CHAPTER NO 1

                                 CHAPTER NO 1 
                           DEFINATIONS
CHEMISTRY: Chemistry is the branch of science which deals with the properties, composition and structure of matter.    Study of chemistry also includes the laws and principles related to the structure and interrelations of    elements and compounds.

   Chemistry has the task of investigating the materials of which our universe is made. Chemistry       investigates chemical changes, conditions under which chemical changes occur. Chemistry also deals with    the way in which similar changes can be brought about in laboratory and on a large scale in industries.

   Chemistry is a very vast field. Chemistry is divided into a number of branches such as Organic chemistry,    Inorganic chemistry, Physical chemistry, biochemistry, Applied chemistry, Nuclear chemistry etc.

1. TEMPERATURE

   Degree of hotness or coldness of a body is called "TEMPERATURE".   "Temperature is a measure of the intensity of heat".   Temperature is defined as :   "the average kinetic energy of the molecules of a body is called temperature"

SCALES OF TEMPERATURE:

   There are three scales of temperature.

   1. Celsius or centigrade scale C.

   2. Fahrenheit scale F.

   3. Kelvin or Absolute scale K.

CONVERSION

   Centigrade & Kelvin

Tk = Tc + 273

   Centigrade & Fahrenheit

C/5 = (F-32) /9

2. VOLUME

   Volume is defined as

   " The space occupied by a body is called its volume."

SYMBOL

   Volume is denoted by "V

UNITS

   a) m3   b) dm3   c) cm3   d) mm3   e) Litre   f) Milli litre

3. MASS

   The quantity of matter contained in a body is called its "Mass".

SYMBOL

   Mass is denoted by "m".

UNITS

   a) Kilogram   b) Gram   c) Milligram   d) Microgram

4. DENSITY

Mass per unit volume of a substance is called its "Density".

FORMULA
UNIT

   a) Kg / m3

   b) gm / cm3

   c) gm /litre

   d) gm / dm3

5. MOLE

"Atomic mass or formula mass or molecular mass of a

substance expressed in grams is called MOLE".Or

Mass of a substance contains 6.02 x 1023 atoms or molecules or ions is called "mole"

   For example:

   1. Atomic mass of carbon = 12 a.m.u.

   therefore 12 gram of carbon = one mole of carbon.

   2. Formula mass of Nacl = 58.5 a.m.u.

   therefore 58.5 gm of Nacl = 1 mole of Nacl.

   3. Molecular mass of CO = 28 a.m.u.

   therefore 28 gm of CO = I mole of CO

FORMULA

6. AVOGADRO'S NUMBER

   One mole of any substance contains 6.02 x 1023 atoms, molecules or ions. This particular number is    called "AVOGADRO'S NUMBER".

   It is denoted by NA.

   For Example.

   1 mole carbon = 6.02 x 1023 carbon atoms.

   1 mole Na+ = 6.02 x 1023 Na+ ions.

   1 mole H2O = 6.02 x 1023 H2O molecules.

7. LAW OF DEFINITE PROPORTION

   STATEMENT

   According to the law of definite proportion

"Every sample of pure substance always contains same elements

in fixed proportion regardless of its method of preparation"

    EXPLANATION

   We can obtain or prepare water by a number of methods but water obtained from any source always    contain 11.11% hydrogen and 88.88% oxygen.

   Similarly CO2 can be prepared by different methods but each sample of CO2 contains C=27.27% and    O=72.72%.

8. SPECIFIC GRAVITY

   Specific gravity of a substance is defined as the ratio of the mass of

substance to the mass of an equal volume of water at a particular temperature.

FORMULA

Specific gravity = mass of substance / mass of an equal volume of water

UNIT

   It has no unit.

9. GRAM ATOMIC MASS

"Atomic mass of an element expressed in gram is called gram atomic mass"

   For example:

   Gram atomic mass of C=12gm.

   Gram atomic mass of H=1 gm.

   Gram atomic mass of O=16 gm.

10. GRAM MOLECULAR MASS

"Molecular mass of a molecule expressed in grams is called gram molecular mass."

   For example:

   Gram molecular mass of hydrogen gas=2 gm.

   Gram molecular mass of oxygen gas =32gm.

   Gram molecular mass of HCl = 36.5 gm

11. ELEMENT

"Element is defined as a pure substance in which all the atoms

have same chemical properties and have same atomic number"

   For example:

   Carbon, sodium, hydrogen, chlorine, copper, gold, iron etc.

TYPES OF ELEMENTS

   Elements can be divided into two classes.

   1. Metals.

   2. Nonmetals.

METALS

   They have shine on their surface.

   They are good conductors of electricity and heat.

   They reflect light.

   Metals are ductile.

