i ii iii units of measurement ch. 2 - measurement
TRANSCRIPT
I
II
III
Units of Measurement
CH. 2 - MEASUREMENT
A. Number vs. Quantity
Quantity - number + unit
UNITS MATTER!!
I
II
III
II. Using Measurements
CH. 2 - MEASUREMENT
A. Accuracy vs. Precision
Accuracy - how close a measurement is to the accepted value
Precision - how close a series of measurements are to each other
ACCURATE = CORRECT
PRECISE = CONSISTENT
A. Accuracy vs. Precision
B. Percent Error
Indicates accuracy of a measurement
100accepted
acceptedalexperimenterror %
your value
given value
B. Percent Error
A student determines the density of a substance to be 1.40 g/mL. Find the % error if the accepted value of the density is 1.36 g/mL.
100g/mL 1.36
g/mL 1.36g/mL 1.40error %
% error = 2.9 %
C. Significant Figures
Indicate precision of a measurement.
Recording Sig Figs
Sig figs in a measurement include the known digits plus a final estimated digit
2.31 cm
C. Significant Figures Counting Sig Figs
Digits from 1-9 are always significant.
Zeros between two other sig figs are always significant
One or more additional zeros to the right of both the decimal place and another sig digit are significant
Count all numbers EXCEPT: Leading zeros -- 0.0025 Trailing zeros without
a decimal point -- 2,500
5085
2.60
739
4. 0.080
3. 5,280
2. 402
1. 23.50
C. Significant Figures
Counting Sig Fig Examples
1. 23.50
2. 402
3. 5,280
4. 0.080
4 sig figs
3 sig figs
3 sig figs
2 sig figs
C. Significant Figures
Calculating with Sig Figs
Multiply/Divide - The # with the fewest sig figs determines the # of sig figs in the answer.
(13.91g/cm3)(23.3cm3) = 324.103g
324 g
4 SF 3 SF3 SF
C. Significant Figures
Calculating with Sig Figs (con’t)
Add/Subtract - The # with the lowest decimal value determines the place of the last sig fig in the answer.
3.75 mL
+ 4.1 mL
7.85 mL
224 g
+ 130 g
354 g 7.9 mL 350 g
3.75 mL
+ 4.1 mL
7.85 mL
224 g
+ 130 g
354 g
C. Significant Figures
Calculating with Sig Figs (con’t)
Exact Numbers do not limit the # of sig figs in the answer.Counting numbers: 12 studentsExact conversions: 1 m = 100 cm “1” in any conversion: 1 in = 2.54 cm
C. Significant Figures
5. (15.30 g) ÷ (6.4 mL)
Practice Problems
= 2.390625 g/mL
18.1 g
6. 18.9 g
- 0.84 g18.06 g
4 SF 2 SF
2.4 g/mL2 SF
D. Scientific Notation
A way to express any number as a number between 1 and 10 (coefficient) multiplied by 10 raised to a power (exponent)
Number of carbon atoms in the Hope diamond
460,000,000,000,000,000,000,000
4.6 x 1023
Mass of one carbon atom
0.00000000000000000000002 g
2 x 10-23 g coefficient exponent
D. Scientific Notation
Converting into Sci. Notation:
Move decimal until there’s 1 digit to its left. Places moved = exponent.
Large # (>1) positive exponentSmall # (<1) negative exponent
Only include sig figs.
65,000 kg 6.5 × 104 kg
D. Scientific Notation
7. 2,400,000 g
8. 0.00256 kg
9. 7 10-5 km
10. 6.2 104 mm
Practice Problems
2.4 106 g
2.56 10-3 kg
0.00007 km
62,000 mm
D. Scientific Notation
Calculating with Sci. Notation
(5.44 × 107 g) ÷ (8.1 × 104 mol) =
5.44EXPEXP
EEEE÷÷
EXPEXP
EEEE ENTERENTER
EXEEXE7 8.1 4
= 671.6049383 = 670 g/mol = 6.7 × 102 g/mol
Type on your calculator:
D. Scientific Notation
11. (4 x 102 cm) x (1 x 108cm)
12. (2.1 x 10-4kg) x (3.3 x 102 kg)
13. (6.25 x 102) ÷ (5.5 x 108)
14. (8.15 x 104) ÷ (4.39 x 101)
15. (6.02 x 1023) ÷ (1.201 x 101)
Practice Problems
4 1010 cm2
6.9 10-2 kg2
1.1 x 10-6
1.86 x 103
5.01 x 1022
Chemistry Binder Organization
Chemistry Binder: (8 tabs)
Reference:
Administrative papers (policies & procedures, etc)
Chemistry reference handouts (Periodic Table, Chemical Reference Sheet, etc)
Notes
Filler Paper for lecture notes
Handouts or worksheets to supplement textbook
Divided by chapter or unit – there are 7 separate sections for the first semester
E. Derived Units
Combination of base units.
