Unit 3: Periodicity
The chapter covers the periodicity in chemistry, highlighting the systematic variations in properties of elements organized by atomic number. It includes periodic trends in atomic properties, such as atomic and ionic radii, ionization energies, and electronegativities, alongside group behaviors of various element families. Special attention is given to transition metals, emphasizing their unique properties and behaviors arising from partially filled d orbitals.
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Sections
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What we have learnt
- Periodic trends in atomic properties are influenced by effective nuclear charge and shielding effects.
- Each group in the periodic table exhibits characteristic properties due to common outer electronic configurations.
- Transition metals display variable oxidation states and complex behaviors due to their electron configurations.
Key Concepts
- -- Effective Nuclear Charge (Z_eff)
- Net positive charge experienced by valence electrons after accounting for shielding by inner electrons.
- -- Ionization Energy (IE)
- Energy required to remove an electron from a gaseous atom or ion in its ground state.
- -- Electron Affinity (EA)
- Energy change when an electron is added to a neutral atom in the gas phase, often released.
- -- Electronegativity (χ)
- Measure of an atom’s ability to attract electrons towards itself in a covalent bond.
- -- Crystal Field Theory (CFT)
- A model describing the electronic structure of transition metal complexes by considering the effect of ligands on d orbitals.
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