   Metals are malleable.

EXAMPLE

   Cu, Fe, Au, Na, Ca etc

NON-METALS

   They have dull surface.

   They are bad conductors of electricity and heat.

   Non-metals are non ductile.

   They cannot be drawn into sheets.

   They are brittle.

   EXAMPLE

   H2, C, Cl2, O2, N2 etc

12. VALENCY

   Valency is defined as

"the combining capacity or combining power of an element with the other element"

   In other words valency may be defined as:

   the number of H-atoms which combine with or displace one atom of an element or a radical is    called valency.

   EXAMPLES

ELEMENT	VALENCY
Na, K	1
Ca, Mg	2
F, Cl	1
N	3

13. MOLECULE

   The smallest unit of an element or compound, which can exist independently, is called "molecule".

14. EMPIRICAL FORMULA

"Empirical Formula is that formula which expresses the relative number

of each kind of atoms present in the molecule of a compound"

OR

"The formula of a compound which expresses the ratio in which atoms of

different elements are combined in a molecule"

Empirical formula only indicates atomic ratios but it does not indicate actual

number of atoms of different kinds present in the molecule of a compound.

Two or more compound may have same empirical formula.

Empirical formula is determined by experiment.

EXAMPLE

   Empirical Formula of Benzene = CH

   Empirical Formula of Glucose = CH2O

MOLECULAR FORMULA

The molecular formula of a compound is defined as:

"The formula of a compound which not only expresses the relative number of atoms of each kind but also expresses the actual number of atoms of each element present in one molecule".

Molecular formula and empirical formula of a compound are related as:

MOLECULAR FORMULA = (EMPIRICAL FORMULA)n

   Where "n" is an integer and is given by:

   n = molecular mass of compound / Empirical formula mass of compound

   Molecular formula of propane = C3H8.

   Molecular formula of sugar = C12H22O11.

SYMBOL

   A symbol is an abbreviation or short form for the chemical name of an element

   A symbol represents only one atom of an element.

   EXAMPLE:

   Carbon = C, Hydrogen= H, Chlorine = Cl, Gold = Au, Silver = Ag, Sodium = Na, bismuth = Bi etc.

FORMULA

The representation of a molecule of a substance or compound in

the form of symbols is called "formula".

   With the help of formula we can find.

   (1) Name of elements present in the molecule.

   (2) Number of atoms of each element.

   (3) Composition of compound.

   EXAMPLE:

   NH3, CO2, CaCO3, H2O, H2SO4 etc.

COMPOUND

"Compounds are pure substances, which consist of two or

more elements combined chemically in a fixed ratio."

   Compounds always have a definite composition.

   EXAMPLE:

   H2SO4, CaCl2, H2O, CO2 etc.

MIXTURE

"A mixture is a substance, which consists of two or more pure substances

not chemically combined with each other in a definite composition ."

   Mixtures do not have definite composition.

   EXAMPLE:

   Air, soil, brass ( cu + zinc) etc.

DIFFERENCE BETWEEN COMPOUND AND MIXTURE

COMPOUND                                                                           MIXTURE

1.It is a pure substance. It is an impure substance.

2. It can not be separated by physical method.         It can be separate by physical method.

3. Element loose their properties in a compound. Substances forming mixture retain their                                                                                              properties.

4.Its composition is fixed through out its mass. It has no fixed composition.

5. It has fixed melting point. It has no sharp melting point.

TYPES OF MIXTURE

 There are two types of mixture:  
 (1) Homogenous mixture.

 (2) Heterogeneous mixture.

HOMOGENEOUS MIXTURE

A homogeneous mixture is defined as "the mixture, which has uniform composition through out its mass".

   EXAMPLE:

   Air, sugar solution, salt solution, alloys, soft drinks (Pepsi, Coca-Cola etc.)

HETEROGENEOUS MIXTURE

"Mixture that do not have uniform composition through out their

mass are known as heterogeneous mixtures".

   EXAMPLE:

   Soil, rocks etc.

MATTER

Any substance which possesses mass and occupies space is called "MATTER".

Matter is the stuff of which our whole universe is made.

All matter on the earth is composed of either pure substance or a mixture of substances.

VARIABLE VALENCY

   Many elements exhibit more than one valency which is known as variable valency.

   EXAMPLE:

   Iron = Ferrous(+2), ferric (+3)

   Copper = Cuperous (+1), cuperic (+2)

   Mercury = Mercurous (+1), mercuric (+2)

MOLECULAR MASS

The molecular mass of an element when it exists in the form of molecular

or a compound in defined as the average mass of the molecule as compared to one atom of 6C12.

OR

The sum of atomic masses of all the atoms present in

one molecules of a substance is called "molecular mass".