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chemistry all note flashcards - 3rd And 4th > 3.5 - Metals > Flashcards

3.5 - Metals Flashcards

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1
Q

what are the two components in the structure of a metal

A
  • lattice of positive metal ions
  • sea of delocalized electrons
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2
Q

what charges do metal ions in the metal structure have

A

their usual charge

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3
Q

what were the delocalized electrons lost by and how do they move

A

lost by the metal ions and they move freely through the lattice

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4
Q

what is metallic bonding

A

the electrostatic attraction between the positive metal ions and the negative delocalized electrons

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5
Q

what type of attraction is metallic bonding

A

usually very strong

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6
Q

what are the properties of metals

A

have high melting points
conduct electricity
malleable

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7
Q

why do metals tend to have high melting points

A

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

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8
Q

why do metals conduct electricity

A

the delocalized electrons are free to move through the lattice

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9
Q

why are metals malleable

A

the layers of metal ions can slide over each other

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10
Q

what is thermal decomposition

A

a thermal decomposition reaction is when heat energy is used to break down a substance

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11
Q

what is the equation for a thermal decomposition

A

metal carbonate –> metal oxide + carbon doxide

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12
Q

what would the thermal decomposition of copper carbonate look like

A

copper carbonate –> copper oxide + carbon dioxide
CuCO3(s) CuO(s) CO2(g)
green solid black solid colourless gas

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13
Q

what is carbon dioxide often collected by in thermal decomposition

A

downward delivery

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14
Q

why is carbon dioxide collected by downward delivery

A

because carbon dioxide is denser than air

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15
Q

what is downward delivery

A

the carbon dioxide sinks to the bottom of a tube and stays there until you want to use it

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16
Q

list the metal reactivity series from lowest to highest

A

Au Ag Cu (H) Pb Fe Zn (C) Al Mg Ca Li Na K

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17
Q

why are hydrogen and carbon included in the reactivity series despite being non-metals

A

their positions are important when considering displacement reactions

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18
Q

what do metals react with cold water to form

A

metal hydroxides and hydrogen

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19
Q

what is the metal and water reaction equation

A

metal + water –> metal hydroxide + hydrogen

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20
Q

what are the two significant observations of metal and water reactions

A

effervescence - due to the hydrogen gas produced
solid disappears - due to being used up in the reaction

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21
Q

what are the metals in group 1 of the periodic table called

A

alkali metals

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22
Q

how do the metals in group 1 of the periodic table react with water

A

violently to form metal hydroxides and hydrogen

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23
Q

group 1 metal and water reaction equation

A

metal + water –> metal hydroxide + hydrogen

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24
Q

what similar observations do the reactions of Li, Na and K with water share

A
  • solid floats - it is less dense than water
  • effervescence - hydrogen gas is produced
  • solid moves - the effervescence propels it around the surface of the water
  • solid disappears - it is used up in the reaction
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25
Q

what happens when universal indicator is added to the water after its reaction with Li, Na or K

A

it turns dark blue - the metal hydroxides are alkalis because they donate OH-

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26
Q

what happens to the reaction of group 1 metals and water` as the reactivity increases

A

it gets more vigorous

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27
Q

what is the increasing reactivity order of Lithium, Sodium and Potassium

A

lithium (Li) , sodium (Na), potassium (K)

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28
Q

what are the extra observations of lithium reacting with water

A

fast

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29
Q

what are extra observations of sodium reacting with water

A

faster (than lithium)
Na melts

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30
Q

what are the extra observations of potassium reacting with water

A

fastest (out of it, sodium and lithium)
K melts
lilac flame

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31
Q

what happens to the group 1 metals as you go down the group

A

they get more reactive

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32
Q

what happens when a group 1 metal atom reacts

A

it loses its outer-shell electrons to get a full outer shell

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33
Q

why does losing outer shell electrons and getting a full shell happen more easily down the group of group 1 metals

