unit two: inorganic chemistry Flashcards
what are the group one metals called
alkali metals
what are lithium, sodium and potassium stored in and why?
oil to prevent them from reacting with oxygen and water.
properties of alkali metals
good conductors of electricity and heat
soft and can easily be cut with a knife
low melting and boiling points compared with more typical metals such as iron and copper
low densities
properties of lithum, sodium and potassium
shiny surface when freshly cut with a knife, but the surface quickly becomes dull as the metal reacts with oxygen in the air.
what does lithium, sodium and potassium form when they burn in air
white solid oxides
what is the equation for when lithium, sodium and potassium burns in air
4M +O2 –> 2M2O
where M = lithium, sodium or potassium
what colour flame does lithium burn with
red
what colour flame does sodium burn with
yellow
what colour flame does potassium burn with
lilac
do lithium sodium and potassium react with water
yes vigorously
what do lithium sodium and potassium give when they react with water
an alkaline solution of the metal hydroxide as well as hydrogen gas
observations when lithium reacts with warer
moves around the surface of the water
hissing sound
bubbles of gas
gets smaller and smaller, eventually disappears
observations when sodium reacts with water
moves around the surface of the water hissing sound bubbles of gas melts into a shiny ball gets smaller and smaller, eventually disappears
observations when potassium reacts with water
moves around the surface of the water hissing sound bubbles of gas melts into a shiny ball burns with a lilac-coloured flame gets smaller and smaller, eventually disappears
order of reactivity of lithium, sodium and potassium
potassium - sodium - lithium (more reactive with increasing atomic number)
what happens involving reactivity as you move down group 1
reactivity of the elements increases
why is potassium more reactive than sodium and lithium
it requires less energy to overcome the electrostatic forces of attraction between the negatively charged electron and the positively charged nucleus.
physical state and colour of chlorine at room temperature
pale green gas
physical state and colour of bromine at room temperature
red-brown liquid
physical state and colour of iodine at room temperature
black solid
what happens when chlorine reacts with iron
brown smoke is formed and a brown solid is left behind
what happens when bromine reacts with water
bromine smoke and a brown solid are formed
what happens when iodine reacts with water
brown smoke and a brown solid are formed
what is a halide
a compound of a halogen and one other element
whats in a metal halide
a compounf of a halogen and a metal
what happens when chlorine reacts with hydrogen
explosion when exposed to UV radiation
what happens when bromine reacts with hydrogen
the vapour formed will react when heated
what happens when iodine reacts with hydrogen
the vapour will react when heated, but the reaction does not go to completion
when is a metal halide formed
e.g. when a halogen is reacted with iron
when is a hydrogen halide formed
e.g. when a halogen is reacted with hydrogen
general rule for displacement reactions
a halogen will displace a less reactive halogen for an aqeous solution of its halide.
what colour is aqueous chlorine
very pale green, usually diluted to colourless
what colour is aqueous bromine
orange but will turn yellow when diluted.
what colour is aqueous iodine
brown
in displacement reactions, the halogen molecule is often being reduced because
it is gaining electrons
in displacement reactions, the halide ions are being oxidised because
they are losing electrons
when both reduction (of a halogen) and oxidisation (of a halide) is happening the reaction is called a
redox reaction
why does reactivity decrease down the group of halogens
the increasing size of the atom means it will be harder for the atom to quickly gain an electron
what percentage of air is nitrogen
78%
what percentage of air is oxygen
21%
what percentage of air is argon
0.9%
what percentage of air is carbon dioxide
0.04%
how would you measure the oxygen content of air using copper
repeatedly pass 100cm cubed of air back and forwards over a silicia tube packed with copper, by heating it with a blue bunsen flame. the copper will react with the oxygen to form black copper oxide.
what would the results be after measuring the oxygen content of air using copper
the final volume of air in the syringe will be approximately 79cm cubed, showing that 21cm cubed has reacted. therefore 21% of the air was oxygen.
how would you measure the oxygen content of air using iron
place wet iron fillings at the end of a burette and place in a water trough. the iron will react with oxygen, and over several days the volume of air in the buretter will have decreased.
how would you measure the oxygen content of air using phosphorus
put a piece of white phosphorus inside a tube inside a beaker filled with water. the water levels inside the tube and the beaker should be equal. touch the phosphorus with a hot metal rod and burn it. when it stops burning the water level inside the tube will have increased due to the oxygen being used up.
observations of magnesium when it burns in oxygen
bright white flame to form a white powder
observations of carbon when it burns in oxygen
yellow-orange flame to form a colourless gas.
