Chapter Wise Solved MCQS Notes (2025)

9th Chemistry MCQs with Answers

Get 9th Class Chemistry MCQs with answers, chapter-wise solved notes and past paper important MCQs for Punjab Board 2025 syllabus. Free PDF and online quiz available.

▶ Chapter 1 - States of Matter and Phase Changes

1. Matter is present in neon signs in the state of:

Supercritical Fluid Plasma Gas Liquid Crystal

2. Hazardous effects of shopping bags are studied in:

Geochemistry Inorganic Chemistry Analytical Chemistry Environmental Chemistry

3. The man-made polymer is:

Starch Polystyrene Protein Cellulose

4. The crystals of which substance hs rhombic shape?

Brass Sulphur Graphite Bronze

5. Which liquid among the following is a colloidal solution?

Milk Slaked lime used for white wash Vinegar Solution Mixture of Silver chloride

6. Which of the following is a heterogeneous mixture?

A solution of Calcium Hydroxide in water A solution of Pottasium Nitrate in water Hot Chocolate Concrete Mixture

7. A state of matter whose properties are between those of liquids and crystalline solids:

Liquid Crystal Spercritical Fluid Plasma Dark matter

8. When the tiny visible particles of a substance are dispersed through medium, the mixture is made an:

True Solution Colloid Suspension Saturated Solution

9. A solution of potassium Chlorate has a solubility of about 13.2 g per 100 cubic meter at 40 degree C. How its solubility will be affected, if you decrease the temperature1:

The solubility will increase The soubility will decrease The soubility will remain the same The soubility will first increase with temp. and then it will decrease

10. You are studying the rate of hydrolysis of starch under diffrent comditions of temperature. In which branch of chemistry this topic will fall?

Organic Chemistry Analytical Chemistry Biochemistry Physical Chemistry

▶ Chapter 2 - Atomic Structure

1. How many electrons can accomodate at the most i the third shell of the elements?

8 18 10 32

2. What information was obtained from discharge tube experiments?

Structure of atom was discovered Neutrons and protons were discovered Electrons and protons were discovered Presence of nucleus in an atom was discovered

3. How many electrons can be accomodated in a f-sub-shell?

2 6 10 14

4. Which particle is present in different number in the isotopes?

Electron Neutron Proton Both neutron and electron

5. In which isotope of oxygen there are the equal number of protons, electrons and neutrons?

Oxygen-15 Oxygen-16 Oxygen-17 Oxygen-18

6. What will be the relative atomic mass of nitrogen given the abundances of its two isotopes, N-14 and N-15 are 99.64 and 0.35 respectively.

14.0210 14.0021 14.2100 14.1200r

7. How is radiocarbon dating useful for archeologists?

It helps determine the age of organic matter. It helps determine the composition of matter. It helps determine the usefulness of matter. It helps determine whether the matter is radioactive or not.

8. What does keep the particles present in the nucleus intact?

Particles are held together by strong nuclear force. Particles are held together by weak nuclear force. Particles are held together by electrostatic force. Particles are held together by dipolar force.

9. How do electrons keep themselves away from the oppositely charged nucleus?

By keeping themselves stationary By revolving around the nucleus Due to their wave-like nature A magnetic field around the nucleus keeps them away

10. Rubidium consists of two isotopes 85Rb and 87Rb. The percent abundance of the light isotope is 72.2%. What is the percent abundance of the heavier isotope? Its atomic mass is 85.47.

15% 27.8% 37% 72%

11. John Dalton put forward his atomic theory in:

1803 1886 1897 1913

12. How much mass of an atom is concentrated in nucleus?

10% 50% 99.99% 9.99%

13. Neutron was discovered in:

1933 1833 1733 1633

14. Which isotope of carbon has 7 neutrons?

C-12 C-13 C-11 Both a and b

15. The cathode rays are:

Positively charged Negatively charged Neutral Both 'a' and 'b'

16. Which instrument is used to measure mass?

Stopwatch Spring Balance Thermometer Voltmeter

17. Which instrument is used to measure mass?

Stopwatch Spring Balance Thermometer Voltmeter

18. Which instrument is used to measure mass?

Stopwatch Spring Balance Thermometer Voltmeter

19. Which instrument is used to measure mass?

Stopwatch Spring Balance Thermometer Voltmeter

20. Which instrument is used to measure mass?

Stopwatch Spring Balance Thermometer Voltmeter

▶ Chapter 3 - Chemical Bonding

1. When molten copper and molten zinc are mixed together, they give rise to a new substance called brass. Predict what type of bond is formed between copper and zinc.

Coordinate covalent bond lonic bond Covalent bond Metallic bond

2. Which element is capable of forming all the three types of bonds; covalent coordinate covalent and ionic?

Carbon Oxygen Magnesium Silicone

3.Why is H₂O a liquid while H₂S is a gas?

