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Chemistry 9th Class Chemistry

Model Paper 9th Class Chemistry

FINAL TERM EXAMINATION YEAR (Model Paper) …….

CLASS: 9th PAPER: Chemistry  DATE:__________

    

Student’s Name: _______________________________     Computer#

Duty Tr:

 

Checked by:

 

 

Re-checked by:
Q:1Q:2Q:3Q:4Q:5Q:6Q:7Q:8Q:9PRTotal
1210101018     60
           

 

  Time Allowed: 15 min

Q: 1 Choose the correct option. (12)

Note: You have four choices for each objective type question as A/B/C/ and D. The choice which you think is correct; fill that circle in front of that question number. Cutting or filling two or more circles will result in zero mark in that question.

 

  1. The molar mass of H2SO4is:
  2. a) 9.8g b) 98g c) 9.8 amu d) 80g

 

  1. The most abundant element occurring in the ocean is:
  2. a) Oxygen b) Hydrogen c) Nitrogen d) Silicon

 

  1. The P subshell has:
  2. a)  One orbital b) Two orbitals c) Three orbitals d) Four orbitals

 

  1. The amount of energy released  when an electron is added to an atom is called:
  2. a) Lattice energy b) Ionization energy c) Electronegativity d) Electron affinity

 

  1. Along the period which one of the following decreases:
  2. a) Atomic radius b) Ionization Energy c) Electron affinity d) Electronegativity

 

  1. Identify the compound which is not soluble in water.
  2. a) C6H6 b) NaCl c) KBr d) MgCl2

 

  1. Which one of the following diffuses fast?
  2. a) Hydrogen b) Helium c) Fluorine d) Chlorine

 

  1. Solid particles possess which one of the following movement?
  2. a) Rotational motion b) Vibrational motion c) Translational motion d) both b and c

 

  1. If 10 cm3of alcohol is dissolved in 100 g of water, it is called:
  2. a) % w/w b) % w/v c) % v/w d) % v/v

 

  1. The oxidation number of chromium in K2Cr2O7is:
  2. a) +2 b) +6 c) +7 d) +14

 

  1. The most common example of corrosion is:
  2. a) Chemical decay b) Rusting of iron c) Rusting of aluminium d) Rusting of tin

 

  1. Sodium is extremely reactive metal, but it does not react with:
  2. a) Hydrogen       b) Nitrogen        c) Sulphur  d) Phosphorous

Essay type Marks:48 Time: 1:45 Hours

 

Section – I 2 X 15=30

 

  1. Write short answers of any five parts from the following. 2×5=10
  2. State three reasons why do you think air is a mixture and water a compound?
  3. Define atomic mass unit. Why is it needed?

iii. An element has an atomic number 17. How many electrons are present in K, L and M shells of the atom?

  1. Give four characteristics of cathode rays.
  2. What are the defects of Rutherford’s atomic model?
  3. Why the second ionization energy of magnesium is higher than the first one?

vii. Why silver and gold are least reactive?

 

  1. Write short answers of any five parts from the following. 2×5=10
  2. Give the trend of ionization energy in a period.
  3. What do you mean by groups and periods in the Periodic Table?

iii. Why shielding effect of electrons makes cation formation easy?

  1. Define electron affinity and ionization energy?
  2. Differentiate between lone pair and bond pair of electrons.
  3. Give the characteristic properties of ionic compounds.

vii. Where do the electrons flow from Zn electrode in Daniel’s cell?

 

  1. Write short answers of any five parts from the following. 2×5=10
  2. Name the by-products produced in Nelson’s cell?
  3. Define standard atmospheric pressure. What are its units? How it is related to Pascal?

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

  1. What do you mean by evaporation how it is affected by surface area.
  2. Differentiate between strong and weak electrolytes.
  3. What do you mean by volume/volume %?

vii. Why we stir paints thoroughly before using?

 

Section-II 9×2=18

Note: Answer any two questions from the following.

  1. (i) Define element and classify the elements with examples.

(ii) How Rutherford discovered that atom has a nucleus located at the centre of the atom?

  1. (i) Explain the types of covalent bonds with at least one example of each type.

(ii) Compare the physical properties of metals and non-metals.

  1. (i) Define and explain Charles’ law of gases.

(ii) 12 M H2SO4 solution is available in the laboratory. We need only 500cm3 of 0.1 M solution , how it will be prepared?

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