Valence electrons are electrons on the outermost shell/orbitals. Sheilding electrons are inner electrons that block valence electrons from protons causing less attraction.
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Electron shielding primarily affects the effective nuclear charge experienced by valence electrons in an atom. It reduces the attraction between the valence electrons and the nucleus, leading to a decrease in the ionization energy and atomic size of the atom. Additionally, electron shielding can influence the chemical reactivity of an element by affecting the ease with which valence electrons can participate in bonding.
potassium belongs to group 1 and has one valence electron. aluminium belongs to group 13 and has three valence electrons.
VSEPR only shows the geometric shape of the element
Alkali metals have 1 valence electron.
VSEPR theory stands for Valence Shell Electron Pair Repulsion theory. It is a model used to predict the geometry of molecules based on minimizing the repulsion between electron pairs in the valence shell of an atom. By considering the repulsions between electron pairs, VSEPR theory helps determine the shape of molecules.