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6991524
Chemisty Revision
Description
Year 10 Chemistry Mind Map on Chemisty Revision, created by Aimee Russell on 14/11/2016.
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chemistry
year 10
Mind Map by
Aimee Russell
, updated more than 1 year ago
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Created by
Aimee Russell
almost 8 years ago
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Resource summary
Chemisty Revision
Periodic table
Elements
Electons
mass;very small (0.0005)
Charge;negative
location;outer shells
Neutron
Location;inside the nucleus
Charge;neutral
Mass; 1
Protons
Mass; 1
Charge;positive
Location;inside the nucleus
Ordered in atomic mass
Columns going across; groups
Rows going across;periods
Group 0;noble gases
Isotops
Atoms with the same number of protons but different number of neutrons
Maxium number of electrons in each shell;
2,8,8,12
Colvent compounds
Covenlent bonds
Bonds ocurring between non-metals
Electrons shared between atoms
Three different types;
simple molecules(very small)
very low boiling point.
Intermolecluar forces are weak (force between molecules)
Chlorine has a low boiling point as it contains simple covent molecules
Nitrogen has a low boiling point as it contains simple colvent molecules
Giant covelent (giant cluster structures)
Polymers(long, straight lines)
long chains of covalently bound molecules.
Along chains are many weak intermolealur forces
Covalent;sharing metals= always lose electrons.
diamond
Structure;each carbon atoms is bonded to other of their own
Melting points;high melting points because of large repeating structures
Electrical conductivity;Doesn't conduct as all carbon electrons are bonded
Graphite
Structure;each carbon in every layer is bonded to three others.
Between the layers are very weak forces meaning they can slide
Used in pemcils
Melting points;high melting points because of large repeating structures
Electrical conductivity;from free delocalised electron it can conduct
Delocalised=negative
Fullerene
Structure;carbon bonded with three other carbons.
hollow, cage like structure.
Properties;
Used in nanotubes
can be used for drug delivery
Graphene
Structure;one graphite layer
Ion;metal=non-metal=electrostatic
Ionic bonds
Formed by the transfer of electrons to form ions. These are attracted to each other by electronic forces.
Ionic structures
Giant repeating lattices
With strong electostatic forces in all directions
Meaning high melting&Boiling points
Lattices;
When dissolved or molten(melted) the ions can move=create electrons
Higher boiling points from giant repeating lattices with strong electrostatic forces in all directions.
Metallic bonding
losing electrons to gain a full outer shell
Electrons form a 'sea of delocalisation'
flows around the positive metals
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