Oxoacids of Halogens and Interhalogen Compounds - Chemistry, Class 12, The p-Block Elements

Contents

1 Oxoacids of Halogens
- 1.1 Acidic Character of Oxoacids of Halogens
2 Interhalogen Compounds
3 Uses of Interhalogen Compounds
4 Pseudo Halogens

Oxoacids of Halogens

Among the halogens, fluorine has very little tendency to form oxoacids due to its high electronegativity and small size. However, it forms one oxoacid HOF known as fluoric (I) acid or hypofluorous acid. The rest of the halogens form four series of oxoacids, HOX, HXO₂, HXO_3, and HXO₄. Most of these cannot be isolated in pure state. They are stable only in aqueous solution or in the form of their salts.

Acidic Character of Oxoacids of Halogens

(i) The acidic strength of oxoacids having the same oxidation number of the halogen atom decreases with increase in atomic number i.e., with decreasing electronegativity of the atom.

For example: HClO is the strongest while HlO is weakest of all the acids in which oxidation state of halogen atom is +1.

Acid	HClO	HBrO	HIO
Ka	2.9 × 10^-8	5 × 10^-9	10^-11

Explanation

The electronegativity of the halogen atom attached to oxygen decreases in the order Cl > Br > I. Therefore, the tendency to withdraw electrons from oxygen atom towards itself decreases from Cl to Br to I. As a result the tendency to pull the electrons from the hydrogen decreases. Consequently, the release of H⁺ ion from HClO will be easier than HBrO. Similarly, the release of H⁺ ion from HBrO will be easier than from HIO. Thus, the acidic strength decreases in the order:

HClO > HBrO > HIO

(ii) With the increase in oxidation number of a particular halogen atom, the acidic character of corresponding oxoacid increases.

For example: The acidic strength of oxoacids of chlorine increases in the order :

HClO < HClO₂ < HClO₃ < HClO₄

Explanation: This can be explained on the basis of Lowry Bronsted concept. According to this concept, a strong acid has a weak conjugate base and a weak acid has a strong conjugate base. The conjugate bases of the oxoacids of chlorine are shown below :

Let us consider the stabilities of the conjugate bases, ClO¯, ClO₂¯, ClO₃‾, and ClO₄¯ formed from these acids, HClO, HClO₂, HClO₃ and HClO₄ respectively.

These anions are stabilized by the delocalisation of the charge between oxygen atoms. If the ion is stabilized to greater extent, it has lesser attraction for the proton and therefore, will behave as weaker base (lesser tendency for the reaction to go in backward direction). Consequently, the corresponding acid will be strong because weak conjugate base has strong acid and strong conjugate base has weak acid and vice versa. Now, the charge stabilization is minimum in ClO¯ and maximum in ClO₄¯. The charge stabilization increases in the order:

ClO¯ < ClO₂¯ < ClO₃¯ < ClO₄‾

This means that ClO¯ will have minimum stability and therefore, will have maximum attraction for the H⁺. In other words, ClO¯ will be strongest base and so its conjugate acid HClO will be the weakest acid.

Similarly, in this series, ClO₄¯ is the weakest base (maximum stabilized) and its conjugate acid HClO₄, is the strongest acid. Thus, the acidic strength increases in the order.

HClO < HClO₂ < HClO₃ <HClO₄

Interhalogen Compounds

The compounds containing two or more halogen atoms are called interhalogen compounds. They may be represented by the general formula XX_n’ , where X is a halogen of larger size and X’ of smaller size and X is more electronegative than X’.

As the ratio between radii of X and X’ increases, the number of atoms per molecule also increases. Thus, iodine (VII) fluoride should have maximum number of atoms because the ratio of radii between I and F is maximum. Each halogen combines with every other halogen to form interhalogen compounds.

For example: CIF, ICl₃, BrF₅ etc.

These are of two types :

(i) Neutral interhalogens

These are neutral molecules containing two or more halogen atoms.

For example: ICl, BrF₅, IF₅, IF₇ etc.

