3.2.2 Group 2, the alkaline earth metals Flashcards
Atomic radius ____ down group 2 ?
Increases due to extra electrons and therefore shells
Ionisation energy ____ down group 2 and why ?
Decreases, due to more shielding and therefore a weaker attraction between nucleus and outer shell electrons making them easier to remove
Melting points generally ____ down the group and why ?
Decrease, as larger ions mean that the distance between the positive nuclei and delocalised electrons is greater which weakens the attractive force
What type of bonding is present in group 2 and what does this mean ?
Metallic bonding, positive metal ions attracted to a negative delocalised sea of electrons
Does reactivity increase or decrease down the group ?
Reactivity increases down the group as there is more shielding
Do group 2 metals act as acids or bases ?
Bases, they are alkaline metals
When group 2 metals react with water, what do they form ?
Metal hydroxides. e.g Mg(OH)2
Group 2 sulphates and hydroxides have ____ solubility as we go down the group
Opposite
Generally if the negative ion has a double charge they become _____ soluble down the group e.g SO4^2-
Less
Generally if a negative ion has a single charge they become _____ soluble down the group e.g OH-
More
What solution is used to test for sulphates ?
Barium chloride
Why must HCl be added before barium chloride ?
In order to remove any carbonate ions that may give a false positive
What is the positive result for a sulphate test with barium chloride ?
White precipitate will be formed, the precipitate is barium sulphate and is insoluble
What group 2 metal is used for medical reasons and what does it do ?
Mg(OH)2, it is used to neutralise stomach acids
What is the ionic equation for neutralisation ?
H+(aq) + OH-(aq) —-> H2O(l)