1. CHEMISTRY CHEMISTRY IS THE SCIENCE THAT DESCRIBES MATTER. ITS CHEMICAL AND PHYSICAL PROPERTIES, THE CHEMICAL AND PHYSICAL CHANGES MATTER UNDERGOES. AND ENERGY CHANGES THAT ACCOMPANY THESE PROCESSES MATTER ANY THING WHICH OCCUPIES SPACE AND HAVING WEIGHT IS CALLED MATTER.

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

3. PHYSICAL PROPERTIES PHYSICAL PROPERTIES WHICH CAN BE OBSERVED IN THE ABSENCE OF ANY CHANGE IN COMPOSITION

4. CHEMICAL CHANGE PHYSICAL CHANGE ONE OR MORE SUBSTANCES ARE CONSUMED ONE OR MORE SUBSTANCES ARE CONSUMED ONE OR MORE NEW SUBSTANCES ARE FORMED ONE OR MORE NEW SUBSTANCES ARE FORMED CHANGE IN COMPOSITION OCCURS. CHANGE IN COMPOSITION OCCURS. ENERGY CHANGES THAT ACCOMPANY THE CHEMICAL PROCESS ENERGY CHANGES THAT ACCOMPANY THE CHEMICAL PROCESS NON OF THESE

5. BRANCHES OF CHEMISTRY ORGANIC CHEMISTRY ORGANIC CHEMISTRY INORGANIC CHEMISTRY INORGANIC CHEMISTRY ANALYTICAL CHEMISTRY ANALYTICAL CHEMISTRY PHYSICAL CHEMISTRY PHYSICAL CHEMISTRY BIO-CHEMISTRY BIO-CHEMISTRY

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

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

8. ANALYTICAL CHEMISTRY Analytical chemistry is the study of the chemical composition of natural and artificial materials. Properties studied in analytical chemistry include geometric features such as molecular morphologies and distributions of species, as well as features such as composition and species identity. Unlike the sub disciplines inorganic chemistry and organic chemistry, analytical chemistry is not restricted to any particular type of chemical compound or reaction.

9. PHYSICAL CHEMISTRY Physical chemistry (also called physico chemistry) is the explanation of macroscopic, microscopic, atomic, subatomic, and particulate phenomena in chemical systems in terms of physical concepts; sometimes using the principles, practices and concepts of physics like thermodynamics, quantum chemistry, statistical mechanics and dynamics. Physical chemistry in contrast to chemical physics is still predominantly a macroscopic or supra-molecular science, as the majority of the principles on which physical chemistry was founded are concepts related to the bulk rather than on molecular/atomic structure alone; for example, colloids, chemical equilibrium etc.

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

11. CLAFFIFICATION ACCORDING TO THE PROFESSION PHARMACEUTICAL CHEMISTRY PHARMACEUTICAL CHEMISTRY CLINICAL CHEMISTRY CLINICAL CHEMISTRY POLYMER CHEMISTRY POLYMER CHEMISTRY ENVIRONMENTAL CHEMISTRY ENVIRONMENTAL CHEMISTRY AGRICULTURAL CHEMISTRY AGRICULTURAL CHEMISTRY SOIL CHEMISTRY SOIL CHEMISTRY NUCLEAR CHEMISTRY NUCLEAR CHEMISTRY CHEMICAL ENGINEERING CHEMICAL ENGINEERING

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

13. ISTOPES ISOTOPES are atoms of the same elements containing different numbers of neutrons in their nuclei. ISOTOPES are atoms of the same elements containing different numbers of neutrons in their nuclei. Isotopes are different types of atoms (nuclides) of the same chemical element, each having a different number of neutrons. Correspondingly, isotopes differ in mass number (or number of nucleons) but not in atomic number. Isotopes are different types of atoms (nuclides) of the same chemical element, each having a different number of neutrons. Correspondingly, isotopes differ in mass number (or number of nucleons) but not in atomic number. The number of protons (the atomic number) is the same because that is what characterizes a chemical element. For example, carbon-12, carbon-13 and carbon-14 are three isotopes of the element carbon with mass numbers 12, 13 and 14, respectively. The atomic number of carbon is 6, so the neutron numbers in these isotopes of carbon are therefore 12−6 = 6, 13−6 = 7, and 14–6 = 8, respectively. The number of protons (the atomic number) is the same because that is what characterizes a chemical element. For example, carbon-12, carbon-13 and carbon-14 are three isotopes of the element carbon with mass numbers 12, 13 and 14, respectively. The atomic number of carbon is 6, so the neutron numbers in these isotopes of carbon are therefore 12−6 = 6, 13−6 = 7, and 14–6 = 8, respectively.

