SPM Chemistry Revision

02 Matter and the Atomic Structure
2.1 Basic Concepts of Matter
6 Topics | 2 Quizzes
2.1.1 Element and Compound
2.1.2 Three States of Matter
2.1.3 Inter-conversion between the States of Matter
2.1 4 Heating Curve
2.1.5 Cooling Curve
2.1 6 Melting Point, Boiling Point and the State of Matter
2.1.1 Matter 1
2.1.2 Matter 2
2.2 The Development of the Atomic Model
1 Topic
2.2.1 History of Development of the Model of Atom
2.3 Atomic Structure
5 Topics | 2 Quizzes
2.3.1 Modern Atomic Model
2.3.2 The Charge of Particles
2.3.3 Proton Number and Nucleon Number
2.3.4 Electron Arrangement in Atom
2.3.5 Valence Electron
2.3.1 The Structure of Atom
2.3.2 Electrons Arrangement
2.4 Isotopes and Its Uses
1 Topic | 1 Quiz
2.4.1 Isotopes
2.4.1 Isotopes
03 The Mole Concept, Chemical Formula and Equation
3.1 Relative Atomic Mass and Relative Molecular Mass
2 Topics | 1 Quiz
3.1.1 Relative Atomic Mass
3.1.2 Relative Molecular Mass
3.1.1 Relative Atomic Mass and Relative Molecular Mass
3.2 Mole Concept
5 Topics | 4 Quizzes
3.2.1 Concept of Mole
3.2.2 Number of Mole and Number of Particles
3.2.3 Number of Mole of Atoms and Number of Mole of Molecules*
3.2.4 Number of Mole and Mass of a Substance
3.2.5 Number of Mole and Volume of Gas
3.2.1 Concept of Mole
3.2.2 Molar Mass of Substances
3.2.3 Molar Volume of Gases
3.2.4 Number of Mole of Solute
3.3 Chemical Formula
6 Topics | 3 Quizzes
3.3.1 Empirical Formula
3.3.2 Molecular Formula
3.3.3 Percentage of Mass*
3.3.4 Formula of Ions
3.3.5 Formula of Ionic Compounds
3.3.6 Formula of Molecules
3.3.1 Chemical Formulae
3.3.2 Formula of Molecule 1
3.3.3 Formula of Molecule 2
3.4 Chemical Equation
1 Topic | 1 Quiz
3.4.1 Chemical Equation*
3.4.1 Chemical Equations
04 The Periodic Table of Elements
4.1 Introduction to Periodic Table
3 Topics | 1 Quiz
4.1.1 History of Development of Periodic Table
4.1.2 Modern Periodic Table
4.1.3 Periodic Table and Electron Arrangement
4.1.1 Introduction to Periodic Table
4.2 Group 18 Elements
2 Topics | 1 Quiz
4.2.1 Group 18 Elements – Noble Gases
4.2.2 Uses of Group 18 Elements
4.2.1 Group 18 Elements
4.3 Group 1 Elements
5 Topics | 1 Quiz
4.3.1 Group 1 Elements – Alkali Metals
4.3.2 Chemical Properties of Group 1 Elements
4.3.3 Reaction of Alkali Metals with Chlorine
4.3.4 Reaction of Alkali Metals with Oxygen
4.3.5 Reaction of Alkali Metals with Water
4.3.1 Group 1 Elements
4.4 Group 17 Elements
6 Topics | 1 Quiz
4.4.1 Group 17 Elements – Halogens
4.4.2 Physical Properties of Group 17 Elements
4.4.3 Chemical Properties of Group 17 Elements
4.4.4 Reaction of Halogens with Water
4.4.5 Reaction of Halogens with Metals
4.4.6 Reaction of Halogens with Sodium Hydroxide
4.4.1 Group 17 Elements
4.5 Period and Transition Metal
1 Topic | 1 Quiz
4.5.1 Transition Metals
4.5.1 Period and Transition Metals
05 Chemical Bond
5.1 Basics of Compound Formation
5 Topics | 2 Quizzes
5.1.1 Stability of Noble Gases
5.1.2 Chemical Bond
5.1.3 Formation of Ion
5.1.4 Formation of Positive Ions
5.1.5 Formation of Negative Ions
5.1.1 Formation of Compounds
5.1.2 Formation of Ions
5.2 Ionic Bond
2 Topics | 1 Quiz
5.2.1 Ionic Bonding
5.2.1 Predicting the Formula of Ionic Compound
5.2.1 Ionic Bonding
5.3 Covalent Bond
3 Topics | 1 Quiz
5.3.1 Covalent Bonding
5.3.2 Covalent Compounds – Number of Bonds
5.3.3 Predicting the Molecular Formula of Covalent Compounds
5.3.1 Covalent Bonding
5.4 Hydrogen Bond
1 Topic
5.4.1 Hydrogen Bond
5.5 Dative Bond
1 Topic
5.5.1 Dative Bond
5.6 Metallic Bond
1 Topic
5.6.1 Metallic Bond
5.7 Properties of Ionic Compounds and Covalent Compounds
3 Topics
5.7.1 Physical Properties – Ionic Compounds
5.7.2 Physical Properties of Covalent Compounds
5.7.3 The Macromolecular Compounds
06 Acids, Bases and Salts
6.1 The Role of Water in Showing Acidic and Alkaline Properties
6 Topics
6.1.1 Acids
6.1.2 Basicity of Acids
6.1.3 Physical Properties of Acids
6.1.4 Bases
6.1.5 Physical Properties of Alkali
6.1.6 Role of Water to Show Properties of Acids
6.2 pH Value
1 Topic
6.2.1 pH Scale
6.3 Strength of Acids and Alkali
1 Topic | 1 Quiz
6.3.1 Strength of Acids/Alkalis
6.3.1 Strength of Acids and Alkalis
6.4 Chemical Properties of Acids and Alkalis
4 Topics | 4 Quizzes
6.4.1 Chemical Properties of Acids
6.4.2 Writing Ionic Equation of the Reactions of Acids
6.4.3 Chemical Properties of Bases/Alkalis
6.4.4 Oxide: Basic, Acidic, Neutral, or Amphoteric
6.4.1 Understanding Acids 1
6.4.2 Understanding Acids 2
6.4.3 Understanding Alkalis I
6.4.4 Understanding Alkalis II
6.5 Concentration of Aqueous Solution
6 Topics | 2 Quizzes
6.5.1 Solute, Solvent and Solution
6.5.2 Concentration of Solution
6.5.3 Conversion of the Unit of Concentration
6.5.4 Molarity and Number of Moles
6.5.5 Molarity and the pH Value of Acid or Alkali
6.5.6 Concentration of Acid
6.5.1 Concentration of Solutions
6.5.2 Dilution and Stoichiometry Calculation
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4.2.1 Group 18 Elements – Noble Gases

