SPM Chemistry (KSSM) Paper 1

01 Introduction to Chemistry
1.1 Chemistry and Its Importance
1 Lesson
1.1.1 Chemistry and Its Importance
1.2 Scientific Investigation
1 Lesson
1.2.1 Scientific Investigation
02 The Structure of Atoms
2.1 The Basic Concept of Matter
2 Lessons
2.1.1 The Particle Theory of Matter
2.1.2 The Three States of Matter
2.2 The History of Development of the Atomic Model
1 Lesson
2.2.1 The History of Development of the Atomic Model
2.3 The Structure of Atom
2 Lessons
2.3.1 The Structure of Atom
2.3.2 Electrons Arrangement in Atom
2.4 Isotopes and Their Uses
1 Lesson
2.4.1 Isotopes and Their Uses
2.5 The Structure of Atom – Practices
03 Concept of Mole, Formulae and Equations
3.1 Relative Atomic Mass and Relative Molecular Mass
1 Lesson
3.1.1 Relative Atomic Mass and Relative Molecular Mass
3.2 Concept of Mole
3 Lessons
3.2.1 Concept of Mole
3.2.2 Number of Mole and Mass
3.2.3 Number of Mole and Volume of Gases
3.3 Chemical Formulae
2 Lessons
3.3.1 Chemical Formulae
3.3.2 Formula of Ionic Compounds and Molecule
3.4 Chemical Equations
1 Lesson
3.4.1 Chemical Equations
3.5 Chemical Formulae and Equations – Practices (Coming Soon)
04 Periodic Table of Elements
4.1 The Development of Periodic Table
1 Lesson
4.1.1 Development of Periodic Table
4.2 Arrangement of Element in Periodic Table
1 Lesson
4.2.1 Arrangement of Electrons in Periodic Table
4.3 Group 18 Elements
1 Lesson
4.3.1 Group 18 Elements
4.4 Group 1 Elements
2 Lessons
4.4.1 Group 1 Elements
4.4.2 Chemical Properties of Group 1 Elements
4.5 Group 17 Elements
2 Lessons
4.5.1 Group 17 Elements
4.5.2 Chemical Properties of Group 17 Elements
4.6 Elements in Period 3
1 Lesson
4.6.1 Elements in Period 3
4.7 Transition Elements
1 Lesson
4.7.1 The Transition Elements
4.8 Periodic Table – Practices (Coming Soon)
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3.4.1 Chemical Equations

SPM Chemistry (KSSM) Paper 1 3.4 Chemical Equations 3.4.1 Chemical Equations

Writing Chemical Equations

A Balance Equation

According to the Law of Conservation of Mass, atoms cannot be created or eliminated in the process of a chemical reaction. Therefore, the amount of atom of each element before reaction must be equal after the reaction. 

Example:
Balance the following chemical equations:

  1. Mg +    O2 →    MgO
  2. CuO + H2 →    Cu + H2O
  3. Na +    H2O →    NaOH + H2
  4. Li +    Cl2 →    LiCl
Answer:
a.
2Mg +    O2 →    2MgO
 

b.

CuO + H2 →    Cu + H2O
 

c.

2Na +    2H2O →    2NaOH + H2
d.
2Li +    Cl2 →    2LiCl
Writing a Balance Equation

Example:
Lead(II) nitrate aqueous reacts with potassium iodide aqueous to produce lead(II) iodide precipitate and potassium nitrate aqueous.

Answer:

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