Because in water, the atomic size of oxygen is smaller than that of sulphur Because water is a polar compound and there exists strong forces of attraction between its molecules Because H₂O molecule is lighter than H2S Because water can easily freeze into ice

4. Which of the following bonds is expected to the weakest?/

C-C Cl - Cl O - O F - F

5. Which form of the carbon is used as a lubricant?

Coal Diamond Graphite Charcoal

6. Keeping in view the intermolecular forces of attraction, indicate which compound has the highest boiling point.

H2O H2S HF NH3

7. Which metal has the lowest melting point?

Li Na K Rb

8. Which ionic compound has the highest melting point?

NaCl KCl LiCl RbCl

9. Which compound contains both covalent and ionic bonds?

MgCl2 NH4Cl CaO PCl3

10. Which among the following has a double covalent bond?

Ethane Methane Ethylene Acetylene

▶ Chapter 4 - Stoichiometry

1.How many atoms are present in one gram of H2O?

1002 × 10²³ 6.022 × 10²³ atoms 0.334 × 10²³ atoms 2.004 × 10²³ atoms

2.Which is the correct formula of calcium phosphide?

CaP CaP2 Ca2P3 Ca3P2

3. How many atomic mass units (amu) are there in one gram?

1 amu 10²³ amu 6.022 × 10²³ amu 6.044 × 10²³ amu

4. Structural formula of 2-hexene is CH3 - CH = CH - (CH2)2 - CH3. What will be empirical formula?

C2H2 CH C6H12 CH2

5. How many moles are there in 25 g of H2SO4?

0.765 moles 0.51 moles 0.255 moles 0.4 moles

6. A necklace has 6 g of diamonds in it. What are the number of carbon atoms in it?

6.02 × 10²³ 12.04 × 10²³ 1.003 × 10²³ 3.01 × 10²³

7. What is the mass of AI in 204 g of aluminum oxide, AI2O3?

26 g 27 g 54 g 108 g

8.Which of the following compounds will have the highest percentage of the mass of nitrogen?

CO (NH2)2 N2H4 NH3 NH2OH

9. What mass of 95% CaCO3 will be required to neutralize 50 cm^3 of 0.5M HCl solution?

9.5g 1.25g 1.32g 1.45g

10. When one mole of each of the following compounds is reacted with oxygen, which will produce the maximum amount of Co2?

Carbon Diamond Ethane (C2H6) Methane (CH4)

11. Which instrument is used to measure mass?

Stopwatch Spring Balance Thermometer Voltmeter

12. ich instrument is used to measure mass?

Stopwatch Spring Balance Thermometer Voltmeter

13.hich instrument is used to measure mass?

Stopwatch Spring Balance Thermometer Voltmeter

14. ch instrument is used to measure mass?

Stopwatch Spring Balance Thermometer Voltmeter

15. ich instrument is used to measure mass?

Stopwatch Spring Balance Thermometer Voltmeter

16. instrument is used to measure mass?

Stopwatch Spring Balance Thermometer Voltmeter

17. ich instrument is used to measure mass?

Stopwatch Spring Balance Thermometer Voltmeter

18. ich instrument is used to measure mass?

Stopwatch Spring Balance Thermometer Voltmeter

19. ich instrument is used to measure mass?

Stopwatch Spring Balance Thermometer Voltmeter

20. ch instrument is used to measure mass?

Stopwatch Spring Balance Thermometer Voltmeter

▶ Chapter 5 - Energetics

1. Which of the following is a base quantity?

Velocity Force Length Pressure

2. Which instrument is used to measure mass?

Stopwatch Spring Balance Thermometer Voltmeter

3. Which instrument is used to measure mass?

Stopwatch Spring Balance Thermometer Voltmeter

4. Which instrument is used to measure mass?

Stopwatch Spring Balance Thermometer Voltmeter

5. Which instrument is used to measure mass?

Stopwatch Spring Balance Thermometer Voltmeter

6. Which instrument is used to measure mass?

Stopwatch Spring Balance Thermometer Voltmeter

7. Which instrument is used to measure mass?

Stopwatch Spring Balance Thermometer Voltmeter

8. Which instrument is used to measure mass?

Stopwatch Spring Balance Thermometer Voltmeter

9. Which instrument is used to measure mass?

Stopwatch Spring Balance Thermometer Voltmeter

10. Which instrument is used to measure mass?

Stopwatch Spring Balance Thermometer Voltmeter

▶ Chapter 6 - Equilibria

1. What will happen if the rates of forward and reverse reactions are very high?

The equilibrium point will reach very soon. The equilibrium point will reach very late. The reaction will jot attain the state of dynamic equilibrium. The reaction will be practically irreversible.

