Bonding structure and properties of matter

Created by

Lorelie

Cards (61)

When are ions made
when electrons are transferred
What are ions
Charged particles
What happens when metals form ions
They lose electrons from their outer shell to form positive ions
What happens when non metals form ions
They gain electrons into their outer shell to form negative ions
What is ionic bonding
transfer of electrons
Ionic bonding is between
metal and non metal
What is an ionic bond
Oppositely charged ions that are strongly attracted to each other by electrostatic forces
What structure does an ionic compound have
Giant ionic lattice
What are the boiling and melting points of ionic compounds
They have high melting and boiling points
Why do they have high melting and boiling points
There's many strong bonds between the ions and it takes lots of energy to overcome the attraction
Can ionic compounds conduct electricity?
Only when molten or dissolved in solution because when they're solid the ions are held in place but in a liquid they are free to move and carry a current
What does covalent bonding involve
sharing of electrons
What atoms form covalent bonds?
nonmetals and nonmetals
Why are covalent bonds very strong
The positively charged nuclei of the bonded atoms are attracted to the shared pair of electrons by electrostatic forces
Where do atoms share electrons
In their outer shells
What is a simple molecular substance
Atoms joined together by covalent bonds
What are the forces of attraction in a simple molecular substance
Very weak, the covalent bonds in the atoms are very strong but the attraction between the the molecules are weak
Why do they have low melting and boiling points?
Because it doesn't take a lot of energy to overcome the intermolecular forces
Do the conduct electricity
No because there are no free electrons or ions
What is a polymer
Long chain of repeating units
How are the atoms in a polymer joined together
By strong covalent bonds
What are the intermolecular forces in polymers
They're larger than covalent molecules so more energy is needed to brake them
What is a giant covalent structure?
All the atoms are bonded to each other by strong covalent bonds
What are the boiling points of giant covalent structures
They have very high melting and boiling points because lots of energy is needed to break the bonds
Do they conduct electricity?
No they don't contain charged particles they don't conduct electricity (except for graphite).
Describe the structure of diamond
Each carbon atom forms four strong covalent bonds in a very rigid giant covalent structure.
Describe the structure of graphite
Each carbon atom forms three covalent bonds to create layers of hexagons. Each carbon atom also has one delocalised electron.
Describe the structure of silicone dioxide
Giant structure of silicone and oxygen
What are the properties of diamond
Really hard
Very high melting point
Doesn't conduct electricity
Why is graphite soft and slippery?
Graphite is formed in layers, there is no covalent bond between the layers and so the layer can slide over each other making graphite slippery
What can graphite be used for and why?
Lubricating materials because it's slippery
Why does graphite have a high melting point?
The covalent bonds in the layers need loads of energy to break
Why can graphite conduct electricity
One election is delocalised so it can carry a charge
What is graphene
A single layer of graphite
What can graphene be used for?
Can be added to improve strength without adding weight
Why does it have the potential to be used in electronics
It can conduct electricity
What is a fullerene
Molecules of carbon shaped like closed tubes or hollow balls
What are they mainly made up of
Carbon atoms arranged in hexagons or pentagons
What can they be used for and why
They can be used to deliver drugs around the body because they can cage other molecules
They can be used for industrial catalysts because they have a huge surface area and individual catalysts could be attached to them
They make good lubricants
What is a nanotube
hollow cylinder of carbon atoms