Chemical changes Flashcards
Metal oxides
What is oxidation and reduction?
Oxidation - when a substance gains oxygen
Reduction - when a substance loses oxygen
Metal oxides
What is the formula for metal oxides?
metal + oxygen -> metal oxide
The reactivity series
What is the reactivity series of metals? What are the trends in reactivities of metals in reactions with acid/water?
The series shows the metals in order of their reactivity.
Metals above H2 in reactivity series react with acid to produce H2. The more reactive the metal is, the quicker and more violent the reaction with acid occurs.
Metals below H2 dont react with acids.
Not all metals above H2 react with water - mostly group 1 and 2 metals. Aluminium is the borderline case
The reactivity series
What is a displacement reaction?
A reaction where a more reactive metal takes the place of a less reactive metal from a compound.
Extraction of metals and reduction
Explain how unreactive metals are found and extracted
In their natural state
Extraction of metals and reduction
Explain how metals less reactive than carbon be extracted
Reduction with carbon (displacement)
Extraction of metals and reduction
Explain how metals more reactive than carbon be extracted
electrolysis
Oxidation and reduction in terms of electrons
Explain what oxidation and reduction is in terms of electrons
Oxidation - loss of electron
Reduction - gain of electron
Reaction of acids with metals
What is the general equation for reactions between metals and acids? What type of reaction is this?
Metal + acid -> salt + hydrogen
Redox reaction, also a displacement reaction
Neutralisation of acids and salt production
What is the general equation for a neutralisation reaction?
acid + base/alkali -> salt + water
Neutralisation of acids and salt production
What is the general equation for the reaction between metal carbonate and acid?
acid + metal carbonate -> salt + water + carbon dioxide
Neutralisation of acids and salt production
Explain why all alkalis are bases but not all bases are alkalis
All alkalis are bases because the react with acids and neutralise them, but not all bases are alkalis because most bases are insoluble, yet alkalis are soluble
