asc 0301z - 01- chemistry, matter, and measurement - 54 slides.ppt

7/28/2019 ASC 0301z - 01- Chemistry, Matter, and Measurement - 54 slides.ppt

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INORGANIC

CHEMISTRY

ASC0301DR SITI SALWA ABD GANI


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Doa Menuntut Ilmu2

Ya Allah! Bukakanlah dan Tambahkanlah

Rahmat daripada KahazanahMu itu kepada

kami. Ya Tuhan, yang Maha Pengasih lagi

Maha Penyayang.


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COURSE TITLE: INORGANIC CHEMISTRY

COURSE CODE: ASC 0301

CREDIT: 2 + 1

LECTURE: 2 HOURS/WEEKLAB: 3 HOURS/2 WEEKS

TUTORIAL: 2 HOURS/2 WEEKS

ASSESSMENT

TEST 1: WEEK 5 15%

TEST 2: WEEK 10 20%

LAB REPORT: 15%

PRESENTATION (TUTORIAL): 10%

FINAL: 40%

REFERENCE BOOK:John W Moore, Conrad L Stanitski and Peter C Jurs, Chemistry -The Molecular Science, 4th. Ed., Brooks/Cole

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COURSE TITLE: INORGANIC CHEMISTRY

COURSE CODE: ASC 0301

CREDIT: 2 + 1 (120 hrs)

Activities Hours

Lecture 2 hrs x 14 28

Revision 2 hrs x 14 28

Prelab report 1 hr x 7 7Laboratory 3 hrs x 7 21

Group discussion 2 hrs x 7 14

Tutorial presentation 2 hrs x 7 14

Test 1 preparation 2.5

Test 1 1.5

Test 2 preparation 2.5

Test 2 1.5

TOTAL 120


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Chemistry and Matter

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ChemistryClassification of Matter

AtomsMoleculesElements, substances and compoundsMixturesStates and Properties of Matter

Changes of matter


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Learning Outcomes

Classify samples of matter as pure substances,homogeneous mixtures, heterogeneousmixtures, compounds, and elements.

Recognize various form of matters.

Relate names to formulas and charges of simple ions.

Combine simple ions to write formulas and names ofsome ionic compounds.

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Chemistry

What is Science ?SCIENCE is the qualitative and quantitativestudy of nature and the natural laws

What is Chemistry ?CHEMISTRY is a science that examines thecomposition, properties and changes of matter.

What is Matter ?

Anything that have mass and occupy space,and can generally be perceived by our senses(color, texture, odor, hardness, and taste)

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Disciplines of Chemistry

Major traditional chemistry disciplines :

Chemistry Study of

Inorganic Non-carbon-containing substance (ASC0301)Physical Structure and changes of matter (ASC 0302)Organic Substance containing carbon (ASC 0303)Analytical Composition of matterBiochemistry Physical and chemical changes of

living organism

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6/4/20139MINGGU

PENGAJA-

RAN

ASC 0301

TOPIK

1Chemistry and Matter

Unit and Measurement

2The Structure of Atoms

Atomic Mass

3 Mole ConceptConcentrations of Solutions

4 Chemical Reactions

5 Stoichiometry of Reactions

6 Electromagnetic radiationAtomic Model

7

Introduction to Quantum

Theory

Electronic configuration

MINGGU

PENGAJA-

RAN

ASC 0301

TOPIK

8 Periodic Table

9 Periodicity

10

Chemical bonding

Ionic BondCovalent Bond

11Polar Bond

VSPER Theory

12 Valence Bond Theory

13Intermolecular Forces and

Solubility

14

Important Elements in Fertilizer

Important elements in Industry

(PRESENTATION)


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Lower THigher T

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Properties of Matter

Matter exhibits two types of properties :

Physical property is displayed by a sample ofmatter without undergoing any change in itscomposition

It includes mass, color, temperature, volume,density, melting point, etc.

Chemical property is displayed by a sample ofmatter as it undergoes a change in its composition.

This includes flammability, toxicity, reactivity,acidity, corrosiveness, etc.

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Matter

In a physical change, there is no change incomposition; no new substances are formed.

Examples: evaporation, melting, dissolution,crystallization

In a chemical change or chemical reaction,matterundergoes a change in composition; newsubstance are formed.

