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Ch. 2 - Classification of Matter
I. Describing Matter (p.34 - 53)–Physical Property
–Physical Change
–Chemical Change
–Chemical Property
MATTER
What is Matter?
•Anything that has mass and volume
Characteristic properties
physical and chemical properties that help to define and identify a given substance. Density, freezing point and boiling point are characteristic physical properties. Reactivity is a characteristic chemical property.
A. Physical Property
A characteristic of a substance that can be observed without changing its identity.
– can be used to separate mixtures
– EX: magnetism, density, color, size, shape,
D. Chemical Property
A characteristic that indicates whether a substance can undergo a specific chemical change.
– EX: flammability, reactivity
A chemical property is the ABILITY of a substance to react with something else (air, water, acids, etc
Boiling pointBoiling pointMelting pointMelting pointColor (gray, red, etc.)Color (gray, red, etc.)CombustibilityCombustibilityConductivityConductivityCrystallinityCrystallinityDensityDensityDuctilityDuctilityFluorescenceFluorescenceMalleability (brittle, malleable)Malleability (brittle, malleable)Fracture / cleavageFracture / cleavageMassMassState (solid, liquid, gas, plasma)State (solid, liquid, gas, plasma)HardnessHardnessSolubility (soluble, insoluble)Solubility (soluble, insoluble)
Appearance / Homogeneity Appearance / Homogeneity (homogeneous, heterogeneous)(homogeneous, heterogeneous)
Reactivity (reactive with…, Reactivity (reactive with…, nonreactive with…, inert)nonreactive with…, inert)
Origin (naturally occurring, organic, Origin (naturally occurring, organic, inorganic, synthetic)inorganic, synthetic)
Luster (dull, shiny)Luster (dull, shiny)Texture (smooth, rough)Texture (smooth, rough)Shape (cubic, pyramidal, elliptical, Shape (cubic, pyramidal, elliptical,
spherical, etc.)spherical, etc.)StreakStreakOptical properties (transparent, Optical properties (transparent,
translucent, opaque)translucent, opaque)VolumeVolumeWeightWeightMagnetic (magnetic, nonmagnetic)Magnetic (magnetic, nonmagnetic)FlammabilityFlammability
Some properties…
=
if if
PROPERTIES OF MATTER
characteristics or qualities that describe matter or its behavior
can be classified as
PHYSICAL PROPERTIES
CHEMICAL PROPERTIES
they are characteristics that can be observed without
__________________________________________________________
they are characteristics that describe the substances ability to _______________ ______________________________________________________________
including including
(t) testable(o) observable
(m) measurable
=
if if
Main Idea
PROPERTIES OF MATTER
characteristics or qualities that describe matter or its behavior
can be classified as
PHYSICAL PROPERTIES
CHEMICAL PROPERTIES
they are characteristics that can be observed without changing the
identity of the substance.
they are characteristics that describe the substances ability to change into a new
substance with different properties / to
undergo a chemical change (reaction)
including
boiling point melting point color conductivitycrystallinity densityductility fluorescencemalleability fracture / cleavagehardness appearance / homogeneityorigin lustertexture shapestreak optical propertiesvolume weight
including
combustibilityreactivity
(t) testable(o) observable
(m) measurable
B. Physical Change
A change in the form of a substance without changing its identity.
– properties remain the same
– reversible
– can be used to separate mixtures
– EX: dissolving, grinding
C. Chemical Change A change in the identity of a substance.
– properties change
– irreversible
– Signs: color change, formation of a gas/solid, release of light/heat
– EX: burning, rusting
Chapter 3: States of MatterAKA: The Kinetic Model Theory (KMT)
4 States of Matter
Matter: is anything that has mass and volume
4 States of Matter: solid, liquid, gas, plasma
Solids Definite Shape and definite volume; particles
vibrate in place 2 types: crystalline and amorphous
1. Crystalline: particles are lined up neatly in repeating patterns of rows.
2. Amorphous: particles do not line up in repeated rows, has no true melting point
Examples of Solids: Crystalline: Amorphous:
Liquids
Definite volume Indefinite shape (takes shape of container) Particles are not arranged in repeating
patterns; particles slide past each other
Gas
Indefinite volume and indefinite shape Particle move rapidly to get away from each
other
Charles’s Law
Charles’s Law: as the temperature of a gas increases, the volume increases proportionally, provided that the pressure and amount of gas remain constant,
V1/T1 = V2/T2
temperature vo
lum
e
Boyle’s Law
This law is named for Charles Boyle, who studied the relationship between pressure, p, and volume, V, in the mid-1600s.
Boyle determined that for the same amount of a gas at constant temperature,
p * V = constant This defines an inverse relationship:
when one goes up, the other comes down.
pressure
volume
Boyle’s Law Boyle’s Law is one of the laws in physics that
concern the behaviour of gases When a gas is under pressure it takes up less
space: The higher the pressure, the smaller the
volume Boyles Law tells us about the relationship
between the volume of a gas and its pressure at a constant temperature
The law states that The law states that pressure is inversely pressure is inversely proportional to the volumeproportional to the volume
What’s up with Gas?
