Chemistry class 9thClass Matric Part 1 Notes

9th class chemistry guess paper

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unit no 1

1. Define organic chemistry?

2. Define term “Anion” and give one example?

3. How many molecules of water are present in half mole of water?

4. Write any three differences between compound and mixture?

5. Define industrial and analytical chemistry?

6. What is the Relative Atomic Mass? How it is related to gram?

7. Write the chemical formulas of caustic soda and washing soda?

8. How to write a chemical formula?

9. Define molecular formula and give example?

10. Calculate the formula mass of nitric Acid HNO3.

11. Define free radical and give example.

12. Difference between compound and mixture.

13. Calculate the number of moles and Atoms present in 6 Grams of water?

14. Difference between Biochemistry and industrial Chemistry?

15. What is meant by molecular formula explains with an example.

16. Write three differences between Atom and Ion.

17. Write four differences between molecule and molecularion.

18. Define organic Chemistry?

19. Differentiate between physical and chemical properties.

20. What is the Valency of following elements?

21. Define Element and classify the elements with examples

22. Define mole and give one example.

23. Define organic and inorganic Chemistry

24. Calculate the Molecular Mass of Nitric Acid (HNO3)

25. What is the difference between Solution and Mixture?

26. Explain Empirical formula and Molecular formula with example.

27. Define industrial chemistry.

28. Define chemical properties and give example.

29. Write two significance of chemical formula.

30. Define empirical formula and give one example.

31. Give any two example of application in biochemistry.

32. How does homogeneous mixture differ from heterogeneous mixture?

33. Define Element.

34. What is a molecule? Write four characteristics of molecular ion.

35. Explain different types of molecules with the help of example.

36. Write any five properties of mixture.

unit no 2

1. Define carbon dating.

2. Write down the electronic configuration of be and ne.

3. Give the applications of isotopes in the field of radiotherapy and medicines.

4. Write two characteristics of cathode rays.

5. Write two defects in Rutherford’s atomic model.

6. Write the electronic configuration of an element having 11 electrons.

7. Write the results of experiments of Rutherford’satomic model.

8. A patient has goiter. How will it be detected?

9. Write down the two characteristics of canal rays.

10. Write down the electronic configuration of chlorineion.

11. Define shielding effect.

12. Define electronic configuration.

13. How does electron differ form a neutron?

14. Name the elements represented by give symbols.

15. State any three properties of cathode rays.

16. How isotopes are useful for us?

17. Write the properties of neutron.

18. Define isotopes. Name the isotopes of hydrogen.

19. Write down any three properties of canal rays.

20. Define nuclear fission reaction with one example.

21. Write down the electronic configuration of phosphorus.

22. Write main points of Dalton atomic theory.

23. What is plum pudding theory?

24. How James Chadwick. Discovered neutron.

25. How goiter is detected in a patient.

26. Define electronic configuration give an example also.

27. D/f between shell and subshell with examples of each.

28. Give two properties of neutron.

29. Who discover proton and neutron?

30. Write any four properties of cathode rays.

31. Describe Rutherford’s atomic model also point out the defects in this model.

32. Write down any three properties of canal rays.

33. Give comparison b/w Rutherford’s and Bohers atomic theories.

unit no 3

1. Write two properties of Neutron Particle.

2. Give trend of Ionization Energy in a period.

3. What is shielding effect?

4. Define Shielding effect. Explain its trend in Groups and Periods.

5. Why are noble gases not reactive?

6. How the Dobereiner arranged the elements in periodic Table.

7. What is meant by Periodic Function?

8. Discuss the important features of Modern Periodic Table.

9. Differentiates between Period and Group.

10. What is meant by Atomic Radius? Write its unit.

11. Distinguish between Groups and period

12. Describe the trends of Electro negativity in a period and in a group.

13. Write the trend of Electro negativity in period and group of periodic table.

14. Give the trend of Ionization Energy in period.

15. Distinguish between period and group in the periodic table.

16. Discuss the important feature of Modern periodic table.

17. 2nd Ionization Energy is greater that 1st Ionization Energy.

18. Define Electron Affinity. Why it increases in a period and decreases in a group in the periodic table.

19. Write down the procedure about the experiment that temperature affects the solubility.

20. Name the raw material used for the commercial preparation of Na2 Co

21. You are provided with 0.1 m solution of sodium carbonate (na2c o3) how would you prepare 100 cm3 of 0-01 m solution of sodium carbonate?

