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Unit 3: Matter and Energy
Part I: Classifying Matter
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Matter is anything that has mass andvolume.
Volume is the amount of threedimensional space an object occupies.
Mass is a measure of the amount ofmatter.
Matter
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Which of the following are examples of matter?
a. Sand
b. Paperc. Heat
d. Air
e. Sound
f. Light
g. Chalk
h. Smoke
f. Water Vapor
Pause for a Cause
Learning Activity 1
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Building matter
An element is a pure substance that cannot be
broken down into simpler, stable substances
and is made of one type of atom.
An atom is the
smallest unit of an
element thatmaintains the
chemical identity of
that element.
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Elements
How many known elements are there in the
universe?
117
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The Periodic Table
Period
Group or
family
PeriodProperties varyTotal of 7 periods
GroupHave similar properties
Total of 18 groups
Metals
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Groups
The vertical columns on the periodic table are calledgroups or families.
Groups are numbered 1-18 on the periodic table
Elements belonging to the same group have similar properties
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Periods
The horizontal row of elements on the periodic table are
called periods or series.
Periods are numbered 1-7.
The closer two elements are to one another in a period, the more
similar their properties.
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Pause for a Cause
Learning Activity #1Identify the element located in:
a) Group 2 Period 4b) Group 17 Period 6
c) Group 13 Period 2
d) Group 10 Period 4
e) Group 1 Period 1
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Metals, nonmetals, and metalloids can be located on the
periodic table by knowing where to find the metalloid line!
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Properties of Metals
Conductive- metals aregood conductors of heat andelectricity
Malleable- metals can be
hammered into thin sheets
Ductile- can be drawn intothin wire
Tenacious- metals havehigh tensile strength andresist being pulled apart
Lustery- metals are
recognized by their shine
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Examples of Metals
Potassium, Kreacts with
water and must
be stored in
kerosene Copper, Cu, is a relatively soft metal, and
a very good electrical conductor.
Mercury, Hg, is the only metal that
exists as a liquid at room
temperature
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Propertiesof NonmetalsCarbon, the graphite in pencil lead is a great example of a
nonmetallic element.
Nonmetals are poor conductors of heat and electricity
Nonmetals tend to be brittle
Many nonmetals are gases at room temperature
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Examples of NonmetalsSulfur, S, was once
known as
brimstoneMicrospheres of
phosphorus, P, a
reactive nonmetal
Graphite is not the only pure form
of carbon, C. Diamond is also
carbon; the color comes fromimpurities caught within the
crystal structure
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Metalloids straddle the
border between metals
and nonmetals on the
periodic table.
They have properties of both metals and nonmetals.
Metalloids are more brittle than metals, less brittle
than most nonmetallic solids Metalloids are semiconductors of electricity
Some metalloids possess metallic luster
Properties of Metalloids
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Silicon, Si A Metalloid
Silicon has metallic luster
Silicon is brittle like a nonmetal
Silicon is a semiconductor of electricity
Other metalloids include: Boron, B
Germanium, Ge Arsenic, As
Antimony, Sb
Tellurium, Te
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Noble Gases
Unreactive
Gases at room
temperature
Neon, argon, krypton
and xenon are used in
lighting
Helium is used in
balloons
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Pause for a Cause
Learning Activity #2Tell whether each of the following elements is a
metal, nonmetal, metalloid or noble gas:
a) Silicon
b) Chlorinec) Sodium
d) Iron
e) Antimony
f) Radon
g) Cesium
h) Sulfur
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Have a silvery appearanceand are soft enough to cut
with a knife.Not found in nature as
free elements.
React violently with waterReact with halogens toform salts
The Properties of a Group:the Alkali Metals
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Harder, denser, andstronger than alkali metals.
Higher melting points thanalkali metals.
Not found in nature as
free elements.
The Properties of a Group:
the Alkaline-Earth Metals
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Good conductors of electricity andhave a higher luster.
Less reactive than the alkali metalsand the alkaline-earth metalsSome exist as free elements
The Properties of a Group:
the Transition Elements
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Most reactive nonmetals.React with most metals to
form salts.