Temperature and volume are directly related-Charles Law
Volume and pressure are inversely related-Boyles Law
2. A sample of gas occupies 3.5 L at 300 K. What volume will it occupy at 200 K?V1 = 3.5 L, T1 = 300K, V2 = ?, T2 = 200KUsing Charles’ law: V1/T1 = V2/T2
3.5 L / 300 K = V2 / 200 KV2 = (3.5 L/300 K) x (200 K) = 2.3 L
For more lessons, visit www.chalkbored.com
K = C + 273
What volume changes occurs to a 400.0 mL gas sample as the temperature increases from 22.0 C to 30.0 C?
Plasma
Plasma
a. Hot, ionized gas particles.
b. Electrically charged.
c. Most common state in universe.
In summary,
Phase Properties
Phase
Particle Properties
Proximity Energy Motion Volume Shape
Solid
Liquid
Gas
close little vibrational definite definite
close moderate rotational definite indefinite
far apart a lot translational indefinite indefinite
ONE state of matter they didn’t teach you about in school…Until Now!
Bose-EinsteinCondensate
5th STATE OF MATTER
We all know about:
LIQUIDSSOLIDS GASES
Higher Temperature
Lower Temperature
What happens if you raise the temperature to super-high levels…between 1000°C and 1,000,000,000°C ?
Will everything just be a gas?
NO!If the gas is made up of particles which carry
an electric charge (“ionized particles”), but the entire gas as a whole has no electric charge, and if the density is not too high, then we can get
The 4th state of matter:
PLASMA
Some places where plasmas are found…
1. Flames
2. Lightning
3. Aurora (Northern Lights)
4. Neon lights
5. Stars
Stars make up 99% of the total matter in the Universe.
Therefore, 99% of everything that exists in the entire Universe is in the plasma state.
The Sun is an example of a star in its plasma state
6
6. Clouds of gas and dust around stars
So now we know all about four states of matter:
LIQUIDSSOLIDS GASES
Higher Temperatur
e
Lower Temperature
PLASMAS
(only for low density ionized
gases)
But now what happens if you lower the temperature way, way, down to100 nano degrees above
“Absolute Zero” (-273°C)
Will everything just be a
frozen solid?
Not Necessarily!In 1924 (84 years ago), two scientists, Albert
Einstein and Satyendra Bose predicted a 5th state of matter which would occur at very, very low temperatures.
Einstein Bose
+
The 5th state of matter:
Bose-Einstein Bose-Einstein CondensateCondensate
Finally, in 1995 (only 16 years ago!), Wolfgang Ketterle and his team of graduate students discovered the 5th state of matter for the first time. Ketterle and his
students
In a Bose-Einstein condensate, atoms can no longer bounce around as individuals.
Instead they must all act in exactly the same way, and you can no longer tell them apart!
Here is a picture a computer took of
Bose-Einstein Condensation The big peak
happens when all the atoms act exactly the same way!(We can’t see
Bose-Einstein condensation with our eyes because the atoms are too small)
Some other computer images of Bose-Einstein Condensates…
To really understand Bose-Einstein condensate you need to knowQuantu
m Physics
In 2002, Ketterle and two other scientists received the highest award in science for
discovering Bose-Einstein condensate:
The Nobel Prize
The five states of matter:
LIQUIDSSOLIDS GASES
Higher Temperatur
e
Lower Temperatur
e
PLASMAS
(only for low density ionized gases)
BOSE-EINSTEIN
CONDENSATE
Ch. 8 - Solids, Liquids, & Gases
II. Changes in State (p.224-227)–Phase Changes
–Heating Curves
MATTER
A. Phase Changes
Melting– solid to liquid
Freezing– liquid to solid
melting point = freezing point
A. Phase Changes
Vaporization (boiling)– liquid to gas at the boiling point
Evaporation– liquid to gas below the boiling point
Condensation– gas to liquid
A. Phase Changes Sublimation
– solid to gas– EX: dry ice, freeze
drying, iodine
A. Phase Changes
B. Heating Curves
Kinetic Energy– motion of particles– related to temperature
Potential Energy– space between particles– related to phase changes
B. Heating Curves
Solid - KE
Melting - PE
Liquid - KE Boiling - PE
Gas - KE
B. Heating Curves
Heat of Fusion– energy required to change from solid to liquid– some attractive forces are broken
B. Heating Curves
Heat of Vaporization– energy required to change from liquid to gas– all attractive forces are broken– EX: steam burns, sweating, and… the drinking
bird
HEATING CURVE
Phase Change Graph
Start from: Change to: Name
solid liquid melting
liquid solid freezing
liquid gas boiling
gas liquid condensation
solidgas
(skipping liquid phase)sublimation
Ch. 16 - Chemical Reactions
IV. Energy & Chemical Reactions
Energy Changes Exothermic Reactions Endothermic Reactions
A. Energy Changes During a chemical reaction…
– energy is used to break bonds– energy is released when new bonds are formed
breakingbonds
makingbonds
C. Endothermic Reaction reaction that absorbs energy
energy req’d to break old bonds outweighs energy released by making new bonds
Feels cooler
Ex. Melting of ice absorbs energy, cold pack first aid kits
process used to obtain aluminum from aluminum ore
2Al2O3 + energy 4Al + 3O2
B. Exothermic Reaction reaction that releases energy
energy released by making new bonds outweighs energy req’d to break old bonds
Feels hot
Ex. Combustions, Digestion of food
H2(l) + O2(l) H2O(g) + energy
reaction that powers the space shuttle lift-off
Blue-Exothermic Green-Endothermic