Covalent Bonding Flashcards
What is small molecule bonding?
with a few bonded atoms
What is Giant covalent structures?
Where millions of atoms are joined together
What are the properties of small molecules?
Eg sugar
White crystals
Solid
Low melting point
Solute
Doesn’t conduct electricity
Why do small molecules have a low melting point?
Weak intermolecular forces between the molecules so it takes little energy to break down
Why do small molecules not conduct electricity?
Molecules have no charge so are neutral. The molecules cannot move and conduct electricity.
Why is diamond hard ?
Each carbon is bonded to 4 others so lots of strong bonds
Why does diamond not conduct electirity?
It has no delocalised electrons that can move
Why does diamond have a high melting point?
It has many strong covalent bonds between atoms because each carbon is bonded to 4 others. It needs a lot of energy to break.
Why is graphite soft/ slippery?
The layers can slide over eachother because there are weak forces between the layers
Why can graphite conduct electricity?
It has delocalised electrons that can move through the whole structure
Why does graphite have a high melting point
Graphite has a giant structure with lots of covalent bonds between each atoms. Each carbon is bonded to 3 other carbon atoms. It needs a lot of energy to break these bonds
Why is silicon dioxide hard?
It has a giant structure and lots of strong covalent bonds.
Why does silicon dioxide not conduct electricity?
Has no delocalised electrons that can move
Why does silicon dioxide have a high melting point ?
It has many strong covalent bonds. It needs a lot of energy to break these bonds.
Similarities between graphene and graphite
Both are giant covalent structures
Both made from carbon
Both have carbon bonded to 3 other carbons
Both have delocalised electrons