Examples: corrosion of metals, polymerization of

alkene, fermentation of food.

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Element, Substance and Compound

Substance is matter that has a definite compositionand do not vary from one sample to another.

Substances are either elements or compounds

Element is matter that cannot be broken down intosimpler substances by chemical reaction.

Compound is made up of two or more elements,chemically bonded in definite proportions and can

be broken down into simpler substances.

Terms Substance and Compound are oftenused synonymously

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Mixture

A mixture can contain two or more differentcomponents in varying proportions.

A homogeneous mixture has the samecomposition throughout a sample of matter.Components are indistinguishable. Examples: alloy,air, salt water.

A heterogeneous mixture varies in composition

from one part of the mixture to another.Components are distinguishable. Examples: Mixtureof salt and charcoal.

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Types of Matter6/4/201315

Matter (may be solid, liquid,

or gas): anything that occupiesspace and has mass

Homogeneous matter:uniform composition throughout

Heterogeneous matter:nonuniform composition

Substances: fixedcomposition; cannotbe further purified

Solutions: homogeneousmixtures; uniform composthat may vary widely

Elements: cannot be subdividedby chemical or physical changes

Compounds: elementsunited in fixed ratios

Physically

separable into

Physically

separable into

Chemically

separable into

Combine chemically

to form


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Atoms

The building blocks of matter; the smallest unit ofmatter that participates in a chemical reaction.

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Molecules

A molecule is the smallest particle of an element

that can have a stable independent existence.Usually have two or more atoms bonded together

Examples of molecules:

H2 O2 S8 NaCl H2O CH4 C2H5OH

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Chemical Formulas

Chemical formula shows the chemical compositionof the substance. Ratio of the elements present inthe molecule or compound.

Monatomic elements: He, Au, NaDiatomic elements: O2, H2, Cl2

More complex elements: O3, S4, P8

Compounds: H2O, NaCl, C12H22O11

Substance consists of two or more elements

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Ions

Cations consist of one atom

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.

Group 1 Group 2 Group 3

Li+ , lithium ion Be2+ , beryllium ion Al3+ , aluminium ion

Na+ , sodium ion Mg2+ , magnesium

ionK+ , potassium

ion

Ca2+ , calcium ion

Rb+ , rubidium

ion

Sr2+ , strontium ion

Cs+ , cesium ion Ba2+ , barium ion


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Anions consist of one atom

H-, hydride N3-, nitride O2-, oxide F-, fluoride

C-, carbide P3-, phosphide S2-, sulfide Cl-, chloride

Si4-, silicide As3-, arsenide Se2-, selenide Br-, bromide

Transition Metals and Post-Transition metals

Cr2+, chromium(II) ion

Cr3+

, chromium(III) ion

Sn2+, tin(II) ion

Sn4+

, tin(IV) ion

Mn2+, manganese (II) ion

Mn3+ , manganese (III) ion

Pb2+, lead(II) ion

Pb4+ , lead(IV) ion

Fe2+, iron(II) ion

Fe3+,iron(III) ion

Cu+, copper(I) ion

Cu2+ , copper(II) ion


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Polyatomic ions contain more than one


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Polyatomic ions contain more than one

atom.6/4/201322

NH4+, ammonium CO3

2-, carbonate

H3O+

, hydronium HCO32-

, hydrogen carbonateOH-, hydroxide SO3

2-, sulfite

CN-, cyanide HSO32-, hydrogen sulfite

NO2-, nitrite SO4

2-, sulfate

NO3-, nitrate CrO4

2-, chromate

ClO-, hypochlorite Cr2 O72-, dichromate

ClO2-, chlorite PO4

3-, phosphate

ClO3-

, chlorate HPO42-

, mono hydrogen phosphateClO4

-, perchlorate H2PO42-, dihydrogen phosphate


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Ionic Compounds

Potassium chloride: KCl = K+

+ Cl-

Calcium sulphate: CaSO4= Ca2++ SO4

2-Sodium carbonate: Na2CO3 = 2Na

+ + CO32-

Barium nitrate: Ba(NO3)2 = Ba2+ + 2NO3

-

Ammonium phosphate: (NH4)3PO4 = 3NH4+ +

PO43-

Chromium(III) chloride: Cr(Cl)3 = Cr3+ + 3Cl-

Iron(II) sulphite: FeSO3= Fe2+ + SO3

2-

an ionic compound is a chemical compound inwhich ions are held together in a lattice structure by ionic

