some about by chemistry

1. CHEMISTRYCHEMISTRY
CHEMISTRY IS THE SCIENCE THATCHEMISTRY IS THE SCIENCE THAT
DESCRIBES MATTER. ITS CHEMICALDESCRIBES MATTER. ITS CHEMICAL
AND PHYSICAL PROPERTIES, THEAND PHYSICAL PROPERTIES, THE
CHEMICAL AND PHYSICAL CHANGESCHEMICAL AND PHYSICAL CHANGES
MATTER UNDERGOES. AND ENERGYMATTER UNDERGOES. AND ENERGY
CHANGES THAT ACCOMPANY THESECHANGES THAT ACCOMPANY THESE
PROCESSESPROCESSES
MATTER ANY THING WHICH OCCUPIESMATTER ANY THING WHICH OCCUPIES
SPACE AND HAVING WEIGHT IS CALLEDSPACE AND HAVING WEIGHT IS CALLED
MATTER.MATTER.

2. CHEMICAL PROPERTIESCHEMICAL PROPERTIES
CHEMICAL PROPERTIES ARE PROPERTIESCHEMICAL PROPERTIES ARE PROPERTIES
THAT MATTER EXHIBITS AS ITTHAT MATTER EXHIBITS AS IT
UNDERGOES CHANGES IN COMPOSITIONUNDERGOES CHANGES IN COMPOSITION

3. PHYSICAL PROPERTIESPHYSICAL PROPERTIES
PHYSICAL PROPERTIES WHICH CAN BEPHYSICAL PROPERTIES WHICH CAN BE
OBSERVED IN THE ABSENCE OF ANYOBSERVED IN THE ABSENCE OF ANY
CHANGE IN COMPOSITIONCHANGE IN COMPOSITION

4. CHEMICAL CHANGE PHYSICALCHEMICAL CHANGE PHYSICAL
CHANGECHANGE
• ONE OR MOREONE OR MORE
SUBSTANCES ARESUBSTANCES ARE
CONSUMEDCONSUMED
• ONE OR MORE NEWONE OR MORE NEW
SUBSTANCES ARESUBSTANCES ARE
FORMEDFORMED
• CHANGE IN COMPOSITIONCHANGE IN COMPOSITION
OCCURS.OCCURS.
• ENERGY CHANGES THATENERGY CHANGES THAT
ACCOMPANY THEACCOMPANY THE
CHEMICAL PROCESSCHEMICAL PROCESS
NON OF THESENON OF THESE

5. BRANCHES OF CHEMISTRYBRANCHES OF CHEMISTRY
• ORGANIC CHEMISTRYORGANIC CHEMISTRY
• INORGANIC CHEMISTRYINORGANIC CHEMISTRY
• ANALYTICAL CHEMISTRYANALYTICAL CHEMISTRY
• PHYSICAL CHEMISTRYPHYSICAL CHEMISTRY
• BIO-CHEMISTRYBIO-CHEMISTRY
(09-05-2012 Evening)(09-05-2012 Evening)

6. ORGANIC CHEMISTRY
Organic chemistry is a discipline withinOrganic chemistry is a discipline within
chemistry which involves the scientific study ofchemistry which involves the scientific study of
the structure, properties, composition,the structure, properties, composition,
reactions, and preparation (by synthesis or byreactions, and preparation (by synthesis or by
other means) of chemical compounds thatother means) of chemical compounds that
contain carbon. These compounds maycontain carbon. These compounds may
contain any number of other elements,contain any number of other elements,
including hydrogen, nitrogen, oxygen, theincluding hydrogen, nitrogen, oxygen, the
halogens as well as phosphorus, silicon andhalogens as well as phosphorus, silicon and
sulfur.sulfur.

7. INORGANIC CHEMISTRYINORGANIC CHEMISTRY
Inorganic chemistry is the branch ofInorganic chemistry is the branch of
Chemistry concerned with the properties andChemistry concerned with the properties and
behavior of inorganic compounds. This fieldbehavior of inorganic compounds. This field
covers all chemical compounds except thecovers all chemical compounds except the
organic/myriad compounds (compoundsorganic/myriad compounds (compounds
containing C-H bonds), which are the subjectscontaining C-H bonds), which are the subjects
of organic chemistry.of organic chemistry.

