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Chemistry IGCSE > 3.5 Metals > Flashcards

3.5 Metals Flashcards

1
Q

structure of metal has… (2 points)

A

1) lattice of positive metal ions
2) sea of delocalized electrons

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2
Q

delocalized electrons were…

A

lost by metal ions so freely move through the lattice

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3
Q

def. metallic bonding

A

very strong electrostatic force of attraction between positive metal ions and negative delocalized electrons

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4
Q

metals tend to have high melting points because…

A

this is because the metallic bonding is usually very strong so lots of energy is needed to break it

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5
Q

metals conduct electricity because…

A

this is because the delocalized electrons are free to move through the lattice

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6
Q

metals are malleable because…

A

this is because the layers of metal ions can slide over each other

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7
Q

def. thermal decomposition

A

heat energy is used to break down a substance

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8
Q

metal carbonates thermally decompose to form…

A

metal carbonate –> metal oxide + carbon dioxide

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9
Q

app. copper carbonate

A

green solid

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10
Q

app. copper oxide

A

black solid

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11
Q

CO2 collected by downward delivery because…

A

CO2 denser than air so sinks to bottom of a tube

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12
Q

eg. metals = lower on reactivity series (3 points)

A

1) Au (Gold)
2) Ag
3) Cu

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13
Q

eg. metals = in middle reactivity series (3 points)

A

1) Pb (lead)
2) Fe
3) Zn

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14
Q

eg. metals = higher on reactivity series (6 points)

A

1) Al
2) Mg
3) Ca
4) Li
5) Na
6) K

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15
Q

metal + cold water –>

A

metal hydroxide + hydrogen

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16
Q

obs. of metal + cold water reaction (2 points)

A

1) effervescence
2) solid disappears

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17
Q

metals in group 1 called and what they do (2 points)

A

1) alkali metals
2) react violently with water

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18
Q

obs. of metal (group 1) + cold water reaction (4 points)

A

1) solid floats
2) effervescence
3) solid moves
4) solid disappears

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19
Q

metals hydroxides are alkalis because…

A

they donate OH-

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20
Q

as metal gets more reactive, reactions are…

A

more vigorous

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21
Q

group 1 metals get ____ ________ as you go down group

A

more reactive

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22
Q

what happens when group 1 metal reacts

A

Loses its outer-shell electron to get full outer-shell

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23
Q

why does a group 1 metals react more quickly as you go down group (4 points)

A

1) atoms get bigger, have more shells
2) outer-electron further from nucleus
3) so attraction between nucleus and outer-electron is weaker
4) less energy needed to break the attraction

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24
Q

metal + steam –>

A

metal oxide + hydrogen

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25
Q

where does magnesium + steam reaction usually occur

A

horizontal tube

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26
Q

why is H2 gas and wet wool present in magnesium + steam reaction (2 points)

A

1) wet wool heated to generate steam for Mg to react with
2) H2 gas ignited to safely destroy it

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27
Q

why do metals react with cold water and hot steam to produce different products

A

steam has more energy, so both bonds in the water molecule can break

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28
Q

acid + metal –>

A

salt + hydrogen

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29
Q

how is salt formed

A

H is displaced from an acid

30
Q

all chlorides soluble except (2 points)

A

1) Ag+
2) Pb 2+

31
Q

all sulphates soluble except (3 points)

A

1) Ca 2+
2) Ba 2+
3) Pb 2+

32
Q

all nitrates are…

A

soluable

33
Q

all carbonates insoluble except (3 points)

A

1) Na+
2) K+
3) NH4+

34
Q

all hydroxides insoluble except (3 points)

A

1) Na+
2) K+
3) Ca 2+

35
Q

all oxides insoluble except (3 points)

A

1) Na+
2) K+
3) NH4+

36
Q

obs. of acid + metal reaction (2 points)

