1. Chemistry Chapter 5 The Periodic Law

2. Mendeleev’s Periodic Table Dmitri Mendeleev

3. Modern Russian Table

4. Chinese Periodic Table

5. Stowe Periodic Table

6. Spiral Periodic Table A Spiral Periodic Table

7. Triangular Periodic Table

8. “Mayan” Periodic Table

9. Orbital filling table

10. IUPAC naming system with Roman numerals And CAS naming system with letters

11. Periodic Table with Group Names

12. The Periodic Law

13. Properties of Metals  Metals are good conductors of heat and electricity  Metals are malleable (can be hammered into thin sheets)  Metals are ductile (can be pulled into wires)  Metals have luster  Metals tend to lose electrons in order to bond with other elements

14. Examples of Metals Potassium, K reacts with water and must be stored in kerosene Zinc, Zn, is more stable than potassium Copper, Cu, is a relatively soft metal, and a very good electrical conductor. Mercury, Hg, is the only metal that exists as a liquid at room temperature

15. Metal Alloys  Substitutional Alloy: some metal atoms replaced by others of similar size. brass = Cu/Zn

16. Propertiesof Nonmetals Properties of Nonmetals Carbon, the graphite in “pencil lead” is a great example of a nonmetallic element.  Nonmetals are poor conductors of heat and electricity  Nonmetals tend to be brittle  Many nonmetals are gases at room temperature  Nonmetals tend to gain electrons to bond

17. Examples of Nonmetals Sulfur, S, was once known as “brimstone” Microspheres of phosphorus, P, a reactive nonmetal Graphite is not the only pure form of carbon, C. Diamond is also carbon; the color comes from impurities caught within the crystal structure

18. Sulfur – S 8

19. Phosphorus – P 4

20. Allotropes -Different forms of the same element. Example: Carbon’s allotropes are diamond, graphite and buckminsterfullerene

21. Buckminsterfullerene

22. Graphite

23. Diamond

24. Some nonmetals exist as diatomic molecules:Br 2, I 2,N 2, Cl 2, H 2, O 2, F 2 Fluorene, F 2 Chlorine Cl 2 Bromine, Br 2 Nitrogen, N 2 Oxygen, O2 Iodine, I 2 Hydrogen, H 2 (Pop test) BrINClHOF

25. Properties of Metalloids Metalloids straddle the border between metals and nonmetals on the periodic table.  They have properties of both metals and nonmetals.  Metalloids are more brittle than metals, less brittle than most nonmetallic solids  Metalloids are semiconductors of electricity  Some metalloids possess metallic luster  Metalloids tend to lose or gain electrons to bond

26. Silicon, Si – A Metalloid  Silicon has metallic luster  Silicon is brittle like a nonmetal  Silicon is a semiconductor of electricity Other metalloids include:  Boron, B  Germanium, Ge  Arsenic, As  Antimony, Sb  Tellurium, Te

27. Half of the distance between nucli in covalently bonded diatomic molecule "covalent atomic radii" Periodic Trends in Atomic Radius Radius decreases across a period Increased effective nuclear charge due to decreased shielding Radius increases down a group Addition of principal quantum levels Determination of Atomic Radius:

28. Table of Atomic Radii

29. Increases for successive electrons taken from the same atom Tends to increase across a period Electrons in the same quantum level do not shield as effectively as electrons in inner levels Irregularities at half filled and filled sublevels due to extra repulsion of electrons paired in orbitals, making them easier to remove Tends to decrease down a group Outer electrons are farther from the nucleus Ionization Energy - the energy required to remove an electron from an atom

30. Ionization of Magnesium Mg + 738 kJ  Mg + + e - Mg + + 1451 kJ  Mg 2+ + e - Mg 2+ + 7733 kJ  Mg 3+ + e -

31. Table of 1 st Ionization Energies

32. Another Way to Look at Ionization Energy

33. Affinity tends to increase across a period Affinity tends to decrease as you go down in a period Electrons farther from the nucleus experience less nuclear attraction Some irregularities due to repulsive forces in the relatively small p orbitals Electron Affinity - the energy change associated with the addition of an electron

34. Table of Electron Affinities

35. Ionic Radii Cations Positively charged ions Smaller than the corresponding atom Anions Negatively charged ions Larger than the corresponding atom

36. Summation of Periodic Trends

37. Table of Ion Sizes

38. Electronegativity A measure of the ability of an atom in a chemical compound to attract electrons Electronegativities tend to increase across a period Electronegativities tend to decrease down a group or remain the same

39. Periodic Table of Electronegativities