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PHYSICAL PROPERTIES
- Naturally occuring in the earth's crust in the form of sand.
- Appearence: white/ whitish yellow solid.
- High melting (1650 - 1730 °C) and boiling points, due to the many covalent bonds that must be broken in order to separate the atoms.
- insoluble in water.
- does not conduct electricity because there are no electrons which are free to move (electricity is a flow of electrons).
HYBRADISATION
Silicon Dioxide has an sp3 type of hybradisation due to the four bonds that silicon forms with the oxygen atoms.
DELOCALISATION
There is no delocalisation within the structure due to the fixed position of the electrons which are not free to move. (infact, the molecule doesn't conduct electricity)
BOND ANGLE
Silicon dioxide has a huge variety of structures. Most of them have a tetrahedral shape with a O−Si−O bond angle of 109.5°.
However there are different type of structures due to the  the flexibility of its

Si−O−Si bonds which causes the bonds angle to vary from 100 to 170 degrees.
TYPE OF BONDING
Silicon dioxide has a giant covalent structure. Part of this structure is shown in the diagram - oxygen atoms are shown as white, silicon atoms shown as red: Each silicon atom is covalently bonded to four oxygen atoms. Each oxygen atom is covalently bonded to two silicon atoms.
USES
Silicon dioxide is used in the production of many products such as glass, food additive and raw material for production.

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Physical properties:
- It is colourless and reflects light very well.
- It exists in a tetrahedral arrangement.
- Has a very high melting point of almost 4000°C. The strong covalent bonds must be broken for the melting to occur.
- It's very hard because of the covalent bonds. It's the strongest natural substance in existence.
- It doesn't conduct electricity because the electrons are held tightly between the atoms and aren't free to move.
- It's insoluble in water because no attraction could outweigh the covalent bonds.

It has an sp3 hybridisation.
The bond angle throughout is of 109.5°.
It has sigma bonds.

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3D STRUCTURE

BONDING
The structure consists of five and six membered carbon rings in which each carbon atoms is attached to three other carbon atoms.
The hybridisation at each carbon is sp2 . It has delocalised electrons spread out over the whole structure in one large molecular orbital.

Carbon- sp2 hybridization

Bonded in geodesic shape

60 carbon in spherical - 20 hexagon/ 12 pentagon

1 π electron free to delocalized.

Surface is not planar, but sphere

Electrons NOT able to flow easily.

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Properties:
The C60 molecule is extremely stable, can withstand high temperatures and pressures. The surface of the structure is able react with other species while maintaining the spherical geometry.

The hollow structure is also able to entrap other smaller species such as helium, while at the same time not reacting with the fullerene molecule. In fact the interior of most buckyballs is so spacious, they can encase any element from the periodic table.

Buckyballs do not bond to one another. They do however, stick together via London forces.

By doping fullerenes, they can be electrically insulating, conducting, semiconducting or even superconducting.

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Consists s a single layer of graphite. The carbon atoms are arranged in hexagonal pattern. Is a crystalline allotrope of carbon in two dimensions. Carbon forms three covalent bonds and leaves a free electron in the structure. Is structure is defined as a "honeycomb" lattice. Can be considered a 2D nanomaterial since is only one atom thick
Physical properties of the structure:
-Semi conductur
-High opacity
-High thermal condusctivity
-Stronger material ever tested
-High tensile strength
Explanations of the physical properties:
-The pi bonds hybridized together to form a pi band in which the free electrons are able to move and carry charge.
-The high opacity is due to the low-energy electronic structure
-High tensile strength:the carbon-carbon bonds are short and strong
Bonding information:
-Has three sigma bonds with other carbon atoms and a pi bond orientated out of the plane
-There is an sp2 hybridisation
-Has a planar shape
-Bond angle C-C-C:  120 degrees
-The fourth electron not bonded forms together with the other a series of delocalized electrons

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Just click on the little + at the bottom right to get started .......

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Physical properties of the structure:
-Conducts electricity because of the electrons between the weak bonds that hold the layers of carbon rings that are free to move
-Lubricant, due to the layers of carbo rings that slide one over the other
-High melting point
-slippery
-Black and you cannot see through it
Description of the bonding:
covalent bonding between the carbon atoms.
Carbon makes three sigma bonds, with a trigonal planar shape (bond angle 120°) therefore it has sp2 Hybridisation. This means that it has a p orbital that doesn't make a bond, therefore there are delocalised electrons that overlap above and below the layers. Between the layers, however, the force that is holding them together is just London Force, which is weak and lets the layers slide.