1. Lesson 7 Chemical Bonding Anything in black letters = write it in your notes (‘knowts’)

2. Review… Elements in the same column have similar properties because… they have the same number of valence electrons electrons in the highest energy level

3. variable

4. Lewis Symbol – show valence electrons as dots around chemical symbol C Na O Br Section 1 – Ionic & Covalent Bonding

5. Lewis Symbols of Some Group A Elements Period Group 1A2A3A4A5A6A7A8A 1 2 3 4

6. Octet Rule – Atoms will gain or lose electrons to have 8 valence electrons. metals lose e - ; to form ca+ions nonmetals tend to gain e - ; to form anions

7. Normal Ion Charges

8. Ionic bonds are formed by electron transfer. (between metal & nonmetal) Covalent bonds are formed by electron sharing. (between 2 nonmetals) The more electronegative element acquires most of the e - charge

9. Ionic compounds consist of cations and anions arranged in repeating patterns; NOT as molecules A formula unit is the lowest ratio of ions in an ionic compound.

10. O2O2 H2H2 double bond single bond Each atom shares e - with another to complete the octet. Covalent Bond

11. IONIC COVALENT transfer of e- (ions!) sharing of e- (COvalent) formula units molecules metal & nonmetal 2 nonmetals high melting points low melting points (most are gases or liquids at room temp) conduct e - when molten or dissolved (aqueous) (solid crystals at room temp) COMPOUNDS

12. Collection of water molecules Molecule of water Chemical formulaH2OH2O Array of sodium ions and chloride ions Formula unit of sodium chloride Chemical formulaNaCl FORMULA UNITS vs.MOLECULES

13. Covalent bonding involves a sharing of electrons between atoms but this sharing may not be equal… Section 2 – Polar Covalent Bonding First, a review of electronegativity….

14. Noble gases do not have e-neg values Electronegativity Review… B<H<C

15. A nonpolar covalent bond occurs between 2 identical atoms. Since each atom in a nonpolar bond has the same electronegativity, the electrons are shared equally. 7 nonpolar (diatomic) molecules (H 2, N 2, O 2, F 2, Cl 2, Br 2, I 2 )

16. Polar Covalent Bond (polar bond) – covalent bond in which the electrons are shared unequally. The more electronegative atom attracts electrons more and has a slightly negative charge ( δ - ) δ-δ- δ+δ+ partial positive charge partial negative charge

17. partial positive charge partial negative charge HCl δ-δ- δ+δ+ H A bond or molecule with +/- charged ends is also called a dipole. “die-pull”

18. The polar nature of a bond can also be shown by an arrow pointing to the more electronegative atom. H—Cl Identify the bonds between these elements as ionic, polar covalent or nonpolar covalent. a)H – Br b) K – Cl c)C – O d) Li – O e)Cl – F f) Br – Br g)H – Oh) H – Br Place a δ - symbol above the more electronegative atom in the bond.

19. If the polar bonds in a molecule cancel out, the molecule is nonpolar. When the polar bonds do NOT cancel out, the molecule is polar.

20. We will not cover molecular geometries and shapes except for that of water… unshared pairs of e - H2OH2O (lone or nonbonding pair) A molecule of water has a bent shape due to the space needed by the lone pairs of e -

21. So far, we have talked about bonding between atoms (ionic, covalent) Now, we will talk about bonding between molecules The bonds between separate molecules are much weaker than ionic or covalent bonds, but without these forces there would be no liquids or solids. Section 3 – Bonding Between Molecules

22. Forces between separate molecules are called Intermolecular Forces (or Van der Waals Forces) 2 types of intermolecular forces that we will discuss, Hydrogen Bonding Dispersion Forces (London Forces)

23. Hydrogen Bond – intermolecular force between H in one molecule and an electronegative atom (N, O or F) in another nearby molecule. Hydrogen Bonds in H 2 O

24. Opposites partial poles attract hydrogen bond

26. Dispersion Forces – temporary attractive forces between molecules due to electron dispersion (motion) F 2 melts at 53 K, Boils at 85 K Without dispersion forces, nonpolar molecules could never be liquids or solids.

27. MoleculeMelt PtBoil Pt F 2 53 K85 K Cl 2 171.6 K239.1 K Br 2 265.8 K332.0 K I 2 386.8 K457.4 K Dispersion Force

28. Cohesion – attraction to same substance. Adhesion – attraction to different substance

29. butane (C 4 H 10 ) 58 amu acetone (C 3 H 6 O) 58 amu b.p. = -0.5°C gas @ room temp b.p. = 56.1°C liquid @ room temp A tale of two molecules… 1. Why does acetone have a higher boiling point? 2. What would cause butane molecules to stick to each other to become a liquid

30. Why does acetone have a higher boiling point? the opposite partial charges on each molecule hold the molecules together. δ+δ+ δ-δ- δ+δ+ etc… butane is a nonpolar molecule and does not have this type of intermolecular attraction

31. 2. What would cause butane molecules to stick to each other to become a liquid? butane, like all molecules, has electrons that are randomly moving. This produces temporary poles within the molecule.

32. The valence electrons in metals are loosely held and are free to move. The properties of metals can be explained by the ‘sea of electrons’ model. Section 4 – Metallic Bonding

33. Alloy – mixture of metals. Steel – Stainless Steel – Bronze – Solder – Brass – Sterling Silver – Amalgam – Nichrome – Alloy – mixture of metals. Steel – Fe & C Stainless Steel – steel w/ Cr, Ni, or Mn Bronze – Cu & Sn Solder – Sn & Pb Brass – Cu & Zn Sterling Silver – Ag & usually Cu Amalgam – Hg w/ other metals (Ag, Sn, Cu) Nichrome – Ni & Cr