2. Predict which components of the atmosphere react in the presence of lightning.

N2 and H2O O2 and H2O CO2 and O2 N2 and O2

3. An inorganic chemist places one mole of PCl5 in a container A and one mole of each Cl2 and PCl3 in container B. Both the containers were sealed and heated to the same temperature to reach the state of equilibriums. Guess about the composition of mixtures in both the containers.

Both of the containers will have the same composition of mixtures. Container A will have more concentration of PCl3 than B. Container A will have less concentration of PCl3 than B Both the containers will have zero concentration of its reactants.

4. CaO or lime is used extensively in steel, glass and paper industries. It is produced in an exothermic reversible reaction by the decomposition of lime (CaCO3). Choose the conditions to produce maximum amount of lime.

Heating at high temperature in a closed vessel Heating at high temperature in an open vessel Cooling it in a closed vessel Cooling it in an open vessel

5. What condition should be met for the reversible reaction to achieve the state of equilibrium?

All the reactants should be converted into the products. 50% of the reactants should be converted into products. The concentrations of all the reactants and the products should become constant. One of the products should be removed from the reaction mixture.

6. Why the gas starts coming out when you open a can of fizzy drink?

Because the solubility of the gas increases Because the gas is insoluble in water Because the gas is dissolved under pressure hence it comes out when pressure is decreased Because the solubility of the gas decreases at high pressure

7.The color of copper sulphate pentahydrate is:

Blue Green White Black

8. When a reaction will become a reversible one?

If the activation energy of the forward reaction is comparable to that of backward reaction If the activation energy of the forward reaction is higher than that of backward reaction If the activation energy of the forward reaction is lower than that of backward reaction If the enthalpy change of both the reactions is zero

9. Is reversible reaction useful for preparing compounds on large scale?

No Yes They are useful only when equilibrium lies far to the right side They are useful only when equilibrium lies far to the left side

10. What will happen to the concentrations of the products if a reversible reaction at equilibrium is not disturbed?

They will remain constant They will keep on increasing They will keep on decreasing They will remain constant for some time and then start decreasing

▶ Chapter 7 - Acid Base Chemistry

1. Which acid is not used as a food or mixed with food?

Tartaric Acid Ascorbic Acid Citric Acid Formic Acid

2. While baking, which gas is responsible for raising the bread and making it soft?

Oxygen Carbon dioxide Nitrogen Carbon monoxide

3.Predict the main characteristics of the reactions 9f metal with acids.

Metals are dissolved Metals are converted into salts Hydrogen gas is evolved All the above mentioned characteristics are true

4. How many hydroxide ions, calcium hydroxide will release in water?

1 2 0 3

5. In a neutralization reaction between KOH and H3PO4, hiw many molecules of KOH will react withone molecule of H3PO4?

2 11 3 4

6. Which acid is used in the preparation of soap?

Tartaric acid Citric acid Stearic acid Oxalic acid

7. Which compound is formed when SO2 is dissolved in water?

SO3 H2SO3 H2SO4 H2S2O7

8. Which of the following contains oxalic acid?

Tomato Orangelabel> Tamarind Sour Milk

9. Which one of the following is an Arrhenius base?

HCl NaCl NaOH H2O

10. The percentage irrigation of glacia acid is:

0.132% 13.2% 1.32% 1.32%

▶ Chapter 8 - Periodic Table and Periodicity

1. In which period and group will you place the element which is an important part of the solar cell?

The third period and 14th group Second period and 14th group Third period and 15th group Third period and 16th group

2. Identify the electronic configuration of the outermost shell of transition metal.

ns2np4 ndxns2 ns2np6 ns2np5

3. Which is the softest metal?.

Na Ca Al Zn

4. A yellow solid element exists in allotropic forms which is also present in fossil fuels. Indicate the name.

Carbon Iodine Aluminum Sulphur

5. How many electrons can nitrogen accept in its outermost shell?

2 3 4 5

6. Which element is the most reactive element?

Oxygen Chlorine Fluorine Nitrogen

7. The element having less value of ionization energy and less value of electron affinity is likely to belong to:

Group 1 Group 13 Group 16 Group 17

8. Which element has the highest melting point?

Na K Rb Cs

9. In what order does the mentalic character change in the second group?

Mg>Ca>Ba>Sr Sr>Ba>Ca>Mg Mg>Sr>Ca>Ba Ba>Sr>Ca>Mg

10. The ionization energy:

Increase down the group Decrease down the groups Neither increase nor decrease down the group None of these

▶ Chapter 9 - Group Properties and Elements

1. Which halogen will have the least reactivity with Alkaline earth metals?

Chlorine Iodine Bromine Flourine

2. Which compound do you expect to be colored?

KCl BaCl2 AlCl3 NiCl2

3. In which element there exists the strongest forces of attraction between atoms?

Mg Ca Sr Ba

4. Elementsbof which group are all coloured?

Second group Sixth group Fourth Group Fifth Group

5. Which halogen acid is unstable at room tempreature?

HBr HI HCl HF

6. Which oxide is the most basic oxide?

Na2O Li2O MgO CO

7. Which group elements are the most reactive elements?

Transition metal group First Group Second Group Third Group

8. The following solutions of a halogen and a sodium halide are mixed together. Which solution will turn dark because of a reaction?

