Studied by 14 people
Describe the trend in ionisation energy down group 2.
There is an extra electron shell compared to the one above, extra inner shells shield the outer electrons from the attraction of the nucleus. The extra shells means the outer electrons are further away from the nucleus.
Group 2 react with water to produce?
Hydroxides. M(OH)2
Group 2 burn in oxygen to form?
Oxides MO
Group 2 react with chlorine to form?
Chlorides, MCl2
Explain the trend in reactivity of Group 2 down the group.
Increases. The higher the ionisation energy the less likely they are to react.
Which group 2 oxide is insoluble.
Beryllium oxide
Group 2 oxides react with H20 to form?
Hydroxides M(OH)2
Group 2 oxides react with dilute acid to form?
Salt, MCl2, and H2O
Hydroxides react with water to form?
Hydroxide M(OH)2
Hydroxides react with dilute acid to form?
Salt MCl2 and water
Describe the solubility trend of the hydroxides down group 2.
Solubility increases.
Describe the solubility trend of the group 2 sulphates.
Decreases.
Which group 2 sulphate is insoluble?
Barium sulfate
Explain why thermal stability increases down a group.
As the ionic radius of the cation gets larger they cause less distortion of the anion, due to the lower charge density, thus more stable the carbonate/nitrate compound.
Why are group 2 compounds less thermally stable than group1.
They have a higher charge thus they cause greater distortion to the anion and the less stable the carbonate/nitrate compound becomes.
Group 1 carbonates decompose to form?
Nothing, they are thermally stable. Except from Lithium: Li2CO3- Li2O and CO2
Which is the exception?
Li2CO3- Li2O and CO2
Group 1 nitrates decompose to form?
Nitrite and oxygen MNO2 + O2
Group 2 carbonates decompose to form?
Oxide and carbon dioxide, MO + CO2
Group 2 Nitrates decompose to form?
Oxide, nitrogen dioxide and oxygen, MO + NO2 + O2
How would you measure the thermal stability of nitrates?
How long it takes for a certain amount of oxygen to be produced. Or the brown NO2 gas.
How would you test the thermal stability of carbonates?
How long it takes for carbon dioxide to be produced. Carbon dioxide bubbled through limewater turns it cloudy.
Flame colour of Lithium
RED
Flame colour of sodium
Orange/yellow
Flame colour for potassium
Lilac
Flame colour for rubidium
Red
Flame colour for caesium
Blue
Flame colour for calcium
Brick-red
Flame colour of Strontium
Crimson
Flame colour of barium
Green
How would you carry out the flame test.
Mix a small amount of the compound being tested with hydrochloric acid. Heat a platinum or nichrome wire in the blue part of the bunsen flame. Dip the wire into the solution and hold it in the blue part of the flame. Note colour produced.
Why do we see colours in the flame test?
The energy absorbed from the flame causes the electrons to move to higher energy levels. When the electrons fall back down to lower energy levels, releasing energy in the form of light. The difference between the higher and lower energy levels determines the wavelength of the light which determines the colour of the light.
Explain the trend of reactivity down group 7,
Down the groups, the atomic radius increases, their outer electrons are further away from the nucleus, and have more shielding. This makes it harder for larger atoms to attract the electron needed to form an ion, therefore larger ions are less reactive.
Explain the trend in electronegativity down group 7.
The increasing number of inner electron shell and the increase in distance between the nucleus and the bonding electrons reduces the atoms ability to attract the bonding pair of electrons.
Explain the trend in melting and boiling points down the group.
Increase. Increase in electron shells and therefore electrons, increasing the force of London forces, which become harder to overcome.
Chlorine will displace...
Both bromide and iodide ions.
Bromine will displace...
Iodide ions
Iodide ions will displace...
Neither chloride or bromide.
What will happen if you mix the reaction mixture with an organic solvent like hexane?
The halogen present will dissolve in the organic solvent, which settles out as a distinct layer.
What colour is chlorine in water?
Virtually colourless
What colour is chlorine in hexane?
