Explain why diamond and graphite have such different properties even though they are both composed of carbon.
Explain why diamond and graphite have such different properties even though they are both composed of...
Explain briefly why cellulose and starch have such different properties even though they are both polymers of hexose sugars
Diamond and graphite are both made of carbon. Diamond is an electrical insulator, is the hardest material in the word and is often used as a cutting tool. In drastic contrast, graphite is an excellent electrical conductor, is easy to be cut and is often used as a lubricant at high-temperature mechanical environments. You have learnt the covalent bond, the van der Waals bond and the hexagonal carbon ring. Please explain why the properties of diamond and graphite are so...
Explain why Carbon Dioxide is a gas at room temperature while a diamond is a solid even though they both have covalent bonds.
Explain why different cells can perform different functions even though they have identical organelles
1) Why don't diamonds convert to graphite under ambient pressures, even though diamonds are thermodynamically less stable than graphite?
explain why the molar enthalpy of formation for Carbon Graphite, is 0 kj/mol, while the molar standard enthalpy of formation for carbon diamond, is +1.90 kj/mol and that of carbon gas is +716.7 kj/mol.
Write down the name of each of the compounds. Identify which one is Diamond, Bucky Ball, Graphite, Carbon Nanotube, and Graphene (single layer Graphite) in the following images. Identify how carbon, diamond, and graphite are related. They are enantiomers of carbon. They arc diastereomers of carbon. They are allotropes of carbon. They have the same properties.
Why is the diamond structure unstable with respect to the graphite structure at room ambient atmospheric pressure? Why is significant pressure required to form diamond crystals
Complete the sentences to explain why CO2 and CCl4 are both nonpolar even though they contain polar bonds.zero one two three four linear trigonal planar tetrahedral trigonal pyramidal bonds are only slightly polar sum of the bond dipoles is zero molecules are relatively smallGiven the Lewis structure of CO2, the central carbon atom has lone pair(s) of electrons and total electron groups. Thus the molecular geometry is Given the Lewis structure of CCl4, the central carbon atom has lone pair(s) of electrons and...
47. Explain why CO2 and CCl4 are both nonpolar, even though they contain polar bonds. MISSED THIS? Read Section 11.5; Watch KCV 11.5, IWE 11.5 all bonds usi a. CH Br2 63. Write a hyt