C3.10 - Giant metallic structures

Question 1

What can metals be?

Answer 1

Metals can be:

1. Hammered and bent into different shapes
2. Drawn out into wires

Question 2

Why can metals be hammered and bent into different shapes and drawn out into wires?

Answer 2

Metals can be:
1. Hammered and bent into different shapes
2. Drawn out into wires
,because the layers of atoms in a pure metal are able to slide easily over each other

Question 3

How are the atoms in a pure metal, such as iron, held together?

Answer 3

The atoms in a pure metal, such as iron, are held together in a giant metallic structure

Question 4

The atoms in a pure metal, such as iron, are held together in a giant metallic structure.
How are the atoms arranged?

Answer 4

The atoms are arranged in closely packed layers

Question 5

The atoms in a pure metal, such as iron, are held together in a giant metallic structure.
The atoms are arranged in closely packed layers.
What does this regular arrangement allow?

Answer 5

This regular arrangement allows the atoms to slide over one another quite easily

Question 6

Why is pure iron relatively soft and easily bent and shaped?

Answer 6

Pure iron is:
1. Relatively soft
2. Easily bent and shaped
,because the atoms in it are held together in a giant metallic structure

Question 7

Alloy

Answer 7

An alloy is a mixture of:
1. 2
Or
2. More
elements, at least one of which is a metal

Question 8

What are alloys usually?

Answer 8

Alloys are usually mixtures of metals

Question 9

Alloys are usually mixtures of metals.

However, what do most steels contain?

Answer 9

Most steels contain iron with controlled amounts of carbon, a non-metal, mixed into its structure

Question 10

Alloys are usually mixtures of metals.
However, most steels contain iron with controlled amounts of carbon, a non-metal, mixed into its structure.
What are the carbon atoms?

Answer 10

The carbon atoms are a different size to the iron atoms

Question 11

Alloys are usually mixtures of metals.
However, most steels contain iron with controlled amounts of carbon, a non-metal, mixed into its structure.
The carbon atoms are a different size to the iron atoms.
What does this do?

Answer 11

The carbon atoms being a different size to the iron atoms makes it more difficult for the layers in the metal’s giant structure to slide over each other

Question 12

Why are alloys harder than the pure metals used to make them?

Answer 12

Alloys are harder than the pure metals used to make them, because the sizes of the substances in the alloy are different sizes

Question 13

How are the atoms in metals arranged?

Answer 13

The atoms in metals are arranged in layers

Question 14

The atoms in metals are arranged in layers, which can easily slide over each other.
In alloys, why can the layers of atoms not slide so easily?

Answer 14

In alloys, the layers of atoms cannot slide so easily, because atoms of other elements distort the layers

Question 15

Why are metal cooking utensils used all over the world?

Answer 15

Metal cooking utensils are used all over the world, because:

1. Metals are good conductors of thermal energy
2. Most of them have high melting points

Question 16

What are pans usually made of?

Answer 16

Pans are usually made of steel

Question 17

Wherever electricity is generated, what happens?

Answer 17

Wherever electricity is generated, it passes through metal wires to get to where it is needed

Question 18

What does drawing copper out into wires depend on?

Answer 18

Drawing copper out into wires depends on being able to make the layers of metal atoms slide easily over each other, without breaking the metal

Question 19

The positive ions in a metal’s giant structure are bonded to each other by what?

Answer 19

The positive ions in a metal’s giant structure are bonded to each other by a sea of delocalised electrons

Question 20

The positive ions in a metal’s giant structure are bonded to each other by a sea of delocalised electrons.
What are these electrons a bit like?

Answer 20

These electrons are a bit like ‘glue’

Question 21

What do opposite charges do?

Answer 21

Opposite charges attract

Question 22

The positive ions in a metal’s giant structure are bonded to each other by a sea of delocalised electrons.
How are these electrons a bit like ‘glue?’

Answer 22

These electrons are a bit like ‘glue,’ because their negative charge between the positively charged ions holds the metal ions in position by electrostatic forces of attraction

Question 23

The positive ions in a metal’s giant structure are bonded to each other by a sea of delocalised electrons.
These electrons are a bit like ‘glue,’ because their negative charge between the positively charged ions holds the metal ions in position by electrostatic forces of attraction.
However, unlike glue, what happens?

