Week Six Lecture Notes
Week Six Lecture Notes Chem 105
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This 2 page Class Notes was uploaded by Marisa Loken on Monday October 19, 2015. The Class Notes belongs to Chem 105 at University of Wisconsin - Stevens Point taught by Dr. Riha in Fall 2015. Since its upload, it has received 16 views. For similar materials see Fundamental Chemistry in Chemistry at University of Wisconsin - Stevens Point.
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Date Created: 10/19/15
Week Six Notes October 5October 9 Periodic trends Ionization energy IE 0 The energy required to remove an electron from an atom Electron af nity EA 0 Energy gained when an atom accepts an electron Electronegativity EN 0 Ability of an atom to attract electrons to itself left side D harder to add electrons easier to remove cations right side D easier to add electrons harder to remove electrons anions Only noble gases exist as single atoms in nature Have a full valence shell Stable atom that doesn39t want to add or take away electrons lfjust on s and p shells a stable con guration has 8 electrons Octet rule Atoms gain lose or share electrons to get 8 electrons in its valence shell Chemical formula Tells us the type of atoms in a compound Molecular formula Speci c to molecules covalent bonds 0 Actual number of atoms and kinds Empirical formula Apply to molecules Dionic and metallic 0 Only tells us relative amount of atoms H20 is a molecular formual lonic or metallic compounds Don39t have discrete quotmoleculesquot charges of an ionic compound must equal zero Wednesday Lewis symbols and Lewis structures One atom versus two or more atoms One dot equals one electron 0 One dot on each side top and bottom before adding additional dots o No more than two dots per side top and bottom Lewis symbol for ions Cations include charge Anions put the dot symbol in brackets with charge on the outside Lewis structures for molecules Dashes represent shared electrons Single dash is 2e or a single bond Double dash is 4e or a double bond Triple dash is 6e or a triple bond bonding capacity refers to how many bonds it can make Single dots allow for bonding H is always on outside never controls an atom FHday Formal Charges FC FC number of valence electrons number associate electrons 0 Associated electrons 1e per bond and 2e per lone pair structures with all atoms having their formal charge 0 are preferred structures with small formal charges are preferred over structures structure with the most electronegative atom having the negative formal charge is preferred sum of all formal charges of atoms in a molecule or polymathic ion must equal the charge on that molecule Resona nce Stl39UCtU res 2 or more lewis structures preferred for a molecule or polyatomic ion 0 Use gt between structures