1. Basic Chemistry 基础化学 主讲人：Xiuli Dong 董秀丽 副教授 Office：实验楼B楼 213
董秀丽 副教授
Office：实验楼B楼 213
Tel： QQ:

2. Course Teachers Xiuli Dong 董秀丽 (15h, 3 weeks )
Wei Hu 胡威 (15h, 3 weeks )
Xiaoyan Wang 王晓艳 (10h, 2 weeks )
Yuling Huang 黄玉玲 (10h, 2 weeks )
Huaibin Zhang 张怀斌 (10h, 2 weeks )

3. Notices Language: English and Chinese Question anytime and anywhere
Method: memorize based on understanding
Notice: focal points
Exercises:

4. 1. the Textbook

5. 2. the main contents Atomic Structure Molecular Structure
Osmotic Pressure of Solutions
Rates and Mechanisms of Chemical Reactions
Basic chemistry
Electrolyte Solutions
Organic chemistry
Buffer Solutions
Coordination Complexes

6. 3. Course Schedule for Basic Chemistry

8. Chapter 1 Introduction 1.1 Introduce to Chemistry
1.2 Measurement and SI Units
1.3 Ways of Expressing Concentration
1.4 Names and Symbols of the Elements
1.5 Nomenclature Inorganic Compounds
Key points: Express the concentration of a solution in several different ways (such as molarity, molality, mole fraction )

9. 1.1 Introduce to Chemistry
1.1.1 What is chemistry?
Term:
The dictionary defines chemistry as "the science of the composition, structure, properties, and reactions of matter, especially of atomic and molecular systems."
Chemistry is the study of matter and its interactions with other matter and with energy.

10. 2. Why do we study chemistry?
Every material thing is a chemical or a mixture of chemicals.
Chemistry is central to all branches of science.
Specialized steels in bicycles
Liquid crystals in computer screens
High-tension polymers in synthetic hip joints

11. Ronald Breslow: Chemistry Today and Tomorrow—The Central, Useful, and Creative Science
Considering the importance of chemistry for understanding life, and the importance of medicinal chemistry for health, it is no surprise that the normal education of physicians involves a lot of chemistry. … Modern doctors need to prepare for a future in which chemistry plays an even larger role in human health.
R. Breslow is Professor of Chemistry at Columbia University and the President of the American Chemical Society.

12. 1.4 Names and Symbols of the Elements

13. 1.2 Names and Symbols of the Elements
(Periods 1 and 2)
Hydrogen H
Helium He
Lithium Li
Beryllium Be
Boron B
Carbon C
Nitrogen N
Oxygen O
Fluorine F
Neon Ne

14. (Periods 3) Sodium Na 22.989768 Magnesium Mg 24.3050
Aluminum Al l539
Silicon Si
Phosphorus P
Sulfur S
Chlorine Cl
Argon Ar

15. (Periods 4) Potassium K 39.0983 Calcium Ca 40.078
Scandium Sc
Titanium Ti
Vanadium V
Chromium Cr
Manganese Mn
Iron Fe
Cobalt Co
Nickel Ni

16. (Periods 4 (continued))
Copper Cu
Zinc Zn
Gallium Ga
Germanium Ge
Arsenic As l59
Selenium Se
Bromine Br
Krypton Kr

17. SI units
Units are standards that are used for quantitative comparison between measurements for the same type of quantity.
The first measurements were probably based on the human body.
In 17th and 18th centuries, scientists found that the lack of standard units was a problem.

18. Our current system of measurement, the metric system, began in 1790 when the National Assembly of France set up a committee to establish consistent unit standards.
In 1960, another international committee met in France to establish the International System of Units, a revised metric system now accepted by scientists throughout the world.
The units of this system are called SI units, from the French Système International d'Unités.

19. The SI system is based on a set of 7 fundamental units, or base units, each of which is identified with a physical quantity.
All other units, called derived units, are combinations of these seven base units. For example, the unit for speed, meters per second (m/s), is the unit for length (m) divided by the unit for time (s).
For quantities that are much smaller or much larger than the base unit, we use decimal prefixes and scientific notation (A×10n ).

