3. 1.1 Units
I will be able to…
• Identify metric and English
units of measurement.
• Explain why scientists use SI
units.
• Measure quantities using
appropriate units for
measurement.
4. 1.1 Units
•Unit – a quantity adopted as a standard
of measurement.
• Measurements must include a quantity
and a unit.
•The two most commonly used units of
measurement are
• English (Imperial) System
• Metric System
7. 1.1 Units
•The English System
• Distance = inch, foot, yard, mile
• Mass = ounce, pound, ton, slug (1 slug = 12 blobs)
• Volume = ounce, cup, pint, quart, gallon
• Time = second, minute, hour, day, year
• Temperature = Fahrenheit
Many English units were based off body
parts of influential people and varied
from region to region.
8. 1.1 Units
•The Metric System
• Distance = cm, m, km
• Mass = gram, kg
• Volume = milliliter, liter
• Time = second, minute, hour, day, year
• Temperature = Celsius
The international prototype kilogram is
made of 90% platinum and 10% iridium.
This mixture of metals is extremely
resistant to environmental factors that
may affect its mass. It is held under very
tight security in St. Cloud, France.
9. 1.1 Units
•Since 1960, scientists worldwide have
used a set of units called the International
System (Le Systeme Internationale in
French) or SI.
11. 1.2 Unit Conversions
I will be able to…
• Define conversion factor.
• Convert from one unit to
another using conversion
factors and dimensional
analysis.
12. 1.2 Unit Conversions
•To change between units of the same
measurement scientists use conversion
factors.
13. 1.2 Unit Conversions
•Conversion Factor – a ratio of the equality
of two different units of the same
measurement.
• Can be used to convert from one unit to
another.
14. 1.2 Unit Conversions
1 hr = 60 min 1 min = 60 sec 1 km = 1000 m 7 days = 1 week
24 hrs = 1 day 1 kg = 2.2 lbs 1 gal = 3.79 L 264.2 gal = 1 m3
1 mi = 5,280 ft 1 kg = 1000 g 1 lb = 16 oz 20 drops = 1 mL
365 days = 1 yr 52 weeks = 1 yr 2.54 cm = 1 in 1 L = 1000 mL
0.621 mi = 1.00 km 1 yd = 36 inches 1 cc is 1 cm3 1 mL = 1 cm3
17. 1.2 Unit Conversions
EXAMPLE
• A high school cross country race is 5
kilometers. How many miles is a cross
country race?
18. 1.2 Unit Conversions
EXAMPLE
• A high school cross country race is 5
kilometers. How many miles is a cross
country race? How many feet?
19. 1.2 Unit Conversions
EXAMPLE
• A high school cross country race is 5
kilometers. How many miles is a cross
country race? How many feet? How
many inches?
20. 1.2 Unit Conversions
•Temperature Conversions
• T°C = Temperature in Degrees Celsius
• T°F = Temperature in Degrees Fahrenheit
• TK = Temperature in Degrees Kelvin
26. 1.3 Density
I will be able to…
• Define and provide
appropriate units for mass,
volume, and density.
• Solve density problems.
27. 1.3 Density
•Volume – the space an object occupies.
• Base Unit = Liter (L)
• Volume of Rectangular Prism = l * w * h
• Volume of a Cylinder = π * r2 * h
• Volume of a Sphere =
4
3
* π * r3
Rectangular Prism Cylinder
Sphere
28. 1.3 Density
•Mass – a measure of the amount of
matter in an object.
• Base Unit = Gram (g)
• Mass ≠ Weight
29. 1.3 Density
•Density - the amount of
matter present in a given
volume of substance.
• The density of a substance
always remains constant.
31. 1.3 Density
EXAMPLE
•The five liquids in the
table were added to a
graduated cylinder.
Identify each liquid
based on the
densities provided in
the table.
33. 1.3 Density
EXAMPLE
•A mason is trying to determine the density
of bricks to determine their quality. Each
brick has a mass of 3.00 x 103 g. Each brick
measures 15 cm x 8 cm x 45 cm. What is
the density (g/cm3) of each brick?
34. 1.3 Density
EXAMPLE
•A shot put has a density of 7.86
grams/cm3. A shot put has a mass of
7.260 kg. What is the volume (cm3) of the
shot put? What metal is the shot put
made of?
35. 1.3 Density
EXAMPLE
•A sample of metal has
a density of 2.699
grams/cm3. The
sample also has a
volume 18.20 cm3.
What is the mass (g)
of the metal sample?
What metal is the
sample made of?
36. 1.4 Significant Figures
I will be able to…
• Define uncertainty.
• Identify the number of significant
figures in a measurement.
• Round numbers to the correct
numbers of significant figures or
decimals.
• Calculate answers and determine
the proper number of significant
figures or decimals.
37. 1.4 Significant Figures
•Uncertainty – the possibility of error in
a measurement.
• When measurements are taken most tools
are not precise and accurate enough to
get exact measurements. To compensate
for this scientists, use significant figures.
38. 1.4 Significant Figures
• Significant Figure – digits that
carry meaning in a
measurement.
• Significant Figures = Sig Figs
• Sig figs are certain (known)
numbers.
• Sig figs determine how answers
are rounded during calculations.
• Sig figs are necessary in science
because they represent
measurements as accurately as
possible.
39. 1.4 Significant Figures
•When measurements are taken
• All certain digits are recorded.
• The last digit is uncertain and you must
estimate the digit.
46. 1.4 Significant Figures
•The Atlantic Ocean
is on our right when
we look at a map.
•The Pacific Ocean is
on our left when we
look at a map.
•You are a swimmer.
47. 1.4 Significant Figures
• If a decimal is ABSENT
you start swimming
on the ATLANTIC side
of the number.
• You can only “swim”
through zeros.
• Once you hit a
number between 1
and 9 you stop
“swimming”.
• All the numbers left
(including zeros) are
significant.
49. 1.4 Significant Figures
• If a decimal is PRESENT you
start swimming on the
PACIFIC side of the number.
• You can only “swim”
through zeros.
• Once you hit a number
between 1 and 9 you stop
“swimming”.
• All the numbers left
(including zeros) are
significant.
51. 1.4 Significant Figures
•Multiplying and Dividing
• The answer should have the same number
of sig figs, as the number with the fewest
sig figs in your problem.
52. 1.4 Significant Figures
EXAMPLES
•How many significant figures should each
answer have? Calculate the answer.
• 834 * 1.002 =
• 7.3 / 2342 =
• 43 * 3.453 =
53. 1.4 Significant Figures
•Adding and Subtracting
• The answer should have the same number
of decimal places, as the number with the
fewest decimal places in the problem.
54. 1.4 Significant Figures
EXAMPLES
•How many decimal places should each
answer have? Calculate the answer.
• 834.7 + 1.002 =
• 7.3 - 2342 =
• 43.4345 + 3.453 =
55. 1.4 Significant Figures
EXAMPLES
•Write the following numbers in scientific
notation, using the given number of sig figs.
• 1,000,000 with two significant figures.
• 1,000,000 with three significant figures.
• 2,232,450 with two significant figures.
56. 1.5 Scientific
Notation
I will be able to…
• Express numbers in both
standard notation and
scientific notation.
• Solve addition, subtraction,
multiplication, and division
problems involving numbers
written in scientific notation.
58. 1.5 Scientific Notation
•Coefficient = a number greater than or
equal to 1 and less than 10.
•Base = must be 10
•Exponent = shows the number of decimal
places that the decimal needs to moved
to change the number to standard
notation.