observations of sulfur when it burns in oxygen
blue flame to form a colourless gas
describe magnesium oxide
basic oxide, slightly soluble in water and a pH of about 10. reacts with water to form magnesium hydroxide
describe carbon and sulfur dioxide
acidic oxides, dissolve in water to form acidic solutions.
the reaction between any metal carbonate and an acid will produce
carbon dioxide
when metal carbonates are heated what is produced
carbon dioxide
observations of the thermal decompisition of copper carbonate
green copper carbonate and black copper oxide are heated, and if carbon dioxide is produced the limewater attacahed to it will turn milky
observations of the thermal decompisition of magnesium carbonate
no change, stays white
observations of the thermal decomposition of calcium carbonate
no change stays white
observations of the thermal decomposition of zinc carbonate
white to yellow when hot and white again when cold
observations of the thermal decomposition of sodium carbonate
no observable change, stays white
how does production of carbon dioxide enhance the greenhouse effect
more heat is re-emitted by the atmosphere and less heat escapes into space .
effects of global warming
polar ice caps melt, sea levels rise, more extreme weather
list the reactivity series
potassium sodium lithium calcium magneisum aluminium zinc iron tin lead copper silver gold platinum
reducing metal oxides
a metal oxide is a compound of metal and oxygen. when the oxygen is removed, the oxide is reduced. it can be reduced by heating it with a metal higher up in the reactivity series.
(reactivity series) the substance that carries out the reduction is called the
reducing agent
why is hydrogen in the reactivity series
although not a metal, it can be displaced from an aquous solution like a metal, only this time, the solution is an acid.
where is carbon in the reactivity series
it can combine with oxygen to form carbon dioxide, between aluminium and zinc.
what is rusting
an oxidation reduction
the iron reacts with water and oxugen to form rust or?
hydrated iron (III) oxide
what is coating
stopping oxygen or water reaching the surface of the metal
examples of coating
oiling (bicycle chains)
greasing (nuts and bolts)
painting (car body panels)
what is alloying
stainless steel is an iron alloy that does not rust. used for sinks etc
what is sacrificial protection
attaching a more reactive metal such as magnesium slows down rusting.
what is plating
iron objects can be covered with a thin layer of metal.
examples of plating
food cans plated with tin
buckets plated with zinc (also gives sacrifical protection.)
give the only two elements that occur as elements in their ores
silver and gold (most unreactive)
how can sulfides be easily converted into oxides
by roasting (heating in air)
how to extract metal from the first 6 metals in the reactivity series
electrolysis of the molten chloride or molten oxide
how to extract metal from the middle 3 metals in the reactivity series (zinc, iron, copper)
heat with a reducing agent such as carbon or carbon monoxide
how to extract metal from the last 2 metals in the reactivity series (silver, gold)
you don’t, they occur naturally as elements
uses of aluminium
aeroplane bodies
saucepans
food cans
window frames
uses of iron
car bodies
iron nails
ships and bridges
why is aluminium and iron rarely used by themselves
they aren’t very strong so aluminium alloys are usually used instead.
how can aluminium be stengthened
by adding other elements such as silicon, copper or magnesium.
what is pure iron also called
wrought iron
describe the structure of ions in a pure metal
the ions in a pure metal are the same size and fit neatly in layers able to slide over each other. a relatively small force is required to slide these layers over each other.
describe the structure of ions in an alloy
the ions are different sizes so there are no regular layers, meaning it requires a greater force to slide these layers of ions over each other.
which end of the pH scale is acidic
0-6 (decreasingly so)
which end of the pH scale is alkaline
8-14 (increasingly so)
which number on the pH scale is neutral
7
give an example of a neutral substance
pure water
what colour does litmus paper turn in a solution where the pH is 5 or less
red
what colour does litmus paper turn in a solution where the pH is 8 or more
blue
what colour does litmus paper turn in a solution between 5 and 8
a shade of purple (between red and blue)
what colour is methyl orange in a solution where the pH is 3 or less
red
what colour is methyl orange in a solution where the pH is 5 or more
yellow
what colour is methyl orange in a solution where the pH is between 3 and 5
orange (between red and yellow)
what colour is phenolphthalein in a solution where the pH is 8 or less
colourless
what colour is phenolphthalein in a solution where the pH is 10 or more
red
what is the simplest way to find an unknown pH
use indicator paper
what is pH paper
paper soaked in universal indicator and then dried.
