Chapter 2 - Bonding Structure And Properties Of Matter

Question 1

How are ions made?

Answer 1

When electrons are transferred

Question 2

Why do atoms gain or lose electrons?

Answer 2

To get a full outer shell

Atoms with a full outer shell are very stable

Question 3

What happens when metals form ions and non metals?

Answer 3

Metals- lose electrons, positive ions

Non-metals- gain electrons, negative ions

Question 4

What groups are most likely to form ions?

Answer 4

1&2

6&7

Question 5

What type of ions will metals form?

Answer 5

Cations

Question 6

What type of ions will non metals form?

Answer 6

Anions

Question 7

What charge will ions from groups 1,2&6,7 form?

Answer 7

1- 1+
2- 2+
6- 6-
7- 7-

Question 8

What are the three type of bonding?

Answer 8

Ionic
Covalent
Metallic

Question 9

Describe what happens during ionic bonding

Answer 9

When a metal and a non-metal react together the metal atom loses electrons to form a positively charged ion and a non-metal gains these electrons to form negatively charged ions. These opposite be charged ions are strongly attached to one another by electrostatic forces. This is called an ionic bond

Question 10

How can we show how ionic compounds are formed?

Answer 10

Dot and cross diagrams

However, they don’t show the structure of the compound, the size of the ions or how they’re arranged

Question 11

What type of structure do Ionic compounds have?

Answer 11

Giant ionic lattice- the ions form a closely packed regular lattice arrangement and there are very strong electrostatic forces of attraction between oppositely charged ions in all directions of the lattice.

Question 12

What are the properties of ionic compounds?

Answer 12

High melting points due to strong bonds between the ions
High boiling points due to strong bonds between the ions

When a solid, the ions are held in place so the compounds cant conduct electricity. When ionic compounds melt, the ions are free to move and they’ll carry electric current

They dissolve easily in water. The ions separate and are free to move in the solution, so they’ll carry electric current.

Question 13

How do you work out the empirical formula?

Answer 13

1) Look at the diagram to work out what ions are in the compound
2) Work out the charges the ions will form
3) Balance the charges to the charge of the empirical formula is zero

Question 14

What are covalent bonds?

Answer 14

When non metal atoms bond together they share pairs of electrons to male covalent bonds.
The positively charged nuclei of the bonded atoms are attracted to the shared pair of electrons by electrostatic forces making covalent bonds very strong.

Question 15

How many electrons are shared in covalent bonding

Answer 15

Each single covalent bond Provides one extra shared electrons for each atom

Each atom involved generally makes enough covalent bonds to fill up its outer shell. Having a full outer shell makes them very stable

Question 16

What can use to draw covalent bonds

Answer 16

You can use the dot and cross diagram to show the bonding covalent compounds Electrons drawn in the overlap between the outer orbitals of two atoms are shared between those atoms

The displayed formula shows the covalent bonds as single lines between atoms

The 3-D model shows the atoms, the covalent bonds and the arrangement in space next to each other

Question 17

What are simple molecular substances

Answer 17

Simple molecular substances are made up of molecules containing a few atoms joined together by covalent bonds

Question 18

What are some examples of simple molecular substances

Answer 18

Hydrogen
Chlorine
Nitrogen
Oxygen
Methane
Water
Hydrogen chloride

Question 19

What are the properties of simple molecular substances

Answer 19

The atoms within the molecules are held together by very strong covalent bonds. In contrast, the forces of attraction between the molecules are very weak

To melt or Boil a simple molecular compound you only need to break this feeble intermolecular forces and not the covalent bonds. This means that melting and boiling points are very low because the molecules are easily parted from each other

Most molecular substances or gases or liquids at room temperature

As molecules get bigger, the strength of the intermolecular forces increases some more energy is needed to break them and the melting or boiling points increase

Simple molecular substances don’t conduct electricity simply because they aren’t charged so there are no free electrons or ions

Question 20

What are polymers

Answer 20

Polymers a long chains of repeating units. Lots of small units are linked together to form a long molecule that has repeating sections. All the atoms in a polymer are joined by strong covalent bonds

Question 21

How do you find the molecular formula of a polymer

Answer 21

Write down the molecular formula of repeating unit in brackets and put an ‘n’ outside

Question 22

What are the properties of a polymer

Answer 22

The intermolecular forces between polymer molecules are larger than between simple covalent molecules so more energy is needed to break them. This means most polymers are solid at room temperature

The intermolecular forces are still weaker than ionic or covalent bonds so they generally have lower boiling points then Ionic or giant molecular compounds

Question 23

In giant covalent structures what are all the atoms bonded to each other by

Answer 23

All the atoms are bonded to each other by strong covalent bonds

Question 24

What are the properties of Giant covalent structures?

Answer 24

They have very high melting and boiling points as lots of energy is needed to break the covalent bonds between the atoms

They don’t contain charge particles they don’t conduct electricity

Question 25

What are some examples of giant covalent structures

Answer 25

Diamond- rigid covalent structure
Graphite- layers of hexagons
Silicone dioxide- one giant structure

Question 26

What are allotropes

Answer 26

Allotropes of different structural forms of the same element in the same physical state

Question 27

What are some allotropes of carbon

Answer 27

Diamonds
Graphite
Graphene

Question 28

Describe the properties of diamond

Answer 28

Giant covalent structure made up of carbon atoms that each form for covalent bonds making diamonds really hard

Strong covalent bonds take a lot of energy to break. Gives diamond a very high melting point

Doesn’t conduct electricity

Question 29

Describe the properties of graphite

Answer 29

Each carbon atom only forms three covalent bonds

There aren’t any covalent bonds between the layers

Graphite is soft and slippery so is ideal as a lubricating material

Has a high melting point. Need a lot of energy to break

Graphite conducts electricity and thermal energy

Question 30

What are fullerenes

Answer 30

Fullerenes on molecules of carbon shaped like closed tubes or hollow balls

They are mainly made up of carbon atoms are arranged in hexagons, but can also contain pentagons.

Question 31

What does metallic bonding involve

Answer 31

Metallic bonding involves delocalised electrons

The electrons in the outer shell of the metal atoms are delocalised which means they are free to move around. There are strong forces of electrostatic attraction between the positive metal ions and shared negative electrons

Question 32

What structure do metals consist of

Answer 32

A giant structure

Question 33

Do compounds with metallic bonds usually have high or low melting and boiling points. Wine?

Answer 33

Electrostatic forces between the metal atoms and the delocalised the electrons are very strong and need lots of energy to be broken.

This means that most compounds with metallic bonds have very high melting and boiling points

Question 34

Why are metals good conductors of heat and electricity

Answer 34

The delocalised electrons carry electrical current and thermal energy through the whole structure

Question 35

What does it mean if most metals are malleable?

Answer 35

It means that they can be bent or hammered all rolled into flat sheets

Question 36

What is an alloy

Answer 36

And alloy is a mixture of two or more metals

Question 37

Why do we use alloys

Answer 37

Pure metals often aren’t quite right for certain jobs. They are often too soft

Question 38

Why does mixing metals make them harder

Answer 38

Different elements have different sized atoms. So when another element is mixed with a pure metal the new metal atoms will distort the layers of metal atoms, making it more difficult for them to slide over each other

Question 39

What does aqueous mean

Answer 39

Dissolved in water