C3 - Structure And bonding

Question 1

What do elements form when they react together?

Answer 1

Compounds

Question 2

How does elements form a compound?

Answer 2

By gaining or losing electrons or by sharing them

Question 3

How does the electrons group effect what the elements react with.

Answer 3

Elements only react with the corresponding group. Etc the elements in group 1 react with the elements in group 7.

Question 4

What type of bond is formed by sharing electrons

Answer 4

Covalent bond

Question 5

What type of bond is formed of gaining or losing electrons

Answer 5

Ionic bond

Question 6

When non-metals react with metals which bond do they create

Answer 6

Ionic bonds

Question 7

Why do elements form ions

Answer 7

To achieve the stable electronic structure of a noble gas

Question 8

What happens to the charge of an element when an electron is gained or lost

Answer 8

If an electron is gained. The charge is negative.

If an electron is lost the charge is positive

Question 9

What is the number of electrons which create a full outer shell.

Answer 9

1st shell - 2
2nd shell - 10 (8 in that shell)
3rd shell - 18 (8 in that shell)
And the each shell on has another 8.

Question 10

Which elements gain or lose an electron during ionic bonding

Answer 10

\+ = positive. - = negative
Group 1 form 1+ ions
Group 2 form 2+ ions
Group 3 for,s 3+ ions
Group 4 don't share electrons
Group 5 form 3- ions
Group 6 form 2- ions
Group 7 form 1- ions

Question 11

How are ionic compunds held together

Answer 11

Ionic compounds are held together by strong forces of attraction between their oppositely charged ions. This is called ionic bonding.

Question 12

Why are all ionic compounds solid at room temperature

Answer 12

They have a high melting point because it takes a lot energy to break the many strong ionic bonds, operating in all directions, that hold a giant ionic lattice together.

Question 13

Can ionic compounds conduct electricty

Answer 13

Ionic compunds will conduct electricty when molten or dissolved in water. This is because their ions can then become mobile and can carry charge through liquid.

They only conduct electricty when molten or in a solution not in a solid.

Question 14

What structure are ionic compunds in?

Answer 14

Giant structure of ions arranged in a lattice. The attractive electrostatic forces between the oppositely charged ions act in all directions and are very strong.

Question 15

What bond is formed when two non-metals share pairs of electrons with each other

Answer 15

Covalent bond. Each shared pair of electrons is a covalent bond.

Question 16

Why do elements covalent bond

Answer 16

They share electrons to create a full outer shell. It has to be a pair of electrons.

Question 17

Structure of covalent bonds

Answer 17

Many substances containing covalent bonds consist of simple molecules but some have giant covalent structures

Question 18

What are the melting and boiling points of substances made up of simple molecules

Answer 18

They have low melting and boiling points because the intermolecular forces between them are weak.

Question 19

Can simple molecules conduct electricty?

Answer 19

Simple molecules have no overall charge, so they cannot carry electrical charge. Therefore, substances made of simple molecules do not conduct electricty

Question 20

What are polymers

Answer 20

Polymers are made up of many small reactive molecules that bond to each other to form long chains. The inetrmolecukar forces are relatively high compared to smaller molecules.

Question 21

What are giant covalent structures

Answer 21

Some substances which didn’t have a relatively small number of atoms arranged in simple molecules. They instead form huge networks atoms held together by strong covalent bonds in giant covalent structures

Question 22

Examples of substances with giant covalent structures

Answer 22

Diamond, graphite and silicon dioxide

Question 23

Properties of substances with giant covalent bonds

Answer 23

Very high melting and boiling points
Insoluble in water
Apart from graphite, they are hard and do not conduct electricity

Question 24

Whats the difference between the bonds in graphite and the bonds in diamond?

Answer 24

In graphite there are no covalent bonds between the layers. This means they can slide over each other, making graphite soft and slippery. However, the carbon atoms in diamond have a figid giant covalent structure, making it a very hard substance.

Question 25

Why can graphite conduct electricty and diamonds can’t

Answer 25

Graphite can conduct electricty and thermal energy because of the delocalised electrons that can move along its layers.

Question 26

In which other form does carbon exist

Answer 26

As well as diamond and graphite, carbon also exists as fullerenes, which can form cage-like structures and tubes, based on hexagonal rings.

Question 27

What are fullerenes being used for?

Answer 27

The fullerenes are finding uses as a transport mechanism for drugs to specific sites in the body, as catalysts, and as reinforcement for composite materials.

Question 28

What is graphene and why is it good?

Answer 28

Graphene is a single layer of graphite and so is just one atom thick. Its properties, such as its excellent electrical conductivity, will help create new developments in the electronics industry in the future.

Question 29

How are the atoms in metals arranged?

Answer 29

The atoms in metals are closely packed together and arranged in regular layers.

Question 30

Why are the particles that make up a metal described as positively charged ions?

Answer 30

Metals lose there outer shells which means they have more protons as their outer shell electrons are donated to the delocslised sea of electrons

Question 31

What are delocalosed electrons?

Answer 31

Free-moving electrons within structure

Question 32

What is an alloy

Answer 32

An alloy is a mixture of two or more elements, at least one of which is a metal.

Question 33

What does ductile mean

Answer 33

Stretch out into wires

Question 34

What does maluable mean

Answer 34

Bend it without breaking

Question 35

Why can metals be bent, shaled, and pulled out into wires when forces are applied.

Answer 35

Layers of atoms slide over each other easily

Question 36

Why can metals be bent and shaped?

Answer 36

Metals can be bent and shaped because the layers of atoms (or positively charged ions) in a giant metallic structure can slide over each other.

Question 37

Why are alloys harder than pure metals?

Answer 37

Alloys are harder than pure metals because the regular layers in a pire metal are distorted by atoms of different sizes in an alloy.

Question 38

How do delocalised electrons effect conductivety

Answer 38

Delocalised electrons in metals enable electricity and thermal energy to be transferred through a metal easily.