8. ANALYTICAL CHEMISTRYANALYTICAL CHEMISTRY
Analytical chemistry is the study of theAnalytical chemistry is the study of the
chemical composition of natural and artificialchemical composition of natural and artificial
materials. Properties studied in analyticalmaterials. Properties studied in analytical
chemistry include geometric features as wellchemistry include geometric features as well
as features such as composition and speciesas features such as composition and species
identity. Unlike the sub disciplines inorganicidentity. Unlike the sub disciplines inorganic
chemistry and organic chemistry, analyticalchemistry and organic chemistry, analytical
chemistry is not restricted to any particularchemistry is not restricted to any particular
type of chemical compound or reaction.type of chemical compound or reaction.

9. PHYSICAL CHEMISTRYPHYSICAL CHEMISTRY
Physical chemistry (also called physico chemistry) is thePhysical chemistry (also called physico chemistry) is the
explanation of macroscopic, microscopic, atomic,explanation of macroscopic, microscopic, atomic,
subatomic, and particulate phenomena in chemicalsubatomic, and particulate phenomena in chemical
systems in terms of physical concepts; sometimes usingsystems in terms of physical concepts; sometimes using
the principles, practices and concepts of physics likethe principles, practices and concepts of physics like
thermodynamics, quantum chemistry, statisticalthermodynamics, quantum chemistry, statistical
mechanics and dynamics.mechanics and dynamics.

10. BIO CHEMISTRYBIO CHEMISTRY
BiochemistryBiochemistry is the study of the chemicalis the study of the chemical
processes in living organisms. It deals with theprocesses in living organisms. It deals with the
structure and function of cellular components suchstructure and function of cellular components such
as proteins, carbohydrates, lipids, nucleic acids andas proteins, carbohydrates, lipids, nucleic acids and
other biomolecules.other biomolecules.

11. CLASIFICATION ACCORDING TOCLASIFICATION ACCORDING TO
THE PROFESSIONTHE PROFESSION
• PHARMACEUTICAL CHEMISTRYPHARMACEUTICAL CHEMISTRY
• CLINICAL CHEMISTRYCLINICAL CHEMISTRY
• POLYMER CHEMISTRYPOLYMER CHEMISTRY
• ENVIRONMENTAL CHEMISTRYENVIRONMENTAL CHEMISTRY
• AGRICULTURAL CHEMISTRYAGRICULTURAL CHEMISTRY
• SOIL CHEMISTRYSOIL CHEMISTRY
• NUCLEAR CHEMISTRYNUCLEAR CHEMISTRY
• CHEMICAL ENGINEERINGCHEMICAL ENGINEERING

12. SUBSTANCESSUBSTANCES
A pure substances is any kind of matter, allA pure substances is any kind of matter, all
samples of which have identical compositionsamples of which have identical composition
and under identical conditions has identicaland under identical conditions has identical
properties.properties.

13. ISTOPESISTOPES
• ISOTOPES are atoms of the same elementsISOTOPES are atoms of the same elements
containing different numbers of neutrons in theircontaining different numbers of neutrons in their
nuclei.nuclei.
• IsotopesIsotopes are different types of atoms (nuclides) ofare different types of atoms (nuclides) of
the same chemical element, each having a differentthe same chemical element, each having a different
number of neutrons. Correspondingly, isotopes differnumber of neutrons. Correspondingly, isotopes differ
in mass number (or number of nucleons) but not inin mass number (or number of nucleons) but not in
atomic number.atomic number.
• The number of protons (the atomic number) is theThe number of protons (the atomic number) is the
same because that is what characterizes a chemicalsame because that is what characterizes a chemical
element. For example, carbon-12, carbon-13 andelement. For example, carbon-12, carbon-13 and
carbon-14 are three isotopes of the element carboncarbon-14 are three isotopes of the element carbon
with mass numbers 12, 13 and 14, respectively. Thewith mass numbers 12, 13 and 14, respectively. The
atomic number of carbon is 6, so the neutron numbersatomic number of carbon is 6, so the neutron numbers
in these isotopes of carbon are therefore 12−6 = 6,in these isotopes of carbon are therefore 12−6 = 6,
13−6 = 7, and 14–6 = 8, respectively. date 9-5-1213−6 = 7, and 14–6 = 8, respectively. date 9-5-12

14. COMPOUNDSCOMPOUNDS
• Compounds are pure substanceCompounds are pure substance
consisting of two or more differentconsisting of two or more different
elements in a fixed ratioelements in a fixed ratio

15. MIXTURESMIXTURES
• Mixtures are combination of two or moreMixtures are combination of two or more
substances in which each substance retains itssubstances in which each substance retains its
own composition and properties.own composition and properties.
• The composition of mixtures can be variedThe composition of mixtures can be varied
widely.widely.
• In chemistry, aIn chemistry, a mixturemixture is when two or moreis when two or more
different substances are mixed together but notdifferent substances are mixed together but not
combined chemically.combined chemically.
• The molecules of two or more differentThe molecules of two or more different
substances are mixed in the form of solutions,substances are mixed in the form of solutions,
suspensions, and colloids.suspensions, and colloids.

