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Chem > Chap 7 - redox, alloys, metals, properties > Flashcards

Chap 7 - redox, alloys, metals, properties Flashcards

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1
Q

note: oxidation & reduction always go tgt

A
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2
Q

diff. in numbering of oxidation state & ionic

A

oxidation state - +2
ionic - 2+

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3
Q

reduction things

A

-loss of oxygen
-gain of electrons
-gain of hydrogen
-oxidising agent

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4
Q

oxidation things

A

-gain of oxygen
-loss of electrons
-loss of hydrogen
-reducing agent

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5
Q

define spectator ion

A

-ion that doesn’t change in a reaction

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6
Q

OILRIG

A

-Oxidation Is Loss of electrons
-Reduction Is Gain of electrons

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7
Q

ionic half equations

A

-find oxidising & reducing agents
Reactants -> Prodcuts
- _a__ -> ___ + ____e (a is oxidised)
- _a__ + ____e -> _____ (a is reduced)
-electrons in both are the same

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8
Q

rules:

A

-all elements oxidation state = 0 - electrically neutral
-rmb charges for some compounds - eg, SO4 = -2
-H oxidation state = +1
-O2 oxidation state = -2
-a compound oxidation state total = 0

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9
Q

ionic equations

A

-rewrite half equations
-cancel electrons from both sides

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10
Q

magnetic metals

A

-iron
-cobalt
-nickle

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11
Q

define delocalised

A

free to move

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12
Q

define metallic bonding

A

positive metal ions in a sea of delocalised electrons held by electrostatic forces

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13
Q

which bonds have giant lattice structure

A

-metallic bonds
-ionic bonds
-giant covalent bonds

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14
Q

why can metals conduct electricity

A

-delocalised electrons are free to move and carry charge freely through the structure

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15
Q

properties of metal

A

-malleable
-high melting/ boiling point
-good thermal conductivity
-good electrical conductivity
-ductile

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16
Q

which metal has a low boiling point

A

mercury

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17
Q

define malleable

A

bent or hammered into shape

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18
Q

define ductile

A

drawn into wires

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19
Q

why are metals malleable/ ductile

A

-particles are in ordered structure
-layer can slide over each other

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20
Q

define good thermal/ electrical conductivity

A

-can conduct heat/ electricity well

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21
Q

why do metals have good thermal/ electrical conductivity

A

-delocalised electrons can more freely & carry energy/ charge through the structure
-Only energy can be passed by vibrating particles too

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22
Q

define alloy

A

A mixture of a metal with another substance

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23
Q

why an alloy is more useful than the pure metal

A

-it’s harder
-because other element disrupts the lattice structure &
-makes it more difficult to remove the layers form the metal

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24
Q

define brass

A

An alloy of copper and zin

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25
Q

define steel

A

alloy that contains iron and other substances

26
Q

Why is nickel and chromium alloyed with iron

A

Chromium prevents rusting
nickel makes it harder

27
Q

uses of aluminum

A

-manufacture of aircraft - low density
-manufacture of overhead cables - low density, good electrical conductivity
-food containers - resistant to corrosion

28
Q

uses of copper

A

-in electrical wiring - good electrical conductivity

29
Q

reactivity series

A

-Please Stop Calling Me A Cute Zebra, I Like Hot Corn Soup Generally
-Potassium K
-Sodium Na
-Calcium Ca
-Magnesium Mg
-Aluminum Al
-Carbon C
-Zinc Zn
-Iron Fe
-Lead Pb
-Hydrogen H
-Copper Cu
-Silver Ag
-Gold Au
(K over Na because it has more periods)

30
Q

How does the reactivity of a metal relate to how easy it is to extract from its ore

A

-more reactive the metal, more difficult to extract the metal form its ore

31
Q

How does the reactivity of a metal relate to its tendency to form a positive ion

A

-more reactive the metal, easier to lose valance electrons and form positive ions

32
Q

what does hardness in metals mean

A

how easily it scratches

33
Q

how does reactivity series reactive with acid (H+)

A

-K, Na, Ca = produce H2 + vigorous
-Mg to Fe = less reactive as go down
-Cu, Ag & Au = don’t react

34
Q

how does reactivity series reactive with O2

A

-K & Na = burns brightly + vigorous
-Ca & Mg= forms oxide + burns brightly
-Al to Cu = less reactive as go down
-Ag & Au = don’t react

35
Q

how does reactivity series reactive with water (solid & liquid)

A

-K, Na, Ca = react liquid water
-Mg to Fe = react with steam, less reactive as go down
-H to Au = don’t react

36
Q

symbol equation for Mg + HCl with state

A

Mg (s) + 2HCl (aq) → MgCl₂ (aq) + H₂ (g)

37
Q

symbol equation for Mg + O2 with state

A

2Mg (s) + O₂ (g) → MgO (s)

38
Q

symbol equation for Na + cold water with state

A

2Na (s) + 2H₂O (l) → 2NaOH (aq) + H₂O (g)

39
Q

symbol equation for Mg + steam with state

A

Mg (s) + 2H₂O (g) → MgO (s) + H₂ (g)

40
Q

define ore

A

A rock that contains a high enough percentage of metal for economic extraction

41
Q

formula for G1/2 metal + cold water

A

-> _________hydroxide + H2

42
Q

formula for G1/2 metal + steam

A

-> _________oxide + H2

43
Q

word equation for rusting

A

Iron 3 + water + oxygen -> hydrated iron 3 oxide

44
Q

Why is it important that metals are recycled

A

metal ores are finite

45
Q

How are elements above carbon in the reactivity series extracted from their ores

A

Electrolysis

46
Q

How are elements below carbon in the reactivity series extracted from their ores

A

using carbon

47
Q

How is iron extracted from the metal ore hematite in the blast furnace

A

By heating with carbon

48
Q

what type of reaction is rusting

A

oxidation

49
Q

factors that increase rusting

A

-more acid rain, more rust
-more salt, more rust
-need water + O2

50
Q

ways to prevent rusting

A

-painting eg. car bodies
-oiling eg bicycle chains
-coated with a layer of plastic
-greasing eg nuts & bolts

51
Q

define galvanizing

A

coating iron/ steel in a layer of zinc

52
Q

how does galvanizing work

A

-zinc is more reactive & reacts with O2 before iron (sacrificial protection)
-zinc stops O2 from reaching iron underneath

53
Q

define hematite

A

-ore containing iron oxide
-Fe2O3

54
Q

define bauxite

A

-ore containing aluminum oxide
-Al2O3

55
Q

which elements don’t need to be extracted & why

A

-Platinum & Silver
-they’re pure metals

56
Q

3 symbol equations with states for process of extracting iron from hematite

A

-C (s) + O₂ (g) → CO₂ (g)
-C (s)+ CO₂ (g)→ 2CO (g)
-Fe₂O₃ (s) + 3CO (g) → 2Fe (L) + 3CO₂ (g)

57
Q

why limestone (CaCO₃) is used in the blast furnace

A

To remove acidic impurities such as silicon (IV) oxide

58
Q

2 symbol equations for process of removing impurities

A

-CaCO₃ → CaO + CO₂ (thermal decomposition)
-CaO + SiO₂ → CaSiO₃ (slag)

59
Q

uses of mild steel and stainless steel

A

-mild steel for car bodies & machinery
-stainless steel for chemical plants and cutlery

60
Q

Describe and explain the apparent unreactivity of aluminum

A

Aluminum forms an oxide layer which protects the metal underneath

Chem (12 decks)

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