C1 - Chemistry

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  • C1
    • 1.1 Atoms
      • An element is  is an atom which cannot be chemically broken down into anything smaller.
      • Can be mixtures, compound or a pure element.
        • Mixture: two or more element physically combined.
        • A solution must consist of a solute and solvent, and contain two or more elements
        • A pure element only contains atoms of that element.
      • Elements are made of electrons, protons and neutrons. They have a positive nucleus and negative electrons in shells
        • These shells fill up with the first having 2 electrons and the rest having a maximum of 8.
      • Using the chemical symbols in the equation mean that anyone no matter the language knows what element it is. Also it means you don’t have to write the whole name each time
    • 1.2 Chemical equations
      • Law Conservation of Mass
        • Mass Cannot be created or destroyed it can only be transformed from one state to another.
    • 1.3 Seperating Mixtures
      • A compound is when two or more elements are chemically bonded.
      • Can be mixtures, compound or a pure element.
        • Mixture: two or more element physically combined.
        • A solution must consist of a solute and solvent, and contain two or more elements
        • A pure element only contains atoms of that element.
      • Chromatography
        • Chromatography can be used to separate ink by using a solid and a liquid.
      • Distillation
      • Evaporation
        • Evaporation works by heating a liquid so that it evaporates, the vapour can then be collected and a solid will be left.
      • Filtration
        • Can be used to separate a solid like dirt from a liquid, for example water.
    • 1.4 Fractional distillation and Chromotography
      • When doing chromatography the line must be drawn in pencil and the ink place on it. Only the bottom of the paper should be touching the water.
      • Fractional Distillation is done by heating up the liquid t the boiling point of the first liquid causing it to evaporate and be collected. this process is then repeated at the different boiling points.
    • 1.5 History of the atom
      • The Plum Pudding Model
        • Discovered By Thomson
      • Billiard Ball Model
        • Discovered by Dalton
        • Idea of an indivisible atom
      • Rutherford Model
        • Discovered by Rutherford
        • Golden Foil experiment. Found a concentration of positive matter (protons) in the centre with electrons surrounding it..
      • Bohr’s model
        • Idea of protons and neutrons in the nucleus with shells of electrons.
    • 1.6 Structure of the atom
      • Atoms have an overall charge of 0 due to the electrons and protons cancelling each other out.
      • The Mass number is the bigger number and shows how many protons and neutrions an element has
      • The Atomic number shows how many protons are in an element. As the number of protons and electrons are always equal the also shows the number of electrons
    • 1.7 Ions, Atoms and Isotopes
      • Ions are atoms with a charge due to being bonded to another element. This means they have either lost or gained an electron.
      • Isotopes are atoms with less or extra neutrons
      • Chlorine doesn’t have a whole mass number due to having two common isotopes, 35 and 37. The equation take s into account the percentage. Which is 75% and 25% therefore giving it 35.5.
    • 1.8 Electronic Structure
      • The maximum number of electrons in the first shell is 2 then the rest can have up to 8. A sell must be complete before another is created.
      • Elements in the same group act in a similar way due to having the same number of electrons in their outer shell

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