Y11 Mock Revision Plan

Suggested revision dates	Revision objectives/what you need to be able to remember	Comments
26^th nov	Atomic structure protons, neutrons and electrons nucleus electrons arranged in shells how reactivity depends on electron arrangement	Volume 1 p32-34
27^th nov	Periodic table about the 100 elements arranged in order of ascending atomic number the position of the metals and non-metals the positions of Gp I, VII & 0 group properties and trends	Volume 1 p34
28^th nov	Halogens their properties (colour, boiling point and physical state at room temperature the reaction of chlorine with sodium and iron halogen displacement reaction uses of chlorine and iodine	Volume 1 p35
29^th nov	Rates of reaction how the rates change when the temperature is increased the concentration of reactant increases the concentration of a solid reactant increases a catalyst is used	Volume 1 p36-38
30^th nov	Collision theory rate of a reaction can be increased by increased frequency of collisions (more collisions more often) greater energy of the collisions how the rate of enzyme catalysed reactions vary with temperature and pH	Volume 1 p38
1^stDec	Atoms and Isotopes each element has an atomic number and atomic mass isotopes have the same number of protons and electrons but the number of neutrons varies calculate the relative atomic mass based on the abundances of each isotope	Volume 2 p42
2^ndDec	Chemical bonds IONIC how ionic bonds form between metals and non-metals formation of ionic bonds involves electron transfer and the formation of charged ions the properties of ionic compounds- HIGH MELTING POINTS, CONDUCT ELECTRICITY WHEN MOLTEN OR IN SOLUTION, GENERALLY SOLUBLE IN WATER	Volume 2 p44
3^rdDec	Chemical bonds COVALENT how covalent bonds form between atoms of non metals covalent bonds involve the sharing of electrons that covalent compounds fall into two groups-simple covalent and giant covalent simple covalent have low melting points and cannot conduct electricity giant covalent (diamond, graphite and silicon dioxide) have high melting points, poor solubility and cannot conduct electricity (except for graphite)	Volume 2 p45-46 Volume 2 p45-46
4^thDec	Energy transfers during reactions reactions can give out heat (EXOTHERMIC) or take in heat (ENDOTHERMIC) when bonds are broken energy is required and when bonds are formed energy is released, it is the balance between these that means the reaction is endo or exo	Volume 2 p47
5^thDec	Using chemical equations to calculate the Relative Atomic Mass Ar calculate the masses of products and reactants using equations working out formulae	Volume 2 p48-50
6^th -7^th Dec	Final revision of all objectives
	You will need to be able to recall the formulae the elements and simple compounds in Module 3 & 10 represent chemical reactions by word equations: write simple balanced equations and use the state symbol (s), (l), (g) and (aq) write balanced equations to describe and explain a wide range of reactions including ionic equations