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Ionic and Covalent Bonding REVIEW valence electrons: • the electrons in the highest occupied energy level of an element’s atom • the number of valence electrons determines the chemical properties of an element • usually the only electrons used in bonds • how to determine # of valence electrons? 1. look at electron configuration 2. trend on periodic table (group# = #valence electrons) Ionic and Covalent Bonding Lewis Dot Structures: • diagrams that show the valence electrons as dots The Octet Rule: • An octet is a set of 8 • In forming compounds, atoms tend to achieve the electron configuration of a noble gas (8 valence electrons) • Exceptions: Boron (wants 6 v.e.’s) and Phosphorous, which uses vacant d orbitals to form extra bonds. Ionic Bonding (metal + nonmetal) • Metals tend to lose their valence electrons, leaving a complete octet in the next-lowest energy level, to form cations. • Nonmetals tend to gain electrons or share electrons with another nonmetal to achieve a complete octet to form anions. Ionic Bonds Anions and cations have opposite charges and attract on another by electrostatic forces. Ionic Bonds bind oppositely charged ions. The total positive charges of cations =’s the total negative charges or the anions ... so, compounds are neutral. Properties of Ionic Bonds Crystalline solids at room temperature Ions are arranged in repeating threedimensional patterns. In these patterns, each ion is strongly attracted to its neighbors and the structure is very stable --> ionic compounds have a high melting point. When melted, ionic compounds can conduct electricity. Metallic Bonding (metal + metal) • Metals are like ionic compounds in some ways. • Metallic Bonds consist of + metal ions packed together, surrounded by a “sea” of valence electrons. • These valence electrons can travel from one end of a piece of metal to the other --> excellent electrical conductors. • Metals = simplest crystalline solids. • Alloys: mixtures made of two or more elements, at least one is a metal. Ex: Brass= Cu + Zn Covalent Bonding (nonmetal + nonmetal) • Atoms form covalent bonds when they share electrons to form an octet. • 1 shared PAIR (2 electrons) = a single bond • 2 shared PAIRS (4 electrons) = a double bond • 3 shared PAIRS (6 electrons) = a triple bond • RESONANCE STRUCTURES: more than one electron dot structure can be drawn.