Bonding, structure and properties of matter Flashcards
What are the properties of the three states of matter
Solids:
Have a fixed shape and cannot flow
Can’t be compressed
Liquids:
Flow and take the shape of their container
Can’t be compressed
Gases:
Flow and completely fill their container
Can be compressed
What is the difference between ionic, covalent and metallic bonding
Ionic - metal and non metal
Covalent - two non metals
Metallic - two metals
What are the properties of ionic compounds
High melting point
High boiling point
Can’t conduct electricity (unless it’s melted)
What are the properties of covalent compounds
Low melting point
Low boiling point
Can conduct electricity (delocalised electrons)
What are the properties of giant covalent structures
High melting point
High boiling point
Can’t conduct electricity
What is the structure and bonding and properties and uses of diamond
Structure and bonding:
Each carbon atom is joined to four other carbon atoms by strong covalent bonds
There are no free electrons
Properties and uses:
Very hard
High melting point
Can’t conduct electricity
Cutting tools
What is the structure and bonding and properties and uses of graphite
Structure and bonding:
Each carbon atom forms three covalent bonds with other carbon atoms
The carbon atoms form layers of hexagonal rings
There is one delocalised electron from each atom
Properties and uses:
Conduct electricity
Slippery
Electrodes in batteries
Lubricant
What is graphene and facts about it
A single layer of graphite
High melting point
Strong
Conducts electricity
Can be used for electronics
What are fullerenes and the types of it
Molecules of carbon atoms with hollow shapes
Their structures are based on hexagonal rings of carbon atoms joined by covalent bonds
Some fullerenes include rings with five or seven carbon atoms
Buckminsterfullerene:
Has 60 carbon molecules (C60)
Weak force between molecules
Slippery
Low melting point
Nanotubes:
A layer of graphene rolled into a tube
High tensile strength
Conducts electricity
What are properties of polymers
Large molecules joined by strong covalent bonds
Strong force between particles
High melting point
What are the properties of metals
They are electrical conductors because their delocalised electrons carry electrical charge through the metal
They are good conductors of thermal energy
They have high melting points and boiling points
What is an alloy
A mixture of two or more elements, where at least one element is a metal
What is stainless steel made out of and what is its properties
Chromium and iron
Hard
Doesn’t rust easily
Why is an alloy stronger than a pure metal
The atoms are different sizes. This means that a greater force is required for the layers to slide over each other as the layers are mixed
