intro chemistry 1
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Transcript of intro chemistry 1
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Branches of Chemistry
Analytical Chemistry - deals with
the separation, identification and
quantification of a chemicalcomponent of natural and artificial
materials
Biochemistry - deals with chemicalreactions that occur in living things
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Branches of Chemistry
Inorganic Chemistry - deals with the
structure, properties and behavior of
inorganic compounds
Organic Chemistry - deals with the
structure, properties and behavior of
organic compounds
Physical Chemistry - uses physics to
study chemical reactions, structure
and properties of chemical substances
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Metal Time
Smoke Space
Car Light
Star Heat
Matter Not Matter
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matter
anything that occupies space and
has mass
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Mass - amount of matter present in an
object or substance; usually measured inkilograms (kg) or grams (g)
Volume - amount of space occupied by a
body or matter; usually measured in cubicmeter (m3), cubic centimeter (cm3) or in
liter (L)
Density - ratio of mass and volume;usually measured in kilograms per cubic
meter (kg/m3) or in grams per milliliter
(g/mL).
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Properties of Matter
Physical Properties - readily observable
without undergoing any change with the
substances composition
color, odor, taste, hardness, softness, ductility,
malleability, boiling and melting point, and
density
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Properties of Matter
Chemical Properties - determined only
when matter undergo changes in identity
and composition
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Properties of Matter
Intensive Properties - do not depend on
the size and amount of the sample
involved
density, freezing point, color, melting point,
reactivity, luster, malleability and conductivity
Extensive Properties - do depend onthe size and amount of the sample
involved
length, volume, mass and weight
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States of Matter
SOLID LIQUID GAS
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Classification of Matter
MATTER
Pure
Substance
element compound
Mixture
homogeneous heterogeneous
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Physical change occurs when there is
only a change in the physical appearance
of matter
melting, boiling, freezing, grinding, cutting
and changing shape
Chemical change or chemical reaction
involves substances that create a new
product/s.
decomposition (breaking of substance into
simple compounds) andsynthesis (fusion of
elements or compounds to form a more
complex substance)
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a. steam becomes water
b. a piece of sliced apple
turns brown
a. flattened copper wire
b. paper burning
c. eggs becoming rotten
physical
physical
chemical
chemical
chemical
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scientific notation
involves the representation of a
number as a power of ten
456,000,000 can be expressed as 4.56 x 108
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Rules in Scientific Notation
RULE 1: To convert a number greater than 1
to scientific notation, the original decimal point
is moved x places to the left and the resulting
number is multiplied by 10x. The exponent (x)is a POSITIVE NUMBER equal to the number
of places the original decimal point was moved.
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Rules in Scientific Notation
RULE 2: To convert a number less than 1 to
scientific notation, the original decimal point is
moved x places to the right and the resulting
number is multiplied by 10-x. The exponent (-x) is a negative number equal to the number of
places the original decimal point was moved.
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significant figures
defined as the accuracy to which
something is measured or
calculated
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Rules in Significant Figures
RULE 1: All nonzero digits are significant.
7.314 has four significant digits
RULE 2: The number of significant digits is
independent of the position of the decimal
point.
73.14 has four significant digits
RULE 3: Zeros located between nonzero digits
are significant.
60.052 has fivesignificant figures
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Rules in Significant Figures
RULE 4: Zeros at the end of a number are
significant if the number contains a decimal
point.
4.70 has threesignificant figures
RULE 5: Trailing zeros are insignificant
because the number does not contain a decimal
point.
100 have onesignificant figure
RULE 6: Zeros to the left of the first nonzero
integer are not significant.
0.0032 has two significant figures
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Rules on Addition and
Subtraction
The answer can only display as many
decimal places as the quantity having the
fewest number of decimal places. Properrounding off of numbers should be
observed.
37.68 + 108.428 + 6.71862 = 152.82662
Final answer: 152.83
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Rules on Multiplication and
Division
The answer may only display as many
significant digits as the multiplied or
divided measurement that shows theleast number of significant digits.
2.13 cm x 12.52 cm x 4.125 cm =
2933.53867026 cm3
Final answer: 2930 cm3
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system of measurement
a set of units which can be used
to specify anything which can be
measured for trade or commerce
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English system
traditionally used in the United States
slowly being replaced by metric system
although its use is still prevalent examples are inch, yard and mile for
length or distance; pint, quart and gallon
for volume; and ounce, pound and ton
for weight
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Metric system
units used for scientific measurements
first developed in France during the late
18th
century used in most countries throughout the
world
use prefixes to indicate different powers
of 10
examples are meter (m) for length, liter
(L) for volume and gram (g) for mass
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International System of
Measurements
specific choice of metric units for use in
scientific measurements
it was adapted at the 11th
generalconference of weights and measures in
year 1960 for scientific purpose
its units are called SI units from its
acronym in French: SystmeInternational d Units
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SI base units
fundamental units where other
units are derived
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SI derived units
units derived from SI base units
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Steps in Converting Units
1. determine which unit(s) must be replaced and
what unit(s) will replace it
2. write the unit equivalence in fractional form If the unit(s) to be replaced is at numerator, put that
unit(s) at denominator and the unit(s) that will
replace it at numerator.
If the unit(s) to be replaced is at denominator, putthat unit(s) at numerator and the unit(s) that will
replace it at denominator.
3. multiply the magnitude with the conversion
factor
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1. Convert 2.5 kg to pound (lb).
lb5.5=lb5.5115=kg1
lb2.2046
1
kg2.5
2. Convert 8.0 106 cm3 to m3.
3
336
8.0mcm100
m1
1
cm108.0
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