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The Student and Tutor reviewed the fundamental rules for filling electrons in atomic orbitals, including the Aufbau principle, Hund's Rule of Maximum Multiplicity, and the Pauli Exclusion Principle. They applied these rules to write electronic configurations for various atoms, discussing special cases like Chromium and Copper due to enhanced stability. The Tutor assigned practice for electronic configurations using the periodic table, and they briefly confirmed previous work on isotope numericals before planning to start a new topic next session.

The Tutor and Student reviewed fundamental concepts in atomic structure, focusing on the wave mechanical model and the four quantum numbers (principal, azimuthal, magnetic, and spin). They clarified how these numbers define electron behavior, subshells, and orbital shapes, and differentiated between 'orbits' and 'orbitals.' The Student practiced identifying quantum numbers for specific subshells, and the Tutor assigned a review of these concepts in preparation for discussing electron filling rules in the next class.

Student and Tutor reviewed key concepts from the periodic table, including electron affinity, electronegativity, their variations, and metallic character. The session then transitioned to atomic structure, covering historical atomic models and their limitations, before introducing atomic orbitals and the four quantum numbers. The Student was encouraged to self-study quantum numbers for clearer understanding in the next session.

The Student and Tutor reviewed foundational Chemistry concepts, including the historical development of the periodic table, atomic radius, ionization energy, and electron affinity. They discussed the definitions, factors affecting these properties, and their trends across periods and down groups, with the Student applying these concepts to comparative problems. The next session is planned to cover electronegativity and different types of electron configurations, including orbitals.

The Tutor and Student discussed metallic bonding and the historical evolution of the periodic table, tracing contributions from Dobereiner, Newlands, and Mendeleev, highlighting their respective laws, features, and limitations. They then explored the modern periodic law by Moseley and the structure of the contemporary periodic table, concluding with an analysis of atomic and ionic radius trends. The Student was assigned to review the periodic table for the next session.

The Student and Tutor reviewed ionic and covalent bonding, including factors affecting their formation and different types of covalent bonds. They then delved into coordinate bonding with multiple examples and concluded by discussing hydrogen bonding and its implications for the density of ice. Metallic bonding and states of matter were mentioned as topics for the next session.