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Bonding

Bonding. Valence Electrons. In the highest energy level Determine chemical properties. Elements bond to get 8 valence e- (octet rule). Anions, Cations, and Electron Configuration. Cations form by losing valance electrons to take on a noble gas configuration (ns 2 np 6 ).

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Bonding

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  1. Bonding

  2. Valence Electrons • In the highest energy level • Determine chemical properties. • Elements bond to get 8 valence e- (octet rule)

  3. Anions, Cations, and Electron Configuration Cations form by losing valance electrons to take on a noble gas configuration (ns2np6)

  4. Anions, Cations, and Electron Configuration Cations form by losing valance electrons to take on a noble gas configuration (ns2np6) So Li loses the 2s1 electron to form Li+1. Mg loses both 3s2 electrons to form Mg+2 Al loses three electrons from 3s23p1 to form Al+3

  5. Anions, Cations, and Electron Configuration Anions form by gaining valance electrons to take on a noble gas configuration (ns2np6) So F becomes F1- by gaining a 2p electron to have the new valance configuration 2s22p6. S becomes S2- by gaining two 2p electrons to have the new valance configuration 3s23p6. N becomes N3- by gaining three 2p electrons to have the new valance configuration 2s22p6.

  6. Ionic Compounds • Made of metal cations (+) and nonmetal anions (-) • Have no charge • Solid at room temperature • High melting points • Conduct electric current when dissolved in water Na+ Cl-

  7. Writing Ionic Formulas Aluminum and oxygen • Write each ion with the correct charge (cations first!) • Bring the charge # (NOT the + or -) down as a subscript and switch which element it goes to Al3+ O2- Al2O3

  8. Naming Ionic Compounds • Name of the cation • Roman numeral for cations with mutliple + charges • Name the anion • ide is single anion • -ate or -ite is polyatomic CaF2 Li3PO4 PbS2 Calcium fluoride Lithium phosphate Lead (IV) sufide

  9. Covalent Bonds • Nonmetal atoms are held together by sharing electrons • low melting and boiling point • All phases at room temperature

  10. Diatomic Molecules H2, N2, O2, F2, Cl2, Br2, I2, At2

  11. Naming and Writing Formulas for Covalent Compounds Indicate # of each atom using prefixes (mono, di, tri, tetra, penta, hexa, hepta, octa, nona, deca) The first element does not use mono if there’s only one. • NO2 • P2O4 nitrogen dioxide diphosphorus tetroxide

  12. Lewis Structures Step 1: Set up the following table to determine bond numbers Step 2: Connect atoms based on bond numbers calculated Step 3: Fill octets with unshared electrons

  13. VSEPR THEORY Valence Shell Electron Pair Repulsion . . bent tetrahedaral linear . . Trig planar Trig pyramid

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