}^{-}$

Solutions are deep blue coloured due to the absorption of light in visible region by solvated electrons.

It is paramagnetic due to the presence of unpaired electrons.

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