<p>State the relative charges and approximate relative masses of protons, neutrons and electrons<br /> Define proton number (atomic number) as the number of protons in the nucleus of an atom<br /> Define nucleon number (mass number) as the total number of protons and neutrons in the nucleus of an atom<br /> Use proton number and the simple structure of atoms to explain the basis of the Periodic Table, with special reference to the elements of proton number<br /> Define isotopes as atoms of the same element which have the same proton number but a different nucleon number<br /> Understand that isotopes have the same properties because they have the same number of electrons in their outer shell<br /> State the two types of isotopes as being radioactive and non-radioactive<br /> State one medical and one industrial use of radioactive isotopes<br /> Describe the build-up of electrons in ‘shells’ and understand the significance of the noble gas.<br /> electronic structures and of the outer shell electrons.<br /> Explain Inertness of group zero elements.</p>

<p>Describe the Periodic Table as a method of classifying elements and its use to predict properties of elements.<br /> Describe the change from metallic to nonmetallic character across a period.<br /> Describe and explain the relationship between Group number, number of outer shell electrons and metallic/non-metallic character.<br /> Describe lithium, sodium and potassium in Group I as a collection of relatively soft metals showing a trend in melting point, density and reaction with water.<br /> Predict the properties of other elements in Group I, given data, where appropriate</p>

<p>Describe the differences between elements, mixtures and compounds, and between metals and non-metals<br /> Describe an alloy, such as brass, as a mixture of a metal with other elements<br /> Describe the formation of ionic bonds between metallic and non-metallic elements.<br /> Describe the lattice structure of ionic compounds as a regular arrangement of alternative positive and negative ions.<br /> Describe the formation of single covalent bonds in H2, Cl2, H2O, CH4, NH3 and HCl as the sharing of pairs of electrons leading to the noble gas configuration.<br /> Describe the electron arrangement in more complex covalent molecules such as N2, C2H4, CH3OH and CO2.<br /> Describe the macromolecular structure of silicon(IV) oxide (Silicon dioxide)<br /> Describe the similarity in properties between diamond and silicon (IV) oxide, related to their structures.<br /> Describe the differences in volatility, solubility, electrical conductivity between ionic and covalent compounds.<br /> Explain the differences in melting point and boiling point of ionic and covalent compounds in terms of attractive forces.</p>

<p>Name appropriate apparatus for the measurement of time, temperature, mass and volume, including burettes, pipettes and measuring cylinders<br /> Demonstrate knowledge and understanding of paper chromatography<br /> Interpret simple chromatograms, including the use of Rf values<br /> Outline how chromatography techniques can be applied to colourless substances by exposing chromatograms to substances called locating agents.</p>