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Form 4 Chemistry

01 Introduction to Chemistry

1.1 Development in Chemistry Field and Its Importance in Daily Life

1.1.1 Development of the Field of Chemistry and Its Importance in Life (Q&A)

1.1.2a Development of Chemistry and its Importance in Life – I (T/F)

1.1.2b – Development of Chemistry and its Importance in Life – II (T/F)

1.1.3 Development of the Field of Chemistry and Its Importance in Life (MCQ)

1.2 Scientific Investigation in Chemistry Sample Lesson

1.2.1 Scientific Investigations in Chemistry (Q&A)

1.2.2 Scientific Investigation in Chemistry (T/F)

1.2.3 Scientific Investigation in Chemistry (MCQ)

1.3 Usage, Management and Handling of Apparatus and Materials Sample Lesson

1.3.1 Use, Management and Handling of Apparatus and Chemical Substances (Q&A)

1.3.2a Use, Management, and Handling of Chemical Apparatus and Materials-I (T/F)

1.3.2b Use, Management, and Handling of Chemical Apparatus and Materials-II (T/F)

1.3.3 Use Management, and Handling of Chemical Apparatus and Materials (MCQ)

02 Matter and Atomic Structure

2.1 Basic Concepts of Matter Sample Lesson

2.1.1 Basic Concepts of Matter (Q&A)

2.1.2a Basic Concept of Matter – I (T/F)

2.1.2b Basic Concept of Matter – II (T/F)

2.1.3 Basic Concept of Matter – I (MCQ)

2.1.4 Basic Concept of Matter – II (MCQ)

2.2 The Development of the Atomic Model Sample Lesson

2.2.1 Development of the Atomic Model (Q&A)

2.2.2 Development of Atomic Models (T/F)

2.2.3 Development of the Atomic Model: A Historical Overview (MCQ)

2.3 Atomic Structure

2.3.1 Atomic Structure (Q&A)

2.3.2a Atomic Structure – I (T/F)

2.3.3b Atomic Structure – II (T/F)

2.3.3 The Structure of Atom (MCQ)

2.3.4 Electrons Arrangement (MCQ)

2.4 Isotopes and Its Uses

2.4.1 Isotopes and Their Uses (Q&A)

2.4.2 – Isotopes and Their Uses (T/F)

2.4.3 Isotopes and Their Uses (MCQ)

03 Concepts of Mole, Formula and Chemical Equations

3.1 Relative Atomic Mass and Relative Molecular Mass

3.1.1 Relative Atomic Mass and Relative Molecular Mass (Q&A)

3.1.2 Relative Atomic Mass and Relative Molecular Mass (T/F)

3.1.3 Relative Atomic Mass and Relative Molecular Mass (MCQ)

3.1.4 Molar Mass of Substances (MCQ)

3.2 Mole Concept

3.2.1 Mole Concept (Q&A)

3.2.2a Mole Concept – I (T/F)

3.2.2b Mole Concept – II (T/F)

3.2.3 Concept of Mole (MCQ)

3.2.4 Molar Volume of Gases (MCQ)

3.2.5 Number of Mole of Solute (MCQ)

3.3 Chemical Formula

3.3.1 Chemical Formula (Q&A)

3.3.2a Chemical Formula – I (T/F)

3.3.2b Chemical Formula – II (T/F)

3.3.3 Chemical Formulae (MCQ)

3.3.2 Flashcards of Ions

3.4 Chemical Equation

3.4.1 Chemical Equations (Q&A)

3.4.2a Chemical Equation – I (T/F)

3.4.2b Chemical Equation – II (T/F)

