End first term exam checklist

Thus far we have taken 2 tests and done commendably on the whole and I am confident that we will all do brilliantly.

As we were all given a copy of the syllabus at the beginning of the year we know what the IGCSE syllabus contains so there’s no point in replicating that information here, though that will provide you with good guidance of the information that you will need to know. If you have lost your copy o want another copy of that syllabus it can be downloaded and printed from the Cambridge website at http://www.cie.org.uk/

In addition to the information contained there what follows is a checklist of the skills you should have picked up in Chemistry so far.

By the time we have broken up for exams you will be able to:

• describe the states of matter and explain their interconversion in terms of the kinetic particle theory
  
• describe and explain diffusion
  
• describe evidence for the movement of particles in gases and liquids
  
• describe dependence of rate of diffusion on molecular mass (treated qualitatively)
  
• state the relative charges and approximate relative masses of protons, neutrons and electrons
  
• define proton number and nucleon number
  
• use proton number and the simple structure of atoms to explain the basis of the Periodic table (see section 9), with special reference to the elements of proton number 1 to 20
  
• define isotopes
  
• state the two types of isotopes as being radioactive and non-radioactive
  
• state one medical and one industrial use of radioactive isotopes
  
• describe the build-up of electrons in ‘shells’ and understand the significance of the noble gas electronic structures and of valency electrons.
  
• (Note that a copy of the Periodic Table will be available in the examination)
  
• describe the Periodic Table as a method of classifying elements and its use to predict properties of elements
  
• describe the change from metallic to non-metallic character across a Period
  
• describe the relationship between Group number, number of valency electrons and metallic/non-metallic character
  
• describe lithium, sodium and potassium in Group I as a collection of relatively soft metals showing a trend in melting point, density, in reaction with water.
  
• predict the properties of other elements in the Group, given data, where appropriate
  
• describe chlorine, bromine and iodine in Group VII as a collection of diatomic non-metals showing a trend in colour, state and their reaction with other halide ions
  
• predict the properties of other elements in the Group given data, where appropriate
  
• identify trends in other Groups given information about the elements concerned
  
• describe the transition elements as a collection of metals having high densities, high melting points, and forming coloured compounds, and which, as elements and compounds, often act as catalysts.
  
• describe the noble gases as being unreactive
  
• describe the uses of the noble gases in providing an inert atmosphere, i.e. argon in lamps; helium for filling balloons
  
• describe the general physical and chemical properties of metals
  
• explain why metals are often used in the form of alloys
  
• Identify representations of alloys from diagrams of structures
  
• describe metallic bonding as a lattice of positive ions in a ‘sea of electrons’ and use this to describe the electrical conductivity and malleability of metals
  
• place in order of reactivity; calcium; copper, (hydrogen), iron, magnesium potassium, sodium and zinc by reference to the reactions, if any, of the metals with water or steam dilute hydrochloric acid and the reduction of their oxides with carbon
  
• deduce an order of reactivity from a given set of experimental results
  
• describe the differences between elements, mixtures and compounds, and between metals and non-metals.
  
• describe alloys, such as brass, as a mixture of a metal with other elements.
  
• describe the formation of ions by electron loss or gain
  
• describe the formation of ionic bonds between elements from Groups I and VII
  
• describe the formation of ionic bonds between metallic and non-metallic elements
  
• describe the lattice structure of ionic compounds as a regular arrangement of alternating positive and negative ions
  
• Describe the reactivity series as related to the tendency of a metal to form its positive ion, illustrated by its reaction, if any, with the aqueous ions, the oxides, of the other listed metals
  
• describe the action of heat on the hydroxides and nitrates of the listed metals
  
• account for the apparent unreactivity of aluminium in terms of the oxide layer which adheres to the metal
  
• describe the ease in obtaining metals from their ores by relating the elements to the reactivity series
  
• describe the essential reactions in the extraction of iron from hematite
  
• describe the conversion of iron into steel
  
• describe in outline, the extraction of zinc from zinc blende
  
• name the main ore of aluminium
  
• name the uses of aluminium: in the manufacture of aircraft because of its strength and low density; in food containers because of its resistance to corrosion
  
• describe the idea of changing the properties of iron by the controlled use of additives to form steel alloys
  
• name the uses of mild steel (car bodies and machinery) and stainless steel (chemical plant and cutlery)
  
• name the uses of zinc for galvanising and for making brass
  
• name the uses of copper related to its properties; electrical wiring and in cooking utensils

and by the end of this week we should be able to tick every single thing in that list and begin revision and exam practice next week.