Chemistry AS 1.

The Mole
1. A mole is the amount of particles in a substance.
2. 1 mole is equal to 6.02 x 10^23 particles. This number is known as the avogadro constant.
3. Number of moles= mass of substance / molar mass
4. Moles= number of particles you have / number of particles in a mole
Gas Volumes
1. If temperature and pressure stay the same, one mole of any gas will always have the same volume, 24dm^3 mol^-1.
2. Number of moles = volume in dm^3 / 24.
3. Ideal Gas Equation
  1. pV = nRT
    1. p= pressure(Pa)
    2. V= volume(m^3)
    3. n= number of moles
    4. R= gas constant (J K^-1 mol^-1)
      1. 8.314 J K^-1 mol^-1
    5. T= temperature (K)
Ionic Compounds
1. Ions are made when electrons tranfer.
2. Charges in ionic compounds always balance. Ionic compounds are made when positive and negative ions bond together.
Concentration Calculations
1. Number of moles= concentration x volume (in dm^3)
Acids and Bases and Salts
1. Acids are proton donors.
2. Bases are proton acceptors. Bases that are soluble in water (alkalis) release OH ions in solution.
3. Acids and bases react to form a salt and a water.
4. Acids React with Metals
  1. Metal + acid = metal salt + hydrogen.
  2. Metal oxide + acid = metal salt + water.
  3. Metal hydroxide + acid = salt + water.
  4. Metal carbonate + acid = metal salt + carbon dioxide + water.
5. Salts
  1. Salts are ionic compounds, all solid salts are made up of a lattice of positive and negative ions.
  2. Sometimes, water molecules are incorporated in the lattice too, this water is called the water of crystallisation.
  3. A salt containing water of crystallisation is hydrated, a salt is anhydrous if it doesn't contain water of crystallisation.
6. Ammonia reacts with acids to make ammonia salts.

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