acid definition
a substance that dissolves in water to produce hydrogen ions (H+)
what is the formula for hydrochloric acid
HCl
what is the formula for nitric acid
HNO3
what is the formula for sulfuric acid
H2SO4
base definition
substances that neutralize acids by combining with the hydrogen ions in them/
alkali definition
bases that dissolve in water to form hydroxide ions.
examples of alkalis
sodium hydroxide
potassium hydroxide
salt definition
the compound formed when the hydrogen ions in an acid are replaced by either a metal ion or by an ammonium ion
what is oxidation
when an atom or a molecule loses an electron in a reaction
what is reduction
when an atom or a molecule gains an electron in a reaction
what does halogen mean
salt producing
what are halogens
non-metallic elements with diatomic molecules
trend in melting and boiling points in group 7
they increase down the group because the relative molecular mass increases
what structure do halogens have
covalent molecular
are halogens good conductors of heat and electricity
no they are non metals
which element would you necer find in a school lab due to its dangerous reactivity
fluorine
when halogens react with hydrogen what do they form
hydrogen halide
describe hydogen halides
they are all acidic, poisonous gases that are covalently bonded. theyre very soluble inwater and react with it to produce solutions of acids.
when halogens react with alkali metals what do they form
salts
trend of reactivity in the halogens
it decreases as you go down the group
if something is more reactive,
it has more tendency to react to form a compound and displace the other element
what is a spectator ion
e.g. the metal ion that doesn’t do anything in a displacement reaction
does an ionic equation include spectator ions
no
recution is
loss of oxygen
oxidation is
losing electrons (sometimes through combining with oxygen which takes the electrons)
why does reduction and oxidation happen at the same time
beacause if something loses oxygen, something else must gain it
what is an oxidising agent
something that oxidises something else by taking oxygen away from it
what is a reducing agent
something that reduces something else by giving electrons to it
when are electrons attracted more strongly to the nucleus
when theyre closer
as you move down the group what changes in the states if matter
it goes from gases to liquid to solid
what do halogens have that get darker down the group
colourd poisonous vapours
when halogens react with metals what forms
ionic salt
when halogens react with non metals what forms
non-metals
properties of astatine
very dark grey or black solid at room temp and high melting point diatomic less reactive than iodine displaced by iodine
how much nitrogen is in the air
78%
how much oxygen is in the air
21%
how much argon is in the air
0.9%
how much carbon dioxide is in the air
0.04%
how would you find the percentage of oxygen in the air
have two gas cylinders with a silica tube packed with copper filings between them. fill them to 100cm cubed collectively, then heat teh silica tube strongly. as the copper turns black as copper oxide forms, the oxygen is consumed, so there will be no change in volume anymore pushing the plungers back and forth. let cool and it will show that the volume of oxygen will have decreased.. then work out the volume of oxyegn recated, and the percentage of oxygen in the air.
how would you determine how much oxugen there is in the ari using the rusting of iron
use a connecting ub between a gas syringe and conical flask containing wet iron filings. record the inital reading on the gas syringe, then leave it for about a week until the reading stops changing. record the final reading and calculate the percentage of oxxygen used.
what could go wrong when using a practical to calculate th percentage of oxygen in the air
the experiment was not set up for long enough. the iron has not had enough chance to react with all the oxygen in the apparatus.
not enough iron was added at the beginning. it must be in excess, so there is enough iron to react with all the oxygen present.
how would you find the percentage of oxygen in air by using phosphorus
put a piece of phosphorus in an evaporating basin floating in a water trough surrounded by a bell jar. mark the inital level of water. remove the bung and touch the phosphorus witha hot metaal wire to ignite it. replace the bunga nd wait untl the white smoke that forms (phosphorus oxide) clears. when the water level stops rising, mark it. then calcualte the percentage using how much oxygen was used up.
what does magnesium burn in oxygen to give
a white, powdery ash of magnesium oxide
what does sulfur burn in oxygen to give
poisonous, colourless suflur dioxide gas of sulfur dioxide
how do you test for hydrogen
squeaky pop
properties of metal oxides
ionic compounds containg O 2-
usually basic oxides, so they react with acids to form salts
usually insoluble in water. those that are soluble react with warer to form alkaline solutions containing hydroxide ions
properties of non metal oxides
covalent compounds
acidic oxides
non metal oxides often soluble in water and react with it to form aidic solutions containing H + ions
how can carbon dioxide be obtained
through the reaction of hydrochloric acid and calcium carbonate or when metal carnonates are heated strongly
when is carbon dioxide produced
when fossil fuels burn
when does the greenhouse effect occur
when high energy UV and visible light from the sum pass througn the atmoshpher and warm up the surface of the earth. the infrared radiation radiated by the earth is absorbed by CO2 molecules in the atmoshoere. they then give out this energy in all directions, heating the atmosphere.
