FEU CLASS OF 2024: INTRODUCTIONS TO GENERAL, ORGANIC AND BIOCHEMISTRY |1
LESSON 1:
MATTER,
ENERGY,
AND MEASUREMENT
MATTER

Is anything that has mass and takes up space
and possess inertia.
Chemistry

Is the science that deals with matter: the
structure and properties of matter and the
transformations from one form of matter to
another
PROPERTIES OF MATTER
 Ability or inability of matter to undergo a
change in its identity or compositions at a
given conditions.
 Flammability- example of chemical
properties, which is ability to burn when in
contact with flame producing new
substances.
 Chemical Change- more commonly called a
chemical reaction, some substances are used
up (disappear) and other are formed to take
their place.
 Physical Change- substances do not change
(ex. Melting of solid and boiling of liquid)
Extensive Properties

Intensive Properties

PROPERTIES OF
MATTER

PHYSICAL
PROPERTIES
CHEMICAL
PROPERTIES
EXTENSIVE
PROPERTIES
Properties that depend on the amount of
materials observed (e.g. mass, volume,
texture, length, and size)
Properties that does not depend on the
amount of material observed (e.g. density,
odor, taste, color, physical state, melting,
boiling, etc.)
Depend on the type of matter
INTENSIVE
PROPERTIES
WHAT IS THE SCIENTIFIC METHOD
Scientific Method
Physical Properties



Is one that can be observed without changing
the composition of a substance
It includes phases (solid, liquid or gas), color,
solubility, density, melting, and boiling
points, volatility, viscosity, and conductivity.
Determining physical property of matter may
be accompanied by a change in its physical
state
Chemical Properties
 Characteristics that can be observed with an
accompanying change in the chemical
composition of a substance



A systematic approach/procedure in
investigating nature
Is a tool that is being used by the scientist
The heart of the scientific method is the
testing of theories
1600


Aristotle (384-322 BCE)
 Believed that if you took the gold out
of a mine it would grow back.
Galen (200-130 BCE)
 A Greek physician, recognized that
the blood on the left side of the heart
somehow gets to the right side.
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FEU CLASS OF 2024: INTRODUCTIONS TO GENERAL, ORGANIC AND BIOCHEMISTRY |2
 Fact- is statement based on direct
experience; it is a consistent and
reproducible observation.
 Hypothesis- is a statement that is
proposed, without actual proof, to
explain the facts and their
relationship.
William Harvey (1578-1657)


Tested Galen’s hypothesis by dissecting
human and animal hearts and blood vessel.
Discovered that one way valves separate the
upper chamber of heart from lower chamber;
also discovered that heart is a pump, by
contracting and expanding pushes blood out.
Fabricius (1537-1619)


Harvey’s teacher
Previously observed that one-way valves
exist in the vein
-
-
Qualitative- consist of
general observation about
the system
Quantitative- consist of
numbers
by
various
measurements of the
system
2. Natural Law
 A pattern of consistency in
observation of natural phenomena; a
verbal or mathematical statement
which relates a series of observation
3. Defining a problem
4. Hypothesis
 An educated guess to explain an
observation; tentative explanation of
a natural law based on observation
5. Experimentation
6. Interpret results
7. Generate a generalization
Malpighi (1628-1694)


1661, Italian anatomist, using the newly
invented microscope found these tiny vessels
which are now called capillaries
Theory- is the formulation of an apparent
relationship among certain observed
phenomena, which has been verified to some
extent
- Explains many interrelated facts
and can be used to make
predictions
about
natural
phenomena (e.g. Newton’s theory
of gravitation and kinetic
molecular theory of gases)
Experiment

One of the most important ways to test a
hypothesis
STEPS IN A SCIENTIFIC METHOD
1. Observation or Data Gathering
 Observations-things perceived by the
senses; can be quantitative or
qualitative
MEASUREMENTS
Exponential notation



Is based on powers of 10
Is a simple way to write and keep track of
very large or very small numbers without
having to deal with a lot of zeros
Helps us deal with the possible sources of
determinant error
Significant figures

Number of digits of a measured number that
have uncertainty only in the last digit.
DETERMINING SIGNIFICANT FIGURES:
1. Non-zero digits are always significant
2. Zeros at the beginning of a number are never
significant
3. Zeros between non-zero digits are always
significant
4. Zeros at the end of a number that contains a
decimal point are always significant
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5. Zeros at the end of a number that contains no
decimal point may or may not be significant
UNITS OF MEASUREMENTS
A measurements consists of two parts: a number and
a unit:
 A number without
meaningless.
a
unit
is
TWO SYSTEM OF UNITS