bonds. Usually, the positively charged portion consists of

metal cations and the negatively charged portion is

an anion or polyatomic ion.
http://en.wikipedia.org/wiki/Chemical_compoundhttp://en.wikipedia.org/wiki/Ionhttp://en.wikipedia.org/wiki/Ionic_bondhttp://en.wikipedia.org/wiki/Ionic_bondhttp://en.wikipedia.org/wiki/Cationhttp://en.wikipedia.org/wiki/Anionhttp://en.wikipedia.org/wiki/Anionhttp://en.wikipedia.org/wiki/Cationhttp://en.wikipedia.org/wiki/Ionic_bondhttp://en.wikipedia.org/wiki/Ionic_bondhttp://en.wikipedia.org/wiki/Ionhttp://en.wikipedia.org/wiki/Chemical_compound


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ASC 0301

Imperial System

Metric System

System International (SI)Accuracy and Precision

Significant Figures

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Learning Outcomes

Apply appropriate units to describe the result of

measurement. Explain the difference between precision and

accuracy.

Apply the concept of significant figures.

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Modern Chemistry

As of 1850s onwards, chemists used weighing

balance more systematically to measure mass (aquantity of matter) in their research

Since then, better equipments and devices were

progressively invented and used; then chemistryinvolves doing all sorts of measurements (simpleand complex; visual and aided)

So, what is it that chemists measure?All sort of properties of matter - distance, vol., temp.,time, energy, area, density, velocity, frequency,luminescence, light absorbance ... etc

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Scientific measurement and unit6/4/201328

All measurements contains 2 essential pieces ofinformation:

(i) a number (the quantitative piece)

(ii) a unit (the qualitative piece)

Example:

The number 50 is somewhat meaningless without

Units.Consider this:

Daily wage = RM50/day

wt of an egg = 50g/egg

size of a square paper = 50cm x 50 cm

S l U it d St d d


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Scale, Unit and Standard

Results of a measurement are always expressed in some kindof ascale that is defined in terms of a particular kind of unit

Example : Scale of lengthBritish Imperial system French Colonial system

Inch = base unit Millimetre = base unit12 inch = 1 foot*** 10 mm = 1 cm

3 feet = 1 yard 100 cm = 1 metre***

1760 yards = 1 mile 1000 m = 1 km

For comparison and communication purposes, the scale mustbe defined by astandard ( a reference value forcomparison)

The scales of length are related & interconvertible by aconversion factor

2.54 cm = 1 inch1 cm = 0.3937 inch

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Imperial System of Unit

Still being used in Britain and USA

Weightounce, pound, ton

16 oz = 1 lb; 14 lb = 1 stone; 2240 lb = 1 ton

Lengthinch, foot, yard, mile12 inches = 1 foot; 3 feet = 1 yd; 5280 feet = 1760 yds = 1 mile

Volumecup, pint, quart, gallon

2 cups = 1 pint; 2 pints = 1 quart; 4 quart = 1 gal

Not employed in scientific work since 1960s

Confusing and have to memorize many conversion tables

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M t i S t f M t


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Metric System of Measurement

Basic/fundamental units/types of measurements are :

Type Name SymbolMass gram gLength metre mVolume litre L

Time second sEnergy joule J

Simple and easy system of measurement

Units of measurement can be multiplied or dividedby

a factor 10

Can use prefixes to change size of unit

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Metric System Prefixes

Base units in the Metric System can be convertedinto units that are more appropriate for the quantitybeing measured by adding a prefix to the name ofthe base unit. Common metric prefixes are:

Prefix Symbol Meaningfemto- f x 1/1,000,000,000,000,000 (10-15)

pico- p x 1/1,000,000,000,000 (10-12)nano- n x 1/1,000,000,000 (10-9)micro- x 1/1,000,000 (10-6)milli- m x 1/1,000 (10-3)centi- c x 1/100 (10-2)

deci- d x l/10 (10-1

)kilo- k x 1,000 (103)mega- M x 1,000,000 (106)giga- G x 1,000,000,000 (109)tera- T x 1,000,000,000,000 (1012)

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Systeme Internationale(SI Units of Measure)

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Before 1960, Science uses the Metric System of UnitsAfter 1960, the International System of Units

(SI = Le Systeme Internationale) was proposed.

