metals, acids and titrations Flashcards
where do metals come from
ores
what is an ore
a naturally occurring rock containing enough metal compound (usually metal oxides) to economically extract the metal
reactivity series acronym
people - potassium
should - sodium
consider - calcium
making - magnesium
a - aluminium
cool - carbon
zoo - zinc
in - iron
London - lead
called - copper
sparkly - silver
giraffe - gold
which metals react with water or dilute acids
everything above copper in the reactivity series
what is oxidation
addition of oxygen to a compound and loss of electrons
what is reduction
removal of oxygen to a compound and the gain of electrons
how do metals react with water
- fizzing
- hydrogen gas produced
- potassium = lilac flame
metal + acid
= salt + hydrogen
acid + base
= salt + water (+co2 if carbonate)
what is displacement
when a more reactive metal replaces a less reactive metal
what are ionic equations
equation that shows only ions or atoms that change in a chemical reaction
- Fe + Cu^2+ = Fe^2+ + Cu
what are half-equations
an equation that describes reduction or oxidation (loss or gain of electrons)
- Fe = Fe^2+ +2e
- Cu^2+ + 2e- = Cu
what is extraction
a method removing metals from ores (reduction of oxide by carbon)
- only used for metals below carbon
what is a native
a metal found on it own, does not need to be extracted
- gold and silver occur native
what is electrolysis
a method of removing metals from ores (reduction of oxide by hydrogen)
- only used for metals above carbon
what are the 3 factors of extraction
- how easy it is to extract
- concentration of metal inside
- demand of the metal
how is salt formed
when the hydrogen in an acid is completely or partially replaced by a metal or ammonium ions
why are alkali metals never used to react with acids
alkali metals are very reactive and would react with acid too violently to be carried out safely
what is the method for making pure dry crystals
- place some acid in a beaker and warm using a water bath or Bunsen burner
- add a spatula metal to the acid and stir with a glass rod, continue until metal is in excess
- filter the mixture to remove the excess metal
- pour the filtrate into an evaporating basin and heat until point of crystallisation
- leave left over solution to dry on its own
- once crystals are formed pat dry with filter paper
what are weak acids
- they partially ionise in aqueous solutions
- have low concentration of H+ ions in solutions
what are strong acids
- they completely ionise in aqueous solutions
- have high concentration of H+ ions in solutions
what is a precipitate
an insoluble solid formed by a reaction taking place in a solution
what is an end point
the point where the acid an alkali have reacted completely without having either of them in excess. point of neutralisation
