GCSE Chemistry Revision Notes
UNIT 1: Monday 22 May 9:15-10:30
1.1: Atomic Structure
1.2: Bonding
1.3: Structures
1.4: Nanoparticles
1.5: Symbols, Formulae and Equations
1.6: The Periodic Table
1.7: Quantitative Chemistry
1.8: Acids, Bases and Salts
1.9: Chemical Analysis
1.10: Solubility
UNIT 2: Tuesday 13 June 9:15-10:45
2.1: Metals and Reactivity Series
2.2: Redox, Rusting and Iron
2.3: Rates of Reaction
2.4: Equilibrium
2.5: Organic Chemistry
2.6: Quantitative Chemistry
2.7: Electrochemistry
2.8: Energy Changes in Chemistry
2.9: Gas Chemistry
,PRESCRIBED PRACTICALS
C1: Determining the mass of water in hydrated crystals.
C2: Investigating the reactions of acids.
C3: Investigating the preparation of soluble salts.
C4: Identifying the ions in an ionic compound using chemical tests.
C5: Investigating the reactivity of metals.
C6: Investigating how changing a variable changes the rate of reaction.
C7: Investigating the reactions of carboxylic acids.
C8: Determining the reacting volumes and concentration of solutions of acid
and alkali by titration.
C9: Investigating the preparation, properties, tests and reactions of the gases
hydrogen, oxygen and carbon dioxide.
,1.1: Atomic Structure
History of Structure of Atom
1897 – An early model of the atom was the ‘plum pudding’ model. Devised by JJ Thompson, it consisted of
negative electrons embedded in a positive sphere.
1911 – Ernest Rutherford revised this model and suggested that an atom had a positive nucleus at its centre,
orbited by negatively-charged electrons.
In 1932, James Chadwick discovered the neutron. It took the longest to discover because it has no charge. This
completed the modern idea of the atom.
Today, scientists use an atomic model that has:
-a central positively charged nucleus containing positively charged protons and neutral neutrons (most of
mass).
-negatively charged electrons orbiting the nucleus in shells.
Protons, Neutrons and Electrons
, Subatomic Particle Relative Mass Relative Charge Location in Atom
Proton 1 +1 In nucleus
Neutron 1 0 In nucleus
Electron 1/1840 -1 In shells surrounding nucleus
Atomic Number = The number of protons in an atom.
Mass Number = The total number of protons and neutrons in an atom.
An atom as a whole has no electrical charge because the number of protons is equal t the number of
electrons.
In an atom:
Number of Protons = Number of Electrons = Atomic Number
Number of Neutrons = Mass Number – Atomic Number
Electronic Configuration
Electrons orbit the nucleus in shells.
1. Each shell is at a different distance from the nucleus, and each hold a different number of electrons.
2. Electrons enter the shell closest to the nucleus first. When it is filled, they begin to fill the next closest shell.
Shell Maximum
1 2
2 8
3 8
4 2
(above table is for elements with atomic numbers 1-20)
The electronic configuration may be shown in a diagram. For example sodium. Sodium has 11 electrons. It has
2 electrons in the first shell, 8 electrons in the second shell and 1 electron in the third shell. You can write
sodium’s electronic configuration with numbers and commas; 2,8,1.
In a diagram, electrons are represented by dots or crosses.
UNIT 1: Monday 22 May 9:15-10:30
1.1: Atomic Structure
1.2: Bonding
1.3: Structures
1.4: Nanoparticles
1.5: Symbols, Formulae and Equations
1.6: The Periodic Table
1.7: Quantitative Chemistry
1.8: Acids, Bases and Salts
1.9: Chemical Analysis
1.10: Solubility
UNIT 2: Tuesday 13 June 9:15-10:45
2.1: Metals and Reactivity Series
2.2: Redox, Rusting and Iron
2.3: Rates of Reaction
2.4: Equilibrium
2.5: Organic Chemistry
2.6: Quantitative Chemistry
2.7: Electrochemistry
2.8: Energy Changes in Chemistry
2.9: Gas Chemistry
,PRESCRIBED PRACTICALS
C1: Determining the mass of water in hydrated crystals.
C2: Investigating the reactions of acids.
C3: Investigating the preparation of soluble salts.
C4: Identifying the ions in an ionic compound using chemical tests.
C5: Investigating the reactivity of metals.
C6: Investigating how changing a variable changes the rate of reaction.
C7: Investigating the reactions of carboxylic acids.
C8: Determining the reacting volumes and concentration of solutions of acid
and alkali by titration.
C9: Investigating the preparation, properties, tests and reactions of the gases
hydrogen, oxygen and carbon dioxide.
,1.1: Atomic Structure
History of Structure of Atom
1897 – An early model of the atom was the ‘plum pudding’ model. Devised by JJ Thompson, it consisted of
negative electrons embedded in a positive sphere.
1911 – Ernest Rutherford revised this model and suggested that an atom had a positive nucleus at its centre,
orbited by negatively-charged electrons.
In 1932, James Chadwick discovered the neutron. It took the longest to discover because it has no charge. This
completed the modern idea of the atom.
Today, scientists use an atomic model that has:
-a central positively charged nucleus containing positively charged protons and neutral neutrons (most of
mass).
-negatively charged electrons orbiting the nucleus in shells.
Protons, Neutrons and Electrons
, Subatomic Particle Relative Mass Relative Charge Location in Atom
Proton 1 +1 In nucleus
Neutron 1 0 In nucleus
Electron 1/1840 -1 In shells surrounding nucleus
Atomic Number = The number of protons in an atom.
Mass Number = The total number of protons and neutrons in an atom.
An atom as a whole has no electrical charge because the number of protons is equal t the number of
electrons.
In an atom:
Number of Protons = Number of Electrons = Atomic Number
Number of Neutrons = Mass Number – Atomic Number
Electronic Configuration
Electrons orbit the nucleus in shells.
1. Each shell is at a different distance from the nucleus, and each hold a different number of electrons.
2. Electrons enter the shell closest to the nucleus first. When it is filled, they begin to fill the next closest shell.
Shell Maximum
1 2
2 8
3 8
4 2
(above table is for elements with atomic numbers 1-20)
The electronic configuration may be shown in a diagram. For example sodium. Sodium has 11 electrons. It has
2 electrons in the first shell, 8 electrons in the second shell and 1 electron in the third shell. You can write
sodium’s electronic configuration with numbers and commas; 2,8,1.
In a diagram, electrons are represented by dots or crosses.
