The greater the nuclear charge, the higher the effective nuclear charge, which affects periodic properties such as atomic radius and ionization energy.The effective nuclear charge increases as the atomic number increases in elements of the same period, despite the shielding parameter remaining constant.The effective nuclear charge increases with atomic number, affecting properties like atomic radius and ionization energy, and is evaluated using the Slater's rule protocol. □ The effective nuclear charge for a cation is much greater than that of a neutral atom, leading to stronger attraction between particles and smaller atomic radius.□ The effective nuclear charge of potassium is only 15% of its total nuclear charge, meaning that only around 3 protons can attract the electrons from the 4s orbital.□ The exclusion principle suggests that electrons in the outermost layer of an atom do not influence the electrons in the innermost layers.□ The effective nuclear charge of an atom increases with a higher atomic number, resulting in a smaller atomic radius and higher ionization energy.□ The effective nuclear charge increases as you move further to the right in the periodic table, resulting in a higher atomic number. ![]() □ The effective nuclear charge is determined by the nuclear charge of an atom minus an empirical parameter that represents the shielding experienced by the electrons, indicating the balance between attraction and repulsion within an atom. ![]() ![]()
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