what does the pH scale tell you
how acidic or alkaline a solution is
part of the PH scale that is strongly acidic
0-3
universal indicator paper
a mixture of indicators which change colour in a gradual way. can be a solution or paper. ranges through a variety of colours form pH 1 to pH 14 but isnt very accurate
what can be used as an indicator
anything that has different colours depending on the pH
what colour is litmus in acid and alkaline solutions
red in acidic solutions an blued in alkaline, and purple in neutral
what colour is universal indicator in neutral solutions
green
what do all acids contain
hyrdogen
what do you measure when you measure pH
the H+ ions
what happens when acids are placed in water
they dissociate (break apart) to form hydrogen ions
define acids
substances that act as a source of hydrogen ions in solution.
what is a base
a substance that neutralises an acid by combining it with the hydrogen ions in them.
what happens when a base dissolves inwater to form solutions
it contins hydroxide ions and are alkalis.
define alkalis
a surce of hydroxide ions (OH - ions) in solution
what do acids react with in a neutralisation reaction
bases or alkalis
why will all neutralisation reactions have the same equation
they all involve the OH - ions from the alkali reacting with the H + ions from the acid ro form water
purpose of titrations
to find out how much of the acid/alkali reacts with a certian volume of the alkali/acid.
how do you carry out a titration
(rough titration first or now)
measure 25cm cubed of HCl using a pipette. transfer to conical flask. fill the burette with sodium hydroxide solution. take initial reading and record to 2 decimal places. add a few drops of phenolphthalein indicator. add sodium hydroxide until the indicator changes colour and then take the final reading on the burette when its a permanent pale pink colour
how do you calculate the volume of alkali added in a titration
subtract the inital reading on the burette from the final reading on the burette
why do you not use universal indicator in a titration
because it has a range of colours and changes gradually between them, so we could not see a clear endpoint.
when you replace the hydrogen in an acid with a metal what do you form
a salt
what are the name of salts formed from HCl
chlorides
what are the name of salts formed from HNO 3
nitrates
what are the name of salts formed from H2SO4
sulfates
what are the name of salts formed from CH3COOH
ethanoates
what are the name of salts formed from K3PO4
phosphates
the higher a metal is in the reactivity series…
the more vigorous the reaction.
(above hydrogen in the reactivity series) metal + acid =
salt + hydrogen
metals below hydrogen in the series…
dont react with dilute acids
magnesium with sulfuric/hydrochloric acid
rapid fizzing
colourless gas which pops with a lighted splint
reaction mixture becomes warmer
produces magnesium sulfate
difference in reaction in xinc and acids
the only difference is its slower because zinc is lower down on the reactivity series
metal oxide + acid =
salt + water
metal hydroxide + acid =
salt + water
neutralisaton reaction
OH- + H+ –> H2O
carbonate + acid =
salt + carbon dioxide + water
carbonataes react with cold dilute acids to
produce carbon dioxide gas.
how do you recognise that green copper carboante reacts with common dilute acids
carbon dioxide is given off and it turns limewater milky.
all sodium potassium and ammonium compounds are
soluble
all nitrates are
soluble
most common chlorides are
soluble except lead (II) chloride and silver chloride
most common sulfates are
soluble except lead (II) sulfate, barium sulfate, silver sulfate and calcium sulfate
most common carbonates are
insoluble except sodium, potassium and ammonium carbonates.
most metal hydreoxides are
insoluble except sodium, potassium and ammonium hydroxides. calcium hydroxide is lightly soluble in water.
how do you make soluble salts (except sodium, potassium, ammonium)
acid + metal (only for magnesium to iron)
acid + metal oxide or hydroxide
acid + carbonate
making copper sulfate crystals
heat 50cm cubed of dilute sulfuric acid into a beaker and heat it on a tripod and gauze using a bunsen burner.
add a spatula full of black copper oxide and continue heating. stir well to make sure no more will react. (excess copper oxide, when there is some left, we know all the acid has been neutralised)
filter off excess copper oxide and transfer the filtrate to a evaporating basin. heat to boil off some water and to concentrate the solution. keep heating until saturated (dip a glass tod and if crystals form its saturated)
allow to cool at room temp for larger crystals.
