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chemistry > topic 2: inorganic chemistry > Flashcards

topic 2: inorganic chemistry Flashcards

(80 cards)

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1
Q

group 1 trend in reactivity + why

A

more reactive the further down you go

this is because the outermost electron is further away from the nucleus, decreasing attraction

this means the electron is more easily lost, becoming more reactive

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2
Q

metals + water

A

–> metal hydroxides + hydrogen gas

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3
Q

metal + oxygen

A

–> metal oxides

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4
Q

chlorine appearance

A

yellowgreen gas

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5
Q

bromine appearance

A

red-brown liquid emitting an orange vapour

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6
Q

iodine appearance

A

dark grey crystalline solid giving off a purple vapour

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7
Q

group 7 trend in reactivity + why

A

reactivity decreases the further down you go

this is because group 7 elements need to attract an electron to become stable.

the down you go, the more shells there are, meaning that attracting the extra electron is more difficult for being further away from the nucleus

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8
Q

abundance of gases in the atmosphere

A

78% nitrogen
21% oxygen
1% argon
0.04% carbon dioxide

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9
Q

reducing agent

A

donates electrons and gets oxidised

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9
Q

oxidising agent

A

accepts electrons and gets reduced

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9
Q

displacement

A

more reactive element pushes out a less reactive element from
a compound

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10
Q

chlorine water + chlorine solution (displacement)

A

nothing

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11
Q

chlorine water + potassium bromide solution (displacement)

A

orange solution (Br2) formed

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12
Q

chlorine water + potassium iodide solution (displacement)

A

brown solution (I2) formed

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13
Q

bromine water + potassium chloride solution (displacement)

A

no reaction

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14
Q

bromine water + potassium bromide solution (displacement)

A

no reaction

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15
Q

bromine water + potassium iodide solution (displacement)

A

brown solution (I2) is formed

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16
Q

iodine water (displacement)

A

displaces literally nothing OLOLOL

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17
Q

oxidation

A

loss of electrons

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18
Q

reduction

A

gain of electron

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19
Q

redox

A

both oxidation and reduction take place

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20
Q

investigate how iron can determine the percentage of oxygen in the air

A

soak some iron wool in acetic acid or water (catalyses the reaction + allows rusting) before pushing it into a measuring cylinder into a beaker of water

record the starting position of the water using the scale on the measuring cylinder (starting volume of air)

over time the level of the water will rise

this is because the oxygen reacts with the iron to make iron oxide!! the water fills up to fill in the space oxygen took up

after a week, record the finishing position of the water. this is the final volume

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21
Q

percentage of oxygen formula

A

start volume - final volume / start volume x 100

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21
Q

investigate how phosphorus can determine the percentage of oxygen in the air

A

place the phosphorus in a tube and attach a glass syringe at both ends

make sure one of the syringes is filled with air and the other is empty

heat the phosphorus and use the syringes to pass the air over it - the phosphorus will react with oxygen in the air to create phosphorus oxide

amount of air in the syringes decrease

measure the starting + final volumes of air using the scale on one of the syringes. push all the air into one syringe to measure the final volume