22. How ironic bond is formed? Example it with an example.

Unit No. 4

1. What are Noble Gases not reactive?

2. Why Ice Floats on Water?

3. Describe four properties of Ionic compounds.

4. Why atoms form chemical bond?

5. What is Ionic Bond? Discuss the formation of Ionic Bond between Sodium and Chlorine Atoms.

6. Why noble gases are not reactive.

7. Define Octet Rule.

8. Why does Ice float on water.

9. How many bond pairs of electrons are found in NH3 Molecule

10. Why does Atom react?

11. Define Boyle’s Law and derive its equation.

12. Ionic compounds are solid. Justify it.

13. Define Hydrogen Bonding and give one example.

14. Explain the types of covalent Bond with at least one example of each type.

15. What is dipole interaction? Give one example.

16. What is the octet Rule?

17. How coordinate covalent Bond is formed? Explain with example.

18. How driller classified the elements.

19. What is octaves law?

20. State the Mendeleev’s periodic law.

21. Why noble gases are note reactive.

22. What do you mean by groups in periodic table?

23. Define ionization energy and give one example.

24. What is the trend of shielding effect in a group and in a period?

25. Define electron affinity and electronegativity.

26. STATE LAW OF OCTAVES.

27. Metals are good conductor of electricity why.

28. Why do atoms react?

29. What is the octet rule? How it differs from the duplet rule.

30. Why ionic compounds conduct electricity in solution form.

31. Write any two properties of covalent compounds.

32. What is the dative covalent bond? Show it with one example.

33. What is triple covalent bond give an example?

34. Write down example of two polar compounds

35. Why Hall has dipole-dipole forces of attraction.

36. Give any two properties of co-ordinate covalent compounds. Explain hydrogen bonding with an example.

37. How a co-ordinate covalent bond is formed? Explain it with example.

Unit No. 5

1. How gases produce Homogeneous mixture?

2. What is standard Atmospheric Pressure?

3. What is meant by Evaporation?

4. Write the factors on which Evaporation depends.

5. Define effusion and give example.

6. What do you mean by Pascal? How many Pascal’s are equal to 1 atom?

7. Define Systolic Pressure?

8. Describe any three typical properties of Gases.

9. Define Boyle’s Law.

10. Write down two factors on which Vapor pressure depends upon?

11. Define Allotropy?

12. Define Pressure and write its unit.

13. Why metals are good conductor of Electricity.

14. Define Diffusion. Give example.

15. Why Densities of Gases are low than that of Liquids?

16. What is Ionic Bond? Discuss the formation of Ionic Bond between Sodium and Chlorine.

17. Define Vapor Pressure.

18. State whether allotropy is shown by Elements or Compounds or both?

19. Why solids show rigidity?

20. Define Boyle’s law and verify it with an example.

21. What is the effect of Temperature on Vapor Pressure?

22. Differentiate between diffusion and effusion.

23. What is Charles law? Write its equation.

24. What is the vapor Pressure? How it is affected by intermolecular forces?

25. Explain the factors on which a vapor pressure depends on.

26. What is vapor pressure? How it changes with changing temperature.

Unit No.6

1. What is solution?

2. What is percentage of Volume / mass? Give example.

3. How suspension is differing from solution?

4. If we add 5 cm3 of Acetone in water to prepare 90 cm3 of aqueous solution. Calculate its concentration of this solution.