20. 1.3.1 SI Base Units and SI Prefixes
Table 1 SI Base Units
Quantity
Unit
Symbol
Chinese
Length
meter m 米
Mass
kilogram kg 千克
Time
second s 秒
Temperature
kelvin K
开尔文
Amount of substance
mole
mol 摩尔
Electric current
ampere A 安培
Luminous intensity
candela cd
坎德拉

21. 1.3.2 SI Base Units and SI Prefixes
Table 2 SI Prefixes
Multiple
Prefix
Symbol
1018
exa E
10-1
deci d
1015
peta P
10-2
centi c
1012
tera T
10-3
milli m
109
giga G
10-6
micro μ
106
mega M
10-9
nano n
103
kilo k
10-12
pico p
102
hecto h
10-15
femto f 10
deka da
10-18
atto a
For example: km、m、dm、cm、mm、μm、nm； s、ps、fs
千米、米、分米、厘米、毫米、微米、纳米；秒、皮米、飞米

22. 1.3.3 Some Important SI Units in Chemistry
Length and Mass
The meter (m) is the SI base unit of length. By combining it with one of the SI prefixes, you can get a unit of appropriate for any length measurement. the nanometer (nm): 1nm=10–9m
The kilogram (kg) is the SI base unit of mass. In forming other SI mass units, prefixes are added to the word gram (g) to give units such as the milligram (1mg=10 –3g).

23. Volume (derived unit):
Volume is the space that a given quantity of matter occupies.
The SI unit for volume is the cubic meter (m3). Since this is a rather large volume for typical laboratory situations, the metric unit, known as the liter, is used.
One liter is defined as the exact volume of one cubic decimeter (i.e. 1 L = 1 dm3 = 10 –3 m3).
On a smaller scale, one milliliter is the exact volume of one cubic centimeter
(1 mL = 1 cm3 = 1 cc = 10 –6 m3).

24. Temperature (derived unit):
The Celsius scale is defined by assigning the freezing point of water a value of 0℃ and the boiling point of water as 100℃. （摄氏温度）
The relationship between Celsius and Kelvin temperature is
TK= TC
T = t
开尔文温度 = 摄氏温度

25. New Words solution 溶液 solute 溶质 solvent 溶剂 dissolve 溶解 dilute 稀的
concentrated 浓的
concentration 浓度
mole 摩尔
liter 升
milliliter 毫升
molar mass 摩尔质量
amount of substance 物质的量
molarity 物质的量浓度
molality 质量摩尔浓度
mole fraction 摩尔分数

26. 1.4 Ways of expressing concentration （溶液的组成标度）
The concentration of a solute is the amount of solute dissolved in a given quantity of solvent or solution.
The quantity of solvent or solution can be expressed in terms of volume or in terms of mass or molar amount.
Thus, there are several ways of expressing the concentration of a solution, such as molarity, molality and mole fraction.

27. The Mole Concept
mol（摩尔）
Definition: The mole is the SI unit for amount of substance. It is defined as the quantity of a given substance that contains as many entities (molecules or formula units) as the number of atoms in exactly 12 g of carbon-12. This number is called Avogadro’s number and has a value of 6.02×1023 units/mol.
1 mol=12g of 12C=6.02×1023 units

28. 1 mol H2 contains 6.02×1023 H2 molecules.
Notice: When using the term mole, it is important to specify the formula of unit to avoid any misunderstanding.
For example,
1 mol H contains 6.02×1023 H atoms.
1 mol H+ contains 6.02×1023 H ions.
1 mol H2 contains 6.02×1023 H2 molecules.
1 mol H mol H
1 mol H2SO mol H+
mol SO42-

29. Problems
What’s the relationsship between the number of the moles and the weight ?
For example,
98 grams of H2SO4 is equivalent to one mole of H2SO4, we can write the following relationship:
49 grams of H2SO4 is equivalent to 0.5 mole of H2SO4, we can write the following relationship:

30. Molar mass = Formula weight
Definition: The molar mass of any substance is the mass (in gram) of one mole of that substance.
mass kg, g MB
def
mB/ nB
Molar mass
kg•mol-1, g•mol-1
Mole mol
Conclusion: For all substances, the molar mass in grams per mole equal to the formula weight in atomic mass grams.
Molar mass = Formula weight

31. nNaOH mNaOH/MNaOH Interconverting Moles and Mass:
Example 1 Conversion of Mass to Mole
(a)How many moles of NaOH are present in 80g?
(b)How many moles of O2 are present in 16g?
(c)How many moles of O are present in 16g?
Procedure
Write down what you have been given.
Find the molar mass (molecular weight ) of the molecule.
Calculate the moles of the molecule.
nNaOH
mNaOH/MNaOH
80 / 40
2 mol

32. 1.4.2 Molarity- Molar Concentration
(摩尔浓度，物质的量浓度)
Definition: The molarity of a solution is the moles of solute in a liter of solution.
Mole of the sulute, mol
Molarity
mol•m-3, mol•L-1, mmol•L-1,μmol•L-1 cB
def
nB/ V
Volume of the sulution m3, L
c(C6H12O6) = 3.9 mmol•L-1 ~ 5.6 mmol•L-1