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22
combustion of magnesium
burns with a bright white flame into a white powder called magnesium oxide its slightly alkaline when dissolved in water
22
combustion of hydrogen
burns very easily - can be explosive makes a squeaky pop when heated
23
combustion of sulfur
burns with a pale blue flame and produces sulfur dioxide acidic when dissolved in water
23
thermal decomposition
substance breaks down into simpler substances by heating
24
copper (II) carbonate (thermal decomposition)
CuCO3 -> CuO + CO2 copper (II) carbonate -> copper oxide + carbon dioxide green powder to black !!!
24
ways to prevent rusting
barrier sacrificial protection galvanising
25
word equation for rusting
iron + oxygen + water -> hydrated iron(III) oxide (aka rust)
26
the reactivity series
please stop laughing calling me a careless zebra!! instead learn how cops save gold (and) platinum potassium sodium lithium calcium magnesium aluminium carbon zinc iron lead hydrogen copper silver gold platinum
27
galvanising
a coating of zinc is sprayed onto the object meaning it will be oxidised instead of iron as it is more reactive
28
sacrificial protection
placing a more reactive metal with iron to absorb the reactions
29
barrier
coat the iron with a barrier to keep out the water/oxygen e.g with paint, greasing, oil, etc
30
acid + metal
--> salt + hydrogen
31
greenhouse effect
they act like an insulating layer, trapping heat from the sun into the earth's atmosphere
32
metals reacting with acids (practical)
set up three boiling tubes and fill them with equal volumes of dilute acid (hydrochloric or sulfuric) place pieces of magnesium, zinc, and iron in separate test tubes, ensuring that they are the same size the speed of reaction is indicated by the rate at which the hydrogen bubbles are given off magnesium reacts vigorously producing loads of bubbles, while zinc and iron react more slowly
33
universal indicator
acid: red -> yellow neutral: green alkali: blue -> purple
34
methyl orange
acid: red alkali: yellow
35
phenolphthalein
acid: colourless alkali: pink
36
litmus
acid: red alkali: blue
36
acids and bases in terms of proton transfer
bases neutralise acids. they accept protons (OH-) acids are proton donors (H+)
36
acid + metal hydroxide
--> salt + water
36
acid + base
--> salt + water (neutralisation!!)
36
acid + metal oxide
--> salt + water
37
acid + ammonia
--> ammonium salt
38
acid + metal carbonate
--> salt + water + carbon dioxide
39
soluble or insoluble? - common salts of sodium, potassium and ammonium
soluble
40
soluble or insoluble? - nitrates
soluble
41
soluble or insoluble? - chlorides
soluble (except silver and lead)
42
soluble or insoluble? - sulfates
soluble (except lead, barium, and calcium)
43
soluble or insoluble? - common carbonates
insoluble (except sodium, potassium and ammonium)
44
soluble or insoluble? - common hydroxides
insoluble (except potassium, sodium and calcium)
45
practical - make a soluble salt
soluble salts can be formed by reacting an acid with an insoluble base start by heating acid in a water bath (speeds up the reaction) do this in a fume cupboard to avoid releasing acid fumes into the room add the base to the acid which will react to produce a soluble salt (+ water) filter off the excess solid to get a solution containing only the salt and water crystallise!!!
46
flame tests (practical)
identify metal ions clean a platinum wire by dipping it in dilute HCl before holding it to a flame once it burns without any colour you can dip it into the sample you want to test, and back into the blue part of the bunsen flame (hottest bit)
47
lithium chloride flame colour
red flame / pink
48
potassium chloride flame colour
lilac flame
49
sodium chloride flame colour
yellow flame
50
calcium chloride flame colour
orange-red flame
51
copper chloride flame colour
blue-green
52
how to form a coloured precipitate with certain metals
add a few drops of sodium hydroxide which will form an insoluble hydroxide hopefully
53
copper(II) precipitate
blue
54
iron(II) precipitate
sludgy green
55
iron(III) precipitate
reddish brown
56
how to draw out ammonia gas from ammonium ions (mystery powder!!)
add some sodium hydroxide to a solution of your mystery substance. then, test for ammonia gas
57
test for carbonates
add dilute hydrochloric acid. if carbonates are present then carbon dioxide will be released test for carbon dioxide to make sure
58
test for sulfates
add dilute hydrochloric acid, followed by a barium chloride solution a white precipitate will form meaning that it is a sulfate!!!!!
59
test for halides
add nitric acid followed with silver nitrate
60
chlorine precipitate colour
white
61
bromide precipitate colour
cream
62
iodide precipitate colour
yellow
63
test for chlorine
apply damp blue litmus paper. it bleaches before turning white
64
test for oxygen
relights a glowing splint
65
test for carbon dioxide
bubble the gas through a test tube of limewater. limewater should turn. cloudy
66
test for hydrogen
hydrogen makes a squeaky pop with a lit splint
67
ammonia
apply damp red litmus paper which should turn blue also smells like piss
68
physical test for water
boil at 100°C/freeze at 0°C
69
chemical test for water
add anhydrous copper (II) sulfate and it should turn blue
70

chemistry (4 decks)

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