Chapter 2
Matter and Energy
Presentation Slides to Accompany Cracolice/Peters Introductory Chemistry: An Active Learning Approach, Third Edition Copyright © 2007 Brooks/Cole, a part of the Thomson Corporation.
Section 2.1
Representations of
Matter: Models and
Symbols
Presentation Slides to Accompany Cracolice/Peters Introductory Chemistry: An Active Learning Approach, Third Edition Copyright © 2007 Brooks/Cole, a part of the Thomson Corporation.
Goal 1
Identify and explain the difference among
observations of matter at the macroscopic,
microscopic, and particulate levels.
Presentation Slides to Accompany Cracolice/Peters Introductory Chemistry: An Active Learning Approach, Third Edition Copyright © 2007 Brooks/Cole, a part of the Thomson Corporation.
Goal 2
Define the term model as it is used in
chemistry to represent pieces of matter too
small to be seen.
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Matter:
Anything that has mass (sometimes expressed
as weight) and takes up space
Matter can be observed and/or
thought about at different levels:
Macroscopic
Microscopic
Particulate
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Macroscopic samples of matter:
Mountains
Rocky cliffs
Huge boulders
Rocks and stones
Gravel
Sand
Macro- means large
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Microscopic samples of matter:
Tiny animals or plants
Cells
Crystals on rock surfaces
Micro- means small
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Particulate samples of matter:
Too small to see, even with the most
powerful optical microscope
Chemists imagine the nature of the behavior of the tiny
particles that make up matter, and they use that
knowledge to carry out changes from one type of macroor microscopic matter to another
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Macroscopic, microscopic, and particulate matter
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Model:
A representation of something else
Geologists model the earth (globe)
Biologists model cells
Chemists model atoms and molecules
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Ball-and-stick model:
Symbolizes atoms as balls and the electrons
that connect those atoms as sticks
Space-filling model:
Shows the outer boundaries of the particle
in three-dimensional space
Presentation Slides to Accompany Cracolice/Peters Introductory Chemistry: An Active Learning Approach, Third Edition Copyright © 2007 Brooks/Cole, a part of the Thomson Corporation.
Models and
symbols used
to represent
particulate
matter
Ball-and-stick
models
Space-filling
models
Chemical formula
and
Lewis diagram
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Models are represented with symbols
Chemical symbols are letters
that represent atoms of elements
H represents an atom of hydrogen
O represents an atom of oxygen
H2O represents a molecule of water:
Two hydrogen atoms and one oxygen atom
Presentation Slides to Accompany Cracolice/Peters Introductory Chemistry: An Active Learning Approach, Third Edition Copyright © 2007 Brooks/Cole, a part of the Thomson Corporation.
Macroscopic,
particulate, and
symbolic forms
and
representations
of matter
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Section 2.2
States of Matter
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Goal 3
Identify and explain the differences among
gases, liquids, and solids in terms of (a)
visible properties, (b) distance between
particles, and (c) particle movement.
Presentation Slides to Accompany Cracolice/Peters Introductory Chemistry: An Active Learning Approach, Third Edition Copyright © 2007 Brooks/Cole, a part of the Thomson Corporation.
States of matter:
Gas
The air you breathe
Liquid
The water you drink
Solid
The food you eat
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Kinetic Molecular Theory:
All matter consists of extremely tiny
particles that are in constant motion
Kinetic refers to motion
Molecular comes from molecule,
the smallest individual particle
that is present in one kind of matter
Theory is a collection of general propositions
that, when taken together, explain a class
of related natural phenomena
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The speed at which particles move is
faster at higher temperatures and
slower at lower temperatures
There is an attraction among particles
in all samples of matter
The state of matter of any sample
depends on temperature and
the attractions among the particles
that make up the sample
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Gas
Particles are independent of one another,
moving in random fashion
Liquid
Particles move freely among themselves,
but clump together
Solid
Particles vibrate in fixed positions
relative to one another
Presentation Slides to Accompany Cracolice/Peters Introductory Chemistry: An Active Learning Approach, Third Edition Copyright © 2007 Brooks/Cole, a part of the Thomson Corporation.
