1. Starter S-53 Mole Day!

2. Starter S-55 What is the value of a mole? What is that number used for?

3. Ionic and Metallic Bonding Chapter 7

4. 7.1 Ions Chapter 7

5. Valence Electrons – highest energy electrons Groups always have the same number of valence electrons 7.1 Ions

6. Valence electrons are related to the group Valence electrons are usually the ones involved in chemical bonding 7.1 Ions

7. Octet Rule Metals tend to lose their valence electrons leaving a complete octet in the next lowest energy level Nonmetals tend to gain or share electrons to complete their octet 7.1 Ions Ionic Bonding

8. Ionic Bonding involves the formation of a Cation – lose electrons Anions – gain electrons 7.1 Ions Formation of Ions

9. Electron configuration change in cation formation 7.1 Ions Al 3s 3p 3d 2s 2p 1s Al +3 Lower Octet

10. Electron configuration change in anion formation 7.1 Ions S 3s 3p 3d 2s 2p 1s S -2 New Octet

11. Oxidation Number – apparent charge in a compound 7.1 Ions

12. Starter S-57 What is an ion? How many electrons does Oxygen need in its outer energy level to be stable? Why does Helium only need two electrons to be stable?

13. 7.2 Ionic Bonds and Ionic Compounds Chapter 7

14. Ionic Compounds – composed of cations and anions One element give electrons to the other element 7.2 Ionic Bonds and Ionic Compounds

15. Writing formulas for ionic compounds The sum of the charges always equals 0 Usually if we flip the number values So the formula would be 7.2 Ionic Bonds and Ionic Compounds

16. Positive ion is always written first Numbers are written after the element and as a subscript The number 1 is never written 7.2 Ionic Bonds and Ionic Compounds

17. Try Aluminum and Oxygen Calculations Formula 7.2 Ionic Bonds and Ionic Compounds

18. Formulas are always given as smallest ratio so Calculations Formula 7.2 Ionic Bonds and Ionic Compounds Pb +4 O -2

19. Formula Unit – the smallest whole number ratio of ions Ionic Compounds are really repeating structures 7.2 Ionic Bonds and Ionic Compounds

20. Properties of Ionic Compounds 1.Most are crystalline solids at room temperature 2.Generally have high melting points 3.Conduct an electric current when melted or dissolved 7.2 Ionic Bonds and Ionic Compounds

21. Starter S-59 What is the formula for 1.Vanadium (VI) and Oxygen 2.Vanadium (V) and Oxygen 3.Lead (IV) and Sulfur 4.Lead (II) and Sulfur

22. 7.3 Bonding in Metals Chapter 7

23. In metals valence electrons are free to move around The individual atoms are free to slide past each other Explains conductivity – electrons are free to move 7.3 Bonding in Metals Bonding Animation

24. Ductility and Malleability – metals free to slide past each other Metals are arranged in compact and orderly crystal patterns Body Centered Cubic-every atom has eight neighbors Na, K, Fe, Cr, W 7.3 Bonding in Metals Crystal Structures

25. Face Centered Cubic – every atom has 12 neighbors Cu, Ag, Au, Al, Pb Hexagonal Close Packed – 12 different pattern Mg, Zn, Cd 7.3 Bonding in Metals

26. Alloys – mixtures composed two or more elements, at least one of which is a metal Sterling silver 92.5% silver, 7.5% copper Harder, more durable than Ag Bronze 87.5% copper, 12.5% tin Harder, more easily cast 7.3 Bonding in Metals

27. Steel Stainless Steel (80.6% Fe, 18.0% Cr, 0.4% C, 1.0 % Ni) Spring Steel (98.6% Fe, 1.0% Cr, 0.4% C) 7.3 Bonding in Metals

28. Surgical Steel (67% Fe, 18% Cr, 12% Ni, 3% Mo) 7.3 Bonding in Metals

29. Starter S-60 What is the chemical formula of A.Iron (III) and Chlorine B.Calcium and Fluorine C.Sodium and Oxygen