SPM Chemistry Revision 4.2 Group 18 Elements 4.2.1 Group 18 Elements – Noble Gases
  1. The “Noble Gases” are the last group in the Periodic Table, they also known as “inert gas”, due to their non-reactive behavior.
  2. This group consist of six elements, namely Helium, Neon, Argon, Kripton, Xenon and Radon.
  3. They are non-metallic, colourless gases at room temperature and pressure with very low melting points and boiling points.
  4. They form 1% of air, and most of this is argon.
  5. The size of atom increases down the group, due to the increase number of electron shell.
Name Proton number Electron arrangement Melting point Boiling point
Helium 2 2 -270°C -269°C
Neon 10 2.8 -249°C -246°C
Argon 18 2.8.8 -189°C -186°C
Krypton 36 2.8.18.8 -157°C -152°C
Xenon 54 2.8.18.18.8 -112°C -108°C
Radon 86 2.8.18.32.18.8 -71°C -62°C

Physical Properties

Solubility and Conductivity

  1. All noble gas are insoluble in water.
  2. They are not conductor of heat and electricity.

Melting Point and Boiling Point

  1. As show in the table above, the melting and boiling point of noble gases are very low.
  2. This is because all noble gases exist as monoatoms. The force in between all these atoms is the weak van de Waals’ Force.
  3. Therefore very little energy is needed to overcome this force during melting and boiling.

Density

  1. The density of noble gases are very low.
  2. Nevertheless, the density increases steadily down the group.
  3. Density of a substance is given by the equation “Density=Mass/Volume”.
  4. Down the group, both the mass and the volume increase, but increase of mass is faster than the volume, hence the density increases down the group.

Chemical Properties

  1. All the noble gases are non-reactive elements.
  2. This is because their valence shell is full of electrons.
  3. In the chemical world, an atom is in the chemically most stable state if their valence shell is full with eight electrons (or 2 electrons for the first shell.).
  4. Therefore all noble gases do not react with other elements, due to their stable electronic structure.
  5. They exist as single atoms, that is they are monatomic.
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