Presentation Slides to Accompany Cracolice/Peters Introductory Chemistry: An Active Learning Approach, Third Edition Copyright © 2007 Brooks/Cole, a part of the Thomson Corporation.
Section 2.3
Physical and Chemical
Properties and Changes
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Goal 4
Distinguish between physical and chemical
properties at both the particulate level and the
macroscopic level.
Presentation Slides to Accompany Cracolice/Peters Introductory Chemistry: An Active Learning Approach, Third Edition Copyright © 2007 Brooks/Cole, a part of the Thomson Corporation.
Goal 5
Distinguish between physical and chemical
changes at both the particulate level and the
macroscopic level.
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Physical Properties:
Description by senses—color, shape, odor, etc.
Measurable properties—density, boiling point, etc.
Charcoal is black
Glass is hard
The boiling point of water is 100°C
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Physical Changes:
New form of old substance
No new substances formed
Ice melts
Dry ice changes to gaseous carbon dioxide
A rock is ground into sand
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In a physical change, the particles of matter
themselves are unchanged
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Chemical Changes:
Old substances destroyed
New substances formed
Water decomposes to hydrogen and oxygen gases
Iron rusts
Food is digested
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When electricity is passed through certain water
solutions, the water decomposes into its elements,
hydrogen and oxygen. This is a chemical change.
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Chemical Properties:
Properties defined by types of
chemical changes possible
Water can be decomposed to its elements
Iron will rust under certain conditions
Starch molecules react to form
sugar molecules during digestion
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Section 2.4
Pure Substances
and Mixtures
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Goal 6
Distinguish between a pure substance and a
mixture at both the macroscopic level and the
particulate level.
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Goal 7
Distinguish between homogeneous and
heterogeneous matter.
Presentation Slides to Accompany Cracolice/Peters Introductory Chemistry: An Active Learning Approach, Third Edition Copyright © 2007 Brooks/Cole, a part of the Thomson Corporation.
Pure Substance:
A single chemical; one kind of matter
Unique set of physical and chemical properties
Cannot be separated into parts
by a physical change
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Mixture:
A sample of matter that consists of
two or more chemicals
Physical and chemical properties vary as the
relative amounts of different parts change
Can be separated into parts
by physical changes
Presentation Slides to Accompany Cracolice/Peters Introductory Chemistry: An Active Learning Approach, Third Edition Copyright © 2007 Brooks/Cole, a part of the Thomson Corporation.
Water is a pure liquid and has a constant boiling
point (a physical property);
The boiling point of a mixture
(solution) changes as the composition
of the mixture changes
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A pure substance cannot be distinguished from
a mixture of uniform appearance by observation alone
at the macroscopic level
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Solution:
A homogeneous mixture
Coffee, air, brass
Homogeneous:
A sample that has a uniform appearance
and composition throughout
Tea, paint, gasoline
Heterogeneous:
Different phases, usually visible
Carbonated beverages, salad dressings
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Homogeneous pure substances and mixtures
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Section 2.5
Separation of Mixtures
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Goal 8
Describe how distillation and filtration rely on
physical changes and properties to separate
components of mixtures.
Presentation Slides to Accompany Cracolice/Peters Introductory Chemistry: An Active Learning Approach, Third Edition Copyright © 2007 Brooks/Cole, a part of the Thomson Corporation.
Most natural substances are mixtures;
chemists separate mixtures into pure substances
Nitrogen and oxygen are purified
from the mixture called air
Pure water is purified
from the mixture called natural water
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Iron and sulfur form a heterogeneous mixture.
Magnetism is a physical property:
Iron is attracted to a magnet,
sulfur is not.
This physical property is the basis
of the separation of this mixture
Presentation Slides to Accompany Cracolice/Peters Introductory Chemistry: An Active Learning Approach, Third Edition Copyright © 2007 Brooks/Cole, a part of the Thomson Corporation.
Distillation:
Separation of the parts of a mixture by heating
a liquid until one component boils to
the gaseous state. The pure gas is
cooled and collected in the liquid state.