Answer 23

Unlike glue, the electrons are able to move throughout the whole giant lattice

Question 24

The positive ions in a metal’s giant structure are bonded to each other by a sea of delocalised electrons.
These electrons are a bit like ‘glue,’ because their negative charge between the positively charged ions holds the metal ions in position by electrostatic forces of attraction.
Unlike glue, the electrons are able to move throughout the whole giant lattice.
Because the electrons can move around and hold the metal ions together at the same time, the delocalised electrons enable the lattice to do what?

Answer 24

Because the electrons can:
1. Move around
2. Hold the metal ions together at the same time
,the delocalised electrons enable the lattice to distort

Question 25

The positive ions in a metal's giant structure are bonded to each other by a sea of delocalised electrons. These electrons are a bit like 'glue,' because their negative charge between the positively charged ions holds the metal ions in position by electrostatic forces of attraction. Because the electrons can move around and hold the metal ions together at the same time, the delocalised electrons enable the lattice to distort. What happens to the metal atoms when struck?

Answer 25

When struck, the metal atoms can slip past one another without breaking up the metal's structure

Question 26

Because the delocalised electrons in a metal's giant structure can move around and hold the metal ions together at the same time, the delocalised electrons enable the lattice to distort. When struck, the metal atoms can slip past one another without breaking up the metal's structure. The metals are what?

Answer 26

The metals are malleable

Question 27

Malleable

Answer 27

Malleable is when they can be hammered into different shapes without cracking

Question 28

What happens when copper metal is being drawn into wires?

Answer 28

When copper metal is being drawn into wires, the metallic bonding is maintained as layers of metal ions slide over each other

Question 29

When copper metal is being drawn into wires, the metallic bonding is maintained as layers of metal ions slide over each other. The metals are what?

Answer 29

The metals are ductile

Question 30

Ductile

Answer 30

Ductile is when they can be drawn out into wires

Question 31

Why are metals essential in our lives?

Answer 31

Metals are essential in our lives, because the delocalised electrons mean that they are good conductors of both: 1. Thermal energy 2. Electricity

Question 32

How are the high melting points of metals explained?

Answer 32

The high melting points of metals are explained by their giant structures

Question 33

The high melting points of metals are explained by their giant structures. What do the electrostatic forces of attraction do?

Answer 33

The electrostatic forces of attraction extend in all directions

Question 34

The high melting points of metals are explained by their giant structures. Why do the electrostatic forces of attraction extend in all directions?

Answer 34

The electrostatic forces of attraction extend in all directions, because the electrons move freely between the positive metal ions in the giant lattices

Question 35

The high melting points of metals are explained by their giant structures. The electrostatic forces of attraction extend in all directions, because the electrons move freely between the positive metal ions in the giant lattices. What therefore happens?

Answer 35

It therefore takes a lot of energy to: 1. Separate the metal ions from their fixed positions 2. Break down the lattice, melting the metal

Question 36

Why are metals good conductors of thermal energy and electricity?

Answer 36

Metals are good conductors of thermal energy and electricity, because their delocalised electrons can readily flow through the giant metallic lattice

Question 37

The atoms in metals are arranged in layers, which can easily what?

Answer 37

The atoms in metals are arranged in layers, which can easily slide over each other

Question 38

Pans are usually made of steel, but what are also used?

Answer 38

``` Pans are usually made of steel, but: 1. Aluminium Or, 2. Copper are also used ```

Question 39

Steel is alloys of what?

Answer 39

Steel is alloys of iron

Question 40

Wherever electricity is generated, it passes through metal wires, usually made of what, to get to where it is needed?

Answer 40

Wherever electricity is generated, it passes through metal wires, usually made of copper, to get to where it is needed

Question 41

Wherever electricity is generated, it passes through metal wires, usually made of copper, to get to where it is needed, because metals are what?

Answer 41

Wherever electricity is generated, it passes through metal wires, usually made of copper, to get to where it is needed, because metals are good conductors of electricity

Question 42

Metals are good conductors of thermal energy and electricity, because their delocalised electrons can readily flow through the giant metallic lattice. The electrical charge and thermal energy are what?

Answer 42

The: 1. Electrical charge 2. Thermal energy are transferred quickly through the metal by the free-moving delocalised electrons