C1

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  • Created by: ak27330
  • Created on: 03-11-19 14:40
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  • C1
    • History of the Atom
      • The plum pudding model
        • Dalton described atoms as solid spheres.
        • Different spheres, different elements.
        • A ball of positive charge with electrons stuck in it
      • Rutherford's nuclear model
        • Gold foil experiment
          • Fire positively charged alpha particles at thin sheet of gold.
            • Expecting- to pass through. Some were deflected.
        • tiny positive nucleus at centre, 'cloud' of negative electrons, mostly empty space.
      • Bohr's nuclear model
        • Rutherford's model- would cause atom to collapse.
        • Electrons orbit the nucleus at fixed distances.
      • The discovery of protons and neutrons
        • Discovered late 1920's
    • The Atom
      • protons- +1 charge, neutron- 0 charge, electron- -1 charge
      • Mass- proton=1, neutron=1, electrons= negligible
      • proton, neutron in nucleus, electrons on shell
    • Isotopes and Relative Atomic Mass
      • Isotopes- same number of protons, different number of neutrons
      • Relative Atomic mass- average mass of an atom
        • RAM= (sum of(isotope abundance X isotope mass number)) / sum of abundances
    • Development of the Periodic Table
      • Mendeleev- order of atomic mass
        • Left gaps so certain elements can be in certain groups due to chemical properties
    • The Modern Periodic Table
      • Sorted via atomic number, vertical= similar chemical properties
      • Period number= shells
    • Electronic configuration
      • shells= 2.8.8.
      • Group 0= full shell, noble gases
    • Ions
      • Charged particles- either lose or gain electrons
      • Cation- positive
      • Anions- negative
    • Ionic Bonding
      • Bond between non-metals and metals
    • Ionic Compounds
      • Strong electrostatic forces between oppositely charged ions
      • Properties
        • High melting and boiling point, to overcome strong electrostatic attraction
        • High solubility
        • Electrical conductivity- doesn't conduct electricity, does when melted or dissolved as ions are free to move and carry a charge
    • Covalent Bonding
      • Between non-metals where they share electrons, by electrostatic forces
    • Simple molecular substances
      • Tiny, atoms joined by covalent bonds
      • Properties
        • No electrical conductivity
        • low melting and boiling points
      • Polymers- long chains of covalntly bonded carbon
    • Giant Covalent Structures
      • Strong covalent bonds, high melting points and boiling points, aren't soluble
      • Diamond- four covalent bonds, rigid, high melting points, doesn't conduct.
      • Graphite- three covalent bonds, sheets of graphene, held w/ weak intermolecular forces, soft/slippery, conductor, high melting.
      • Fullerenes used in medicine, catalysts and strengthening materials.
    • Metallic Bonding
      • Giant structure, delocalised electrons, conduct electricity
      • High melting and boiling points, high conductivity, malleable, dense.
    • Relative Mass
      • Relative formula mass= masses of atoms in compound added together.
      • Empirical formula= simplest whole number ratio of atoms of each element within a compound.
      • Molecular formula- empirical formula of a compound with the RFM to work out how it was originally.
    • No atoms can be destroyed or created.
    • Learn empirical formula separately.
    • Concentration(g dm-3)= mass of solute(g) / volume of solution(dm3)
    • The mole
      • Avogadro constant= 6.02 X 10^23
      • How many particles there are
      • Num of moles= mass(g) / RAM or RFM
    • Mass of product w/ balanced equation
      • If you know the mass of a product and have a balanced equation you can work out the other substances with it.
        • Limiting reactants- when a reactant is used up before reaction can finish.

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