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Chemistry 3rd form > Metals and reactivity > Flashcards

Metals and reactivity Flashcards

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1
Q

What are the elements in group 1 called

A

The alkali metals

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2
Q

Are metals in group 1 reactive

A

Yes very

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3
Q

How common are group 1 elements

A

Rarely found in nature as pure elements

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4
Q

How many electrons do the alkali metals have in there outer shell s

A

1

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5
Q

What are the characteristics properties of the alkali metals

A

They are soft they have low density they have low melting and boiling points they are good conductors of heat and electricity they are shiny when freshly cut

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6
Q

How are the melting and boiling points affected with alkali metals and why

A

They decrease going down the group for example lithium has a melting point of 181 sodium 98 potassium 64 rubidium 39 caesium 28 this is because as the atoms get larger the attraction between the positive metal ions and the delocalized sea of electrons gets weaker and so the metal becomes easier to melt and boil

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7
Q

How do alkali metals react with oxygen

A

Who alkali metals react with oxygen to form metal oxides this produces a layer of dull oxide on the surface of the metal

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8
Q

How does the speed of the alkali metal reacting with the oxygen compare to where they are on the table

A

The speed increases going down the group

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9
Q

What is the reaction between an alkali metal and oxygen called

A

Oxidation reaction that takes place when an atoms outer electron is lost

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10
Q

What is the word equation for the oxidation reaction between an alkali metal and an oxygen

A

Alkali metal add oxygen arrow alkali metal oxide

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11
Q

What is the ionic equation for the Oxidation of sodium atom

A

Na arrow Na+ + e-

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12
Q

How does a positive ion with a charge of +1 get formed

A

The atom loses one electron

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13
Q

How to all of the alkali metals react with water

A

Vigourously

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14
Q

How do the reactions change as descend down the group 1

A

Does it get more vigourous

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15
Q

What is an exothermic reaction

A

One that releases heat

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16
Q

Is the alkali metals reacting with water an exothermic reaction

A

Yes it produces heat

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17
Q

Why is the group 1 elements called the alkali metals

A

Because the reaction with water creates alkaline hydroxide ions

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18
Q

How does lithium react with water

A

List him is the least reactive when added to water it fishes and moves around slowly across the surface of the water it also produces hydrogen

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19
Q

How does sodium reacts with water

A

When added to water it freezes more than lithium and move quickly across the surface of the water the sodium melts as it reacts and becomes spherical and shiny the hydrogen sometimes catches fire because of the heat from the reaction but not often

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20
Q

How does potassium react with water

A

When added to water potassium is quickly across the surface of the water like sodium it melts with the heat of the reaction reaction produces so much heat the hydrogen catches fire and burns a purple flame

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21
Q

Why does reactivity increase when you go down the group one elements

A

The metal atoms have to lose the outer electrons to form positive ions to react reactivity depends on how easily the electron can be lost the bigger of the atom the more easily electron is lost as the atom gets bigger the outer electron gets further away so it is not so attracted to the nucleus is lost more easily going down the group the atom is bigger

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22
Q

Does lithium float when reacted with water

A

Yes

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23
Q

Is there any energy change when lithium reacts with water

A

Yes gives of heat

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24
Q

Does lithium give off gas when reactive with water

A

Yes

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25
Q

Is there a flame when lithium is reactive of water

A

No

26
Q

Does lithium change the colour of the indicator when reacted to water

A

Yes changes from green to purple

27
Q

When reacted with water does sodium float is there any energy change is gas given off is there a flame and is there any change in the colour of the indicator

A

It does float the energy change is it melts because of the heat is hydrogen gas given off there is sometimes a flame and the indicator changes from green to yellow

28
Q

When potassium reacts with water does it float is there any energy change is gas given off is there a flame and does the indicator colour change

A

It does float the heat and light of energy change hydrogen gas is given off there is always a flame and the indicator changes from green to lilac

29
Q

What happens to calcium when reacted with cold and warm water and cold and warm hydrochloric acid

A

In the cold water it first white and made a pop it would have gone worse reactions from there

30
Q

What happens to iron wool when reacted with cold and warm water and cold and warm hydrochloric acid

A

In the warm hydrochloric acid fizzes gently with a white squeaky pop with the rest it does nothing

31
Q

What happens to zinc when reacted with cold and warm water and cold and warm hydrochloric acid