14. IMAGES OF ISOTOPES

15. COMPOUNDS Compounds are pure substance consisting of two or more different elements in a fixed ratio Compounds are pure substance consisting of two or more different elements in a fixed ratio

16. MIXTURES Mixtures are combination of two or more substances in which each substance retains its own composition and properties. Mixtures are combination of two or more substances in which each substance retains its own composition and properties. The composition of mixtures can be varied widely. The composition of mixtures can be varied widely. In chemistry, a mixture is when two or more different substances are mixed together but not combined chemically. In chemistry, a mixture is when two or more different substances are mixed together but not combined chemically. The molecules of two or more different substances are mixed in the form of solutions, suspensions, and colloids. The molecules of two or more different substances are mixed in the form of solutions, suspensions, and colloids.

17. HOMOGENEOUS HETEROGENEOUS Mixtures can be classified as homogeneous or heterogeneous. Mixtures can be classified as homogeneous or heterogeneous. HOMOGENEOUS MIXTURE, also called a solution, has uniform composition and properties throughout mixture. HOMOGENEOUS MIXTURE, also called a solution, has uniform composition and properties throughout mixture.

18. ATOMS An atom is the smallest particle of an element. Historically an atom has been defined as the smallest particle of an element that can enter into a chemical combination.

19. MOLECULE Molecule is the smallest particle of an element or compound that can have a stable independent existence.

20. AVOGADRO’S NUMBER Avogadro’s Number for any element, A Mass in grams numerically equal to its atomic mass contains the same no of atoms, this number is Avogadro's number. MOLE Avogadro’s number = Mole (atomic or molecular weight expessed in GMS.

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

22. THE LAW OF CONSERVATION OF MATTER States that there is no detectable gain or loss in the quantity of matter, before and after the reaction.

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

24. SOLUTION Solution may be defined as homogenous mixture of different chemical substances, which having the same chemical composition and physical properties every where. Solution may be defined as homogenous mixture of different chemical substances, which having the same chemical composition and physical properties every where..

25. CONCENTRATION OF A SOLUTION The concentration of solution is defined as: The amount of solute present in a given amount of solution. Concentration is generally expressed as the quantity of solution in a unit volume of solution. Quantity of solute Quantity of solute Concentration: ---------------------------- Volume of solution Volume of solution

26. TYPES OF SOLUTIONS. SR. NO STATE OF SOLUTE STATE OF SOLVENT E X A M P L E 1 GAS AIR 2 GASLIQUIDOXYGEN IN WATER, CO2 + WATER 3 GASSOLIDADSORPTION CFE2 BY PALLADIUM 4 LIQUID ALCOHOL IN WATER 5 LIQUIDSOLIDMERCURY IN SILVER 6 LIQUIDGASMISY 7 SOLIDLIQUIDSUGAR, SALT IN WATER 8 SOLID METAL ALLOYS, CARBON IN STEEL 9 SOLIDGASSMOKE

27. DILUTE SOLUTION A solution containing a relatively low concentration of solute is called dilute solutions. WAY OF EXPRESSING CONCENTRATION A. Percent by weight B. Mole Fraction C. Molarity D. Molality E. Normality

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

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

30. EXAMPLE Calculate the mole fraction of HCI in a solution of Hydrochloric Acid in water, containing 36% HCI by weight. Calculate the mole fraction of HCI in a solution of Hydrochloric Acid in water, containing 36% HCI by weight.

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

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

33. MOLALITY Molality (Symbol m) : It is defined as the number of moles of solute per kilogram of solvent. Moles of solute Moles of solute Molality (m) =-------------------------- Mass of solvent in Kg A solution obtained by dissolving one mole of the solute in 1000 G of solvent is called one molal or 1 m solution. Example What is the molality of a solution prepared by dissolving 5 G of toluene (C7H8) in 225 G of benzene (C6H6)?

34. NORMALITY Normality (Symbol N) : It is defined as the number of equivalents of solute per litre of solution. Equivalents of solute Equivalents of solute Normality (N)=----------------------------- Litres of solution Litres of solution