A
  • atoms get bigger and have more shells
  • the outer-shell electron is further from the nucleus
  • the attraction between the nucleus and the outer-electron is weaker
  • so less energy is needed to break the attraction
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34
Q

what do metals react with steam to produce

A

metal oxide and hydrogen

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35
Q

metal reaction with steam equation

A

metal + steam –> metal oxide + hydrogen

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36
Q

what is a metal and steam reaction usually conducted in

A

a horizontal tube

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37
Q

in a metal and steam reaction what set up inside the horizontal tube

A

wet wool is heated to generate steam for the Mg to react with
the H2 gas product is ignited to safely destroy it

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38
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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39
Q

what do acids react with metals to form

A

a salt and hydrogen gas

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40
Q

acid and metal reaction equation

A

acid + metal –> salt + hydrogen

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41
Q

what happens in an acid and metal reaction

A

a salt compound is formed when H is displaced from the acid

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42
Q

what salt does hydrochloric acid form

A

metal chloride (contains Cl-)

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43
Q

what salt does sulphuric acid form

A

metal sulphate (contains SO4 2-)

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44
Q

what salt does nitric acid form

A

metal nitrate (contains NO 3-)

45
Q

what salt does phosphoric acid form

A

metal phosphate (contains PO4 3-)

46
Q

is sodium (Na +) soluble

A

yes

47
Q

is potassium (K +) soluble

A

yes

48
Q

is ammonium (NH4 +) soluble

A

yes

49
Q

is nitrate (NO3 -) soluble

A

yes

50
Q

is chloride (Cl -)

A

yes - except with Ag + and Pb 2+

51
Q

is sulphate (So4 2-) soluble

A

yes - except with Ca 2+, Ba 2+ and Pb 2+

52
Q

is carbonate (CO3 2-) soluble

A

no - except with Na +, K+ and NH4 +

53
Q

is hydroxide (OH -) soluble

A

no - except with Na +, K+ and Ca 2+

54
Q

is oxide (O 2-) soluble

A

no - except with Na +, K+ and NH4 +)

55
Q

what are the two important observations in an acid and metal reaction

A

the metal disappears
there is fizzing

56
Q

why does the metal disappear in a metal and acid reaction

A

because it is used up in the reaction

57
Q

why is there fizzing in a metal and acid reaction

A

because a gas (hydrogen) is produced

58
Q

what happens to the reaction of a metal and an acid as the reactivity of a metal increases

A

the faster it reacts

59
Q

which metals cannot react with acids and why

A

Au, Ag and Cu
it is not possible because they are less reactive than H so cannot displace it

60
Q

which metals are not allowed to react with acids and why

A

Li, Na and K
reaction with acids is too violent

61
Q

what is the chemical test for hydrogen

A

hydrogen in a test tube
lit splint -> squeaky pop
because the combustion of the hydrogen causes the test tube to resonate

62
Q

what happens in displacement reactions

A

more reactive metals can displace less reactive metals from their compounds

63
Q

what would the equation for the displacement of magnesium from copper from copper suphate

A

magnesium + copper sulphate –> copper + magnesium sulphate

Mg(s) + CuSO4(aq) –> Cu(s) + MgSO4(aq)
grey solid blue solution pink-orange colourless
solid solution

64
Q

what are the two observations to always think about in metal displacement reactions

A

solid colour change
solution colour change

65
Q

what happens to the non-metal part of the compound in a displacement reaction

A

remains unchanged

66
Q

when can a displacement reaction occur

A

if the metal used is more reactive than the metal already in the compound

67
Q

where are most metals found and what as

A

in the Earth’s crust as compounds with oxygen and sulphur
this is because over a long time those metals have reacted with oxygen and sulphur

68
Q

what are ores

A

rocks containing specific metal compounds

69
Q

what does native mean

A

chemically uncombined

70
Q

which elements are too unreactive to combine with oxygen or sulphur

A

gold - Au
silver Ag

71
Q

why don’t native metals need to be chemically extracted

A

they already exist on their own

72
Q

what do metal ores need to be chemically extracted from

A

their compounds

73
Q

what ways can metal ores be chemically extracted

A

1- using electricity
2- carbon extraction

74
Q

what is using electricity for extraction of ores

A

metals more reactive than carbon cannot be displaced by carbon
instead we have to use electricity to break down their ore compounds

