Flashcards in C3e Deck (10):
What are the properties of a diamond?
-very high melting point
-doesn't conduct electricity
What is the structure pf a diamond?
-each carbon forms four covalent bonds in a very rigid giant covalent structure making it really hard
-the strong covalent bonds take lots of energy to break, giving diamond an very high melting point
-no free electrons or ions, so no conducting electricity
What is the structure of graphite?
-each carbon atom form three covalent bonds, creating sheets of carbon atoms which are free to slide over each other
-layers held together weakly so they are slippery and can be rubbed off (how pencils work)
-lots of energy needed to break covalent bonds so high melting point
-since only three out of each carbons' four outer electrons are used in bonds, there are lots of delocalised (spare) electrons that can move, conducts electricity
What are the properties of graphite?
-kind of shiny
-rubs off on paper
-high melting point
What are the uses of diamonds and why?
-cutting tool because high melting point and hardness
-jewellery because lustrous
What are the uses of graphite and why?
-pencils as layers are slippery and can be rubbed off
-lubricating material, as slippery
What are giant molecular structures
-usually don't conduct electricity because there aren't any fee electrons (graphite is an exception)
-carbon can form giant molecular structures because it can form lots of covalent bonds with itself
-all the covalent bonds give giant molecular structures strength, high melting point and they do not dissolve in water
What are nanotubes?
-tiny hollow carbon tubes
-huge surface area, so can make great industrial catalysts (individual catalyst molecules cab be attached to the nanotubes)
What are fullerenes?
-molecules of carbon
-shaped like closed tubes or hollow balls
-used to cage other molecules, fullerene structure forms around another atom or molecule which is then trapped inside
-could be a new way of delivering drugs in the body, e.g.slow release