CHEM 110 How to reach me? General Chemistry King Abdul Aziz University

CHEM 110
General Chemistry
King Abdul Aziz University
Jeddah KSA
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How to reach me?
Dr. Hadi M. Marwani
Associate Professor of Analytical and Environmental
Chemistry
• Faculty of Science, Chemistry Department
• Room 362.
• E-mail address: [email protected]
• Website: www.kau.edu.sa/hmarwani
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Text Book
• Any General Chemistry Book
• Selected textbooks:
• Chemistry 10th Edition by Raymond Chang
• General Chemistry System, Marwani and Albar at Dar
Hafez
• General Chemistry, McMurray
• Chemistry,
Ch i t Whitten
Whitt
• Chemistry, By C. Mortimer, 6th edition
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Grading System
30% First midterm
30% Second midterm
40% Final exam
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Grading System
95 – 100 % A+
90 – 95 % A
85 – 89 % B+
80 – 84 % B
75 – 79 % C+
70 – 74 % C
65 – 69 % D+
60 – 64 % D
< 60 %
F (Fail)
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Chemistry: The Study of Change
Chapter 1
General Chemistry
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What is Chemistry?
Chemistry is defined as "the
study of matter and its change"
Matter
Matter is everything around us.
Matter is anything that has a mass and occupy a space.
Matter exists in three states: solid, liquid and gas.
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Matter
Pure substance
Element
Compounds
Mixture
Heterogeneous
Homogeneous
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Classification of Matter
Matter
Anything with mass and volume.
Pure Substance
Matter with constant composition
Element
Substance
made up of
only one
type of
atom
Examples gold, silver,
carbon,
oxygen and
hydrogen
Compound
Two or more
elements that are
chemically
combined
Examples - water,
carbon dioxide,
sodium
bicarbonate,
carbon monoxide
Mixture
Matter with variable composition
Heterogeneous Mixture
Mixtures that are made
up of more than one
phase
Homogeneous Mixtures
Also called
solutions. Mixtures that
are made up of only one
phase
Examples - sand, soil,
chicken soup, pizza,
chocolate chip cookies.
Examples - salt water, pure
air, metal alloys, seltzer
water.
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Pure Substance:
A material with a constant composition such as NaCl, H2O, H2, CO2, and O2.
Elements:
Any substance that contains only one kind of an atom, such as H2 and O2.
2H2O ---> 2H2 + O2
Symbols for Some Elements
Name of
Element
Name of
Element
Symbol
Aluminum
Al
magnesium
Mg
Bromine
Br
Neon
Ne
Calcium
Ca
Nickel
Ni
Carbon
C
Nitrogen
N
Chlorine
Cl
Oxygen
O
Copper
Cu
phosphorus
P
Gold
Au
potassium
K
Helium
He
Silicon
Si
Hydrogen
H
Sodium
Na
I
Sulfur
Iodine
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Symbol
S
Iron
Fe
Tin
Sn
Lead
Pb
Zinc
Zn
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Example: Write the symbols for the following:
chlorine, copper, hydrogen, sodium, nickel,
carbon, and oxygen.
•
•
•
•
•
•
•
•
Answer:
chlorine
hl i (Cl)
copper (Cu)
hydrogen (H)
sodium (Na)
nickel (Ni)
carbon (C)
oxygen (O)
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• Compound is a material that
consists of two or more
elements united together in
definite proportion.
• Compounds are represented
by chemical formulas.
•
Chemical formula shows the
symbols of the elements that are
combined to make the compound.
Examples of Some Chemical Formulas
Compound
Common
N
Name
Chemical
F
Formula
l
calcium
carbonate
chalk
CaCO3
carbon dioxide
dry ice
CO2
hydrochloric acid
muriatic acid
HCl
hydrogen sulfide
rotten-egg
gas
H2S
sodium hydrogen
carbonate
(or sodium
bicarbonate)
baking soda
NaHCO3
sodium chloride
table salt
NaCl
sodium nitrate
fertilizer
NaNO3
sulfuric acid
battery acid
H2SO4
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• Mixtures - Mixtures are made up of two or more
substances that are physically combined.
• The specific composition will vary from sample to
sample.
Homogenous mixtures - you cannot distinguish between its
component such as milk, apple juice, and air.
Heterogeneous mixtures - made up of more than one substance and
theyy can be separated
p
p
physically
y
y such as sandwich,, smoke coming
g out
of the car.
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Physical and Chemical Properties
Physical properties can be observed or measured without
changing the composition of matter.
Physical properties are used to observe and describe matter, such
as appearance, texture, color, odor, melting point, boiling point,
density, solubility, polarity, and many others.
Chemical properties are only observable during a chemical
reaction. For example, you might not know if sulfur is combustible
unless you tried to burn it.
Mater Change
Physical change involves a change in the physical properties of the
matter and it could be reversed, such as melting solid ice to liquid
water.
Chemical change involves a change in the chemical composition of
the matter and it could not be reversed, such as burning sugar.
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Example
Classify each of the following changes as physical or
chemical:
g Iron
Melting
Melting Ice
Burning Paper
Chopping Wood
Mixing Salt & Water
Breaking Glass
Burning Wood
Mixing Peas & Carrots
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Measurements
The International System of
Measurements (SI)
There are seven SI base units.
PROPERTY
UNIT
Length
Meter
m
Mass
Kilogram
kg
Time
Second
s
Amount
Mole
mol
Temperature
Electrical
Current
Luminosity
Derived Units: Units that are
made
d up off some combination
bi ti off
SI base units are called Derived
Units.
SYMBOL
Kelvin
K
Ampere
A
Candela
Cd
PROPERTY
UNIT
SYMBO
L
Force
Newton
N
kg m/s2
Pressure
Pascal
Pa
N/m2
or kg/m s2
Energy
Joule
J
kg m2/s2
or N m
DEFINITION
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SI Prefixes: used with
the base units in order to
increase or decrease the
value that they represent.
To remove a prefix from a value,
insert the numerical value of the
prefix in place of the symbol.
Example:
Convert 5.83 pm to meters
Replace "p" with x 10-12
= 5.83 x 10-12 m
To insert a prefix into a value,
insert both the prefix and the
inverse of its numerical value.
PREFIX
SYMBO
L
exa-
E
1 000 000 000 000 000 000 (1018)
peta-
P
1 000 000 000 000 000 (1015)
tera-
T
1 000 000 000 000 (1012)
Giga
G
1 000 000 000 (109)
Mega
M
1 000 000 (106)
NUMERICAL EQUIVALENT
Kilo
K
1000 (103)
hecto-
H
100 (102)
deca-
Da
10 (101)
deci-
D
0.1 (10-1)
Centi
C
0.01 (10-2)
milli-
M
0.001 (10-3)
micro-

