<em>Diamond and graphite are allotropes of carbon and have various differences in their physical properties.</em>
Explanation:
<u>Diamond:</u>
- It is crystalline in nature
- Each Each C is
hybridized and forms 4 covalent binds with neighboring C atoms - The geometry is tetrahedral
- C-C bond length is 154 pm
- It has rigid covalent boning which is difficult to break.
- It acts as an electric insulator
<u>Graphite:</u>
-
It has layered structure
- Each C atom is sp2 hybridized and forms 3 sigma bonds with 3 other C atoms. Fourth electron forms pi bond.
-
The geometry is planar
- C-C bond length is 141.5 pm
- It is soft. Its layers can be separated easily
- It is good conductor of electricity.
This is the comparison of the physical properties of two forms of carbon: diamond and graphite
F---atomic number 9---1s2 2s2 2p5 -----7 electrons
<span>Answer: Correct answer is 507g FeCl2 x (1 mol FeCl2 / 126.8 g FeC2) x (1 mol Fe(OH)2 / 1 mol FeCl2) x (89.8 g Fe(OH)2/ 1 mol Fe(OH)2) = 359 g Fe(OH)2.</span>
Answer:
b. upper mantle
Explanation:
low velocity zone of the upper mantle