1
Chapter
Matter and Measurement
Chemistry, 4th Edition
McMurry/Fay
Dr. Paul Charlesworth
Michigan Technological University
Properties of Matter
01
•
Matter: anything that has both mass & volume.
•
Properties: describe or identify matter.
•
Intensive Properties do not depend on amount.
•
Extensive Properties do depend on amount.
Prentice Hall ©2004
Chapter 01
Slide 2
Chemistry and the Elements
Names of Som e Comm on Elements and Their Symbols
Alum inum
Al
Chlorine
Cl
M anganese
Mn
C opper (cuprium )
Cu
Argon
Ar
Fluorine
F
Nitrogen
N
Iron (ferrum )
Fe
Barium
Ba
Helium
He
Oxygen
O
Lead (plum bum )
Pb
Boron
B
Hydrogen
H
Phosphorus
P
M ercury (hydrargyrum )
Hg
Brom ine
Br
Iodine
I
Silicon
Si
Potassium (kalium )
K
C alcium
Ca
Lithium
Li
Sulfur
S
Silver (argentum )
Ag
C arbon
C
M agnesium
Mg
Zinc
Zn
Sodium (natrium )
Na
Prentice Hall ©2004
Chapter 01
Slide 3
Chapter 01: Matter and Measurement
Elements and the Periodic Table 01
•
Periods: The seven horizontal rows that group
elements based on their principal quantum number.
•
Groups: The 18 vertical columns that group
elements based on their angular momentum
quantum number.
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Chapter 01
Slide 4
Elements and the Periodic Table 02
•
•
Main Groups:
•
s-block elements: Two groups on the left (1 & 2)
•
p-block elements: Six groups on the right (13–18)
Transition Metal Groups:
•
d-block elements: Ten groups in the middle (3–12)
•
f-block elements: Fourteen groups between 3 & 4
are called inner transition metals.
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Chapter 01
Slide 5
Properties of Matter
02
•
Physical Properties can be determined without
changing the chemical makeup of the sample.
•
Some typical physical properties are:
Melting Point, Boiling Point, Density, Mass, Touch, Taste,
Temperature, Size, Color, Hardness, Conductivity.
•
Some typical physical changes are:
Melting, Freezing, Boiling, Condensation, Evaporation,
Dissolving, Stretching, Bending, Breaking.
Prentice Hall ©2004
Chapter 01
Slide 6
Chapter 01: Matter and Measurement
Properties of Matter
03
• Chemical
Properties are those that do change
the chemical makeup of the sample.
•
Some typical chemical properties are:
Burning, Cooking, Rusting, Color change, Souring of milk,
Ripening of fruit, Browning of apples, Taking a photograph,
Digesting food.
•
Note: Chemical properties are actually chemical changes.
Prentice Hall ©2004
Chapter 01
Slide 7
Properties of Matter
PHYSICAL
CHANGE
PROPERTIES
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New form of old
substance.
No new substances
formed.
04
CHEMICAL
Old substance
destroyed.
New substance
formed.
Description by senses – List of chemical
shape, color, odor, etc.
changes possible.
Measurable properties –
density, boiling point,
etc.
Chapter 01
Slide 8
Properties of Matter
•
05
Homogeneous matter has the same appearance,
composition, and properties throughout.
•
Heterogeneous matter has visibly different phases
which can be seen, or properties that vary through
the substance.
Prentice Hall ©2004
Chapter 01
Slide 9
Chapter 01: Matter and Measurement
Properties of Matter
•
06
Pure substances have a distinct set of physical
and chemical properties and cannot be separated
by physical changes.
•
A mixture is two or more pure substances that can
be separated by physical changes.
Prentice Hall ©2004
Chapter 01
Properties of Matter
•
Slide 10
07
An element is a pure substance with its own set of physical
and chemical properties that cannot be decomposed into
simpler substances.
•
A compound is a pure substance that can be decomposed
by a chemical change into two or more pure substances.
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Chapter 01
Properties of Matter
•
Slide 11
08
Matter Classification: Matter can be
subdivided into mixtures and pure substances.
