(i) Due to this double bond character of C-X bond in haloarenes, the C-X bond length is shorter length and stronger than in haloalkanes.
(ii) Example:

(i) Bromoethane reacts with alcoholic KCN to form ethyl cyanide.
\(\underset { Bromoethane }{ { CH }_{ 3 }-{ CH }_{ 2 }Br+KCN } \xrightarrow [ ]{ Alcohol } \underset { Ethyl\quad eyaine }{ { CH }_{ 3 }-{ CH }_{ 2 }CN } +KBr\)
(ii) Bromoethane reacts with alcoholic AgCN to form alkyl isocyanide
\({ CH }_{ 3 }-{ CH }_{ 2 }Br+AgCN\xrightarrow [ ]{ Alcohol } \underset { Ethyl\quad eyaine }{ { CH }_{ 3 }-{ CH }_{ 2 }NC } +AgBr\)

With excess of haloalkanes, ammonia react to give primary, secondary, tertiary amines along with quarternary ammonium salt:
\(\underset { Ethyl \ bromide }{ { CH }_{ 3 }-{ CH }_{ 2 }Br+{ NH }_{ 3 } } \xrightarrow [ -HBr ]{ Alcohol } \underset { Ethylamine({ 1 }^{ 0 }) }{ { CH }_{ 3 }-{ CH }_{ 2 }{ NH }_{ 2 } } +HBr\)

C₄H₉Cl (4 isomers):
(i) CH₃-CH₂-CH₂-CH₂Cl 1-Chlorobutane
(ii)  2-Chlorobutane
(iii)  1-Chloro-2-methylpropane
(iv)  2-Chloro-2-methylpropane

The boiling points of isomeric dihalobenzene are pearly the same. The melting point of para isomer is generally higher than the melting points of ortho and meta isomers. The higher melting point of p-isomer is due to its symmetry which leads to more close packing of its molecules in the crystal lattice and consequently strong intermolecular attractive force which requires more energy for melting. p-Dihalobenzene> o-Dichlorobenzene> m-Dichloro benzene.

Uses of haloalkane :
Chloroform : As a solvent in pharmaceutical industry and for producing pesticides and drugs As an anaesthetic.
As a preservative for anatomical specimens.
Iodoform : Iodoform is used as an antiseptic for dressing wounds.
Carbon tetrachloride : Carbon tetrachloride is used as dry cleaning agent. It is used as a solvent for oils, fats and waxes. As the vapour of CCl4 is non - combustible, it is used under the name pyrene for extinguishing the fire in oil or petrol.

\(\overset { \underset { | }{ Cl } }{ \underset { \overset { | }{ Cl } }{ CH } } -{ CH }_{ 3 }\quad (A)\) 1, 1,-dichloro ethane
\(\underset { \overset { | }{ Cl } }{ { CH }_{ 2 } } -\underset { \overset { | }{ Cl } }{ { CH }_{ 2 } } \) (B) 1, 2, dichloro ethane
\(\overset { \underset { | }{ Cl } }{ \underset { \overset { | }{ Cl } }{ CH } } -{ CH }_{ 3 }\underset { aq\quad KOH }{ \longrightarrow } \left[ \overset { \underset { | }{ OH } }{ \underset { \overset { | }{ OH } }{ CH } } -{ CH }_{ 3 } \right] \underset { -{ H }_{ 2 }) }{ \longrightarrow } { CH }_{ 3 }CHO\)
(A)                                                                    (C)
1, 1, dichloro ethane                                      Acetaldhyde
\(A \ \ \overset { \underset { | }{ Cl } }{ \underset { \overset { | }{ Cl } }{ CH } } -{ CH }_{ 3 }\)  -1,1 dichloro ethane
B  \(\underset { \overset { | }{ Cl } }{ { CH }_{ 2 } } -\underset { \overset { | }{ Cl } }{ { CH }_{ 2 } } \)-1, 2 dichloro ethane
C CH₃CHO -Acetaldehyde 
D \(\underset { \overset { | }{ OH } }{ { CH }_{ 2 } } -\underset { \overset { | }{ OH } }{ { CH }_{ 2 } } \)-Ethyleneglycol

CH₂ =CH₂ +HCI⟶CH₃ -CH₂CI
(A)                   (B)
Ethene   Chloroethane
CH₃CH₂CI+ NH₃⟶CH₃CH₂NH₂
(B)                        (C)
Chloroethane        Ethyl amine
A CH₂ =CH₂      Ethene
B CH₃CH₂CI     Chloroethane
C CH₃CH₂NH₂  Ethylamine