Which is the best reason for the difference between the properties of diamond and graphite?

Laron Walter asked a question: Which is the best reason for the difference between the properties of diamond and graphite?
Asked By: Laron Walter
Date created: Wed, Mar 17, 2021 7:34 PM

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FAQ

Those who are looking for an answer to the question «Which is the best reason for the difference between the properties of diamond and graphite?» often ask the following questions:

👉 What best reason for the difference between the properties of a diamond and graphite?

The difference is simple; they have different atomic structures, or their atoms are arranged differently.

👉 What is the difference between the properties of graphite and diamond?

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.

👉 Difference between the properties of diamonds and graphite?

Some differences between diamond and graphite:

  • different crystalline lattice
  • different aspect
  • graphite is a good electrical conductor, graphite not
  • diamond has a very good thermal conductivity
  • the density of diamond is approx. 3,5 g/cm2 and the density of graphite is 2,15+/- 0,o7 g/cm2
  • the Mohs hardness of diamond is 10; the Mohs hardness of graphite is between 1 and 2

1 other answer

Diamond and graphite are different structural forms of carbon.

Your Answer

We've handpicked 25 related questions for you, similar to «Which is the best reason for the difference between the properties of diamond and graphite?» so you can surely find the answer!

What is the difference between diamond and graphite structure?

Diamond and also graphite are chemically the same, both made up of the element carbon, however, they have entirely different atomic and also crystal frameworks. Diamond atoms have a rigid 3 dimensional structure with each atom carefully loaded with each other as well as connected to 4 other carbon atoms. The factor for the differences in firmness as well as various other physical homes can be ...

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Why graphite and diamond have different properties?

In Diamonds, the atoms are carefully packed with together with each atom connected to various other carbon atoms as compared to Graphite where the bonds in between the layers are weak. Graphite forms flat sheets. Graphite is a lot less thick compared to diamond due to the fact that of the space between the layers.

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Differences between diamond and graphite?

Diamond and graphite are both composed of carbon, but they are physically different from each other. Diamond is the hardest mineral known, is usually transparent and very abrasive. Graphite on the other hand, is soft, opaque and a very good lubricant.

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Differnce between diamond and graphite?

One thing is that diamond is more expensive and more prettier. Diamond is also a really hard mineral, probably the hardest. Graphite is a rock, not a mineral.

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What is the structural difference between a diamond and graphite?

graphite has hexagonal crystals and diamond tetrahedron

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Why do graphite and diamond have different physical properties?

Most physical properties of a solid like hardness, melting point, conductivity of heat/electricity, etc. largely depend on it's crystal structure. Graphite and diamond have very different structures. Graphite has a layered sheet-like structure with each layer consisting of hexagonal rings, this is because all carbon atoms are sp2 hybridised.

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Can the existence of isotopes explain the differences in properties between diamond and graphite?

This explanation is not correct.

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What are the differences between between graphite and diamond?

Graphite and diamond are allotropes of carbon. In other words they're both carbon in different "forms" this difference is represented in thevaryingstructures of the atoms. Specifically, graphite is aspecific structure (layers of atoms) and diamond is formed by face-centered cubic crystals disposed in a diamond type lattice.

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Question: what are the physical properties of diamond and graphite?

Covalent Network Solids are giant covalent substances like diamond, graphite and silicon dioxide (silicon(IV) oxide). Physical Properties of Diamond has a very high melting point (almost 4000°C). is very hard. doesn’t conduct electricity. is insoluble in water and organic solvents. 5 Jun 2019 What are the physical and chemical properties of diamond?

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What is the difference between diamonds and graphite?

They have different structures that make their properties vary

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What is the difference between graphite and diamonds?

difference between graphite and diamond is as follows --Diamond--

  1. It is hard substance.
  2. It is a electric conductor.
  3. Diamond are transparent.
  4. A rare very expensive.
Graphite--
  1. It is a soft substance.
  2. It is a good insulator.
  3. Graphite are opaque.
  4. They are least expensive.

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What are 3 differences between diamond and graphite?

What are three differences between diamond and graphite? Diamond is an electrical insulator while graphite is a good conductor of electricity. Diamond is usually transparent, but graphite is opaque. Diamond is obviously far more valuable than graphite.

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What are three differences between diamond and graphite?

Diamond and also graphite are chemically the same, both made up of the element carbon, however, they have entirely different atomic and also crystal frameworks. Diamond atoms have a rigid 3 dimensional structure with each atom carefully loaded with each other as well as connected to 4 other carbon atoms.

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The marks which make difference between real diamond and false diamond?

There are no 'marks' used to differentiate between real diamonds and fake diamonds.

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Difference between talc and diamond?

A diamond is harder, less abundant in nature and therefore of greater value.

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Why might you expect diamond and graphite to have the same properties?

Diamond and graphite are both allotropes of the base element carbon, and each with different molecular patterns.

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What is the difference between the thermal conductivity and electrical conductivity among graphite and diamond?

Graphite conducts far more electrical conductivity vise versa the diamond conducting far more thermal conductivity. Diamonds are hard. Graphite is soft.

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Why does graphite and diamonds have properties?

Everything has 'properties' used to identify the object/ item/ mineral/ material.

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Difference between gold, platinum and diamond?

Platinum rings also tend to be more expensive than gold because more pure platinum is used in each ring and platinum is a heavy metal. You can have two identical rings – one made of gold and the other of platinum. The platinum ring will weigh more than the gold one and so it will cost more.

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Difference / similarity between kite and diamond?

A Diamond is an elementary term for "Rhombus". It has 4 equal sides. A Kite has two pairs of equal sides that are adjacent to each other. kite can fly diamond can't diamonds are shiny kites are not

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What's the difference between diamond cuts?

Choose the right diamond cut shape. Internationally acclaimed Gemmologist explains in simple terms what is best suited for each individual’s budget and taste, types of diamond cuts and diamond shapes pros and cons.

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Which element makes up a diamond and graphite?

Carbon is the only element necessarily contained in diamond and graphite.

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Which has a greater density graphite or diamond?

Diamond has a greater density than graphite.

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Which has the less density graphite or diamond?

Graphite is less dense than diamond, due to the differences in crystal structure.

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Which is harder a diamond or a graphite?

  • On the Moh s array, Diamond rates as 10 making it the hardest mineral as compared to Graphite, which is the softest. Thus, based upon the physical buildings, they are utilized for various functions. Also, as a result of the rarity, a Diamond is far more expensive than Graphite.

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