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Chemistry > C 5.1-5.8 chemical changes > Flashcards

C 5.1-5.8 chemical changes Flashcards

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1
Q

what is the reactivity series

A

a list of metals in order of their reactivity

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2
Q

how can you order metals

A

by comparing how they react with water or whit dilute acid

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3
Q

reaction with water of metals + order of reactivity

A

alkali metals react giving off hydrogen gas and leaving alkaline solutions, most metals don’t react
potassium
sodium
lithium

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4
Q

when do you use acids to show reactivity series

A

when reaction with water is too slow

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5
Q

how do we compare the reactivity of metals

A

by looking at how fast or violent their reaction with water and acids are

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6
Q

the speed of reaction with dilute acids is indicated by…,

A

rate at which bubbles of hydrogen are given off

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7
Q

when does a displacement reaction occur

A

when a more reactive element displaces a less reactive element from a compound

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8
Q

eg of displacemnt reaction

A

Mg + CuSO4=MGSO4+ Cu

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9
Q

what is an ionic equation (eg with Mg + CuSO4=MGSO4+ Cu)

A

shows only atom and ion that change in a reaction
Mg + Cu(2+)= mg (2+) + Cu

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10
Q

how can you give positions in the reactivity series to the non-metals hydrogen and carbon

A

on the basis of displacement reactions.
carbon can displace zinc from its oxide but not alumionium so in the series is placed in between them two.
copper can’t displace H from an acid whereas lead can so H is in between them

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11
Q

most of metals need to be

A

extracted from a compound

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12
Q

what do metals often need to be extracted from

A

oxides are the ores ,

created from reaction with oxygen

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13
Q

name of reaction that separates a metal from its oxide

A

reduction reaction

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14
Q

how does reactivity series help you in ores extraction

A

help you decide best way to extract the metal

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15
Q

what will carbon(non-metal) do to extract metals

A

will displace less reactive metals from their oxides

can only be used when carbon is more reactive

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16
Q

process and equation to extract metals with carbon

A

heat metal oxide with carbon, removing the hydrogen

metal oxide + carbon = metal + carbon dioxide

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17
Q

when is electrolysis used

A

to extract metals more reactive than metals

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18
Q

how and from what is aluminum extracted from compound (aluminum oxide)

A

electrolysis from bauxite

19
Q

process of electrolysis with aluminum

A 
aluminum oxide is mixed with molten cryolite to lower the very high melting point and reducing the energy needed.
molten mixture contains free ions(conducts energy)
positive ions of AL(3+) are attracted to the negative electrode where they each pick up 3 electrons and turn into neutral atoms.
negative O(-2) ions are attracted to positive electrode where they each lose electrons, forming neutral oxygen that combine to form O2 molecules
20
Q

when is salt formed (metal)

equation

A

reaction takes place between a metal and an acid, when hydrogen in an acid is wholly or partially replaced by metal or ammonium ions
metal + acid =salt+ hydrogen

21
Q

why are alkali metals never added to acid

A

too reactive, dangerous

22
Q

what kind of metals can react to form salt

A

metal must be above hydrogen in reactivity series but not too reactive

23
Q

the salt you make depends on

A

metal you use

zinc metal will always make zinc salts

24
Q

how can a sample of the salt make from reaction be crystalized

A

by evaporating off the water

25
Q

what are bases

A

compounds that can neutralize acids (alaklis)

26
Q

WHAT IS NEUTRALISATION

A

acid + base = salt + water

27
Q

two reactions where you can make salts

A

solutions of an acid and an alkali
acid with carbonate

28
Q

purpose of indicator

A

indicate if reaction is acid or alkaline

29
Q

acids react with …. to form salts

A

metals, bases and carbonates

30
Q

A soluble salt can be prepared by reacting an acid with a suitable insoluble reactant including:

A

a metal
a metal oxide
a metal hydroxide
a carbonate

31
Q

process to get a soluble salt

A

Add powdered insoluble reactant to acid in a beaker, one spatula at a time, stirring to mix. Continue adding powder until it is in excess (some unreacted powder is left over). All the acid has now reacted.
Filter the mixture in the beaker to remove the excess solid. The filtrate now contains only the salt and water.
Heat the solution in an evaporating dish over a water bath. Stop heating when small crystals start to appear around the edge of the evaporating basin. The solution is now saturated.
Leave the saturated solution at room temperature for a day or two. This gives time for large crystals to form.
If necessary, dry the crystals by dabbing gently with filter paper.

32
Q

what is an acid

A

substance that forms aqueous solutions with pH less than 7

33
Q

what is a base

A

substance with pH greater than 7

metal oxides are bases

34
Q

what do alkalis form in water

A

OH- ions

35
Q

what do acids do in aqueous solution

A

they ionise, produce hydrogen ions

36
Q

what happen to strong acids in water

A

ionise completely , all acids particles dissociate to realese H+ ions

37
Q

what happen to weak acids in solution

A

do not fully ionise, only a small portion of particles dissociate to release H+ IONS

38
Q

WHAT DOES THE IONISATION OF A weak acid set up

A

equilibrium between undissociated and dissociated acid, as it is a reversible reaction
equilibrium lies to the left as only a few H+ released

39
Q

why are the strong aciuds more reactive on the same concentartion

A

concentration of H+ higher , rate if reaction faster

40
Q

why is pH of strong acid always less than weak acid in same concentration

A

for every 1 on pH cale , concentration of H+ ions increase by a factor of 10

41
Q

what is the concentration acids

A

how much acid in a certain volume of water

42
Q

when will pH decrease(concentartion)

A

with increasing acid concentration

43
Q

reaction with metal and acid produces

and kind of reactio

A

hydrogen + salt

redox reaction

44
Q

a carbonate reacts with acid to produce

A

salt+ water+ carbon dioxide gas

Chemistry (14 decks)

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