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Anomalous Behaviour of Fluorine

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Question

(a) Complete the following chemical equation :

(i) $C u + H N O_{3} (d i l .) \to$
(ii) $X e F_{4} + O_{2} F_{2} \to$
(b) Explain the following observations :

(i) Phosphorus has a grater tendency for catenation than nitrogen.
(ii) Oxygen is a gas but sulphur a solid.
(iii) The halogens are coloured. Why?

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Solution

(a) (i) $3 C u + 8 H N O_{3 (d i l u t e)} ⟶ 3 C u (N O_{3})_{2} + 2 N O + 4 H_{2} O$

(ii) $X e F_{4} + O_{2} F_{2} ⟶ X e F_{6} + O_{2}$

(b)
(i) Catenation is much more common in phosphorous compounds than in nitrogen compounds. This is because of the relative weakness of the N-N single bond as compared to the P-P single bond. Since nitrogen atom is smaller, there is greater repulsion of electron density of two nitrogen atoms, thereby weakening the N-N single bond.

(ii) Oxygen is smaller in size as compared to sulphur. Due to its smaller size, it can effectively form $p π - p π$ bonds and form $O_{2} (O = O)$ molecule. Also, the intermolecular forces in oxygen are weak van der Waal forces, which causes it to exist as a gas. On the other hand, sulphur does not form $S_{2}$ molecule but exists as a puckered structure held together by strong covalent bonds.
Hence, it is solid.

(iii) Almost all halogens are coloured. This is because of halogens absorb radiations in the visible region. This results in the excitation of valence electrons to a higher energy region. Since the amount of energy required for excitation differs for each halogen, each halogen displays a different colour.

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Similar questions

Q. (a) Draw the structures of the following molecules:
(i)

H_{3} P O_{2}

C l F_{3}

(b) Explain the following observations:
(i) Nitrogen is much less reactive than phosphorus.
(ii) Despite having greater polarity, hydrogen fluoride boils at a lower temperature than water.
(iii) Sulphur has a greater tendency for catenation than oxygen in the same group.

Q. (a) Draw the molecular structures of the following compounds:
(i)

N_{2} O_{5}

X_{e} O F_{4}

(b) Explain the following observations
(i) Sulphur has a greater tendency for catenation than oxygen.
(ii)

I - C l

is more reactive than

I_{2}

.
(iii) Despite lower value of its electron gain enthalpy with negative sign, fluorine

(F_{2})

is a stronger oxidizing agent than

C l_{2}

Q. (a) Complete the following chemical equations:
(i)

N a O H (h o t a n d c o n c .) + C l_{2} \to

X_{e} F_{4} + O_{2} F_{2} \to

(b) Draw the structures of the following molecules :
(i)

H_{3} P O_{2}

H_{2} S_{2} O_{7}

X e O F_{4}

Q. (a) Complete the following chemical equations:
(i)

X e F_{4} + S b F_{5} \to

C l_{2} + F_{2} (e x c e s s) \to

(b) Explain each of the following:
(i) Nitrogen is much less reactive than phosphorus.
(ii) The stability of +5 oxidation state decreases down group 15.
(iii) The bond angles (

O - N - O

) are not of the same value in

N O_{2}^{-}

N O_{2}^{+}

Q. Assign reason for the following:
(i)

H_{3} P O_{2}

is a stronger reducing agent than

H_{3} P O_{4}

.
(ii) Sulphur shows more tendency for catenation than Oxygen.
(iii) Reducing character increases from

H F

H I

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