Chapter 1: Matter and Measurement
Chapter 1 Problem Set
Pages 51-55
4, 6, 8, 16, 34, 46, 54, 60
1.1
CLASSIFYING MATTER
States of Matter
What are the 3 states of matter?
Kinetic-Molecular Theory
What is the energy of motion that particles possess?
What effect does an increase in temperature have upon particles?
Matter at the Macroscopic Level and Particulate Level
What is meant by the statement, “Chemists carry out experiments at the macroscopic level, but
they think about chemistry at the particulate level”?
Pure Substances
What are some characteristic properties of a pure substance?
A pure substance cannot be separated into two different species by a physical process.
Mixtures: Heterogeneous & Homogeneous
What are some examples of a heterogeneous mixture?
What are some examples of a homogeneous mixture?
Is air a solution?
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1.2
ELEMENTS & ATOMS
What is an element?
How many elements are found in nature?
What is an atom?
1.3
COMPOUNDS AND MOLECULES
What is the difference between NO and No?
What is a chemical compound?
Are the characteristic properties of a compound different than those of the elements which
make up the compound?
For example…
1.4
PHYSICAL PROPERTIES
What are physical properties?
Density
What is the equation for calculating density?
Knowing the density and mass of an object, how is its volume calculated?
Knowing the density and volume of an object, how is its mass calculated?
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Example 1L.1 Density
Calculate the mass of magnesium that occupies the same volume as 94.3 g of iron.
Density of Mg = 1.74 g/cm3 and Fe = 7.87 g/cm3.
Exercise 1L.1
A cubic block of pure metal which is 4.0 cm long weighed1.26 lb. (1 lb = 453.6 g)
The metal is:
a. Al, d = 2.70 g/cm3
d. Ag, d = 10.5 g/cm3
b. Cu, d = 8.96 g/cm3
e. Au, d = 19.3 g/cm3
3
c. Pb, d = 11.4 g/cm
Temperature
Temperature is the property of matter that …
The freezing point and boiling point of water on the Celsius and Fahrenheit scales are …
The relationship between 0F and 0C is …
The Kelvin Temperature Scale
The relationship between temperatures in K and 0C is …
Temperature Dependence of Physical Properties
What is the seasonal “turnover” of water in lakes?
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Extensive and Intensive Properties
Extensive properties depend on …
Intensive properties are those that …
Exercise 1L.2
All of the following are intensive properties EXCEPT
a. color
d. melting point
b. density
e. solubility
c. heat
1.5
Physical and Chemical Change
What is a physical change?
What is a chemical change?
Exercise 1L.3
Which of the following results in a physical change and not a chemical change?
a. A banana peel turning a dark color
b. The development of a Polaroid picture
c. Making a cup of tea from a tea bag and hot water
d. The souring of milk
e. Bleaching of hair
Exercise 1L.4
Which of the following is (are) chemical change(s)?
1. rusting
2. boiling
3. cooking
a. 1 only
b. 3 only
c. 1 and 2 only
d. 1 and 3 only
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e. 1, 2, and 3
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1.6
UNITS OF MEASUREMENT
What are some examples of qualitative measurements?
How are they different from quantitative measurements?
SI Units
What are the SI base units?
metric prefixes Appendix C
1.7
USING NUMERICAL INFORMATION
For each conversion factor, the numerator of the factor must be equivalent to the denominator.
A single relationship such as 1 cal = 4.184 J gives two conversion factors.
1cal
4.184 J
or
4.184 J
1cal
Initial quantity x conversion factor(s) = desired quantity
Conversion factor used must cancel given units
Example 1L.2 Conversions
The average velocity of hydrogen molecules at O°C is 1.69 x 105 cm/s. Convert this
value to miles per hour using the following conversion factors.
1 in. = 2.54 cm
1ft. = 12 in
1 mile = 5280 ft
1min.= 60 s
1 hr. = 60 min
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Exercise IL.5
All of the following are equivalent EXCEPT
a. 0.001 mL = 10-6 L
b. 10 cm = 100 mm
c. 10 C = 1 K
d. 100 g = 10-3 g
e. 10 Mg = 104 kg
EXAMPLE IL.3 Units of Volume
A volumetric flask has the volume of 0.001000 L. What is its volume in cubic
centimeters and milliliters?
EXAMPLE lL.4 Density in Different Units
A piece of iron with a volume of 1.452 gal. weighs 95.31 Lbs. Calculate the density of iron in
scruple/drachm. Some conversion factors are:
1.00 L = 0.264 gal
1.000 kg = 2.205 lb
1.000 scruple = 1.296 g
1.000 mL = 0.2816 drachm
1000 g = 1 kg
1000 mL = 1.00 L
Exercise lL.6
The heat of combustion of glucose, C6H12O6, is -15600 J.g-1. Expressed in kJ kg-1, the heat of
combustion is
a. -1.56 x 101 kJ.kg-1
b. -1.56 x 104 kJ.kg-1
c. -1.56 x 106 kJ.kg-1
d. -1.56 x 107 kJ.kg-1
e. -1.56 x 109 kJ.kg-1
Precision, Accuracy, and Experimental Error
What is meant by the precision of a measurement?
What is accuracy?
What is the average deviation?
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EXAMPLE lL.5 Precision and Accuracy
Student A titrated a 1.000 g sample of NaHCO3 with a sodium hydroxide using a buret with
markings every tenth of a mL, whereas student B used a buret with markings at every mL. The
following results were reported:
Student A
Deviation from
Average
Student B
Deviation from
Average
35.6 mL
35.2
36.0
34.9
Ave = 35.4
35.12 mL
34.88
35.24
34.75
Ave = 35.10
Calculate the average deviation for each set of data. Whose results are more precise?
Significant Figures
A calculated result can be no more precise than the least precise piece of information that went
into the calculation.
Guidelines for Determining Significant Figures
Rule1
To determine the number of significant figures in a measurement that contains a decimal, read
the number from left to right and count all digits, starting with the first digit that is not zero.
Rule 2
When adding or subtracting numbers, the number of decimal places in the answer should be
equal to the number of decimal places in the number with the fewest places.
Rule 3
In multiplication or division, the number of significant figures in the answer should be the same
as that in the quantity with the fewest significant figures.
Rule 4
When a number is rounded off, the last digit to be retained is increased by one only if the
following digit is 5 or greater.
Exercise lL.7
The number of significant figures in 405000 is
a. 2
b. 3
c. 4
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d. 5
e. 6
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Exercise lL.8
Four samples were weighed using four different balances. (All are as precise as indicated by
the individual masses.) The masses are 0.94 kg, 58.2 g, 1.55 g, and 250 mg. The total mass
should be reported as …
Exercise 1L.9
A physics student measured the electronic charge of one electron by using the Millikan oil
droplet experiment and obtained the following three values:
4.635 x 10-10 esu
4.923 x 10-10 esu
4.768 x 10-10 esu
Which of the following values should he report?
4.7753 x 10-10 esu
4.775 x 10-10 esu
4.78 x 10-10 esu
4.8 x 10-10 esu
5 x 10-10 esu
1.8
PROBLEM SOLVING
Step 1. Define the problem.
Step 2. Develop a plan.
Step 3. Execute the plan.
Step 4. Is the answer reasonable?
EXAMPLE 1L.6 Problem Solving
A 0.680 g sample of paraffin oil with a density of 0.858 g/cm3 was spread over the
surface of water in a large beaker which has a diameter of 154 mm. How thick is the
oil layer in centimeters?
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