Table 2 compares three ions and a neutral atom. In Table, the common oxidation numbers in the last column are interpreted as the result of either losing the valence electrons (leaving a positive ion) or gaining enough electrons to fill that valence subshell. For example, in the H 2O molecule, each H has an oxidation number of +1, and the O is –2. In molecules, the various atoms are assigned chargelike values so the sum of the oxidation numbers equals the charge on the molecule. These are the valence electrons.įor ions, the valence equals the electrical charge. These electrons are most distant from the positive nucleus and, therefore, are most easily transferred between atoms in chemical reactions. Valence electrons, which comprise the valence shell of the atom.įor brevity, many chemists record the electron configuration of an atom by giving only its outermost subshell, like 4 s 1 for potassium or 4 s 2 for calcium. The electrons in the highest numbered subshells are the Study the third column of complete electronic configurations carefully so you understand how electrons are added to the subshell of lowest energy until it reaches its capacity then the subshell of the next energy level begins to be filled. The electronic configuration of an atom is given by listing its subshells with the number of electrons in each subshell, as shown in Tableġ. Quiz: Introduction to Oxidation-Reduction Reactions.Introduction to Oxidation-Reduction Reactions. Quiz: Heat Capacities and Transformations.Quiz: Introduction to Organic Compounds.Quiz: Compounds with Additional Elements.
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