Allotropes and Properties of Carbon

This video explores the allotropes of carbon, focusing on diamond, graphite, and buckminsterfullerene. Each allotrope has unique structures and properties. Diamond is hard and non-conductive due to its tetrahedral bonding. Graphite's layered structure allows it to conduct electricity and act as a lubricant. Buckminsterfullerene, with its spherical shape, is slippery and conductive. The video highlights how the arrangement of carbon atoms affects the properties of each allotrope.

What are allotropes?

• Different structures containing the same element

• The same element with identical properties

• Different elements with the same structure

• Different elements with different structures

Which of the following is NOT an allotrope of carbon?

• Diamond

• Quartz

• Graphite

• Buckminsterfullerene

Why is diamond considered very hard and strong?

• Because it has free electrons

• Because of its triangular shape and even weight distribution

• Because it is made of multiple layers

• Because it has a low melting point

Why can't diamond conduct electricity?

• It is arranged in layers

• It lacks free electrons

• It is too hard

• It has a low melting point

What allows graphite to conduct electricity?

• The presence of free electrons

• Its triangular shape

• Its low melting point

• Its hardness

Which property is shared by both graphite and buckminsterfullerene?

• High melting point

• Ability to conduct electricity

• Inability to conduct electricity

• Bonding of each atom to four others