Boiling is a physical change;
a homogeneous mixture is
changed so that at least one component
is separated as a pure substance
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Laboratory distillation apparatus
Presentation Slides to Accompany Cracolice/Peters Introductory Chemistry: An Active Learning Approach, Third Edition Copyright © 2007 Brooks/Cole, a part of the Thomson Corporation.
Filtration:
Separation of the parts of a mixture by
using a porous medium, such as filter paper,
to separate components based on size
Filtration is based on the physical properties of a
mixture: the particle sizes of a component must be
significantly larger or smaller than the pore size of the
filtration medium
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Gravity filtration
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Section 2.6
Elements and
Compounds
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Goal 9
Distinguish between elements and compounds.
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Goal 10
Distinguish between elemental symbols and
the formulas of chemical compounds.
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Goal 11
Distinguish between atoms and molecules.
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Element:
Pure substance that cannot be separated
into other stable pure substances
Atom:
Smallest unit particle of an element
Compound:
Pure substance that can be decomposed
by a chemical change into two or more
other pure substances
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The element silver and
a particulate-level model of silver atoms
Presentation Slides to Accompany Cracolice/Peters Introductory Chemistry: An Active Learning Approach, Third Edition Copyright © 2007 Brooks/Cole, a part of the Thomson Corporation.
Elements
At least 88 occur in nature
Examples: copper, sulfur, gold, silver
11 occur in nature as gases
2 occur as liquids (mercury and bromine)
the others occur as solids
Name of an element is always a single word;
compound names usually two words
or a multisyllabic compound word
Presentation Slides to Accompany Cracolice/Peters Introductory Chemistry: An Active Learning Approach, Third Edition Copyright © 2007 Brooks/Cole, a part of the Thomson Corporation.
Presentation Slides to Accompany Cracolice/Peters Introductory Chemistry: An Active Learning Approach, Third Edition Copyright © 2007 Brooks/Cole, a part of the Thomson Corporation.
Familiar objects that are nearly pure elements
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Familiar objects that are compounds
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Elemental symbols:
Letters that symbolize elements
The first letter of the name of the element,
written in uppercase, is often its symbol
If more than one element begins with the same letter, a
second letter written in lowercase is added
hydrogen, H
oxygen, O
carbon, C
chlorine, Cl
sodium, Na
(from natrium)
iron, Fe
(from ferrum)
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Chemical formula:
Symbolic representation of the particles
of a pure substance
A combination of the symbols of all the
elements in the substance
The formula of most elements is the same
as the symbol of the element:
helium, He; sodium, Na
Other elements exist in nature as molecules;
their formulas indicate the number of atoms
of the element in the molecule:
hydrogen, H2; oxygen, O2
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Formula unit:
A real or hypothetical particle represented
by a chemical formula
Ammonia molecules are real particles
with the formula NH3:
3 atoms of hydrogen and 1 atom of nitrogen
Barium chloride exists as an orderly, repeating pattern
of barium and chlorine, but there is no barium chloride
molecule--its hypothetical particle has the formula
BaCl2:
2 chlorine atoms and 1 atom of barium
Presentation Slides to Accompany Cracolice/Peters Introductory Chemistry: An Active Learning Approach, Third Edition Copyright © 2007 Brooks/Cole, a part of the Thomson Corporation.
Law of Definite Composition
(also Law of Constant Composition):
Any compound is always made up of elements
in the same proportion by mass (weight)
No matter its source,
water is 11.1 parts hydrogen
per 88.9 parts oxygen
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The properties of a compound are different
from the properties of the elements that
make up the compound
You are familiar with water
Hydrogen and oxygen
are very different from water
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Particulate and macroscopic views
of elements and compounds
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Particulate and macroscopic views
of elements and compounds
Presentation Slides to Accompany Cracolice/Peters Introductory Chemistry: An Active Learning Approach, Third Edition Copyright © 2007 Brooks/Cole, a part of the Thomson Corporation.
