General Chemistry (I) -------------------------------------------------------

1. General Chemistry (I) ------------------------------------------------------- Instructor: 魏國佐 (Guor-Tzo Wei) Office:數學館524 (05-2428121) Lab: 物理館424 (-61406) Email:chegtw@ccu.edu.tw Website:http://www.ccunix.ccu.edu.tw/~deptche/faculty/gtw.html Office hour: Tue(11:00~13:00) at 化學館424 ----------------------------------------------------------------

2. General Chemistry (I) Course contents: Ch. 1 :Chemical Foundation Ch. 2 : Atoms, Molecules, and Ions Ch. 3: Stoichiometry Ch. 4: Types of Chemical Reactions and Solution Stoichiometry Ch. 5: Gases Ch. 10: Liquids and Solids Mid-term 11/9 19:00 ------ 40% Ch. 11 : Properties of Solution Ch. 13: Chemical Eqillibrium Ch. 14: Acids and Bases Ch. 15: Applications of Aqueous Equillibrium Ch. 18: The Nucleus Final exam. 1/9 19:00 ------ 40% Homework and Quiz ------------------------ 20% Textbook:Chemistry 6/eSteven S. Zumdahl and Susan A. Zumdah

3. Subjects of study_ (研究課題) Life Science (生命科學) Material Science (材料科學) Environmental Science (環境科學) Physical Science (物理科學) Chemistry’s Fields (領域) Physical Chemistry (物理化學) Organic Chemistry (有機化學) Inorganic Chemistry (無機化學) Analytical Chemistry (分析化學) Biochemistry (生物化學) General Chemistry

4. Proteome Researches Nanotechnology Related Researches Optical, Magnetic, Electronic Materials Sustainable (Green) Chemistry etc. 目前熱門研究課題

5. Chapter 2: ATOMS, MOLECULES, AND IONS

6. The Early History of Chemistry • Before 16th Century • Greeks: 4 fundamental substances: fire, earth, water, and air. • Alchemy: Attempts (scientific or otherwise) to change cheap metals into gold. • 17th Century • Robert Boyle: First “chemist” to perform quantitative experiments to measure the relationship between pressure and volume. Define chemical elements: substance cannot further break down. • 18th Century • George Stahl: Phlogiston flows out of a burning material. • Joseph Priestley: Discovers oxygen gas, “dephlogisticated air.” “The Priestley Award” of Am. Chem. Soc.

7. Discovered by Antoine Lavoisier Combustion involves oxygen, not phlogiston Mass is neither created nor destroyed Law of Conservation of Mass In 1789 Lavoisier published the 1st modern chem. textbook: “Elementary Treatise on chemistry”

8. A given compound always contains exactly the same proportion of elements by mass. Copper carbonate is always 5.3 parts Cu to 4 parts O to 1 part C (by mass). Other Fundamental Chemical Laws Law of Definite Proportion (Joseph Proust)

9. Mass of O that contributes with 1 g of C ----------------------------------------------------------------------------- Compound 1 1.33 g Compound II 2.66 g When two elements form a series of compounds, the ratios of the masses of the second element that combine with 1 gram of the first element can always be reduced to small whole numbers. The ratio of the masses of oxygen in CO2 and CO will be a small whole number (“2”). Other Fundamental Chemical Laws Law of Multiple Proportions (by John Dalton)

10. Each element is made up of tiny particles called atoms. The atoms of a given element are identical; the atoms of different elements are different in some fundamental way or ways. Dalton’s Atomic Theory (1808)

11. Chemical compounds are formed when atoms combine with each other.A given compound always has the same relative numbers and types of atoms. Chemical reactions involve reorganization of the atoms- changes in the way they are bound together. The atoms themselves are not changed in a chemical reaction. Dalton’s Atomic Theory(continued)

12. Figure 2.4: A representation of some of Gay-Lussac's experimental results on combining gas volumes.

13. 5 liters of oxygen 5 liters of nitrogen Same number of particles! Avogadro’s Hypothesis (1811) At the same temperature and pressure, equal volumes of different gasescontain the same number of particles.

