Periodicity of properties in Periodic table

This course explores the periodicity of chemical and physical properties of elements as they relate to the periodic table. By analyzing trends across periods (horizontal rows) and groups (vertical columns), students will gain a comprehensive understanding of atomic behavior. The course begins with atomic size, highlighting how atomic radii decrease across a period due to increasing nuclear charge and increase down a group due to additional electron shells. Next, we examine the shielding effect—the phenomenon where inner electrons reduce the effective nuclear pull on valence electrons. This effect becomes more pronounced down a group, impacting many other periodic trends.

Ionization energy, or the energy required to remove an electron from an atom, is another key focus. It increases across a period and decreases down a group, directly influenced by atomic size and shielding. The course also delves into electron affinity, the energy change when an atom gains an electron. Generally, electron affinity becomes more negative across a period, reflecting stronger attraction for electrons, and less negative down a group due to increased shielding and atomic size.

Finally, electronegativity—an atom’s ability to attract electrons in a bond—is studied. This property also increases across a period and decreases down a group, following patterns established by atomic size and nuclear charge. Through visual aids and  examples, students will build a strong foundation in understanding these periodic trends and their implications in chemical behavior and reactivity.