3.4.3 Chemical Equations (MCQ)

04 Periodic Table of Elements

4.1 Development of the Periodic Table of Elements

4.1.1 Development of the Periodic Table of Elements (Q&A)

4.1.2 Development of the Periodic Table (T/F)

4.1.3 History of Development of Periodic Table (MCQ)

4.1.4 Development of Periodic Table (MCQ)

4.2 Arrangement of Elements in the Modern Periodic Table

4.2.1 Arrangement of Elements in the Modern Periodic Table (Q&A)

4.2.2 Arrangement of Elements in the Modern Periodic Table (T/F)

4.2.3 Arrangement of Elements in the Modern Periodic Table (MCQ)

4.3 Elements in Group 18

4.3.1 Elements in Group 18 (Q&A)

4.3.2 Group 18 Elements (T/F)

4.3.3 Group 18 Elements (MCQ)

4.4 Elements in Group 1

4.4.1 Elements in Group 17 (Q&A)

4.4.2 Group 1 Elements (T/F)

4.4.3 Group 1 Elements (MCQ)

4.5 Elements in Group 17

4.5.1 Elements in Group 17 (Q&A)

4.5.2 Group 17 Elements (T/F)

4.5.3 Group 17 Elements (MCQ)

4.6 Elements in Period 3

4.6.1 Elements in Period 3 (Q&A)

4.6.2 Group 3 Elements (T/F)

4.6.3 Period 3 Elements (MCQ)

4.7 Transition Elements

4.7.1 Transition Elements (Q&A)

4.7.2 Transition Elements (T/F)

4.7.3 Period and Transition Metals (MCQ)

05 Chemical Bonds

5.1 Basics of Compound Formation

5.1.1 Basics of Compound Formation (Q&A)

5.1.2 Basics of Compound Formation (T/F)

5.1.3 Formation of Ions (MCQ)

5.1.4 Formation of Compounds (MCQ)

5.2 Ionic Bonds

5.2.1 Ionic Bonds (Q&A)

5.2.2 Ionic Bond (T/F)

5.2.3 Ionic Bond (MCQ)

5.3 Covalent Bonds

5.3.1 Covalent Bonds (Q&A)

5.3.2 Covalent Bond (T/F)

5.3.3 Covalent Bonding (MCQ)

5.4 Hydrogen Bonds

5.4.1 Hydrogen Bonds (Q&A)

5.4.2 Hydrogen Bond (T/F)

5.4.3 Hydrogen Bond (MCQ)

5.5 Dative Bonds

5.5.1 Dative Bond (Q&A)

5.5.2 Dative Bond and Metallic Bond (T/F)

5.5.3 Dative Bond (MCQ)

5.6 Metallic Bonds

5.6.1 Metallic Bond (Q&A)

5.6.2 Metallic Bond（T/F）

5.6.3 Metallic Bond (MCQ)

5.7 Properties of Ionic and Covalent Compounds

5.7.1 Properties of Ionic and Covalent Compounds (Q&A)

5.7.2 Properties of Ionic and Covalent Compounds (T/F)

5.7.3 Properties of Ionic and Covalent Compounds (MCQ)

06 Acids, Bases and Salts

6.1 The Role of Water in Showing Acidity and Alkalinity

6.1.1 The Role of Water in Showing Acidity and Alkalinity (Q&A)

6.1.2a Role of Water in Showing Acidity and Alkalinity I (T/F)

6.1.2b Role of Water in Showing Acidity and Alkalinity II (T/F)

6.1.3 The Role of Water in Showing Acidity and Alkalinity (MCQ)

6.2.1 pH Value (Q&A)

6.2.2 pH Value (T/F)

6.2.3 pH Value (MCQ)

6.3 Strength of Acids and Alkalis

6.3.1 Strength of Acids and Alkalis (Q&A)

6.3.2 Strength of Acids and Alkalis (T/F)

6.3.3 Strength of Acids and Alkalis (MCQ)

6.4 Chemical Properties of Acids and Alkalis

6.4.1 Chemical Properties of Acids and Alkalis (Q&A)

6.4.2 Chemical Properties of Acids and Alkalis (T/F)

6.4.3a Understanding Alkalis I (MCQ)

6.4.3b Understanding Alkalis II (MCQ)

6.4.4a Understanding Acids I (MCQ)

6.4.4b Understanding Acids II (MCQ)

6.5 Concentration of Aqueous Solutions

6.5.1 Concentration of Aqueous Solution (MCQ)

6.5.2a Standard Solutions (T/F)

6.5.2b Concentration of Aqueous Solutions (T/F)

6.5.3a Dilution and Stoichiometry Calculation (MCQ)

6.5.3b Concentration of Solutions (MCQ)

