CHM 1045 Chapter Notes - Chapter 6: Chemical Formula, Formal Charge, Electronegativity
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Octet rule atoms will lose, gain, or share electrons to achieve a noble gas configuration. Valence electrons that do not participate in the bonding are called lone pairs. Single bond consists of only one shared pair of electrons. Multiple bonds consist of two or more shared pair of electrons; Electronegativity and polarity (cid:4666)ex:h2(cid:4667) (ex: hf) (ex: naf) Electronegativity the ability of an atom to draw shared electrons (covalent bonds) toward itself. An element with high electronegativity has a greater tendency to attract shared electrons. Note: generally, the closer an element is to f in the periodic table, the more electronegative it is. Drawing lewis structures: from the molecular formula, draw the skeletal structure of the compound, using chemical symbols and placing bonded atoms next to one another. The least electronegative atom is generally the central atom. Draw a single covalent bond (dash) between the central atom and each of the surrounding atoms.
