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What element has 3 substances?
An element is a pure substance it can not be 3 different substances. However some elements can arrange themselves to look like completely different substances. These variations are called "Allotropes" of the element. The element Sulfur forms 30 solid allotropes, more than any other element. The next element to commonly form allotropes is the element Carbon, which forms - Soot (amorphous carbon), Graphite, Diamond, Buckminsterfullerene, Lonsdaleite, Graphine, and Carbon nanotubes.
How is graphite different from other allotrope's of carbon?
The carbon atoms in graphite are arranged in widely spaced layers.
Is quartz an allotrope of carbon?
When an elemnt has more than one form, where the atoms are bonded together differently these forms are called allotrpes. Carbon has a number of allotrpes, the best known are diamond and graphite. Other elements have allotropes such as phosphorus where ther are red phosphorus, white phosphorus black phosphorus and violet phosphorus.
How can diamond and graphite be made out of same substance and be so different?
Diamond and graphite are both forms of carbon atoms, but they have different structures due to the arrangement of these atoms. In a diamond, carbon atoms are strongly bonded in a 3D lattice structure, making it hard and durable. In graphite, carbon atoms are arranged in layers that can easily slide over each other, making it soft and slippery. The difference in bonding and structure results in the distinct properties of diamond and graphite.
How are diamonds and graphites different and the same?
Diamonds and graphite are both made of carbon atoms but have different structures. In diamonds, carbon atoms are arranged in a 3D network of covalent bonds, making it the hardest natural substance. On the other hand, graphite has carbon atoms arranged in layers with weak van der Waals forces between layers, giving it a slippery feel.
How is graphite different from other types of allotropes of carbon?
Graphite consists of layers of carbon atoms arranged in a hexagonal lattice structure, which allows it to have a soft and slippery texture. Other allotropes of carbon, such as diamond, have different arrangements of carbon atoms that make them harder and have different physical properties. Graphene, another allotrope, is a single layer of graphite but has unique electronic properties that make it a promising material for various applications.
Are carbon and graphite same material?
Yes. Graphite is an allotrope of carbon. Allotropes are composed of the same element but the arrangement differs. Diamond and fullerenes are also allotropes of carbon. Allotropes of carbon differ in the arrangement of the carbon atoms. The structure of graphite enables it to be used in pencils (the "lead") and as a lubricant, but the arrangement of carbon in diamond makes it the hardest substance known on the earth.
What is the atomic number of graphite?
'6' Graphite is the commonest allotrope of CARBON. Carbon has Atomic No. (Z) = 6 , and Atomic Mass (Ar) = 12 Other allotropes of carbon are 'Diamond' and 'Buckminster Fullerene(Footballene)'. Allotropes are the same element , exhibiting itself in different physical states, because of the arrangement of the atoms in a sample.
Are carbon and aluminium good conductors of heat?
Aluminium is a good conductor. Carbon, in the form (allotrope) of graphite is a good conductor but its other allotropes are not.
What is the crystal form of Graphite?
Graphite is in the hexagonal crystal system. Graphite is made up of thin layers of the element carbon and is one of the only two allotropes of the element. The other is diamond.
Is one form of carbon a diamond?
Yes. Other allotropes include coal and graphite, such as you might find in a pencil as 'lead'.
What is graphite' s chemical formula?
Graphite is just an allotrope of the element carbon, in that it is carbon in a different form. Graphite exists in a hexagonal planar structure which allows sheets of graphite to slide over each other easily which is what you see when you write; it is also used as a lubricant (though not in a vacuum) The allotropes of Carbon include diamond, graphite and fullerenes.
Which of the following is an example of a carbon allotrope?
There are many allotropes of carbon, some are:Amorphous Carbon (No real structure to speak of)Diamond (Tetrahedral Crystalline Structure)Graphite (Hexagonal 'Graphene' Sheets)C-nanotubes (Cylindrical Graphene)Buckyballs (Spherical Graphene)Note that buckyballs and carbon nanotubes are templates of the 'fullerene family' of carbon allotropes, of which there are many.Another note: Soot is not an allotrope of carbon, it is a collection of particles left from the incomplete combustion of hydrocarbons. Carbon dioxide (CO2) is not an allotrope since it contains oxygen.
What do diamonds graphite and coal have in common?
The are all composed of carbon (although coal commonly also contains other elements such as sulphur).
What are 3 forms of carbon?
Diamond: A form of carbon where carbon atoms are arranged in a rigid lattice structure, making it the hardest known natural material. Graphite: A form of carbon where carbon atoms are arranged in layers that can slide over each other easily, making it a good lubricant. Fullerenes: Molecules composed entirely of carbon, such as buckyballs and carbon nanotubes, that can have unique properties due to their structures.
What element is diamond and your pencil led are made of?
Diamonds are made of carbon atoms bonded in a crystal lattice structure, while pencil lead is comprised mostly of graphite, which is also made of carbon atoms arranged in layers. Both materials are composed primarily of carbon, but their different structures result in distinct properties.
Are carbon and graphite same materialwhy?
Carbon and graphite are not the same material. Graphite is a form of carbon that is made up of layers of carbon atoms arranged in a specific structure that allows for easy movement of electrons, making graphite a good conductor of electricity. Carbon, on the other hand, can exist in various forms such as diamond, amorphous carbon, and graphite, with each form having different physical and chemical properties.
