Honors Chemistry, Chapter 2 Page 1. Evolution of a Gas (Bubbles, Odor) Formation of a Precipitate...
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Transcript of Honors Chemistry, Chapter 2 Page 1. Evolution of a Gas (Bubbles, Odor) Formation of a Precipitate...
Honors Chemistry, Chapter 2Page 1
Evolution of a Gas (Bubbles, Odor) Formation of a Precipitate (Formation
of Cloudiness in a Clear Solution, Solids Collecting at the Bottom or Top)
Release of Energy (Heat, Light) Color Change
Honors Chemistry, Chapter 2Page 2
Observing and Collecting Data• Qualitative (Bubbles Formed)• Quantitative (1 gram/liter of catalyst
speeded the reaction by 25%)• Chemists Study Systems (Region Selected
for Study) Formulate Hypothesis
• Generalization about Data • Testable Statement
Honors Chemistry, Chapter 2Page 3
Testing Hypothesis (Experimentation)• Supported, Retained• Not Supported, Discarded, Modified
Theorizing – Create a Model• Model: An Explanation of How Phenomena
Occur and How Data or Events are Related. Visual Verbal Mathematical
Honors Chemistry, Chapter 2Page 4
Honors Chemistry, Chapter 2Page 5
JFHICW FH VHHVLBFND FL N ZGVHFIVLB, BTV NZZVNGNLPV CY JFHICW JFDD IC FL N PNLIFINBV. – VGFP HVRNGVFI.
JFHICW FH VHHVLBFND FL N ZGVHFIVLB, BTV NZZVNGNLPV CY JFHICW JFDD IC FL N PNLIFINBV. – VGFP HVRNGVFI.
(Wisdom is essential in a president, the appearance of wisdom will do in a candidate. – Eric Severeid)
Honors Chemistry, Chapter 2Page 6
1. What is the purpose of the scientific method?
2. Distinguish between qualitative and quantitative observations.
3. Describe the differences between hypothesis, theories, and models.
Honors Chemistry, Chapter 2Page 7
Measurements Are Quantitative Information
Quantity: Something That Has Size or Amount
Honors Chemistry, Chapter 2Page 8
SI Units Are Defined in Terms of Standards of Measurement
Seven Basic Units All Others Derived From Seven Basic
Units
Honors Chemistry, Chapter 2Page 9
Quantity Symbol Unit Abbreviation
Length l meter m
Mass m Kilogram Kg
Time t second s
Thermodynamic Temperature T Kelvin K
Amount of a Substance n mole mol
Electric Current I ampere ALuminous Intensity Iv candela cd
Honors Chemistry, Chapter 2Page 10
Prefix AbbreviationExponent Multiplier Meaning Example Using Length
tera- T 10121000000000000 1 terameter (Tm)
giga- G 1091000000000 1 gigameter (Gm)
mega- M 1061000000 1 megameter (Mm)
kilo- k 1031000 1 kilometer (km) = 1000 m
hecto- h 102100 1 hectometer (hm) = 100 m
deka- da 10110 1 dekameter (dam) = 10 m
1001 1 meter (m)
Honors Chemistry, Chapter 2Page 11
Prefix AbbreviationExponent Multiplier Meaning Example Using Length
1001 1 meter (m)
deci- d 10-10.1 1 decimeter (dm)
centi- c 10-20.01 1 centimeter (cm)
milli- m 10-30.001 1 millimeter (km)
micro- 10-60.000001 1 micrometer (m)
nano- n 10-90.00000001 1 nanometer (nm)
pico- p 10-120.000000000001 1 picometer (pm)
Honors Chemistry, Chapter 2Page 12
Honors Chemistry, Chapter 2Page 13
Useful Conversion Factors
• 1000 ml = 1 L
• 1 cm3 = 1 ml
• 1000 g = 1 kg
• 1000 mg = 1 g
• 1000 g = 1 mg
• 1000000 g = 1 g
• 1000 mmol = 1 mol
1. 1000 m = 1 1. 1000 m = 1 ______ a) mm b) km a) mm b) km
c) dmc) dm
2. 0.001 g = 1 2. 0.001 g = 1 ___ ___ a) mg b) kg a) mg b) kg
c) dgc) dg
3. 0.1 L = 1 3. 0.1 L = 1 ______ a) mL b) cL c) dLa) mL b) cL c) dL
4. 0.01 m = 1 ___ 4. 0.01 m = 1 ___ a) mm b) cm c) dma) mm b) cm c) dm
