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Chemistry > Chemical Change Part One > Flashcards

Chemical Change Part One Flashcards

1
Q

how does sodium react with oxygen

A

a bright yellow flame
reaction happened quickly
hot and explosive

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2
Q

how does iron react with oxygen

A

sparks

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3
Q

how does copper react with oxygen

A

turns black from red/brown

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4
Q

how does magnesium react with oxygen

A

bright white flame
turned into white powder

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5
Q

what happens when a metal reacts with oxygen

A

creates a metal oxide

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6
Q

what kind of reaction happens when a metal reacts with oxygen and why

A

oxidation reaction as they gain oxygen

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7
Q

what is the word equation for metals + oxygen

A

metal + oxygen —–> metal oxide

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8
Q

what do metals reacting with water form

A

a metal hydroxide and water

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9
Q

what is the word equation for metals + water

A

metal + water ——> metal hydroxide + hydrogen

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10
Q

what happens when lithium reacts with water

A

floats on water
fizzes
let off steam

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11
Q

what happens when sodium reacts with water

A

fizzed
moved fast on surface of water
sparked

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12
Q

how does potassium react with water

A

lilac flame
exploded
fizzed very quickly
sparked

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13
Q

what condition is the metal hydroxide

A

alkaline
turns universal indicator purple

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14
Q

what is the formula for sulfuric acid

A

4
H. SO
2

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15
Q

what is the formula for nitric acid

A

HNO
3

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16
Q

what is the word equation for metals and acid

A

metal + acid ——> salt + hydrogen

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17
Q

what is the hydrogen test

A

a lit splint that pops

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18
Q

how do you name salts

A

1 first word of salts name is metal in experiment
2 second word of salts name is acid

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19
Q

what is the reactivity series

A

potassium
sodium
calcium
magnesium
aluminium
carbon - non metal
zinc
iron
tin
lead
hydrogen - non metal
copper
silver
gold]
platinum

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20
Q

what does the reactivity series go in order of

A

most reactive to least reactive

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21
Q

what is the acronym to remember the reactivity series

A

please
send
charlie’s
monkeys
and
chris’s
zebras
in
tall
lead
hard
cages
securely
guarded
promptly

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22
Q

how are metals displaced in the reactivity series

A

if a metal is above the other metal in the compound the reaction will happen
if a metal is below the other metal in a compound the reaction will not happen

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23
Q

what is a displacement reaction

A

when a more reactive metal can displace a less reactive metal from a compound

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24
Q

which are the more reactive metals in the reactivity series and how are they extracted

A

potassium
sodium
calcium
magnesium
aluminium

extracted using electrolysis

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25
Q

what are the less reactive metals in the reactivity series and how are they extracted

A

using carbon in a displacement reaction

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26
Q

which are the reactivity series unreactive metals and how are they extracted

A

silver
gold

found in natural state and don’t need to be extracted

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27
Q

what is the rock called when there is enough of the metal to make it work extracting

A

an ore

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28
Q

where are metals found

A

the ground

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29
Q

what is it called when a rock has metal but not enough worth extracting

A

just a rock

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30
Q

how is a metal turned from ore to metal oxide

A

metal oxide is separated from rock

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31
Q

how is metal oxide turned into a metal after being ore

A

the metal is chemically separated from the oxygen

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32
Q

why does how the metal is separated from oxygen vary

A

depends on where it is in the reactivity series

33
Q

why is carbon used to extract less reactive metals

A

it is higher than the metals in the reactivity series so it is more reactive
steals the oxygen away
leaves metal by itself and makes carbon dioxide
called a displacement reaction

34
Q

what is it called as each metal loses oxygen

A

called a reduction reaction

35
Q

how are the most reactive metals extracted

A

electrolysis

36
Q

what is electrolysis

A

when we split the substance using electricity
the metal oxide is separated from the oxygen

37
Q

what is oxidation

A

when a substance gains oxygen
when a substance loses electrons

38
Q

what is reduction

A

when a substance loses oxygen
when a substance gains electrons

39
Q

where are the electrons on an oxidation half equation

A

always on the right

40
Q

where are the electrons in a reduction reaction half equation

A

always on the left

41
Q

what is a redox reaction

A

when a substance has been oxidised and a substance has been reduced at the same time

