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 OXIDE2Mg + 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(DIOXIDE)

SIO2 (SILICON DIOXIDE)

HIGH M.P AND B.P

16100c

22300c

CONDUCTIVITY

REACTION WITH WATER?

SILICON CHLORIDE (TETRACHLORIDE)

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

PHOSPHORUS!!

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: 3.16

Electronegativity: 3.44

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

PROPERTIES OF OXIDES: 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+H2O2HClO4

PROPERTIES OF CHLORINE

Chlorine bonds with itself to form Cl2

It has covalent bonds as the electronegativity difference is 0

Cl Cl

Electronegativity: 3.16

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