03-59-140-01 General Chemistry I

Prentice-Hall © 2002General Chemistry: Chapter 1Slide 1 of 19

03-59-140-01General Chemistry I

Lectures: M W F 12:30 - 1:20 p.m.

Professor: Dr. David Tramontozzi

Section 1: Room OD104

Office Hours: Monday and Friday9:00-11:30 for now.

Location: Essex Hall Rm. 186-1 (Chemistry Resource Room) for now.

Contact: [email protected]

Text: General Chemistry Edition 8 Author: Petrucci, Harwood, Herring   

Publisher: Pearson

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Students need to purchase the following items from around the university before they come to the labs (starting September 26th):

1.- Laboratory manual (Document Services)$10.00-$15.00

2.- Breakage card (Cashiers Office)$25.00

3.- Safety glasses (Bookstore)$ 5.00

Lab CoatsRequired, $30.00

Essex Hall Lab D 12:00-3:00pm MWFSee Jenny or Sharonna

Laboratory Requirements

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Chapter 1: Matter—Its Properties and Measurement

General ChemistryPrinciples and Modern Applications

Petrucci • Harwood • Herring

8th Edition

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Contents

Physical properties and states of matter Système International Units Uncertainty and significant figures Dimensional analysis

http://cwx.prenhall.com/petrucci/chapter1/deluxe.html

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Properties of Matter

Matter: Occupies space, has mass and inertia

Composition: Parts or componentsex. H2O, 11.19% H and 88.81% O by mass

Properties: Distinguishing features physical and chemical properties

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States of Matter

Examples of physical

changes. The chemical

composition remains constant.

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1_15

Matter(materials)

Substances Mixtures

Elements CompoundsHomogeneous

mixtures(solutions)

Heterogeneousmixtures

Physical processes

Chemical

reactions

Classification of Matter

PhysicalSeparation ?

YESNO

UniformThroughout ?

ChemicalSeparation ?NO NOYES YES

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Separations

Filtration Distillation

Paper Chromatography

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Separating Mixtures

1_17

Substances tobe separateddissolved in liquid

Pureliquid

A B C

mixture

ChromatographyChromatography

As the mixture moves through the

stationary phase, the components are

separated based on their retention time.

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Significant Figures

Number

6.29 g0.00348 g9.0 1.0 10-8

100 eggs100 g = 3.14159

Count from left from first non-zero digit.

Adding and subtracting.

Use the number of decimal places in the number with thefewest decimal places.

1.14 0.611.67613.416

SignificantFigures

3322Infinite (exact)bad notationvarious

13.4

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Significant figures

Multiplying and dividing.

Use the fewest significant figures.

0.01208 0.236

Rounding Off

3rd digit is increased if4th digit 5

Report to 3 significant figures.

10.235 12.4590 19.75 15.651

.

10.212.519.815.7

= 0.512

= 5.12 10-3

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Units

S.I. Units

Length metre, m

Mass Kilogram, kg

Time second, s

Temperature Kelvin, K

Quantity Mole, 6.022×1023 mol-1

Derived Quantities (based on SI units)

Force Newton, kg m s-2

Pressure Pascal, kg m-1 s-2

Energy Joule, kg m2 s-2

Other Common Units

Length Angstrom, Å, 10-8 cm

Volume Litre, L, 10-3 m3

Energy Calorie, cal, 4.184 J

Pressure 1 Atm = 1.064 x 102 kPa

1 Atm = 760 mm Hg

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SI Prefixes

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Temperature

T(K) = t(°C) + 273.15

t(°C) = 5/9 [t(°F) – 32]

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Relative Temperatures

Boiling Pointof Water

Melting Pointof Ice

Boiling Point of Liquid Nitrogen

Hot Day

Very Cold Day

Absolute Zero

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Volume

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Density

= m/V

m = VV = m/

g/mL

Mass and volume are extensive properties

Density is an intensive property

Dependent on the quantity of matter present

Independent on the quantity of matter present

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Conversion

What is the mass of a cube of osmium that is 1.25 inches on each side?

Have volume, need density = 22.48g/cm3

Does the answer make sense ??

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Wrong units

The Gimli Glider, Q86, p30

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Uncertainties

• Systematic errors.– Thermometer constantly 2°C too low.

• Random errors– Limitation in reading a scale.

• Precision– Reproducibility of a measurement.

• Accuracy– How close to the real value.

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End of Chapter Questions

1, 3, 5, 12, 14, 17,18, 20, 30, 35, 41, 49, 50, 61, 72, 74, 79.