Isomerization

             Isomerization is a chemical process. In this process compounds is transformed into any of its isomeric forms. ( same atom but different molecular rearrangements.

Examples :
             Pentane, hydrocarbon with five carbon atoms joined in a straight chain to its branched chain isomer 2-methylbutane and 2,2-dimethylpropane.

             In gasoline manufacturing, straight chain hydrocarbons are converted into branched chain hydrocarbons in the presence of a catalyst.

Hydrolysis Reaction

                    Hydrolysis is a chemical reaction that involves a salt reacting with water to produce hydrogen ions and hydroxide ions. It is a type of decomposition reaction one reactant is water. Hydrolysis means " water separation ".
Example:

CH₃COOH    +   H₂O   →   H₃O⁺   +   CH₃COO^-

NH₃   +   H₂O     →    NH₄⁺   +    OH^-

H₂SO₄   +   H₂O    →   H₃O⁺   +   HSO4^-

HCN   +   H₂O   →   H₃O⁺   +   CN^-

Combustion Reaction

     Combustion reaction is a chemical reaction. In this reaction hydrocarbons react with oxygen to give carbon-dioxide and water. It is a exothermic reaction so it release heat.

Types :
*Complete combustion reaction
*Incomplete combustion reaction.

Complete reaction :
     In this of reaction hydrocarbons react with oxygen to gives carbon-dioxide and water. Here the oxygen fully react with reactants to gives product.

Incomplete reaction :
     In this types not enough oxygen in reactants. so it will react to give carbon, carbon-monoxide and carbon-dioxide.

Examples :

( C, H and O )   +   O₂   →   CO₂   +   H₂O   +   Heat

CH₄   +   2O₂   →   CO₂   +   2H₂O   +   Heat

C₁₀H₈   +   12O₂   →   10CO₂   +   4H₂O   +   Heat

C₃H₈   +   5O₂   →   3CO₂   +   4H₂O   +   Heat

2CH₃OH   +   3O₂   →   2CO₂   +   4H₂0   +   Heat

Redox Reaction ( Oxidation - Reduction reaction )

            Redox reaction is a chemical reaction, that involves electron transfer between two chemical species.
* loss of an electron is oxidized
*gain of an electron is reduced.
It is also known as oxidation - reduction reaction.

Example:

Redox reaction :
 H₂   +   F₂   →   2HF
overall reaction may be written as two half - reaction.

Oxidation reaction :

H₂   →   2H⁺   +   2e^-

Reduction reaction :

F₂   +   2e^-   →   2F^-

Now we adding the reactions together the electrons are canceled.
                 H₂   →   2H⁺   +   2e^-

F₂   +   2e^-   →   2F-

----------------------------------------

H₂   +  F₂    →   2H⁺   +   2F^-

2H⁺   +   2F^{-  combine to give 2HF.}

Acid-Base Reaction

Lewis Definition :
       Acid - base reaction is a chemical reaction. In this reaction acids are electron pair acceptors (lewis acid ). Bases are electron pair donars ( Lewis base ).

General Formula :

A⁺   +   B^-    →   A-B

Example :

BF₃   +   F^-   →   BF4^-

HCl   +   OH^-  →   H2O  +  Cl^-

H⁺    +   OH^- →   H2O

H⁺    +  NH3  →   NH4⁺

COCl⁺  +  Cl^-  →   COCl2

Double displacement Reaction ( Metathesis )

                        In double displacement reaction one of the part of reactant is replaced by another part of reactant. The two reactant replaces to forming two new compounds or product. It is also known as double displacement reaction or metathesis reaction.

General Formula :
AB  +  CD     ---->   AD  +  CB  

Example :

AgNO₃   +   NaCl    →   AgCl   +   NaNO₃

AgNO₃   +   HCl     →   AgCl    +   HNO₃

NaOH    +    HCl     →   NaCl    +   H₂O

Li₂SO₄   +  BaCl₂  →   2LiCl    +   BaSO₄

Na₂SO₃ +  2HNO₃  →  2NaNO₃   +   H₂SO₂

Single Displacement Reaction ( Substitution Reaction )

                       In single displacement reaction one element replaced from a compound by another element. It is also known as substitution reaction or single replacement reaction.

Types  :
* cation replacement . ( positively charged ions mostly metals )
* anion replacement . ( negatively charged ions  mostly non-metals )

General Formula :
A     +      BC        ---->       AB     +       C
A     +      BC        ---->       AC     +       B

Examples:

Cl₂  +  2NaBr    →   2NaCl   +   Br₂

Cu   +   2AgNO₃  → Cu(NO₃)   +   2Ag

Zn    +  2HCl    →  ZnCl₂   +  H₂

Fe    +  CuSO₄  →   FeSO₄     +   Cu

Zn    +  CuCl₂    →  ZnCl₂  +  Cu

Cl₂   +   2KBr    →  2KCl   +  Br₂

Br₂   +   2KI     →   2KBr   +   I₂

Decomposition Reaction ( Analysis Reaction )

                          In decomposition reaction a compound is broken into elements or simpler compounds. It is also known analysis reaction.

General Reaction:
            AB       ----->   A     +      B

Example :
Split into two elements.

2H₂O    →   2H₂    +   O₂

MgCl₂    →  Mg    +   Cl₂

2KCl    →     2K    +     Cl₂

FeS       →  Fe    +    S

2KClO₃    →   2KCl     +    3O₂

Split into two simpler compounds.

CaCO₃  →  CaO  +  CO₂

H₂CO₃  →  H₂O  +  CO₂

Na₂CO₃  →  Na₂O  +  CO₂

Synthesis Reaction ( Combination Reaction )

                    A chemical reaction of two or more substances react to give a single product. It is also known as combination.
General Formula :
      A     +       B       ---->     AB
A and B are elements or compound.

Example:

2Na  +  Cl₂  →  2NaCl

8Fe  +  S₈   →  8FeS

Cao  +  H₂O  →  Ca(OH)₂

2CO  +  O₂  →  2CO₂

4Fe  +  3O₂  →  2Fe₂O₃

Zn  +  I₂    →  ZnI₂