16. HOMOGENEOUSHOMOGENEOUS
HETEROGENEOUSHETEROGENEOUS
• Mixtures can be classified as homogeneousMixtures can be classified as homogeneous
or heterogeneous.or heterogeneous.
• HOMOGENEOUS MIXTURE, also called aHOMOGENEOUS MIXTURE, also called a
solution, has uniform composition andsolution, has uniform composition and
properties throughout mixture.properties throughout mixture.

17. ATOMSATOMS
An atom is the smallest particle of an element.An atom is the smallest particle of an element.
Historically an atom has been defined as theHistorically an atom has been defined as the
smallest particle of an element that can entersmallest particle of an element that can enter
into a chemical combination.into a chemical combination.

18. MOLECULEMOLECULE
Molecule is the smallest particle of an elementMolecule is the smallest particle of an element
or compound that can have a stableor compound that can have a stable
independent existence.independent existence.

19. AVOGADRO’S NUMBERAVOGADRO’S NUMBER
Avogadro’s Number for any element, A MassAvogadro’s Number for any element, A Mass
in grams numerically equal to its atomic massin grams numerically equal to its atomic mass
contains the same no of atoms,=6.02xcontains the same no of atoms,=6.02x1023
this number is Avogadro's number.this number is Avogadro's number.
MOLEMOLE
Avogadro’s number = Mole (atomic or molecularAvogadro’s number = Mole (atomic or molecular
weight expressed in GMS.weight expressed in GMS.

20. Avogadro number connects massesAvogadro number connects masses
with number of atoms. It enable us towith number of atoms. It enable us to
define a convenient unit for dealingdefine a convenient unit for dealing
quantitatively with what takes place inquantitatively with what takes place in
chemical reaction.chemical reaction.
AN IONSAN IONS
An ion is an atom or group of atomsAn ion is an atom or group of atoms
that carries an electrical charge.that carries an electrical charge.

21. THE LAW OF CONSERVATION OFTHE LAW OF CONSERVATION OF
MATTERMATTER
States that there is no detectable gain or loss inStates that there is no detectable gain or loss in
the quantity of matter, before and after thethe quantity of matter, before and after the
reaction.reaction.

22. DALTON’S ATOMIC THEORYDALTON’S ATOMIC THEORY
Dalton’s ideas may be stated as follows:Dalton’s ideas may be stated as follows:
• An element is composed of extremely smallAn element is composed of extremely small
individual particles called atoms.individual particles called atoms.
• All atoms of a given element have identicalAll atoms of a given element have identical
properties which differ from those of otherproperties which differ from those of other
element.element.
• Atoms can not be created, destroyed, orAtoms can not be created, destroyed, or
transformed into atoms of an other element.transformed into atoms of an other element.
• Compounds are formed when atoms of differentCompounds are formed when atoms of different
element combine with each other in simpleelement combine with each other in simple
numerical ratio.numerical ratio.

23. SOLUTIONSOLUTION
• Solution may be defined asSolution may be defined as
homogenous mixture ofhomogenous mixture of
different chemical substances,different chemical substances,
which having the samewhich having the same
chemical composition andchemical composition and
physical properties everyphysical properties every
where.where.
..

24. CONCENTRATION OF ACONCENTRATION OF A
SOLUTIONSOLUTION
The concentration of solution is defined as:The concentration of solution is defined as:
The amount of solute present in a givenThe amount of solute present in a given
amount of solution. Concentration is generallyamount of solution. Concentration is generally
expressed as the quantity of solution in a unitexpressed as the quantity of solution in a unit
volume of solution.volume of solution.
Quantity of soluteQuantity of solute
Concentration: ----------------------------Concentration: ----------------------------
Volume of solutionVolume of solution

25. TYPES OF SOLUTIONSTYPES OF SOLUTIONS
..SR.
NO
STATE OF
SOLUTE
STATE OF
SOLVENT
E X A M P L E
1 GAS GAS AIR
2 GAS LIQUID OXYGEN IN WATER, CO2 + WATER
3 GAS SOLID ADSORPTION CFE2 BY PALLADIUM
4 LIQUID LIQUID ALCOHOL IN WATER
5 LIQUID SOLID MERCURY IN SILVER
6 LIQUID GAS MISY
7 SOLID LIQUID SUGAR, SALT IN WATER
8 SOLID SOLID METAL ALLOYS, CARBON IN STEEL
9 SOLID GAS SMOKE