filter
leave them to dry in a warm place
why dont you evaporate the copper sulfate crystals
you would get anhydrous copper sulfate. this is water of crystallisation.
when is a salt said to be hydrated
when it contains water of crystallisation,
what is water of crystallisation
when water from the solution becomes chemically bound up with a salt
making magnesuymn sulfate crystals
add magnesium to asulfuric acid. wait until fizzing stops. heat and allow to crystallise.
how do you know whether to heat the mixture
carbonates and magnesium can react in the cold, everythin else needs heat
why cant you make sodium, potassium, ammonium like this
theyre soluble in water
making sodium sulfate crystals
25 cm cubed of sodium hydroxide is transferred to a conical flask using a pipette and a few drops of methyl orange.
dilute sulfuric acid is run in from the burette until the indicator just turns from yellow to orange.
colume of acid needed is noted, and the same volumes of cid and alkali are mixed in a clean flask with NO indicator
this is heataed to evaporate off some of the water until a saturated solution is formed. it is then left to for cool for crystals.
filtration
left to dry in warm place
making sodium chloride crystals
do a titration with dilute HCl not dilute sulfuric acid, and then use the same procedure as sodium sulfate
how do you make insoluble salts
mix two soluble salts to form an insoluble salt and a solution of a soluble one. this is a PRECIPITATION REACTION
what is a precipitate
a solid formed by a chemical reaction involving liquids and gases
what do we mix to form an insoluble salt
the nitrate of the metal part and the sodium/potassium of the non-metal part
if the salt is soluble but not a sodium, potassium, ammonium salt how do you make it
react an acid with an excess of a solid metal (if suitably reactive) metal poxide, hydroxide or carbonatae
if the salt is soluble and a sodium, potassium, ammonium salt how do tou make it
use a titration method. react an acid with a solution of sodium, potassium hydroxide or carbonate (or use ammonia solution)
if the salt is insoluble how do you make it
use precipitation method. mix two solutions, one contianing the correct pos ion and one the correct neg ion
an acid is
a proton (hydrogen ion) doner
a base is
a proton (hydrogen ion) acceptor
test for oxygen gas
a glowing splint is put into the tube containing the gas. oxygen will erlight it.
test for CO2
the carbon dioxide is bubbled through limewater. carbon dioxide turns limewater milky.
whats limewater
a calcium hydroxide solution. CO2 reacts with it to form a white precipitate of calcium carbonate
test for chlorine gas
damp litmus paper or universal indicator paper put in/held over mouth of test tube. chlorine will bleach the papers
test for ammonia
turns damp universla indicator paper or red litmus paper blue
water turns anhydrous copper sulfate
blue
physical test for purity of water
does it freeze at 0 or boil at 100
what is a flame test used for
to show the presence of cations
describe the preciptation method for making salts
combine two solutions containing the necessary positive and negative ions
describe the excess base method for making salts
react an acid with an excess of a metal (if suitably reactive) , metal oxide, metal hydroxide or metal carbonate and then fliter
does reactivity increase or decrease as you go down the alkali metals
increase
what makes an element reactive
the ability of it to lose electrons. if it loses an electron easily, it is more reactive
what factor contributes to an element’s reactivity
how strongly the electron is attracted to the nucleus of the atom.
how does the nucelus attract electrons
the nucleus is positive due to the charge of protons, and so it can attract negative electrons
why does reactitivty increase down the alkali metals
the electrons are further away from the centre/nucleus of the atom so the attaction between the oppositely charged electron and nucleus is weaker, allowing it to be lost more easily.
why does reactivity decrease down the halogens
because the electrons are further away from the centre/nucleus of the atom so the attraction between the oppositely charged electron and nucleus is weaker, meaning it cannot attract or gain electrons as easily.
why is carbon included in the reactivity series
its important in extracting several metals from metal oxides.
what happens if you heat carbon with a less reactive metal
it can be a cheap way of removing oxygen from the oxide to leave the metal.
why does an oxidising agent always get reduced
it oxidises something else by giving away oxygen
why can’t you just evaporate off all water to gain copper sulfate crystals
you would get white anhydrous copper sulfate not blue copper sulfate crystals
why can’t you use the method for making soluble salts for sodium potassium and ammonium
they are soluble in water so they would not react with the acid but issolve.
