Bonding of Diamond: Unreactivity & Impurity

In summary, the conversation discusses the 3D structure of a diamond and the presence of a remaining electron in each carbon atom. It also questions the possibility of a diamond with 100% purity.
  • #1
jadelamlam
51
0

Homework Statement


Hi,
there are 2 pictures in the above,pic 2 shows a diamond in rectangular shape.
pic 1 shows the 3D structure of that diamond at a corner of it.
As we know,diamond has a giant covalent structure,which means atoms in it are linked together by covalent bonds only.
Now,please see the pink circle,3 electrons of that carbon atom are covalently bonded to 3 other carbon atoms.
Each carbon atom has 4 outermost electrons.Where is the remaining electron?

Homework Equations





The Attempt at a Solution



Is it forming a covalent bond with another element?(e.g.oxygen in the air)
If not,it should be reactive due to the unbonded electron but in fact diamond is unreactive.
From the above deduction,there is no diamond with 100% purity(i.e.no impurities)?

just a guess :)

Please help,thx :)
 

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  • #2
There is nothing with 100% purity. You can approach to one, like 99.9999...%, but no 100%.
 
  • #3
I don't remember much chemistry, but I have done some programming imaging various 2D / 3D tilings & 3D / 4D lattices as Pascal's Triangle like structures. A suppositional electron?

https://sites.google.com/site/pascalloids/home
 

Related to Bonding of Diamond: Unreactivity & Impurity

1. What makes diamond such a strong and durable material?

Diamond's strength and durability is due to its unique bonding structure. Each carbon atom in a diamond is bonded to four other carbon atoms in a tetrahedral arrangement, creating a strong 3D network structure. This makes it difficult for external forces to break the bonds between the atoms, making diamond one of the hardest materials known.

2. Why is diamond considered unreactive?

Diamond is considered unreactive because of its strong carbon-carbon covalent bonds. These bonds are very difficult to break, meaning that diamond does not easily react with other substances. Additionally, diamond is chemically inert and does not easily undergo chemical reactions or changes in its structure.

3. Can diamond be chemically altered or "impure"?

Yes, diamond can be chemically altered by introducing impurities into its crystal lattice. These impurities can change the color of the diamond or alter its properties, such as making it more conductive or magnetic. However, this process is typically done intentionally and requires high temperatures and pressures.

4. How do impurities affect the bonding of diamond?

Impurities can affect the bonding of diamond by disrupting the regular lattice structure of the carbon atoms. This can weaken the bonds between the atoms and alter the physical and chemical properties of the diamond. For example, introducing boron atoms can create blue diamonds, while nitrogen impurities can create yellow diamonds.

5. Is diamond bonding affected by temperature and pressure?

Yes, diamond bonding is affected by temperature and pressure. High temperatures and pressures can cause the diamond structure to rearrange, which can affect the strength and durability of the bonding. This is why diamonds are typically formed under extreme conditions in the Earth's mantle, and why they can also be created in a laboratory using high pressure and temperature techniques.

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