The Properties of a Group:
the Halogens
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Noble GasesGroup 18 Elements
Unreactive
Gases at room
temperature
Neon, argon, krypton
and xenon are used in
lighting
Helium is used in
balloons
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Learning Activity #3The following questions refer to the following
elements
A. Sodium
B. Fluorine
C. Boron
D. Argon
1. Does not interact readily with other elements
2. Reacts explosively with water
3. Is classified as a halogen
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Pure substances
Element
Made of the same types of
atom
Can be just one atom
Chemically bonded
Compound
Made of different types of
atoms
Must be more than one
Chemically bonded
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Building blocks of matter
Elements and compounds can combine to
create mixtures.
Mixtures are combinations of two or more
substances in which each substance maintains
its own chemical identity.
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Types of mixtures
Homogeneous (solutions) Heterogeneous
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Pause for a Cause
Learning Activity #4
Identify each of the following as eitherhomogeneous or heterogeneous:
a) Paper
b) Sweetened Teac) Pencil Lead
d) Fresh-squeezed Lemonade
e) Goldf) Chocolate Chip Cookies
g) Oil and Vinegar Salad Dressing
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Classifying matter
Learning Activity #5
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Learning Activity #5
Classify each of the following as an element,
compound, heterogeneous or
homogeneous mixture.
Chex Mix
Gold ring
Sea water (salt and water)
C6H12O6
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Colloid
Colloids are solutions.They can be described asa substance trappedinside another substance.They can be identified bytheir characteristicscattering of light.
For example: air trappedinside the fat molecules inwhipped cream.
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Suspension
Mixture that contains
solid particles
These particles will fall
out of solution overtime (sedimentation)
Muddy water
Dust particles in the air
Paint
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So you say
Mixtures are combinations in which each part
maintains its own chemical identity.
We can use these identities to separate the
components.
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How would you separate the following?
Have them move! They
will all go at different
speeds.
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What about these?
Iron
Gold
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What about these?
Sand
Water
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Filtration
Used for theseparation ofsolids from fluids(liquids or gases)
by interjecting amedium which thefluid can pass, butthe solids (or at
least part of thesolids) in the fluidare retained.
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And these?
Purple dye
Pink dye
Yellow dye
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Chromatography
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And these?
Salt
Water
Distillation
A
B
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Lab intro
Mixture contains
Salt
Sand
Iron fillings Poppy seeds
All in water
Available equipment
Cotton balls
Filter funnels
Filter paper
Forceps Magnet
Paperclips
Paper towels
Petri dish
Pipettes
Rubber stoppers
Test tubes
Tissue paper
Experiment 1; Modern Chemistry pg 26
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Matter and Energy
Part II: Properties and Changes
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Same, samebut different?
P f M
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Properties of Matter
Extensive properties
Intensive properties
Volume
Mass
Energy Content (think Calories!)
depend on theamount of matter that is present.
do not dependon the amount of matter present.
Melting point
Boiling point
Density
Ability to conduct electricity
Ability to transfer energy as heat
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Tell whether each of the following represents an
extensive or intensive property:a. volume
b. density
c. boiling point
d. ability to conduct heat
e. mass
Pause for a Cause
Learning Activity 7
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Properties of matter can
also either bechemical or physical.
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Physical properties
Characteristics that can be observed
or measured without changing the
identity of the substance.
Melting pointBoiling point
Ch i l P ti
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Relates to a
substances ability to
undergo changes thattransform it into
different substances.
Chemical reactivity
Combusts or Rusts
Chemical Properties
C i f Ph i l d Ch i l
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Comparison of Physical and Chemical
Properties
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Pause for a Cause
Learning Activity #8
Classify each of the following properties as
either chemical or physical properties:
a. color i. tarnishing
b. reactivity j. decay c. flammability k. texture
d. odor l. density
e. ductility
f. solubility
g. length
h. melting point/boiling point
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Physical ChangeA change in a substance that does not involve a
change in the identity of the substance.Example:
Phase Changes(Change of State):
A change of a
substance from one
state of matter toanother.