6.6 Neutralisation

6.6.1 Neutralisation (Q&A)

6.6.2 Neutralization (T/F)

6.6.3 Neutralisation (MCQ)

6.7 Salts, Crystals and Their Uses in Life

6.7.1 Salts, Crystals and Their Uses in Life (Q&A)

6.7.2 Salts, Crystals, and Their Uses in Life (T/F)

6.7.3 Salts and Their Uses (MCQ)

6.8 Preparation of Salts

6.8.1 Preparation of Salts

6.8.2a Salt Preparation I (T/F)

6.8.2b Salt Preparation II (T/F)

6.8.3a Preparing Salts I (MCQ)

6.8.3b Preparing Salts II (MCQ)

6.9 Action of Heat on Salts

6.9.1 Action of Heat on Salts (Q&A)

6.9.2 Action of Heat on Salts (T/F)

6.9.3 Action of Heat on Salts (MCQ)

6.10 Qualitative Analysis

6.10.1 Qualitative Analysis (Q&A)

6.10.2a Qualitative Analysis I (T/F)

6.10.2b Qualitative Analysis II (T/F)

6.10.2c Qualitative Analysis III (T/F)

6.10.2d Qualitative Analysis IV (T/F)

6.10.2e Qualitative Analysis V (T/F)

6.10.2f Qualitative Analysis VI (T/F)

6.10.3a Qualitative Analysis I (MCQ)

6.10.3b Qualitative Analysis II (MCQ)

07 Reaction Rates

7.1 Determination of Reaction Rates

7.1.1 Determining Rate of Reaction (Q&A)

7.1.2a Determination of Rate of Reaction I (T/F)

7.1.2b Determination of Rate of Reaction II (T/F)

7.1.3 Introduction to Rate of Reaction (MCQ)

7.1.4 Finding the Rate of Reaction (MCQ)

7.1.5 Reactant/Product-Time Graph (MCQ)

7.2 Factors Affecting Reaction Rates

7.2.1 Factors Affecting Reaction Rates (Q&A)

7.2.2 Factors Affecting Rate of Reaction (T/F)

7.2.3 Factors Affecting the Rate of Reaction (MCQ)

7.3 Application of Factors Affecting Reaction Rates in Life

7.3.1 Application of Factors Affecting Reaction Rates in Life (Q&A)

7.3.2 Application of Factors Affecting Rate of Reaction in Life (T/F)

7.3.3 Application of Factors Affecting Rate of Reaction in Life (MCQ)

7.4 Collision Theory

7.4.1 Collision Theory

7.4.2a Collision Theory I (T/F)

7.4.2b Collision Theory II (T/F)

7.4.3 Collision Theory and Application of Rate of Reaction (MCQ)

08 Manufactured Substances in Industry

8.1 Alloys and Their Importance

8.1.1 Alloys and Their Importance (Q&A)

8.1.2 Alloys and Their Importance (T/F)

8.1.3 Alloys (MCQ)

8.2 Glass Composition and Its Uses

8.2.1 Glass Composition and Its Uses (Q&A)

8.2.2 Glass Composition and Its Uses (T/F)

8.2.3 Glass Composition and Its Uses (MCQ)

8.3 Ceramic Composition and Its Uses

8.3.1 Ceramic Composition and Its Uses (Q&A)

8.3.2 Ceramic Composition and Its Uses (T/F)

8.3.3 Ceramic Composition and Its Uses (MCQ)

8.4 Composite Materials and Their Importance

8.4.1 Composite Materials and Their Importance (Q&A)

8.4.2 Composite Materials and Their Importance (T/F)

8.4.3 Composite Materials and Their Importance (MCQ)

2.2.3 Development of the Atomic Model: A Historical Overview (MCQ)

Form 4 Chemistry
2.2 The Development of the Atomic Model
2.2.1 Development of the Atomic Model (Q&A)
2.2.3 Development of the Atomic Model: A Historical Overview (MCQ)

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Question 1 of 14

1. Question
0 point(s)
John Dalton’s atomic theory was a major step forward. Which of his core ideas was overturned by J.J. Thomson’s discovery of the electron?
- Atoms are the smallest, indivisible particles of an element.
- Atoms of the same element are identical in mass and properties.
- Atoms combine in simple, fixed, whole-number ratios to form compounds.
- Atoms are neither created nor destroyed in chemical reactions.
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Question 2 of 14

