Section 1 – pg 292 Properties of Carbon Chapter 8 Section 1 – pg 292 Properties of Carbon

Carbon Atoms and Bonding Pg 293 Carbon Atoms and Bonding Carbon: atomic number of 6 meaning it has 6 protons and 6 electrons – 4 valence electrons Carbon shares its electrons to form covalent bonds B/c of its unique ability to combine in many ways with itself and other elements, carbon has a central role in the chemistry of living organisms

Pg 294 Forms of Pure Carbon Because carbon can bond in so many ways, the pure element can exist in different forms Diamonds, graphite, fullerenes, and nanotubes are four forms of the element carbon

Pg 294 Diamond Diamond: a crystalline form of carbon in which each carbon atom is bonded strongly to four other carbon atoms Extremely hard and non reactive Industrial chemists are able to make diamonds in the labs but they are not considered beautiful enough to be used in jewelry Diamonds work well in cutting tools, such as drills

Pg 294 Graphite Graphite: each carbon atom is bonded tightly to three other carbon atoms in flat layers The bonds between atoms in different layers are very weak, so layers slide past one another easily

The loosely connected layers makes graphite slippery Pg 294 The loosely connected layers makes graphite slippery Is often used as a lubricant in machines because it reduces the friction between the moving parts

Fullerenes Pg 295 Made in 1985 by scientists Named after architect Buckminster Fuller who designed dome-shaped buildings Consists of carbon atoms arranged in the shape of a hollow sphere Buckyballs are a type of fullerenes

Nanotubes Pg 295 Made in 1991 by scientists Carbon atoms are arranged in the shape of long, hollow cylinder Tiny, light, flexible and extremely strong Good conductors of electricity and heat Used as conductors in electronic devices and as super-strong cables

Chapter 8 Section 1 Homework – pg 295

1A. How many bonds can a carbon atom form?

1B. Why is carbon unique among the elements?

2A. List the four forms of pure carbon

2B. Describe the carbon bonds in graphite

2C. How do the differences in carbon bonds explain why graphite and diamonds have different properties?