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
Ionic and Metallic Bonding

4. Chapter 7
7.1 Ions

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

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

7. 7.1 Ions
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
Ionic Bonding

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

9. Al3+ Al 7.1 Ions Electron configuration change in cation formation
3s 3p 3d
2s 2p 1s
Lower Octet

10. S2- S 7.1 Ions Electron configuration change in anion formation
3s 3p 3d
2s 2p 1s
New Octet

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

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
7.2 Ionic Bonds and Ionic Compounds

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

15. 7.2 Ionic Bonds and Ionic Compounds
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

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

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

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

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

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

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

22. Chapter 7
7.3 Bonding in Metals

23. 7.3 Bonding in Metals
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
Bonding Animation

24. 7.3 Bonding in Metals
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
Crystal Structures

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

26. 7.3 Bonding in Metals
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

27. 7.3 Bonding in Metals 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)

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

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