Year 11 students, check the dates!
The periodic table provides chemists with a structured organisation of the known chemical elements from which they can make sense of their physical and chemical properties. The historical development of the periodic table and models of atomic structure provide good examples of how scientific ideas and explanations develop over time as new evidence emerges. The arrangement of elements in the modern periodic table can be explained in terms of atomic structure which provides evidence for the model of a nuclear atom with electrons in energy levels.
Objectives. You should be able to:
Describe the basic structure of an atom.
Explain, including diagrams, the difference between a pure element, a mixture, and a compound.
Name and give the chemical symbol of the first 20 elements in the Periodic Table.
Study Resources
Objectives. You should be able to:
Explain why mass is conserved in a chemical reaction.
Describe familiar chemical reactions with balanced symbol equations including state symbols.
Balance given symbol equations.
Study Resources
Objectives. You should be able to:
Explain the difference between a compound and a mixture.
Explain how the chemical properties of a mixture relate to the chemical it is made from.
Describe different separation techniques.
Study Resources
Objectives. You should be able to:
Describe the process of fractional distillation.
Explain the main processes occurring in paper chromatography.
Safely make & analyse a paper chromatogram
Study Resources
Objectives. You should be able to:
List the significant models proposed for atoms.
Identify the key parts of the plum-pudding model and the nuclear model of the atom.
Describe the differences between the plum-pudding model and the nuclear model of the atom.
Explain how evidence from scattering experiments changed the model of the atom.
Study Resources
Objectives. You should be able to:
State the relative charges and masses of sub-atomic particles.
Describe atoms using the atomic model.
Explain why atoms have no overall charge.
Use atomic number and mass numbers of familiar atoms to determine the number of each sub-atomic particle.
Study Resources
Objectives. You should be able to:
State what an ion is.
Define an isotope.
State the relative sizes of an atom and its nucleus.
Explain why ions have a charge.
Use atomic number and mass numbers of familiar ions to determine the number of each sub-atomic particle.
Study Resources
Objectives. You should be able to:
State that electrons are found in energy levels of an atom.
State the maximum number of electrons in the first three energy levels.
Write the standard electronic configuration notation from a diagram for the first 20 elements.
Explain why elements in the same group react in a similar way.
Study Resources
You should be able to:
List the significant models for ordering the elements.
Describe how the elements are arranged in groups and periods in the periodic table.
Explain why the periodic table was a breakthrough in how to order elements.
Study Resources
You should be able to:
Define a group and period in the periodic table.
Describe how the electronic structure of metals and non-metals are different.
Explain in terms of electronic structure how the elements are arranged in the periodic table.
Explain why the noble gases are unreactive and the trend in their boiling points.
Study Resources
You should be able to:
Name the first three elements in Group 1.
Explain why the elements in Group 1 react similarly and why the first three elements float on water.
Describe how you can show that hydrogen and metal hydroxides are made when Group 1 metals react with water.
Study Resources
You should be able to:
Name the first four elements in Group 7.
Explain why the elements in Group 7 react similarly.
Explain how to complete a halogen displacement reaction and explain what happens in the reaction.
Study Resources
You should be able to:
State that Group 0 elements are unreactive.
Use data to describe a trend in physical properties of Group 0 elements.
Explain how electronic structure is linked to the chemical properties of Group 0 elements.
Use data to show a trend in physical properties and predict missing values for Group 0 elements.
Study Resources
You should be able to:
State the trend in reactivity in Group 1.
State the trend in reactivity in Group 7.
Explain how electronic structure affects the trend in reactivity of Group 1 and Group 7 elements.
Use the nuclear model to explain how the outer electrons experience different levels of attraction to the nucleus.
Study Resources
You should be able to:
List the typical properties of transition metals and their compounds.
Describe how the properties of Group 1 metals compare with transition metals.
Interpret the formula and names of familiar transition metal compounds.
Study Resources
Other Resources