Presentation on theme: "Na-Sodium Na2O- Sodium Oxide and NaCl- Sodium Chloride At standard condition- Solid Bonding and Structure: Ionic lattice Electrical Conductivity: Good."— Presentation transcript:
1 Na-SodiumNa2O- 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 powderForms giant ionic lattice and strong ionic bonds hold the ions togetherConducts electricity when moltenHowever, 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 bondsConducts electricityIons dissociate when in molten stateMelting point is 714°C
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 easilyIons 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.
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 bondsElectronegativity difference between chlorine and oxygen is 0.28Chloride: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 forcesClOElectronegativity: 3.44Electronegativity: 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+H2O2HClO4
36 Properties of chlorine Chlorine bonds with itself to form Cl2 It has covalent bonds as the electronegativity difference is 0ClClElectronegativity: 3.16Electronegativity: 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