CHEM 1111: CHAPTER 1
34 Cards in this Set
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Science
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The study of something.
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Scientific Method
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Observation
Experiment
Hypothesis
Theory
Law
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Experiment
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observation of natural phenomena carried out in a CONTROLLED MANNER so that results can be duplicated and rational conclusions obtained.
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Theory
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tested explanation of basic natural phenomena. Can not be "proven" can only be DISPROVED.
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Law
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concise statement or mathematical equation about a fundamental relationship or regularity of nature that stands the test of TIME.
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Pure Substances
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Compounds
Two or more different elements
Still have constant composition
Cannot be physically separated back into original parts
Elements
Same kind of atom
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Mixtures
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2 or more substances that are mixed
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HeterogeneousMixture
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Is not uniformed much like raisins in cookie dough, or oil & water
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Homogenous mixture
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object that has the same composure thoughout.
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States of Matter
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Solid
Liquid
Gas
Plasma
Bose-Einstein Condensate
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Physical Change
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A usually reversible change in the physical properties of a substance, as size or shape: Freezing a liquid is a physical change.
retains chemical identity.
crumpling paper
cracking an egg
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chemical change
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one in which a given substance becomes a new substance with different properties and different compositions
burning paper
cooking an egg
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Properties of Matter
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Chemical
Physical
Identification
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chemical property
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when substances react to make a new substance
reactivity
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Physical Property
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you can observe with without changing its properties.
melting point
boiling point
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Intensive
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Independent of amount (color, bp, mp)
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Extensive
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depends upon the amount of a substance (Volume, Mass)
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Measurement
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physical quantity based on a defined unit.
includes NUMBER and UNIT
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Precision
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How close measured values are to each other.
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Accuracy
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How close measured value is to actual value of quantity
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Significant figures
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minimum number of digits required to express a value in scientific notation without loss of accuracy.
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What are the SI base units?
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Length - meter (m)
Mass - kilogram (kg)
Time - second (s)
Temperature - kelvin (K)
Amount of substance - mole (mol)
Electric Current - empere (A)
Luminous intensity - candela (cd)
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What are metric base units?
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meter (m)
gram (g)
second (s)
Celsius (*C)
mole (mol)
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Area (length squared)
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(SI)m^2
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Volume (Length cubed)
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(SI)m^3
(Metric) Liter - L
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Density (Mass per unit volume)
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(SI) kg/m^3
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Speed (distance traveled over time)
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(SI) m/s
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Acceleration (speed changed over time)
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(SI) m/s^2
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Force (Mass times acceleration)
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(SI) kgm/s^2 = 1 Newton
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Pressure (Force per unit area)
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kg/ms^2 = 1 Pascal, Pa
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Temperature
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Fehrenheit
Celcius
Kelvin
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Fehrenheit-Celsius Conversion Formula
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F=(C)9/5 + 32
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Celsius-Fehrenheit Conversion
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C=(F-32) * 5/9
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Celcuis to kelvin
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k=(C)+273.15
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CHEM 1111: CHAPTER 1