International System of Units ( SI units)
 Is based on the metric system and
uses some metric units
 Metric
system-a
system
that
originated in France about 1800
BASE UNITS IN THE METRIC SYSTEM
Length
Volume
Mass
Time
Temperature
Energy
Amount of substance

Meter (m)
Liter (L)
Gram (g)
Seconds (s)
Kelvin (K)
Joules (J)
Mole (mol)
English System
 Still widely used in the United State,
include
ounce(oz),
pound(lb),
inch(in), mile(mi), and quart(qt)
Length


Symbol
G
Mega
Kilo
Deci
Centi
Milli
Micro
Nano
M
k
d
c
m
µ
n
Pico
p
Value
10^9=1,000,000,000(one
billion)
10^6=1,000,000(one million)
10^3= 1,000(one thousand)
10^-1= 0.1(one-tenth)
10^-2= 0.01(one- hundredth
10^-3= 0.001(one-thousandth
10^-6= 0.000001(one- millionth
10^-9=
0.000000001(onebillionth)
10^-12= 0.000000000001(onetrillionth)
Some Conversion Factors between English and
Metric Systems
Length
1 in.= 2.54cm
1 m = 39.37in.
1 mile = 1.609km
Mass
1 oz = 28.35g
1 lb = 453.6g
1 kg = 2.205 lb
Volume
1 qt = 0.946 L
1 gal = 3.785 L
1 L = 33.81 fl oz
1 g = 15.43 1 fl oz. = 29.57
grains
mL
1 L = 1.057qt
Volume



Is the amount of space occupied by an object
Base unit of volume is Liter (L)
Larger than quart
Conversion Unit
1 mL= 0.001 L (or 1x10^-8L)
The base unit of length is meter(m)
To convert from one metric or SI unit to
another, we only have to move the decimal
point
Conversion factors:
5280 ft.
1760 yard
3ft.
12inch
Prefix
Giga
1 mile
1 mile
1 yard
1 foot
1000 mL(or 1x10^3mL) = 1 L
1 mL = 1 cc (cubic centimeter or cm^3)
1000 cc = 1 L
Mass




Is the quantity of matter in an object
Base unit of mass is grams (g)
Gram- small unit
Independent location
Conversion Unit
Most Common Metric Prefixes
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1 kg = 1000 g
1 mg = 0.001 g
453.6 g = 1 lb
Weight


molecules stop moving altogether. Therefore, the
temperature cannot get any lower.)
Formulas:
℉=
Is not independent location
Is the force a mass experiences under the pull
of gravity
℃=
(Note: mass and weight are different concepts, they
are related to each other by force of gravity)
9
℃ + 32
5
5
(℉ − 32)
9
𝐾 = ℃ + 273
℃ = 𝐾 − 273
Instruments for measuring mass of substances:



Triple beam balance – is accurate to one
decimal place in grams
Top loading balance – accurate to two
decimal places
Analytical balance- accurate to three decimal
places
Time


Is the one quantity for which the units are the
same in all systems
Base unit is seconds (s)
60 s = 1 min
60 min = 1 hr
(Note: -273℃ or 0 K is the lowest possible
temperature)
Factor- label method

A procedure in which equations are set up so that
all the unwanted units cancel and only the desired
units remain
(Rule: when multiplying numbers, we also multiply units
and when dividing numbers, we also divide units.)
Conversion Factors

The ratio of two different units
STATES OF MATTER
MATTER CAN EXIST IN THREE STATES:
Temperature


Measure of hotness and coldness of matter
Indicates the energy of the particles
 Heat – total energy that results from
molecular motion inside an object
 Temperature- measures the average
heat or thermal energy of particles of
an object
 Centigrade or Celsius- metric system
use; boiling point of water is
100℃ and the freezing point at 0℃
 Kelvin (K)-also called the absolute
scale
 Absolute Zero- is known as 0 K
(Temperature reflects how fast molecules move. The more
slowly they move, the colder it gets. At absolute zero,