0.000 001 (10-6)
N
0.000 000 001 (10-9)
nanopico-
P
0.000 000 000 001 (10-12)
femto-
F
0.000 000 000 000 001 (10-15)
atto-
A
0.000 000 000 000 000 001 (10-18)
Example:
Convert 0.000462 g to milligrams
(note that the inverse of milli is 10+3)
= 0.000462 x 10+3 mg = 4.62 x 10-1 mg OR 0.462 mg
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K = 0C + 273.15
273 K = 0 0C
373 K = 100 0C
0F
= 9 x 0C + 3
32
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32 0F = 0 0C
212 0F = 100 0C
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Convert 172.9 0F to degrees Celsius.
= 9 x 0C + 32
5
0F – 32 = 9 x 0C
5
0F
5 x (0F – 32) = 0C
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0C = 5 x (0F – 32)
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0C = 5 x (172
(172.9
9 – 32) = 78.3
78 3
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Density
Density is an important property, which can be used to help determine the
identity of an unknown substance.
densiy 
mass ( g )
volume (ml )
A student determines that a piece of an unknown material has a mass of
5.854 g and a volume of 7.57 cm3. What is the density of the material,
rounded to the correct number of significant figures?
densiy 
mass (g )
5.854( g )

volume (cm 3 ) 7.57(cm 3 )
d = 0.77331571994 g/cm3
= 0.773 g/cm3
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