Br2 and NaCl Br2 and NaF Cl2 and NaF Cl2 and Nal

9. Which property is correct from group I element?

low catalytic activity High density Low electrical conductivity High melting point

10. X is a monoatomic gas, which statement about this is correct?

X burns in air X is coloured X is unreactive X will displace iodine from it

▶ Chapter 10 - Environmental Chemistry

1.

Velocity Force Length Pressure

2. Which instrument is used to measure mass?

Stopwatch Spring Balance Thermometer Voltmeter

3. Which of the following is a base quantity?

Velocity Force Length Pressure

4. Which of the following is a base quantity?

Velocity Force Length Pressure

5. Which of the following is a base quantity?

Velocity Force Length Pressure

6. Which of the following is a base quantity?

Velocity Force Length Pressure

7. Which of the following is a base quantity?

Velocity Force Length Pressure

8. Which of the following is a base quantity?

Velocity Force Length Pressure

9. Which of the following is a base quantity?

Velocity Force Length Pressure

10. Which of the following is a base quantity?

Velocity Force Length Pressure

▶ Chapter 11 - Hydrocarbons

1. Which other atom is almost always present along with carbon atom in all organic compounds?

Oxygen Nitrogen Hydrogen Halogen

2. Which other metal can be used to reduce alkyl halides?

Al Mg Ni Co

3. In naphtha undergoes a combination reaction what products do you expect it to form?

Alkanes Alkenes CO2 and H2O Both alkanes and alkenes

4. Why does a mixture of zinc and hydrochloric acid acts as a reducing agent?

Because zinc acts as a reducing agent. Because atomic hydrogen is produced with Zn/HCl which acts as a reducing agent. Because molecular hydrogen is produced with Zn/HCl which acts as reducing agent. Because chloride ions are produced with Zn/HCl which acts as a reducing agent.

5. Which alkane will evolve the most amount of heat when it is burnt with oxygen?

Ethane Propane n-Butane iso-Butane

6. Which reaction is not given by alkanes?

Substitution Combustion Addition Cracking

7. Which hydrocarbon is responsible for explosions in coal mines?

Butane Pentane Methane Ethane

8. The alkanes are almost?

Polar Non-polar Both a and b None of these

9. Which of the following is not a process of halogenation of alkanes?

Cracking Chlorination Bromination Iodination

10. How many moles of oxygen will be required to completely burn propane?

4 moles 5 moles 3 moles 6 moles

▶ Chapter 12 - Empirical Data Collection and Analysis

Q1: Which of the following pairs of quantities may be measured in the same unit?

Heat and temperature Temperature and area Heat and work Length and work

Q2: In which unit we usually measure the energy present in the food?

Kilojoules Megajoules Calorie Joule

Q3: What prefix is used for 10^-12?

Mega Pico Giga Tessa

Q4: In SI unit of pressure is expressed in:

Newton per meter Newton per meter square Joule Pascal

Q5: Which symbol is used for kilogram in SI units?

K k Kgm Kg

Q6: What does a mole represent?

Number Mass Volume Length

Q7: Which unit of volume should usually be used in Chemistry?

Mililitre Litre Cubic centimeter Cubic metre

Q8: The closeness of two or more measurements to each other is called:

Error Accuracy Precision J

Q9: The difference between measured value and actual value is called:

Precision Accuracy Error All of these

▶ Chapter 13 - Laboratory and Practical Skills

Q1: Safety in the chemistry laboratory is:

the responsibility of the students only the responsibility of the professor only the responsibility of the lab. incharge only a shared responsibility

Q2: Accidents often result from:

making mistakes failure to use common sense failure to follow instruction all of the above

Q3: The label "Warming" on a chemical bottle signifies:

that the chemical can cause less serious injury that the chemical can cause serious injury that user should be careful when using chemical that user should open it only in the presence of a teacher

Q4: The label "Corrosive" on a chemical bottle indicates:

that the material is an oxidating agent that the material can degrade rapidly upon exposure that its contact destroys living tissue that the chemical can explode

Q5: Example of high toxic chemical:

Ethanol Acetic Acid Potassium Cyanide Potassium permanganate

Q6: Example of self-reactive chemical:

Potassium Phenol Picric Acid n-Hexane

Q7: When diluting an acid with water:

do it quickly do not stir the container always add acid to water always add water to acid

Q8: What should you do in case of a fire drill in the lab?

run to safety shower climb into the fume cupboard close gas valves and turn off all equipments carry chemicals out of the lab