Gases
 Have no definite shape or volume
 Expand to fill whatever container
they are put into
 Highly compressible and can be
forced into small container
 Particles in a gas are usually much
farther apart than those liquid
 Expand when heated
 Has low densities
Liquids
 No definite shape but has definite
volume
 Slightly compressible
 Particles in a liquid are close with one
another, but not as close as those solid
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
 Particles are not arranged in a rigid or
orderly manner; they can slide past
each other
 Allowing liquid to flow freely and
take the shape of container
 Have medium densities
Solid
 Have definite shape and volume
 Essentially incompressible
 Particles of solid are tightly packed
together
 Particles vibrate in a fixed position
 Cannot move around or slide past
each other
 Has high densities ad can expand
slightly when heated
(Substances whether it is a solid, liquid or gas it will
depend on its temperature and pressure)
Density


Any substances is defined as its mass per unit
volume.
It is calculated by dividing the mass of a
substances by its volume
greater density of liquid, the higher
the hydrometer floats
 Urinometer – is a hydrometer
measuring a urine sample
 Normal urine can vary
specific gravity from 1.010 to
1.030
 Patients with diabetes mellitus
have abnormally high specific
gravity of their urine sample;
while those have kidney
disease have an abnormally
low specific gravity.
ENERGY


Kinetic Energy (KE)



𝑚
; 𝑑 = 𝑑𝑒𝑛𝑠𝑖𝑡𝑦, 𝑚 = 𝑚𝑎𝑠𝑠, 𝑉 = 𝑣𝑜𝑙𝑢𝑚𝑒
𝑉
(Density of any liquid or solid is a physical property
that is constant, which means that it always has the
same value at a given temperature)
Specific gravity



Is numerically the same as density, but it has
no units(it is dimensionless)
Is defined as a comparison of the density of
substances with the density of water, which
taken as a standard
Often measured by a hydrometer
 Hydrometer – simple device consists
of a weighted glass bulb that is
inserted into a liquid and allowed to
float; either float or sink in the liquid
whose density is being determined;
Is energy of motion
Any object that is moving possesses KE
To calculate the KE:
1
 𝐾𝐸 = 2 𝑚𝑣 2
 𝑚 Is the mass of an object and v is its
velocity.
Formula:
𝑑=
Is defined as the capacity to do work
Can be described either kinetic energy or
potential energy
Kinetic Energy means;
1. Increases when object moves faster and;
2. When a heavier object is moving
Potential Energy


Is stored energy
Possessed by an object arises from its
capacity to move or to cause motion.
 Work – is done by gravity in the
process
Several forms of energy exist:
1. Most important are mechanical energy, light,
heat and electrical energy which are
examples of KE, possessed by all moving
objects, whether elephants or molecules or
electrons and;
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2. Chemical energy and nuclear energy, which
are examples of potentials energy
 Chemical energy- energy stored
within chemical substances and given
off when they take part in chemical
reaction
Law of Conservation of Energy

Energy can be neither created nor destroyed
HEAT AND TEMPERATURE
Aluminum
Copper
Lead
0.22
0.092
0.031
Substances
Wood (typical)
Glass (typical)
Rock (typical)
Ethanol
Methanol
Ether
Carbon tetrachloride
Specific Heat (cal./g, ℃)
0.42
0.22
0.20
0.59
0.61
0.56
0.21
Heat







One form of energy that is particularly
important in chemistry
Form of energy that most frequently
accompanies chemical reactions
Calorie- is defined as the amount of heat
necessary to raise the temperature
Hypothermia- at extremely low temperatures;
too much heat is lost and body temperature
drops condition
Hyperthermia – opposite condition; can be
caused either by high outside temperature or
by body itself when an individual develops
high fever
Kilocalorie (kcal)- is the small unit and
chemists more often use
 1 kcal = 1000 cal.
Joules (J)-is the official SI unit for heat; about
one-fourth of a calorie
 1 cal. = 4.184 J
Equation to calculate specific heat:


Amount of heat = specific heat × mass ×
change in temperature or;
Amount of heat = SH × m × ∆𝑇
 ∆𝑇 is the change in temperature
We can also write this equation as:
 Amount of heat= SH × m × (T2− T1)
Where T2 is the final temperature and T1 is the initial
temperature in °C.
Specific Heat (SH)

Is the amount of heat necessary to raise the
temperature of 1 g of any substances by 1℃
SPECIFIC HEATS
SUBSTANCES
Substances
Water
Ice
Steam
Iron
FOR
SOME
COMMON
Specific Heat (cal./g, ℃)
1.00
0.48
0.48
0.11
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