(ii) Interhalogen anions and cations

These are negatively charged interhalogen polyhalide anions XX’_2n^¯, (n = 1, 2, 3, 4) and polyhalonium cations (XX’_2n⁺). The most important of these compounds is the linear triatomic iodide ion, I₃¯ which is formed when iodine dissolves in an aqueous solution of potassium iodide.

I₂(s) + I¯(aq) → I₃¯(aq)

Some other polyhalide anions are ICl₂¯, ICl₄¯ and polyhalonium cations are ClF₂⁺, Cl₂F⁺ , BrF₂⁺, IF₂⁺ , ICl₂⁺ , ICl₄⁺ etc.

Nomenclature

The interhalogen compounds are named as halogen halides. The halogen with the positive oxidation state (i.e., A) is named as such and the halogen with negative oxidation state (i.e, X) is named as halide.

For example:

BrF₃ Bromine trifluoride

ClF Chlorine fluorine

IF₇ : Iodine heptafluoride

The different types of interhalogens of the type XX’ (diatomic), XX₃‘ (tri atomic), XX₅‘ (hexa atomic) and XX’₇ (hepta atomic)

Preparation

All interhalogen compounds are prepared by direct combination or by the reactions of halogen with other interhalogen compounds.

For example:

Cl₂ + F₂ → 2ClF

Cl2 + 3 F₂ → 2ClF₃

ClF + F₂ → ClF₃

ClF₃ + F₂ → ClF₅

I₂ + Cl₂ → 2ICl

I₂ + 3 Cl₂ → 2ICl₃

Br₂ + F₂ → 2 BrF

Br₂ + 3F₂ → 2 BrF₃

Br₂ + 5F₂ → 2BrF₅

I₂ + 5F₂ → 2IF₅

Cl₂ + 5F₂ → 2ClF₅

I₂ + 7F₂ → 2 IF₇

Lower interhalogens combine to form higher interhalogen.

ClF + F₂ → ClF₃

ClF₃ + F₂ → ClF₅

IF₅ + F₂ → IF₇

Some interhalogen compounds are prepared from some halides,

KBr + 3F₂ → KF + BrF₅

KI + 4F₂ → KF + IF₇

General Properties of Interhalogen Compounds

Some of the important general properties of interhalogen compounds are:

(i) Polar Nature

All the interhalogen compounds are essentially covalent and are diamagnetic. They have some polarity. The polarity is due to the difference in electronegativity between the two halogen atoms. The more electronegative halogen atom acquires a negative charge.

(ii) Physical State

Interhalogen compounds exist as gases, liquids and solids. They are volatile solids or liquids except CIF which is a gas at 298 K. Their physical properties are intermediate between those of constituent halogens except that their melting and boiling points are a little higher than expected.

(iii) Reactivity

The interhalogen compounds have almost similar reactions to those of component halogens. However, these are generally more reactive than the component halogens (except F₂). This is because covalent bond between dissimilar atoms (X-X’) in interhalogen compounds is weaker than between similar atoms (X-X or X’-X) in halogens except F-F bond.

For example: the bond dissociation enthalpy of X-X’ bond is less than the bond dissociation enthalpy of X₂ and X₂‘. Thus, they readily convert metals into mixed halides.

2M + XX’ → MX + MX’
2Na + ICI → NaI + NaCl

(iv) Fluorinating Agents

Most of the interhalogens containing fluorine act as powerful fluorinating agents. They convert several metals into their oxides and chlorides to fluorides.

W + 6ClF → WF₆ + 3Cl₂
2AgCl + ClF₃ → 2AgF + Cl₂ + ClF

CIF₃ or BrF₃ are used for the production of UF₆ in the enrichment of uranium (²³⁶U).

(v) Hydrolysis

All the interhalogen compounds undergo hydrolysis giving halide ion (derived from the smaller halogen atom) and a hypohalite (for XX’), halite (for XX₃’), halate (for XX₅‘) and perhalate (for XX₇‘) anion derived from the larger halogen.

