Chemistry 212 - Course OutlineChemistry 212 - Course Outline

M atter

Therm ochem istry

Chem ical Bonding

Kinetics(optional)

Solutions Interm olecular Forces

Gases Atom ic Structure

Stoichiom etry Nom enclature

Basic Principles

Grade Distrn

The REQUIRED textbook for this course is: Author/Title:Brown/LeMay/Bursten/Murphy/

Woodward/Stoltzfus, “Chemistry, The Central Science”. 13e, 2014.

Course/Section:Principles of Chemistry I, 212 Sec’s 1,2,3

Professor:Dr. C.B. William Ng

Why you NEED this text:  You will be TESTED from this textbook  

 Reading assignments, Practice problems 

 Online Assignments via MasteringChemistry (5% course total)

Ng-Website

Study of ChemistryStudy of Chemistry

Composition Structure

Properties Interactions

Life Sciences

Physical Sciences

MacroscopicMacroscopicMicroscopicMicroscopic

cold hot HC

Nitrogen

Degree Celsius

( C )

Degree Fahrenheit( F )

Degree Kelvin

( K )

Melting point -210 -346 63

Boiling point -200 -328 73

Lab To Do’s ListLab To Do’s List

SI Units

T em perature Density

Problem SolvingDim ensional Analysis

Significant Figures Unit Conversions

Quantitative M easurem ents

Scientific M ethod

Introduction: Basic Principles of Chemistry [Ch. 1]Introduction: Basic Principles of Chemistry [Ch. 1]

The Scientific MethodThe Scientific Method

ObservationsObservations

LawLaw

Theory Tested by Further Experiments

Theory Tested by Further Experiments

TheoryTheory

Theory ModifiedTheory

Modified

Major Fields in ChemistryMajor Fields in Chemistry

Winona State

University

BiochemistryPhysical

Chemistry

NgZemke

Nydegger, M

OrganicChemistry

InorganicChemistry

PolymerChemistry

ChemicalEducation

&Information

AnalyticalEnvironmental

NalliHeinChan

Sichula

FranzEngen

Whaley

MannLee

Mauser

WestZemkeGilman

Nydegger, I

Kopitzke Zemke

Dept. Manager: Peggy KillianLab. Specialist: Barb Keller

Basic SI UnitsBasic SI Units

Commonly Used Metric PrefixesCommonly Used Metric Prefixes

Scientific NotationScientific Notation

unit(s) 10 x # #

± integer± real

10 x 10 x 10 103 001.010

110

33

baba 101010ba

b

a10

10

10 baba 1010

22-112 1

cm ; :unit(s) toapplies Alsocm

cmcmcm

32

218

102

]1000.3[)100.4(

mx

mxxmx

Uncertainty in Measurement• All scientific measures are subject to error.• These errors are reflected in the number of figures reported for

the measurement.• These errors are also reflected in the observation that two

successive measures of the same quantity are different.

Precision and Accuracy• Measurements that are close to the “correct” value are accurate.• Measurements that are close to each other are precise.

Uncertainty in MeasurementUncertainty in Measurement

Precision and Accuracy

Uncertainty in MeasurementUncertainty in Measurement

Rules of Significant FiguresRules of Significant Figures

• Counting zeros

• Rounding

• Product/Quotient can have no more sig. Figs. Than numbers with the least sig. Figs.

• Sum/Difference can have no more decimals than numbers with least decimals.

• Keep at least one extra digit for intermediate calculations

• Exact Numbers

112

2223

10254.1

10951076.1

cmx

cmxcmx

112

2223

10254.1

10951076.1

cmx

cmxcmx

Dimensional Analysis• Method of calculation utilizing a knowledge of units

• Conversion factors => simple ratios relating two units

• Desired unit = given unit (conversion factor)

Dimensional AnalysisDimensional Analysis

unitgiven unit desired

factor Conversion

Box #’s and Class/Random-ID#’sBox #’s and Class/Random-ID#’s

Test Etiquette

Example-1Example-1 Convert 6,352x104 km to ? m (con. sci. notn.)

6.352x1010 m

Example-2Example-2 Change 952 cg to ? ng (csn)

9.52x109 ng

Example-3Example-3 Convert 723 cm-2 to ? m-2 (csn)

7.23x106 m-2

Example-4Example-4

Example #5: Speed Conversions

Example-5Example-5

Example #5: Speed Conversions

Density• Used to characterize substances.• Defined as mass divided by volume:

• Units: g/cm3 or g/mL . • Originally based on mass (the density was defined as the

mass of 1.00 g of pure water).

Units of MeasurementUnits of Measurement

volumemass

Density

Test Etiquette

Density ExampleDensity Example

• The sun is estimated to have a mass of 2x1036 kg . Assuming it to be a sphere of average radius 6.96x105 km , calculate the average density of the sun in units of g cm-3 .

Mathcad Solution

Density CalculationsDensity Calculations

Mathcad Solution

Density of Sun example

m 2 1036 kg

m 2 1036 kg

103

gm1 kg

m 2 1039 gm

r 6.96105 km r 6.9610

5 km10

3m

1 km

1 cm

102

m

r 6.960 1010 cm

V4

3 r

3 V4

3 6.9610

10 cm 3 V 1.412 10

33 cm3

3.141592653589793d

m

Vd

m

V

d2 10

39 gm

1.4121033 cm

3

d 1 106 gm cm

3

Temperature ConversionsTemperature Conversions

15.273TT CKBetween Celsius and Kelvin

]32[*9

5F

F

C o

Fo

o

C TT

FC

F oo

o

CF TT 32)]5

9(*[

Bet. Cel. and Fehr.

SI Units

T em perature Density

Problem SolvingDim ensional Analysis

Significant Figures Unit Conversions

Quantitative M easurem ents

Scientific M ethod

15.273CK oTT

V

md

Test Etiquette

Introduction: Basic Principles of Chemistry [Ch. 1]Introduction: Basic Principles of Chemistry [Ch. 1]