Unit 2 - WELCOME STUDENTS
Transcript of Unit 2 - WELCOME STUDENTS
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UNIT 2:
C L A S S I F I C AT I O N O F M AT T E R
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MATTER
Reflect:
What is matter?
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MATTER
Matter: Anything that
has mass and occupies
space.
You can describe matter in
terms of quantity by mass
NOT weight.
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MATTERIn chemistry we will look at 3 different categories or phases of matter. Each
phase can be described and classified by using a PARTICLE MODEL.
Solid Liquid Gas
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PROPERTIES OF MATTER
Particle Diagram
of a solid
= solid particle
Solid
Definite shape &
volume
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PROPERTIES OF MATTER
Liquid
Definite volume, but
takes the shape of
its container
Particle Diagram
of a liquid
= liquid particle
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PROPERTIES OF MATTER
Gas
Takes shape of
container. No
definite shape or
volume
Particle Diagram
of a gas
= gas particle
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KINETIC MOLECULAR THEORY OF MATTER
• Atoms & molecules are constantly in motion
(kinetic energy) in any phase.
• We measure the average kinetic energy of these
movements of the molecules/atoms as
temperature!
• Avg. KE = Temp.
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3 PHASES OF MATTER & KMT
Kinetic Molecular Theory
Solids
- Particles do move
(vibrate)
- Held tightly together
- Particles are ordered
- Least amount of energy
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3 PHASES OF MATTER & KMT
Kinetic Molecular Theory
Liquids
- Some particle movement
- Still highly attracted to
each other
- Particles are disordered
- Moderate amount of energy
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3 PHASES OF MATTER & KMT
Kinetic Molecular Theory
Gases:
- Lots of particle
movement
- Large distances
between the particles
- Particles are disordered
- Most amount of K.E.
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HOW DO YOU CHANGE BETWEEN THE PHASES?
Big Idea:
You can change between the 3 phases of matter
by either putting energy IN or taking energy
OUT.
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Increase in Temp. Causes atoms/molecules to gain more energy
(KE) and move faster
Sublimation
Fusion/Melting
Freezing
solidification
crystallization
Condensation
Vaporizing/evap
Deposition
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Melting/Fusion
Freezing
Evap
Condensation
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http://www.kentchemistry.com/links/Matter/HeatingCurve.htm
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Big Idea: Temperature MEASURES the average kinetic energy of
particles in a sample of matter.
1. Convert 50 K to the Celsius scale.
2. Normal body temperature is 310 K. Convert this to the Celsius scale.
3. Antifreeze, or ethylene glycol, boils at 199 °C. Convert to the Kelvin scale.
Converting between Kelvin and Celsius:
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Key Points on the temperature scales!
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REAL GASES VS. IDEAL GASES
L I F E V S . I D E A
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KINETIC MOLECULAR THEORY OF GASES: HOW CHANGES IN TEMPERATURE AFFECT VOLUME AND PRESSURE OF A GAS.
Demo Observable
Characteristic
of the Gas
Explain in terms of
particles.
Measuring
a Balloon
REA
L G
ASE
S
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GASES & KMT
Demo Observable
Characteristic
of the Gas
Explain in terms of
particles.
Measuring
a Balloon
Gases have mass. Each particle has a mass
(total mass of the
sample is equal to the
sum of the masses of
the particles.
REA
L G
ASE
S
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GASES & KMT
Demo Observable
Characteristic of
the Gas
Explain in terms of
particles.
Vapor
Ramp
REA
L G
ASE
S
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GASES & KMT
Demo Observable
Characteristic of
the Gas
Explain in terms of
particles.
Vapor
Ramp
Gases have specific
densities.
The compactness of the
particles differs from gas
to gas.
REA
L G
ASE
S
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GASES & KMT
Demo Observable
Characteristic
of the Gas
Explain in terms of
particles.
Compression(syringe)
REA
L G
ASE
S
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GASES & KMT
Demo Observable
Characteristic
of the Gas
Explain in terms of
particles.
Compression(syringe)
Gases are
compressible
The space between
particles can be
reduced.
REA
L G
ASE
S
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GASES & KMTDemo Observable
Characteristic of
the Gas
Explain in terms of
particles.
White
Smoke
(perfume)
REA
L G
ASE
S
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GASES & KMT
Demo Observable
Characteristic of
the Gas
Explain in terms of
particles.