5. State any four properties of Colloids.

6. Give the general principals of solubility

7. Define Aqueous Solution and give example.

8. What is the difference between Dilute Solution and concentrated Solution?

9. Define Morality. Also write the formula for preparation of Molar Solutions.

10. Define Solubility.

11. Write a note on Colloid.

12. Compare the characteristics of Colloid and Suspension.

13. Why does not the suspension form Homogeneous Mixture?

14. Why we stir paints thoroughly before using.

15. How will you test whether give solution is a colloidal solution or not?

16. What do you mean “like dissolves like”. Explain with example.

17. Why does the colloid show Tyndall effects?

18. What is the difference between solution and Mixture?

19. Differentiate between Solute and solvent.

20. Give at least three characteristics of suspensions.

21. How much amount of KOH is required to prepare one molar Solution?

22. Define Saturated and Unsaturated Solution.

23. Define aqueous solution. Write the two components of Solution.

24. Define solubility. Which are the factors which affect the solubility of solute?

25. What is difference between Saturated and unsaturated Solution?

26. Define Solubility.

27. What is Tindal effect?

28. Give the four characteristics of colloid.

29. Draw dot and cross formula of methane.

30. Why gases are compressible.

31. Define effusion.

32. Convert 300 c to kelvin temperature.

33. Convert 450c to kelvin temperature.

34. Justify why evaporation is a cooling process.

35. Explain the rigidity in solids.

36. Why gases have less density than liquids and solids.

37. State charmless law and write down its mathematical expression.

38. What do you mean by transition temperature?

39. What is solute give two example?

40. Convert 1000 c kelvin.

41. Define dynamic equilibrium.

42. Define solution and give two examples.

43. D/f between solute and solvent.

44. Why suspension is does not form a homogeneous mixture.

45. What is meant by volume/volume %?

46. What is solute .give two example?

47. What is mean by saturated solution?

48. what is meant by m/m%

49. How one molar solution is prepared?

50. Describe the effects of temperature of solubility.

Unit No.7

1. Differentiate between spontaneous and non-spontaneous reactions.

2. Differentiate between oxidation and reduction.

3. Calculate oxidation number of subpar in h2so4 when h= +1 and o= -2

4. Differentiate between oxidizing agent and reducing agent.

5. Define strong electrolytes with example.

6. Write down three differences between electrolytic cell and galvanic cell.

7. Complete and balance the following chemical equations.

8. What happens at the cathode in a galvanic cell?

9. Name the by-products produced in nelson’s cell.

10. Differentiate between strong and weal electrolytes.

11. Define oxidation in terms of electron. Give example.

12. What is the shape of cathode in nelson’s cell? Why is it perforated?

13. What is the difference between corrosion and rusting?

14. What type of reaction take place at anode in electrolyte cell?

15. Where do the electrons flow from an electrode in Daniel’s cell?

16. What is meant by Metallic Coating? Explain its two physical methods.

17. Compare Electrolytic cell and Galvanic cell.

18. Write the chemical reaction which takes place during working of Nelson cell.

19. What is meant by Redox Reaction?

20. Define corrosion.

21. What is Electrolysis? Give one example

22. What is Electroplating? Write down the procedure of Electroplating.

23. Write down the reaction of Sodium with the following.

24. How electroplating of chromium is carried out

25. What are Non-Electrolytes? Give an example.

26. What is meant by Galvanizing?

27. Define Electro Chemistry.

28. Calculate the Oxidation number of Nitrogen in HNO3

29. Define Electrolysis. Explain the electrolysis of water.

30. Define electroplating describe the Chromium Electroplating in detail.

31. What is electrochemistry?

32. Define oxidation and give two examples.

33. What is the difference b/w Valency and oxidation state?

24. Why an iron grill is painted frequently.

25. What is electroplating? How electroplating of silver is carried out.

26. Give any four characteristics of electrolytic cell.

Unit No. 8

1. Write down tow chemical properties of Metals.

2. Write down two uses of Calcium Metal.

3. Write down four physical properties of Non-Metals.

4. Give any four rules for assigning Oxidation Number to an element

5. Define the Oxidation.

6. Define the Oxidation number of MN and KMnO4

7. What is the meant by Non- Electrolytes?

8. Define the electro Chemistry

9. What is meant by Electrolytic cell?

10. Write down names of two very Reactive Metals.

11. Write down two properties of Calcium

12. Write down two properties of Gold.

13. Write four important physical properties of Non- Metals

14. Write two uses of Sodium Metal.

15. Write four physical properties of Metals.

6. What are the uses of Silver?

17. Describe the physical properties of Non-Metals.

18. What is the relationship between Electro positivity and Ionization Energy?

19. Why reactivity of metals increases down the group.

20. Give two uses of calcium

21. Write down any two uses of Magnesium

22. Why Sodium Metal is more reactive than magnesium.

23. Write down the important physical properties of Non- metals.

24. Why magnesium is harder than sodium.

25. State the four physical properties of metals.

26. Write two chemical properties of nonmetals.

27. Write down the name of two strong electrolysis.

28. Define alloy and give examples.

29. Write down the name of very reactive metals.

30. WHAT ARE TWO USES OF SILVER?

31. Write down two physical properties of nonmetals.

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