Download Unit 3: Properties and States of Matter

Feb 10
• Warm up – grab a packet from the black cart
And
• Warm up - Get your lab notebook set it up for a
demo
If you did not take the test or finish the test
yesterday see me
Demo # 2 Kinetic Theory
• Introduction to unit 3
• Title = kinetic theory demo
• Question – is the kinetic theory of matter
true??
Demo – Kinetic theory
• Main idea – all matter is made up of
particles and these particles are always
moving to some extent
• Crushing this can without using my hands
is an example of this
Unit 3: Properties and States
of Matter
Kinetic Theory
• The kinetic theory explains how particles move
in different states of matter.
– All matter is composed of small particles (molecules,
atoms, and ions).
– The particles are in constant, random motion.
– The amount of motion is proportional to the
temperature. Increased temperature means
increased motion.
– Solids, liquids and gases differ in the freedom of
motion of their particles and the extent to which the
particles interact.
Three states of matter
SOLID
LIQUID
GAS
•Definite Shape
•Definite Volume
•Definite Volume
•Can flow
•No definite
Volume
•Cannot be
compressed
•Cannot flow
•No definite
Shape
•Cannot be
compressed
•No definite
Shape
•Can flow
•Can be
compressed
Plasma
• The new fourth state of matter
• When any matter becomes tooo hot the
electrons are stripped / fall off
• This matter shares properties of a gas and a
liquid
• Examples - sun
Plasma TV
• Different type of plasma
• Here we have a gas that the electrons are
just loose- not bound to any nucleus
• lightning
Kinetic Theory
•
Motion in a gas
The constant motion of particles
in a gas allows a gas to
fill any container
•
Three Main points
1. Particles of a gas are in constant, random motion
2. The motion of one particle is unaffected by another
unless they collide
3. The Forces of attraction among particles can be ignored
• POSITIVE AND NEGATIVE CHARGES
Ex) air freshener
Kinetic Theory
• Motion in a liquid
– Particles in a liquid are more closely packed
than particles in a solid
• Attractive forces apply
– A Liquid can take the shape of a container
because the particles of a liquid can flow to
new locations
• The Volume of a liquid is constant because of the attractive
forces between particles keep them together
Kinetic Theory
• Motion in a solid
– Solids have a definite shape and volume
because particles are in a solid vibrate in a
fixed location
ex) People sitting in a theatre or a classroom
Warm-Up – get you lab notebook
• Put this in your lab notebook
• What state of matter has…
– 1. Definite shape, definite volume
– 2. No definite shape, no definite volume
– 3. Definite volume, no definite shape
– Choices – solid, liquid , and gases
Schedule
• Warm up-fast fact
• Phase Changes
• Kinetic theory lab
• Phase change handout – in you packet
from yesterday
Fast Fact - What is the origins of
Valentines day
• 290 AD – Rome declared
the soldiers could not be
married
• Secretly went to Bishop
Valentine to get married
• Became a saint and his
day is Feb 14th
Kinetic theory lab – put this in lab
note book
Title – kinetic theory lab
Problem – we need to understand what is a
phase change
Data- leave space for a data table
Conclusion – “ answer questions from lab ”
Kinetic Theory Lab
• Remember
– Every minute take a reading from the thermometer
– Once the beaker is on the hot plate DO NOT TOUCH
IT
– Mark , highlight when the ice has completely turned
into water, and when water begins to boil
– Continue to take data until the water has completely
boiled for 5 minutes
Example
Data Table in notebook
time (min)
temperature (C)
0
1
1
5
2
11
3
12
4
13
5
14
6
15
7
15
After your done with the water
• Build your graph
• Answer the conclusion questions
Honors
• You must write a formal lab on this
experiment
Thermal Energy
• Thermal energy is heat. It can also be defined as the
sum of the kinetic energy of the particles in a substance.
Has to do with temperature and mass.
– Temperature is a measurement of the average
kinetic energy of a substance.
• Increases kinetic energy (speed of particles)
• Higher Temperature = molecules moving faster
– Solid < Liquid < Gas
Phase Change
• Definition – the reversible physical change
that occurs when a substance changes
from one state of mater into another
• The temperature does not change during a
phase change
• Energy is either stored or released during
a phase change
Phase Change Graph
Common Phase changes
•
•
•
•
1. Melting
2. Freezing
3. Vaporization
4. Evaporation
solid -> liquid
liquid -> solid
liquid -> gas , endothermic
liquid -> gas ,
below boiling point
• 5. Condensation
gas - > liquid, cloudy
bathroom mirror
• 6. Sublimation
• 7. Deposition
solid - > gas, dry ice
Gas -> solid, Frost on a window
Freezing / Melting point
• Freezing point
– Temperature in which a liquid becomes a solid
• Molecules become more closely packed together
• Water – below 0 degrees C
• Melting Point
– temperature in which a solid become a liquid
– Every solid has a different MP
• Water – Above 0 Celsius
• Mercury - -32 C
Boiling Point / Condensation
• Boiling point
– Temperature where a liquid becomes a gas
• Water 90-100 degrees C
Surface area – part of water that is exposed
Larger surface area – faster reaction
• Condensation
– A Gas cools to become a liquid
– Water on a mirror after a shower
Sublimation
•
•
•
•
Were a solid changes into a gas
Dry ice
Endothermic reaction – need energy
Dry ice absorbed the heat energy from its
environment and transformed straight into
a gas
After Lab
• Vocab – now its late
• Phase change handout
• Was in back of packet
• Atomic Model Project is due
Monday
Liquid Nitrogen
•
•
•
•
Beaker: What is the boiling point?
