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chemistry gcse > chemistry ( making salts) > Flashcards

chemistry ( making salts) Flashcards

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1
Q

what are ores

A

ores are rocks from which it is economical to extract the metals that they contain

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2
Q

what happens to most metals in ores

A

they are chemically bonded to other elements in compounds. many of these metals have been oxidized (have oxygen added) by oxygen in air to form oxides

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3
Q

order or reactivity series

A 
potassium 
sodium
lithium 
calcium 
magnesium 
zinc
iron
tin
lead
copper 
silver 
gold
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4
Q

what happens when potassium sodium lithium calcium react with water

A

they fizz, giving off hydrogen gas leaving an alkaline solution of metal hydroxide

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5
Q

what happens when magnesium aluminum zinc iron react with water

A

very slow reaction

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6
Q

what happens when tin and lead react with water

A

slight reaction with steam

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7
Q

what happens when copper silver gold react with water

A

no reaction even with steam

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8
Q

what happens in displacement reactions

A

a more reactive metal with displace a less reactive metal from an aqueous solution of one of its salts.

e.g harry chelsea
megan

becomes
harry megan
chelsea

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9
Q

copper sulfate + zinc becomes what in displacement reaction & why

A

zinc sulfate + copper

because zinc is more reactive than lead - it is higher in the reactivity series so zinc displaces lead

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10
Q

what is oxidation

A

oxidation is los of electrons

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11
Q

what is reduction

A

reduction is gained

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12
Q

what is the equation of making a metal hydroxide

A

metal + water = metal hydroxide + hydrogen

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13
Q

why is jewellery made from gold and silver

A

because both gold and silver have low reactivity and therefore won’t react with skin, oxygen or acid

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14
Q

equation for making salts

A

metal + acid = metal salt + hydrogen

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15
Q

why are teeth fillings not made from lithium

A

because it is very reactive and it will react with water and acids and break down

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16
Q

when does iron rust

A

iron rusts when iron and oxygen react in the presence of water or moisture in the air. it then rusts when iron or its alloys corrode

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17
Q

what happens when potassium is added to water

A

the metal melts and floats it moves around very quickly on surface of water. the hydrogen reacts instantly and causes fizzing

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18
Q

what is an oxide layer

A

an oxide layer is a thin layer of coating of an oxide. a coating may be more protective , decorative or functional . the more dense and tightly bound the oxides are the more corrosion resistant it is.

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19
Q

why does aluminum have an oxide layer

A

aluminum develops a thin oxide layer on surface when metal comes in contact with oxygen. oxide layer protects aluminum against corrosion and if damaged will immediately regenerate , provided their is oxygen present

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20
Q

what is diff abt carbon and hydrogen in reactivity series to other metals

A

they are non metals

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21
Q

oxidation abd reductioh table

A

oxidation:
oxygen : gain
hydrogen: lose
electron : lose

reduction:
oxygen: lost
hydrogen: gain
election : gain

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22
Q

copper, lead, iron and zinc can be purified using carbon . aluminum cannot- why not?

A

aluminum is higher than carbon in reactivity series

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23
Q

how can we purify metals above carbon and hydrogen in the reactivity series

A

heating with another metal won’t work so use electrolysis

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24
Q

what does ductile mean

A

can be drawn into long thin wires

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25
Q

what does dense mean

A

heavy for its size - particles tightly packed together

26
Q

what does malleable mean

A

change it’s shape, especially when heated and hammered

27
Q

what does sonorous mean

A

shaped metal gives a musical ringing tone when hammered

28
Q

what does conductivity mean

A

rate at which heat / electricity passes through metal

29
Q

what does lustre mean

A

can be polished to a shine

30
Q

what does corrosion mean

A

metal can damage by rusting or tarnishing

31
Q

metals will only react with acids if they are

A

more reactive than the hydrogen in the acid

32
Q

when making salts what does nitric acid , sulphuric acid and hydrochloric acid make

