4.2.1/2/3 Bonding, structure properties of matter (must know) PAPER 1 Part 2 Flashcards
Structure of diamond
Giant lattice of carbon atoms
C atoms are covalently bonded to 4 others
Tetrahedral shape
Why does diamond have a high mtp
Lots of energy needed to break strong covalent bonds throughout giant lattice
Why are diamonds hard
Each C atom covalently bonded to 4 others by strong covalent bonds which stops atoms from moving
Why doesn’t diamond conduct electricity
No delocalised electrons to carry charge throughout the structure
Uses for diamonds
Drill bits
Cutting other diamonds
Structure of graphite
Giant lattice of carbon atoms
C atoms are covalently bonded to 3 others in hexagon layers which are held by weak forces of attraction
Why does graphite have a high mtp
Lots of energy needed to break strong covalent bonds throughout giant lattice
Why is graphite soft
Weak forces of attraction allows layers to slide
Why does graphite conduct electricity
Delocalised electrons carry charge through the structure
Uses for graphite
Pencil ‘lead’ (soft)
Lubricating machinery (slippery)
Electric motor contacts (conducts electricity)
Structure of fullerenes
Linked hexagonal/pentagonal rings of C atoms
Each C atom is bonded to 3 others
Why do fullerenes have low mtps
Little energy is needed to break weak intermolecular forces in the molecular structure
Why do fullerenes conduct electricity
Delocalised electrons carry charge through the structure
Uses of fullerenes
Delivering drugs to where needed in the body
Catalysts
Strengthening materials
Very small electrical circuits
Structure of graphene
One single layer of graphite
Why does graphene conduct electricity
Delocalised electrons carry charge through the structure
Why does graphene have a high mtp
Lots of energy needed to break strong covalent bonds in giant lattice
Why is graphene hard (unlike graphite)
No layers so no weak forces
Only strong covalent bonds
So atoms cannot move/slide
Describe metallic bonding/structure of a metal
A giant lattice of positive metal ions attracted to delocalised electrons
Atoms in metals are arranged in a regular pattern
What is the bonding like in metals
In metals, the outer shells contain delocalised electrons and can move throughout the whole structure
There are strong forces of electrostatic attraction between the positive metal ions and negative electrons. These forces hold the metal structure together
What are the physical properties of metals and why
Malleable - Layers of metal ions are same size and slide over each other
Conduct heat - Delocalised electrons carry energy through the structure
Conduct electricity - Delocalised electrons carry charge through the structure
High mpt/bpt - Lots of energy needed to break strong metallic bonds throughout the giant lattice
What are alloys
A mixture of metals or a metal + a non metal to make it stronger and harder
Why are alloys harder than pure metals
They have atoms of different sizes which will distort the layers of metal atoms, making it harder for them to slide over each other
Limitations of states of matter diagrams
No forces shown
All particles are represented as spheres
The spheres are solid
What do stronger forces between particles mean
The stronger the forces between the particles the higher the melting point and boiling point of the substance.
What does the amount of energy needed to change state depend on
The strength of the forces between the particles of the substance.
How are atoms in polymers linked to eachother
What are the forces between polymer molecules
What state are polymers at room temperature
The atoms in the polymer molecules are linked to other atoms by strong covalent bonds
The intermolecular forces between polymer molecules are relatively strong
These substances are solids at room temperature
Why are metals good conductors of thermal energy
Metals are good conductors of thermal energy because energy is transferred by the delocalised electrons
What do the charges have to equal in ionic compounds
0, they have to cancel eachother out