2. Question
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What was the key conclusion Ernest Rutherford drew from the observation that a few alpha particles were deflected at large angles in his gold foil experiment?
- The atom has a small, dense, positively charged nucleus.
- The atom is mostly composed of empty space.
- Electrons are negatively charged particles.
- Electrons are embedded within a sphere of positive charge.
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Question 3 of 14

3. Question
0 point(s)
What major instability in Rutherford’s nuclear model did Niels Bohr’s model of the atom successfully address?
- Why electrons don't lose energy and spiral into the nucleus.
- Why the atom has an overall neutral charge.
- Why most of the atom's mass is in the nucleus.
- Why atoms of the same element have identical properties.
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Question 4 of 14

4. Question
0 point(s)
James Chadwick’s discovery in 1932 was crucial for completing our basic picture of the atom. What did he discover?
- The neutron, a neutral particle located in the nucleus.
- The proton, a positive particle located in the nucleus.
- The electron, a negative particle orbiting the nucleus.
- Fixed energy shells where electrons orbit.
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Question 5 of 14

5. Question
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Which subatomic particle’s count uniquely determines the chemical identity of an element?
- Proton
- Neutron
- Electron
- Nucleon
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Question 6 of 14

6. Question
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An atom of an element is represented by the notation 15 31 P. How many neutrons does this atom contain?
- 16
- 15
- 31
- 46
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Question 7 of 14

7. Question
0 point(s)
How did J.J. Thomson’s ‘plum pudding’ model visualize an atom?
- A uniform sphere of positive charge with electrons scattered throughout.
- A dense, positive nucleus with electrons orbiting at a distance.
- A solid, indivisible sphere with no internal structure.
- A central nucleus with electrons orbiting in fixed energy levels.
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Question 8 of 14

8. Question
0 point(s)
Which statement accurately compares the relative masses of the fundamental subatomic particles?
- Protons and neutrons have similar masses, while electrons are much less massive.
- The proton is significantly more massive than the neutron.
- The electron is the most massive particle in the atom.
- All three particles—proton, neutron, and electron—have roughly the same mass.
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Question 9 of 14

9. Question
0 point(s)
In a neutral atom, what is the relationship between its subatomic particles?
- The number of electrons is equal to the number of protons.
- The number of neutrons must equal the number of protons.
- The number of electrons is equal to the number of neutrons.
- The number of protons is greater than the number of electrons.
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Question 10 of 14

10. Question
0 point(s)
Arrange the following atomic models in chronological order, from the earliest to the most recent.
- Dalton's Model, Thomson's Model, Rutherford's Model
- Rutherford's Model, Thomson's Model, Dalton's Model
- Thomson's Model, Dalton's Model, Rutherford's Model
- Dalton's Model, Rutherford's Model, Thomson's Model
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Question 11 of 14

11. Question
0 point(s)
CHEM0203010

Which of the following is not the hypothesis of Dalton’s Atomic Theory?
- All matter is composed of extremely small particles called atoms.
- All atoms of a given element are identical, having the same size, mass, and chemical properties.
- The atom is mostly empty space
- Atoms cannot be created, divided into smaller particles, or destroyed.
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Question 12 of 14

12. Question
0 point(s)
CHEM0203020

Which of the following statement is true about Neils Bohr’s atomic model?
- The electrons in an atom orbiting the nucleus at shells with certain energy level.
- Almost the whole mass of the atom concentrates in the nucleus.
- There are proton and neutron in the nucleus.
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Question 13 of 14

13. Question
0 point(s)
CHEM0203030

Which of the following statements is the hypothesis of Rutherford’s Model of atom?
- I. The atom is mostly empty space,
- II. Most of the atom’s mass concentrated in the nucleus of the atom.
- III. Electrons being held around the nucleus by electrostatic attraction.
- IV. There are positively charge subatomic particles in the nucleus of the atom.
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Question 14 of 14

14. Question
0 point(s)
CHEM0203040

Which of the following match is not true about the scientist and their contribution?
- J.J. Thompson – Discover electron
- James Chadwick – Discover neutron
- Rutherford – Discover proton
- Neils Bohr – Suggest that electrons are moving around the nucleus of an atom.
Correct

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