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Group 2 (Metal oxides with water (Not a redox reaction, Solubility of…
Group 2
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Group 2 sulfates
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Testing for sulfate ion- add solution of barium chloride/ nitrate to solution -if sulfate ions present a white ppt of barium sulfate formed
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Group 1 and 2 carbonates
Because size of metal cation increase so its charge density decreases and therefore the ability to polarise the CO3 2- and weaken the C-O bond decreases
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Group 1 carbonates only lithium carbonate decomposes on heating and all of gp 1 carbonates are stable to heating for the same reason
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Trends
First ionisation energy decreases as you go down group 2 because e- is being removed from a shell that is further from the nucleus and so there is less electrostatic attraction from the nucleus. Also there is more shielding from inner electrons
When group 2 metals react they lose their 2 outer electrons to form 2+ ions. Reactivity increases down the group because of the same reasons as 1st ionisation energy
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Reactions with water
eg. calcium +water -> calcium hydroxide + hydrogen can be asked to use half equations and oxidation numbers
Magnesium reacts slowly in cold water to form magnesium hydroxide HOWEVER, when reacted with steam it forms magnesium oxide
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Reactions with oxygen
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Can be asked to do oxidation numbers and half equations. For example Mg + Mg2+ + 2e- and O2 + 4e- -> 2O2-
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