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Chemistry > Chemical Change Part One > Flashcards

Chemical Change Part One Flashcards

(79 cards)

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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
what are the less reactive metals in the reactivity series and how are they extracted
using carbon in a displacement reaction
26
which are the reactivity series unreactive metals and how are they extracted
silver gold found in natural state and don't need to be extracted
27
what is the rock called when there is enough of the metal to make it work extracting
an ore
28
where are metals found
the ground
29
what is it called when a rock has metal but not enough worth extracting
just a rock
30
how is a metal turned from ore to metal oxide
metal oxide is separated from rock
31
how is metal oxide turned into a metal after being ore
the metal is chemically separated from the oxygen
32
why does how the metal is separated from oxygen vary
depends on where it is in the reactivity series
33
why is carbon used to extract less reactive metals
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
what is it called as each metal loses oxygen
called a reduction reaction
35
how are the most reactive metals extracted
electrolysis
36
what is electrolysis
when we split the substance using electricity the metal oxide is separated from the oxygen
37
what is oxidation
when a substance gains oxygen when a substance loses electrons
38
what is reduction
when a substance loses oxygen when a substance gains electrons
39
where are the electrons on an oxidation half equation
always on the right
40
where are the electrons in a reduction reaction half equation
always on the left
41
what is a redox reaction
when a substance has been oxidised and a substance has been reduced at the same time
42
what is an indicator
a substance which changes colour to tell you if something is acid or alkali
43
what are indicator examples
litmus paper universal indicators
44
what is the colour and numbers of strong acids
1-3 red
45
what is the colour and number of weak acids
4-5 orange/yellow
46
what are everyday examples of acids
lemon juice vinegar fizzy drinks
47
what are lab examples of acids
nitric acid sulfuric acid hydrochloric acid
48
how does acid taste
sour
49
what does an acid form in a solution
H+ ions
50
what are the number and colours of weak alkalis
8-11 dark green/blue
51
what are the number and colours of strong alkali
12-14 blue/purple
52
what are the everyday examples of alkali
bleach soap toothpaste indigestion tablets
53
what is a base
metal oxide or metal hydroxide that is insoluble
54
what is an alkali
metal hydroxide that is soluble
55
how do alkalis taste
bitter
56
what do alkalis form in a solution
OH- ion
57
how do you write ionic equations
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
what does the volume have to be in for concentration
dm^3
59
how do you change cm^3 to dm^3
divide by 1000
60
what is the concentration equation
concentration = mass of solute/ volume of solvent
61
what units is concentration in
g/dm^3
62
how would a change in mass of the solute affect the concentration
if we increase the mass the concentration will increase
63
how would a change in volume of the solvent affect the concentration
decreasing the volume increases the concentration
64
how do you identify strong and weak acids (test 1)
- 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
how do you identity strong and weak acids (test 2)
- 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
what is the result of test 1 of identifying strong and weak acids
strong acid turns red weak acid turns orange
67
what is the result of test 2 for strong and weak acids
strong acid would bubble more and would stop reacting first
68
what is test 3 for identifying strong and weak acids
- 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
what are the results of test 3 of identifying strong and weak acids
strong acid bubbles more and stops reacting quicker
70
what are 3 examples of a strong acid
hydrochloric acid sulfuric acid nitric acid
71
what are 3 examples of a weak acid
ethanoic acid (vinegar) citric acid (citrus fruits) carbonic acid (fizzy drinks)
72
what do strong acids do in water
completely ionise in water (this means the ions split up)
73
what does strong acids completely ionising in water mean
the solution has a high concentration of H+ ions low ph this is not reversible
74
what do weak acids do in water
partially ionise in water (only a small amount of acid molecules split up )
75
why do weak acids partially ionise in water
have a low concentration of H+ IONS higher pH
76
how do you calculate pH
-log. [H+] 10
77
how do you calculate [H+]
[H+] = 10^-PH
78
what is a concordant result
two titres that are within 0.1cm^3 of eachother
79
titration calculation steps
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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