White
Smoke
(perfume)
Gases diffuse Because motion is
random, given enough
time particles will
spread out
evenly/randomly in the
given space.
REA
L G
ASE
S
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When a ‘smelly gas’ such as a deodorant is let loose in a room, its particles mix
with the particles of air. The particles of ‘smelly gas’ are free to move quickly in all
directions. They eventually spread through the whole room. This is diffusion.
Diffusion in gases is quick because the particles in a gas move quickly. It happens
even faster in hot gases
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GASES & KMT
Demo Observable
Characteristic of
the Gas
Explain in terms of
particles.
Ethanol
Canon(potato gun)
REA
L G
ASE
S
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GASES & KMTDemo Observable
Characteristic of
the Gas
Explain in terms of
particles.
Ethanol
Canon
(potato gun)
Gases exert pressure.
This pressure exists
as a force.
Particles collide more
(create pressure) in
smaller spaces or when
they are moving faster.
REA
L G
ASE
S
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Big Idea
Pressure:
Pressure is created when atoms/molecules
collide with other particles or the walls of
their container.
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KMT & IDEAL GASES
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THEORETICAL CHARACTERISTICS OF AN IDEAL GAS
Gases:
Postulate #1
Gas particles travel in
straight lines.
IDEA
L G
ASE
S
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THEORETICAL CHARACTERISTICS OF AN IDEAL GAS
Gases:
Postulate #2
Particles collide with the walls of the
container & each other with elastic collisions.
Elastic collisions = Complete transfer of
energy.
IDEA
L G
ASE
S
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INELASTIC VS. ELASTIC COLLISIONS
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There are no bonds between the particles in a gas, so they are free to move
in any direction. They strike the walls of their container and create a
pressure.
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THEORETICAL CHARACTERISTICS OF AN IDEAL GAS
Gases:
Postulate #3
Particles have no volume themselves.
(Exist as points)
IDEA
L G
ASE
S
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THEORETICAL CHARACTERISTICS OF AN IDEAL GAS
Gases: IDEA
L G
ASE
S
Postulate #4
There are no attractive
forces between
molecules
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Big Idea
Real gases act most ideal at HIGH
temperatures and LOW pressure.
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KMT
Practice Regents Questions
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PRESSURE & VOLUME
Boyle’s Law:
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TEMPERATURE & VOLUME
Charles’ Law:
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TEMPERATURE & PRESSURE
Gay – Lussac/Amonton:
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GAS LAWS
Combined Gas Law:
P1V1 = P2V2
T1 T2
(temperature must be in Kelvin)
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GAS LAWS Practice Problem 1: A gas at 608mm Hg is held in
a container with a volume of 545 cm3. The volume of
the container is increased to 1065 cm3 without a
change in temperature. Calculate the new pressure of
the gas.
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GAS LAWS
Practice Problem 2: What will be the volume of a gas
sample at 335 K if its volume at 273 K is 8.57 L?
Assume pressure remains unchanged.
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GAS LAWS Practice Problem 3: A sample of oxygen gas has a
volume of 205 cm3 when its temperature is 22.0 °C
and its pressure is 30.8 kPa. What volume will the gas
occupy at STP? (Hint: Table A)
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GAS LAWS
Avogadro’s Law:
Gases with the same
Volume (at the same
temperature and
pressure) have the same
number of particles.
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GAS LAWS
Practice Regents Questions.
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PLEASE CREATE AN ACCOUNT
• Go to testwizard.com
• Create an account using your gmail account
• Please join the class using the following code: CCOS-2CIM-XV
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PLEASE GO TO GOOGLE CLASSROOM
• Complete the assignment U1V4 Classification of Matter
• RESULTS WILL BE SUBMITTED AND SENT IN FOR A GRADE!!
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PURE SUBSTANCE: ONE TYPE OF
PARTICLE.
Definition: Made of 1 type of atom
Representation:
Characteristics:
- Cannot be broken down/separated (chemically)
- Pure Substances (contains only 1 type of particle)
- Written w/ symbols
- 92 natural, aprox 118 total (named after people, places, Latin names, etc)
- Ex: Copper, Calcium, Hydrogen, O2, Mg, Cu, F2
Elements
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COMPOUNDSDefinition: Made up of 2 or more elements chemically combined.
(bonded together)
Representation:
Characteristics:
- Chemically bonded (can be chemically separated)
- Pure substance
- Have different properties than the elements that make them up
- Specific ratio of elements within the compound
- Written with formulas
Examples: Copper (II) Chloride, Sodium Chloride, H2O, C6H12O6
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CLASSIFICATION OF MATTERParticle Diagram Practice: Label the boxes below
as an element, mixture or compound.