Virtually colourless
What colour is bromine in water?
yellow/orange
What colour is bromine in hexane?
Orange/red
What colour is iodine in water?
Brown
What colour is iodine in hexane?
Pink/violet
Halogens are examples of...
Oxidising agents, they themselves are reduced (gain an electron) by oxidised other substances.
Halogens react with group 1 and 2 to produce
Halide salts.
X2 + 2NaOH --> This is an example of...
NaOX +NaX +H2O.... Disproportionation.
What is bleach? And how is it made?
Sodium chlorate solution. Reacting chlorine gas with cold, dilute aqueous sodium hydroxide.
Another example of disproportionation...
Halogens reacting with hot alkalis. NaXO3 + 5NaX + 3H2O
Chlorine and water undergoes disproportionation too...
Cl2 + H2O --> HCl + HClO
What is that use of chlorate ions?
They kill bacteria, very useful in water treatment.
Why does the reducing power of the halides increase down the group?
The ions get bigger, so electrons are further away from the positive nucleus, there are extra inner electron shells, so greater effect from shielding, therefore the outer electron can be lost more easily.
KF + H2SO4-->KHSO4 + HF KCl + H2SO4-->KHSO4 + HCl
Misty fumes as HF and HCl comes into contact with moisture in the air. Fluoride and chloride ions aren't strong enough reducing agents to reduce the sulphuric acid so reaction stops.
KBr + H2SO4-->KHSO4 + Her 2HBr + H2SO4 --> Br2 + SO2 + 2H2O
Misty fumes of HBr Bromide ions are stronger reducing agents so react with H2SO4 in a redox. Produces choking fumes of surfer dioxide and orange fumes of bromine.
KI + H2SO4 --? KHSO4 + HI 2HI + H2SO4 --> I2 +SO2 + 2H2O 6HI + SO2 --> H2S +3I2 +2H20
Iodide ions reduce H2SO4. Iodide ions keeps reducing are reduces SO2 to H2S. Which is a toxic, bad egg smelling gas.
What colour will dissolved hydrogen halides turn litmus paper?
Blue as the hydrogen halides are acidic gases.
Outline a test for testing halide ions.
Add dilute nitric acid to remove any ions which might interfere with the reaction. Add silver nitrate solution, a precipitate of the silver halide is formed.
Name the colours of the potential precipitates formed.
Fluoride- np ppt Chloride- white ppt Bromide- cream ppt Iodide- yellow ppt
Describe the reaction of AgCl with ammonia solution.
Ppt dissolves in dilute ammonia solution to give a colourless solution.
Describe the reaction of AgBr with ammonia solution.
ppt remains unchanged if dilute ammonia is added, but will dissolve in concentrated ammonia.
Describe the reaction of AgI in ammonia.
ppt doesn't dissolve even in concentrated.
Outline a test to detect carbonates.
CO32- + 2H+ --> CO2 + H20 Carbonates will fizz as they give off CO2 HCO3- + H+ --> CO2 + H20 hsydrogencarbonates will also fizz as they give off CO2. The CO2 can then be tested by bubbling through limewater, if it goes cloudy CO2 is present, and a carbonate or hydrogen carbonate ion is identified.
Outline a test to test for sulfate ions.
Add HCl, followed by barium chloride solution. Ba2+ + SO42- -->BaSO4 BaSO4 is a white ppt that forms, indicating original compound contained a sulphate.
Outline a test to test for ammonium compounds.
Add sodium hydroxide to substance in test tube and gently heat, if ammonia is given off, it can be tested with a damp piece of red litmus paper, if ammonia is present, it'll dissolve in the water on the paper and turn it blue. NH4Cl + NaCl --> NH3 + H20 + NaCl
What is a use for Calcium hydroxide?
(1) is reasonably soluble in water. It is used in agriculture to neutralize acidic soils (2)An aqueous solution of calcium hydroxide is called lime water and can be used a test for carbon dioxide. The limewater turns cloudy as white calcium carbonate is produced. Ca(OH)2 (aq) + CO2 (g) CaCO3 (s) + H2O(l)
