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Chemistry YR10 > Metals > Flashcards

Metals Flashcards

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1
Q

Metallic bonding?

A

Metallic bonding is the electrostatic force of attraction between a 3 dimensional lattice of positive ions and a sea of delocalised electrons.

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2
Q

Metallic bonding and electrical conductivity?

A

Metals can conduct electricity, because the electrons (negatively charged) are free to move through the structure (delocalised) when pushed by a voltage (electric motive force). They conduct in solid/ liquid form.

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3
Q

Metallic bonding and malleability of metals?

A

Metals are malleable because they are made of hexagonal and cubic packed structures that can be moved by applying force to them. The sliding of ions when force is applied is the reason that metals can change their shapes. The ions in a metal must be moved in order to change the shape of the metal, it is easier for this to be done when it is heated.

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4
Q

Compare ionic and metallic bonding

E.g magnesium oxide and steel

A

Melting points: both high
A lot of energy need to break ionic bonds,
Strong metallic bonds
Crystallinity:
Both
Ionic form a giant lattice
Metallic have a regular lattice structure
Malleability:
Ionic no, metallic yes
Because they are made of + and - atoms that repel when they touch each other
Metallic because they can slide over each other

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5
Q

Alloy?

A

Alloys are mixtures of metals with other substances

E.g brass

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6
Q

Why are alloys used instead of pure metals?

A

Alloys contains ions of different sizes, which distort the regular arrangement of ions in the metal structure. This makes it more difficult for the layers to slide over each other, so alloys are harder than the pure metal.
Copper, gold are to soft for many uses

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7
Q

Changing the properties of iron?

A

Carbon is added to iron to form steel, which is harder that iron because of the distorted arrangments of alloys, disallowing them to slide over each other.

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8
Q

List the physical properties

A

Shiny, sonorous, conducts heat and electricity, malleable, ductile, high melting/ boiling points

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9
Q

Metals react with oxygen?

A

Form metal oxides

Sodium + oxygen — sodium oxide

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10
Q

Some oxide such as nitrogen monoxide

A

Are neutral

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11
Q

Oxides such as zinc oxide

A

Are amphoteric, they react with both acids and bases

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12
Q

Reactive metals react with water to form

A

Metal hydroxides and hydrogen

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13
Q

Reactions with steam and metal

A

Produce metal oxide and hydrogen

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14
Q

Reaction with metals and acid

A

Produce salt and hydrogen

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15
Q

Place in the order of reactivity, most reactive to least reactive

A 
Potassium
Sodium
Calcium
(All of the above react with cold water)
Magnesium
Aluminium
Carbon
( All of the above, their oxides are not displaced by carbon) 
Zinc
Iron
(All of the above React with steam)
(All of the above react with acid)
Hydrogen
Lead
Copper
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16
Q

The reactivity series

A

Is related to the tendency of a metal to form a positive ion, by its displacement reaction or carbon. We heat metal oxides with carbon, to see where that metal would stand in the reactivity series, if the metal is dispatched by carbon it is less reactive than carbon.
E.g burning iron with carbon

17
Q

The reactivity series 2

A

When metals react they become part of a compound, they lose their outer shell electrons to become a positive ions. Therefore the reactivity series lists the metals in order, of the ease with which they become positive ions.

18
Q

Aluminium apparent unreactivity?

A

Aluminium oxide acts as a protective layer for aluminium. It adheres to the metal, causing aluminium to seem unreactive. However once this oxide layer is removed, aluminium reacts quickly with steam or acid for example.

19
Q

What is decomposition?

A

The breaking down of a substance by heat

20
Q

Heat on hydroxides?

A

Thermal decomposition

Most metal hydroxides (except group 1 metals) decompose to form metal oxide and water when heated.
All group 2 hydroxides decompose in a similar way.

21
Q

Most of Group 1 metal hydroxide…

A

Do not decompose, except lithium hydroxide, it is the least reactive of the alkali metals.

22
Q

Most metal nitrates decompose into metal oxides, nitrogen dioxide gas and oxygen gas. Group 1 nitrates….

A

Except lithium which behaves like other nitrates, only decompose as far as the metal nitrate and oxygen.

23
Q

Nitrates are…

A

Very unreactive metals such silver Ag

24
Q

Most metal carbonates decompose to form…

A

Metal oxide and carbon dioxide. Group 1 carbonates do not decompose

25
Q

Limestone calcium carbonate

A

Formula: CaCO3
Uses: making glass and cement, building, making iron, neutralise acid in soil and lakes

Limestone calcium carbonate is decomposed into Quicklime by heat it gives off CO2 as a gas it is an endothermic reaction.

26
Q

Quicklime calcium oxide is a base…

A

Formula: CaO
Uses: neutralising acids soil to make slaked lime
It also neutralises industrial waste products, desulphurisation
If water is added to quicklime calcium oxide, it become Slaked lime calcium hyrdroxide, this is an exothermic reaction. Process called slaking.

27
Q

Slaked lime calcium hydroxide…

A

Formula: Ca(OH)2
Uses: neutralising acids in soil neutralise industrial waste products desulphurisation

28
Q

Oxidising agents are reduced

A

And reducing agents are oxidised during a redox reaction

29
Q

Oxidation is defined as

A

The addition of oxygen to substance

30
Q

Reduction is defined as

A

The removal of oxygen from the substance

31
Q

An oxidising agent is a substance which oxidises another substance during a redox reaction

A

It adds oxygen to the other substance

32
Q

Reducing agent reduces oxygen from another substance

A

It takes away oxygen from another substance

33
Q

During redox reactions electrons are…

A

Transferred from one substance to another

34
Q

Uses of aluminium

A

In the manufacture of aircraft because of its strength and low density
In food containers because of its resistance to corrosion.

35
Q

Uses of copper

A

Electrical wiring and copper saucepans

36
Q

What is mild steel used for?

A

Mild steel is used for car bodies and machinery

37
Q

What is stainless steel useful for?

A

chemical plant and cutlery

Chemistry YR10 (1 decks)

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