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Chapter 01
Slide 12
Chapter 01: Matter and Measurement
Properties of Matter
Prentice Hall ©2004
09
Chapter 01
Slide 13
Properties of Matter
10
•
Metals: Found on left side of periodic table.
•
Nonmetals: Found on the right side of periodic
table.
•
Semimetals: Form a zigzag line at the boundary
between metals and nonmetals.
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Chapter 01
Slide 14
Properties of Matter
•
10
Which of the following represents a mixture?
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Chapter 01
Slide 15
Chapter 01: Matter and Measurement
Properties of Matter
•
If the red spheres are oxygen and the white are
hydrogen, which of the following represents (a)
hydrogen peroxide, (b) hydroxide ions, and (c) a
mixture of hydrogen and oxygen gas?
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Chapter 01
Measurement and Units
•
11
Slide 16
01
Seven Fundamental SI Units of Measurement.
Physical Quantity
Mass
Length
Temperature
Amount of substance
Time
Electric current
Luminous intensity
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Name of Unit
kilogram
meter
kelvin
mole
second
ampere
candela
Chapter 01
Measurement and Units
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Chapter 01
Abbreviation
kg
m
K
mol
s
A
cd
Slide 17
02
Slide 18
Chapter 01: Matter and Measurement
Measurement and Units
•
03
Some Prefixes for Multiples of SI Units.
Factor
1,000,000,000 = 10 9
1,000,000 = 10 6
1,000 = 10 3
100 = 102
10 = 101
0.1 = 10-1
0.01 = 10 -2
0.001 = 10 -3
0.000,001 = 10 -6
0.000,000,001 = 10 -9
0.000,000,000,001 = 10-12
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Prefix
giga
mega
kilo
hecto
deka
deci
centi
milli
micro
nano
pico
Symbol
G
M
k
h
da
d
c
m
µ
n
p
Chapter 01
Slide 19
Measurement and Units
•
04
Some Derived Quantities.
Quantity
Definition
Derived Unit (Name)
Area
Volume
Density
Speed
Acceleration
Force
Pressure
Energy
Length times length
Area times length
Mass per unit volume
Distance per unit time
Change in speed per unit time
Mass times acceleration
Force per unit area
Force times distance
m2
m3
kg/m3
m/s
m/s2
(kg·m)/s2 (newton, N)
kg/(m·s2) (pascal, Pa)
(kg·m2)/s2 (joule, J)
Prentice Hall ©2004
Chapter 01
Slide 20
Measurement and Units
05
•
Density relates the mass of an object to its volume.
•
Density decreases as a substance is heated
because the substance’s volume increases.
•
Knowing the density of a substance allows
measurements in volume to be recorded in mass.
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Chapter 01
Slide 21
Chapter 01: Matter and Measurement
Measurement and Units
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06
Chapter 01
Slide 22
Measurement and Units
•
07
Densities of Some Common Materials.
Substance
Ice (0.0°C)
Density (g/cm3)
0.917
Substance
Human Fat
Density (g/cm3)
0.94
Water (4.0°C)
Gold
Helium (25.0°C)
Air (25.0°C)
1.0000
19.31
0.000164
0.001185
Cork
Table Sugar
Balsa Wood
Earth
0.22–0.26
1.59
0.12
5.54
Prentice Hall ©2004
Chapter 01
Slide 23
Measurement and Units
•
08
What is the density of glass (in grams per cubic
centimeter) if a sample weighing 26.43 g has a
volume of 12.40 cm3?
•
Chloroform, a substance once used as an
anesthetic, has a density of 1.483 g/mL at 20°C.
How many mL would you use if you needed 9.37 g?
Prentice Hall ©2004
Chapter 01
Slide 24
Chapter 01: Matter and Measurement
Measurement and Units
•
Temperature Conversions:
•
The Kelvin and Celsius
09
degree are essentially
the same because both
are one hundredth of the
interval between freezing
and boiling points of water.
