Metallic Bonding -Chemistry

Subdecks (3)

Cards (44)

  • Properties of metals
    • They conduct heat: let's heat flow through them easily
    • They conduct electricity: let's electricity flow through them easily
    • They have high melting points
    • They are strong and tough but bendable
    • They will shine when freshly cut or scratched
    • They have higher densities than non metals
  • Alloy
    A mixture of a metal plus other metals or non metals, eg carbon
  • Pure metals are too soft for many uses, so they can be made harder by adding another element to the pure metal forming an alloy
  • Metals are good conductors of heat and electricity

    Because they have free delocalised electrons that are free to move throughout the structure
  • Metals have high melting points

    Because a lot of energy is needed to overcome the attraction between metal ions and delocalised electrons
  • Elements
    All of the atoms are the same
  • Compounds
    Contain two or more different elements chemically combined in fixed proportions
  • Mixtures
    Different elements or compounds, but they are not chemically combined
  • Filtration
    Used to separate a soluble solid from a liquid
  • Crystallisation
    1. Used to separate a soluble solid from a liquid
    2. Can happen faster for the water to evaporate by gently heating the solution
  • Simple distillation
    Used to separate a soluble solid from a liquid, but you save the water
  • Fractional distillation
    Used to separate two or more liquids with different boiling points
  • Paper chromatography
    Used to separate dissolved substances from another based on their different solubilities, e.g. ink and food colouring
  • Plum pudding model
    • An atom is a ball of positive charge with negative electrons embedded in it
  • Alpha scattering experiment
    1. Scientists fired tiny, positive alpha particles at a piece of gold foil
    2. Some particles deflected (changed direction) as they passed through
    3. Some bounced back
    4. This tells us the centre of the atom must have a positive charge as some atoms were deflected
  • John Newlands
    • Arranged elements in increasing atomic weight, invented "Law of Octaves"
  • Dmitri Mendeleev
    • Arranged elements in increasing atomic weight, switched some elements so they would fit into the same group with similar patterns
    • Left gaps in areas he thought an element was missing, predicted the properties of undiscovered elements with elements in the same group
  • Atomic mass number
    • The centre part of the atom is the nucleus
    • Electrons have a negative charge (-1)
    • Protons have a positive charge (+1)
    • Neutrons have a neutral charge (0)
  • Isotopes
    Atoms of the same element with a different amount of neutrons, but the same amount of protons
  • Ions
    Atoms that have an overall charge, because they have lost or gained electrons