? kilometer (km) = 500 meters (m)? kilometer (km) = 500 meters (m) 2.5 meter (m) = ? centimeters (cm)2.5 meter (m) = ? centimeters (cm) 1 centimeter (cm) = ? millimeter (mm)1 centimeter (cm) = ? millimeter (mm) 1 nanometer (nm) = 1.0 x 101 nanometer (nm) = 1.0 x 10-9-9 meter meter
O—H distance =O—H distance =9.4 x 109.4 x 10-11 -11 mm9.4 x 109.4 x 10-9 -9 cmcm0.094 nm0.094 nm
O—H distance =O—H distance =9.4 x 109.4 x 10-11 -11 mm9.4 x 109.4 x 10-9 -9 cmcm0.094 nm0.094 nm
Select the unit you would use to measure Select the unit you would use to measure 1. Your height1. Your height
a) millimeters a) millimeters b) metersb) meters c) c) kilometerskilometers2. Your mass2. Your mass
a) milligramsa) milligrams b) gramsb) grams c) kilograms c) kilograms
3. The distance between two cities3. The distance between two cities a) millimetersa) millimeters b) metersb) meters c) kilometers c) kilometers
4. The width of an artery4. The width of an arterya) millimetersa) millimeters b) metersb) meters c) kilometers c) kilometers
Area A m2
Volume V m3
Density D kg/m3 (=m/V) Molar Mass M kilograms/mol Concentration c mol/liter Molar Volume Vm m3/mol Energy E joule
Honors Chemistry, Chapter 2Page 18
Relationship Between D, m, and V:
Honors Chemistry, Chapter 2Page 19
D
m
V
StrategyStrategy1.1. Use density to calc. mass (g) from Use density to calc. mass (g) from
volume.volume.2.2. Convert mass (g) to mass (lb)Convert mass (g) to mass (lb)
Need to know conversion factorNeed to know conversion factor= 454 g / 1 lb= 454 g / 1 lb
First, note thatFirst, note that 1 cm1 cm33 = 1 mL = 1 mL
1.1. Convert volume to massConvert volume to mass
95 cm3 • 13.6 g
cm3 = 1.3 x 103 g
1.3 x 103 g • 1 lb
454 g = 2.8 lb
2.2. Convert mass (g) to mass (lb)Convert mass (g) to mass (lb)
Osmium is a very dense metal. What is its Osmium is a very dense metal. What is its density in g/cmdensity in g/cm3 3 if 50.00 g of the metal if 50.00 g of the metal occupiesoccupiesa volume of 2.22cma volume of 2.22cm33??
1) 2.25 g/cm1) 2.25 g/cm33
2)2) 22.5 g/cm22.5 g/cm33
3)3) 111 g/cm111 g/cm33
2) Placing the mass and volume of the 2) Placing the mass and volume of the osmium metal into the density setup, we osmium metal into the density setup, we obtainobtain
D = D = massmass = = 50.00 g 50.00 g = = volumevolume 2.22 cm2.22 cm33
= 22.522522 g/cm= 22.522522 g/cm33 == 22.5 g/cm22.5 g/cm33
A solid displaces a matching volume of A solid displaces a matching volume of water when the solid is placed in water.water when the solid is placed in water.
33 mL33 mL25 mL 25 mL
What is the density (g/cmWhat is the density (g/cm33) of 48 g of a metal ) of 48 g of a metal if the metal raises the level of water in a if the metal raises the level of water in a graduated cylinder from 25 mL to 33 mL? graduated cylinder from 25 mL to 33 mL? 1) 0.2 g/ cm1) 0.2 g/ cm33 2) 6 g/m 2) 6 g/m33 3) 252 3) 252 g/cmg/cm33
33 mL33 mL 25 mL25 mL
Which diagram represents the Which diagram represents the liquid layers in the cylinder?liquid layers in the cylinder?(K) Karo syrup (1.4 g/mL), (V) (K) Karo syrup (1.4 g/mL), (V) vegetable oil (0.91 g/mL,) (W) vegetable oil (0.91 g/mL,) (W) water (1.0 g/mL)water (1.0 g/mL)
1)1) 2) 2) 3)3)
K
K
W
W
W
V
V
V
K
The density of octane, a component of The density of octane, a component of gasoline, is 0.702 g/mL. What is the mass, gasoline, is 0.702 g/mL. What is the mass, in kg, of 875 mL of octane?in kg, of 875 mL of octane?
