chapter 1 biochemistry study guide
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Chapter 1 ³Measurement´
1.1 Units of Measurement
Length
o Meter (m) ± slightly longer than a yard
1 m = 100 cm
1 m = 39.4 in.
o Centimeter (cm) ± smaller unit of length
and commonly used in chemistry
2.54 cm = 1 in.
Volume ± amount of space a substance
occupies
o Liter (L) ± slightly larger than the quart
and commonly used to measure volume
1 L = 1000 mL
1 L = 1.06 qt
o Milliliter (mL) ± more convenient for
measuring smaller volume of fluids in
hospital or lab
946 mL = 1 qt
Mass (weight) ± measure of the quantity of
material it contains
o Gram (g)
454 g = 1 lb
o Kilogram (kg)
1 kg = 1000 g
1 kg = 2.20 lb
Temperature ± how hot or cold that object is
(metric system measured on the Celsius
temperature scale but SI system measured on
the Kelvin (K) temperature scale
o Celsius (°C) scale ± water freezes at
0 °C and boils at 100 °C
o Fahrenheit (°F) scale ± water freezes at
32 °F and boils at 212 °F
o Kelvin (K) ± 0 K
Time
o Years
o Days
o Minutes
o Seconds
Table 1.1 ³Units of Measurement´
Measurement Metric SI
Length Meter (m) Meter (m)
Volume Liter (L) Cubic meter
(m3)
Mass Gram (g) Kilogram (kg)
Time Second (s) Second (s)
Temperature Celsius (°C) Kelvin (K)
1.2 Scientific Notation
Scientific notation ± easy way to write small and
large numbers
o Example
Width of a human hair is
0.000008 m, but in scientific
notation is 8 * 10-6
m
Writing a number in scientific notation:
o Two parts ±
A coefficient
Power of 10
o Example
2.4 * 103
Coefficient is 2.4
103
shows the power of 10
Table 1.2 ³Some Powers of 10´
Number Multiples of Ten Scientific
Notation
10000 10*10*10*10 1 * 104
1000 10*10*10 1 * 103
100 10*10 1 * 102
10 10 1 * 101
1 0 1 *100
0.1 1/10 1 * 10-1
0.01 1/10*1/10 = 1/100 1 * 10-2
0.001 1/10*1/10*1/10 =
1/1000
1 * 10-3
0.0001 1/10*1/10*1/10*1/10
= 1/10000
1 * 10-4
Scientific notation and calculators:
o Using the EE or EXP key on calculator
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1.3 Measured Numbers and Significant Figures
Measured numbers ± number that I obtain from
using a measuring tool
o Example
Height
Weight
Temperature
Table 1.4 ³Significant Figures in Measured
Numbers´
Rule Measured
Number
Number of
Significant
Figures
A number is a
significant figure
if it is
(a) Not a
zero
4.5 g 2
122.35 m 5
(b) A zero
b/t
nonzero
digits
205 m 3
5.082 kg 4
(c) A zero at
the end
of a
decimal
number
50. L 2
25.0 °C 3
16.00 g 4
(d) Any digit
in the
coefficient of a
number
written in
scientific
notation
4.0 * 105
m 2
5.70 * 10-3
g 3
A zero is not
significant if it is
(a) At the
beginnin
g of a
decimal
number
0.0004 lb 1
0075 m 2
(b) Used as
a
placehol
der in a
large
number
without a
decimal
point
850000 m 2
1250000 g 3
Significant figures ± all the digits including the
estimated digit
Exact numbers ± numbers obtained by counting
items
o Example
1 ft = 12 in.
