Haloalkanes and Haloarenes Notes for Class 12 Chemistry

CBSE Class 12 Chemistry
Quick Revision Notes
Chapter 10

Haloalkanes and Haloarenes

• Nature of C-X bond in alkyl halides: X is more electronegative than carbon. So, the
  C-X bond is polarized with C having a partial positive charge and X having a partial
  negative charge.
• Preparation of haloalkanes:

• Preparation of haloarenes:

1. By elecrophilic substitution reaction:

b) Sandmeyer’s reaction:

Physical properties ofhaloalkanes:

a) Solubility

Although haloalkanes are polar in nature, yet they are practically very slightly soluble in
water.

In order for a haloalkane to dissolve in water, energy is required to overcome the
attractions between the haloalkane molecules and break the hydrogen bonds between
water molecules.

However Haloalkanes are not able to form hydrogen bonds with water and therefore,

less energy is released when new attractions are set up between the haloalkane and the
water molecules because these are not as strong as the original hydrogen bonds in water
molecules.

1. As a result, solubility of haloalkanes in water is low.
2. Density
3. Simple fluoro and chloroalkanes are lighter than water while bromides and
   polychlorodevrivatives are heavier than water.
4. With the increase in number of carbon atoms, the densities go on increasing. With the
   increase in number of halogen atoms, the densities go on increasing. The densities
   increase in the order: Fluoride < chloride < bromide < iodide
5. The density also increases with increasing number and atomic mass of the halogen.
6. Boiling Points
7. Molecules of organic halogen compounds are generally polar.
8. Due to the polarity as well as higher molecular mass as compared to the parent
   hydrocarbon, the intermolecular forces of attraction (dipole – dipole and van der Waals)
   between the molecules are stronger in halogen derivatives of alkanes.
9. As a result melting and boiling points of chlorides, bromides and iodides are considerably
   higher than those of the parent hydrocarbon of comparable molecular mass.
10. For the same alkyl group the boiling points of alkyl chlorides, bromides and iodides
    follow the order RI >RBr>RCl> RF where R is an alkyl group. This is because with the
    increase in the size of the halogen, the magnitude of van der Waals force increase.
11. In general, the boiling points of chloro, bromo and iodo compounds increase with
    increase in the number of halogen atoms.
12. For the same halogen atom, the boiling points of haloalkanes increase with increase in
    the size of alkyl groups.
13. For isomeric alkyl halides, the boiling points decrease with branching. This is because
    branching of the chain makes the molecule more compact and, therefore, decrease the
    surface area. Due to decrease in surface area, the magnitude of van der Waals forces of
    attraction decreases and consequently, the boiling points of the branched chain
    compound is less than those of the straight chain compounds.
14. These are generally colourless liquids or crystalline solids.
15. These are heavier than water.
16. Melting and boiling points of haloarenes
17. Melting and boiling points of haloarenes are nearly the same as those of alkyl halides
    containing the same number of carbon atoms.
18. The boiling points of monohalogen derivatives of benzene are in the order:
    iodo>bromo>chloro>fluoro
19. For the same halogen atom, the melting and boiling points increase as the size of the aryl
    group increases.
20. The melting point of para isomer is quite higher than that of ortho or meta isomers. This
    is due to the fast that is has symmetrical structure and therefore, its molecules can easily
    pack loosely in the crystal lattice. As a result intermolecular forces of attraction are stronger
    and therefore, greater energy is required to break its lattice and it melts at higher
    temperature.

• Chemical properties of haloalkanes:

Nucleophilic substitution reaction:

_ \8⁺ S“

\ ^
.C-Nu + X

*?

Reaction:

Nu + -C-X »•

/

Mechanism of Nucleophilic Substitution
SN1 Mechanism

1. First order reaction.
2. Rate = k [RX] [Nu]
3. Racemic mixture
4. One step reaction
5. Order: CH3X < 10< 20< 30

SN2 Mechanism

1. Second order reaction
2. Rate = k [RX]
3. Inversion of configuration
4. Two step reaction
5. Order: CH3X > 10> 20> 30

R – X + aq. KOH ^ R – OH + KX

R – X + NH₃ ^> R – NH₂ + HX

R -X + KCN ^ R – CN + KX

R -X + AgCN ^ R – NC + KX

• Elimination reaction: Dehydrohalogentaion(/?- elimination): When a haloalkane with
  P-hydrogen atom is heated with alcoholic solution of potassium hydroxide, there is
  elimination of hydrogen atom from p-carbon and a halogen atom from the a-carbon
  atom. As a result, an alkene is formed as a product. Zaitsev rule (also pronounced as
  Saytzeff) is followed.It states that “In dehydrohalogenation reactions, the preferred
  product is that alkene which has the greater number of alkyl groups attached to the
  doubly bonded carbon atoms.”
• Reaction with metals:

1. Reaction with Magnesium

dry ether

R -X + Mg ► RMgX

1. Wurtz reaction

R-X+2Na + X-R^R-R + 2NaX

• Chemical properties ofhaloarenes:

a) Dow’s Process

b) With halogens

c) With conc. nitric and sulphuric acid

d) On heating with conc. sulphuric acid

e) With methyl chloride

f) With acetyl chloride