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CLASSIFICATION OF MATTER
Reflect:
If solid water melts into liquid water, has the basic identity of the water changed? Explain.
No, it is still water, it is just in a different phase.
If water is decomposed into oxygen and hydrogen gas, has the basic identity of the water changed? Explain.
Yes, it is no longer 2 hydrogens and an oxygen bonded together. The molecule has been separated into two distinct different elements.
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Big Idea
Regardless if matter is going through a physical change or a
chemical change, the amount of matter ALWAYS STAYS
CONSTANT.
Amount of matter before the change = Amount of matter
after the change
Law of Conservation of Matter:
Matter (mass) can not be created or destroyed, it just changes form.
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Complete the Practice Regents Questions
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SEPARATING MIXTURES BASED ON THEIR COMPOSITION:SEPARATION OF HETEROGENEOUS MIXTURESFiltration
• Based on differences in phase
• Works on separating particles
that do NOT dissolve.
• Ex: separating sand and water
mixture
Magnetism
• Based on magnetic/ metallic
properties
Ex: separating iron filings from a
nonmetallic substance (sulfur).
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SEPARATING MIXTURES BASED ON THEIR COMPOSITION:SEPARATION OF HOMOGENEOUS MIXTURES
Distillation
• Based on differences in boiling
points
• Separates liquids from each
other. Liquid w/ the lower boiling
point boils off first.
Ex: separating
crude oil
Chromatography
• Based on differences in solubility
& polarity
Ex: separating plant pigments or
ink
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SEPARATING MIXTURES BASED ON THEIR COMPOSITION:SEPARATION OF HOMOGENEOUS MIXTURES
Evaporation/Crystallization:
• For use in separating solids dissolved in a liquid.
Ex: aqueous salt solution (separating the salt from salt
water).
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KINETIC MOLECULAR THEORY
Kinetic Molecular Theory: The theory of the
movement of molecules at different pressures
and temperatures.
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GASES & KMT
Temperature:
Total average kinetic energy of
particles
Pressure:
Sum of collisions between
particles/walls of container
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GAS LAWS II
Reflect: Explain, in terms of kinetic molecular theory, why the pressure increases in a gas sample if you increase temperature (assume the volume remains constant)
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GAS LAWS IIGraham’s Law: The lighter a gas is, the quicker it
diffuses (or effuses – goes through a small hole).
Which gas would diffuse (or
effuse) fastest?
CH4
CO2
He
H2
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GAS LAWS II
Dalton’s Law of Partial Pressures:
The total pressure of a gas is equal to the sum of
the partial pressures of the individual gases that
make up the sample. Pt = Pa + Pb + Pc….
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GAS LAWS II
Practice Problem 1: What is the atmospheric
pressure if the partial pressure of nitrogen,
oxygen and argon are 604.5 mm Hg, 162.8 mm
Hg, and 0.5 mm Hg, respectively?
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GAS LAWS IIPractice Problem 2: If the total pressure of a gas
sample is 33.9 atm, what is the partial pressure
of an unknown gas if the other gases have partial
pressures as follows: oxygen gas is 10.4 atm,
hydrogen 7.8, and carbon dioxide is 4.2 atm?
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CLASSIFICATION OF MATTER
Reflect:
State the term for as many phase changes as you can.
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CLASSIFICATION OF MATTER
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PURE SUBSTANCE: ONE TYPE OF
PARTICLE.
Definition: Made of 1 type of atom
Representation:
Characteristics:
- Cannot be broken down/separated (chemically)
- Pure Substances
- Written w/ symbols
- 92 natural, aprox 118 total (named after people, places, Latin names, etc)
- Ex: Copper, Calcium, Hydrogen, O2, Mg, Cu, F2
Elements
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COMPOUNDSDefinition: Made up of 2 or more elements chemically combined.
(bonded together)
Representation:
Characteristics:
- Chemically bonded (can be chemically separated)
- Pure substance
- Have different properties than the elements that make them up
- Specific ratio of atoms
- Written with formulas
Examples: Copper (II) Chloride, Sodium Chloride, H2O, C6H12O6
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CLASSIFICATION OF MATTERParticle Diagram Practice: Label the boxes below
as an element, mixture or compound.
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Answer Practice Regents Questions