The shielding effect refers to the reduction in effective nuclear charge on the electron cloud, due to the repulsion between electrons in different shells. This phenomenon explains why electrons in outer shells are less tightly bound to the nucleus, influencing atomic size, ionization energy, and electron affinity.

Shielding Effect

shielding effect

Effective nuclear charge is the net positive charge experienced by an electron in a multi-electron atom, accounting for both the actual nuclear charge and the shielding effect of other electrons. It plays a crucial role in determining atomic properties such as atomic radius, ionization energy, and electron affinity.

effective nuclear charge

The electron cloud is a model used to describe the probable locations of electrons around an atom's nucleus, emphasizing the uncertainty and probabilistic nature of electron positions as dictated by quantum mechanics. This model replaces the earlier Bohr model by incorporating the principles of wave-particle duality and Heisenberg's uncertainty principle, providing a more accurate representation of atomic structure.

electron cloud

repulsion between electrons

outer shells

Tight binding to the nucleus

Atomic size refers to the distance from the nucleus of an atom to the outermost shell of electrons, influencing properties such as reactivity and bonding. It generally decreases across a period due to increased nuclear charge and increases down a group due to additional electron shells.

atomic size

Ionization energy is the amount of energy required to remove an electron from an isolated atom or ion in its gaseous state. It is a fundamental property that reveals the reactivity of elements, with higher ionization energies indicating a stronger hold on electrons and typically less reactivity.

ionization energy

Electron affinity is the energy change that occurs when an electron is added to a neutral atom in the gaseous state, indicating how strongly an atom can attract additional electrons. It generally becomes more exothermic across a period due to increasing nuclear charge and less exothermic down a group due to increased atomic radius and electron shielding.

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