1) 0.614 kg1) 0.614 kg
2) 614 kg2) 614 kg
3) 1.25 kg3) 1.25 kg
If blood has a density of 1.05 g/mL, If blood has a density of 1.05 g/mL, how many liters of blood are donated how many liters of blood are donated if 575 g of blood are given?if 575 g of blood are given?
1) 1) 0.548 L0.548 L2) 2) 1.25 L1.25 L3) 3) 1.83 L1.83 L
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.
Write conversion factors that relate Write conversion factors that relate each of the following pairs of units:each of the following pairs of units:1. Liters and mL1. Liters and mL
2. Hours and minutes2. Hours and minutes
3. Meters and kilometers3. Meters and kilometers
Conversion factor
2.5 hr x 2.5 hr x 60 min 60 min = 150 min = 150 min 1 hr1 hr
cancel
By using dimensional analysis / factor-label method, the By using dimensional analysis / factor-label method, the UNITS ensure that you have the conversion right side up, UNITS ensure that you have the conversion right side up, and the UNITS are calculated as well as the numbersand the UNITS are calculated as well as the numbers!!
Express 4.5 kg as grams Begin by Expressing as a Fraction: 4.5 kg
1 Identify Conversion Factor: 1 kg = 1000
grams Express as a Fraction:
Honors Chemistry, Chapter 2Page 33
1 kg 1000 g1 = --------------- or -------------- 1000 g 1 kg
Write Equation Including Proper Factor
Cancel Units Multiply Numbers to Get Final Result
Honors Chemistry, Chapter 2Page 34
4.5 kg 1000 g--------- x -------------- = 4500 g 1 1 kg
Honors Chemistry, Chapter 2Page 35
Factor Label Steps
1. Express as a Fraction2. Identify Conversion Factor3. Express Conversion Factor as Two
Fractions4. Select Proper Factor (units in denom.)5. Write Equation Including Proper Factor6. Cancel Units7. Multiply Numbers to Get Final Result
1. Distinguish between a quantity, a unit, and a measurement standard.
2. Name SI units for length, mass, time, volume, and density.
3. Distinguish between mass and weight.4. Perform a density calculation.5. Transform a statement of equality to a
conversion factor (factor label method).
Honors Chemistry, Chapter 2Page 36
Accuracy – The Closeness of Measurements to the Correct or Accepted Value
Precision – The Closeness of a Set of Measurements
Honors Chemistry, Chapter 2Page 37
Honors Chemistry, Chapter 2Page 38
XXXX
XXXX
High Precision
High Accuracy
High Precision
Low Accuracy
Honors Chemistry, Chapter 2Page 39
Accuracy vs. Precision
X X
X X
X X
X X
Low Precision
Low Accuracy
Low Precision
High Accuracy
(on average)
Valueaccepted - Valueexperimental
%Error = --------------------------------------- Valueaccepted
X 100
Honors Chemistry, Chapter 2Page 40
All the Digits Known With Certainty Plus One Final Digit Which is Somewhat Uncertain
Honors Chemistry, Chapter 2Page 41
| I I I I | I I I I | I I I I | I I I I |
7 8 9
8.36
1. Zeros Appearing Between Nonzero Digits are Significant
2. Zeros Appearing in Front of All Nonzero Digits are Not Significant
3. Zeros Appearing to the Right of the Decimal Point And at the End of the Number are Significant
Honors Chemistry, Chapter 2Page 42
Honors Chemistry, Chapter 2Page 43
Rules for Significant Figures
4. Zeros at the End of a Number but to the Left of the Decimal Point May or May Not be Significant. If a Zero Has Not Been Measured or Estimated but is Just a Placeholder, it is Not Significant. A Decimal Point Placed After Zeros Indicates They are Significant.
