------------------------------------------------------- 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 ----------------------------------------------------------------

Textbook:Chemistry 6/e Steven S. Zumdahl and Susan A. Zumdah 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/e Steven S. Zumdahl and Susan A. Zumdah

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) 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) General Chemistry

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

ATOMS, MOLECULES, AND IONS Chapter 2: ATOMS, MOLECULES, AND IONS

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.

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

Other Fundamental Chemical Laws Law of Definite Proportion (Joseph Proust) 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 Multiple Proportions (by John Dalton) 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”).

Dalton’s Atomic Theory (1808) 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 (continued) 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.

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

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

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

Early Experiments to Characterize the Atom 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.

Figure 2. 7: A cathode-ray tube Figure 2.7: A cathode-ray tube. The fast-moving electrons excite the gas in the tube, causing a glow between the electrodes.

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

Figure 2.9: The plum pudding model of the atom.

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

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

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

Figure 2. 14: A nuclear atom viewed in cross section Figure 2.14: A nuclear atom viewed in cross section. Note that this drawing is not to scale.

Figure 2. 15: Two isotopes of sodium 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.

Figure 2.16: The structural formula for methane.

Figure 2. 17: Space-filling model of methane 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.

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

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

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

Figure 2.21: The Periodic Table.

Crystals of copper(II) sulfate.

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

Figure 2.22: The common cations and anions

Figure 2.23: A flowchart for naming binary compounds.

Figure 2.24: Overall strategy for naming chemical compounds.

Figure 2. 25: A flowchart for naming acids Figure 2.25: A flowchart for naming acids. An acid is best considered as one or more H+ ions attached to an anion.

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

Pure Appl. Chem., 2000, 72, 2275–2287

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

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.

What is a Room Temperature Ionic Liquid? (Room Temperature Molten Salt) 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”

The Twelve Principles of Green Chemistry*   1. Prevention It is better to prevent waste than to treat or clean up waste after it has been created. 2. Atom Economy Synthetic methods should be designed to maximize the incorporation of all materials used in the process into the final product. 3. Less Hazardous Chemical Syntheses Wherever practicable, synthetic methods should be designed to use and generate substances that possess little or no toxicity to human health and the environment. 4. Designing Safer Chemicals Chemical products should be designed to effect their desired function while minimizing their toxicity. 5. Safer Solvents and Auxiliaries The use of auxiliary substances (e.g., solvents, separation agents, etc.) should be made unnecessary wherever possible and innocuous when used. 6. Design for Energy Efficiency Energy requirements of chemical processes should be recognized for their environmental and economic impacts and should be minimized. If possible, synthetic methods should be conducted at ambient temperature and pressure. 7. Use of Renewable Feedstocks A raw material or feedstock should be renewable rather than depleting whenever technically and economically practicable. *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.

8. Reduce Derivatives Unnecessary derivatization (use of blocking groups, protection/ deprotection, temporary modification of physical/chemical processes) should be minimized or avoided if possible, because such steps require additional reagents and can generate waste. 9. Catalysis Catalytic reagents (as selective as possible) are superior to stoichiometric reagents. 10. Design for Degradation Chemical products should be designed so that at the end of their function they break down into innocuous degradation products and do not persist in the environment. 11. Real-time analysis for Pollution Prevention Analytical methodologies need to be further developed to allow for real-time, in-process monitoring and control prior to the formation of hazardous substances. 12. Inherently Safer Chemistry for Accident Prevention Substances and the form of a substance used in a chemical process should be chosen to minimize the potential for chemical accidents, including releases, explosions, and fires. *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.