Bonding, Structure & Properties

    Cards (246)

    • Ionic Compounds: Describe in terms of electrons what happens when magnesium reacts with fluorine to form the ionic compound magnesium fluoride (MgF2).
    • Explain why sodium chloride is NaCl, but sodium oxide is Na2O.
    • Explain why the ball and stick model is not a true representation of the structure of an ionic compound.
    • Ammonia is a liquid between -77.7 °C and -33.3°C.
    • Use the kinetic theory to explain the three states of matter in this case.
    • Using the particle theory, predict how temperature and pressure affect the density of a fixed mass of gas.
    • Explain the limitations of the particle theory.
    • NaCl has a very high melting point, but can be easily crushed.
    • Explain why ionic compounds conduct electricity only when molten or dissolved in water.
    • Suggest how electrolysis can be used to separate lead selenide (PbSe).
    • Nitrogen gas is a diatomic molecule.
    • Explain how the atoms are joined together in nitrogen gas.
    • Explain why the melting point of hydrogen chloride is -115°C, whereas sodium chloride’s melting point is 801°C.
    • Sulphur hexafluoride SF6 is an insulating gas.
    • Explain the type of bonding present and explain why it is gaseous at STP (Standard Temperature and Pressure).
    • Ionic lattices are brittle.
    • Compare and contrast metallic and ionic bonding to explain why metallic compounds are not brittle.
    • Explain, in terms of structure and bonding why metals are good conductors of heat energy and electricity.
    • Alloying a metal can make the metal harder.
    • Explain the properties of diamond in terms of its structure and bonding.
    • Graphite can be used to reduce the friction between two substances.
    • Diamond coating would make smartphones and tablets far stronger but would remove their touch-screen capability.
    • Sun cream uses nanoparticles.
    • Some scientists believe there should be restrictions on the use of nano particles.
    • Explain some of the possible risks associated with the use of nanoparticles.
    • Explain how the atoms of Group 1 and Group 7 elements react with each other, in terms of their electronic structure.
    • Explain, using their position in the periodic table, what the charges on metallic and non-metallic ions relates to.
    • Explain how the ions are held together in solid magnesium oxide (MgO).
    • The PiXL Club Ltd, Company number 07321607, is the copyright holder of the resource "GCSE Chemistry AQA Topic – Bonding, structure and the properties of matter".
    • Coarse particles have diameters between 1 x 10-5m and 2.5 x10-6m.
    • Nanoparticles have different properties from those for the same materials in bulk due to their high surface area to volume ratio.
    • The uses of nanoparticles include medicine, electronics, cosmetics, sunscreens, deodorants, catalysts.
    • Nanoparticles are structures that are 1-100nm in size, a few hundred atoms.
    • Nanoparticles are smaller than fine particles.
    • Graphite conducts electricity due to each carbon having one delocalised electron.
    • Graphene is a single layer of graphite, 1 atom thick.
    • Fullerenes are molecules of carbon atoms with hollow shapes.
    • Graphite has layers of hexagonal rings and each carbon makes 3 covalent bonds.
    • Diamond does not conduct electricity due to the lack of delocalised electrons.
    • In a diamond, each carbon makes 4 covalent bonds.
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