Prentice Hall ©2004
Chapter 01
Slide 25
Measurement and Units
•
10
Temperature Conversions:
• Celsius (°C) — Kelvin temperature conversion:
Kelvin (K) = °C + 273.15
• Fahrenheit (°F) — Celsius temperature conversions:
°C =
5
9
9 
°F =  °C  + 32
5 
(°F − 32)
Prentice Hall ©2004
Chapter 01
Measurement and Units
•
Slide 26
11
Carry out the indicated temperature conversions:
(a) –78°C = ? K
(b) 158°C = ? °F
(c) 375 K = ? °C
(d) 98.6°F = ? °C
(e) 98.6°F = ? K
Prentice Hall ©2004
Chapter 01
Slide 27
Chapter 01: Matter and Measurement
Measurement and Units
•
12
Dimensional-Analysis method uses a conversion
factor to express the relationship between units.
Original Quantity × ConversionFactor = Equivalent Quantity
Example: Express 2.50 kg in lb.
ConversionFactor: 1.00 kg = 2.205 lb arranged as 2.205 lb
1.00 kg
∴ 2.50 kg × 2.205 lb = 6.00 lb (correct to 3 significant figures)
1.00 kg
Prentice Hall ©2004
Chapter 01
Slide 28
Measurement and Units
•
13
The volcanic explosion that destroyed Krakatau on
August 17, 1883, released an estimated 4.3 cubic
miles (mi3) of debris into the atmosphere. In SI
units, how many cubic meters (m3) were released?
Prentice Hall ©2004
Chapter 01
Slide 29
Measurement and Units
•
14
How many meters are there in a marathon race
(26 miles and 385 yd)?
•
How large, in cubic centimeters, is the volume of a
red blood cell if the cell has a circular shape with a
diameter of 6.0 x 10–6 m and a height of 2.0 x 10–6 m?
Prentice Hall ©2004
Chapter 01
Slide 30
Chapter 01: Matter and Measurement
Accuracy, Precision, and Significant
Figures in Measurement
01
•
Accuracy is how close
to the true value a
given measurement is.
•
Precision is how well a
number of independent
measurements agree
with one another.
Prentice Hall ©2004
Chapter 01
Slide 31
Accuracy, Precision, and Significant
Figures in Measurement
02
•
Significant Figures are the total number of digits
in the measurement.
•
The results of calculations are only as reliable as
the least precise measurement.
•
Rules exist to govern the use of significant figures
after the measurements have been made.
Prentice Hall ©2004
Chapter 01
Slide 32
Accuracy, Precision, and Significant
Figures in Measurement
03
•
Rules for Significant Figures:
•
Zeros in the middle of a number are significant
•
Zeros at the beginning of a number are not significant
•
Zeros at the end of a number and following a period are
significant
•
Zeros at the end of a number and before a period may or
may not be significant.
Prentice Hall ©2004
Chapter 01
Slide 33
Chapter 01: Matter and Measurement
Accuracy, Precision, and Significant
Figures in Measurement
04
•
Rules for Calculating Numbers:
•
During multiplication or division, the answer can’t
have more sig figs than any of the original numbers.
•
During addition or subtraction, the answer can’t have
more digits to the right of the decimal point than any
of the original numbers.
Prentice Hall ©2004
Chapter 01
Slide 34
Accuracy, Precision, and Significant
Figures in Measurement
05
•
Rules for Rounding Numbers:
•
If the first digit removed is less than 5 - round down
•
If the first digit removed is greater than 5 - round up
•
If the first digit removed is 5 and following numbers
are nonzero - round up
•
If the first digit removed is 5 and following numbers
are zero - round down
Prentice Hall ©2004
Chapter 01
Slide 35
Accuracy, Precision, and Significant
Figures in Measurement
06
•
How many significant figures does each of the
following measurements have?
(a) 0.036653 m
(b) 7.2100 x 10–3 g
(c) 72,100 km
(d) $25.03
Prentice Hall ©2004
Chapter 01
Slide 36
Chapter 01: Matter and Measurement
Accuracy, Precision, and Significant
Figures in Measurement
07
•
Round off each of the following measurements.
(a) 3.774499 L to four significant figures
(b) 255.0974 K to three significant figures
(c) 55.265 kg to four significant figures
Prentice Hall ©2004
Chapter 01
Slide 37
Chapter 01: Matter and Measurement