Atomic structure and the periodic table

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What this unit covers

• A simple model of the atom, symbols, relative atomic mass, electronic charge and isotopes: Describe chromatography as a separation technique for mixtures.
• A simple model of the atom, symbols, relative atomic mass, electronic charge and isotopes: Describe filtration as a separation technique for suitable mixtures.
• A simple model of the atom, symbols, relative atomic mass, electronic charge and isotopes: State the relative electrical charge of a proton.
• A simple model of the atom, symbols, relative atomic mass, electronic charge and isotopes: Explain why atoms have no overall electrical charge when the number of electrons equals the number of protons.
• A simple model of the atom, symbols, relative atomic mass, electronic charge and isotopes: Define isotopes as atoms of the same element with different numbers of neutrons.
• A simple model of the atom, symbols, relative atomic mass, electronic charge and isotopes: State that atoms are very small, with a radius of about 0.1 nm.
• A simple model of the atom, symbols, relative atomic mass, electronic charge and isotopes: Interpret isotope abundance data to compare contributions to relative atomic mass.
• A simple model of the atom, symbols, relative atomic mass, electronic charge and isotopes: Explain why relative atomic mass is often not a whole number.
• A simple model of the atom, symbols, relative atomic mass, electronic charge and isotopes: Interpret electron-shell diagrams for atoms of the first 20 elements.
• A simple model of the atom, symbols, relative atomic mass, electronic charge and isotopes: Represent electronic structure using numbers such as 2,8,1 for sodium.
• A simple model of the atom, symbols, relative atomic mass, electronic charge and isotopes: Describe how discovery of the electron led to the plum pudding model.
• A simple model of the atom, symbols, relative atomic mass, electronic charge and isotopes: Explain why alpha particle scattering evidence led scientists to replace the plum pudding model.
• A simple model of the atom, symbols, relative atomic mass, electronic charge and isotopes: Define an atom as the smallest part of an element that can exist.
• A simple model of the atom, symbols, relative atomic mass, electronic charge and isotopes: (HT only) Write balanced half equations and ionic equations where appropriate.
• The periodic table: Describe the trend in boiling points of the noble gases down Group 0.
• The periodic table: Explain why noble gases do not easily form molecules.
• The periodic table: Identify Group 1 elements as alkali metals.
• The periodic table: Explain why Group 1 elements have similar chemical properties.
• The periodic table: Describe and explain why reactivity decreases down Group 7.
• The periodic table: Explain that halogens have seven electrons in their outer shell.
• The periodic table: Explain that elements in the same group have the same number of outer-shell electrons.
• The periodic table: Explain that columns in the periodic table are called groups.
• The periodic table: Explain how discovery of predicted elements supported Mendeleev's table.
• The periodic table: Explain how Mendeleev changed some element orders based on chemical properties.
• The periodic table: Describe where non-metals are found in the periodic table.
• The periodic table: Define metals as elements that react to form positive ions.
• Properties of transition metals (chemistry only): (chemistry only) Use named examples to illustrate typical transition-metal properties.
• Properties of transition metals (chemistry only): (chemistry only) Compare transition metals with Group 1 metals in terms of melting points.
• Properties of transition metals (chemistry only): (chemistry only) Describe that many transition metals form ions with different charges.
• Properties of transition metals (chemistry only): (chemistry only) Describe that many transition-metal compounds are coloured.