Unit 3 Matter and Its Transformations
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Transcript of Unit 3 Matter and Its Transformations
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Read the Introduction to Chapter 1, and Sections 1.7 and 1.8 of the textbook before viewing this slide show.
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Unit 3Matter and Its Transformations
•What is chemistry? (Introduction to Chapter 1)
•Physical and chemical properties (1.7)
•Physical and chemical changes (1.7)
•Classification of matter (1.8)
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What is Chemistry? (Intro to Chapter 1)
• Matter – anything that occupies space and has a mass (1.7)
• Chemistry – the study of matter and its transformations (Introduction to Chapter 1)
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Physical Properties (1.7)
• Physical property – a physical characteristic or behavior of the material – Examples: boiling point, hardness, color– To get a feel for physical properties, you might want to
go to this link http://www.chemeddl.org/resources/ptl/• Click on any of the elements in the periodic table
and then click on the Physical button in the left menu
• You will see what are primarily physical properties listed for that element (I am not sure cost is one, but it is at least interesting.)
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Chemical Properties (1.7)
• Chemical property – describes how the material reacts with (or doesn’t react with) with other types of matter– Examples: iron rusts in moist air, hydrogen and oxygen react
violently to form water, neon does not react with much of anything
– To get a feel for chemical properties, you might want to go to this link http://www.chemeddl.org/resources/ptl/
• Click on any of the elements in the periodic table and then click on the Media button in the left menu
• You will see under the Video heading short film clips of reactions the material undergoes with various other materials. Its interaction (or noninteraction) with other materials is a chemical property.
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Physical and Chemical Changes (1.7)
• Physical change – a change in the appearance of a substance without changing its chemical identity or composition– Examples: melting ice, cutting a piece of wood in half
• Chemical change – a change in the chemical identity of matter into other substances that are different– Examples: hydrogen and oxygen react to form water, a
piece of iron rusts – The video clips mentioned on the previous slide are
examples of materials undergoing a chemical change.
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Classification of Matter (1.8)
• With over 18 million characterized compounds, classification is important to provide a framework for study
• This initial classification system provides a good starting point
• As you might imagine, there are subclassifications under many of these basic groupings
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States of Matter (1.8)• Three common states of matter (plus a bonus):
– Gas – takes shape of container, flows easily, compressible
– Liquid – takes shape of container but with a flat top, flows easily, not very compressible
– Solid – retains shape, does not flow appreciably, not very compressible
– (A bonus state: plasma – a stream of charged particles – this is the stuff of plasma TV)
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Particle Level Description of States of Matter
Gas:•Particles “far” apart•Particles moving rapidly
Liquid:•Particles “close” together•Particles moving slowly•Particles more ordered than gas, but not as much as solid
Solid:•Particles “close” together•Particles vibrating but not changing location•Particles very ordered
Images are screen shots from States of Matter simulationPhET Interactive SimulationsUniversity of Coloradohttp://phet.colorado.edu
Notice that as the temperature decreases the particles get closer together and move more slowly
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Pure Substances and Compounds (1.8)
• Pure substance – has a definite fixed composition that does not vary from one sample to another– Examples: pure copper, pure water
• Mixture – variable composition that can be different from one sample to another– Examples: salt water, air, sand and water mixed
together
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Further Classification ofPure Substances
• Pure substances can further be categorized as:– Elements – substances which cannot be
broken down into simpler substances by chemical means
– Compounds – chemical combination of two or more elements
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Periodic table from common.wikimedia.org
Periodic Table – the elements
A sample periodic table - if it’s a known element it is on here. Compounds are chemical combinations of multiple elements. A large portion of our course will be involved with studying the periodic chart.
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Further Classification of Mixtures
• Mixtures can further be categorized as:– Homogeneous – all parts of the mixture have
the same composition and appearance• Examples: sugar dissolved in water, air, a “pinch”
of salt dissolved in water– Heterogeneous – appearance is not the same
throughout• Examples: sand in water, oil in water
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An Early Atomic View (1.7)
• Some of these terms become a little clearer if we consider them on a microscopic scale. We will look at atoms in considerable detail soon but for now let’s take a simplistic view.
• An atom is the basic building block of matter. The elements of the periodic chart are composed of atoms.
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An Early Atomic View (cont.) (1.7)
• Atoms of different elements are different. • Molecules are formed when atoms
chemically unite, or bond.• If a molecule consists of all of one kind of
atom, it is an element.• If a molecule has two or more different
elements in it, it is a compound.
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An Early Atomic View (cont.) (1.7)
• Consider a hydrogen molecule which can be represented by H-H. An oxygen molecule can be represented by O-O.
• Hydrogen is flammable, oxygen supports combustion.
• If a balloon is filled with hydrogen and oxygen gas it could be filled to any ratio we wanted – example 2:1, 5:3, 1:8, etc.
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An Early Atomic View (cont.) (1.7)
• If we hold a match to the balloon, it will explode.• In the process, water which may be represented
by H-O-H is formed.• The elements H-H and O-O reacted to form the
compound H-O-H.• Notice that H-H is flammable, O-O is
combustible, but H-O-H is used to put out fires. Compounds have different properties than the elements from which they are made.
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Summary of Classification of Matter
Matter
Pure Substances
Elements Compounds
Mixtures
Homogeneous Mixtures
Heterogeneous Mixtures
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The EndThe End End