They determine how "willing" the elements are to bond with each other to form new compounds. Valence electrons are responsible for the reactivity of an element. You can easily determine the number of valence electrons an atom can have by looking at its Group in the periodic table.įor example, atoms in Groups 1 and 2 have 1 and 2 valence electrons, respectively.Ītoms in Groups 13 and 18 have 3 and 8 valence electrons, respectively. Valence electrons are the electrons present in the outermost shell of an atom. To form a covalent bond, one electron from the halogen and one electron from another atom form a shared pair.įor example, in #"H–F"#, the dash represents a shared pair of valence electrons, one from #"H"# and one from #"F"#. To form an ionic bond, a halogen atom can remove an electron from another atom in order to form an anion (e.g., #"F"^"-", "Cl"^"-"#, etc.). They have one less electron configuration than a noble gas, so they require only one additional valence electron gain an octet. The most reactive nonmetals are the halogens, e.g., #"F"# and #"Cl"#. Nonmetals tend to attract additional valence electrons to form either ionic or covalent bonds. They need to lose only one or two valence electrons to form positive ions with a noble gas configuration. The most reactive metals are those from Groups 1 and 2. Generally, elements in Groups 1, 2, and 13 to 17 tend to react to form a closed shell with a noble gas electron configuration ending in #ns^2 np^6#. Elements whose atoms have the same number of valence electrons are grouped together in the Periodic Table.
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