75
Q

what is using carbon extraction for ores

A

metals less reactive than carbon can be displaced by carbon

76
Q

what type of reaction is using carbon to displace a metal from its compound

A

a redox reaction

77
Q

what is reduction

A

loss of oxygen

78
Q

what is a reducing agent

A

takes oxygen away from something else

79
Q

what is oxidation

A

gain of oxygen

80
Q

what is oxidising agent

A

gives oxygen to something else

81
Q

what is redox

A

reduction and oxidation in the same reaction

82
Q

what is rusting

A

a chemical process by which iron is oxidised to form rust

83
Q

what is the chemical name for rust

A

hydrated iron(III) oxide

84
Q

what is the word equation for rust

A

iron –> iron(III) oxide –> hydrated iron(III) oxide

85
Q

what is the chemical equation for rust

A

Fe(s) —> Fe2O3(s) —> Fe2O3.xH2O(s)

86
Q

what are the properties of iron

A

grey
shiny
malleable

87
Q

what are the properties of rust - hydrated iron(III) oxide

A

brown
dull
brittle

88
Q

what two substances does rusting require

A

oxygen and water

89
Q

how does rusting happen

A

1- iron is oxidized by oxygen to form iron(III) oxide

Fe has gained oxygen and it has also lost electrons to form Fe 3+ ions - it has been oxidized

2- iron(III) oxide is hydrated by water

90
Q

what methods can prevent rusting

A

using barriers
sacrificial protection
galvanising

91
Q

what is using barriers

A

coating the iron in paint, oil, grease or plastic prevents iron from coming into contact with oxygen or water

this only works as long as the coating is intact - as soon as it breaks rusting happens

92
Q

what barrier would you use for a bike chain or for buckets

A

oil or grease for moving parts such as bike chains
paint or plastic for larger stationary objects such as buckets

93
Q

what is sacrificial protection

A

attach a block of a more reactive metal to the iron
this works by displacing the iron from rust as soon as the rust forms

94
Q

what is the downside to the sacrificial protection

A

the block such as block of magnesium has to be replaced often

95
Q

what is galvanising

A

specifically involves coating the iron in zinc

96
Q

why does galvanising work both ways

A

coating it prevents O2 and H2O from coming into contact with the iron
but even if a crack appears zinc is more reactive than iron so acts as sacrificial protection as well

97
Q

what are alloys

A

mixtures of a metal with one or more other elements, usually other metals or carbon

98
Q

list common alloys

A

steel
brass
bronze

99
Q

elements in steel

A

iron + carbon

100
Q

elements in brass

A

copper + zinc

101
Q

elements in bronze

A

copper + tin

102
Q

why are alloys harder than pure metals

A

because the different-sized atoms/ions prevent the layers of metal ions from sliding over each other which means the alloy is less malleable

103
Q

what is the use of iron and why

A

making steel because it is more useful than iron

104
Q

what is the use of low-carbon steel and why

A

ships, cars, bridges etc
because it is strong but carbon can also be hammered into many shapes

105
Q

what is the use of high-carbon steel and why

A

tools - knives and screwdrivers
because high-carbon so less malleable and stiffer than low-carbon steel

106
Q

what is the use of stainless steel and why

A

cutlery, cooking utensils, kitchen sinks
because Cr forms oxide layer that resists corrosion so stays shiny and clean

107
Q

what is the use of copper and why

A

wires, cooking pans, water pipes
because excellent conductor of electricity, excellent conductor of heat, unreactive and malleable

108
Q

what is the use of aluminiun and why

A

aircraft bodies, power cables
low-density and high strength, low-density and conducts

chemistry all note flashcards - 3rd And 4th (13 decks)

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