A

nitric- nitrates
sulphuric- sulphates
hydrochloric- chlorides

33
Q

crystallization in salts

A

when water evaporates from a salt solution , crystals will start to appear

at this point the solution is saturated and cannot hold any more solute

dipping a glass rod in the solution will show crystals on rod end

34
Q

when making salts what happens to metal ions

A

metal ions has lost electrons so it has been oxidized

35
Q

in making salts what happens hydrogen ions

A

hydrogen ions has gained electrons it has been reduced

36
Q

making salts required practical method

A

measure 40 cm cubes of sulfuric acid and put it into 100 cm cubed beaker

set up bunsen burner, tripod , gauze and heatproof mat. put the beaker on the gauze and heat the acid gently until it is almond boiling. then turn off bunsen burner

remove glass beaker from tripod. use spatula to add a small amount of copper oxide power to the hot acid. stir with glass rod. the copper oxide will disappear and solution will turn clear blue

continuously add copper oxide until some of it remains after stirring

allow apparatus to cool completely

set up the filter funnel and paper over comical flask

pour the filtrate from comical flask into evaporating basin

set up a water bath using the 250 cm cubed beaker on tripod and gauze

evaporate the filtrate gently using the water bath

when crystals start to form stop heating the water bath

pour remaining solution into the crystallizing dish

leave crystallizing dish in a cool palce

remove crystals from concentrated solitarily with a spatula

37
Q

equation for neutralization reaction

A

acid + alkali»> salt + water

38
Q

how can u tell when a neutralization reaction has been achieved

A

use an indicator which changes colour and shows all PHs

litmus paper

39
Q

what do neutralization reactions produce

A

salt , water and oxygen

40
Q

what is PH in neutralization reaction

A

7

41
Q

what is an aqueous solution

A

it is a solute (solid) dissolved in a liquid . can be acidic , alkaline or neutral depending on the solute

42
Q

alkali in neutral solutions

A

are soluble hydroxides e.g sodium hydroxide

43
Q

base in neutral solutions

A

such as alkalis. metal oxides and metal hydroxide can neutralize acids

44
Q

acids in neutral solutions

A

taste source.g citric acid, sulfuric acid and ethanoic acid

45
Q

what do strong acids do in solution

A

completely ionise

46
Q

weak acids in solution

A

most molecules stay as they are and don’t release H+ ions

47
Q

what is electrolysis

A

splitting with electricity

48
Q

what is an electrolyte

A

the compound that is broken down

49
Q

what are electrodes made

A

an unreactive substance

50
Q

what should electrodes not do

A

interfere with the reaction

51
Q

what are cations

A

positive and move to the cathode

52
Q

what are anions

A

negative and move to the anode

53
Q

what happens to cations and anions at electrodes

A

they lose their charge and become elements

54
Q

practical : electrolysis of copper sulphate (blue solution )

1) both electrons will b made of?
2) the negative cathode will form?
3) the positive anode will evolve ?

A

both electrons will be made of carbon

the negative cathode will form copper metal.

the positive anode will evolve oxygen gas (bubbles )

55
Q

will ectrolysis conduct with solids

A

electrolysis will not conduct with solids because electrons need space to move even if they are iconic

56
Q

required practical : electrolysis

A

1) pour approximately 50 cm cubed copper chloride solution into the beaker
2) add the petri dish lid and insert the carbon rods through the holes. RODS MUST NOT TOUCH EACHOTHER
3) attach crocodile clips to the rods. connect rods to the dc terminals of a low voltage power supply
4) select a 4V power supply and switch on
5) look at both electrodes and record observations
6) use forceps to hold a piece of blue litmus paper in the solution next to the anode and identify the element
7) record ur results in a table

57
Q

what does the effect of water do in electrolysis

A

aqueous soluatiobs make electrolysis more complicated to predict

58
Q

what do half equations show

A

what happens at each electrode

59
Q

how can you tell if chlorine has formed at the positive electrode

A

bubbling and smell like swimming pool

60
Q

how can u test if oxygen has formed at positive electrode

A

it religjts the splint

61
Q

what happens to cations when they form elements at electrodes

A

they gain negative electrons and become no charge

62
Q

what happens to anions when they form elements at electrodes

A

they lose electrons to become not charged

chemistry gcse (6 decks)

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