giant covalent molecules

Question 1

What state are giant covalent molecules in room temp, and why?

Answer 1

they are always solid, as they have a high melting and boiling point (millions of strong covalent bonds)

Question 2

what is a diamond formed from

Answer 2

the element carbon

Question 3

how many covalent bonds does each carbon atom form in diamond

Answer 3

4 strong covalent bonds, meaning they have many covalent bonds, meaning they have a high melting and boiling point

Question 4

can diamonds conduct electricity, and why

Answer 4

diamonds cannot conduct electricity, there are no free electrons to carry a charge

Question 5

silicon dixoide is what and waht combined

Answer 5

silicon and oxygen

Question 6

silicon dioxide, all properties

Answer 6

• has a very high melting and boiling point
• huge number of strong covalent bonds must be broken, takes a great deal of energy

Question 7

graphite properties

Answer 7

• 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

Question 8

what does graphite form from, and how many covalent bonds does each element form

Answer 8

• graphite formed from element carbon
• each carbon atom forms 3 covalent bonds

the carbon atoms form hexagonal rings

Question 9

why is graphite slippery

Answer 9

as the hexagonal rings are in layers, and there are no covalent bonds in between them, meaning the layers can slide

Question 10

why is graphite good for conducting heat and electricity

Answer 10

as they have de localised electrons (they can move)

each carbon atom has a single electron thats not in the covalent bond