Bonding, structure and properties of matter

Question 1

Describe a solid?

Answer 1

extremely hard to compress, particles are packed together(no spaces) in a regular pattern
Fixed shape, cannot flow but can vibrate

Question 2

What happens when a solid or liquid changes state?

Answer 2

We can change the state by putting in or taking out energy

Melting and freezing takes place at the melting point

Question 3

What happens when liquid goes to gas (vice versa)

Answer 3

strong forces there is a high boiling point

Boiling and condensing takes place at boiling point

Question 4

What is ionic bonding?

Answer 4

Elements have to react in order to get a full outer shell
metal+non-metal=ionic bonding 
ion is an atoms with an overall charge
METAL LOSES AN ION TO FORM + CHARGE
NON-METALGAIN AN ION TO FORM - CHARGE

Question 5

What is the structure of an ionic compound?

Answer 5

Ionic compounds form giant structures where every positive ion is surrounded by a negative ion

Question 6

What is metallic bonding?

Answer 6

Giant structure and regular layers
strong electrostatic attraction between sea of delocalised electrons and positive metal ions
electrons in the outer shell are delocalised

Question 7

What are the properties of metallic bonding?

Answer 7

• high melting and boiling points because lots of energy is required to break the strong metallic bonds
• Layers of atoms can slide over each other so they can be bent and shaped

Question 8

What is an alloy?

Answer 8

mixture of metals
pure metals are to soft to use
in alloys the added elements disturbs the regular pattern of metal atoms so layers do not slide over each other easily
alloys are stronger then pure metals

Question 9

What is a Steel?

Answer 9

steel are alloys of iron containing specific amount of non-metal carbon

Question 10

What is covalent bonding?

Answer 10

Share pair of electrons between atoms covalent bonding takes place between non-metal elements
H-H (single bond)
O=O(double bond)
H2O H-O-H

Question 11

What is a simple molecule?

Answer 11

low melting and boiling points this means they are gases or liquid at room temp
The atoms in each molecule are held by strong covalent bonds

Question 12

What do giant covalent structures do and give an example?

Answer 12

Always solid at room temperature and they have million strong covalent bonds
high melting point
EG. diamond and silicon dioxide and graphite

Question 13

What is graphite made from?

Answer 13

FORM OF CARBON- each carbon atoms forms 3 covalent bonds, form hexagonal rings

Question 14

What is fullerene and give an example?

Answer 14

Molecules of carbon atoms with hollow shapes
hexagonal rings
EG.BUCKMINISTER FULLERENE
CARBON NANOTUBES

Question 15

What is graphene?

Answer 15

single layer of graphite
Extremely strong
Excellent conductor of electricity because it has delocalised electrons

Question 16

What are the properties of polyemrs?

Answer 16

Consist of very large molecules
plastics are made of polymers
atoms within the polymer molecules are held together by strong covalent bonds 
intermolecular forces are strong
solid at room temp

Question 17

What is a liquid?

Answer 17

extremely hard to compress, particles are close together, take the shape of their container and can flow because particles can move

Question 18

Describe a gas?

Answer 18

: easy to compress because particles are widely spaced, gases spread out and fill their container because particles move quickly/randomly

Question 19

How are solids broken?

Answer 19

Liquid has more kinetic energy than solid. Energy is put in to covert the state, the energy is used to break the force of attraction, once broken they move around
STRONGER THE FORCE OF ATTRACTION,MORE ENERGY IS NEEDED TO BREAK PARTICLES,HIGHER MELTING POINT

Question 20

What is the limitations of the particle model?

Answer 20

• All particles are solid sphere(they have different shapes and not solid)
• No forces between particles (forces have an impact on melting/boiling points)

Question 21

What are the properties of ionic bonding?

Answer 21

: high melting/boiling points, strong electrostatic forces require a great deal of heat energy to break

Question 22

Can ionic bonds conduct electricity?

Answer 22

Cannot conduct electricity when solid due to strong electrostatic forces and ions cannot move BUT can conduct electricity when they are molten because the ions can move and carry charge

Question 23

What do giant ionic lattice have?

Answer 23

very strong force of attraction between the positive/negative ions this is called electrostatic forces(ionic bonds)

Question 24

Why are metallic bonds a good conductor and why do they carry thermal energy?

Answer 24

• Good conductors of heat and electricity because of delocalised electrons
• electron carry electric current + carry thermal energy which allows metal to conduct heat

Question 25

Give an example of an alloy?

Answer 25

``` EG. bronze is an alloy of copper and tin Brass is an alloy of copper and zinc Gold is mixed with silver,copper and zinc to form an alloy and is used for coins 24 CARAT GOLD IS 100% GOLD ```

Question 26

What does high/low carbon steel and aluminium alloy make?

Answer 26

High carbon steel- can make chisels low carbon steel-soft, easily shaped and used to make car bodies Aluminium alloys are low density and used to make aeroplanes

Question 27

Why does steal rust what is done to prevent this?

Answer 27

steel can rust because it contains iron to prevent this chromium and nickel is added to make stainless steel which is hard and corrosive resistant

Question 28

How does a simple molecule turn into a gas?

Answer 28

weak intermolecular forces between molecules as temp increases molecules vibrate more and to a certain point were the weak intermolecular force is broken, molecules then turn into a gas

Question 29

Why does a simple molecule not conduct electricity?

Answer 29

do not conduct electricity because molecules do not have an overall electric charge

Question 30

Why does silicon dioxide have a very high melting/boiling point?

Answer 30

Contains silicon and oxygen | Very high melting and boiling point because there are a lot of covalent bonds and this takes a lot of energy to break

Question 31

What is the structure of diamond?

Answer 31

formed from the element carbon | each carbon atoms form four strong covalent bonds with other carbon atoms

Question 32

What are the properties of diamond?

Answer 32

High melting/boiling point covalent bonds are broken when diamond is melted so we need a lot of energy cannot conduct electricity because there's no free electrons to carry charge

Question 33

Why does graphite have high melting/boiling point/Do they conduct electricity?

Answer 33

HIGH MELTING & BOILING POINTS-a lot of energy is needed to break bonds CONDUCTORS OF HEAT AND ELECTRCITY-Delocalised electrons between layers

Question 34

Can layers of graphite slide?

Answer 34

SOFT AND SLIPPERY-arranged in layers and there's no covalent bond between the layers so they can slide

Question 35

What are the properties of Buckminster fullerene?

Answer 35

contains 60 carbon atoms Can be used as lubricant and catalyst joined together as hexagons or pentagons

Question 36

What are the properties of carbon nanotubes?

Answer 36

High tensile strength (stretched without breaking) cylindrical excellent conductors of heat and electricity