26. DILUTE SOLUTIONDILUTE SOLUTION
A solution containing a relatively lowA solution containing a relatively low
concentration of solute is called diluteconcentration of solute is called dilute
solutions.solutions.
WAY OF EXPRESSING CONCENTRATIONWAY OF EXPRESSING CONCENTRATION
A.A. Percent by weightPercent by weight
B.B. Mole FractionMole Fraction
C.C. MolarityMolarity
D.D. MolalityMolality
E.E. NormalityNormality

27. PERCENT BY WEIGHT.PERCENT BY WEIGHT.
It is the weight of the solute as a percent of the totalIt is the weight of the solute as a percent of the total
weight of the solution.weight of the solution.
Wt. of soluteWt. of solute
% By weight of solute = ---------------- X 100% By weight of solute = ---------------- X 100
Wt. of SolutionWt. of Solution
EXAMPLE:EXAMPLE:
If a solution of HCI contains 36% HCI by weight, itIf a solution of HCI contains 36% HCI by weight, it
has 36 GM of HCI for 100 G of solution.has 36 GM of HCI for 100 G of solution.
EXAMPLE:EXAMPLE:
What is the % by weight of NaCl if 1.75 G of NaCl isWhat is the % by weight of NaCl if 1.75 G of NaCl is
dissolved in 5.85 G of water.dissolved in 5.85 G of water.

28. MOLE FRACTIONMOLE FRACTION
(It is denoted by X) of solute is defined as the ratio(It is denoted by X) of solute is defined as the ratio
of the number of moles of solute and the totalof the number of moles of solute and the total
number of moles of solute and solvent:number of moles of solute and solvent:
Moles of soluteMoles of solute
X solute = --------------------------------------------X solute = --------------------------------------------
Moles of solute + Moles of solventMoles of solute + Moles of solvent
n Nn N
X Solute +--------- X Solvent------------X Solute +--------- X Solvent------------
n + N n + Nn + N n + N
X Solute + X Solvent = 1X Solute + X Solvent = 1

29. EXAMPLEEXAMPLE
• Calculate the mole fraction of HCI in aCalculate the mole fraction of HCI in a
solution of Hydrochloric Acid in water,solution of Hydrochloric Acid in water,
containing 36% HCI by weight.containing 36% HCI by weight.

30. MOLARITYMOLARITY
(Symbol M) It is defined as No of moles of solute per(Symbol M) It is defined as No of moles of solute per
litre of solution. If n is the number of moles of solutelitre of solution. If n is the number of moles of solute
and V litres . The volume of solution.and V litres . The volume of solution.
Moles of soluteMoles of solute
Molarity= ----------------------Molarity= ----------------------
Volume in LitresVolume in Litres
nn
Molarity = ---------------------Molarity = ---------------------
V (in Litres)V (in Litres)
If one mole of solute is dissolved in one litre ofIf one mole of solute is dissolved in one litre of
solution then concentration of solution will be onesolution then concentration of solution will be one
molar or 1 M.molar or 1 M.

31. Example-1Example-1
What is the molarity of a solution preparedWhat is the molarity of a solution prepared
by dissolving 75.5 G of pure KOH in 540 MLby dissolving 75.5 G of pure KOH in 540 ML
of solution.of solution.
Example – 2Example – 2
What weight of Hcl is present in 155 ML of aWhat weight of Hcl is present in 155 ML of a
0.540 M Solution.0.540 M Solution.

32. MOLALITYMOLALITY
Molality (Symbol m) : It is defined as the number ofMolality (Symbol m) : It is defined as the number of
moles of solute per kilogram of solvent.moles of solute per kilogram of solvent.
Moles of soluteMoles of solute
Molality (m) =Molality (m) = ----------------------------------------------------
Mass of solvent in KgMass of solvent in Kg
A solution obtained by dissolving one mole of theA solution obtained by dissolving one mole of the
solute in 1000 G of solvent is called one molal or 1 msolute in 1000 G of solvent is called one molal or 1 m
solution.solution.
ExampleExample
What is the molality of a solution prepared byWhat is the molality of a solution prepared by
dissolving 5 G of toluene (C7H8) in 225 G of benzenedissolving 5 G of toluene (C7H8) in 225 G of benzene
(C6H6)?(C6H6)?

33. NORMALITYNORMALITY
Normality (Symbol N) : It is defined as theNormality (Symbol N) : It is defined as the
number of equivalents of solute per litre ofnumber of equivalents of solute per litre of
solution.solution.
Equivalents of soluteEquivalents of solute
Normality (N)=Normality (N)= ----------------------------------------------------------
Litres of solutionLitres of solution