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GCSE Chemistry > 4) Extracting Metals & Equilibria > Flashcards

4) Extracting Metals & Equilibria Flashcards

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1
Q

What is the oxidation and reduction acronym?

A

OIL RIG

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2
Q

What does an oxidation reaction involve?

A

Gaining oxyxgen

Losing electrons

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3
Q

What happens when a metal reacts with oxygen?

A

Metal oxides are produced

Magnesium + oxygen –> magnesium oxide

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4
Q

What does a reduction reaction involve?

A

Losing oxygen

Gaining electrongs

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5
Q

What happens when metal oxides lose oxygen?

A

They return to their atomic form

Iron oxide + carbon monoxide –> iron + carbon dioxide

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6
Q

What type of ion do metal atoms always form?

A

Positive cations

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7
Q

What do we call very unreactive metals such as gold and platinum?

A

Native metals

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8
Q

What is the reactivity of a metal linked to?

A

How easy it is to form its positive ion

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9
Q

What happens in a displacement reaction?

A

A more reactive metal displaces a less reactive metal from a compound

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10
Q

What is an example of a redox reaction?

A

Displacement

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11
Q

WHat happens in metal displacement reactions?

A

More reactive metal is oxidised

Less reactive metal is reduced

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12
Q

What do we call ions that do not change in reactions?

A

Spectator ions

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13
Q

What type of reaction has added electrons in the products?

A

Reduction

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14
Q

What type of reaction has added electrons in the reactants?

A

Oxidation

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15
Q

What happens when the alkali metals react with water?

A

A metal hydroxide and hydrogen gas is produced

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16
Q

What happens when potassium reacts with water?

A

Ignites instantly

Sparking and burning with lilac flame

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17
Q

What happens when sodium reacts with water?

A

Fizzes rapidly and melts to form a ball that moves on water’s surface

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18
Q

What happens when lithium reacts with water?

A

Fizzes steadily and floats, becoming smaller until it disappears

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19
Q

How does reactivity change for the alkali metals?

A

Reactivity increases up the group

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20
Q

What metals don’t react with dilute acids?

A

Copper
Silver
Gold
Platinum

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21
Q

What does most metals react with dilute acids to form?

A

Salt

Hydrogen gas

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22
Q

Why is carbon used to extarct metals?

A

High on reactivity series

Cheap and abundant

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23
Q

How is carbon used to extract metals?

A

In the reduction, metal oxide loses oxygen to form a pure metal
Usually metal oxide is heated in presence of carbon uusally in coal form

24
Q

What 5 metals react with dilute acids but not water?

A 
Magnesium
Aluminium
Zinc
Iron
Lead
25
Q

What is phytomining?

A

Extracting copper from contaminated land

26
Q

What is the process of phytomining?

A

1) Plants growing on contaminated land absorb copper ions

2) These plants are harvetsed and burned producing ash containing high concentrations of copper compounds

27
Q

What is a disadvantage of phytomining?

A

Takes longer than other methods

28
Q

What is the process of bioleaching?

A

1) Bacteria are added to low-grade ores
2) Bacteria breaks down ores creatinga solution rich in copper compounds (leachate solution), we can easily extract copper from leachate solution

29
Q

WHat is a disadvantage of bioleaching?

A

Slower than traditional mining

30
Q

What does the process of recycling metals involve?

A

Melting metals before reshaping them

31
Q

Why is recycling metals preferable to mining and extracting new resources?

A

Less energy required
Reduced burning of fossil fuels
Conserves finite resources
Fewer waste rock heaps

32
Q

What do LCAs assess?

A

All 4 stages of a product’s life cycle to calcualte its environmental costs

33
Q

What does LCA stand for?

A

Life Cycle Assessment

34
Q

What are thhe 4 stages of a product’s lifecycle?

A

1) Collecting raw materials needed
2) Making and packaging product
3) Product use
4) Disposal of product

35
Q

What are reversible reactions?

A

When the reactants and products can combine each way

36
Q

What is endo and exothermic reaction’s relation to reversible reactions?

A

If the forward reaction is exothermic, the backwards reaction will be endothermic

37
Q

How much energy is relseased compared to energy absorbed in reversible reactions?

A

Energy relseased is exaclty equal to energy absorbed

38
Q

What is an example of a reversible reaction?

A

The Haber process

39
Q

What is formed in the Haber process?

A

Ammonia through the reaction of nitrogen and hydrogen

40
Q

What temperature and pressure if the Haber process carried out at?

A

450 degrees C with a pressure of 200 atmospheres

41
Q

When does a dynamic equilibrium occur?

A

When reversible reactions happen within a closed system

42
Q

What is a closed system?

A

A system where reactants and products can not be added or removed

43
Q

How does reaction rate and concentration of products and reactants change in a dynamic equilibrium?

A

Equal reaction rate

Concentrations of reactants and products do not change

44
Q

What do the conditions of a reversible reaction deermine?

A

The relative quantities of the different reactants and products in a reaction at equilibrium

45
Q

What does Le Chatelier’s principle state?

A

If any of the conditions of a reversible reaction at equilibrium change, the closed system will counteract whatever has changed

46
Q

What is Le Chatelier’s principle used to predict?

A

The outcome of any changes imposed on a system at equilibrium

47
Q

What does a decrease in temperature cause in equilibrium?

A

The position of equilibrium will shift in the exothermic direction

48
Q

How does a decrease in temperature affect the amount of products and reactants generated?

A

Products generated by exothermic reaction increases

Products generated by endothermic reaction decreases

49
Q

What does an increase in temperature cause in equilibrium?

A

The position of equilibrium will shift in the endothermic direction

50
Q

How does an increase in temperature affect the amount of products and reactants generated?

A

Products generated by endothermic reaction increases

Products generated by exothermic reaction decreases

51
Q

How does an increase in pressure affect the position of equilibrium?

A

Position shifts to favour reaction producing fewest gas molecules

52
Q

How does a decrease in pressure affect the position of equilibrium?

A

Position shifts to favour reaction producing most gas molecules

53
Q

What must be assessed to predict the outcome of a pressure change?

A

Balanced equations to see how many gas molecules are one ach side of the equation

54
Q

How does an increase in concentration of a reactant in equilibrium shift the position?

A

Forward reaction is favoured

Equilibrium position shifts towards products

55
Q

How does an increase in concentration of a product in equilibrium shift the position?

A

Backwards reaction is favoured

Equilibrium position shifts towards reactants

GCSE Chemistry (10 decks)

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