CH2 - Inorganic Chemistry
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- Created on: 23-05-16 11:27
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- CH2 - Inorganic Chemistry
- Periodic Table
- An element id placed into a period according to the number of occupied shells present in its atoms.
- E.G. Calcium/Ca is in period 4 because it has 4 occupied shells.
- An element is placed into a group according to the number of outermost electrons present in its atoms.
- E.G. Oxygen is in group 6 because its atoms have 6 outermost electrons.
- Trends Within the Periodic Table
- Ionisation Energies
- 1st Ionisation energy is the energy required to remove one mole of outermost electrons from one mole of gaseous atoms to form one mole of uni-positive ions.
- Down A Group
- 1st I.E decreases
- Outermost electron is progressively further from the nucleus.
- Outermost electron is more shielded from the nucleus by inner electrons.
- This outweighs the increasing nuclear charge.
- 1st I.E decreases
- Across A Period
- 1st I.E increases
- An electron is being added to the same energy level as you go across.
- No change in shielding or distance from the nucleus.
- Increasing nuclear charge
- An electron is being added to the same energy level as you go across.
- 1st I.E increases
- Electro-negativity
- Down A Group
- Electro-negativity decreases
- Shared pair of electrons that make up the covalent bond are further from the nucleus.
- They are less attracted to the nucleus.
- Shared pair of electrons that make up the covalent bond are further from the nucleus.
- Electro-negativity decreases
- Across A Period
- Electro-negativity increases
- Nuclear charge increases
- Shared pair of electrons making up the covalent bond are more strongly attracted to the nucleus.
- Nuclear charge increases
- Electro-negativity increases
- The ability of an atom to attract the shared pair of electrons in a covalent bond.
- Down A Group
- Melting Point
- Down A Metallic Group
- Melting points decrease
- Attraction between the uni-positive ions and the sea of delocalised electrons is the metallic bond.
- Positive ions increase in size as you descend the group.
- Because the 1+ charge is spread over an increasingly large area it is less effective in attracting the delocalised electrons.
- Positive ions have a lower 'charge to size ratio' as you descend the group.
- Down A Non-Metallic Group
- Melting points increase
- Molecules increase in size as you go down a group.
- Halogens exist as non-polar diatomic molecules, X2
- Number of electrons present increases.
- Greater instantaneous dipole - instantaneous dipole attractions between molecules of iodine (I2) than between molecules of fluorine (F2).
- At room temp. I2 is solid and F2 is a gas.
- Down A Metallic Group
- Ionisation Energies
- An element id placed into a period according to the number of occupied shells present in its atoms.
- Metallic Oxides
- Basic (alkaline) oxides
- They react with ACIDS to form SALT & WATER.
- Na2O + 2HCl
- 2NaCl + H2O
- Non-Metallic Oxides
- Acidic oxides
- They react with WATER to form an ACID.
- CaCl2 + H2O
- CaO + 2HCl
- Redox Reactions
- Electron Transfer
- Reduction Is Gain of electrons
- RIG
- Oxidation Is Loss of electrons
- OIL
- Reduction Is Gain of electrons
- Oxidation States
- Oxidation - the oxidation state of the element increases.
- Reduction - The oxidation state of the element decreases.
- Using electron transfer to identify redox reactions
- Mg(s)+CuSO4(aq)
- MgSO4(aq)+Cu(s)
- Mg (0) + Cu2+
- Mg2+ + Cu (0)
- Copper has been reduced because it has gained electrons.
- Magnesium has been oxidised because it has lost electrons.
- Mg2+ + Cu (0)
- Mg(s)+CuSO4(aq)
- Electron Transfer
- Periodic Table
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- SO4(2-) is not needed in the ionic equation because it is a spectator ion.
- It doesn't change its charge.
- SO4(2-) is not needed in the ionic equation because it is a spectator ion.
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