Question
What are general characteristics of interhalogen compounds?
✓
Answer
The general characteristics of interhalogen compounds are as follows :
- In $XX \ ’_n, X$ is the halogen which has larger size and is more electropositive, while $X \ ’$ is the halogen having smaller size and is less electropositive, $n$ is the number of atoms of $X’$ attached to $X.$
- Interhalogen compounds are named as halogen halides. The more electropositive halogen is named as such and the less electropositive halogen is named as the halide. In $ClF,$ since $Cl$ is larger and more electropositive than $F,$ the interhalogen compound is named as Chlorine monofluoride,
- As the ratio of radii $($radius of $X$ : radius of $X \ ’ )$ between the atoms $X$ and $X \ ’$ increases, the number of halogen atoms $(n)$ per interhalogen compound also increases.
- The interhalogen compounds have even number of atoms i.e. $2,4,6,8.$ For example, $ClF_3$ has $4$ atoms and $BrF_5$ has $6$ atoms.
- The number of $X \ ’$ atoms in the interhalogen compounds are always odd.
- The properties of interhalogen compounds are generally intermediate between those of the halogens from which they are made.
- The oxidation state of the atom $X$ in $XX \ ’_n,$ is equal to $+1, +3, +5, +7$ and that of $X \ ’$ is $-1.$
- Since the electronegativity difference between two different halogens is low, the interhalogen compounds are covalent in nature.
- Interhalogen compounds exist as gases, liquids and solids depending upon their composition. They are volatile and less stable but not explosive.
- They are diamagnetic in nature.
- Since the interhalogen bond $(X – X \ ’)$ is weaker than parent halogens, they are more reactive than halogens.
$x- l$ so $>$ oui bruin Timor $! N$
Need a full question paper?
Generate a complete, print-ready paper with questions like this in minutes — across 16+ boards, with answer keys.
Explore more
Similar questions
Calculate the enthalpy of the reaction,
$CH _3 COOH _{( g )}+ CH _3 CH _2 OH _{( g )} \rightarrow CH _3 COOCH _2 CH _{3( g )}+ H _2 O _{( g )}$
Bond enthalpies of $O - H , C - O$, in $kJmol ^{-1}$ are 464,351 respectively.
→$CH _3 COOH _{( g )}+ CH _3 CH _2 OH _{( g )} \rightarrow CH _3 COOCH _2 CH _{3( g )}+ H _2 O _{( g )}$
Bond enthalpies of $O - H , C - O$, in $kJmol ^{-1}$ are 464,351 respectively.
Write reaction showing conversion of p- bromoisopropyl benzene into p-Isopropyl benzoic acid (3 steps).
Write reactions for the action of the following reagents on p-chlorobenzaldehyde.
Phenyl hydrazine
Phenyl hydrazine
Answer the following
How will you illustrate the use of a safer solvent and auxiliaries?
How will you illustrate the use of a safer solvent and auxiliaries?
Obtain a relation between conductivity $( k )$ and molar conductivity $\left(\wedge_m\right.$ ).
→Calculate $E ^0$ Cell, $\Delta G ^0$ and equilibrium constant for the reaction $2 Cu ^{+} \rightarrow Cu ^{2+}+ Cu$.
$E ^0 Cu ^{+} / Cu =0.52 V$ and $E ^0 Cu ^{2+}, Cu +=0.16 V$.
→$E ^0 Cu ^{+} / Cu =0.52 V$ and $E ^0 Cu ^{2+}, Cu +=0.16 V$.
Write chemical reactions for the following conversions:
(i) Ethyl bromide to ethyl methyl ether (ii) Ethyl bromide to ethene (iii) Bromobenzene to toluene. (iv) Chlorobenzene to biphenyl.
(i) Ethyl bromide to ethyl methyl ether (ii) Ethyl bromide to ethene (iii) Bromobenzene to toluene. (iv) Chlorobenzene to biphenyl.
Derive the equation $p^H + p^{OH} = 14.$
→Convert 1-chlorobutane into the following compounds :
Calculate the standard enthalpy of formation of liquid methanol from the following data:
1.$CH _3 OH _{( l )}+\frac{3}{2} O _{2( g )} \longrightarrow CO _{2( g )}+2 H _2 O _{( l )}$
$\Delta H ^{\circ}=-726 kJ mol ^{-1}$
2.$C _{(\text {Graphite })}+ O _{2( g )} \longrightarrow CO _{2( g )}$
$\Delta_{ C } H ^{\circ}=-393 kJ mol ^{-1}$
3.$H _{2( g )}+\frac{1}{2} O _{2( g )} \longrightarrow H _2 O _{( l )}$
$\Delta_{ f } H ^{\circ}=-286 kJ mol ^{-1}$
→1.$CH _3 OH _{( l )}+\frac{3}{2} O _{2( g )} \longrightarrow CO _{2( g )}+2 H _2 O _{( l )}$
$\Delta H ^{\circ}=-726 kJ mol ^{-1}$
2.$C _{(\text {Graphite })}+ O _{2( g )} \longrightarrow CO _{2( g )}$
$\Delta_{ C } H ^{\circ}=-393 kJ mol ^{-1}$
3.$H _{2( g )}+\frac{1}{2} O _{2( g )} \longrightarrow H _2 O _{( l )}$
$\Delta_{ f } H ^{\circ}=-286 kJ mol ^{-1}$