XX’ + H₂O → HX’ + HOX
ICI + H₂O → HCl + HOI
BrF₅ + H₂O → 5HF + HBrO₃

(v) Ionisation

Interhalogen compounds are partially ionised in the solution or in the liquid state.

For example: Fused ICI and ICI₃ have specific conductance of the order of 10 ohm^-3 cm^-1

2ICI ⇔ I⁺+ ICl₂¯
2ICl₃ ⇔ ICl₂⁺ + ICI₄¯

(vi) Oxidising Agents

The interhalogen compounds act as strong oxidising agents.

(vii) Thermal Stability

The thermal stability of the interhalogen compounds depends upon the electronegativity difference between the two component halogen atoms. In general, the thermal stability of AX type interhalogens decreases as the electronegativity difference between them decreases.

For example: Thermal stability decreases as IF > BrF > CIF > ICl > IBr > BrCl

Structures of some common Interhalogen Compounds

(a) Neutral Interhalogens

(i) XX₃’ involves sp³d hybridisation of the central halogen atom and the molecule has trigonal bipyramidal geometry with two positions occupied by lone pairs. Its structure is termed as T-shaped.

For example: CIF₃ has T-shaped structure.

(ii) XX₅‘ involves sp³d² hybridisation of the central halogen atom and the molecule has octahedral geometry with one position occupied by a lone pair. Its structure is termed as square pyramidal.

For example: IF₇ has square pyramidal structure.

(ii) XX₇’ involves sp³d² hybridisation of iodine atom and the molecule has pentagonal bipyramidal structure.

For example: IF₇ has pentagonal bipyramidal structure.

(b) Interhalogen Ions

Triatomic (XX’₂) ions

(i) XX’₂‾ ions involved sp³d hybridisation having trigonal bipyramidal geometry with three position occupied by lone pairs, The structure is linear.

For example: ICl₂‾ is linear .

(ii) XX’₄¯ involve sp³d² hybridisation having octahedral geometry with two positions occupied by lone pairs. The two lone pairs are present on positions above and below the square plane and the structure is regarded as square planar.

For example: ICl₄¯ has square planar geometry.

Evidence of Cationic lodine

All halogens are non-metallic due to high electronegativities and ionisation energies. However, the last element iodine exhibits some properties showing the presence of positive ions. The positive iodine is found in unipositive (I⁺) and tripositive (I³⁺) states.

(i) Iodine monochloride (ICl) conducts electricity in the molten state. On electrolysis, iodine is liberated at the cathode while both iodine and chlorine are liberated at the anode. The liberation of Iodine at the cathode indicates the presence of cationic iodine. The ionisation of ICl may he represented as :

2ICl ⇔ I⁺ + ICl_2¯

(ii) ICl₃ conducts electricity and on electrolysis, iodine and chlorine are liberated at both the electrodes. Therefore, the jonization may be represented as

2ICl₃⇔ ICl₂⁺+ ICl₄¯

The ions ICl₂⁺ and ICl₄¯ contain I³⁺ ions.(iii) A large number of compounds containing iodine as I³⁺ have been isolated which are ionic.

For example: iodine triacetate, I(CH₃COO)₃, iodine phosphate, IPO₄, iodine triperchlorate I(ClO₄)_3.On electrolysis, these compounds in aqueous solution liberate iodine at the cathode as:

IPO₄⇔ I³⁺ + PO₄^3-

Uses of Interhalogen Compounds

(i) The interhalogen compounds can be used as non-aqueous solvents.

(ii) Interhalogen compounds of fluorine are very useful fluorinating agents.

Pseudo Halogens

There are certain uninegative ions made up of two electronegative atoms which have properties similar to the halide ions. These are called pseudo halides. Like the halides, the pseudo halides have the corresponding pseudo halogens which behave like halogens in their chemistry.

Some Examples :

Pseudo halogens	Pseudo halides
Cyanogen :(CN)₂	Cyanide : CN^–
Thiocyanogen : (SCN)₂	Thiocyanate : SCN‾
Oxycyanogen : (OCN)₂	Cyanate : OCN¯