• 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

• ----------------------------------------------------------------

• 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

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

目前熱門研究課題

• Proteome Researches

• Nanotechnology Related Researches

• Optical, Magnetic, Electronic Materials

• Sustainable (Green) Chemistry

• etc.

Chapter 2: ATOMS, MOLECULES, AND IONS

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.

The Early History of Chemistry

Law of Conservation of MassLaw 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 LawsOther Fundamental Chemical Laws

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).

Law of Definite Proportion(Joseph Proust)

Other Fundamental Chemical LawsOther Fundamental Chemical Laws

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”).

Law of Multiple Proportions (by John Dalton)

Dalton’s Atomic Theory (1808)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)

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)Avogadro’s Hypothesis (1811)

• 5 liters of oxygen

• 5 liters of nitrogen

• Same number of particles!

At the same temperature and pressure, equal At the same temperature and pressure, equal volumes of different volumes of different gasesgases contain the same contain the same number of particles.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

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. 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. Note that this drawing is not to scale.

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. 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. 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. An acid is best considered as one or more H+ ions

attached to an anion.

Room Temperature Ionic LiquidsRoom Temperature Ionic Liquids室溫離子液體室溫離子液體

(pp 520)(pp 520)

Room Temperature Ionic LiquidsRoom Temperature Ionic Liquids室溫離子液體室溫離子液體

(pp 520)(pp 520)

Pure Appl. Chem., 2000, 72, 2275–2287

RTIL Structures

• Cations

• Anions– PF6

- SbF6-

– BF4- CF3SO3

- (TfO)

– Cl- N(CF3SO2)2- (NTf2)

1-butyl-3-methylimidazolium, BMIM, C4MIM

N N+R R`

R: methyl; R’: n-butyl

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 0.17PF6

- -8 1.36 312 0.14Cl- 65 1.10 solid solidCF3COO- ~-40(g) 1.21 73 0.32CF3SO3

- 16 1.29 90 0.37(CF3SO2)N- -4 1.43 52 0.39C3F7COO- ~-40(g) 1.33 182 0.10C4F9SO3

- 20 1.47 373 0.045----------------------------------------------------------------------------------(g) Glass transitionP.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* 

*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.

1. PreventionIt is better to prevent waste than to treat or clean up waste after it has been created.

2. Atom EconomySynthetic methods should be designed to maximize the incorporation of all materials used in the process into the final product.

3. Less Hazardous Chemical SynthesesWherever 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 ChemicalsChemical products should be designed to effect their desired function while minimizing their toxicity.

5. Safer Solvents and AuxiliariesThe use of auxiliary substances (e.g., solvents, separation agents, etc.) should be made unnecessary wherever possible and innocuous when used.

6. Design for Energy EfficiencyEnergy 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 FeedstocksA raw material or feedstock should be renewable rather than depleting whenever technically and economically practicable.

8. Reduce DerivativesUnnecessary 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. CatalysisCatalytic reagents (as selective as possible) are superior to stoichiometric reagents.

10. Design for DegradationChemical 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 PreventionAnalytical 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 PreventionSubstances 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.