1. (Chemistry10th ed., R-Chang,2011)
First lecture
General Chemistry
Chapter 1, p10:29
(Chemistry10th ed., R-Chang,2011)
Layla Almazroai

2. The study of matter and the changes it undergoes
First lecture
What is chemistry?
The study of matter and the changes it undergoes
Layla Almazroai

3. Matter mixture Pure substance compound element
First lecture
Matter
mixture
Pure substance
compound
element
Separation by physical methods
Separation by chemical methods
homogeneous
heterogeneous
Any thing that occupies space and has mass
Matter includes things we can see and touch (such as water, earth, and trees), as well as things we cannot (such as air).
A combination of two or more substances in which the substances retain their distinct identities
Has a definite composition and distinct properties
cannot be separated into simpler substances by chemical means
composed of two different elements or more chemically united in fixed proportions.
The composition is not uniform
The composition is the same throughout
Layla Almazroai

4. a homogeneous mixture a heterogeneous mixture
Compound
Element
Dr AishaDawood

5. NaCl Salt water Iron sugar air helium water
First lecture
NaCl
Salt water
Iron
sugar
air
helium
water
Compound element homogeneous mixture heterogeneous
Layla Almazroai

6. NaCl Salt water Iron sugar air helium water salad
First lecture
NaCl
Salt water
Iron
sugar
air
helium
water
salad
Compound
homogeneous mixture
element
Compound
homogeneous mixture
element
Compound
heterogeneous mixture
Compound element homogeneous mixture heterogeneous
Layla Almazroai

7. First lecture
Matter states
The difference between the states is the distance between the molecules.
The three states of matter can be converted without changing the composition of the 
substance
Layla Almazroai

8. Physical Chemical Matter properties
First lecture
Matter properties
Chemical
Physical
color, mass, size, Shape, Solubility
Reactivity
flammability
is a property when the matter undergoes a chemical change or reaction
Can be measured and observed without changing the composition or identity of a substances
Layla Almazroai

9. Measurable properties of matter
First lecture
Measurable properties of matter
Extensive
Is additive
Intensive
Isn't additive
depends on how much matter is being considered
Does not depend on how much matter is being considered
Mass
volume
Density
temperature
How can these properties be measured ??
Layla Almazroai

10. International system of units
First lecture
Measurement
SI Units
International system of units
Symbol
Name of unit
Base Quantity m
meter
Length Kg
Kilogram
Mass s
Second
Time A
Ampere
Electrical current K
Kelvin
Temperature
mol
Mole
Amount of substance cd
candela
Luminous intensity
Layla Almazroai

11. International system of units
First lecture
Measurement
SI Units
International system of units
Symbol
Name of unit
Base Quantity m
meter
Length Kg
Kilogram
Mass s
Second
Time A
Ampere
Electrical current K
Kelvin
Temperature
mol
Mole
Amount of substance cd
candela
Luminous intensity
Layla Almazroai

12. Prefixes Used with SI Units
First lecture
Prefix
Symbol
Multiple of Base Unit
Giga G
1,000,000,000 or 109
Mega M
1,000,000 or 106
kilo k
1,000 or 103
deci d
0.1 or 10-1
centi c
0.01 or 10-2
milli m
0.001 or 10-3
micro
or 10-6
nano n
10-9
pico p
10-12
Femto f
10-15
Layla Almazroai

13. Mass and weight 1 Kg = 1000 g = 1 ×103 g Newton (N)
First lecture
Mass and weight
What is the difference between mass and weight?
Mass: is a measure of amount of matter in an object
Weight: is the force that gravity exerts on an object
1 Kg = 1000 g = 1 ×103 g
Newton (N)
Layla Almazroai

14. First lecture
Volume
1 L = 1 dm3 = (10 cm) (10 cm) (10 cm) = 1000 cm3
1 L = 1000 ml
= 1000 cm3
= 1 dm3
1 mL = 1 cm3
Layla Almazroai

15. Density g/cm3 for solids g/ml for liquids g/L for gases
First lecture
Density
Density is defined as the mass per unit volume.
density = mass/volume
d = m V
S.I. units for density = kg/m3
g/cm3 for solids
g/ml for liquids
g/L for gases
Layla Almazroai

16. Density S.I. units for density = kg/m3 density = mass/volume m d = V
First lecture
Density
S.I. units for density = kg/m3
density = mass/volume
d = m V
A piece of platinum metal with a density of 21.5 g/cm3 has a volume of
4.49 cm3. What is its mass?
d = m V
m = 21.5 g/cm3 x 4.49 cm3 = 96.5 g
m = d x V
Layla Almazroai

17. Temperature T(in Kelvin) = T(in Celsius) + 273.15 9 0F = x 0C + 32 5
First lecture
Temperature scales
Fahrenheit oF
Celsius oC
Kelvin K
0F = x 0C + 32 9 5
32 0F = 0 0C
212 0F = 100 0C
273 K = 0 0C
373 K = 100 0C
T(in Kelvin) = T(in Celsius)
Layla Almazroai

18. Precision and Accuracy:
First lecture
Student A Student B Student C
1.964 g g g
1.978 g g g
Average g g g
The true mass of object= g
Precision: degree of reproducibility of a measured number.
Accuracy: how close your measurements are to the true value.
Layla Almazroai

