honors chemistry, chapter 2 page 1. evolution of a gas (bubbles, odor) formation of a precipitate...

Honors Chemistry, Chapter 2

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


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


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



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)


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.


Measurements Are Quantitative Information

Quantity: Something That Has Size or Amount


SI Units Are Defined in Terms of Standards of Measurement

Seven Basic Units All Others Derived From Seven Basic

Units


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


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)


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)



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


Relationship Between D, m, and V:


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:


1 kg 1000 g1 = --------------- or -------------- 1000 g 1 kg

Write Equation Including Proper Factor

Cancel Units Multiply Numbers to Get Final Result


4.5 kg 1000 g--------- x -------------- = 4500 g 1 1 kg


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).


Accuracy – The Closeness of Measurements to the Correct or Accepted Value

Precision – The Closeness of a Set of Measurements



XXXX

XXXX

High Precision

High Accuracy

High Precision

Low Accuracy


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


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



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



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.



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.


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.)


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

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


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


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


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)


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)


k = XY or Y = k/X As X Increases, Y Decreases Example: Pressure-Volume Data


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


0

100

200

300

400

500

600

0 200 400 600

Pressure (kPa)

Vo

lum

e (

cm

3)

Volume (cm3)



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.

honors chemistry, chapter 2 page 1. evolution of a gas (bubbles, odor) formation of a precipitate...

Documents

molhonors chemistry

amounthonors chemistry

mass g

basic unitshonors chemistry

eric severeidhonors

mass lbneed

mass lbosmium

ml1000 g