Balloons: Do you see the three phases?
Apples and Bananas: Solids are Brittle
Placed in a bottle: Can Anyone Explain?
Composition of Matter
Matter
• Anything that has mass and takes
up space
• pure substance or mixture
Pure Substance
• A pure substance can not be
broken down physically into
anything else.
–Element
–Compound
Element
• Element – on periodic
table
• Elements are composed
of only one type of atom
• Has one capital letter
– Na
– Cl
–F
• Atom – smallest particle
of an element
Compound or Molecule
• Compound – combo of 2 or more
elements
• Two or more capital letters
– NaCl
– H2O
– MgO2
– CO2
• Molecule – smallest part of a compound
Pure Substances
• Compound
– properties differ from those of
individual elements
– EX: table salt (NaCl)
Pure Substances
• For example…
Two different compounds,
each has a definite composition.
Inorganic vs. Organic Compounds
• Inorganic compounds have no Carbon
– NaCl, H2O, NH4
• Organic compounds have carbon
– C6H12O6
C2H6
Biological Organic Compounds
• Proteins – egg, meat
• Carbohydrates – bread, sugar, pasta
• Lipids – lard, butter, oil
Quick Quiz
On A separate piece of paper answer the
following question using your notes
1.
2.
3.
4.
5.
What is the difference between the melting phase and
the freezing phase?
List the qualification of a liquid?
Write an example of a substance in each phase of
matter?
What is the difference between an Element and a
compound?
What is the difference between a organic and
inorganic compound?
Mixtures
• two or more substances that can
be physically separated
Heterogeneous Mixtures
• Heterogeneous mixture: See
component parts
• Examples
–Granite
–Concrete
–Dry Soup Mix
Homogeneous Mixtures
• Homogeneous mixture: cannot
see component parts
• Examples:
–Kool Aid
–Sweet Tea
Mixtures can be…
•
•
•
•
Gas in Gas (air) – what we breath
Gas in Liquid (soda) the carbonation
Liquid in Liquid (mixed fruit juices)
Liquid in Solid (Iced Tea) – energy needs
to be implied
• Solid in Solid (Concrete, Alloys)
A “microscopic” view
Classifying Matter
Quiz
1. Classify the following as an element, compound, or mixture
(heterogeneous or homogeneous).
HO
E
• _____
air
_____
oxygen
• _____
E
tin can
_____
OC sugar
• _____
Windex
_____
Salad dressing
HO
HE
HE sand and sugar
HO
• _____
_____
gummi bear
-Which box represents an
2. A white solid is dissolved in water. The resulting colorless,
element,
a compound
a
clear liquid is boiled in a beaker
until dryness.
White and
crystals
remain in the beaker. Themixture?
liquid can be classified as a(n)
Homogeneous mixture
______________.
Complete Identification and
Separation Lab
Identify each of the items as an element, an inorganic compound, an organic
Compound, a homogeneous mixture, or a heterogeneous mixture. If it is a
Mixture, tell the type (gas/gas, gas/liquid, etc)
• Example
– Saltwater
Composition
Homo mixture
Type of Mixture
Solid/liquid
Review Lab
Mixtures can be separated by…
•
•
•
•
•
Dissolving
Filtering
Evaporating
Magnetic Separation
Chromatography
Unit 6 Quiz
Warm Up
• Please place your formal lab report on the front
table.
• What type of substance can be separated using
physical means such as evaporating, distilling,
filtering, chromatography, or magnetic
separation?
– Answer choices: elements, compounds, or
mixtures
Review Quiz
• More Practice Identifying Matter
Physical/Chemical Properties Lab
• Label the top of the next full page in your composition
notebook with the title above and today’s date
(2/21/2008).
• Write the definition for Physical and Chemical properties.
– Physical Properties: Any characteristic of a material that you
can observe directly or measure with a tool without changing the
composition of the substance. (It does not change chemically)
– Chemical Properties: Any characteristic of a material that
indicates whether it can undergo change that will alter the
composition of the substance. (It does change chemically)
Make a table like this in your
composition notebook to record
your data
Physical/Chemical Properties Lab
• You and your lab partner must go around
to each station and identify whether the
property being demonstrated is a physical
or chemical property and state why.
