Inorganic Chemistry
• Periodicity • Transition metals
• Group 2 • Isomerism
• Trends • Redox titrations
• Reactions, solubility • Ligand substitution reactions 1 2
• Uses • Coloured complexes
• Group 7 • Measuring concentration through
• Appearance • Colours
• Redox • Variable oxidation states
• Trends • Acidity
• Chlorine and water • Heterogeneous catalysts
• Homogeneous catalysts
• Period 3 • Autocatalysis
• Trends, structure, and bonding
• Reaction with water, oxygen
• Oxides
, regularly occurring patterns in properties that occur re
Periodicity across a period in the periodic table
Element Na Mg Al Si P || P4 S || S8 Cl || Cl2
Bonding Giant metallic lattice Covalent Covalent (simple molecular) Mon
(macromolecular)
Particles Positive ions, delocalised Atoms Molecules Ato
electrons
Melting/boiling Increased charge on Many strong Van der Waals forces between Wea
point ions/more delocalised covalent bonds molecules require little energy der
electrons, greater breaking, to overcome betw
attraction between requires lots of S8 highest MP (largest req
positive ions and energy molecule, most electrons) ene
electrons ove
Atomic radius more protons, sim
Decreases
Electronegativity m
Increases simi
1st ionisation Mg -> Al, higher energy level decre
energy Increases* P -> S, electron pair repulsion
, Group 2 - trends
Atomic radius Melting points Decreases
Element Melting point/K down the group
Increases down
the group Be 1551 Shielding increase
More shells down Mg 922 down the group
∴
the group Ca 1112 Atomic radius incre
Sr 1042
down the group
First ionisation energy Ba 998 Nucleus-electr
⇒ attraction decr
Decreases Ra 973
down the group down the group
Magnesium is
Shielding increases an outlier ∴ Weaker metallic b
down the group
Atomic radius increases
down the group
Nucleus-electron attraction
⇒ decreases down the group
∴ Easier to lose a valence shell electron
• Periodicity • Transition metals
• Group 2 • Isomerism
• Trends • Redox titrations
• Reactions, solubility • Ligand substitution reactions 1 2
• Uses • Coloured complexes
• Group 7 • Measuring concentration through
• Appearance • Colours
• Redox • Variable oxidation states
• Trends • Acidity
• Chlorine and water • Heterogeneous catalysts
• Homogeneous catalysts
• Period 3 • Autocatalysis
• Trends, structure, and bonding
• Reaction with water, oxygen
• Oxides
, regularly occurring patterns in properties that occur re
Periodicity across a period in the periodic table
Element Na Mg Al Si P || P4 S || S8 Cl || Cl2
Bonding Giant metallic lattice Covalent Covalent (simple molecular) Mon
(macromolecular)
Particles Positive ions, delocalised Atoms Molecules Ato
electrons
Melting/boiling Increased charge on Many strong Van der Waals forces between Wea
point ions/more delocalised covalent bonds molecules require little energy der
electrons, greater breaking, to overcome betw
attraction between requires lots of S8 highest MP (largest req
positive ions and energy molecule, most electrons) ene
electrons ove
Atomic radius more protons, sim
Decreases
Electronegativity m
Increases simi
1st ionisation Mg -> Al, higher energy level decre
energy Increases* P -> S, electron pair repulsion
, Group 2 - trends
Atomic radius Melting points Decreases
Element Melting point/K down the group
Increases down
the group Be 1551 Shielding increase
More shells down Mg 922 down the group
∴
the group Ca 1112 Atomic radius incre
Sr 1042
down the group
First ionisation energy Ba 998 Nucleus-electr
⇒ attraction decr
Decreases Ra 973
down the group down the group
Magnesium is
Shielding increases an outlier ∴ Weaker metallic b
down the group
Atomic radius increases
down the group
Nucleus-electron attraction
⇒ decreases down the group
∴ Easier to lose a valence shell electron
