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REVISION NOTES

IGCSE Edexcel Chemistry

1.4 The Periodic Table

1.4.1 Understand how elements are arranged in the Periodic Table:

  • In order of atomic number
  • In groups and periods.

Elements on the periodic table are arranged in order of increasing atomic number.

GROUPS

  • Vertical columns in the table
  • Group number shows the number of valence (outermost shell) electrons
    • E.g. elements in group 2 have 2 electrons in the valence shell
  • The final group is called group 18 or 8 or 0

PERIODS

  • Horizontal rows in the table
  • Period number shows the number of electron shells in an atom
    • E.g. elements in period 2 have two electron shells
edexcel_igcse_chemistry_topic 04_the periodic table_001_periodic table-01

1.4.2 Understand how to deduce the electronic configurations of the first 20 elements from their positions in the Periodic Table

Deducing total number of electrons

  • Number of electron = number of proton = atomic number (for an atom)

Each electron shell can accommodate a fixed number of electrons

  • 1st shell: 2 electrons
  • 2nd shell: 8 electrons
  • 3rd shell: 8 electrons
edexcel_igcse_chemistry_topic 04_the periodic table_002_electron shells diagram labelled-01

Electronic Configuration of First 20 Elements

1.4.3 Understand how to use electrical conductivity and the acid-base character of oxides to classify elements as metals or non-metals

edexcel_igcse_chemistry_topic 04 tables_the periodic table_002_metals vs non metals-01

1.4.4 Identify an element as a metal or a non-metal according to its position in the Periodic Table

In general,

  • Metals are on the left of the periodic table
  • Non-metals are on the right of the periodic table
  • They are separated by metalloids (semimetals) which form a zig-zag line
edexcel_igcse_chemistry_topic 04_the periodic table_001_periodic table-01

1.4.5 Understand how the electronic configuration of a main group element is related to its position in the Periodic Table

Period number: number of electron shells

Group number: number of electrons in the outer shell

1.4.6 Understand why elements in the same group of the Periodic Table have similar chemical properties

  • The chemical properties of an element depend on the number of electrons in the outer shell
  • Elements in the same group have same number of electrons in the outer shell
  • Therefore, elements in the same group have similar chemical properties

1.4.7 Understand why the noble gases (Group 0) do not readily react

  • Noble gases (group 0) have 8 electrons in their outer shell (except for helium, which has 2)
  • Noble gases reach octet rule, meaning that they have full electron shells
  • They do not lose or gain electrons easily
  • Therefore, they are unreactive and do not easily form molecules
Back
Next
1. Principles of Chemistry

1.1 State of Matter

1.2 Elements, Compounds and Mixtures

1.3 Atomic Structure

1.4 The Periodic Table

1.5 Chemical Formulae, Equations and Calculations

1.6 Ionic Bonding

1.7 Covalent Bonding

1.8 Metallic Bonding

1.9 Electrolysis

2. Inorganic Chemistry

2.1 Group 1 (Alkali Metals) – Lithium, Sodium and Potassium

2.2 Group 7 (Halogens) – Chlorine, Bromine and Iodine

2.3 Gases in the Atmosphere

2.4 Reactivity Series

2.5 Extraction and Uses of Metals

2.6 Acids, Alkalis and Titrations

2.7 Acids, Bases and Salt Preparations

2.8 Chemical Tests

3. Physical Chemistry

3.1 Energetics

3.2 Rates of Reaction

3.3 Reversible Reactions and Equilibria

4. Organic Chemistry

4.1 Introduction

4.2 Crude Oil

4.3 Alkanes

4.4 Alkenes

4.5 Alcohols

4.6 Carboxylic Acids

4.7 Esters

4.8 Synthetic Polymers

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