NA-SODIUM
Na2O- Sodium Oxide and NaCl- Sodium Chloride
At standard condition- Solid
Bonding and Structure: Ionic lattice
Electrical Conductivity: Good conductor of
electricity in molten state.
MAGNESIUM OXIDE
2Mg + O₂  2MgO
Heating Magnesium in air
Physical State = Solid white powder
• Forms giant ionic lattice and strong ionic bonds hold the ions
together
Conducts electricity when molten
• However, melting point is very high (2850°C)
MAGNESIUM
CHLORIDE
Mg + Cl₂  MgCl₂
Physical State = Solid
• Held together in a giant ionic lattice with strong ionic bonds
Conducts electricity
• Ions dissociate when in molten state
• Melting point is 714°C
OXIDES
AND
CHLORIDES
OF
ALUMINUM
ALUMINIUM OXIDE
(AL₂O₃)
Physical Properties:
Solid under standard conditions, with metallic
properties
Has strong bonds, ionic bonding (ionic lattice)
However, it is more covalent than usual. (All bonds
are covalent to a degree)
NOTE: Aluminium Oxide is amphoteric!
Electrical Conductivity:
When melted, it is a good conductor
Ionic lattice breaks, ions become free flowing
Has free moving charged particles, conducts easily
Ions are held
together tightly
when in an
ionic lattice.
ALUMINIUM
CHLORIDE (AL₂CL₆)
Physical Properties:
Physical property changes depending on the type of bonding
Can either be bonded through an ionic lattice, or a covalent
bond
Empirical formula (AlCl₃), ionic lattice (has a lot of covalent
properties though), is a solid
Aluminium and Chlorine do not have a strong bond
Al₂Cl₆, covalent bond (partly due to polarization).
Sublimes from AlCl₃ to Al₂Cl₆ at 180°C (gas), turns to liquid at
190°C and 2 atmospheric pressure.
Electrical Conductivity:
Electrical conductivity is poor (Al₂Cl₆)
Some electrical conductivity since there is still some ionic
bonding left.
SILICON
BY THEONLYFRANKIE 
SILICON
OXIDE(DIOX
IDE)
SIO2 (SILICON
DIOXIDE)
HIGH M.P AND B.P
16100c
22300c
CONDUCTIVITY
REACTION WITH
WATER?
SILICON
CHLORIDE
(TETRACHLO
RIDE)
SICL4
M.P AND B.P
-70
58
CONDUCTIVITY
WHY LIQUID?
Intermolecular (van der Waals) forces only
SICL4+2H2O --->
SIO2+4HCI
Acidic
React wildly with water (therefore It fumes with moist air)
Product -Hydrogen Chloride
PHOSPHOR
US!!
OXIDES
P4O6 ( Tetraphosphorus hexaoxide)
P4O10 (Tetraphosphorus Decaoxide)
P4O6
Crystalline Solid
One Phosphorus atom bonds with 3 oxygen atoms.
Boiling Point: 173°c
Cant conduct electricity
P4O10
Crystalline Solid
One atom of phosphorus bonds with 3 oxygen atom
Boiling Point: 605°c
Cant conduct electricity
CHLORIDES
PCl3 (Phosphorus Trichloride)
PCl5 ( Phosphorus Pentachloride)
PCL3
Liquid
It has weak Van der Waal force
One atom of phosphorus bonds with 3 chloride atoms
Cant conduct electricity ( covalent bond)
PCL5
Crystalline Solid
Cannot conduct electricity
SULFUR
OXIDES (SO2, SO3)
covalent small gaseous molecules
Physical state is gaseous because covalent bonding has
weak intermolecular forces between the molecules.
Sulfur dioxide does not conduct electricity because covalent
bonding has no charges to produce current.
CHLORIDES (S2CL2)
covalent small liquid molecules
Physical state is liquid because covalent bonding has weak
intermolecular forces between the molecules.
Sulfur chloride does not conduct electricity because covalent
bonding has no charges to produce current.
CHLORINE
PROPERTIES
Oxide:
• Creates Cl20, ClO2, Cl2O6, Cl207
• Creates covalent bonds
• Electronegativity difference between chlorine and oxygen is
0.28
Chloride:
• Only forms Cl2
PROPERTIES OF
OXIDES: BONDING
Covalent bonds are form as the electronegativity difference
is small so it is not polar so there are weak inter molecular
forces
O
Cl
Electronegativity:
3.44
Electronegativity:
3.16
PROPERTIES OF OXIDES:
PHYSICAL STATES
Cl20 and Cl02 are gases as they have weak intermolecular forces
and have a low atomic mass
Cl206 and Cl2O7 are liquids as they have covalent bonds and
have a higher atomic mass
ELECTRICAL
CONDUCTIVITY AND
ACIDITY
In the liquid state they are not electrically conductive as they
do not have freely moving ions.
Chlorine forms an acid when it reacts with water.
Cl207+H2O2HClO4
PROPERTIES OF
CHLORINE
Chlorine bonds with itself to form Cl2
It has covalent bonds as the electronegativity difference is 0
Cl
Electronegativity:
3.16
Cl
Electronegativity:
3.16
BONDING CHANGE
ACROSS PERIOD 3
Group 1 to 3 are ionic bonding
Group 4 to 7 are covalent bonding
Group 4 is giant structure
Group 5 to 7 are small molecules
PHYSICAL STATES
ACROSS PERIOD 3
Group 1 to 5 are solid
Group 6 is gaseous
Group 7 is gas/liquid