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Which is the best reason for the difference between the properties of diamond and graphite?
Graphite and diamonds are both network covalent carbon chains. The only difference is the structure of each. Graphite is very soft and is used as a lubricant, due to the fact that its carbon atoms are bonded together in layers which slide apart easily. Diamond, however, is very abrasive, because its carbons are all bonded to each other in a very rigid fashion.
What else can I help you with?
A diamond and your pencil lead graphite are made of this same element?
graphite in a pencil and diamond are from carbon .both are the allotrope of carbon
Graphite and diamond are examples of?
Both graphite and diamond are allotropes of carbon.
Do both diamond and graphite have a crystal structure?
Yes. Diamond is isometric, graphite is hexagonal.
What happens to graphite when you change it to diamond?
Graphite's carbon atoms will become more compact, and the density will increase to that of diamond. Both are made of carbon atoms, but different densities. By the way, I am answering the exact same question right now on my chemistry honors homework.
What forms of carbon are the the best lubricant?
Graphite and diamond are two forms of carbon that can act as good lubricants. Graphite is commonly used as a dry lubricant due to its layered structure, which allows for easy sliding between the layers. Diamond can also be used as a lubricant at high pressures and temperatures due to its hardness and low friction properties.
Similarities between Graphite and Fullerenes?
difference between diamond graphite and fullrene
What is the difference between diamond and grapite?
There is none, diamond has about 60 bonds of graphite inside of it.
What are the key differences between the properties of diamond and graphite?
Diamond and graphite are both forms of carbon, but they have different properties. Diamond is a hard, transparent crystal with a high melting point, while graphite is a soft, opaque material with a lower melting point. Diamond has a three-dimensional structure, making it hard and durable, while graphite has a layered structure, allowing it to be used as a lubricant.
Can the existence of isotopes explain the differences in properties between diamond and graphite?
Yes, the differences in properties between diamond and graphite can be explained by the existence of isotopes. Isotopes are atoms of the same element with different numbers of neutrons, which can affect the atomic structure and bonding in materials. In the case of diamond and graphite, the arrangement of carbon atoms and the bonding configuration due to isotopes lead to their distinct properties.
What are the key differences between the diamond structure and graphite, and how do these variances impact their properties and applications?
The key differences between diamond and graphite lie in their atomic structure and bonding. Diamond has a three-dimensional network of carbon atoms bonded together in a tetrahedral arrangement, making it extremely hard and durable. Graphite, on the other hand, consists of layers of carbon atoms arranged in a hexagonal lattice, allowing for easy sliding between layers. This difference in structure results in diamond being hard and transparent, while graphite is soft and opaque. These variances impact their properties and applications, with diamond being used in cutting tools and jewelry due to its hardness, and graphite being used as a lubricant and in pencils due to its slippery nature.
What are the key differences between graphite and diamond in terms of their physical properties and uses?
Graphite and diamond are both forms of carbon, but they have different physical properties and uses. Graphite is soft, opaque, and a good conductor of electricity, while diamond is hard, transparent, and a poor conductor of electricity. Graphite is commonly used in pencils, lubricants, and electrodes, while diamond is used in jewelry, cutting tools, and industrial applications requiring hardness and durability.
What is the structural difference between a diamond and graphite?
The structural difference between diamond and graphite is in their arrangement of carbon atoms. Diamond has a three-dimensional network structure where each carbon atom is bonded to four other carbon atoms in a tetrahedral arrangement. In contrast, graphite consists of layers of carbon atoms arranged in hexagonal rings with each carbon atom bonded to three others in the same plane, allowing for easy slippage between the layers.
What is the difference between Diamonds and graphite?
Diamond and graphite are both pure carbon but graphite's atoms attach to three other carbon atoms and are connected in plates that are parallel to eachother. Diamond's atoms attach to four other carbon atoms in a crystal form, and graphite is a lot softer than diamond.
Differnce between diamond and graphite?
diamonds form a 3 dimensional latice. they also have have four bonds per atom. This makes a very strong material. graphite forms a 2 dimensional latice. it has 3 bonds per atoms (the fourth bond is added to the other three making partial double bonds). it forms sheets. it has excellent 2-d strength: it is what is used in carbon fibers. it also is an excellent lubricant because the sheets slide on one another. fullerenes are like graphite, but the small sheets are wrapped up into small balls or tubes. this gives them 3 d strength on a nano scale. But they lack large scale 3d properties
What are two difference between copper and carbon?
Copper is a metal, while carbon is a non-metal. Copper is a good conductor of electricity, whereas carbon can exist in various allotropes with different properties, such as graphite and diamond.
What is the significance of the graphite-diamond phase diagram in understanding the transformation between these two forms of carbon?
The graphite-diamond phase diagram is important because it shows the conditions under which carbon can transform between graphite and diamond. By studying this diagram, scientists can understand the factors that influence this transformation, such as temperature and pressure. This helps in controlling the production of synthetic diamonds and in exploring the properties of carbon materials.
What element is name of diamond and graphite?
Both diamonds and graphite are allotropes of carbon.
