Inorganic Chemistry: Principles of Structure and Reactivity

Understanding atomic structure and periodicity is fundamental to the study of inorganic chemistry, as it lays the groundwork for interpreting the behavior of elements and compounds. Atoms are composed of subatomic particles—protons, neutrons, and electrons—whose arrangement and interactions define the chemical identity and properties of an element. The modern atomic model is deeply rooted in quantum mechanics, which describes electrons as existing in orbitals, regions of space where the probability of finding an electron is highest.

Each electron in an atom is characterized by a unique set of quantum numbers, which describe its energy, shape, orientation, and spin. These quantum numbers help determine the distribution of electrons among atomic orbitals, leading to electron configurations that follow the Pauli exclusion principle and Hund’s rule. These configurations not only reveal how electrons fill orbitals but also explain chemical behavior, especially the tendencies of atoms to gain, lose, or share electrons in chemical reactions.

The periodic table organizes elements based on recurring trends in their chemical properties. These periodic trends arise from the electron configurations and the structure of the atom. One key trend is atomic radius, which generally decreases across a period due to increasing nuclear charge pulling electrons closer, and increases down a group due to additional electron shells. Another important trend is ionization energy—the energy required to remove an electron from an atom. This energy increases across a period and decreases down a group, again reflecting the influence of nuclear charge and distance of electrons from the nucleus.

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