Diamond and Silicon Dioxide

What state are giant covalent molecules in room temperature?

Solid

Giant covalent molecules have ______ melting and boiling points

high

Why does giant covalent molecules have high melting and boiling point?

Because they have millions of strong covalent bonds (in order to melt or boil these substances, we have to break all of these covalent bonds, which requires a lot of energy)

Diamond is formed by

huge number of carbon atoms joined by covalent bonds

In a diamond, each carbon atom forms

4 strong covalent bonds

Diamonds requires a great deal of energy to melt because

they have a huge number of covalent bond which needs to be broken, so it has a very high melting/boiling point

Diamond cannot conduct electricity because

all of the outer electrons are in covalent bonds, so there are no free electrons to carry electrical charge

Silicon dioxide contains the elements

silicon and oxygen covalently bonded together

Silicon dioxide have a _______ melting and boiling point

very high

Why does silicon dioxide have a very high melting and boiling point?

a huge number of strong covalent bonds must be broken which takes a lot of energy