group 2 Flashcards
why are group 2 known as alkaline earth metals
- they react with water to form alkalis (metal hydroxides) and hydrogen.
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write an equation for the first ionisation energy of magnesium .
Mg (g) —> Mg+ (g) + e-
what happens to the first ionisation energy as you go down group 2? why?
- decreases as number of filled electron shells increases down group —> increased shielding, increased atomic radius —> weaker force between outer electron and nucleus —> less energy needed to remove electron
how does reactivity with water change as you go down group 2?
- increases (Mg lease —> Ba most)
- outer electrons get further away from nucleus , reducing nuclear attraction
- electron shielding increases, further reduces attraction between positive nucleus + outer electrons
- outer two electrons more easily lost to form +2 ions .
write an equation for the reaction of Barium and water.
- Ba (s) + 2H2O (l) —> Ba(OH)2 (aq) + H2 (g)
- metal + water —> metal hydroxide + hydrogen
write an equation for the reaction of magnesium and steam .
- Mg (S) + H2O (g) —> MgO (s) + H2 (g)
What’s the trend in hydroxide solubility down group 2?
- Increases down the group
- Mg(OH)2 is almost insoluble
- Ba(OH)2 creates strong alkaline solution.
what’s the trend in sulphate solubility down group 2?
- decreases down group
- MgSO4 is soluble
- BaSO4 is insoluble
What’s the equation when calcium oxide neutralises hydrochloric acid to form a salt and water ? (bases which neutralise acids)
- CaO + 2HCl —> CaCl2 + H2O
what’s the trend in melting point down group 2 ? why?
- decreases down group
- because sea of delocalised electrons is further from the positive charge of the nucleus —> weaker metallic bonds/ forces of attraction which take less energy to weaken.
what’s the trend in atomic radius down group 2?
- increases as more occupied electron shells down the group .
write the equation for the extraction of Titanium using Magnesium.
- TiO2 + 2Cl2 + C —> TiCl4 + CO2
- TiCl4 (l) + 2Mg (s) —> 2MgCl2 (s) + Ti (s)
what are flue gases ?
- gases produced by power stations which are harmful to environment
how can CaO or CaCO3 be used to remove flue gases? write equations
- CaCO3 (s) + SO2 (g) —> CaSO3 (s) + CO2 (g)
- CaO (s) + SO2 (g) —> CaSO3 (s)
what is Ca(OH)2 used for ? write an equation related to one of its uses.
- used to neutralise soil
- Ca(OH)2 (aq) + 2HCl (aq) —> 2H2O (l) + CaCl2 (aq)