These are the properties you
have to choose from
• boiling point, combustion, freezing/melting
point, density, oxidation, solubility,
viscosity, conductivity, corrosion, acid or
base
Warm-Up
• Please make a list of physical and
chemical properties:
Physical Properties (7)
Boiling point
Melting/freezing point
Solubility
Conductivity
Density
Viscosity
Acid or base
Chemical Properties (3)
Oxidation
Corrosion
Combustion
Physical Property
• Any characteristic of a material that
you can observe directly or measure
with a tool without changing the
composition of the substance. (It does
not change chemically)
• Examples: boiling point, freezing/melting
point, density, solubility, viscosity,
electrical conductivity.
Viscosity
• A fluid’s resistance to flow
– High viscosity fluids take longer to pour.
– Viscosity may change with temperature.
• Viscosity Demo
Conductivity
• Ability to transmit electrons (electricity)
– Conductors vs. insulators
• Metals – good conductors
• Non metals – insulators
• Some solutions are good conductors that contain
dissolved ions (electrolytes).
Solubility
• Ability to dissolve or be dissolved
• Solubility increased by:
1. Temperature
2. Surface Area
3. Stirring
Density
• Density – the amount of mass of an object
related to its volume
• Density = mass (Kg) / volume (cm3)
Complete Density Lab
• When finished let me see your data.
• Once I check your data:
• Work on the density problems on the last page
of your packet.
• HW: Density Drill (In your packet) front side only
Review Density Lab
Density Problems
• HW: Lab Report and Density Sheet due
tomorrow
Warm-Up
• What is the density of a piece of wood that
has a mass of 24.0 grams and a volume of
12.0 cm3?
– What would the density be if the piece of
wood were cut in half?
• A piece of wood that measures 3.0 cm
by 6.0 cm by 4.0 cm has a mass of 36.0
grams. What is the density of the
wood? Would the piece of wood float in
water? (volume = L x W x H)
• The volume of a solution went from 40 ml to
what you see above in a graduated cylinder after
putting in a gold ring. If the mass of the gold ring
is measured to be 30 grams, what is the density
of the gold ring?
Review Density Lab
1 cm3 = 1mL = 1 g
Acids and Bases
• Acids
–
–
–
–
–
–
–
–
Form hydrogen (H+) ions in solution
Low pH ( < 7 )
Sour/tart taste
electrolytes
React with metals to form H2 gas
Corrosive – tissue damage/burns
Change color of indicators
React with bases to form salt & water
• Bases
–
–
–
–
–
–
–
–
–
Form hydroxide (OH-) ions in solution
High pH ( > 7 )
Bitter taste
electrolytes
Feel slippery
Often crystalline solids when undissolved
Corrosive – burns
Change color of indicators
React with acids to form salt & water
pH
• pH is a measure of the concentration of H+ ions in solution (0-14)
– Acids < 7
– Neutral = 7
– Bases > 7
• pH meter uses electrodes to read electrical conductivity in solution
• pH paper changes color when exposed to acids/bases
– match pH paper color to a chart to get pH
– Follows ROYGBIV A-B
Litmus
• Litmus paper is another common indicator
– Acids turn it red
– Bases turn it blue
Common Examples
• Acids
–
–
–
–
–
–
Citric
Lactic
Acetic (vinegar)
Carbonic (carbonated drinks)
Hydrochloric (HCl – stomach acid)
Sulfuric, Nitric, Phosphoric (fertilizers)
• Bases
–
–
–
–
Ammonia
Clorox
Magnesium Hydroxide (antacid)
Sodium hydroxide (soap, oven/drain
cleaners)
– Aluminum Hydroxide (antacid, water
purification, color-fast fabrics)
LAB: Acids and Bases
Warm Up
• Get started on Acid-Base WS from your
packet.
– Omit #’s 7, 13, 15 on front and compound B
on the back
Neutralization
• Acids and Bases neutralize each other
– Acid + Base  Salt + Water
• HCl + NaOH  H2O + NaCl
Chemical Property
• Characteristic of a material that
indicates whether it can undergo
change that will alter the composition
of the substance. (It does change
chemically)
• Examples: Oxidation, Corrosion,
Combustion
Oxidation
• Ability to bind with oxygen during a
reaction
– Iron rusting
• Iron + Oxygen
2 Fe + O2
Iron oxide
2 FeO
Combustibility
• Ability to burn
– Cremora Demo
Corrosion
• Ability to break down a metal
– Silver Tarnishing
• Silver + Sulfur
Ag + S
Silver Sulfide
AgS
Decomposition
React/Not react with acids
Warm Up
• Get out practice test and get ready for
review.