Bonding, Structure and Properties of Matter Flashcards
What are Ions?
They are Atoms with a Charge
What Ions do Metals make?
Positive ions
What Ions do Non-Metals make?
Negative ions
Atoms with full outer shells are what?
Very stable
What is Ionic bonding?
An electrostatic attractions between oppositely charged ions.
Why are atoms neutral?
Because they have the same number of protons and electrons
What do many ionic compounds form?
salts
What do Ionic Compounds form?
Giant ionic lattice structures where every postie ion is surrounded by every negative ions.
What do Giant ionic lattices have?
They have strong forces electrostatic of attraction between negative and positive charged ions in all directions in the lattice.
Name two Properties of Ionic compounds
Have very high melting and boiling points
Cannot conduct electricity when solids
Why do Ionic compounds have High melting and boiling points?
The strong electrostatic forces require a great deal of energy to break.
Why cant ionic compounds conduct electricity when solids?
This is because ions cannot move and they are locked together in place by strong electrostatic forces forces of attraction.
Why can Ionic compounds conduct electricity when they are dissolved in water or melted?
This is because ions can move freely and carry a charge.
What is a covalent bond?
When non-metals react together to share electrons.
Give an example of a Small covalent bond?
Oxygen
What are the two properties of small covalent bonds?
Have low melting and boiling points
Doesn’t conduct electricity
Why do small covalent bonds have low melting and boiling points?
The weak intermolecular forces between the molecules do not require a lot of energy to break
Do Small covalent bonds have strong Covalent bonds?
Yes
Why can’t small covalent bonds conduct electricity?
This is because the molecules do not have an overall electric charge.
Are small covalent bonds gas at room temperature?
Yes
Name 2 properties of Giant covalent bonds?
Very high melting and boiling points
Don’t conduct electricity
Why do Giant covalent bonds have very high melting and boiling points?
They have millions of strong covalent bonds so a lot of heat energy is required to break the covalent bonds.
Why cant Giant covalent bonds conduct electricity?
This is because the molecules do not have an overall electric charge, not even when they are molten.
Name 3 examples of Giant Covalent bonds.
Diamond, graphite and Silicon dioxide
Are giant Covalent bonds gases or Solids at room temperature?
Always solids at room temperature
What element is Diamond formed from?
Carbon
In diamond how many Covalent bonds are made from one carbon atoms
4 Covalent bonds
Why do diamonds have high melting and boiling points?
They have a huge amount of carbon atoms joined by Covalent bonds which means it requires a lot of energy to break the bonds
Why cant Diamonds conduct electricity?
This is because there are no free electrons to carry a charge.
What elements do Silicon dioxide have?
Silicon and Oxygen which have been Covalently bonded together.
In Silicon dioxide how many Covalent bonds are made from one carbon atoms
One giant structure
What is Silicon dioxide?
Sand is made from it.
In Graphite how many Covalent bonds are made from one carbon atoms
three Covalent bonds .
Name 3 properties of Graphite.
Have melting and boiling points.
It is soft and slippery
Great conductors of heat and electricity
What do the carbon atoms in Graphite form.
Hexagonal rings
Why does Graphite have high melting and boiling points
They have many strong covalent bonds so it takes a great deal of energy to break the bonds.
Why is Graphite slippery?
They have hexagonal rings in layers which have no covalent bonds in between them so they can slide and be slippery.
Why is Graphite great conductors of Electricity and Heat?
They have delocalised electrons that can move.
What is Graphene?
It is a single layer of graphite and is one atom thick.
Name 2 properties of Graphene
Good conductors of electricity.
Extremely strong.
Why are Graphene good conductors of electricity?
Because they have delocalised electrons that can move.
What can Graphene be used for?
It can be added to composite materials to improve strength without adding too much weight.
What are fullerenes?
Molecules of carbon atoms which are shaped like closed tubes or hollow balls.
How are Carbon atoms in fullerenes usually arranged?
In hexagons or sometimes in pentagons(rings of five carbon atoms) or heptagons (rings of 7 carbon atoms)
What was the first fullerene to be Discovered?
Buckministerfullerene
How many carbon atoms do fullerenes contain
60 carbon atoms
Name 2 uses of Fullerenes
Lubricants
Catalysts
Name one group of Fullerenes.
Carbon nanotubes
What are Carbon nanotubes?
Fullerenes shaped into long cylinders.
Name 2 properties of Carbon nanotubes.
Excellent conductors of electricity
have high tensile strength (stretched without breaking)
Name one use of Carbon nanotubes
To reinforce materials like Tennis rackets
What are Polymers?
Are very long molecules of of repeating units joined by strong covalent bonding.
What is it called when scientists draw draw long polymers in a short hand way?
Repeating unit
Are polymers Solids or gases at room temperature?
Solids
Name 2 properties of Polymers.
High melting points
Lower boiling points
Why do Polymers have High melting points?
This is because the Intermolecular forces between each polymer atom are strong so it requires a lot of energy to break the bonds.
What is Metallic bonding?
The bonding between electrostatic attraction between a lattice of positive metal ions and a sea of decoliased electrons
Are metallic bonds weak or strong?
Strong
Why are do Metals have high melting and boiling points?
This is because it requires a lot of energy to break the bonds.
Why are metals good conductors of heat and electricity?
This is because the decoliased electron can move carrying electrical current and heat energy.
Why are metals malleable?
This is because in metals the layers of atoms are able to slide over each other.
What is a Alloy?
a mixture of metals
Why are Alloys harder than pure metals?
The different size of atoms changes the length of the layers making it more difficult for them to slide over each other.
3 Features of Solids?
Fixed shape
Strong forces of attraction
The particles vibrate about their positions
3 Features of Liquids?
Weaker forces of attraction
Fixed volume/ Randomly arranged
No fixed shape
3 features of Gases?
No forces of Attraction
No fixed shape or volume
Move randomly.
If the temperature is below its melting point of a substance is it a solid liquid or gas?
Solid
If the temperature is above the boiling point of a substances is it a liquid solid or gas?
Gas
If the temperature is between its melting and boiling point of a substance is it a solid liquid or gas?
Liquid
