T4 chemical changes Flashcards

1
Q

what is oxidation/reduction

A

oxidation - when a substance gains oxygen

reduction - when a substance loses oxygen

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2
Q

what are the trends in reactivities of metals in reactions with acids/water

A

metals above H2 in reactivity react with acid to produce H2, the more reactive the metal is, the quicker and more violent reaction with acid occurs

metals below H2 don’t react with acid

not all metals above H2 react with water - mostly group 1 and 2 metals
aluminium is the borderline case

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3
Q

what is a displacement reaction

A

reaction where a more reactive metals displaces a less reactive metal from a compound

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4
Q

how are unreactive metals found in earth

A

in their natural state

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5
Q

how can metals less reactive than carbon be extracted

A

reduction with carbon

carbon displaces the metal in a metal oxide - gets oxidised to carbon oxides

metal from the metal oxide gets reduced to the pure metal

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6
Q

how are metals more reactive than carbon extracted

A

electrolysis

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7
Q

how are oxidation and reduction defined in terms of electron transfer

A

oxidation - loss of electrons

reduction - gain of electrons

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8
Q

general equation for a reaction between metals and acids

what type of reaction is this

A

metal + acid > salt + hydrogen

redox reaction, also displacement reaction

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9
Q

which metals in the reactivity series will react with acid

A

those above hydrogen

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10
Q

general equation for a neutralisation reaction

A

base + acid > salt + water

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11
Q

general equation for the reaction between metal carbonate and acid

A

metal carbonate + acid > salt + water + carbon dioxide

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12
Q

general equation for the reaction between metal oxides and acids

A

metal oxide + acid > a salt + water

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13
Q

what is a redox reaction

A

reaction where both oxidation and reduction occurs

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14
Q

how is a soluble salt formed

A
  1. react the excess with some insoluble chemicals
  2. filter off the leftovers
  3. crystalise the product
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15
Q

what do acids and alkalis produce in aqueous solutions

A

acids - hydrogen ions

alkalis - hydroxide ions

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16
Q

what are bases, acids and alkalis

A

b - compounds that neutralise acids
acids - produce hydrogen ions in aqueous solutions
alkalis - soluble bases which produce hydroxide ions in aqueous solutions

17
Q

what is the pH scale and what does a pH of 7 show

A

measure of acidity/alkalinity of a solution

neutral solution

18
Q

state the general equation for a neutralisation reaction in a short, ionic form

A

H+ + OH- > H2O

19
Q

what is a strong acid and a weak acid

A

S - completely ionised in aqueous solution

w - only partially ionised in aqueous solution

20
Q

what happens to pH as concentration of H+ increases

A

decreases

21
Q

what is a concentrated acid and what is a dilute acid

is this the same as a strong and weak acid

A

c - has more moles of acid per unit volume than dilute
d - refers to solutions of low concentration

not the same - concentration is different to strength of an acid

strength refers to whether the acid is completely ionised in water (strong) or only partially (weak)

22
Q

as the pH is decreased by one unit, what change is seen in the hydrogen ion concentration

A

increases by a factor of 10

23
Q

what is electrolysis

A

passing of an electric current through ionic substances that are molten or in solution to break them down into elements

ions are discharged at electrodes to produce these

24
Q

what is an electrolyte

A

liquid/solution which conducts electricity

25
Q

what is a cathode and what is an anode

A

c - negative electrode

a - positive electrode

26
Q

what occurs at the cathode and what occurs at the anode during electrolysis

A

c - reduction occurs

a - oxidation occurs

27
Q

in aqueous electrolysis, which element is discharged at the cathode

oxygen is produced at the anode unless what

A

less reactive element discharges at the cathode, hydrogen is produced unless there is a less reactive metal in which the metal is produced

oxygen is produced at anode unless the solution contains halide ions in which halogen molecules are produced

28
Q

how is aluminium manufactured

why is it expensive

A

made through the electrolysis of aluminium oxide and cryolite

lots of energy is needed to produce the current in electrolysis which makes this process expensive

29
Q

half equations in the extraction of aluminium

A

Al3+ + 3e- > Al (cathode)
2O2- >O2 + 4e- (anode)

oxygen reacts with C of the anode producing CO2

30
Q

why is cryolite used in manufacturing of aluminium

A

lowers the melting point of aluminium oxide, reducing energy costs

31
Q

what are the half equations in electrolysis of the aqueous Na2SO4

A

2H+ + 2e- > H2 (cathode)

4OH- > 2H2O + O2 + 4e- (anode)

32
Q

what are the half equations in electrolysis of the molten and aqueous KCl

A

K+ + e- > K (cathode)
2Cl- > Cl2 + 2e- (anode)

2H+ + 2e- > H2 (cathode)
2O2- > O2 + 4e- (anode)

33
Q

half equations in electrolysis of the aqueous CuBr2

A

Cu2+ + 2e- > Cu (cathode)

2Br- > Br2 + 2e- (anode)