1. General Chemistry I Chem 110
Dr. Laila Mohammed Al-Harbi
Assistant professor
Contact Info:
Web Site:

2. Technicalities Class hours: SMW 8:00 am to 8:50 am (AA)
SMW 10:00 am to 10:50 am (AE)
Locations:
Science tower 07 room 173 first floor
phone ext
web site:
Exam schedule:
1st exam : from lecture ( Chapters 1-4) = 30 marks
2nd exam: from lecture (Chapters 5,7-9) = 30 marks
Final exam: from lecture = 40 marks
(Chapters 1,2,3,4,5,7,8,9,10,14,15,24,25)
Home works = Bonus marks

3. Dr. Laila Mohammed Al-harbi Assistant professor in physical chemistry 1st term schedule (2010-2011)
DAY
8-9
9-10
10-11
11-12
12-1
1-2
2-3
3-4
4-5
Saturday
CHEM 110
(AA)
Office hour
(EA)
Sunday
Lab281
(BB)
Monody
Lab 281
(JD)
(JC)
Tuesday
CHEM
491
Wednesday
CHEM 110 (EA) >>> room 2167 at 1st floor
CHEM 110(AA) >>> room 101 A at ground floor
Web site:

4. Chemistry, by Chang, 10th. ed., 2007, McGraw-Hill.
Course No.
Course Title
No. of Units
Pre-requisites
Th.
Pr.
Credit
Chem 110
General Chemistry  I 3 -
Course Objectives:
The course aims to introduce students to basic knowledge and principle in chemistry.
Course Description :
It provides an introduction to the general principles of chemistry for students planning a professional career in chemistry, a related science, the health professions, or engineering. By the end of this course the student will be able to understand the following: Significant figures, scientific notation and units, stoichiometry, atomic structure & periodic table, chemical bonding, gases, ionic equilibrium, basic principles of organic and basic principles of biochemistry .
 Main text books:
  Chemistry, by Chang, 10th. ed., 2007, McGraw-Hill.
Chemistry, by Steven S. Zumdahl, 6th ed., Houghton Mifflin College Div.
Subsidiary books :
       Chemistry, by Mortimer, 6th ed., Wadsworth Inc.

5. Chemistry, by Chang, 10th. ed., 2007, McGraw-Hill.
 Main text book :
  Chemistry, by Chang, 10th. ed., 2007, McGraw-Hill.

11. Chapter 1 The study of change
1-7 Measurement
SI units
Mass and weight
Volume
Temperature scales
Homework
Page 33
1.17,1.19,1.22,1.23,1.25,1.26.

12. Introduction
Chemistry is the study of matter and the changes it undergoes
There are three states of matter
solid
liquid
gas

13. 1.7 Measurement and Units Macroscopic Which can be determined directly
Ex: volume
Microscopic
Determined indirectly on atomic
or molecular scale

14. Extensive and Intensive Properties
An extensive property of a material depends upon how much matter is being considered.
mass
length
volume
An intensive property of a material does not depend upon how much matter is being considered.
density
temperature
color

15. The International System of units (SI Units)
used for commerce and science around the world
Table 1.2 SI Base Units
Base Quantity
Name of Unit
Symbol
Length
meter m
Mass
kilogram kg
Time
second s
Temperature
kelvin K
Amount of substance
mole
mol

16. m

17. to measure some thing too small (atomic radius of nitrogen )
some thing too big (distance between earth and moon)
7×10-9 m = 7 nm
m = 384 Mm

18. Example 1 A) 6.0 km is how many micrometers? Solution 1 1 km = 103 m
6 km = x = 6 × 103 m
1µm = 1× 10-6 m
x = 6 × 103 m
x = 6 × 109µm
Solution 2
1 km = 103 m → 1 m = 10-3 km
1µm = 1× 10-9 m → 1 m = 106µm
10-3 km = 106µm
6 km = x
X = 6 × 106 µm/ 10-3 km =
x = 6 × 109µm

19. Which of these quantities represents the largest mass?
Examples 2
The diameter of an atom is approximately 1  10-7 mm. What is this diameter when expressed in nanometers? 
A. 1  nm
B. 1  nm
C. 1  10-9 nm
D. 1  10-1 nm
= 1× 10-7 × 1 × 106 =
1 × 10-1 nm = 0.1 nm
Examples 3
Which of these quantities represents the largest mass? 
A. 2.0  102 mg
B kg
C. 1.0  105 g
D. 2.0  102 cg
Put all of them in the same unit

