topic 1 matter, measurement, and methods

8/14/2019 Topic 1 Matter, Measurement, And Methods

1/26

Topic 1

Matter and Measurement

1


2/26

[1] Discuss chemistry and describe the

interrelationship of chemistry with other fields ofscience.[2] Describe the properties of the solid, liquid,and gaseous states.[3] Classify matter as element, compound or mixture.

[4] Provide specific examples of physical andchemical properties and physical and chemicalchange.[5] Distinguish between intensive and extensiveproperties.[6] Discuss the approach to science, the scientificmethod, and distinguish among the terms hypothesis,theory, and scientific law.

Learning Objectives

2


3/26

[7] Learn the major units of measure in the metric

systems.[8] Know the three common temperature scales, and beable to convert from one system to another.

[9] Use density, mass and volume in problem solvingand calculate the specific gravity of a substancefrom its density.[10] Report data and results using scientificnotation and the proper number of significantfigures.

[11] Use dimensional analysis in conversion ofunits.

Learning Objectives (contd)

3


4/26

------------------------------LEARNING OBJECTIVE 1

[1] Discuss chemistry anddescribe the interrelationshipof chemistry with other fields

of science.-----------------------------

4


5/26

ChemistryChemistry is the study of the composition,structure, properties, and changes of matter.

Composition of matter relates to the kinds ofelements it contains.

Structure of matter relates to the ways the

atoms of these elements are arranged. Property of matter is any characteristic that

gives a sample of matter its unique identity. Changes of matter can be physical or chemical

change.

5


6/26

Why study chemistry?

Chemistry is the central science , central to afundamental understanding of other sciences andtechnologies.

6


7/26


[2] Describe the properties ofthe solid, liquid, and gaseousstates.------------------------------LEARNING OBJECTIVE 3[3] Classify matter aselement, compound or mixture.

-----------------------------

7


8/26

Gas (also known as vapor)

has no fixed volume or shape conforms to the volume and

shape of its container andcompressible

Liquid has a distinct volume has no specific shape assumes the shape of the

portion of the container itoccupies and incompressible

Solid has both definite volume and

shape incompressible

States of Matter

8


9/26

Classification of Matter

9


10/26


[4] Provide specific examplesof physical and chemicalproperties and physical andchemical change.------------------------------LEARNING OBJECTIVE 5[5] Distinguish between

intensive and extensiveproperties.

----------------------------- 10


11/26


12/26

Physical and Chemical Change

Physical Change produces a recognizable

difference in theappearance of a substancewithout causing any change

in its composition oridentity.

Example: boiling of water,crushing a can, melting anice, mixing sand and water,breaking a glass, dissolving

sugar and water, shreddingpaper, chopping wood, mixingred and green marbles,sublimating ice

Chemical Change process of rearranging,

removing, replacing, oradding atoms to producenew substances.

Example:electrolysis of water,rusting of iron, combustionof wood, metabolism of foodin the body, mixing acid andbase, cooking an egg,digesting sugar with amylasein saliva, mixing bakingsoda and vinegar to produceCO2 gas, baking a cake,electroplating a metal,using a chemical battery

12


13/26

Intensive and Extensive Properties

Intensive Properties Independent of the

amount of matterexamined

Example:

Temperature, Color, Odor,Luster, Malleability,Ductility, Conductivity,Hardness, Melting andFreezing Point, BoilingPoint, Density

Extensive Properties Relate to the amount of

substance present

Example:

Mass, Weight, Volume,Length

13


14/26


[6] Discuss the approach toscience, the scientificmethod, and distinguish amongthe terms hypothesis, theory,and scientific law.-----------------------------

14


15/26

Scientific Method

Observation of

a phenomenon

A question

A hypothesis

(a potentialanswer)

Experimentation

Data analysis

Theory

Scientific law

15


16/26


[7] Learn the major units ofmeasure in the metric systems.-----------------------------

16


17/26

SI Base Units

Systeme Internaional dUnites or the SI units

developed in France is widely used today!

Units of Measurement

Physical Quantity Name of Unit Abbreviation

Mass Kilogram kg Length Meter m

Time Second s or sec

Temperature Kelvin K

Amount of substance Mole mol Electric current Ampere A or amp

Luminous intensity Candela cd

17


18/26

------------------------------LEARNING OBJECTIVE 8[8] Know the three common

temperature scales, and beable to convert from onesystem to another.

------------------------------LEARNING OBJECTIVE 9[9] Use density, mass andvolume in problem solving andcalculate the specific gravityof a substance from itsdensity.----------------------------- 18


19/26

Prefixes used in the Metric System

Prefix Abbreviation Meaning

Peta P 1015

Tera T 10 12

Giga G 10 9

Mega M 10 6

Kilo k 10 3

Deci d 10 -1

Centi c 10 -2

Milli m 10 -3

Micro 10 -6

Nano n 10 -9

Pico p 10 -12

Femto f 10 -15

Atto a 10 -18

Zepto z 10-21

19


20/26

Base UnitsLength 1m = 3.28ftMass 1kg = 2.2 lbTemperature K = C + 273.15

F = ( 9/5) ( C)+32C = ( 5/9) ( F-32)

Derived Units

Volume V=(L)3

, V =A.L, L=(V)1/3,

where: V=volume;L=length;1m3 = 35.29ft 3

Density D=M/V, M=D.V, V=M/Dwhere: D=density;M=mass;V=volume

Specific Gravity SG=D subs /D refwhere: D subs =density of substance

Dref =density of reference

20


21/26


[10] Report data and resultsusing scientific notation andthe proper number ofsignificant figures.------------------------------LEARNING OBJECTIVE 11[11] Use dimensional analysis

in conversion of units.

-----------------------------

21


22/26

Exact numbers and Inexact numbers Exact numbers those whose value are known exactly.

1 kilometer = 1000 meter Exact number Inexact numbers those whose values have some

uncertainty.

mass of beaker Inexact number

Precision and Accuracy Precision is a measure of how closely individual

measurements agree with one another. Accuracy refers to how closely individual

measurements agree with the correct, or truevalue.

Uncertainty in Measurement

22


23/26

Significant Figures

Rules to determine the number of significant figures:

[1] All nonzero digits are significant.

1634 four significant figure

[2] Zero between nonzero digits are alwayssignificant.

1005 kg four significant figures, 7.03 cm threesignificant figures

[3] Zeros at the beginning of a number are neversignificant; they merely indicate the position of thedecimal point.

0.02 one significant figure, 0.0026 two

significant figure[4] Zeros at the end of a number are significant ifthe number contains a decimal point.

0.0200 g three significant figures, 3.0 cm twosignificant figures

23


24/26

If the leftmost digit removed is less than 5, the

preceding number is left unchanged.Rounding 9.241 to two significant figures, 9.2. If the leftmost digit removed is 5 or greater, the

preceding number is increase by 1.Rounding 5.235 to three significant figures, 5.24.

Significant Figures for addition and subtraction22.3 + 3.98 + 1.221 =

Significant Figures for multiplication and division2.22 x 1.1 =

Rounding off numbers

24


25/26

The key to using dimensional analysis is the

correct use conversion factors to change oneunit into another.

87.3 ft to m 124.23 m 3 to ft 3

32.19 kg to lb

Convert the following:

Dimensional analysis

25


26/26

topic 1 matter, measurement, and methods

Documents