Topic 8: Group 2 and Group 7 Flashcards
State one observation when magnesium reacts with steam
White solid forms
Mg (s) + H2O (g) –> MgO (s) + H2 (g)
what is the equation for when barium reacts with water and evidence for the formation of barium hydroxide
Ba (s) + 2H2O (l) –> Ba(OH)2 (aq) + H2 (g)
-fizzing shows formation of hydrogen gas
-litmus paper can be used to show alkaline solution
contrast these observations with those for calcium with water
-when calcium reacts with water a solid suspension is formed rather than aqueous as calcium is less soluble and less alkaline
-Calcium reacts less vigorously
what happens to hydroxides and sulfates down group 2
hydroxides are more soluble
sulfates are less soluble down group 2
what is the correct observation when barium metal is added to an excess of water
forms a colourless solution and effervesces
which compound is used to treat symptoms of indigestion
Mg(OH)2
equation for stronium with cold water
Sr (s) + 2H2O (l) –> Sr(OH)2 (aq) + H2 (g)
aqueous formed as more soluble
describe what you would see if you dropped some pieces of calcium into cold water
-vigorous reaction producing a colourless gas
-calcium would disappear to leave a white precipitate in a colourless solution
what is the least reactive element in group 2 and why
Be (Beryllium) is the least reactive element in group 2 as it has the smallest atomic radius, least shielding and the same nuclear charge. This means that there are stronger electrostatic forces of attraction
reactions with water (1)
-Mg to Ba in group 2 react with water
-As you go down group rate of reaction increases
-As you go down group 2 reactivity with water increases (Barium reacts most vigorously with water)
Mg (s) + 2H2O (l) —> Mg(OH)2 (s) + H2 (g)
what happens to reactivity down group 2
increases
group 2 reactions with water (2)
Mg –> very slow reaction with cold water
Ca –> fizzes and milky white alkaline suspension formed (solid)
Sr –> Fizzes vigorously and alkaline solution (aqueous)
Ba –> Fizzes very vigorously and strongly alkaline solution (aqueous)
magnesium reacting with steam
Magnesium reacts more rapidly with water when its steam to form a white solid and burns with a bright, white light
Mg (s) + H2O (g) –> MgO (s) + H2 (g)
why does beryllium not react with water
Beryllium doesn’t react with water as it has an insoluble surface oxide layer
reactions of Mg,Ca,Sr
reacts with oxygen to form metal oxide MgO
Ba reacts with excess oxygen to form what
Ba reacts with excess oxygen to form BaO2
group 2 metals react with chlorine to form
-all group 2 metals react with chlorine to form XCl2 e.g BaCl2
Group 2 metals (not including Be) react with water to form
-Mg – Ba reacts with water to form a metal hydroxide with hydrogen e.g Mg(OH)2 + H2
group 2 oxides reacting with water
-Group 2 oxides react with water but they do not fizz so no hydrogen gas is formed
g MgO (s) + H2O (l) –> Mg(OH)2 (s)
Metal oxide + water –> metal hydroxide
what forms when group 2 oxides e.g MgO react with water
BeO –> No reaction
MgO –> Little reaction, slightly alkaline suspension
CaO –> White, weakly alkaline suspension (pH 10)
SrO –> Colourless, alkaline solution (pH 12)
BaO –> Colourless, very alkaline solution (pH 14)
hydroxides
-Hydroxides become more soluble as you go down the group to form alkaline solutions
-Solubility increases as alkalinity increase (more OH- ions)
calcium hydroxide
Calcium hydroxide is only slightly soluble in water and forms a solution called limewater. Lime water is used to test for carbon dioxide; it turns cloudy when CO2 has bubbled through it. It turns cloudy as it forms a white precipitate known as calcium carbonate which is insoluble in water
Ca(OH)2 + CO2 –> CaCO3
soluble vs insoluble hydroxides
Ba and Sr = soluble (aq)
Mg and Be = insoluble (s)
soluble vs insoluble sulfates
Be and Mg = soluble
Ba and Sr = insoluble
barium sulfates
-Barium sulfate is used as a radiocontrast agent to help take x-ray images of the digestive system. It is a very good absorber of x-rays so therefore helps to define structures of the digestive system to aid diagnosis.
