Important Definitions:

1. Chemistry
2. Atomic mass
3. Atomic number
4. Periodicity
5. Metals
6. Molarity
7. Chemical reaction
8. Radioactivity
9. Electronegativity
10. Ionization potential
11. Atomic radii
12. Formula mass
13. Mole
14. Molar mass
15. Avogadros number
16. Co-efficient
17. Brownian movement
18. Faraday
19. Coloumb
20. Ampere
21. Electron affinity
22. Homologous series
23. Functional group
24. Aliphatic hydrocarbon
25. Alicyclic hydrocarbon
26. Aromatic hydrocarbon
27. Alkanes
28. Alkenes
29. Alkynes
30. Isotopes
31. Oxidation
32. Reduction
33. Oxidizing agent
34. Reducing agent
35. Allotropy
36. Aqua regia
37. Isomerism
38. Monoprotic acid
39. Poly protic acid
40. Neutralization or titration
41. Ore
42. Minerals
43. Gangue
44. Tempering
45. sublimation

Important Differences:

1. Solution and suspension
2. Diamond and graphite
3. Saturated and unsaturated solution
4. Molarity and normality
5. Electrolytes and non electrolytes
6. Conductors and insulators
7. Ordinary and heavy water
8. Thermoplastic and thermosetting plastic
9. Alpha, beta and gema rays
10. Ionic and covalent bond
11. Covelent and co-ordinate covalent bond
12. Exothermic and endothermic reaction

Important Preparations:

1. Laboratory preparation of chlorine
2. Industrial preparation of HNO3 by Ostwald Process
3. Industrial preparation of H2SO4 by Contact process
4. Industrial Preparation of NaHCO3 sodium Bi Carbonate
5. Industrial Preparation of Caustic Soda NaOH by Castner- Kellner Cell and Nelson Cell.
6. Industrial Preparation Of Washing Soda Na2CO3.10H2O
7. Preparation of Methane
8. Preparation of Ethene
9. Preparation of Ethyne
10. Extraction of Sulphur by Herman Frasch Process

Write Properties:

1. Cathode rays
2. Anode rays
3. Periodic group V, Vll, lll
4. Ethyne gas
5. Portable water
6. Alkali metals
7. Halogens
8. Noble gases
9. Transition elements
10. Use of chlorine gas
11. Use of Ammonia gas
12. Uses of H2O2
13. Sillicon
14. Silica jel
15. Water glass
16. Methane gas
17. Hydrogen gas

Important Questions:

1. Branches of Chemistry
2. Scientific method
3. Types of Chemical reaction
4. Bohrs atomic model
5. Mandeleeve’s periodic law
6. Define solubility abd briefly write the effect of temperature on solubility.
7. Name the solute and solvent in the following solutions Butter, foam, haze
8. Electroplating and its uses
9. PH, its range and effect of raise and fall of Ph value in human blood on health.
10. Electolysis of NaCl
11. How Aqua regia dissolve gold?
12. Saponification
13. Causes of food spoilage and food preservation method
14. Oxidation and reduction in terms of transfer of electron
15. Allotropic forms of Sulphur
16. Ores of coppers and their formulae
17. Oxide and its kinds
18. Deltons atomic theory and its defects
19. Discovery of electron
20. Capacity of K shell, L Shell, and M Shell

Important laws:

1. Faraday’s first and second law of eletrolysis
2. Law of conservation of mass
3. Law of constant composition
4. Dobereiner’s law
5. Newland’s law
6. Arhenius concept of acid and base
7. Lowry and Bronsted concept
8. Lewis concept

Important Numericals:

1. Calculate the number of Oxygen atoms in 4 gm of Oxygen.
2. How many moles of Oxygen  required to burn 10 moles of ethane gas

C2H4 +3O2----------2CO2 +2H2O

1. Calculate how many grams of CaO can be obtained by heating 8 moles of CaCO3?

CaCO3--------CaO + CO2

1. Calculate the molarity of 250 ml solution containing 20gm of NaOh

A) CO2
B) H2O

1. Calculate the PH and POH of 0.001M HCl?
2. A current of 5 ampere was passed through a solution of CuSO4 for one hour, calculate the mass of the copper metal deposited on the cathode.( Z of copper = 0.000329gm/c)
3. How many grams of oxygen gas is liberated by the electrolysis of water after passing 0.0565 ampere for 185 seconds.
4. The formula for rust is Fe2O3. how many moles of Fe are present in 30 gms of rust?
5. Find no of atoms in different elements.
6. Find the empirical formula of C6H12O6.

Reasons:

1. Common salt dissolve in water but not in petrol
2. Cold drinks are bottled under a CO2 pressure greater than 1 atm.
3. 100 ml solution of KNO3 can not hold more than 37gm of KNO3 in dissolved states