https://padlet.com/beenaramakrishnan/456G 10 G en-us 2017-09-22 11:13:41 UTC 2026-03-10 02:25:38 UTC hello@padlet.com beenaramakrishnan https://padlet.com/beenaramakrishnan/456G/wish/190068793 2017-09-22 11:15:17 UTC https://padlet.com/beenaramakrishnan/456G/wish/190068793 https://padlet.com/beenaramakrishnan/456G/wish/191578600 1. In diamond, each carbon atom is covalently bonded to 4 other carbon atoms. This carbon atoms gives rise to tetrahedral structure. This makes it hard.
 
2. Since the atoms of this carbon gives rise to tetrahedral structure, a lot of energy is needed to separate them this they have a high melting point.

3. Graphite contains delocalised electrons. These electrons are able to move freely and thus are good conductors of electricity. 

The electrons of Diamond on the other hand can't move freely and thus are non conductors. ]]> 2017-09-27 09:26:53 UTC https://padlet.com/beenaramakrishnan/456G/wish/191578600 vikramstablet https://padlet.com/beenaramakrishnan/456G/wish/191578766 1. the various layers of graphite atoms are joined by weak forces, and they can slide over each other.Due to this 'sheet' like structure, graphite is soft to touch, SInce diamond atoms are held by strong forces, it is hard.
2. Since diamond atoms have stronger forces of attraction, breaking it will require a lot of energy.
3. Because graphite has a fourth valence electron free so it can conduct electricity.]]> 2017-09-27 09:27:28 UTC https://padlet.com/beenaramakrishnan/456G/wish/191578766 mailmohammedaman https://padlet.com/beenaramakrishnan/456G/wish/191579014 1. There are stonger covalent bonds between carbon atoms in each layers in diamond.Diamond is harder due to the strong forces holding them.so, the force holding the atoms in graphite is weaker compared to diamond.Therefore, diamond is harder.
2. Graphite is a much better conductor of electricity than diamond due to the mobility of electrons in the outer valence shell..]]> 2017-09-27 09:28:23 UTC https://padlet.com/beenaramakrishnan/456G/wish/191579014 https://padlet.com/beenaramakrishnan/456G/wish/191579059 diamond has a giant molecular structure. Each carbon atom is covalently bonded to four other carbon atoms. 
2, A lot of energy is needed to separate the atoms diamond This is because covalent bonds are strong, and diamond  contains very many covalent bonds. This makes diamonds melting point high.

]]> 2017-09-27 09:28:32 UTC https://padlet.com/beenaramakrishnan/456G/wish/191579059 https://padlet.com/beenaramakrishnan/456G/wish/191579102 1) 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.

2) Diamond has a giant molecular structure. Each carbon atom is covalently bonded to four other carbon atoms. ... This is because covalent bonds are strong, and diamond contains very many 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.]]> 2017-09-27 09:28:42 UTC https://padlet.com/beenaramakrishnan/456G/wish/191579102 https://padlet.com/beenaramakrishnan/456G/wish/191579107 1) Diamond has a more stronger covalent bond than graphite. In diamond crystal is  linked to four other carbon atoms.
2)The compact and rigid three dimensional arrangements of carbon atom gives it a high melting point.
3)Each carbon in graphite is linked to only three atoms and thus conducts electricity but diamond is covalently bonded to four carbon atoms.


]]> 2017-09-27 09:28:43 UTC https://padlet.com/beenaramakrishnan/456G/wish/191579107 https://padlet.com/beenaramakrishnan/456G/wish/191579310 The four surrounding atoms are at the four vertices of a regular tetrahedron. The compact and rigid three dimensional arrangements of carbon atoms gives it a high density.Hence diamond is hard
Graphite is soft because it is lighter than diamond.a graphite consists of layer of carbon atoms or sheets of carbon atoms. Each carbon atom in a graphite layer is jointed to three other carbon atoms by strong covalent bond to form hexagonal rings.since the various sources of carbon atoms are joint by weak forces they can slide over one another .]]> 2017-09-27 09:29:32 UTC https://padlet.com/beenaramakrishnan/456G/wish/191579310 https://padlet.com/beenaramakrishnan/456G/wish/191579367 1) Diamonds atoms are held by strong covalent bonding ,it is hard. Graphite atoms are joined by weak forces ,it is soft .
2) The carbon atoms in diamond are connected to four other atoms ,this increases the strength of bond. thus it has high melting point.
3)Graphite has the fourth cvalance electron free. So it conducts electricity.

]]> 2017-09-27 09:29:43 UTC https://padlet.com/beenaramakrishnan/456G/wish/191579367 https://padlet.com/beenaramakrishnan/456G/wish/191579479 1)The fourth valence electron of carbon is free to move, which reduces the strength of the covalent bond.
2) Diamond has stronger covalent bonds which give it a higher melting point.
3)Graphite has a better conductivity because of its fourth free electron.

]]> 2017-09-27 09:30:09 UTC https://padlet.com/beenaramakrishnan/456G/wish/191579479 https://padlet.com/beenaramakrishnan/456G/wish/191579615  there are strong covalent bonds between carbon atoms in each layer. This allows layers of carbon to slide over each other in graphite ]]> 2017-09-27 09:30:46 UTC https://padlet.com/beenaramakrishnan/456G/wish/191579615 https://padlet.com/beenaramakrishnan/456G/wish/191580320 Nihal vs savitran ]]> 2017-09-27 09:34:27 UTC https://padlet.com/beenaramakrishnan/456G/wish/191580320 https://padlet.com/beenaramakrishnan/456G/wish/191581357 savy babess weds nihalll]]> 2017-09-27 09:39:10 UTC https://padlet.com/beenaramakrishnan/456G/wish/191581357 https://padlet.com/beenaramakrishnan/456G/wish/191591444 2017-09-27 10:23:18 UTC https://padlet.com/beenaramakrishnan/456G/wish/191591444