A modern version of the Metric System of Units.

It is used globally in science, industry and commerce

as a standard/reference measurement units.

The seven base/standard units of the SI system are:

length meter m

mass kilogram kg

time second sElectric current ampere A

Temperature kelvin K

Amount of substance mole mol

Luminous intensity candela cd

U it t id SI t


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Units outside SI systemhonorary units

SI has 7 base/fundamental units 3 more are included as honorary members

Base unit Symbol Dimension1. Litre L 1 L = 1 dm3 = 103 ml

2. Metric tonne t 1 t = 103

kg3. Unified atomicmass unit amu (u) 1 u = 1.66054 X 10-27 kg

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Derived SI units


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Derived SI units[dimension]

Other units of measurement can be derived by combining one

or more of the 10 SI base units. Some of the common non-SI orderived units used in chemistry are :

Physical Quantity Name of derived unit Symboldensity kg/m3

electric charge coulomb C (A.s)

electric potential volt V (J/C)energy joule J (kg-m2/s2)force newton N (kg-m/s2)frequency hertz Hz (s-1)pressure pascal Pa (N/m2)

velocity meters/second m/svolume cubic meter m3

** Symbol of a derived unit is termed the DIMENSION/UNIT of thephysical quantity

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Exact numbers

Exact numbers = numbers that are known/exact by

definition They are called exact values because they are

measured in complete units and are not dividedinto smaller parts.

Examples of exact values: 17 people; 28 cars

Conversion factors have an infinite (never ending)number of significant figures.

Examples:

60 seconds in one minute

1000 meters in one kilometer7 days in one week

1 inch = 25.4 mm

1 yard = 36 inches

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Measured numbers

Measured numbers= an actual estimated

reading:

(a) as shown by meters/detectors of instruments

(b) by visual account from calibrated/graduated

equipment (burette, pipette)(c) from mathematical calculations (average,

standard deviation)

Measurements by these methods have inherentuncertainty or experimental errors

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MeasurementChemistry is an experimental science; it involves

measurements of properties of matter

Measuring properties of matter involves 3 parameters:(a) magnitude/quantity(b) base unit or dimension

(c) uncertainty/error

Example: weighing a sample of salt(a) average magnitude = 5.7076(b) base unit = gram(c) uncertainty (using 4 different balances)

5.6785 g; 5.702 g; 5.65 g; 5.8 g

So, what is the true/real weight of the salt sample?

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ypes o exper men a errors


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ypes o exper men a errors(Lab no 1ASC 0301)

SystematicInstruments not calibrated properlyReagents are not correctly and properly preparedImperfections/limitations of instrument and glasswareCan be improved by proper calibration, adherenceto strict preparation procedures, use more sensitiveand reliable instruments, run control/blanks ... etc

RandomTests done at different times, different room T ... etcPersonal mistakes and carelessnessCan be improved by tight control of environmentalfactors, replication of tests, applying appropriatestatistical analyses on data obtained ...etc

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U t i t i t


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Uncertainty in measurement

Measurement of a property of matter involves 2

parameters(A) PRECISION(B) ACCURACY

(A) PRECISION = degree of reproducibility i.e.

(a) how close are the measurements to each other(b) how well they agree with each other

(B) ACCURACY = how close measurements are to thetrue/accepted value

AIM = experimental measurements must be as preciseand accurate as possible; i.e. least possible errors

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Accuracy vs Precision

Accuracy refers to the proximityof a measurement to the true(accepted) value of a quantity.

Precision refers to the proximity ofseveral measurements to eachother.

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In the real world, we never know whether themeasurement we make is accurate. Why not?

We make repeated measurements; calculate the mean,x and the standard deviation, s,

We hope (but not always correctly) that good precisionimplies good accuracy.

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Accuracy vs Precision

Uncertainty in measurements


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Different measuring devices have differentuses and different degrees of accuracy.

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Uncertainty in measurements 6/4/201344The smallest division of this graduatedcylinder is 1 mL. Therefore, our reading

error will be 0.1 mL or 1/10 of the smallestdivision. An appropriate reading of thevolume is 36.5 0.1 mL. An equallyprecise value would be 36.6 mL or 36.4mL.

