Chemical Analysis

Spring, 2011 by

駱碧秀老師

• When & Where: 9:10-12:00 (Mon. at M0301)• Office ： 醫學大樓 6F，自然科共同實驗室，分機： 5018 • 教學網站： http://memo.cgu.edu.tw/bih-show/

• E-mail: blou@mail.cgu.edu.tw

• Office Hours: Wed. 16:10-18:00

Lecture & Assignment Schedule• Week Date Topics• 1 2/21 Introduction & Naming Compounds • 2 2/28 Holiday• 3 3/07 Chapter 3 Math Toolkit• 4 3/14 Chapter 4 Statistics• 5 3/21 Chapter 9~10 Buffers & Titrations• 6 3/28 Chapter 11 Polyprotic Acids & Bases• 3/30 期中考 I （工六第一會議室） 18:00-21:00• 7 4/04 Holiday• 8 4/11 Chapter 18 Let There Be Light• 9 4/18 Molecular Orbital• 10 4/25 Chapter 19 Spectrometry• 11 5/02 Chapter 14 Electrochemistry• 12 5/09 Chapter 15 Electrode Measurements• 5/11期中考 II（工六第一會議室） 18:00-21:00• 13 5/16 Chapter 13 Coordination Chemistry & EDTA Titrations• 14 5/23 Chapter 21 Principles of Chromatography• 15 5/30 Chapter 22 GC & LC• 16 6/06 Holiday • 17 6/13 Chapter 23 Capillary Electrophoresis• 18 6/20 期末考 （工六第一會議室） 9:00-12:00

Text Book

Daniel C. Harris,

“Exploring Chemical Analysis”, 4th Edition, 2009

by W.H. Freeman & Company.

Grade:• 作業 : 5 %• 小考 : 10% • 期中考 I : 25%• 期中考 II& 期末考 : 各 30%

「成績，不只是在於你知道什麼，而在於你表現什麼。」

成功法則第一招：一定要來上課！

For most its users, analytical chemistry is a tool – not an end in itself.

If you are interested in biology, medicine, environmental science, geology, oceanography, or archeology, you will rely on chemical analyses to answer important questions.

It is possible that you will make measurements yourself, but it is more likely that you will simply be a consumer of analytical results.

What Am I Doing in This Course?

Goals of this course

(1) To understand how analysts derive the results that you will use.

(2) To understand the limitations (the uncertainties) of the results.

(3) To develop laboratory skills and careful work habits that you can apply in your field.

This course will help you, as an informed citizen.

To appreciate how quantitative information is obtained and interpreted.

And it should help give you a basis for positive actions in your own field of interest.

How do you measure the caffeine content of a chocolate bar ?

Theobromine Diuretic, smooth muscle relaxant, cardiac stimulant, and vasodilator

Caffeine Central nervous system stimulant and diuretic

Extracting fat from chocolate

Centrifugation & Filtration

Chemical Analysis

Calibration

Results:

FYI:

General Steps in a Chemical Analysis

1) Formulation the question

2) Selecting analytical procedures

3) Sampling

4) Sample preparation

5) Analysis

6) Reporting & interpretation

7) Drawing conclusions

Naming Simple Compounds IUPAC - I

1. Binary compounds (Type I ; ionic)1) cation + anion (ide)

Left right

2) See Table 1 & example : NaCl

sodium chlorine ide

2. Binary compounds (Type II ; ionic)– for metals with more than one type of ion– Table 2 -ic / -ous– exception : IA , IIA , Al3+ , Zn2+ , Ag+

Table 1 Common Monatomic Cations and Anions

Cation Name Anion Name

H+ hydrogen H- hydride

Li+ lithium F- fluoride

Na+ sodium Cl- chloride

K+ potassium Br- bromide

Cs+ cesium I- iodide

Be2+ beryllium O2- oxide

Mg2+ magnesium S2- sulfide

Ca2+ calcium N3- nitride

Ba2+ barium P3- phosphide

Al3+ aluminum

Ag+ silver

Zn2+ zinc

Table 2 Common Type II Cations

Ion Systematic Name Alternate Name

Fe3+ iron (III) ferric

Fe2+ iron (II) ferrous

Cu2+ copper (II) cupric

Cu+ copper (I) cuprous

Co3+ cobalt (III) cobaltic

Co2+ cobalt (II) cobaltous

Sn4+ tin (IV) stannic

Sn2+ tin (II) stannous

Pb4+ lead (IV) plumbic

Pb2+ lead (II) plumbous

Hg2+ mercury (II) mercuric

Hg22+ * mercury (I) mercurous

* Note that mercury (I) ions always occur bound together to from Hg22+.

Naming Simple Compounds IUPAC - II

3. Polyatomic ions1) NH4NO3 NH4

+ + NO3-

2) Table 3 (memorized !!)

3) O : hypo- / -ite / -ate / per-

4. Binary compounds (Type III ; covalent : nonmetals)– see p.39-40 for rules & examples

– H2O (water) , NH3 (ammonia) , CH4 (methane)

– Table 4

Table 3 Commmon Polyatomic Ions

Ion Name Ion Name

NH4+ ammonium CO3

2- carbonate

NO2- nitrite HCO3

- hydrogen carbonate

(bicarbonate is a widely used common name)

NO3- nitrate

SO32- sulfite

SO42- sulfate ClO- hypochlorite

HSO4- hydrogen sulfate

(bisulfate is a widely used common name)

ClO2- chlorite

ClO3- chlorate

ClO4- perchlorate

OH- hydroxide C2H3O2- acetate

CN- cyanide MnO4- permanganate

PO43- phosphate Cr2O7

2- dichromate

HPO42- hydrogen phosphate CrO4

2- chromate

H2PO4- dihydrogen phosphate O2

2- peroxide

Table 4 Prefixes Used to Indicate Number in Chemical Names

Prefix Number Indicated

mono 1

di- 2

tri- 3

tetra- 4

penta- 5

hexa- 6

hepta- 7

octa- 8

Naming chemical compounds

Naming acids

Chapter 1 Chemical Measurements

• Microelectrode by Optical Micrograph

SI units

Ex: Exocytosis of Neurotransmitters

• 1ppm ～ 1ug/mL• 1ppb ～ 1 ng/mL

Parts per Million and Parts per BillionParts per Million and Parts per Billion• Concentrations of trace components of a

sample can be expressed as parts per million (ppm) or parts per billion (ppb), terms that mean grams of substance per million or billion grams of total solution or mixture.

P. 29

Figure 1-6 A volumetric flask contains a specified volume when the liquid level is adjusted to the middle of the mark in the thin neck of the flask.

1-4 Preparing Solution