In this unit, students are taught how to recognise and explain patterns in the Periodic Table in terms of atomic structure. Material covered includes the Periodic Table, physical and chemical properties, trends across period three and first row transition elements.
Atomic structure is the unifying concept in Chemistry.
Topic 3: Periodicity (6 hours)- SL & HL Students
3.1 The periodic table
Unique Individuals - Often the greatest leaps in Science are made when scientists think outside the box.
- Deduce the electron configuration of an atom from the position of the element in the Periodic Table
3.2 Periodic Trends
- Predict and explain metallic/non-metallic behaviour based on position in the Periodic Table
- Discuss similarities and differences in properties (atomic radius, ionic radius, ionization energy, electron affinity, electronegativity) of elements in the same group/period
- Write chemical equations to explain pH changes for the reactions of oxides of Na, Mg, P, N and S with water.
Topic 13: Periodicity - the transition metals (4 hours) - HL Students only
13.1 First-row d-block elements
- List the characteristic properties of transition elements
- Explain why Zn is not considered to be transition a element
- Understand that transition elements exhibit the +2 oxidation state when the s-electrons are removed
- Explain the existence of variable oxidation number in ions of transition elements
- Define the term ligand.
- Describe and explain the formation of complexes of d-block elements.
- Explain why some complexes of d-block elements are coloured
- Deduce charge on complex given the formula of the ion and the ligands present
- Explanation of magnetic properties of transition metals with unpaired electrons
13.2 Coloured Complexes
- Understand and explain the origin of colour in transition metals complexes
- Explain how various factors affect the colour of complexes
The detailed curriculum can be consulted here.