Particulate and macroscopic views
of elements and compounds
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Summary of the Classification System for Matter
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Section 2.7
The Electrical Character
of Matter
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Goal 12
Match electrostatic forces of attraction and
repulsion with combinations of positive and
negative charges.
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Two of the fundamental forces that govern the operation
of the universe are:
Force of gravity
Electromagnetic force
The electromagnetic force plays an important
role in understanding chemistry
It includes electricity and magnetism
Presentation Slides to Accompany Cracolice/Peters Introductory Chemistry: An Active Learning Approach, Third Edition Copyright © 2007 Brooks/Cole, a part of the Thomson Corporation.
Force field:
Region in space where the force is effective
Electrostatic force:
The force of an electrical charge
that does not move
A charged object exerts
an invisible electrostatic force
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Two objects having the same charge,
both positive or both negative,
repel each other
Two objects having unlike charges,
one positive and one negative,
attract each other
Presentation Slides to Accompany Cracolice/Peters Introductory Chemistry: An Active Learning Approach, Third Edition Copyright © 2007 Brooks/Cole, a part of the Thomson Corporation.
Presentation Slides to Accompany Cracolice/Peters Introductory Chemistry: An Active Learning Approach, Third Edition Copyright © 2007 Brooks/Cole, a part of the Thomson Corporation.
Presentation Slides to Accompany Cracolice/Peters Introductory Chemistry: An Active Learning Approach, Third Edition Copyright © 2007 Brooks/Cole, a part of the Thomson Corporation.
Matter has electrical properties
There forces are responsible for the energy absorbed or
released in chemical changes
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Section 2.8
Characteristics of a
Chemical Change
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Goal 13
Distinguish between reactants and products
in a chemical equation.
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Chemical Equation:
Symbolic representation of the
essence of a chemical change
Reactants: Beginning substances
Products: Substances formed
C + O2
Reactants
2 H2O
CO2
Products
2 H2 + O2
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Goal 14
Distinguish between exothermic and
endothermic changes.
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Goal 15
Distinguish between potential energy and
kinetic energy.
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Exothermic Reaction:
A chemical change that releases
energy to its surroundings
Burning charcoal:
C + O2
CO2 + energy
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Endothermic Reaction:
A chemical change that absorbs
energy from its surroundings
Decomposition of water:
H2O + energy
2 H 2 + O2
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Potential Energy:
Energy due to position in a field where forces
of attraction and/or repulsion are present
Gravitational potential energy:
Position in the earth’s gravitational field
Electrical potential energy:
Position in an electrical field
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Minimization of energy is one of the driving
forces that cause chemical reactions to occur
Chemical energy comes largely from
the rearrangement of charged particles
in an electrostatic field
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Kinetic Energy:
Energy of motion
The temperature of an object
is related to the average
kinetic energy of its particles
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Section 2.9
Conservation Laws and
Chemical Change
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The Conservation Law:
In any change,
the sum of mass plus energy is conserved;
they are neither created nor destroyed
∆E = ∆m  c2
Matter is an extremely
concentrated form of energy
Presentation Slides to Accompany Cracolice/Peters Introductory Chemistry: An Active Learning Approach, Third Edition Copyright © 2007 Brooks/Cole, a part of the Thomson Corporation.
A uranium fuel pellet of this size produces energy equal
to the energy that would be produced by burning about
one ton of coal
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Goal 16
State the meaning of, or draw conclusions
based on, the Law of Conservation of Mass.
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Law of Conservation of Mass:
In a non-nuclear change,
mass is conserved;
it is neither created nor destroyed
In any ordinary chemical change,
Total mass of reactants = Total mass of products
Presentation Slides to Accompany Cracolice/Peters Introductory Chemistry: An Active Learning Approach, Third Edition Copyright © 2007 Brooks/Cole, a part of the Thomson Corporation.
Goal 17
State the meaning of, or draw conclusions
based on, the Law of Conservation of Energy.
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Law of Conservation of Energy:
In a non-nuclear change,
energy is conserved;
it is neither created nor destroyed
The energy lost in one form is always exactly
equal to the energy gained in another form
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Common events in which energy is
changed from one form to another
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