Solidification

       In solidification reaction substances changes from a liquid to a solid when its temperature is lowered below its freezing point. It is also known as freezing.
Example:
  Water changing to ice.

Saponification

               Animal fats and vegetable oils are esters of carboxylic acids. These fats and oils are called triglycerides. Triglycerides reacted with sodium or potassium hydroxide to produce fatty acid salt and glycerol. The salt of fatty acid is called soap.

*Saponification process is a hydrolysis reaction.
*Soap is produced by saponification of a triglyceride.
*Soap is a salt composed of a mixture of carboxylate anion and univalent cations.
*Sodium hydroxide produce hard soap.
*Potassium hydroxide produce soft soap.
*Potassium soaps are more soluble than sodium soaps and readily produce lather.

How Soap Clean ?
       The hydrophilic (carboxylate) end of the soap molecules attached to water. The hydrophobic (hydrocarbon chain ) end attached to oil and grease. The more and more soap molecules embedded
into a grease to forming micelles around oil droplets. The hydrophobic ends of the soap molecules attached towards the grease while the hydrophilic ends of the soap face outward into the water, resulting is an emulsion of soapy grease particles suspended in the water. Then the oily particles are easily washed away. The water agitation can help to clean greasy and oil. The micelles are dispersed into the water.

                                          Hydrophilic -  ( water loving )
                                         Hydrophobic- ( water hating )
              Soap do not work well in hard water. Hard water containing calcium and magnesium ions. these ions react with soap to form an insoluble precipitate known as soap film. This precipitate is often seen as a gray line on a bathtub or sink and is often called scum.

Detergents:
       Detergents are similar to soaps. They work in both soft and hard water. The detergent removes the oil film and the dirt can be washed away.

Solidification

          Substance changes from a liquid phase to solid phase when its temperature is lowered below its freezing point. it is also known as freezing.

Saponification

              Triglycerides reacted with sodium or potassium hydroxide to produce fatty acid salt and glycerol.

Rusting of Iron

         Iron combine with oxygen in the presence of water molecule to form a iron oxides. (rust).

Combustion

                 Energetic molecules (hydrocarbons) combine with oxygen to produce carbon-dioxide and water.

Aerobic Respiration

             Respiration helps to breaks down glucose into carbon-dioxide and water.

Photosynthesis

               In the presence of sunlight carbon-dioxide and water molecule reacts to form a glucose (food) and oxygen.

Izomerization

               In this process compounds are transformed into any of its isomeric forms. ( same atom but different molecular rearrangements).

Acid-Base Reaction

Lewis Definition:

   Acids are electron pair acceptors. ( lewis acid ).

   Bases are electron pair donors. ( lewia base ).

Double Displacement Reaction

                 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 Metathesis reaction.

Single Displacement Reaction

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

Decomposition Reaction

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

Synthesis Reaction

              A chemical reaction of two or more substances react to give a single product. It is also known as combination.

Rusting Of Ion

               Irons form a red-brown stuff that is called rust. Rusting of iron is a chemical process. In this case iron combine with oxygen in the presence of water molecules to form a iron oxide.

Fe   +   O₂   +   H₂O   →   Fe₂O₃.XH₂O

Combustion

             Energetic molecules combine with oxygen to produce carbon-dioxide and water. Combustion reaction is a exothermic reaction. So it release heat.
Example:

C₃H₈   +   5O₂   →   4H₂O   +   3CO₂   +   Energy ( Heat )

            Burning, light a grill, strike a match sticks combustion of propane gas these are the combustion reactions.

Aerobic Respiration

                 Respiration helps to breaks down glucose into carbon-dioxide and water. Energy used by cells is chemical energy in the form of ATP ( adenosine triphosphate ). Aerobic respiration is the opposite process of photosynthesis.

C₆H₁₂O₆+   6O₂   →   6CO₂   +   6H₂O   +   Energy ( 36 ATPs )

Photosynthesis

              Photosynthesis is a chemical reaction by which green plants make their own food. In the presence of sun light carbon-dioxide and water molecule react to form a glucose ( Food ) and oxygen. This is the most common everyday chemical reaction.

6CO₂   +   6H₂O   +   light   →   C₆H₁₂O₆   +   6O₂

Formation Of Covalent Bond

                    Covalent bond occurs between the non-metal. Two atoms share their valence electrons. The two atoms sharing the outer most ( valence ) electron each other.

Formation Of Ionic Bond

                   Usually metals have low ionization energy, so that metals (Na) release some of their electrons to attain a stable configuration. Now the atoms becomes cations. Some of the non-metals (Cl) electron affinity is positive, so that non-metals accept the electron to attain a stable configuration. Anions are formed.

Example :

Na   +   Cl   →   Na⁺   +   Cl^-

Na⁺   +   Cl^-   →   NaCl

     A piece of sodium metal atom react with chlorine gas a vigorous reaction takes place, it will give sodium chloride a common table salt.

Key Point :

         Electron transfer from metal to non-metal atom.

