UJ INORGANIC CHEMISTRY 3
GOLD REVISION PACK
Mainstream Student Notes | Third-Year Level
What this pack is
A detailed tutoring-style guide for students revising Inorganic Chemistry 3. It is original learning material, not an official UJ
document, not a past-paper memo, and not copied from paid study-note websites.
How to use it
Read each chapter once for understanding, then redo the worked examples without looking. Use the final practice section as a
mini test before exams.
Prepared for tutoring and revision use
UJ Inorganic Chemistry 3 Gold Revision Pack | Tutoring notes | Not an official UJ document
,Contents
1. Gold Pack study method
2. Periodic trends and bonding foundations
3. Symmetry, shapes and stereochemistry
4. Coordination chemistry: ligands, naming and isomerism
5. Crystal field theory and ligand field thinking
6. Magnetism and electronic spectra
7. Coordination reaction mechanisms
8. Redox chemistry and electron transfer
9. Organometallic chemistry
10. Main-group chemistry at third-year level
11. Solid-state inorganic chemistry
12. Bioinorganic and environmental inorganic chemistry
13. High-yield revision tables
14. Worked examples
15. Practice questions
16. Memo-style answers
17. Glossary and references
UJ Inorganic Chemistry 3 Gold Revision Pack | Tutoring notes | Not an official UJ document
,1. Gold Pack study method
This Gold Pack is designed to help a third-year student move from memorising isolated facts to explaining inorganic
chemistry with reasons. Inorganic Chemistry 3 usually rewards students who can connect periodic trends, bonding,
structure, ligand behaviour, electronic configuration, spectroscopy, magnetism, redox chemistry and reaction mechanisms.
Student promise
This pack uses simple English, but it does not lower the academic level. The goal is to make hard ideas understandable
without removing the chemistry.
1.1 The three-pass method
1. Pass 1: Read the notes to build a mental map. Do not try to memorise every detail on the first reading.
2. Pass 2: Cover the explanations and reproduce the diagrams, tables and steps from memory.
3. Pass 3: Attempt the practice questions under time pressure and mark yourself using the memo section.
1.2 How exam answers should sound
A strong answer usually has three parts: the correct chemical fact, the reason behind it, and the application to the
molecule or complex in the question. For example, instead of only saying that a complex is low spin, explain that the ligand
field splitting is large enough for pairing to occur before electrons occupy higher-energy orbitals.
1.3 Symbols and shortcuts used in this pack
Symbol Meaning
M metal centre
L neutral ligand
X anionic ligand
CN coordination number
d^n number of d electrons on the metal
Delta_o octahedral crystal field splitting
Delta_t tetrahedral crystal field splitting
LFSE ligand field stabilisation energy
HSAB hard and soft acids and bases
UJ Inorganic Chemistry 3 Gold Revision Pack | Tutoring notes | Not an official UJ document
, 2. Periodic trends and bonding foundations
Third-year inorganic chemistry often starts from patterns in the periodic table. These patterns explain why elements form
certain oxidation states, why some ions are small and strongly polarising, why some complexes are stable, and why some
ligands bind more strongly than others.
2.1 Core periodic trends
Trend Across a period Down a group Why it matters
Controls bond length, lattice
Atomic radius Usually decreases Usually increases
energy and steric crowding.
Affects ease of forming cations
Ionisation energy Usually increases Usually decreases
and high oxidation states.
Affects bond polarity and acid-
Electronegativity Usually increases Usually decreases
base behaviour.
Explains transition from
Metallic character Usually decreases Usually increases ionic/metallic to covalent
behaviour.
High for small, highly charged Explains Fajans-type covalent
Polarising power Lower for large cations
cations character.
2.2 Oxidation states
An oxidation state is a bookkeeping charge assigned by assuming bonds are ionic. It does not always equal the real
charge on an atom, but it helps us track redox reactions and assign d-electron counts.
Exam habit
Always find the metal oxidation state before predicting d-electron count, spin state, magnetism or LFSE.
2.3 Ionic, covalent and metallic bonding
Ionic bonding is useful for salts and simple solids, but many inorganic compounds are not purely ionic. Covalent bonding
becomes more important when atoms are similar in electronegativity or when small, highly charged cations polarise
anions. Metallic bonding is best understood as positive metal cores held together by delocalised valence electrons.
Bonding model Main idea Useful for Limitation
Electrostatic attraction Salts, lattice energy, simple Does not show covalent mixing
Ionic
between ions solids well.
Shared electron density Molecular compounds, ligand May not describe extended
Covalent
between atoms bonding solids fully.
Delocalised electrons over Too simple for many
Metallic Metals, conductivity, alloys
metal centres semiconductors.
Ligand donates electron pair to Complex ions and Can hide back-bonding unless
Coordinate covalent
metal organometallics expanded.
2.4 HSAB theory
HSAB theory says hard acids prefer hard bases, and soft acids prefer soft bases. It is not a magic rule, but it is very useful
for predicting stability and reaction preference.
Type Typical features Examples
Hard acids Small, high charge, low polarizability H+, Al3+, Fe3+, Cr3+
Soft acids Larger, lower charge, high polarizability Ag+, Pd2+, Pt2+, Hg2+
Hard bases Small donor atom, not easily distorted F-, OH-, H2O, NH3
Soft bases Large/polarisable donor atom I-, S2-, RS-, PR3
A hard metal ion such as Fe3+ often binds strongly to oxygen donors. A soft metal ion such as Pd2+ or Pt2+ often binds
well to sulfur or phosphine donors. This idea is helpful in coordination chemistry, catalysis and bioinorganic chemistry.
