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GCSE Chemistry > C4 - Predicting Chemical Reactions > Flashcards

C4 - Predicting Chemical Reactions Flashcards

1
Q

which group are the alkali metals

A

group 1

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2
Q

what do all group 1 metals have in their outer shell

A

1 electron

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3
Q

what do all group 1 metals want to lose

A

all want to lose an electron (be oxidised) to form a cation with a +1 charge

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4
Q

what are some physical properties of the group 1 metals

A

they are dull on the outside but shiny when freshly cut - can be cut with a knife. they have low density - will often float on water. they are good conductors of electricity

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5
Q

what is a chemical property of the group 1 metals

A

they react with water so need to be stored under oil

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6
Q

what are the group 1 metals in order from least reactive to most reactive

A

Li, Na, K, Rb, Cs, Fr

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7
Q

as you go down the group, 1 metals what increases/decreases

A

reactivity increases, density increases and melting and boiling points decrease

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8
Q

which 3 metals in the group 1 metals float on water

A

lithium, sodium and potassium

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9
Q

why are elements reactive

A

elements are reactive because atoms will gain or lose electrons until they have a full outer shell

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10
Q

why do the group 1 metals become more reactive going down the group

A

because the outermost electron gets further away from the nucleus, so the force of attraction between the electron and the nucleus is weaker

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11
Q

what are the transition metals

A

the elements between group 2 and group 3 of the periodic table

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12
Q

what are the transition metals used for

A

used as catalysts in chemical reactions

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13
Q

what do the transition metals form with diferent charges

A

they form coloured ions

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14
Q

what are some physical properties of the transition metals

A

they are shiny when cut. they are good conductors of electricity. they are strong, dense and malleable. they have high melting points. they are not as reactive as metals in groups 1/2

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15
Q

what are some chemical properties of the transition metals

A

they react slowly to produce coloured compounds. they can form ions with different charges

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16
Q

what are the noble gases

A

the non metals in group 0

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17
Q

what are some chemical properties of the group 0 elements

A

they are unreactive. they are monatomic. they are gases at room temperature.

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18
Q

what is the elctronic structure of the group 1 metals

A

they all have one electron in their outer shell. they all want to lose an electron to form a cation with a +1 charge

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19
Q

what is the electronic structure of the group 0 elements

A

they all have a full outer shell. they do not react with other elements. they do not form ions or covenlently bonded molecules

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20
Q

which group have intermolecular forces of attraction

A

the group 0 metals

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21
Q

what are the halogens

A

the non metals in group 1

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22
Q

what colour gas in fluorine

A

green gas

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23
Q

what colour gas in chlorine

A

yellow gas

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24
Q

what colour gas in bromine

A

orange gas

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25
what colour solid is iodine
grey solid
26
what is the electronic structure of the group 7 elements
they all have 7 electrons in their outer shell. they can be reduced to form an ion (or anion) with a -1 charge
27
which group can be dissolved directly in water
the group 7 elements
28
which non metals in the group 7 elements are halogens
fluorine, chlorine, bromine and iodine
29
as you go down the group 7 elements, what increases/decreases
reactivity decreases and melting/boiling points increase
30
what are the group 7 elements in order from least to most reactive
At, I, Br, CI, F
31
what are the group 0 metals
He, Ne, Ar, Kr, Xe, Rn
32
which group can be dissolved directly in non polar solvent
group 7 elements
33
why do group 7 elements become less reactive going down the group
because the closer the outer shell is to the nucleus, the stronger the force of attraction, and the easier it is to gain an electron
34
what does the more reactive halogen end up with
the more reactive halogen ends up with its own electron as a halide ion
35
what does the least reactive halogen end up with
the least reactive halogen ends up having to share electrons in a halogen molecule
36
how do you detect C02
limewater (calcium hydroxide solution) turns cloudy white when carbon dioxide is bubbled through. it is cauded by the formation of a calcium carbonate precipitate
37
how do you detect chlorine
chlorine reacts with water to produce hydrochloric acid and bleach
38
what is the method of detecting chlorine
1) dampen a piece of blue litmus paper with tap water. 2) hold the paper near container the holds substance. 3) chlorine turns paper red than white
39
how do you know that you've detected hydrogen
a lighted splint will produce a squeaky pop
40
how do you know that you've detected oxygen
it relights a glowing splint
41
how do you carry out a flame test, to test for cations
use a nichrome wire loop. then dip in acid and rinse in distilled water. dip in powder and put in flames
42
what is the ion for lithium
Li+
43
what is the ion for sodium
Na+
44
what is the ion for potassium
K+
45
what is the ion for calcium
Ca2+
46
what is the ion for copper
Cu2+
47
what is the flame test colour for lithium
red
48
what is the flame test colour for sodium
yellow
49
what is the flame test colour for potassium
lilac
50
what is the flame test colour for calcium
orange-red
51
what is the flame test colour for copper
green-blue
52
which group hydroxides are soluble in water
group 1 hydroxides are solible in water, other metal hydroxides are insoluble in water
53
how do you test for hydroxide
add a few drops of sodium hydroxide, observe colour of precipitate
54
what is the formula of iron (II) ion
Fe2+
55
what is the formula of iron (III) ion
Fe3+
56
what is the formula of copper (II) ion
Cu2+
57
what is the formula of calcium ion
Ca2+
58
what is the formula of zinc ion
Zn2+
59
what is the colour of iron (II) hydroxide precipitate
green
60
what is the colour of iron (III) hydroxide precipitate
orange brown
61
what is the colour of copper hydroxide precipitate
blue
62
what is the colour of calcium hydroxide precipitate
white
63
what is the colour of zinc hydroxide precipitate
white
64
what is the method of detecting sulphate ions
add a few drops of dilute hydrochloric acid. then add a few drops of barium chloride/nitrate. a white precipitate indicates sulphate ions are present
65
what is the ionic equation for sulphate ions
Ba 2+ + S04 2- → BaSO4
66
what is the method of detecting carbonate ions
add a few drops of dilute hydrochloric acid. Bubbles/effervesce (carbon dioxide) will be absorbed
67
what is the ionic equation for carbonate ions
2H+ + CO3 2- → CO2 + H2O
68
what is the method of detecting halide ions
add a few drops of dilute nitric acid. then add silver nitrate solution. a white, cream or yellow precipitate will form
69
what is the ionic equation for halide ions
Ag+ + CI- → AgCI
70
how does instrumental analysis work
a machine carries out the analysis
71
what are some advantages of instrumental analysis over chemical tests
sensitivity, accuracy, speed
72
what does each peak represent in gas chromatography
each peak represents a substance in a mixture
73
what do the areas under each peak show, in gas chromatography
the areas under each peak shows the relative amouts of each substance in the mixture
74
what is the rention time
the rention time is the time that it takes for the substance to travel through the chromatography column
75
how does infrared spectroscope work
infrared is absorbed at certain wavelengths by different bonds. these bonds can be identified in a sample
76
what does a mass spectrometer measure
a mass spectrometer can measure the masses of atoms and molecules
77
how does mass spectrometry work
the sample molecules are broken down to form fragment ions which are then detected
78
what does each peak represent in mass spectrometry
each peak represents a fragment of the molecule
79
what does the peak on the far right represent
the peak on the far right represents the molecular ion and gived the RFM

GCSE Chemistry (12 decks)

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