42
Q

what is an indicator

A

a substance which changes colour to tell you if something is acid or alkali

43
Q

what are indicator examples

A

litmus paper
universal indicators

44
Q

what is the colour and numbers of strong acids

A

1-3
red

45
Q

what is the colour and number of weak acids

A

4-5
orange/yellow

46
Q

what are everyday examples of acids

A

lemon juice
vinegar
fizzy drinks

47
Q

what are lab examples of acids

A

nitric acid
sulfuric acid
hydrochloric acid

48
Q

how does acid taste

A

sour

49
Q

what does an acid form in a solution

A

H+ ions

50
Q

what are the number and colours of weak alkalis

A

8-11
dark green/blue

51
Q

what are the number and colours of
strong alkali

A

12-14
blue/purple

52
Q

what are the everyday examples of alkali

A

bleach
soap
toothpaste
indigestion tablets

53
Q

what is a base

A

metal oxide or metal hydroxide that is insoluble

54
Q

what is an alkali

A

metal hydroxide that is soluble

55
Q

how do alkalis taste

A

bitter

56
Q

what do alkalis form in a solution

A

OH- ion

57
Q

how do you write ionic equations

A

re write the equation showing separate ions present in each substance
remove any spectator ions (ions that don’t change state or charge)
rewrite out the equation without the spectator ion

58
Q

what does the volume have to be in for concentration

A

dm^3

59
Q

how do you change cm^3 to dm^3

A

divide by 1000

60
Q

what is the concentration equation

A

concentration = mass of solute/ volume of solvent

61
Q

what units is concentration in

A

g/dm^3

62
Q

how would a change in mass of the solute affect the concentration

A

if we increase the mass the concentration will increase

63
Q

how would a change in volume of the solvent affect the concentration

A

decreasing the volume increases the concentration

64
Q

how do you identify strong and weak acids (test 1)

A
  • 2cm depth of each acid in 2 separate test tubes
  • add two drops of universal indicator to each acid and record the colour observed and work out ph number
65
Q

how do you identity strong and weak acids (test 2)

A
  • 2 cm depth of each acid into separate test tubes and add a piece of magnesium ribbon to each one
  • time how long it takes for the reaction to stop
66
Q

what is the result of test 1 of identifying strong and weak acids

A

strong acid turns red
weak acid turns orange

67
Q

what is the result of test 2 for strong and weak acids

A

strong acid would bubble more and would stop reacting first

68
Q

what is test 3 for identifying strong and weak acids

A
  • put 2cm depth of each acid into separate test tubes and add a spatula full of powdered sodium carbonate to each one
  • time how long it takes for the reaction to stop
69
Q

what are the results of test 3 of identifying strong and weak acids

A

strong acid bubbles more and stops reacting quicker

70
Q

what are 3 examples of a strong acid

A

hydrochloric acid
sulfuric acid
nitric acid

71
Q

what are 3 examples of a weak acid

A

ethanoic acid (vinegar)
citric acid (citrus fruits)
carbonic acid (fizzy drinks)

72
Q

what do strong acids do in water

A

completely ionise in water (this means the ions split up)

73
Q

what does strong acids completely ionising in water mean

A

the solution has a high concentration of H+ ions
low ph
this is not reversible

74
Q

what do weak acids do in water

A

partially ionise in water (only a small amount of acid molecules split up )

75
Q

why do weak acids partially ionise in water

A

have a low concentration of H+ IONS
higher pH

76
Q

how do you calculate pH

A

-log. [H+]
10

77
Q

how do you calculate [H+]

A

[H+] = 10^-PH

78
Q

what is a concordant result

A

two titres that are within 0.1cm^3 of eachother

79
Q

titration calculation steps

A

write known and unknown
moles= conc x volume/ 100
work out ratio
workout unknown concentration
convert mol/dm^3 to g/dm^3 = CONCENTRATION G/DM3 = concentration in mol/dm3 x mr of substance

Chemistry (36 decks)

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