20. The weight of man on earth is 50 pounds.
Mass and Weight
Mass is the measure of the amount of matter in an object.
SI unit of mass is the kilogram (kg)
1 kg = 1000 g = 1 x 103 g
Weight is the measurement of the pull of gravity on an object.
The Mass of an object doesn't change when an object's location changes. Weight, on the other hand does change with location.
Chemist are interested primarily in mass
weight = c x mass
The weight of man on earth is 50 pounds.
is 8.25 pounds on moon

21. Volume – SI derived unit for volume is cubic meter (m3)
1 cm3 = (1 x 10-2 m)3 = 1 x 10-6 m3
1 dm3 = (1 x 10-1 m)3 = 1 x 10-3 m3
1 L = 1000 mL = 1000 cm3 = 1 dm3
1 mL = 1 cm3
Common unit of volume is liter

22. Density mass density = volume The density of copper is 8.94 g/cm3.
Density is defined as the amount of matter in a given amount of space.
d = m/V
SI derived unit for density is kg/m3
1 g/cm3 = 1 g/mL = 1000 kg/m3
Density is intensive property
Density decrease with temperature
Unit of density is Kg/l
g/ml )g/cm3 for liquid and solids
g/l = 0.001g/ml for gases
Because density of gases are very low
density =
mass
volume
The density of copper is 8.94 g/cm3.

23. Example 1.1
A piece of Gold metal has a volume of cm3, with a mass of 301 g What is its density?
A piece of platinum metal with a density of g/cm3 has a volume of 4.49 cm3. What is its mass?
d = m V
d = m V
m = d x V
301 g/ cm3
= 19.3 g/ cm3
= 21.5 g/cm3 x 4.49 cm3
= 96.5 g

24. Example 1.2
The density of mercury is 13.6 g/mL has a volume of 5.50 mL. What is its mass?
The density of sulfuric acid is 1.41 g/mL has a volume of 242 mL. What is its mass?
d = m V
d = m V
m = d x V
= 13.6 g/mL x 5.50 mL
= 74.8 g
m = d x V
= 1.41 g/mL x 242 mL
= g

25. Fahrenheit °F →°F = [ (9/5) × °C] + 32
Temperature Scales
Fahrenheit °F →°F = [ (9/5) × °C] + 32
Celsius °C → °C = (5/9) (°F - 32)
Kelvin ° K → ° K = °C

26. Example 1.3 Convert -452 0F to degrees Celsius.
Convert 224 0C to degrees Fahrenheit?
°F = (9 0F /5 0C) × °C + 32
[°F = (9 0F /5 0C) × 224 °C] C = 435 0F
Convert F to degrees Celsius.
°C = (5 0C /9 0F) (°F F)
°C = (5 0C /9 0F) (-452 °F F) = C
Convert C to degrees Kelvin..
° K = [-38.9 °C °C ] × 1 K/ 1 0C = K

27. Test bank 1. The SI unit of time is the A. hour B. second C. minute
D. ampere
2. The diameter of an atom is approximately 1  10-7 mm. What is this diameter when expressed in nanometers? 
A. 1  nm
B. 1  nm
C. 1  10-9 nm
D. 1  10-1 nm

28. 3. 6.0 km is how many micrometers? 
A. 6.0  106 µm
B. 1.7  10-7 µm
C. 6.0  109 µm
D. 1.7  10-4 µm
4. The SI prefixes giga and micro represent, respectively: 
A and 10-6.
B. 106 and 10-3.
C. 103 and 10-3.
D. 109 and 10-6.

29. 6. How many cubic centimeters are there in exactly one cubic meter? 
A. 1  10-6 cm3
B. 1  10-3 cm3
C. 1  10-2 cm3
D. 1  106 cm3
Solution
(1m )3 = (1  10-2 cm )3
1m3 = 1  10-6 cm 3
5. Which of these quantities represents the largest mass? 
A. 2.0  102 mg
B kg
C. 1.0  105 g
D. 2.0  102 cg
Solution
A) 0.2 g
B)1 g
C) 0.1 g
D) 2 g

30. 7. Ammonia boils at -33.4C. What temperature is this in F? 
A F
B F
C F
D F
F = (9 0F /5 0C) × °C + 32
[°F = (9 0F /5 0C) × °C] C = 435 0F