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Ur mom too

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Whereas, in graphite each carbon atom is only bonded to three other atoms. Therefore, there are delocalised (free) electrons in graphite, which can move and carry a charge so graphite conducts electricty

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Each carbon atom is covalently bonded to four other carbon atoms. A lot of energy is needed to separate the atoms in diamond. This is because covalent bonds are strong, and diamond contains very many covalent bonds. This makes diamond's melting point and boiling point very high.

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Diamond and graphite are both giant covalent substances made entirely of carbon atoms. Both have chemical formula , but they do not have a molecular formula.Diamond and graphite are allotropes of carbon. Allotropes are different forms of the same element due to differences in structure.Molecular structureDiamond: Giant covalent structure, with each carbon covalently bonded to four other carbon atoms in a tetrahedral arrangement to form a rigid structure.Graphite: Giant covalent structure, with each carbon covalently bonded to three other carbon atoms in a hexagonal arrangement.HardnessDiamond: Extremely hard. Due to rigid, tetrahedral arrangement of carbon atoms.Graphite: Soft. Layers of hexagonally arranged carbon atoms can slide over one another, as the layers are held together by van der Waals forces of attraction.Melting and boiling pointsDiamond and graphite: Very high. A large amount of energy is required to break numerous, strong covalent bonds between carbon atoms.Electrical conductivityDiamond: Insulator. Mobile electrons are absent. All four valence electrons are used in covalent bonds.Graphite: Conductor. Three out of four valence electrons are used for covalent bonding with other carbon atoms. Remaining valence electrons can be delocalised across the planes of carbon atoms.

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Diamond and graphite are both giant covalent substances made entirely of carbon atoms. Both have chemical formula , but they do not have a molecular formula.Diamond and graphite are allotropes of carbon. Allotropes are different forms of the same element due to differences in structure.Molecular structureDiamond: Giant covalent structure, with each carbon covalently bonded to four other carbon atoms in a tetrahedral arrangement to form a rigid structure.Graphite: Giant covalent structure, with each carbon covalently bonded to three other carbon atoms in a hexagonal arrangement.HardnessDiamond: Extremely hard. Due to rigid, tetrahedral arrangement of carbon atoms.Graphite: Soft. Layers of hexagonally arranged carbon atoms can slide over one another, as the layers are held together by van der Waals forces of attraction.Melting and boiling pointsDiamond and graphite: Very high. A large amount of energy is required to break numerous, strong covalent bonds between carbon atoms.Electrical conductivityDiamond: Insulator. Mobile electrons are absent. All four valence electrons are used in covalent bonds.Graphite: Conductor. Three out of four valence electrons are used for covalent bonding with other carbon atoms. Remaining valence electrons can be delocalised across the planes of carbon atoms.

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1.In diamond, each carbon atom forms 4 covalent bonds in a tetrahedral structure. Whereas, in graphite the carbon atoms only form 3 covalent bonds, creating hexagonally packed sheets of carbon.
2.In diamond each carbon atom is linked to four other carbon atoms by covalent bonds
3.Each carbon atom is bonded into its layer with three strong covalent bonds. This leaves each atom with a spare electron, which together form a delocalised 'sea' of electrons loosely bonding the layers together. These delocalised electrons can all move along together – making graphite a good electrical conductor.

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Each carbon atom is covalently bonded to four other carbon atoms. A lot of energy is needed to separate the atoms in diamond. This is because covalent bonds are strong, and diamond contains very many covalent bonds. This makes diamond's melting point and boiling point very high.

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Diamond is hard since each carbon atom is attached to four other carbon atoms with strong covalent bonds making it very rigid and hard. Whereas in graphite, carbon atoms are attached to only 3 other carbon atoms and are present is layers making it less rigid

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1. The covalent bonds in diamond are really strong. The bonds in graphite, however, are weaker and allow the particles to slide.
2.The structure of diamond is hard and rigid because there are 4 bonds attached. Hence, the energy required to draw these particles away is very high and hence diamond has high MP.
3.Graphite forms a sharing of only 3 electrons. The 4th is free to move. Hence, it conducts electricity. Diamonds share all four electrons. So it cannot conduct electricity.