1 qt = 4 cups
1 lb = 16 ounces
1 L = 1000 mL
1 m = 100 cm
1 kg = 1000 g
1.4 Significant Figures in Calculations
Rounding off
o Rules for rounding off:
If the first digit to be
dropped is 4 or less, it and
all following digits are
simply dropped from the
number
If the first digit to be
dropped is 5 or greater, the
last retained digit of the
number is increased by 1
Example:
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y 8.4234 rounds off to
8.42 or 8.4
y 14.780 rounds off to
14.8 or 15
Multiplication and division ± final answer is
written so it has the same number of
significant figures as the measurement with
the fewest significant figures (SFs)
o Example
24.65 * 0.67 = 16.5155 ± 17
Adding significant zeros ± significant zeros
may need to be written after the calculator
result
o Example
8.00 / 2.00 = 4 = 4.00
Addition and subtraction ± final answer iswritten so it has the same number of
decimal places as the measurement with the
fewest decimal places
o Example
2.045 + 34.1 = 36.145 =
36.1
1.5 Prefixes and equalities
Prefix ± attached to any unit to increase or
decrease its size by some factor of ten Prefixes that increase the size of the unit ±
o Tera = 1000000000000
o Giga = 1000000000
o Mega = 1000000
o Kilo = 1000
Prefixes that decrease the size of the unit ±
o Deci = 0.1
o Centi = 0.01
o Milli = 0.001
o Micro = 0.000001
o Nano = 0.000000001
o Pico = 0.000000000001
Measuring length
o Some length qualities:
1 m = 100 cm
1 m = 1000 mm
1 cm = 10 mm
Measuring volume
o Some volume equalities:
1 L = 10 dL
1 L = 1000 mL
1 dL = 100 mL
o Cubic centimeter (cm3)
1 cm3
= 1 cc = 1 mL
Measuring mass
o Some mass equalities:
1 kg = 1000 g
1 g = 1000 mg
1 mg = 1000 µg
1.6 Writing Conversion Factors
Conversion factors ± one of the quantities is
the numerator and the other is thedenominator
o Example
Numerator / Denominator
60 min / 1 h and 1 h / 60
min
Metric conversion factors
o Example
Metric equality (1 m = 100
cm) Conversion factors (100 cm
/ 1 m and 1 m / 100 cm)
Table 1.9 ³Some Common Equalities
Quantity U.S. Metric (SI) Metric (U.S)
Length
1 ft = 12 in. 1 km =
1000 m
2.54 cm = 1
in.
1 yard = 3 ft 1 m = 1000
mm
1 m = 39.4
in.
1 mile =
5280 ft
1 cm = 10
mm
1 km =
0.621 mi
Volume
1 qt = 4
cups
1 L = 1000
mL
946 mL = 1
qt
1 qt = 2 pt 1 dL = 100 1 L = 1.06
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mL qt
1 gallon = 4
qt
1 mL = 1
cm3
Mass
1 lb = 16 oz 1 kg = 1000
g
1 kg = 2.20
lb
1 g = 1000mg
454 g = 1 lb
Time
1 h = 60
min
1 min = 60 s
Metric (U.S) system conversion factors
o Example
1 kg = 2.20 lb
Conversion factors
y 2.20 lb / 1 kg or 1 kg /
2.20 lb
Conversion factors stated within a problem
o Example
1 h = 85 km
Conversion factors
y 85 km / 1 h or 1 h / 85
km
Conversion factors for a percentage, ppm, and
ppb
o Example
18% body fat by mass = 100 kg
body mass
Conversion factors
y 100 kg body mass / 18
kg body fat or 18 kg
body fat / 100 kg body
mass
1.7 Problem Solving
Example
o Given quantity * one or more
conversion factors = desired
quantity
Guide to problem solving (GPS) using
conversion factors
o Given/Need
o Plan
o Equalities/Conversion Factors
o Set Up Problem
Using two or more conversion factors ± each
factor is arranged to cancel the preceding
unit until the final unit is obtained
1.8 Density
Density ± to determine an object will sink or
float
Formula
o Density = mass of substance /
volume of substance
Density of solids ± calculated from its mass
and volume
Specific gravity (sp gr) ± ratio between thedensity of a substance and the density of
water
Formula
o Specific gravity = density of sample
/ density of water