Ionic, Metallic, Covalent Bonding

define ionic bonding

the electrostatic attraction between oppositely charged ions

ionic bonding happens between what type of elements?

non-metal + metal

what is the structure for ionic bonding?

giant ionic lattice

why does giant ionic substances have a high melting point?

strong electrostatic attraction between positive + negative ions require a lot of energy to overcome

why are giant ionic substances sometimes insulators?

only when solid as ions are fixed in place in lattice therefore ions can’t move

why are giant ionic substances sometimes conductors?

only when liquid of aqueous as ions are free to move 

define oxidation and reduction in terms of electrons

Oxidation

is

Loss

Reduction

is

Gain

define metallic bonding

electrostatic attraction between positive metal ions + delocalised electrons

metallic bonding happens between what type of elements?

metals

what is the structure for metallic bonding?

• giant metallic lattice 

• rows of positive metal ions

• delocalised electrons 

why are giant metallic substances conductors of electricity?

delocalised electrons are free to move

why are giant metallic substances malleable?

rows of positive ions can slide over each other

what ae alloys?

mixture of a metal and another element

fill in the blank and finish the sentence!

Alloys are ____ than pure metals because…

• harder 

• because : 

  • ions of different size 

  • disrupts the rows of ions

  • harder for the rows to slide over each other

define covalent bonding

electrostatic attraction between shared pairs of electrons and positive nuclei

covalent bonding happens between what type of elements?

non-metals

give 3 examples of giant covalent substances

• diamond

• graphite 

• silicon dioxide

give uses for diamond and graphite 

• diamond = cutting tools

• graphite = solid lubricant

why does diamond have a high melting point?

many strong covalent bonds require a lot of energy to overcome 

why does graphite have a high melting point?

many strong covalent bonds require a lot of energy to overcome

can diamond conduct electricity? Explain!

• non-conductive - diamond can’t conduct

• no delocalised electrons 

can graphite conduct electricity? Explain!

• each carbon atom is bonded to 3 others therefore it has delocalised electrons that can move

• graphite can conduct 

describe the hardness of diamond and explain.

• very hard

• each carbon tom is bonded to 4 others so there are many strong covalent bonds 

describe the hardness of graphite and explain

• soft

• arranged in layers which can slide over each other

what is the structure for simple molecular substances?

simple molecules

why do simple molecules have low boiling point?

weak intermolecular forces require little energy to overcome

explain why simple molecules are electrical insulators

• no ions free to move 

• no delocalised electrons 

compare the melting point of F₂ and I₂

I₂ = bigger molecule therefore stronger intermolecular forces therefore higher melting point

formula for fullerene

C₆₀

why does fullerene have a higher melting point than water?

bigger molecule therefore stronger intermolecular forces therefore higher melting point

use for fullerene 

its hollow so it can be used to transport medicine