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While there are strong covalent bonds between carbon atoms in each layer, there are only weak forces between layers. This allows layers of carbon to slide over each other in graphite. On the other hand, in diamond each carbon atom is the same distance to each of its neighboring carbon atoms.

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1.diamond is hard cuz each carbon atom in the diamond crystal is linked to four other carbon atoms by strong covalent bonds.in graphite crystal consists of layers of carbon atoms and each carbon atom in graphite are joined by the week forces.in graphite layers is joined to three other carbon atoms.
3.since diamond is made of carbon atoms only .in graphite the fourth valence electrons of carbon atom is free to move .

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1. Diamond is hard because of its strong covalent bonds which also gives it a high density while graphite has weaker covalent bonds and not all of its valence electrons are not used.

2. It has very strong 3 dimensional covalent bonds.

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Diamond is hard because  In diamond, each carbon atom forms 4 covalent bonds in a tetrahedral structure. ... The sheets of carbon become bonded by weaker intermolecular forces. It is because of these weak intermolecular forces that the layersof graphite can slide over eachother, making the overall substance a lot weaker than diamond

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1. This is because the intramolecular bond between the carbon atoms is very high
2. This is because diamond has   a high intramolecular covalent bond between its constituent carbon atoms.
3. This because diamond does not have my spare electrons, however, graphite atoms have a spare electron  allowing it to conduct electricity

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1)It is connected to 4 other carbon atoms by a strong covalent bond. This compact and rigid 3 dimensional structure gives diamond its high density, which makes it hard. Graphite is soft because of its sheet-like structure. Each layer of carbon atoms in graphite is weakly linked, hence it is softer.

2) The carbon atoms in diamond are joined by covalent bonds, it takes a lot of energy to break these bonds, therefore diamond has a high melting point.

3) In diamond the carbon atoms are bonded to four other atoms. Whereas, in graphite each carbon atom is only bonded to three other atoms. Therefore, there are delocalised (free) electrons in graphite, which can move and carry a charge so graphite conducts electricty.

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Dimond has a strong Coviolent bond and it's structure is a regular tetrahedron and each carbon atom is linked by 4 other carbon atoms
Wihole graphites carbon atoms are lineed only by 3 carbon atoms to for flat hexagonal rings and are formed in layers and the attractive force is lesser than in dimond

Because the force of attraction of the atoms in the dimensions is really high while in graphite it is weak

I think because the 4th valance electron is free to move that why it can conduct electricity

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1.Diamond has strong covalent bonds  with four other carbon atoms. This makes diamond hard.
Graphite atoms are connected in  sheets. Graphite is connected to three other layers in hexaganol rings. They are loosely connected with only three other atoms and can slide over each other which makes graphite soft.
2. Diamond has a high force of attraction and is arranged in a tetrahedral pattern. This is why Carbon Has High Melting point.
3. Graphite contains free electrons which allows it to conduct electricity but diamond doesn't contain free electrons.

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1. There is a strong bond formation in diamond as each carbon atom forms 4 covalent bonds in a tetrahedral structure. Whereas, graphite can slide over each other.
2. This because the dimensional arrangement of carbon atoms in diamond which gives it a high melting point.
3.  Each carbon atom is bonded into its layer with three strong covalent bonds. This leaves each atom with a spare electron, which together form a delocalised 'sea' of electrons loosely bonding the layers together. These delocalised electrons can all move along together – making graphite a good electrical conductor.

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1-diamond is hard because  In diamond, each carbon atom forms 4 covalent bonds in a tetrahedral structure. ... The sheets of carbon become bonded by weaker intermolecular forces. It is because of these weak intermolecular forces that the layersof graphite can slide over eachother, making the overall substance a lot weaker than diamond

2-Each carbon atom is covalently bonded to four other carbon atoms. A lot of energy is needed to separate the atoms in diamond. This is because covalent bonds are strong, and diamond contains very many covalent bonds. This makes diamond's melting point and boiling point very high

3-Graphite is soft and slippery because there are only weak intermolecular forces between its layers. Graphite is a good conductor of heat and electricity. This is because, like metals, graphite contains delocalised electrons. These electrons are free to move through the structure of the graphite

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1.      Explain why, diamond is hard while graphite is soft.

2.      Explain why diamond has a high melting point.

3.      Why is graphite a good conductor of electricity but diamond is a non-conductor of electricity?