Yes its a good conductor
yes
Yes. It does not conduct which means it is an insulator. Silicon Dioxide is a giant covelent bonding which means there are no free electrons.
Because graphite has one free electron that is not involved in bonding. The one delocalized electron can be used to conduct electricity. However silicon carbide is tetrahedrally bonded to 4 carbon atoms. There is not free electrons in the arrangement. With no delocalized electron, silicon carbide is unable to conduct electricity.
Does it have a Photovoltaic affect? Ive seen this in a pdf . Diamond Gives off a charge when rubbed "Carbon" and silicon makes electricity in the sun. So I think the conduct electricity. They however have large resistance to electricity and produce extreme heat eg Atkinson Furnace Carbon electrodes and Silicon used in pc components and electrical devices like resistors.So combining them should conduct electricity Jono
To conduct electricity a substance needs charged particles free to move. Metals have metallic bonding, so they have delocalised electrons free to move. Graphite, a covalent network compound, also has delocalised electrons. Ionic compounds conduct when molten or in solution because the ions break free from the crystal lattice and can move. Since carbon dioxide is covalent molecular bonding, it has neither delocalised electrons or ions, and this lack of charged particles free to move means it does not conduct.
Becuase there is silicon in the gas. Silicon is a form of metal so it would only make sense.
yes
Yes. It does not conduct which means it is an insulator. Silicon Dioxide is a giant covelent bonding which means there are no free electrons.
For a material to conduct electricity , it has to be impure , so for example pure silicon cannot conduct electricity but Silicon chips in computers that are mixed with other things can. So the materials that conduct are charged with little particles that allow the flow of electricityBecause of electrolytes. Or because of the metal something is made of.
Because graphite has one free electron that is not involved in bonding. The one delocalized electron can be used to conduct electricity. However silicon carbide is tetrahedrally bonded to 4 carbon atoms. There is not free electrons in the arrangement. With no delocalized electron, silicon carbide is unable to conduct electricity.
No. Silicon is classed as a semiconductor. Meaning it has a moderate ability to conduct electricity.
yes. For instance graphite or silicon.
it conductz it bettter than hydroelectricity
For a material to conduct electricity , it has to be impure , so for example pure silicon cannot conduct electricity but Silicon chips in computers that are mixed with other things can. So the materials that conduct are charged with little particles that allow the flow of electricityBecause of electrolytes. Or because of the metal something is made of.
yes
currently there is no evidence of this.
To conduct electricity a substance needs charged particles free to move. Metals have metallic bonding, so they have delocalised electrons free to move. Graphite, a covalent network compound, also has delocalised electrons. Ionic compounds conduct when molten or in solution because the ions break free from the crystal lattice and can move. Since carbon dioxide is covalent molecular bonding, it has neither delocalised electrons or ions, and this lack of charged particles free to move means it does not conduct.