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Valances

In chemistry, valence electrons are the electrons contained in the outermost, or valence, electron shell of an atom. One must know these valences to be able to determine chemical reactions. more...

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Valence electrons are important in determining how an element reacts with other elements because the less number of valence electrons an atom holds, the less stable it is which means it is more likely to react.

The number of valence electrons

To determine the quantity of valence electrons an element has, one must look at the periodic table group (vertical column) in which the element is categorized. With the exception of groups 3–12 (transition metals), the number within the unit's place identifies how many valence electrons are contained within the elements listed under that particular column.

*Except for chromium and copper, which only has one valence electron. **Except for helium, which only has two valence electrons.

Valence electrons in chemical reactions

The number of electrons in an atom's outermost valence shell governs its bonding behavior. Therefore, elements with the same number of valence electrons are grouped together in the periodic table of the elements. As a general rule, the fewer electrons in an atom's valence shell, the more reactive it is. Group 1 metals are therefore very reactive, with caesium, rubidium, and francium being the most reactive of all metals.

Every atom is much more stable, or less reactive, with a full valence shell. This can be achieved one of two ways: an atom can either share electrons with neighboring atoms, a covalent bond, or it can remove electrons from other atoms, an ionic bond. Another form of ionic bonding involves an atom giving some of its electrons to another atom; this also works because it can end up with a full valence by giving up its entire outer shell. By moving electrons, the two atoms become linked. This is known as chemical bonding and serves to build atoms into molecules or ionic compounds. Five major types of bonds exist:

ionic bonds; covalent bonds; coordinate covalent bonds (Also called dative covalent bonds); hydrogen bonds; metallic bonds;