The smallest division in this buret is 0.1mL. Therefore, our reading error is 0.01

mL. A good volume reading is 20.380.01 mL. An equally precise answerwould be 20.39 mL or 20.37 mL.

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Significant figures

Topics Determining the number of significant figures

Scientific notation

Addition & Substraction

Multiplication & Division

Rounding off

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Significant figures

When we measure quantities, esp. for the very first time,it is difficult to know if measurement is accurate.

To know if a measurement is accurate, you need toknow its true value. If you knew its true value, then,

you dont need to do the measurement!

But, it is easy to know if your measurements are precise.One indicator of the preciseness of a measurement is

the number of significant figures in a measurednumber.

Significant figures relate to certainty of themeasurement. As the number of significant figures

increases, the more certain is the measurement.

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Number of significant figures

Significant figures = number of digits that expressesthe result to the true measured precision

Example: Consider a number

92.154 (5 sig. Figures)

Start from the left and count the digits. There is5 significant figuresin this number

DO NOT worry about the decimal point !!

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Zeroes in significant figures

Zeroes are special digits

Sometimes they count as a sig. digit, sometimes theydont. It depends on their position.

Example: 0.092060 has 5 significant figures

First two zeroes are not significant, they are justposition holders

So, when counting significant digits, always start fromthe left and don't start counting until you meet the firstnon-zero digit. Then everything after that counts,including the zeroes !!

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Rules for counting significant figures are summarizedbelow.

Leading zeros are not significant.0.421 has three significant figures.

Zeros within a number are always significant.Both 4012 and 40.05 contain four significant figures.

Trailing zeros in the whole number are not significant.Thus, 470,000 has two significant figures.

Trailing zeros that aren't needed to hold the decimalpoint are significant.For example, 114.20 has five significant figures.

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Scientific notation

A good way to avoid problems of significant and non-

significant zeroes is to use scientific notation

Example

920000 = 9.2 x 105 Has 2 sig. figs.

0.092067 = 9.2067 X 10-2 Has 5 sig. figs.

0.092 = 9.2 X 10-2 Has 2 sig. figs.

0.0920 = 9.20 X 10-2 Has 3 sig. figs.

When using scientific notation, all digits includingzeroes are significant

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Rounding off

Chemistry is an inexact science

All physical measurements have some error

Thus, there is some inexactness in the last digit of anynumber

Use what ever round-off procedures you so choose

Reasonably close answers are acceptable

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Ro nding significant fig res 6/4/201352


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Rounding significant figures

A salt sample is weighed 3 times:12.4330 g 12.4334 g 12.4335 g 6 sig. figures

Calculate the average:(12.4337 + 12.4334 + 12.4335) / 3 = 12.43353333(calculator display)

Makes no sense to write down all the numbers; averagevalue cannot have sig. figures more than that of themeasurements.

Need to round off the number to the correct number ofsig. figures.

In this caseInsignificant digits 3333 are dropped2.43353333 is rounded off to 6 sig. figures; i.e.12.4335

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Rounding off numbers 6/4/201353


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Rounding off numbers

When insignificant digits are dropped from anumber, the last digit should be rounded for bestaccuracy

Example :

To determine how the last digit should be rounded,

convert the digits to be dropped to a decimal fraction( .333333); then follow the rules for rounding numbers

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Rules for rounding numbers to the 6/4/201354


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Rules for rounding numbers to thecorrect number of significant figures

1. If the decimal fraction is greater than ,

add one to the last digit retained

2. If the decimal fraction is less than ,

do not change the last retained digit

3. If the decimal fraction is exactly ,

add one to the last digit retained if it is odd

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Examples

Round off 9.473, 9.437, 9.450 & 9.750 to 2 sig. figures.

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For 9.473 the last digit retained is 4; decimal fraction is.73. So Rule #1 applies; 9.473 is rounded to 9.5

For 9.437 the last digit retained is 4; the decimalfraction is .37. So Rule #2 applies; 9.437 rounded to 9.4

For 9.450 the last digit retained is 4; the decimalfraction is .50. So Rule #3 applies; 450 is rounded

to 9.4

For 9.750 the last digit retained is 7; the decimalfraction is .50. So Rule #3 applies; 9.750 is rounded

to 9.8

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THANK YOU

asc 0301z - 01- chemistry, matter, and measurement - 54 slides.ppt

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