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Why study chemistry?
1. It’s required.
2. It sounds interesting.
3. It’s unavoidable.
4. It truly is the central science.
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Introduction: Matter and Measurement
Chapter 1 BLB 11th
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Expectations
Classify matter Properties of matter g ↔ mL (using density) Solve for any variable in a formula. Metric unit conversions Other conversions: temperature, metric-
English, etc. Identify and work with significant figures.
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1.1 The Study of Chemistry
Chemistry is everywhere! Matter is everywhere! Thus, chemistry matters!
Chemistry involves the study of matter – its properties and behavior.
Macroscopic observations are rooted in microscopic structure.
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The Periodic Table of the Elements
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Checking in…
Name an element:
Name a compound:
Name a mixture:
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A. There are three atoms making up a water molecule.
B. The water molecule contains atoms of two different types of elements.
C. A water molecule has more than one bond.
D. A water molecule has a larger mass than the sum of masses of its constituent atoms.
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Molecules
O2, H2O, CO2, C2H5OH, C2H6O2, C9H8O4
Models shown on p. 4
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1.2 Classification of Matter
Matter – anything which has mass and takes up space.
States of matter (p. 7):1. Solid – rigid, regular
2. Liquid – fluid, irregular
3. Gas – open, random
Phases of matter
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States of Matter
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States of Matter
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Physical or chemical separation?
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The Periodic Table of the Elements
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Elements
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Group Activity
Assemble into groups of four or five.
Introduce yourself.
Work together.
Discuss, argue, and intellectually engage.
Record and report your group’s result.
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Group Activity
Describe the contents of the containers.
Devise a plan to determine which liquid is in each of the two containers.
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Description
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Strategy for identification
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1.3 Properties of Matter
physical – measured or observed without changing the identity of a substance, e.g. physical state, color, odor, density, boiling point
chemical – describes a substance’s reactivity, e.g. flammability, corrosiveness
extensive – depends on the amount of matter present, e.g. mass, volume
intensive – does not depend on the amount of matter present, e.g. density, color, temperature
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Physical & Chemical Changes
Physical – change in appearance, not in composition, e.g. phase changes, separation of mixtures: filtration, distillation, chromatography
Chemical – new substance is formed as the chemical identities change, e.g. any chemical
Dissolve vs. react Explode vs. ignite
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Physical or chemical?
Helium leaks out of a balloon? Growth of plants by photosynthesis? Salt added to a bowl of soup? Blood turning red upon exposure to air?
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Mixture, compound, pure substance?
Fruit punch? Sugar? Milk? Gold? Tap water?
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1.4 Units of Measurement (SI Units)
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Volume – a derived unit
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Angstrom Å 10-10 m
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Temperature Scales
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Temperature Conversions
°F → °C
°C → °F
°C → K
)32(9
5 FC
32)(5
9 CF
15.273 CK
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Density
Density – mass per unit volume
D = m/V (g/cm3 or g/mL) Measured at a specific temperature Useful as a conversion factor (g ↔ mL) Most substances become more dense at lower
temperatures. Specific gravity – density of a substance
divided by the density of a reference substance (usually water); no units
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Difference in density values is the reason some things float and others sink.
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0.91
0.92
0.93
0.94
0.95
0.96
0.97
0.98
0.99
1
0 10
20
30
40
50
60
70
80
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Temp. (oF)
Den
sit
y (
g/m
L)
Ice, 0.917
Water, 0.99987
Density of Water
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Calculate the volume (in mL) of 87.6 g of platinum. (DPt = 21.5 g/cm3)
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1.5 Uncertainty in Measurement
Exact numbers have a defined value, e.g. 12-dozen, 2.54 cm/in; 1000 g = 1 kg; count of objects
All measurements have some degree of uncertainty; inexact
Types of error: systematic & random The last digit of a measured quantity is uncertain. The more significant figures, the greater the certainty. precision – agreement among data accuracy – agreement of data with true value
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Different measuring devices have different uses and different degrees of accuracy and precision.
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Significant Figures
nonzero numbers always significant
zeroes
before never
between always
behind sometimesw/decimal – yesw/o decimal - no
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Significant Figures in Calculations
A calculated result can be no more certain than the data measured.
Mathematical operations (pp. 23-24)Averaging least number of decimal places+ and - least number of decimal placesx and ÷ least number of sig. figs.
Round off at the end at the end of a multi-step problem.
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Sig. Fig. examples
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1.6 Dimensional Analysis
Problem-solving strategies: Estimate and then calculate your answer.
Do the two agree? Get your units correct and your answer
should be correct. Report to correct number of sig. figs. Practice, practice, practice!