33. nNaCl mNaCl/MNaCl cNaCl nNaCl/V
Example2 Calculating Molarity of a Solution
What is the molarity of a solution prepared by dissolved 4.5 g of NaCl in enough water to form 500 mL of solution?
Procedure
Write down the formula for molarity and what you have been given.
Convert the mass of solute to moles of solute by using the molar mass.
Calculate the molarity.
nNaCl
mNaCl/MNaCl
4.5 / 58.5
0.077 mol
cNaCl
nNaCl/V
0.077 / 0.500
0.154 mol•L-1

34. cd cc·Vc / Vd Dilution of Concentrated Solution
When a solution is diluted, the volume is increased by adding more solvent and the concentration is decreased, but the total amount of solute is constant.
cc·Vc = cd ·Vd = n
Example 3 Calculation of Molarity of a Dilute Solution
What is the molarity of a solution of KCl that is prepared by dilution of 855 mL of a mol•L-1 solution to a volume of 1.25 L? cd
cc·Vc / Vd
0.475*0.855 / 1.25
0.325 mol•L-1

35. Conversion of Mass Percent of Solute to Molarity
Example 4 Calculation of Molarity from Mass Percent
Concentrated laboratory acid is 35.0% by mass HC1 and has a density of 1.18 g/mL. What is its molarity?
Conclusion:

36. Procedure
You can get mass of solute in 100 g of solution using definition of mass percent.
Convert the mass of solution to volume of solution by using the density.
Convert the mass of solute to moles of solute by using the molar mass.
Write down the formula for molarity and what you have been given.
Calculate the molarity.

37. Chapter 2 Colligative Properties of Solutions(稀溶液的依数性)
Introduction
Injection of a hypertonic solution into the blood stream will cause crenation, while a hypotonic solution will cause hemolysis. Why?
Solution
Concentration
Vapor pressure lowering
Colligative
properties
Boiling point elevation
Freezing point depression
Osmosis and osmotic pressure

38. Key points:
To relate the osmosis and osmotic pressure to the concentrations of solution
To calculate osmotic pressure of electrolytes and nonelectrolytes
To understand the importance of osmosis in medicine

39. New Words osmolarity 渗透浓度 electrolyte 电解质 isotonic 等渗的
hypotonic 低渗的
hypertonic 高渗的
hemolysis 溶血
electrolyte 电解质
nonelectrolyte 非电解质
osmosis 渗透
osmotic pressure 渗透压
semipermeable membrane半透膜

40. 2.4 Osmosis and Osmotic Pressure of Solutions （溶液的渗透与渗透压）
Case 1 Isotonic solution
Surrounding sol’n at 9 g/L NaCl
Red blood cells normal.
Case 2 Hypotonic solution
Surrounding sol’n less than 9g/L NaCl
Red blood cells rupture. Hemolysis
Case 3 Hypertonic solution
Surrounding sol’n more than 9g/L NaCl
Red blood cells shrivel. Crenation

41. Problems What’s the Osmosis and Osmotic Pressure? 2.4.1 Osmosis （渗透）
Experiment:
On the left is a pure solvent, and on the right, a solution. The two are separated by a semipermeable membrane. As a result, the water level rises on the right and drops on the left.

42. Term:
Semipermeable membrane -Certain membranes allow solvent molecules to pass through them but not solute molecules.
Osmosis -When a solution and its pure solvent are separated by a semi-permeable membrane, the pure solvent will diffuse through the membrane and dilute the solution.
This process is known as osmosis.

43. Problems
Why?
Solvent molecules can pass through the membrane in both directions, but the concentration of water is larger in the pure water, more water molecules strike the membrane per second on that side, and more water moves into the solution than leaves it.

44. Problems If a solution of lower C and a solution of higher C
are separated by a semi-permeable membrane, will there be the osmosis? Why?
Concentrated solution
Dilute solution
Semipermeable membrane

45. Problems Problems Condition ? Direction ? a semipermeable membrane
Concentrated solution
Dilute solution
Semipermeable membrane
a semipermeable membrane
solutions of different C on either side of the membrane
Problems
Direction ?
from a solvent system to a solution system
from the solution of lower C to the solution of higher C

46. 2.4.2 Osmotic pressure（渗透压）
Term: The amount of pressure that must be exerted just to prevent net transport of solvent across a semipermeable membrane is the osmotic pressure.
Symbol: π
Unit:Pa (kPa)

47. Problems How to calculate the osmotic pressure ? Π = cB RT
Van’t Hoff equation：
the gas constant
8.314 J • K-1 • mol-1
the absolute temperature, K
Osmotic pressure
kPa
Π = cB RT
Molarity of solutions
mol• L-1