                       Sodium atom transfer an electron to the chlorine atom the ions attract each other to form Na+ and Cl- ions. The lose of electrons from the sodium atom into a positively charged Na+ ions. ( cations ). The gain of electrons from the chlorine atom into a negatively charged Cl- ions. (Anions ). The cations and anions combine to form NaCl.

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  

Types Of Colloidal Dispersion

Solute	Solvent	Dispersion	Name	Example
Solid	Solid	Solid In Solid	Solid Sol	Pearl, Gemstone
Solid	Liquid	Solid In Liquid	Sol	Ink
Solid	Gas	Solid In Gas	Solid Aerosol	Dust, Smoke
Liquid	Solid	Liquid In Solid	Gel	Cheese, Butter
Liquid	Liquid	Liquid In Liquid	Emulsion	Milk
Liquid	Gas	Liquid In Gas	Liquid Aerosol	Cloud, Fog
Gas	Solid	Gas In Solid	Solid Foam	Cork
Gas	Liquid	Gas In Liquid	Foam	Soda water, Soap

Types Of Solution

SOLUTE	SOLVENT	TYPE	EXAMPLE
Solid                                ( Zinc )	Solid                ( Copper )	Solid In Solid	Brass
Liquid             ( Mercury )	Solid                ( Silver )	Liquid In Solid	Dental Amalgam
Solid                ( Salt )	Liquid                ( Water )	Solid In Liquid	Seawater
Liquid                 ( Acetic Acid )	Liquid               ( Water )	Liquid In Liquid	Vinegar
Gas                 ( CO2 )	Liquid              ( Water )	Gas In Solid	Soda Water
Gas              ( Air )	Gas                 ( Nitrogen )	Gas In Gas	Air

Relationship Between Atomic Number, Mass Number and Istope

* For Example :   In Carbon-12 and Carbon-14,
¹²₆C                                                          ¹⁴₆C
Neutron - 6                                             Neutron - 8
Proton    - 6                                             Proton    - 6
Electron - 6                                              Electron - 6
Carbon-12 and carbon-14 have same atomic number and different mass number. It's known as isotopes.

* A number of proton in an atom is known as atomic number. Carbon-12 and carbon-14 both of them ontain 6 protons so that the atomic number is 6.
                 Z = 6
Z ==> Atomic number.

*    In carbon-12 , the mass number is 12 and the atomic number is 6. Mass number is bigger than the atomic number.Mass number is equal to the total number of protons and neutrons.

Butyric Acid

          Butyric acid molecular is C₄H₈O<sub>2. It is a carboxylic acid and unpleasant smell. It is also known as butanoic acid and butyrates.

Sources :  Goat, Sheep, Buffalo and milk.</sub>

Stearic Acid

               Stearic acid molecular formula is C₁₈H₃₆O<sub>2. It is a waxy solid. Stearic acid is a saturated fatty acid and also it is a colorless and odorless acid.

Source:  Animal fat And vegetable oil.</sub>

Lactic Acid

          Lactic acid molecular formula is C₃H₆O<sub>3. It is otherwise known as milk acid. Lactic acid has two optical isomers. One is known as L (+) Lactic acid Or (S) Lactic acid and its mirror image is D  (-)  Lactic acid or (R) lactic acid. Lactic acid is chiral. It is a syrupy carboxylic acid miscible with water or ethanol. Synthetic form of lactic acid used as a preservative in textile and pharmaceuticals.

Source :
      Dairy product, Soy sauce, Pickled vegetables.</sub>

Uric Acid

           Uric acid molecular formula is C₅H₄N₄O<sub>3. Uric acid is a white odorless,tasteless, crystalline product of protein metabolism, present in the blood and urine. It is hetero cyclic compound. High blood concentration of uric acid can lead to gout. 

Source :
        Lamb, Beef, Pork, Spinach, Cauliflower etc.</sub>

Acetic Acid

                    Acetic acid molecular formula is C₂H₄O<sub>2. It is a weak organic acid. It gives source taste and pungent smell. It is otherwise known ethanoic acid or methane carboxylic acid.

Source :  Vinegar.</sub>

Cholic Acid

            Cholic acid molecular formula is  C₂₄H₄₀O_{5. It is a white crystalline substance. It is insoluble in water. Chloic acid is the important human bile acid. ( Bile acids are steroid acids found in the bile of mammals.}

Citric Acid

            Citric acid molecular formula is C₆H₈O₇ . It is a weak organic acid. It gives source taste to food and drinks. And also it is used as a natural preservative. It is also known as 3-carboxy-3-hydroxy pentanedioic acid. It is a white crystalline powder at room temperature.

Source: 
    Lemon, Berries, Tomatoes, pineapple.

Bleaching Powder

        It's chemical name is calcium hypochlorite. Chemical formula is Ca(ClO)_{2. It is otherwise known as bleaching powder or calcium oxychloride. It is mostly used for water treatment as a bleaching agent.}