A

1) metal disappears
2) fizzing as hydrogen produced

37
Q

the more reactive a metal is…

A

the faster it will react with an acid

38
Q

why can’t Au, Ag, Cu react with acid

A

not possible as less reactive than H so can’t displace it

39
Q

why shouldn’t Li, Na, K react with acid

A

reaction with acids is too violent

40
Q

test for H2

A

lit splint produces a squeaky pop

41
Q

____ reactive metals can displace ____ reactive metals from their compounds (2 points)

A

More Less

42
Q

magnesium is a ____ solid

A

grey

43
Q

copper sulphate is a…

A

blue solution

44
Q

copper is a ____-______ solid

A

pink-orange

45
Q

magnesium sulphate is a…

A

colourless solution

46
Q

obs. in displacement reaction (2 points)

A

1) solid colour change
2) solution colour change

47
Q

in Mg (s) + CuSO4 (aq) –> Cu (s) + MgSO4 (aq) displacement reaction describe solid and solution colour change (2 points)

A

1) solid turns grey to pink-orange
2) solution turns blue to colourless

48
Q

a displacement reaction can only occur if the metal used is ____ ________ than the metal
already in the compound

A

more reactive

49
Q

most metals are found in the Earth’s crust as compounds with ______ and _______

A

oxygen sulphur

50
Q

the rocks containing specific metal compounds are called ____

A

ores

51
Q

gold (Au) and silver (Ag) are too unreactive to have combined with oxygen or sulphur so they are found…

A

native meaning chemically uncombined

52
Q

native metals don’t need to be chemically extracted because…

A

they already exist on their own

53
Q

redox reaction is… (2 points)

A

1) using carbon to displace a metal from its oxide
2) which are less reactive than carbon

54
Q

example of redox reaction

A

copper being displaced from its ore (copper oxide) via heating with carbon

55
Q

reduction (in terms of O2) is

A

loss of O2

56
Q

reducing agent (in terms of O2)

A

takes oxygen away from something else

57
Q

oxidation (in terms of O2)

A

gain of O2

58
Q

oxidising agent (in terms of O2)

A

gives O2 to something else

59
Q

redox (in terms of O2)

A

reduction and oxidation in the same reaction

60
Q

2 ways to extract from ores (2 points)

A

use electricity - metals more reactive than carbon
carbon extraction - metals less reactive than carbon

61
Q

def. rusting

A

chemical process when iron is oxidized to form rust

62
Q

rust =

A

hydrated iron (III) oxide

63
Q

app. of iron (3 points)

A

grey solid
shiny
malleable

64
Q

app. of rust/hydrated iron (III) oxide (3 points)

A

brown
dull
brittle

65
Q

describe 2 stages of rusting (2 points)

A

1) iron oxidised to form iron (III) oxide
2) iron (III) oxide hydrated by water to make rust/hydrated iron (III) oxide

66
Q

hydrated iron (III) oxide

A

Fe2O3.xH2O

67
Q

rust prevented by 3 methods (3 points)

A

1) Use barriers such as paint, oil, grease, plastic
but if breaks, rusting occurs
2) Sacrificial protection
3) Galvanisation

68
Q

M. Sacrificial protection (3 points)

A

1) Attach block of more reactive metal (Mg)
2) Displaces iron from rust as soon as rust forms
3) Mg block has to be replaced often

69
Q

M. Galvanisation (x points)

A

1) Coat iron with zinc
2) prevents O2 and H2O coming in contact with iron
3) but if crack appears zinc more reactive than iron so acts as sacrificial protection

70
Q

def. alloys

A

mixture of a metal with 1+ elements

71
Q

eg. alloys (3 points)

A

1) Steel (Iron + Carbon)
2) Brass
3) Bronze

72
Q

why alloys harder than pure metals (2 points)

A

1) the different-sized atoms/ions prevent the layers of metal ions from sliding over each other
2) so they are less malleable

Chemistry IGCSE (8 decks)

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