Melting and Boiling points - There are many strong bonds throughout the lattice, which need lots of energy to break and so there is a high melting point and boiling points.
Conducting Electricity - When melted or dissolved in water, the ions are free to move around and so can carry a current when a potential is applied.
Hard substances - The many strong bonds throughout the lattice, which each need a lot of energy (e.g.force) to break, which means that the substance is harder and stronger.
Solubility - Water molecules are able to separate the ions from the ionic lattice, so that it breaks apart and the substance dissolves.
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Metallic Bonding
Melting and Boiling points - There is a very strong electrostatic attraction between the delocalised electrons and the cations, so lots of energy is required to break these bonds (except mercury).
Conducting Electricity - The delocalised electrons can move throughout the giant metallic lattice and so can carry a current when a potential is applied.
Conducting Heat - The cations are arranged in a regular arrangement touching each other. Therefore, when heated they vibrate more and their energy is easily passed through the lattice.
Malleable and Ductile - The regular arrangment means that the layers can easily slide over each other when a force is applied.
Insoluble
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Simple Molecular
Low melting and Boiling points - The weak intermolecular forces between molecules means that little energy is needed to overcome these, hence the low melting and boiling points.
Doesn't Conduct Electricity - There are no free electrons because they have NO overall charge.
Insoluble
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Giant Covalent
Diamond ( and Silicon) -
Each Carbon atom forms 4 strong covalent bonds with other atoms to give a tetrahedral structure.
High melting and boiling points - A lot of energy is required to break the many strong bonds, hence the high melting and boiling points.
Hard Substance - The many strong bonds each require a large force to break them.
Doesn't conduct electricity - No free electrons to carry a current when a potential is applied.
Insoluble
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Giant Covalent (Continued)
Graphite
Each Carbon atoms forms 3 strong covalent bonds with other Carbon atoms, resulting in a layered structure.
One spare electron is delocalised between the layers.
The layers are held together by weak intermolecular forces.
High Melting and Boiling points - The many strong bonds require a lot of energy to break, hence the high melting and boiling points.
Soft Substance - Little force is needed to overcome the weak intermolecular forces.
Conducting Electricity - The free delocalised electron is able to carry a current when a potential is applied.
Insoluble
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Giant Covalent (Continued)
Silicon Dioxide
Each Silicon atom is covalently bonded to 4 oxygen atoms in a tetrahedral structure.
High Melting and Boiling Points- Many strong bonds mean that a lot of energy is required to break them, hence the high melting and boiling points.
Hard Substance - There are many strong bonds, therefore a large force is required to break them.
Doesn't Conduct Electricity - There are no free electrons to carry a current when a potential is applied.
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