Reactivety Series

Question 1

How do metals occur naturally ?

Answer 1

Found combined with other elements eg oxygen or sulphur

Question 2

What do you take into account when extracting a metal?

Answer 2

Ore contains enough of metal compound to make it worth extracting also taking into account Abundance, demand and ease of extraction

Question 3

How do you extract metals below carbon in the reactivity series?

Answer 3

By heating metal oxide with carbon eg

Carbon + lead oxide = carbon dioxide +lead

Question 4

How do you extract copper?

Answer 4

Not visable with naked eye After heating with carbon remove copper oxide by reacting with hydrogen sulphate

Question 5

What’s pattern for reaction of metals with acids?

Answer 5

Same as for the reaction between the metals and water but reaction is more vigorous

Question 6

whats metals+acids=

Answer 6

salt +hydrogen

Question 7

whats metal+dilute sulphuric acid=

Answer 7

metal sulphate +hydrogen

Question 8

whats metal+dilute hydrochloric acid=

Answer 8

metal chloride +hydrogen

Question 9

what do metals below hydrogen react with?

Answer 9

metals such as copper silver and gold don’t react with simple dilute acids such as sulphuric or hydrochloric acid

Question 10

what happens when potassium, sodium, lithium and calcium react with acids?

Answer 10

they are too reactive to add safety to acids the reaction is too violent calcium can be used if the acid is very dilute

Question 11

what happens when magnesium reacts with cold dilute acids?

Answer 11

reacts vigorously mixture become hot

Question 12

oxidation

Answer 12

gain charge loss of electrons

Question 13

reduction

Answer 13

lose charge gain electrons

Question 14

how do you know whether it’s oxidisation or reduction?

Answer 14

write ionic equations to see change in charge to show what is changing in equation leaving out anything that stays the same on both sides (spectator ions) then add in the charges and if gain =oxidisation if lose=reduction

Question 15

reducing agent

Answer 15

element/compound that is taking/gaining the oxygen

Question 16

oxidising agent

Answer 16

thing that is giving reducing agent the oxygen

Question 17

what are metals usually found as?

Answer 17

usually found combined with other elements

Question 18

how can you find out what causes rusting ?

Answer 18

5 test tubes with different conditions

• salty water
• normal air
• boiled water with oil at top to removes gases from water
• normal water and air
• air without water vapour (calcium chloride)

Question 19

how can you prevent rusting?

Answer 19

putting more reactive metals over iron so they corrode not iron e.g. zinc, magnesium and nail polish

Question 20

what metal rusts?

Answer 20

iron

Question 21

how can you prove that oxygen is needed for rusting?

Answer 21

glass tube lined with damp iron fillings put in trough of water as gas in air is used volume of air in tube will decrease replaced by water from trough rising up tube the %the water rises will be %of gas used

Question 22

how is iron extracted from iron ore?

Answer 22

charge (limestone (calcium carbonate), iron ore (iron oxide) and coke (heated coal) is put into a blast furnace waste gases (co2)come out the top, hot air is blown in and molten slag and molten iron come out the bottom

Question 23

equations of turning iron ore into iron

Answer 23

C+O2=Co2
C+Co2=2Co
Fe2O3+3Co=2Fe+3Co2
CaCo3=CaO+Co2
CaO+SiO2=CaSiO3

Question 24

whats aluminium ore?

Answer 24

bauxite mainly Al2O3

Question 25

how do you extract aluminium ?

Answer 25

using electrolysis- splits up compounds using electricity purified aluminium ore dissolved in molten cryolite put in a steel case with graphite anode(+) and cathode(-) negative ions attracted to anode and positive ions attracted to cathode cathode= aluminum 3+ +3 electrons- balances out no charge anode = o2- -4 electrons - charge gone up to 02+ as lost electrons lots of energy used in process therefore expensive

Question 26

how do extract metal above carbon in reactivity series ?

Answer 26

electrolysis

Question 27

how do extract metal below carbon in reactivity series ?

Answer 27

reduction with carbon or co

Question 28

disadvantages and advantage of electrolysis

Answer 28

very expensive and a lot of energy but pure metal is produced

Question 29

disadvantages and advantage of reduction

Answer 29

con not pure metal may contain carbon but cheap

Question 30

how do you know to extract a metal?

Answer 30

abundance of ore percentage of metal in ore cost of extraction demand of metal

Question 31

what is an ore?

Answer 31

rock containing metal in high enough concentration to make it economically viable to extract some metals are found native e.g. gold

Question 32

How can metals be tested for reactivity?

Answer 32

Using water eg group 1 reactivity increase down group calcium group 2 reacts rapidly in cold water whereas magnesium reacts slowly in cold water but faster in steam

Question 33

How can reactivity of less reactive metals be determined?

Answer 33

Reacting with dilute acids

Question 34

What is the reactivity series? Most reactive first

Answer 34

``` Potassium Sodium Lithium Calcium Magnesium Aluminium Carbon Zinc Iron Hydrogen Copper Silver Gold ```

Question 35

Reactions of cu fe mg and Zn with hydrochloric acid

Answer 35

Cu =no reaction Fe =lots of little bubbles fizzed hydrogen produced Mg=fizzes cloudy, become hot big pop of hydrogen Zinc=some bubbles and fizzed popped Fe+2HCl=FeCl2+H2

Question 36

oder of reactivity in iron, copper, magnesium, zinc , lithium, potassium,francium rubidium, caesium, sodium,

Answer 36

``` francium most reactive caesium rubidium potassium sodium lithium calcium magnesium zinc iron ```

Question 37

whats the displacement rule

Answer 37

more reactive metal will displace a less reactive metal from it's solution

Question 38

whats a redox reaction

Answer 38

a more reactive metal can displace a less reactive metal from it's oxide, this is classified as a redox reaction

Question 39

whats reduced and oxidised in a redox reaction

Answer 39

the more reactive metal gets oxidised as it takes the oxygen away from the less reactive metal which is reduced e.g. mg+CuO=Cu+MgO

Question 40

whats the structure of a pure metal?

Answer 40

regular lattice of positively charged metal ions attached together by sea of delocalised electrons which come from the outer shell of the metal atoms are malleable and ductile because layers of ions slide over each other without breaking attraction

Question 41

whats the structure of an alloy?

Answer 41

metal ions are different sizes disrupts the lattice and prevents layers of ions from sliding over each other makes alloy stronger and harder

Question 42

name of alloys and elements made up of

Answer 42

brass-zinc and copper bronze-copper and tin duralumin- aluminum and magnesium

Question 43

whats a sacrificial method?

Answer 43

adding more reactive metals to stop iron rusting

Question 44

whats barrier methods ?

Answer 44

protect iron from atmosphere which makes iron rust

Question 45

whats galvanising it?

Answer 45

coating it with a layer of metal e.g. zinc

Question 46

properties of aluminium

Answer 46

ductile, strong, light weight, resistant to oxidisation and conductor, used in cars, pans, transportation-planes and trains , electrical lines and packaging

Question 47

properties of iron

Answer 47

ductile, malleable , strong, heavy, used in cargo ships, washing machines, cars, nails, pans