If the Digit Following the Last Digit to be Retained is:> 5 Then Round Up< 5 Then Round Down5 Followed by non Zero Digits
Then Round Up
Honors Chemistry, Chapter 2Page 44
Honors Chemistry, Chapter 2Page 45
Rules for Rounding
If the Digit Following the Last Digit to be Retained is:
5 Followed by Non-Zero Digit(s), and Preceeded by an Odd Digit
Round Up
5 Followed by Non-Zero Digit(s), and
Preceeded by an Even Digit
Leave Unchanged
When Adding or Subtracting Decimals, the Answer Must Have the Same Number of Digits to the Right of the Decimal Point as There are in the Measurement Having the Fewest Digits to the Right of the Decimal Point.
Honors Chemistry, Chapter 2Page 46
Honors Chemistry, Chapter 2Page 47
Significant Figures With Multiplication/Division
• When Multiplying or Dividing, the Answer Can Have no More Significant Figures Than are in the Measurement with the Fewest Number of Significant Figures.
• (Conversion Factors Have Unlimited Digits of Accuracy.)
The numbers reported in a The numbers reported in a measurement are limited by the measurement are limited by the measuring toolmeasuring tool
Significant figures in a measurement Significant figures in a measurement include the known digits plus one include the known digits plus one estimated digitestimated digit
RULE 1. All non-zero digits in a measured RULE 1. All non-zero digits in a measured
number are significant. Only a zero could number are significant. Only a zero could indicate that rounding occurred.indicate that rounding occurred.
Number of Significant Figures
38.15 cm38.15 cm 445.6 ft5.6 ft 2265.6 lb65.6 lb ______122.55 m122.55 m ___
RULE 2. Leading zeros in decimal numbers RULE 2. Leading zeros in decimal numbers
are are NOTNOT significant. significant.
Number of Significant Figures
0.008 mm0.008 mm 11
0.0156 oz0.0156 oz 33
0.0042 lb0.0042 lb ________
0.000262 mL 0.000262 mL ____
RULE 3. Zeros between nonzero numbers RULE 3. Zeros between nonzero numbers are significant. (They can not be rounded are significant. (They can not be rounded unless they are on an end of a number.)unless they are on an end of a number.)
Number of Significant Figures
50.8 mm50.8 mm 33
2001 min2001 min 44
0.702 lb0.702 lb ________
0.00405 m0.00405 m ____
RULE 4. Trailing zeros in numbers without RULE 4. Trailing zeros in numbers without
decimals are NOT significant. They are decimals are NOT significant. They are
only serving as place holders.only serving as place holders. Number of Significant Figures
25,000 in. 25,000 in. 22
200. yr200. yr 33
48,600 gal48,600 gal ________
25,005,000 g 25,005,000 g ________
A. Which answers contain 3 significant A. Which answers contain 3 significant figures?figures?1) 0.47601) 0.4760 2) 0.00476 2) 0.00476 3) 4760 3) 4760
B. All the zeros are significant inB. All the zeros are significant in 1) 0.00307 1) 0.00307 2) 25.300 2) 25.300 3) 2.050 x 3) 2.050 x 101033
C. 534,675 rounded to 3 significant figures isC. 534,675 rounded to 3 significant figures is
1) 535 1) 535 2) 535,000 2) 535,000 3) 5.35 x 10 3) 5.35 x 1055
In which set(s) do both numbers In which set(s) do both numbers contain the contain the samesame number of number of significant figures?significant figures?
1) 22.0 and 22.00 1) 22.0 and 22.00
2) 400.0 and 40 2) 400.0 and 40
3) 0.000015 and 150,0003) 0.000015 and 150,000
State the number of significant figures in each State the number of significant figures in each of the following:of the following:A. 0.030 mA. 0.030 m 1 1 2 2 3 3
B. 4.050 LB. 4.050 L 2 2 3 3 4 4
C. 0.0008 gC. 0.0008 g 1 1 2 2 4 4
D. 3.00 mD. 3.00 m 1 1 2 2 3 3
E. 2,080,000 beesE. 2,080,000 bees 3 3 5 5 7 7
A calculated answer cannot be more A calculated answer cannot be more precise than the measuring tool. precise than the measuring tool.