19. Scientific Notation The number of atoms in 12 g of carbon:
602,200,000,000,000,000,000,000
6.022 x 1023
The mass of a single carbon atom in grams:
1.99 x 10-23
N x 10n
N is a number
between 1 and 10
n is a positive or
negative integer
uqu chemistry website 9/23/2013

20. Significant Figures: Any digit that is not zero is significant
First lecture
Any digit that is not zero is significant
1.234 kg 4 significant figures
Zeros between nonzero digits are significant
606 m 3 significant figures
Zeros to the left of the first nonzero digit are not significant
0.08 L 1 significant figure
If a number is greater than 1, then all zeros to the right of the decimal point are significant
2.0 mg 2 significant figures
If a number is less than 1, then only the zeros that are at the end and in the middle of the number are significant
g significant figures
uqu chemistry website 9/23/2013

21. First lecture
How many significant figures are in each of the following measurements?
24 ml
3001 g
𝒎 𝟑
6.4 × 𝟏𝟎 𝟒 molecules
560 kg
2 significant figures
4 significant figures
3 significant figures
uqu chemistry website 9/23/2013

22. Significant Figures: 568.762 = 5.68762 × 𝟏𝟎 𝟐 (6 SF)
First lecture
= × 𝟏𝟎 𝟐 (6 SF)
N>1 , 2.00 (3 SF)
N<1 , 0.02 (1 SF)
0.20 (2 SF)
= 7.72 × 𝟏𝟎 −𝟔 (3 SF)
If addition or subtraction: 1- must have same power before addition or subtraction
2- sig. fig. in the answer is as the smaller digits after decimal point
4.31 × 𝟏𝟎 𝟒 +
3.𝟗× 𝟏𝟎 𝟑 ( 0.39 × 𝟏𝟎 𝟒 )
= × 𝟏𝟎 𝟒 (3 SF)
7.4 × 𝟏𝟎 𝟑
(1 decimal digit: this has the smallest digit)
0.10× 𝟏𝟎 𝟑
= × 𝟏𝟎 𝟑 (2 SF)

23. Significant Figures:
First lecture
If multiplication or division subtraction: 1- add exponent for multiplication or subtract exponent for division write the answer with the smaller sig. fig.
( 8.0 × 𝟏𝟎 𝟒 ) . (5.00× 𝟏𝟎 𝟐 )=𝟒𝟎× 𝟏𝟎 𝟔 or 4 .0× 𝟏𝟎 𝟕
(2 SF) (3 SF) (2 SF) (2 SF)
4.51 x = ≈𝟏6.5
(3 sf) (5 sf) (3 sf)
6.8 ÷ = ≈ 0.061
(2 sf) (5 sf) (2 sf)

24. First lecture Layla Almazroai
[ Length ] L 1.00m 100 cm yd 1000 mm km 1.00x106 microns 1.06x10-16 light yr 3.28 ft 39.4 in 1.00x1010 A 6.21x 10-4 mile Delzell
[ Area ] L2 1.00m Delzell2 [ Volume ] L3 1.00L 1000 mL 1000 cm3 1.00x 10-3 m gal(US liq) 1.06 qt(US liq) 61.0 in3 ** ft3
[ Mass ] M 1.00kg 1000 g slug 6.023x1026 AMU Eisen [ Density ] M/L3 1.00g/mL 1.00kg/L 1.00x103 kg/m Lenker
[ Time ] T 1.00h 60.0 min 3600 s d week 1.14x10-4 y 1.14x10-6 Cappel [ Velocity ] L/T 1.00m/s 1.00x10 –4 Lucey
[ Force ] ML/T2 1.00N (newton) 1.00kg m/s2 1.00x105 dyne 1.00x105 g cm/s lb (pound) 1.12x ton 1.00x10-12 WellingTON 6.45 Fig Newtons* 5.18 fat free Fig Newtons*
[ Energy ] ML2/T2 1.00J (joule) 1.00N m 1.00x10 7 erg 1.00x10 7 dyne cm ft lb .239 cal 9.48x10 -4 BTU L atm 2.78 x 10 –7 kW H 6.24x10 18 eV 1.00 v coulomb
[Momentum] ML/T 1.00kg m/s 103 hoogenBOOMS [Pressure ] M/LT2 1.00atm 760 mm Hg 760 torr 1.013x105 N/m x10 5 Pa 14.7 lb/in2 1.0x10 –5 Kilgour 29.9 in Hg
[ Power ] ML2/T3 1.00W 1.00J/s horsepower kW 1.00x107 erg/s 1.00x10 53 Liptack 5.00x1099 RobPerry [Acceleration ] L/T2 1.00m/s2 1.00x10 -4Lucey/s
[ Number ] 1.00mole 6.023x x1022 dozen 1.00x1047 Bliz pt
[ Frequency ] 1/T 1.00cycle/sec 1.00 hertz 108 Williams 103 Lippincott 103 Karas
[Temperature] K (Kelvin) ° C Jacobs Jacobs-Abs
[ Angles ] 1.00circle 360 deg min 6.28 radians 1.30x106 sec
Layla Almazroai