A

There are tiny bubbles fizzing and a big pop in warm hydrochloric acid in the rest it does nothing

32
Q

What happens to copper when reacted with cold and warm water and cold and warm hydrochloric acid

A

Does nothing in all of them

33
Q

What happens to lead when reacted with cold and warm water and cold and warm hydrochloric acid

A

In warm hydrochloric acid there are slight bubbles in the rest there are no reactions

34
Q

What happens to magnesium when reacted with cold and warm water and cold and warm hydrochloric acid

A

In warm water fizzes gently with no pop in cold hydrochloric acid it reacts vigourously and will react worse in warm hydrochloric acid it does nothing in cold water

35
Q

What does a more reactive metal do to a less reactive metal in a compound

A

It displaces the less reactive mental from the compound

36
Q

What is the reactivity series

A 
Potassium
Sodium
Calcium
Magnesium
Aluminium
Carbon
Zinc
Iron
Tin
Lead
Hydrogen
Copper
Silver
Gold
Platinum
37
Q

How would you extract potassium sodium and aluminium from their ores

A

By electrolysis

38
Q

How would you extract zinc iron and copper from their ores

A

Buy reduction by carbon

39
Q

How would you extract silver and gold from there or

A

Not necessary found pure in the ground

40
Q

What do metals above hydrogen react with and produce

A

They react with water to produce hydrogen

41
Q

What is displacement

A

The metal in a compound is replaced with a more reactive metal to form a new compound e.g. copper sulphate

42
Q

What do you displacement reactions determine

A

Whether one metal is more reactive than another e.g. magnesium is able to displace copper from copper sulphate

43
Q

What is reduction

A

A loss of oxygen

44
Q

What is oxidisation

A

A gain of oxygen

45
Q

What is a redox reaction

A

One in which both oxidation and reduction are occurring

46
Q

In terms of electrons what happens in oxidation

A

Loses electrons

47
Q

In terms of electrons what happens in reduction

A

Gains electrons

48
Q

What is Rust

A

Corrosion of iron

49
Q

When does iron rust

A

It rusts in the presence of oxygen and water

50
Q

What barriers can you use to prevent rust

A

Painting plastic coating covering in oil or grease

51
Q

How else can you prevent rust without using a barrier

A

Alloying
Mixing the iron with chromium and nickel to produce stainless steel prevents rust
Galvanised iron
Coated with a layer of zinc

52
Q

How does galvanisation work

A

Zinc is more reactive than iron so it corrodes instead of the iron

53
Q

What are the 4 main ores

A

Haematite magnetite iron oxide
Malachite copper carbonate
Bauxite aluminium oxide

54
Q

What is bioleaching

A

It is the extraction of specific metals from their ores through the use of bacteria

55
Q

What are three advantages of bioleaching

A

It is very economical as it is simple this makes it cheap it is environmentally friendly unlike traditional methods bioleaching can be used on or is that a poor in quality this is important because high grade ores are limited

56
Q

What are three disadvantages of Bioleaching

A

The process is very slow there are also some toxic chemicals which are harmful to the environment deficiency by which the bacteria convert the copper ore into copper metal is very slow so there is a lot of waste

57
Q

What are the advantages of mining

A

lots of copper can be extracted makes money for the company provides jobs for local people

58
Q

What are the disadvantages of mining

A

Dangerous destroys habitats creates pollution from cars dust and noise smelting releases gases such as SO2 requires energy to extract copper from that or creating carbon dioxide electrolysis uses large amounts of energy only worthwhile extracting high-grade all

59
Q

What are the five stages of phytomining

A

Plants grow in soil containing low-grade all
Copper ions are absorbed by roots and become concentrated in the plant
Copper ions join with oxide ions from the air during burning ash containing copper is reacted with sulphuric acid and then filtered
Electrolysis of the copper sulphate solution produces very pure copper

60
Q

What are the advantages of phytomining

A

Use low-grade copper or requires less energy than smelting produces less air pollution reduces amount of waste rock

61
Q

What are the disadvantages of phytomining

A

Can produce toxic chemicals much slower process electrolysis requires large amounts of electricity

62
Q

What is leachate solution

A

It contains the copper compound is produced by bacteria and is formed when a liquid passes through an organism

Chemistry 3rd form (3 decks)

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