A calculated answer must match the least A calculated answer must match the least precise measurement.precise measurement.
Significant figures are needed for final Significant figures are needed for final answers fromanswers from 1) adding or subtracting1) adding or subtracting
2) multiplying or dividing2) multiplying or dividing
The answer has the same number of The answer has the same number of decimal places as the measurement with decimal places as the measurement with the fewest decimal places.the fewest decimal places.
25.25.22 one decimal placeone decimal place
+ 1.+ 1.3434 two decimal placestwo decimal places 26.5426.54answer 26.5answer 26.5 one decimal placeone decimal place
The answer has the same number of The answer has the same number of decimal places as the measurement with decimal places as the measurement with the fewest decimal places.the fewest decimal places.
25.25.22 one decimal placeone decimal place
+ 1.+ 1.3434 two decimal placestwo decimal places 26.5426.54answer 26.5answer 26.5 one decimal placeone decimal place
In each calculation, round the answer to In each calculation, round the answer to the correct number of significant figures.the correct number of significant figures.A. 235.05 + 19.6 + 2.1 = A. 235.05 + 19.6 + 2.1 =
1) 256.751) 256.75 2) 256.8 2) 256.8 3) 2573) 257
B. 58.925 - 18.2B. 58.925 - 18.2 ==1) 40.7251) 40.725 2) 40.73 2) 40.73 3) 40.73) 40.7
Round (or add zeros) to the Round (or add zeros) to the calculated answer until you have the calculated answer until you have the same number of significant figures same number of significant figures as the measurement with the fewest as the measurement with the fewest significant figures.significant figures.
A. 2.19 X 4.2 =A. 2.19 X 4.2 = 1) 91) 9 2) 9.2 2) 9.2 3) 9.1983) 9.198
B. 4.311 ÷ 0.07 =B. 4.311 ÷ 0.07 = 1)1) 61.5861.58 2) 62 2) 62 3) 603) 60
C. C. 2.54 X 0.00282.54 X 0.0028 = = 0.0105 X 0.060 0.0105 X 0.060 1) 11.31) 11.3 2) 112) 11 3) 0.041 3) 0.041
. l. l22. . . . I . . . . I. . . . I . . . . I33 . . . .I . . . . I . . . .I . . . . I44. . cm. . cm
First digit (known)First digit (known) = 2 = 2 2.?? cm2.?? cmSecond digit (known)Second digit (known) = 0.7 = 0.7 2.7? cm2.7? cmThird digit (estimated) between 0.05- 0.07Third digit (estimated) between 0.05- 0.07Length reportedLength reported == 2.75 cm 2.75 cm
oror 2.74 2.74 cm cm
oror 2.76 2.76 cmcm
In 2.76 cm…In 2.76 cm…
• Known digitsKnown digits 2 andand 7 are 100% certainare 100% certain
• The third digit 6 is estimated (uncertain)The third digit 6 is estimated (uncertain)
• In the reported length, all three digits (2.76 In the reported length, all three digits (2.76 cm) are significant including the estimated cm) are significant including the estimated oneone
. l8. . . . I . . . . I9. . . .I . . . . I10. . cm
What is the length of the line?What is the length of the line?
1) 9.6 cm 1) 9.6 cm
2) 9.62 cm 2) 9.62 cm
3) 9.63 cm3) 9.63 cm
How does your answer compare with your How does your answer compare with your
neighbor’s answer? Why or why not?neighbor’s answer? Why or why not?
. l3. . . . I . . . . I4 . . . . I . . . . I5. . cm
What is the length of the line?What is the length of the line?First digitFirst digit 5.?? cm5.?? cmSecond digitSecond digit 55.0? cm.0? cmLast (estimated) digit isLast (estimated) digit is 5.05.00 cm0 cm
Always estimate ONE place past the smallest mark!Always estimate ONE place past the smallest mark!