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Ph
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PhaseDifferences
Soliddefinite volume and shape; particlespacked in fixed positions.
Liquid definite volume but indefiniteshape; particles close together but not infixed positions.
Gasneither definite volume nor definite
shape; particles are at great distancesfrom one another.Plasma high temperature, atoms lose mostof their electrons (fluorescent).
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Heat can be used to change the state of matter.
Low Temperature= Low energy
High Temperature= High energy
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Pause for a Cause #9
a. How does a solid differ from a liquid?
b.How does a liquid differ from a gas?
c. How is a liquid similar to a gas?
d.What is a plasma?
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Chemical Change or Chemical Reaction
A change in which one or more substancesare converted into different substances.
Reactants the substance that react, usually
on the left side of the reactionProducts the substance that are formed,usually on the right side of the reaction
C2H5OH + 3O2 2 CO2 + 3 H2O + EnergyReactants Products
The arrow always points to the products!!
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Evidence of a Chemical Change
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Classify each of the following as a
chemical or physical change:1. Iron metal is melted.
2. Wood burns in air.
3. Milk turns sour.
4. A rock is broken.
5. Iron combines with oxygen to form rust.
6. Moth balls vaporize in a closet.
7. Grapes ferment.8. Salt dissolves in water.
9. Flashlight batteries corrode.
Pause for a Cause
Law of Conservation of Mass
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Law of Conservation of Mass
Energy and Changes in Matter
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Energy and Changes in Matter
Energy is always involved when physical or
chemical changes occur.
Energy can be in various forms.
heat
light
sound
Energy can be absorbed or released in a change,
it is not destroyed or created.
law of conservation of energy
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PART 3: ENERGY AND SPECIFIC HEAT
Matter and Energy
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Energy changes
Endothermicenergy flows into the system, so
the temperature of the surroundings
_______________
Exothermicenergy out of the system, so the
temperature of the surroundings
________________
Are the following processes
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Are the following processes
endothermic or exothermic?
1. Freezing ice
2. Sweat evaporating
3. Fuel burning
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Endothermic vs. Exothermic
In an endothermic reaction, heat is a
_____________ (reactant or product).
In an exothermic reaction, heat is a
_______________ (reactant or product).
The following reaction is _______________
(exothermic or endothermic):
O2 + 2H2 2H2O + heat
http://www learn360 com/ShowVi
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http://www.learn360.com/ShowVi
deo.aspx?SearchText=specific+heat
&ID=139937 Specific heat video
Specific Heat Capacity
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p p y
Also known simply as specific heat (c).
The measure of the heat energy required to
increase the temperature of a substance An intensive property.
Unique for each compound.
The specific heat for water is 4.184 J/gC
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Calculation with Specific Heat
q = mcT
q is the heat absorbed or released(When heat is absorbed the process is said to be endothermic, when heat is
released the process is said to be exothermic.)
m is mass
c is specific heat capacity
T is the change in temperature( means change in, to calculate take the final value initial value)
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A 4.0 g sample of glass was heated from 274 K to 314 K and
was found to have absorbed 32 J of energy as heat.
A. What is the specific heat of this type of glass?
B. How much energy will the same glass sample gain when it
is heated from 314 K to 344 K?
Specific Heat Problems
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Specific Heat Problems
Determine the specific heat of a material if a
35 g sample absorbed 96 J as it was heated
from 293 to 313 K.
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Specific Heat Problems
If 980 kJ of energy are added to 6.2 L of water
at 291 K, what will the final temperature of
the water be?
Specific Heat Problems (No
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Specific Heat Problems (No
calculator)
How many calories of energy are transferred
when 20 mL of water cool to a temperature of
30 C from a temperature of 90 C. Assume the
density of water is 1 g/mL and the specificheat capacity of water is 1 cal/g*C.
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11.8
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If you have a mixture of water and ice at 0 C and you add a
piece of metal that is 50 C, which of the following will
occur?
A. The temperature of the water will decrease.
B. The temperature of the water will increase
C More ice will form