1. 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.

2. 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)

3. 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

4. Oxides and Chlorides of Aluminum

5. 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!

6. 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.

7. 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.

8. Electrical Conductivity: Electrical conductivity is poor (Al₂Cl₆) Some electrical conductivity since there is still some ionic bonding left.

9. Silicon
By TheOnlyFrankie 

11. Silicon Oxide(Dioxide)

12. SiO2 (silicon dioxide)

13. HIGH M.P and B.P
16100c 22300c

14. Conductivity

15. Reaction with Water?

16. Silicon Chloride (Tetrachloride)

17. SiCl4

18. M.P and B.P
-70 58

19. Conductivity

20. Why Liquid?
Intermolecular (van der Waals) forces only

21. SiCl4+2H2O ---> SiO2+4HCI
Acidic React wildly with water (therefore It fumes with moist air) Product -Hydrogen Chloride

22. Phosphorus!!

23. Oxides
P4O6 ( Tetraphosphorus hexaoxide) P4O10 (Tetraphosphorus Decaoxide)

24. P4O6
Crystalline Solid One Phosphorus atom bonds with 3 oxygen atoms. Boiling Point: 173°c Cant conduct electricity

25. P4O10
Crystalline Solid One atom of phosphorus bonds with 3 oxygen atom Boiling Point: 605°c Cant conduct electricity

26. Chlorides
PCl3 (Phosphorus Trichloride) PCl5 ( Phosphorus Pentachloride)

27. PCL3
Liquid It has weak Van der Waal force One atom of phosphorus bonds with 3 chloride atoms Cant conduct electricity ( covalent bond)

28. PCl5
Crystalline Solid Cannot conduct electricity

29. Sulfur

30. 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.

31. 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.

32. Chlorine properties Oxide: Creates Cl20, ClO2, Cl2O6, Cl207
Creates covalent bonds
Electronegativity difference between chlorine and oxygen is 0.28
Chloride:
Only forms Cl2

33. 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 Cl O
Electronegativity: 3.44
Electronegativity: 3.16

34. 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

35. 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+H2O2HClO4

36. 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

37. 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

38. Physical states across period 3
Group 1 to 5 are solid Group 6 is gaseous Group 7 is gas/liquid