Move the Decimal Point Left or Right Until the Mantissa is Greater Than or Equal to 1.0 and Less Than 10
Express the Number as: M x 10n Where n Represents the Number of Places the Decimal Point was Moved, Positive if the Decimal is Moved Left and Negative if the Decimal is Moved Right
Honors Chemistry, Chapter 2Page 67
Scientific notation is a way of Scientific notation is a way of expressing really big numbers or expressing really big numbers or really small numbers.really small numbers.
For very large and very small For very large and very small numbers, scientific notation is more numbers, scientific notation is more concise.concise.
A number between 1 and 10A number between 1 and 10
A power of 10A power of 10
N x 10N x 10xx
Place the decimal point so that there is Place the decimal point so that there is one non-zero digit to the left of the one non-zero digit to the left of the decimal point.decimal point.
Count the number of decimal places the Count the number of decimal places the decimal point has “moved” from the decimal point has “moved” from the original number. This will be the exponent original number. This will be the exponent on the 10.on the 10.
If the original number was less than 1, If the original number was less than 1, then the exponent is negative. If the then the exponent is negative. If the original number was greater than 1, then original number was greater than 1, then the exponent is positive.the exponent is positive.
Given: 289,800,000Given: 289,800,000 Use: 2.898 (moved 8 places)Use: 2.898 (moved 8 places) Answer:Answer: 2.898 x 102.898 x 1088
Given: 0.000567Given: 0.000567 Use: 5.67 (moved 4 places)Use: 5.67 (moved 4 places) Answer:Answer: 5.67 x 105.67 x 10-4-4
Simply move the decimal point to the Simply move the decimal point to the right for positive exponent 10. right for positive exponent 10.
Move the decimal point to the left for Move the decimal point to the left for negative exponent 10.negative exponent 10.
(Use zeros to fill in places.)(Use zeros to fill in places.)
Given: 5.093 x 10Given: 5.093 x 1066
Answer: Answer: 5,093,0005,093,000 (moved 6 (moved 6 places to the right)places to the right)
Given: 1.976 x 10Given: 1.976 x 10-4-4
Answer: Answer: 0.00019760.0001976 (moved 4 (moved 4 places to the left)places to the left)
Express these numbers in Express these numbers in Scientific Notation:Scientific Notation:
1)1) 4057894057892)2) 0.0038720.0038723)3) 300000000030000000004)4) 225)5) 0.4782600.478260
Y = kX Example Mass vs. Volume Data for
Aluminum Slope of the Line (k) is the Density
Honors Chemistry, Chapter 2Page 75
Block Number Mass (g) Volume (cm3)
1 1.20 0.442 3.69 1.393 5.72 2.104 12.80 4.685 15.30 5.716 18.80 6.907 22.70 8.458 26.50 9.649 34.00 12.80
10 36.40 13.50
Honors Chemistry, Chapter 2Page 76
Mass (g) As a Function of Volume (V)
0
5
10
15
20
25
30
35
40
0 5 10 15
Volume - cubic centimeters
Ma
ss
- g
ram
s
Mass (g)
Honors Chemistry, Chapter 2Page 77
Y = mX + b= slope x Volume + intercept
Slope = 2.69 g/cm3
Intercept = 0.09 grams (!) (Actually Zero)
From Table of Densities: Sample is Aluminum (Al)
Honors Chemistry, Chapter 2Page 78
k = XY or Y = k/X As X Increases, Y Decreases Example: Pressure-Volume Data
Honors Chemistry, Chapter 2Page 79
Pressure (k-Pa) Volume (cm3) P x V
100 500 50000150 333 49950200 250 50000250 200 50000300 166 49800350 143 50050400 125 50000450 110 49500
Honors Chemistry, Chapter 2Page 80
0
100
200
300
400
500
600
0 200 400 600
Pressure (kPa)
Vo
lum
e (
cm
3)
Volume (cm3)
Honors Chemistry, Chapter 2Page 81
Honors Chemistry, Chapter 2Page 82
Chapter 2, Section 3 Review
1. Distinguish between accuracy and precision.
2. Determine the number of significant figures in a measurement.
3. Perform mathematical operations (+,-,x,/) involving significant digits.
4. Convert measurements into scientific notation.
5. Distinguish between inversely proportional and directly proportional relationships.