1. IIIIIIIV Chemical Bonding I. Introduction to Bonding

2. A. Vocabulary zChemical Bond yattractive force between atoms or ions that binds them together as a unit ybonds form in order to… xdecrease potential energy (PE) xincrease stability

3. A. Vocabulary CHEMICAL FORMULA Molecular Formula Unit IONICCOVALENT CO 2 NaCl

4. A. Vocabulary COMPOUND Ternary Compound Binary Compound 2 elements more than 2 elements NaNO 3 NaCl

5. A. Vocabulary ION Polyatomic Ion Monatomic Ion 1 atom 2 or more atoms NO 3 - Na +

6. IONIC COVALENT Bond Formation Type of Structure Solubility in Water Electrical Conductivity Other Properties e - are transferred from metal to nonmetal high yes (solution or liquid) yes e - are shared between two nonmetals low no usually not Melting Point crystal lattice true molecules B. Types of Bonds Physical State solid liquid or gas odorous

7. “electron sea” METALLIC Bond Formation Type of Structure Solubility in Water Electrical Conductivity Other Properties Melting Point B. Types of Bonds Physical State e - are delocalized among metal atoms very high yes (any form) no malleable, ductile, lustrous solid

8. RETURN B. Types of Bonds

9. RETURN B. Types of Bonds

10. Ionic Bonding - Crystal Lattice RETURN B. Types of Bonds

11. Covalent Bonding - True Molecules RETURN B. Types of Bonds Diatomic Molecule

12. Metallic Bonding - “Electron Sea” RETURN B. Types of Bonds

13. C. Bond Polarity zMost bonds are a blend of ionic and covalent characteristics. zDifference in electronegativity determines bond type.

14. C. Bond Polarity zElectronegativity yAttraction an atom has for a shared pair of electrons. yhigher e - neg atom   - ylower e - neg atom   +

15. C. Bond Polarity zElectronegativity Trend (p. 151) yIncreases up and to the right.

16. zNonpolar Covalent Bond ye - are shared equally ysymmetrical e - density yusually identical atoms C. Bond Polarity

17. ++ -- zPolar Covalent Bond ye - are shared unequally yasymmetrical e - density yresults in partial charges (dipole)

18. zNonpolar zPolar zIonic View Bonding Animations.Bonding Animations C. Bond Polarity

19. Examples: zCl 2 zHCl zNaCl 3.0-3.0=0.0 Nonpolar 3.0-2.1=0.9 Polar 3.0-0.9=2.1 Ionic

20. IIIIIIIV II. Ionic Compounds Chemical Bonding

21. A. Energy of Bond Formation zLattice Energy yEnergy released when one mole of an ionic crystalline compound is formed from gaseous ions

22. B. Lewis Structures zCovalent – show sharing of e - zIonic – show transfer of e -

23. B. Lewis Structures zCovalent – show sharing of e - zIonic – show transfer of e -

24. C. Ionic Nomenclature Ionic Formulas zWrite each ion, cation first. Don’t show charges in the final formula. zOverall charge must equal zero. yIf charges cancel, just write symbols. yIf not, use subscripts to balance charges. zUse parentheses to show more than one polyatomic ion. zStock System - Roman numerals indicate the ion’s charge.

25. C. Ionic Nomenclature Ionic Names zWrite the names of both ions, cation first. zChange ending of monatomic ions to -ide. zPolyatomic ions have special names. zStock System - Use Roman numerals to show the ion’s charge if more than one is possible. Overall charge must equal zero.

26. C. Ionic Nomenclature zConsider the following: yDoes it contain a polyatomic ion? x-ide, 2 elements  no x-ate, -ite, 3+ elements  yes yDoes it contain a Roman numeral? xCheck the table for metals not in Groups 1 or 2. yNo prefixes!

27. Common Ion Charges 1+ 2+3+NA3-2-1- 0 C. Ionic Nomenclature

28. zpotassium chloride zmagnesium nitrate zcopper(II) chloride  K + Cl   Mg 2+ NO 3   Cu 2+ Cl   KCl  Mg(NO 3 ) 2  CuCl 2 C. Ionic Nomenclature

29. zNaBr zNa 2 CO 3 zFeCl 3 ysodium bromide ysodium carbonate yiron(III) chloride C. Ionic Nomenclature

30. IIIIIIIV Chemical Bonding III. Molecular Compounds

31. A. Energy of Bond Formation zPotential Energy ybased on position of an object ylow PE = high stability

32. no interaction attraction vs. repulsion increased attraction A. Energy of Bond Formation zPotential Energy Diagram

33. balanced attraction & repulsion increased repulsion attraction vs. repulsion A. Energy of Bond Formation zPotential Energy Diagram

34. Bond Energy A. Energy of Bond Formation Bond Length zBond Energy yEnergy required to break a bond

35. A. Energy of Bond Formation zBond Energy yShort bond = high bond energy

36. B. Lewis Structures zElectron Dot Diagrams yshow valence e - as dots ydistribute dots like arrows in an orbital diagram y4 sides = 1 s-orbital, 3 p-orbitals yEX: oxygen 2s2p O X

37. B. Lewis Structures zOctet Rule yMost atoms form bonds in order to obtain 8 valence e - yFull energy level stability ~ Noble Gases Ne

38. ++ -- ++ B. Lewis Structures zNonpolar Covalent - no charges zPolar Covalent - partial charges

39. C. Molecular Nomenclature zPrefix System (binary compounds) 1.Less e - neg atom comes first. 2.Add prefixes to indicate # of atoms. Omit mono- prefix on first element. 3.Change the ending of the second element to -ide.

40. PREFIX mono- di- tri- tetra- penta- hexa- hepta- octa- nona- deca- NUMBER 1 2 3 4 5 6 7 8 9 10 C. Molecular Nomenclature

41. zCCl 4 zN 2 O zSF 6 ycarbon tetrachloride ydinitrogen monoxide ysulfur hexafluoride C. Molecular Nomenclature

42. zarsenic trichloride zdinitrogen pentoxide ztetraphosphorus decoxide yAsCl 3 yN2O5yN2O5 yP 4 O 10 C. Molecular Nomenclature

43. NOF Cl Br I H C. Molecular Nomenclature zThe Seven Diatomic Elements Br 2 I 2 N 2 Cl 2 H 2 O 2 F 2