Introduction
Matter and Measurement
Forms of Matter
 Gases
 No
definite volume or shape.
 Volume depends on temperature and pressure.
 Very compressible.
 Less dense than the liquid form
 Experience flow
 Very large spaces between the particles.
 High energy form of matter.
Forms of Matter
Plasma is a high temperature physical state of matter in
which atoms lose their electrons and become ionized. The
sun is a good example of a plasma as is a fluorescent bulb.
 Bose-Einstein Condensate(BEC)

Newest form of matter
 Occurs at very low temperatures
 Easiest to make with Group IA elements
 Called “fuzzy matter”

State Changes
 When
one form of matter changes into another
form of matter, a state ,or phase, change occurs.
 Solid
to liquid
 Liquid to gas
 Solid to gas
 Liquid to solid
 Gas to liquid
 Gas to solid
Properties of Matter
There are chemical and physical properties of matter.
 Chemical properties are those which cause a substance to
change its features into something else. A new substance
is formed when a chemical property is observed. A
chemical change occurs in which one or more substances
are converted into something new.
 There are several evidences that a chemical change has
occurred. They may include large energy change,
evolution of gas, change in color, formation of a
precipitate, odor change and difficulty of reversal.
 In a chemical reaction the starting substances are called
reactants while the ending substances are called products.

Classification of Matter

Pure Substances
Uniform composition
 Definite composition
 Homogeneous
 Identical properties
 Cannot be separated and
maintain its identity


Mixtures
Physical
combination(blend) of two
or more substances
 Separable by physical
means
 Variable composition
 Components retain their
properties

Kinds of Mixtures

Homogeneous
Also called a solution
 Physical combinations
 Uniform throughout a given
sample
 Components uniformly
distributed
 Composition may vary
from sample to sample
 Separable by physical
means


Heterogeneous
Physical combinations
 Nonuniform within a
sample
 Components are
distinguishable
 Separable by physical
means


Kinds of Substances
Elements
 Compounds
 All samples are
 All samples are identical.
identical.
 Chemical combinations
 Cannot be physically separated
 Approximately 120
and keep identity.
 Approximately 90 are
 New properties that are different
naturally occurring
from component properties
 May be metal,
 Definite composition
metalloid, or nonmetal  Homogeneous
 Exist as solids,
 Can be broken into elements by a
liquids, or gases
chemical change.
Elements
Elements are summarized on the Periodic Table.
 They are represented by symbols of 1, 2, or 3 letters.
 The vertical columns are groups or families whose
members have similar properties.
 The horizontal rows or periods have members whose
properties change regularly as one moves from left to
right.
 All elements may be classified as representative (Gps 1-2
and 13-18) or transition (Gps 3-12).
 The lanthanides and actinides are transition elements.

Metallic Elements
 Conduct
heat and electricity.
 Are malleable.
 Are ductile.
 Have luster.
 Are solids, except for mercury which is a liquid.
 Have high tensile strength.
 Are found on the left side of the Periodic Table.
Nonmetallic Elements
 Do
not conduct well.
 Are brittle.
 Are dull in color.
 May be gases or solids, except bromine which is a
liquid.
 Are found on the right side of the Periodic Table.
Elemental Abundance
 The
most abundant element in the Earth’s crust is
oxygen. (Si, Al, Fe, Ca)
 The most abundant metal in the Earth’s crust is
aluminum.
 The most abundant element in our atmosphere is
nitrogen. (O2, Ar)
 The most abundant element in our universe is
hydrogen.
 The most abundant element in the human body is
oxygen.(C, H2)
The Importance of Measurement
 There
are two kinds of measurement. Both
provide important information.
 One kind of measurement is quantitative. It
gives results in numerical form. It is
objective because it requires an instrument.
 The other kind of measurement is
qualititative. It gives results in a descriptive
form. It is subjective because it depends on
the bias of the observer.
Lavoisier: The Founder of Modern
Chemistry
Lived in the mid 1700’s
 His work overthrew the
phlogiston theory of
burning.
 Mercury experiments were
carefully measured to help
disprove that theory.

