SPM Chemistry (KSSM) Paper 1

05 Chemical Bonds
5.1 Formation of Compounds
1 Lesson
5.1.1 Formation of Compounds
5.2 Ionic Bonds
2 Lessons
5.2.1 Formation of Ion
5.2.2 Ionic Bonding
5.3 Covalent Bonds
1 Lesson
5.3.1 Covalent Bonding
5.4 Hydrogen Bonds
5.5 Dative Bonds
5.6 Metallic Bonds
5.7 Ionic and Covalent Compounds
1 Lesson
5.7.1 Properties of Ionic and Covalent Compounds
5.8 Chemical Bonds - Practices (Coming Soon)
06 Acids, Bases and Salts
6.1 The Role of Water in Acidic and Basic Properties
3 Lessons
6.1.1 Acids
6.1.2 Bases and Alkali
6.1.3 The Role of Water in Acidic and Basic Properties
6.2 Meaning of pH and Determination of pH
1 Lesson
6.2.1 Meaning of pH and Determination of pH
6.3 Strength of Acids and Alkalis
1 Lesson
6.3.1 Strength of Acids and Alkalis
6.4 Chemical Properties of Acids and Alkalis
3 Lessons
6.4.1 Chemical Properties of Acids
6.4.2 Chemical Properties of Alkalis
6.4.3 Writing Ionic Equation of The Reaction of Acids and Alkalies
6.5 Concentration of Aqueous Solution
2 Lessons
6.5.1 Concentration of Aqueous Solution
6.5.2 Molarity and Number of Moles
6.6 Standard Solution
2 Lessons
6.6.1 Standard Solution
6.6.2 Dilution
6.7 Neutralisation
2 Lessons
6.7.1 Neutralisation
6.7.2 Acid-Base Titration
6.8 Salts, Crystals and Their Uses in Daily Life
1 Lesson
6.8.1 Introduction to Salts
6.9 Preparation of Salts
4 Lessons
6.9.1 Solubility of Salts, Oxide and Hydroxide
6.9.2 Preparing Salts
6.9.3 Preparing Soluble Salts
6.9.4 Preparing Insoluble Salts
6.10 Action of Heat on Salts
2 Lessons
6.10.1 Identifying Gases
6.10.2 Effect of Heat on Salts
6.11 Qualitative Analysis
3 Lessons
6.11.1 Colour of Salts
6.11.2 Identifying Anions
6.11.3 Identifying Cations
6.12 Acids, Bases and Salts - Practices (Coming Soon)
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6.4.2 Chemical Properties of Alkalis

SPM Chemistry (KSSM) Paper 1 6.4 Chemical Properties of Acids and Alkalis 6.4.2 Chemical Properties of Alkalis
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Chemical Properties of Bases/Alkalis

  1. Alkalis react with acids to form a salt and water — this is a neutralisation reaction:
  2. Alkalis, when warmed with ammonium salts, give off ammonia gas:

Reaction between Alkalis and Acids

Acid + Alkali → Salt + Water
 

Example:
Potassium hydroxide + Nitric Acid → Potassium Nitrate + Water

KOH + HNO3  → KNO3  +  H2O

Alkali heat with Ammonium Salts

Ammonium Salt + Alkali → Salt + Ammonia + Water


Example:
Ammonium Chloride + Sodium Hydroxide → Sodium chloride + Water + Ammonia

NH4Cl + NaOH → NaCl +  H2O + NH3

More examples:

2NH4Cl +    Ca(OH)2  → CaCl2 + 2H2O + 2NH3
(NH4)2SO4 + 2NaOH→ Na2SO4 + 2H2O+ 2NH3

Ammonia as an Alkali

  1. By nature, ammonia is a covalent compound.
  2. Ammonia exists as gas at room temperature.
  3. Ammonia gas is soluble in water.
  4. Physical properties of ammonia:
    1. Pungent smell
    2. Colourless
    3. Turn litmus from red to blue

Oxide: Basic, Acidic, Neutral, or Amphoteric​

Basic Oxide

  1. Most oxides of metal, especially alkali and alkaline earth metals, are basic oxides.
  2. Basic oxides that dissolve in water are called alkalis. 
  3. A basic oxide is an oxide that shows basic properties in opposition to acidic oxides and that either
    1. reacts with water to form an alkali; or
    2. reacts with an acid to form a salt.

Examples:

  1. Sodium oxide, which reacts with water to produce sodium hydroxide
  2. Magnesium oxide, which reacts with hydrochloric acid to form magnesium chloride
  3. Copper(II) oxide, which reacts with nitric acid to form copper nitrate
Acidic Oxide
  1. Most non-metal oxides dissolve in water to form acids and are called acidic oxides.
  2. An acidic oxide is an oxide that either
    1. reacts with water to form an acid; or
    2. reacts with a base to form a salt.

Examples :

  1. Carbon dioxide reacts with water to produce carbonic acid.
  2. Sulfur dioxide, which does not form the non-existent sulfurous acid but does react with bases to form sulfites.
  3. Silicon dioxide, which does not react with water but will react with bases to form silicates

Note:

Not all oxide of non-metal is an acidic oxide. For example, carbon monoxide (CO) is neutral.
 

Amphoteric Oxide

  1. The metal oxides that can behave as both acids and bases and are said to be amphoteric oxides.
  2. Examples of amphoteric oxides are lead oxide, aluminium oxide and zinc oxide.
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