A cylinder of copper (8.92 g/cm 3 ) is found to have a mass of 1681 grams.

1. A cylinder of copper (8.92 g/cm3) is found to have a mass of 1681 grams. • The cylinder is 15.0 cm tall. Calculate the radius. (2.0cm) • A rectangular piece of copper has a mass of 0.330 kg. The dimensions are 1.00 cm and a width of 4.000 cm by 9.000 cm. Calculate the experimental density.(9.17g/cm3) • Calculate the percent error. (2.8%) • 3. 1220 J of heat is added to 50.0 grams of water at 25.0oC. • Calculate the change in temperature of the water. (5.8oC) • Calculate the final temperature of the water. (30.8oC) • Convert the heat to kilojoules. (1.22 kJ) • Convert the heat to calories. (292 cal)

2. What type of element is: Ba Br Th S Rb Ti Kr Ce • What year did Mendeleev publish his periodic table? • How is the modern table different than Mendeleev’s? • Why do metals conduct and non-metals do not?

3. John Newlands (1863) Law of octaves – properties repeat every 7 elements

4. John Newlands (1863)

5. John Newlands (1863)

6. Mendeleev (1869) • Dmitri Mendeleev – 1869 • Father of the Periodic Table

7. Mendeleev (1869)

8. Mendeleev (1869) • Major Success - Left spaces where there should be an element

9. Mendeleev (1869) Eka-Silicon - “below silicon” Eka-Silicon(1871) ~72 g/mol Density ~5.5 g/mL Dark Gray Metal EsO2 (4.7 g/mL)

10. Mendeleev (1869) Eka-Silicon(1871) Germanium(1886) ~72 g/mol 72.6 g/mol Density ~5.5 g/mL 5.36 g/mL Dark Gray Metal Dark Gray Metal EsO2 (4.7 g/mL) GeO2 (4.7 g/mL) (Scandium and Gallium predicted also)

12. Mendeleev (1869) Modern Table -Different than Mendeleev’s • Problem with Mendeleev’s table - Arranged his table by atomic mass • Modern table arranged by atomic number (Moseley)

14. Metals Properties a. Solids b. Ductile c. Malleable d. Conduct Electricity and heat e. Large - Tend to lose electrons

18. Non-Metals Properties a. Gases or solids b. Brittle c. Don’t conduct Electricity & heat well d. Essential for Life CHONSP e. Small - Tend to gain electrons

21. Metalloids Properties a. Have properties of both metals and non-metals b. Semi-Conductors - Conduct electricity only if a larger current is applied c. Used in computer chips, cell phones, etc… d. B, Si, Ge, As, Sb, Te

23. Group Names Period – Across Group – Down

24. Group Names

25. States • Standard Temperature = 25oC • Solids – Most Elements Liquids – Hg and Br2 Gases – H2, N2, O2,F2, Cl2 & Noble Gases

29. No Roman # Ionics I. Binary Compounds A. Used for Gr 1 and Gr 2 metals (and Aluminum) B. Metal has only one standard charge C. Rules • Write Metal First • Non-metal becomes “ide”

30. No Roman # Ionics D. Examples NaCl BaO Al2O3 magnesium bromide aluminum sulfide potassium oxide

31. No Roman # Ionics II. Compounds with Polyatomics A. Polyatomic Ion - An Ion with more than one atom (Consider the overall charge) B. Examples Hydroxide Sulfate Nitrate Acetate

32. No Roman # Ionics C. Examples sodium hydroxide sodium carbonate aluminum sulfate NaNO3 Ca(OH)2 (NH4)3PO4

33. No Roman # Ionics D. Mixed Examples magnesium sulfide magnesium sulfite magnesium sulfate lithium phosphide lithium phosphate Ba(ClO3)2 BaCl2

34. Roman # Ionics 1. An example Fe(II)and oxygen Fe(III) and oxygen How do we distinguish? 2. Metals which have multiple oxidation states Transition and post-transition metals

35. Roman # Ionics 3. The Roman Numeral tells you the charge, NOT how many atoms you have. copper(II)nitride copper(III)nitride

36. Roman # Ionics 4. Examples iron (III)bromide tin(II) nitrate cobalt(III)oxide CoCl2 MnO2 Ru2(SO4)3 VO3

37. Roman # Ionics 5. Mixed Examples calcium bromide chromium (III)nitrate aluminum sulfate iron(III)carbonate Li2S CoCl2 Ti3N2 Mg(NO2)2

38. Molecular Naming 1. Prefixes Mono Hexa Di Hepta Tri Octa Tetra Nona Penta Deca May skip “mono” for first element

39. Molecular Naming 2. Examples P4O10 SiO2 CO diphosphorus tetroxide carbon tetrachloride

40. dinitrogen tetroxide dichlorine decoxide carbon disulfide sulfur hexafluoride SeF4 Cl2O7 KrF4 CH4

41. Rev. of All Naming calcium chloride CS2 NO3 silicon dioxide N2O Ba(OH)2 copper(II)carbonate NaI magnesium phosphate K2CO3 dicarbon octahydride HgI2 chromium(III)oxide FeF2 dihydrogen monsulfide PCl5

42. Rev. of All Naming calcium chloride silicon dioxide copper(II) carbonate magnesium phosphate dicarbon pctahydride chromium(III) oxide fluorine pentachloride

43. Oxidation Numbers • Involves taking compounds apart • Oxidation numbers – Pretend charges for all compounds (as if they exist as a monoatomic ion) • Rules

44. Fe H2 P4 Cl2 Elements = 0 Monoatomic Ions = Charge Na+ O2- Al3+ Use “bankables” to calculate the rest H2S Cl2O Na2SO4 PO43- NO3- CaCr2O7 SnBr4 Gr I Gr II O-2 H+ F- “the higher the oxidation #, the more oxidized the element”

45. Calculate the oxidation numbers for: HClO SO32- S8 HSO4- Mn2O3 NO2- KMnO4 SO42- Cr3+ Fe2(SO4)3

46. V2O5 • XeCl4 • Ca(NO3)2 • Barium nitride • Iron(III)carbonate

47. a) N2 d) F2 e) H2 h)Hg2 • a) Br2 b) Ar c) I2 d)H2 or C

48. 19. calcium iodide magnesium phosphide francium fluoride radium sulfide beryllium selenide • KH Cs2S K3P BaTe 23. chromium (III) iodide titanium(IV) chloride iridium(VIII) oxide manganese(II) hydride nickel(II) chloride 25. YH3 BiF5 PbCl4 PaSe

49. sodium oxalate calcium chromate iron(III) carbonate copper(II) hydroxide • Zr3(PO4)4 NaCN TlNO2 Ni(OH)2 Ra(HSO4)2 Be3P2 Cr(ClO)3

50. Ionic (No Roman #) Sodium fluoride (NaF) Lithium phosphate (Li3PO4) Sodium carbonate (Na2CO3) Aluminum sulfide (Al2S3) Barium nitrate (Ba(NO3)2) Sodium bicarbonate (NaHCO3) Barium nitride (Ba3N2) Potassium hydrogen sulfate (KHSO4) Potassium permangante (KMnO4) Sodium hydroxide (NaOH)