Accuracy vs. Precision
Closeness to a true value
 Dependent upon the
quality of the measuring
device.
 Only one measurement.

Closeness of a set of
values
 Not related to accurate
value
 Dependent upon the skill
of the person making the
measurement.

Significant Figures in Measurements
 These
are digits which may be read from an
instrument plus one digit which is estimated.
 Check each instrument before using it to determine
how many figures may be read from it. Then
estimate one more figure.
 The use of these lends reliability and consistency
to measurements.
What digits are significant?
 All
nonzero digits are significant.
 All captive zeroes are significant.
 All beginning zeroes are NOT significant.
 All zeroes to the right of a nonzero digit and
a decimal point are significant.
 Ending zeroes in numbers without a decimal
may or may not be significant. The final
significant zero may be noted with a bar over
it.
What about calculations?
 When
adding or subtracting, the answer may have
only as many DECIMAL PLACES as the least
precise number in the operation.
 When multiplying or dividing, the answer may
have only as many SIGNIFICANT DIGITS as the
least precise number in the operation.
Comparing and Contrasting
measurement systems
The English system has no
standard of comparison.
 The English system has no
easy conversion from a
small unit to a larger unit
measuring the same
quantity.

The metric and SI
systems have standards.
The metric system is
based on Pt-Ir objects
whereas the SI is based
on physical
phenomena.
 The metric/SI
conversions are based
on powers of 10.

Comparing and Contrasting
measurement systems
The English system is
not widely used.
 The English system
has no base unit for a
quantity.
 The English system
uses commas.

The metric/SI systems
are widely used and are
the foundation of
scientific measurement.
 The metric/SI systems
use base units.
 The SI system uses
spaces.

Comparing and Contrasting the
measurement systems

The English system uses
oF for temperature.

The English system uses
fractions.
The metric system uses oC
for temperature whereas
the SI system uses K for
temperature.
 The metric/SI system uses
decimals.

The SI System
 There
are seven fundamental units: meter,
kilogram, second, Ampere, candela, mole,
and kelvin.
 All other units are derived from these.
 The meter is based on the distance light
travels in a vacuum in 1/3x108 ths of a
second.
 The second is based on the number of
disintegrations from a cesium-133 atom.
Metric Prefixes
yotta
zetta
exa
peta
tera
giga
mega
kilo
hecto
deka
1.00E+24
1.00E+21
1.00E+18
1.00E+15
1.00E+12
1.00E+09
1.00E+06
1.00E+03
1.00E+02
1.00E+01
yocto
zepto
atto
femto
pico
nano
micro
milli
centi
deci
1.00E-24
1.00E-21
1.00E-18
1.00E-15
1.00E-12
1.00E-09
1.00E-06
1.00E-03
1.00E-02
1.00E-01
Instruments and Methods
 Length
is measured with a meter stick or metric
ruler.
 Mass is measured with a triple beam balance.
 Volume is measured in 3 different ways depending
upon the substance to be measured.
Measuring Volume
 Liquids
are measured with a graduated cylinder,
never with a beaker or a flask.
 Regular solids are measured to find dimensions
and then volume formulas are used.
 Irregular solids are measured by displacement.
 One
Random Details
liter is equal to 1 decimeter cubed.
 One gram of water is equal to 1 centimeter
cubed at 4oC.
 Approximately 20 drops of water is 1 mL.
 A kilogram of water is the mass of 1 liter.
 Density is mass divided by volume.
 Specific gravity is a comparison of the density
of a substance to the density of a reference
material. It has no units.
Random Details
 Temperature
is the degree of hotness or coldness
of an object.
 Heat transfer occurs when two objects differ in
temperature.
 Heat energy flows from a warm object to a cooler
one.
 Temperature is measured in degrees and heat is
measured in calories or joules.
Specific Heat Capacity
 Specific
heat capacity is defined as the quantity of
heat required to change the temperature of an
object by 1 degree Celsius.
 The formula for calculating heat required is Q =
m C (t2 - t1), where Q is heat, m is mass, C is
specific heat, and t is temperature.