-Barium sulfate is used as it is insoluble so it is not absorbed by the body when swallowed.
uses of group 2 metals
Mg is used to extract Ti from TiCl4 as Mg is more reactive than Ti so displacement reaction occurs
Mg(OH)2 is used to treat indigestion as it neutralises acid reflux.
Ca(OH2) is used to raise the pH of acidic soil as it is alkaline so neutralises soil
CaO and CaCO3 are used to remove SO2 from flue gases as SO2 is acidic so reacts with basic compounds (alkaline)
BaSO4 used as an x-ray contrast agent in the body
Explain why iodine forms essentially covalent compounds with metals
-iodine is a large anion so has a greater electron cloud and atomic radius
-this means that there is an overlap of electron density which leads to the compounds being essentially covalent
Explain why flourine forms ionic compounds with hydrogen
-flourine is very electronegative which means covalent bond is so polarised that electrons are essentially fully transferred
true or false - group 7 elements are diatomic
true
what happens to reactivity as you go down the group 7
decreases as it becomes harder to add an electron
colours of bromine, chlorine and iodine
Chlorine = green-yellow gas
-Bromine = dark red liquid
-Iodine = dark grey solid
group 7
All four of the main halogens are reactive non-metals
-Flourine and chlorine are the most reaction elements in group 7
-the stronger the intermolecular force, the higher the boiling point
why does the boiling point of halogens increase down group 7
Halogens increase in boiling point as we go down the group as there are more electrons per molecule so stronger van der waal forces between molecules which require more energy to overcome
cl-cl bond
Cl-Cl = same electronegativity so is non-polar
Halogens = anions
Group 7 halogens colour in aqueous and vapor
Flourine (gas) = pale yellow but yellow vapour
Chlorine (gas) = pale green but green vapour
Bromine (liquid) = orange and orange vapour
Iodine (solid) = grey but purple vapour
halogens dissolve freely in hydrocarbon solvents
Halogens dissolve freely in hydrocarbon solvents such as cyclohexane and they produce the colours of their vapours e.g iodine = purple
why does flourine attract the most electrons
Flourine would attract electrons the most easily as it has the highest electronegativity and the smallest atomic radius/less shielding which means greater electrostatic force of attraction so most oxidising.
why are halogen bonds essentially covalent
Due to its large size, iodine is heavily polarised when placed next to a small cation such as Li+. This means that compounds are essentially covalent.
displacement reaction
-a more reactive halogen will displace a less reactive halide from its compound
-most displacement reactions occur in an aqueous solution
e.g Flourine displaces iodine from potassium iodide
displacement observations
Displacement observations (colour of halogen released)
-Chlorine = pale green
-Bromine = orange
-Iodine = brown
testing for halides
-halides = negative anions
-Halides are colourless ions which we can test for by adding aqueous silver nitrate solution (AgNO3)
halide precipitate colours
-Chloride = white precipitate
-Bromide = cream precipitate
-Iodide = yellow precipitate
steps of halide test
1) Add nitric acid to remove carbonate impurities
2) Add a few drops of silver nitrate solution
3) Chloride ions would form a white precipitate of silver
4) Bromide ions would form a cream precipitate of silver bromide
5) Iodide ions would form a yellow precipitate of silver iodide
distinguish between precipitates
-We can add aqueous ammonia to the precipitate of silver halide
1) Add ammonia solution to the precipitate
2) AgCl would dissolve in both a dilute and concentrated ammonia
3) AgBr would only dissolve in concentrated ammonia
4) AgI wouldn’t dissolve in dilute or concentrated ammonia