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Covalent Bond vs Ionic Bond

Which of the ...

Question

Which of the following reaction(s) is/are exothermic for the formation of $N a F (s)$ ?
I. $N a_{(g)} \to N a_{(g)}^{+} + e^{-}$
II. $F_{(g)} + e^{-} \to F_{(g)}^{-}$
III. $N a_{(g)}^{+} + F_{(g)}^{-} \to N a F_{(s)}$

I only

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II only

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I and III only

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II and III only

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Solution

The correct option is D II and III only
Case I
$N a$ is ionised to $N a^{+}$ and energy is required in the ionisation process, i.e., it is an endothermic process.

Case II
Due to high electron affinity, $F$ atom gains an electron and thus energy is released, i.e., it is an exothermic reaction.

Case III
This is the case of bond formation during which energy is released, i.e., exothermic reaction.

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Similar questions

N a F (s)

N a_{(g)} \to N a_{(g)}^{+} + e^{-}

F_{(g)} + e^{-} \to F_{(g)}^{-}

N a_{(g)}^{+} + F_{(g)}^{-} \to N a F_{(s)}

N a F (s)

N a_{(g)} \to N a_{(g)}^{+} + e^{-}

F_{(g)} + e^{-} \to F_{(g)}^{-}

N a_{(g)}^{+} + F_{(g)}^{-} \to N a F_{(s)}

N a (s) \frac{1}{2} {C I}_{2} ⟶ N a C I (s) Δ H = Q

N a (s) ⟶ N a (g) Δ H = S

N a (g) ⟶ {N a}^{+} (g) + e^{-} Δ H = I

\frac{1}{2} {C I}_{2} (g) ⟶ C I (g) Δ H = \frac{D}{2}

C I (g) + e^{-} ⟶ C I^{-} (g) Δ H = ?

{N a}^{+} (g) + {C I}^{-} (g) ⟶ N a C I (s) Δ H = - U

N a (s) S - ------------ \to Energy of subtimation N a (g)

N a (g) I - ---------- \to Ionisation potenital N a^{+} (g) + e^{-}

C l_{2} (g) D - -------------- \to Bond dissociation energy 2 C l (g)

C l (g) + e^{-} E - --------- \to Electron - affinity C l^{-} (g)

C l^{-} (g) + N a^{+} (g) U - ------- \to Lattice energy N a C l (s)

U = {a, b, c, d, e, f, g, h},

(i) A = {a, b, c} (i i) B = {d, e, f, g}

(i i i) C = {a, c, e, g} (i v) D = {f, g, h, a}

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