Group 2: called alkaline earth metals due to their oxides and hydroxides being alkaline
They are S-Block element but are less reactive than Group 1
Electron Arrangement
All have 2 electrions in the highest energy level
The Sizes of the Atoms
Atoms get bigger down the group
Atomic radii increases due to extra filled energy level
Melting Points
High melting points due to giant metallic structure.
Decreases down the group due to sea of delocalised electrons being further away from the nucleus so metallic bonds strength decreases down the group
Magnesium has the lowest melting point due to different lattice arrangement of atoms
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Physical Properties Cont.
Ionisation Energies
All reactions in group 2 they lose their 2 highest energy electrons to form positive ions
M -> M2+ + 2e- : 1st and 2nd Ionisation energies together
Both the 1st and 2nd ionisation energies decrease down the group
Takes less energy to remove the electrons as they become further away from the nucleus
The nucleus also experiences more shielding by extra electron energy level
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The Chemical Properties Mg to Ba
Oxidation is the loss of electrons, all group 2 metals are oxidised
The metals have oxidation states that change from 0 to 2+
These are redox reactions
Reaction with Water
The metals get more reactive down the group
M(s) + 2H2O(l) -> M(OH)2(aq) + H2(g)
Magnesium reacts slowly with cold water but rapidly with steam to form an alkaline oxide and hydrogen:
Mg(s) + H20(g) -> MgO(s) + H2(g)
Calcium reacts more vigorously, then strontium and barium
Calcium Hydroxide (Slaked Lime) is used to treat acidic soil
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Chemical Properties Cont.
Hydroxide
Down the group the hydroxides become more soluble
The hydroxides are white solids
Magnesium Hydroxide is almost insoluble
Calcium hydroxide is sparingly soluble, its used in lime water
Strontium Hydroxide is more soluble
Barium Hydroxide dissolves to produce a strong alkaline solution
Ba(OH)2(s) + aq -> Ba2+(aq) + 2(OH)-(aq)
Sulfates
They become less soluble down the group
Barium Sulfate:outlines the gut as it absorbs x-rays and since it's insoluble it's safe
Barium sulfate is used to test sulfate ions: first acidified with nitric/hydrochloric acid, barium chloride is added to the solution, if sulfate is present a white precipitate is formed
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