what method can you use to make sodium, potassium and ammonium salts
use a titration to neutralise them
how do you make sodium potassium and ammonium salts
titration
(acid run from beaker until indicator changes)
volume of acid needed is noted, and same volumes of acid and alkali are mixed together in a beaker without indicator
solution is heated to evaporate off some of it and until a saturated solution forms. it is left to cool for crystals.
the crystals are separated by filtration
then are dried by patting them dry with a paper towel or by leaving them in a warm place.
what is a precipitation reaction
where two soluble salts are mixed to form an insoluble salt and a solution of a soluble one. it forms a precipitate
what is a precipitate
a solid that is formed by a chemical reaction involving liquids or gases.
how does a precipitation reaction work
one solution has ions that are attracted to eachother but not very strongly, and when mixed with another solution, are far more attracted to one of the ions in it, and clump together tightly to form a solid or precipitate.
how do yo u know what to mix to create an insolubel salt
the nitrate of the metal part of the insoluble salt, and the sodium/potassium part of the non-metal.
the salt isn’t soluble so…
use a precipitation reaction
the salt is soluble but it is not a sodium/potassium/ammonium salt so…
react an acid with an excess of a solid metal (if suitably reactive), metal oxide, hydroxide or carbonate.
the salt is soluble and is a sodium/potassium/ammonium salt so…
use a titration method. react an acid with a solution of sodium or potassium hydroxide or carbonate.
what is an ore
a sample of rock that contains enough of a mineral for it to be worthwhile to extract the metal
where are most ores extracted from
the earths crust
which metals are found native and what does this mean
they exist naturally as the uncombined element, like gold (or silver or copper)
most metals are found in the earths crust combined with other elements. what are the indiviual compounds called
minerals
what is roasting
the proccess of converting into an oxide by heating in air
how do you obtain the metal from the oxide and what is this called
remove the oxygen, and reduction
what is the main reducing agent for metals below carbon in the reactivity series
carbon monoxide
why can’t metals higher than zinc be reduced by carbon at reasonable temperatures
the metals aremove reactive than carbon and therefore carbonc annot take the oxygen away from themetal oxide.
what are metals above zinc usually produced by
electrolysis
what molten salt does aluminium oxide dissolve in
cryolite
why is aluminium oxide dissolved in cryolite
it makes the process more economical as opposed to over 2000 degrees, the process can now be carried out at 1000 degrees
where does the cathode typically go in extraction of metals via electrolysis
as the lining
where does the anode typically go in extraction of metals via electrolysis
as the electrodes inserted at the top
why is electrolysis expensive
it requires a lot of energy
what is an alloy
a mixture of a metal ususally with other metals or carbon.
why are alloys harder than the metals from which they are originally made
the different metals/elements have slightly different sized atoms. this breaks up the regular lattice arrangement and makes it more difficult for the layers of ions to slide over eachother.
uses of aluminium (alloys)
planes, electricity cables, pots and pans
what do metals’ uses depend on
(low) density and strength
why does aluminium resist corrosion
because it has a thin but strong layer of aluminium oxide on the surface, which prevents anything reaching the surface and reacting with it.
what is mild steel
the name given to an alloy or iron contianing up to about 25% carbon
characteristics of mild steel
strong material that can be easily hammered into various shapes (malleable) and drawn into wires (ductile).
what can mild steel be used for
nails, car bodies, ship building, girders and bridges
disadvantage of mild steel
it rusts when exposed to oxygen and water
is three times denser than aluminium
advantage of car bodies being made of aluminium
lighter, so less fuel is needed.
what is high carbon steel
contains 0.6-1.2% carbon, and a little manganese
characteristics of high carbon steel
harder and more resistant to wear than mild steel but more brittle. (not as malleable and ductile).
what is high carbon steel used for
cutting tools like knives
what is stainless steel
an alloy of iron with chromium and often nickel.
characteristics of stainless steel
the chromium forms a strong oxide layer like aluminium and this oxide layer protects the iron as well, so it is very resistant to corrosion.
what is stainless steel used for
kitchen sinks, saucepans, knives and forks, gardening tools, brewing, dariy and chemical industries
which type of steel is most expensive
stainless steel
properties of electrical wires made of copper and alloys
very good conductor of electricity and ductile
properties of pots and pans made of copper and alloys
very good conductor of heat, very unreactive and malleable
properties of water pipes made of copper and alloys
unreactive, does not react with hot or cold water and malleable
surfaces in hospitals
antimicrobial properties and malleable
what is mixed with iron when it is being extracted
coke
limestone
what is the outside of a blast furnace made of
steel lined heat resistant rock