14. Figure 2.5: A representation of combining gases at the molecular level. The spheres represent atoms in the molecules.

15. J. J. Thomson- postulated the existence of electrons using cathode ray tubes. Ernest Rutherford - explained the nuclear atom, containing a dense nucleus with electrons traveling around the nucleus at a large distance. Early Experiments to Characterize the Atom

16. Figure 2.7: A cathode-ray tube. The fast-moving electrons excite the gas in the tube, causing a glow between the electrodes.

17. Figure 2.8: Deflection of cathode rays by an applied electric field.

18. Figure 2.9: The plum pudding model of the atom.

19. Figure 2.10: A schematic representation of the apparatus Millikan used to determine the charge on the electron.

20. Figure 2.12: Rutherford's experiment on -particle bombardment of metal foil.

21. Figure 2.13: (a) The expected results of the metal foil experiment if Thomson's model were correct. (b)Actual results.

22. Figure 2.14: A nuclear atom viewed in cross section. Note that this drawing is not to scale.

24. Figure 2.15: Two isotopes of sodium. Both have eleven protons and eleven electrons, but they differ in the number of neutrons in their nuclei.

25. Figure 2.16: The structural formula for methane.

26. Figure 2.17: Space-filling model of methane. This type of model shows both the relative sizes of the atoms in the molecule and their spatial relationships.

27. Figure 2.18: Ball-and-stick model of methane.

28. Figure 2.19: Sodium metal reacts with chlorine gas to form solid sodium chloride.

29. Figure 2.20: Ball-and-stick models of the ammonium ion and the nitrate ion.

30. Figure 2.21: The Periodic Table.

34. Crystals of copper(II) sulfate.

35. Various chromium compounds dissolved in water. From left to right; CrCl2, K2Cr2O7, Cr(NO3)3, CrCl3, K2CrO4.

36. Figure 2.22: The common cations and anions

39. Figure 2.23: A flowchart for naming binary compounds.

40. Figure 2.24: Overall strategy for naming chemical compounds.

43. Figure 2.25: A flowchart for naming acids. An acid is best considered as one or more H+ ions attached to an anion.

44. Room Temperature Ionic Liquids 室溫離子液體 (pp 520)

45. Pure Appl. Chem., 2000, 72, 2275–2287

46. RTIL Structures R: methyl; R’: n-butyl • Cations • Anions • PF6-SbF6- • BF4-CF3SO3- (TfO) • Cl-N(CF3SO2)2- (NTf2) 1-butyl-3-methylimidazolium, BMIM, C4MIM 1-butyl-3-methylimidazolium hexafluorophosphate [BMIM][PF6]

47. Effect of the nature of anion on physical properties of BMIM salt ----------------------------------------------------------------------------------- Anion m.p. d Viscosity Conductivity oC g/cm3 cP (20oC) S/m ---------------------------------------------------------------------------------- BF4- -82(g) 1.17 233 0.17 PF6- -8 1.36 312 0.14 Cl- 65 1.10 solid solid CF3COO- ~-40(g) 1.21 73 0.32 CF3SO3- 16 1.29 90 0.37 (CF3SO2)N- -4 1.43 52 0.39 C3F7COO- ~-40(g) 1.33 182 0.10 C4F9SO3- 20 1.47 373 0.045 ---------------------------------------------------------------------------------- (g) Glass transition P.S. viscosity of water 1 cP.

48. Liquid salt consisting of at least one organic component (cation or anion) Room temperature ionic liquid (RTIL) with melting point is below room temperature Properties: Negligible vapor pressure High thermal stability (~250-400°C) High viscosity Hydrophobic or hydrophilic Dissolve many organic, organometallic, and inorganic compounds RTILs are regarding as “Green solvents” What is a Room Temperature Ionic Liquid?(Room Temperature Molten Salt)

49. *Anastas, P. T.; Warner, J. C. Green Chemistry: Theory and Practice, Oxford University Press: New York, 1998, p.30. By permission of Oxford University Press.

50. *Anastas, P. T.; Warner, J. C. Green Chemistry: Theory and Practice, Oxford University Press: New York, 1998, p.30. By permission of Oxford University Press.