giant covalent molecules Flashcards
What state are giant covalent molecules in room temp, and why?
they are always solid, as they have a high melting and boiling point (millions of strong covalent bonds)
what is a diamond formed from
the element carbon
how many covalent bonds does each carbon atom form in diamond
4 strong covalent bonds, meaning they have many covalent bonds, meaning they have a high melting and boiling point
can diamonds conduct electricity, and why
diamonds cannot conduct electricity, there are no free electrons to carry a charge
silicon dixoide is what and waht combined
silicon and oxygen
silicon dioxide, all properties
- has a very high melting and boiling point
- huge number of strong covalent bonds must be broken, takes a great deal of energy
graphite properties
- has high melting and boiling point (due to many strong covalent bonds)
- graphite is soft and slippery
-graphite is an excellent conductor of both electricity and of heat
what does graphite form from, and how many covalent bonds does each element form
- graphite formed from element carbon
- each carbon atom forms 3 covalent bonds
the carbon atoms form hexagonal rings
why is graphite slippery
as the hexagonal rings are in layers, and there are no covalent bonds in between them, meaning the layers can slide
why is graphite good for conducting heat and electricity
as they have de localised electrons (they can move)
each carbon atom has a single electron thats not in the covalent bond