chemistry Flashcards
examples of metals found as pure metals in nature+ name of state
silver and gold, free state
how metals can be obtained from ores
extraction
how metals can be extracted from their ores
heating the metal ore alone
heating the metal ore with carbon(carbon reduction)
electrolysis of the molten ore
the relationship between the difficulty of extracting the metal and the time of discovery
the earlier the easier
factors affecting the availability of a metal
the abundance of the metal in the earth’s crust
ease and cost of mining the ore
ease and cost of extracting the metal from its core
how to conserve metals
reuse, reduce, recycle :/
What is reactivity
The readiness of it to react with other substances
What is the metal reactivity series?
A series of common metals arranged in decreasing order of reactivity
What is a chemical equation?
shows the physical states and relative numbers of particles of the reactants and products in a chemical reaction
What is displacement in a reaction
A metal higher in the reactivity series will displace any metal lower in the solution of a compound
Why does displacement happen
A more reactive metal loses electrons more readily
What is an ionic equation?
Equation that includes kind formed or changed during the reaction
What depends on the method used to extract a metal from ores
The position of it in the reactivity series
What is the relationship between the position of the metal in the reactivity series and the difficulty of extracting it from its ore
The lower the easier
Bauxite
Aluminum
Copper pyrite
Copper
Haematite
Iron
Galena
Lead
Cinnabar
Mercury
the factors of the reactivities of metals
the lowest temperature at which the reaction starts
the rate of reaction
the amount of heat given out during the reaction
the metal reactivity series
k na ca mg al zn fe pb cu hg ag au
what happens if metals in the reactivity series are in contact with water or steam
k na ca react with water, mg al zn reacts with steam, the rest are unreactive
which metals require gentle heating for a reaction to occur
k,na
which metals require strong heating for a reaction to occur
ca,mg,al,zn,fe,pb
which metals require v. strong heating for a reaction to occur
cu,hg
which metals have no observable change in very strong heating
ag,pt,au
which metals can burn
k,na,ca,mg,al,zn,fe
which metals do not burn
pb,cu,hg
which metals have no reaction
ag,pt,au
potassium heating observations
burns vigorously, lilac flame, produces white powder
sodium heating observations
burns vigorously,golden yellow flame, produces white powder
ca heating observations
burns vigorously, brick red flame, produces white powder
Mg heating observations
burns with bright white flame, produces white powder
Al heating observations
burns to give out much heat, forms white powder
zinc heating observations
burns to give heat powder is formed, yellow when hot, white when cold
Fe heating observations
burns with yellow sparks produces black solid
pb heating observations
melts when heated, powder forms on the surface, orange when hot, yellow when cold
Copper heating observations
surface becomes black after heating
mercury heating observations
has a red powder form on the surface
ag,pt,au heating observations
no observable change
k,na,ca metals react with cold water to produce
metal hydroxide and hydrogen
mg,al,zn,fe react with steam to produce
metal oxide and hydrogen
metals from pb
dont do anything:/ no reaction
products of k,na,ca metals with cold water
metal hydroxide and hydrogen
products of mg,al,zn,fe with steam
produce metal oxide and hydrogen
metals from pb
dont do anything:/
metals k,na with acid
explosive reaction
metal+hydrochloric acid=
metal chloride+hydrogen
metal+dilute sulphuric acid=
metal sulphate+hydrogen
ca,mg,al,zn,fe react with dilute acid
more slowly down the series
pb with dilute acid
very slow reaction
metals below cu with dilute acid
no reaction