UJ Inorganic Chemistry 3 Gold Revision Pack | Tutoring notes | Not an official UJ document
GOLD REVISION PACK
Mainstream Student Notes | Third-Year Level
What this pack is
A detailed tutoring-style guide for students revising Inorganic Chemistry 3. It is original learning material, not an official UJ
document, not a past-paper memo, and not copied from paid study-note websites.
How to use it
Read each chapter once for understanding, then redo the worked examples without looking. Use the final practice section as a
mini test before exams.
Prepared for tutoring and revision use
UJ Inorganic Chemistry 3 Gold Revision Pack | Tutoring notes | Not an official UJ document
,Contents
1. Gold Pack study method
2. Periodic trends and bonding foundations
3. Symmetry, shapes and stereochemistry
4. Coordination chemistry: ligands, naming and isomerism
5. Crystal field theory and ligand field thinking
6. Magnetism and electronic spectra
7. Coordination reaction mechanisms
8. Redox chemistry and electron transfer
9. Organometallic chemistry
10. Main-group chemistry at third-year level
11. Solid-state inorganic chemistry
12. Bioinorganic and environmental inorganic chemistry
13. High-yield revision tables
14. Worked examples
15. Practice questions
16. Memo-style answers
17. Glossary and references
UJ Inorganic Chemistry 3 Gold Revision Pack | Tutoring notes | Not an official UJ document
,1. Gold Pack study method
This Gold Pack is designed to help a third-year student move from memorising isolated facts to explaining inorganic
chemistry with reasons. Inorganic Chemistry 3 usually rewards students who can connect periodic trends, bonding,
structure, ligand behaviour, electronic configuration, spectroscopy, magnetism, redox chemistry and reaction mechanisms.
Student promise
This pack uses simple English, but it does not lower the academic level. The goal is to make hard ideas understandable
without removing the chemistry.
1.1 The three-pass method
1. Pass 1: Read the notes to build a mental map. Do not try to memorise every detail on the first reading.
2. Pass 2: Cover the explanations and reproduce the diagrams, tables and steps from memory.
3. Pass 3: Attempt the practice questions under time pressure and mark yourself using the memo section.
1.2 How exam answers should sound
A strong answer usually has three parts: the correct chemical fact, the reason behind it, and the application to the
molecule or complex in the question. For example, instead of only saying that a complex is low spin, explain that the ligand
field splitting is large enough for pairing to occur before electrons occupy higher-energy orbitals.
1.3 Symbols and shortcuts used in this pack
Symbol Meaning
M metal centre
L neutral ligand
X anionic ligand
CN coordination number
d^n number of d electrons on the metal
Delta_o octahedral crystal field splitting
Delta_t tetrahedral crystal field splitting
LFSE ligand field stabilisation energy
HSAB hard and soft acids and bases
UJ Inorganic Chemistry 3 Gold Revision Pack | Tutoring notes | Not an official UJ document
, 2. Periodic trends and bonding foundations
Third-year inorganic chemistry often starts from patterns in the periodic table. These patterns explain why elements form
certain oxidation states, why some ions are small and strongly polarising, why some complexes are stable, and why some
ligands bind more strongly than others.
2.1 Core periodic trends
Trend Across a period Down a group Why it matters
Controls bond length, lattice
Atomic radius Usually decreases Usually increases
energy and steric crowding.
Affects ease of forming cations
Ionisation energy Usually increases Usually decreases
and high oxidation states.
Affects bond polarity and acid-
Electronegativity Usually increases Usually decreases
base behaviour.
Explains transition from
Metallic character Usually decreases Usually increases ionic/metallic to covalent
behaviour.
High for small, highly charged Explains Fajans-type covalent
Polarising power Lower for large cations
cations character.
2.2 Oxidation states
An oxidation state is a bookkeeping charge assigned by assuming bonds are ionic. It does not always equal the real
charge on an atom, but it helps us track redox reactions and assign d-electron counts.
Exam habit
Always find the metal oxidation state before predicting d-electron count, spin state, magnetism or LFSE.
2.3 Ionic, covalent and metallic bonding
Ionic bonding is useful for salts and simple solids, but many inorganic compounds are not purely ionic. Covalent bonding
becomes more important when atoms are similar in electronegativity or when small, highly charged cations polarise
anions. Metallic bonding is best understood as positive metal cores held together by delocalised valence electrons.
Bonding model Main idea Useful for Limitation
Electrostatic attraction Salts, lattice energy, simple Does not show covalent mixing
Ionic
between ions solids well.
Shared electron density Molecular compounds, ligand May not describe extended
Covalent
between atoms bonding solids fully.
Delocalised electrons over Too simple for many
Metallic Metals, conductivity, alloys
metal centres semiconductors.
Ligand donates electron pair to Complex ions and Can hide back-bonding unless
Coordinate covalent
metal organometallics expanded.
2.4 HSAB theory
HSAB theory says hard acids prefer hard bases, and soft acids prefer soft bases. It is not a magic rule, but it is very useful
for predicting stability and reaction preference.
Type Typical features Examples
Hard acids Small, high charge, low polarizability H+, Al3+, Fe3+, Cr3+
Soft acids Larger, lower charge, high polarizability Ag+, Pd2+, Pt2+, Hg2+
Hard bases Small donor atom, not easily distorted F-, OH-, H2O, NH3
Soft bases Large/polarisable donor atom I-, S2-, RS-, PR3
A hard metal ion such as Fe3+ often binds strongly to oxygen donors. A soft metal ion such as Pd2+ or Pt2+ often binds
well to sulfur or phosphine donors. This idea is helpful in coordination chemistry, catalysis and bioinorganic chemistry.
UJ Inorganic Chemistry 3 Gold Revision Pack | Tutoring notes | Not an official UJ document