48. 1:1 NaCl→ Na++Cl- total m = 2 cB 1:2 CaCl2→ Ca2++ 2Cl- total m = 3 cB
Attention: cB is the total molarity of all the dissociated solute species present.
Nonelectrolyte(非电解质): total molarity =cB
Electrolyte (电解质): total molarity = i cB
1:1 NaCl→ Na++Cl- total m = 2 cB
1:2 CaCl2→ Ca2++ 2Cl- total m = 3 cB

49. Nonelectrolyte (非电解质)
Example1 When 2.00 g of sucrose (蔗糖，C12H22O11) is dissolved in 50.0 mL of water solution, what is the osmotic pressure at 37℃? 解：

50. Π ＝ i cBRT Electrolyte (电解质): Π ＝ i cBRT
Example 2 The 9.0 g ·L-1 salt (NaCl) solution is called physiological saline. What is the osmotic pressure at 37℃? 解：
Π ＝ i cBRT

51. The red blood cells in different molarity solutions
2.4.3 Importance of Osmosis (osmotic pressure) in medicine
Why？
physiological saline
Less than 9 g/L
more than 9 g/L
The red blood cells in different molarity solutions

52. cos nos/ V 2.4.3.1 Osmolarity(渗透浓度) Term:
osmotically active substances（渗透活性物质）：In body fluids, there are ions, small molecules, and large molecules. All these substances have an osmotic effect.
osmolarity -the total molarity of osmotically active substances
cos
def
nos/ V

53. cos
def
nos/ V
Example 3 What is the osmolarity of (1) 50.0 g ·L-1 glucose (C6H12O6) solution and (2) 9.0 g ·L-1 salt (NaCl) solution ?

54. Example 4 The 0. 4 mol. L-1 glucose (C6H12O6) solution 1L and 0. 2 mol
Example 4 The 0.4 mol.L-1 glucose (C6H12O6) solution 1L and 0.2 mol.L-1 salt (NaCl) solution 1L are mixed with each other. What is the osmolarity of the final solution?

55. 2.4.3.2 isotonic, hypertonic and hypotonic sulutions
Standard: blood plasma
hypotonic
isotonic
hypertonic
280 mmol.Ｌ-1
320 mmol.Ｌ-1
Terms:
Isotonic: two solutions with the same  separated by a semipermeable membrane.
Hypertonic: having a higher osmotic pressure
Hypotonic: a solution of lower  than a isotonic solution.

56. Isotonic solution: 0.9% (9g/L) NaCl
Red blood cells:
osmolarity = 0.306mol/L
0.9% (9g/L) NaCl
osmolarity = 2×9g/L /58.5g/mol =0.306mol/L
Red blood cells normal.

57. Hypotonic solution: 0.5% (5g/L) NaCl
Red blood cells: osmolarity = 0.306mol/L
5g/L NaCl:
osmolarity = 0.171mol/L
Hemolysis (溶血): red blood cells placed in a hypotonic solution (relative to intracellular solution); there is a higher solute concentration in the cell; osmosis occurs and water moves into the cell. The cell bursts.

58. Hypertonic solution: 1.5% (15g/L) NaCl
Red blood cells: osmolarity = 0.306mol/L
15g/L NaCl:
osmolarity = 0.513mol/L
Crenation（血栓）: red blood cells placed in hypertonic solution (relative to intracellular solution); there is a lower solute concentration in the cell than the surrounding tissue; osmosis occurs and water passes through the membrane out of the cell. The cell shrivels up.

59. Conclusion:
For intravenous feeding, it is necessary that the nutrient solution have exactly the osmotic pressure of blood plasma. If it does not, the blood cells may collapse or burst as a result of osmosis.
To prevent crenation or hemolysis, solutions must be isotonic.
Range of Isotonic Solution: 280 ~ 320 mmol·L-1
Isotonic Solution: physiological saline solution (9g/L NaCl), 50g/L glucose
Standard: blood plasma

60. Problems Examples of osmosis?
Limp carrot placed in water becomes firm because water enters via osmosis.
Salty food causes retention of water and swelling of tissues (edema).
Water moves into plants through osmosis.
Salt added to meat or sugar to fruit prevents bacterial infection (a bacterium placed on the salt will lose water through osmosis and die)
Cucumber placed in NaCl solution loses water to shrivel up and become a pickle.

61. Conclusions cB nB/ V Π = i cB RT 【key points】
1. Molarity- Molar Concentration (摩尔浓度，物质的量浓度)
2. Osmosis and Osmotic Pressure （渗透与渗透压）
3. isotonic, hypertonic and hypotonic sulutions
【homework】
p20 T2，T p39 T6，T9 cB
def
nB/ V
Π = i cB RT