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Understanding Chemical Bonding: Lewis Symbols, Octet Rule, and Ionic Bonding

Dive into the world of chemical bonding with an exploration of Lewis symbols, the octet rule, and ionic bonding. Learn how atoms strive for stability, the characteristics of ionic compounds, and the significance of lattice energy. Discover the rules of covalent bonding, including multiple bonds and molecular structures. Delve into concepts such as electronegativity, bond polarity, and naming conventions in chemistry. Get insights into drawing Lewis structures, resonance, bond order, and exceptions to the octet rule. Explore the strengths of covalent bonds through bond enthalpy and enthalpy of reactions, with examples like the synthesis of nitroglycerin. Unravel the complexities of chemical bonding to enhance your understanding of fundamental concepts in chemistry.

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Understanding Chemical Bonding: Lewis Symbols, Octet Rule, and Ionic Bonding

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  1. AP Chemistry Chapter 8

  2. 8.1 A. Lewis symbols Lewis symbols B. Octet rule- every atom wants a full outer shell of electrons, that’s 8, to be more stable

  3. 8.2 Ionic bonding (salts) brittle solids, high melting point A. + - Na Cl transfer of electrons usu. metal with nonmetal B. Lattice NRG-NRG required to completely separate a mole of a solid ionic compound into gases ions.

  4. http://www.youtube.com/watch?v=_M9khs87xQ8&sns=em

  5. Dogs teaching chemistry • http://www.youtube.com/watch?v=_M9khs87xQ8&sns=em

  6. …Continue 8.2 1. E=kQ1Q2 d NRG increases as charge increases and distance decreases. C. electronic configuration of ions Fe = [Ar] 4s2 3d6 Fe+3 = [Ar] 3d5

  7. 8.3 A. size of ions 1. Metals-smaller, pos, lost electrons 2. Nonmetals- larger, neg, gained electrons B. Isoelectric series = same # e- 1. Increase nuclear charge (ENC) 2. Decrease ionic radius

  8. 8.4 A. Covalent bonding sharing of electrons 1. Usu. 2 nonmetals 2. Lewis structures B. Multiple bonds 1. O2 - double bond = 2 pair shared e- 2. N2 - triple bond = 3 pair of shared e- 3. single – longest bond triple – shortest bond 4. triple – strongest, highest bond NRG C. Metallic bond – sea of e-

  9. 8.5 I. Electronegativity – ability to attract shared e- A. trend F=4.0 B. Linus Pauling II. Bond Character > 1.67  ionic 0.20<1.67  polar covalent <0.20  nonpolar covalent

  10. …Continue 8.5 III. Polarity A. polar – unsymmetrical molecule B. nonpolar – symmetrical molecule C. dipole – polar bond or molecule D. dipole moment – measure of polarity. 0dm = NP IV. NAMING

  11. 8.6 Drawing Lewis Structures I. Formal Charges = # val. E in isolated atom - #e assigned to the atom in the Lewis structure. OR F.C. = (val e- - bonds – unshared e-) Do not represent real charges.

  12. 8.7 A. Resonance Structure 1. More than one way to draw 2. Need double or triple bond that can move 3. All bond lengths are same, they average out.

  13. …Continue 8.7 BOND ORDER 1 = single bond 2 = double bond 3 = triple bond B. benzene B.O. = 9 bonds = 1.5 6 spaces

  14. 8.8 Exception 1. NO2 – odd # of e- 2. BF3 – less than octet 3. PCl5 – expanded octet

  15. 8.9 Strengths of Covalent Bonds • Bond Enthalpy (bond NRG) – how easily are bonds broken. Always positive. • Enthalpy of Reactions = (bond broken – bonds formed) CH4 + Cl2 CH3Cl + HCl (pg. 326) 4C-H 4(413) 3C-H 3(413) Cl-Cl(242) H-Cl 431 C-Cl328 +1894 -1998 ΔH= - 104 kJ/mol • ΔH = reactants - products

  16. Nitroglycerin • 4C3H5N3O9(l)  6N2(g) + 12CO2(g) + 10H2O(g) + O2(g) 4 moles of liquid makes 29 moles of gas!!

  17. City Hall in Stockholm.

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