Volume (m3 or cm3) length length length
D = MV
1 cm3 = 1 mL1 dm3 = 1 L
Density (kg/m3 or g/cm3)mass per volume
F. DensityM
ass
(g)
Volume (cm3)
Δx
Δyslope D
V
M
F. Density
An object has a volume of 825 cm3 and a density of 13.6 g/cm3. Find its mass.
GIVEN:
V = 825 cm3
D = 13.6 g/cm3
M = ?
WORK:
M = DV
M = (13.6 g/cm3)(825cm3)
M = 11,200 g
V
MD
F. Density
A liquid has a density of 0.87 g/mL. What volume is occupied by 25 g of the liquid?
GIVEN:
D = 0.87 g/mL
V = ?
M = 25 g
WORK:
V = M D
V = 25 g
0.87 g/mL
V = 29 mLV
MD
Homework
Complete Worksheet “Using Measurements – Chapter 2”: due Monday (skip section on Dimensional Analysis – we will learn this next week )
Study for test tomorrow
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Dimensional Analysis
Conversion Factors
Problems
A. Problem-Solving Steps
1. Analyze
2. Plan
3. Compute
4. Evaluate
B. Dimensional Analysis
Dimensional Analysis A tool often used in science for
converting units within a measurement system
Conversion Factor A numerical factor by which a quantity
expressed in one system of units may be converted to another system
3
3
cm
gcm
B. Dimensional Analysis
The “Factor-Label” Method Units, or “labels” are canceled, or
“factored” out
g
B. Dimensional Analysis
Steps:
1. Identify starting & ending units.
2. Line up conversion factors so units cancel.
3. Multiply all top numbers & divide by each bottom number.
4. Check units & answer.
Fractions in which the numerator and Fractions in which the numerator and denominator are EQUAL quantities denominator are EQUAL quantities expressed in different unitsexpressed in different units
Example: 1 in. = 2.54 cm
Factors: 1 in. and 2.54 cm
2.54 cm 1 in.
C. Conversion FactorsC. Conversion Factors
Conversion factor
cancel
By using dimensional analysis / factor-label method, By using dimensional analysis / factor-label method, the UNITS ensure that you have the conversion right the UNITS ensure that you have the conversion right side up, and the UNITS are calculated as well as the side up, and the UNITS are calculated as well as the
numbers!numbers!
How many minutes are in 2.5 hours?
2.5 hr 2.5 hr x x 60 min60 min
1 hr
= 150 min
Write conversion factors that Write conversion factors that relate each of the following relate each of the following pairs of units:pairs of units:
1. Liters and mL1. Liters and mL
2. Hours and minutes2. Hours and minutes
3. Meters and kilometers3. Meters and kilometers
C. Conversion FactorsLearning Check:
1 L1000 mL
1 hr60 min
1000 m1 km
You have $7.25 in your You have $7.25 in your pocket in quarters. How pocket in quarters. How many quarters do you many quarters do you have?have?
7.25 dollars 4 quarters7.25 dollars 4 quarters
1 dollar1 dollar
X = 29 quarters= 29 quarters
D. Dimensional Analysis Practice
How many seconds are in 1.4 days?
Plan: days hr min seconds1.4 days x 24 hr x 60 min x 60 sec =
1 day1 hr 1 min
D. Dimensional Analysis Practice
120960 sec 120000 sec
D. Dimensional Analysis Practice
How many milliliters are in 1.00 quart of milk?
1.00 qt 1 L
1.057 qt= 946 mL
qt mL
1000 mL
1 L
You have 1.5 pounds of gold. Find its volume in cm3 if the density of gold is 19.3 g/cm3.
lb cm3
1.5 lb 1 kg
2.2 lb= 35 cm3
1000 g
1 kg
1 cm3
19.3 g
D. Dimensional Analysis Practice
5) Your European hairdresser wants to cut your hair 8.0 cm shorter. How many inches will he be cutting off?
8.0 cm 1 in
2.54 cm= 3.1 in
cm in
D. Dimensional Analysis Practice
6) Roswell football needs 550 cm for a 1st down. How many yards is this?
550 cm 1 in
2.54 cm= 6.0 yd
cm yd
1 ft
12 in
1 yd
3 ft
D. Dimensional Analysis Practice
7) A piece of wire is 1.3 m long. How many 1.5-cm pieces can be cut from this wire?
1.3 m 100 cm
1 m= 86 pieces
m pieces
1 piece
1.5 cm
D. Dimensional Analysis Practice
How many liters of water would fill a container that measures 75.0 in3?
75.0 in3 (2.54 cm)3
(1 in)3= 1.23 L
in3 L
1 L
1000 cm3
D. Dimensional Analysis Practice