unit 2: nature of matter and kinetic theory. part 1: the nature of matter
TRANSCRIPT
![Page 1: Unit 2: Nature of Matter and Kinetic Theory. Part 1: The Nature of Matter](https://reader034.vdocument.in/reader034/viewer/2022051214/56649e055503460f94af1f5d/html5/thumbnails/1.jpg)
Unit 2: Nature of Matter and Kinetic Theory
![Page 2: Unit 2: Nature of Matter and Kinetic Theory. Part 1: The Nature of Matter](https://reader034.vdocument.in/reader034/viewer/2022051214/56649e055503460f94af1f5d/html5/thumbnails/2.jpg)
Part 1: The Nature of Matter
![Page 3: Unit 2: Nature of Matter and Kinetic Theory. Part 1: The Nature of Matter](https://reader034.vdocument.in/reader034/viewer/2022051214/56649e055503460f94af1f5d/html5/thumbnails/3.jpg)
properties = characteristics and behavior of matter (includes changes that matter undergoes).
What color is it?Is it solid, liquid or gasIs it reactive?
structure = composition
• what matter is made of
• how matter is organized.
How do we classify matter?
![Page 4: Unit 2: Nature of Matter and Kinetic Theory. Part 1: The Nature of Matter](https://reader034.vdocument.in/reader034/viewer/2022051214/56649e055503460f94af1f5d/html5/thumbnails/4.jpg)
• Examples of physical properties :
• solubility, - dissolves in water?• melting point, boiling point
• color,• density,
• electrical conductivity,
• physical state (solid, liquid, or gas).
![Page 5: Unit 2: Nature of Matter and Kinetic Theory. Part 1: The Nature of Matter](https://reader034.vdocument.in/reader034/viewer/2022051214/56649e055503460f94af1f5d/html5/thumbnails/5.jpg)
• physical change - change in matter that does not involve a change in the chemical identity
• Change of state is a physical change:
![Page 6: Unit 2: Nature of Matter and Kinetic Theory. Part 1: The Nature of Matter](https://reader034.vdocument.in/reader034/viewer/2022051214/56649e055503460f94af1f5d/html5/thumbnails/6.jpg)
Classify by purityIs it a pure substance or mixture?
Pure substance = sample of matter that has definite chemical and physical properties, can be either an element or a compound
Classifying Matter
![Page 7: Unit 2: Nature of Matter and Kinetic Theory. Part 1: The Nature of Matter](https://reader034.vdocument.in/reader034/viewer/2022051214/56649e055503460f94af1f5d/html5/thumbnails/7.jpg)
![Page 8: Unit 2: Nature of Matter and Kinetic Theory. Part 1: The Nature of Matter](https://reader034.vdocument.in/reader034/viewer/2022051214/56649e055503460f94af1f5d/html5/thumbnails/8.jpg)
compound = pure substance that can be broken down into simpler substances.
element = substance that cannot be broken down into simpler substances.
Element or Compound?
salt
gold
![Page 9: Unit 2: Nature of Matter and Kinetic Theory. Part 1: The Nature of Matter](https://reader034.vdocument.in/reader034/viewer/2022051214/56649e055503460f94af1f5d/html5/thumbnails/9.jpg)
Compounds Are More Than One Element
formula = combination of the chemical symbols that show what elements make up a compound and the number of atoms of each element
Compound Formula
caffeine
salt
water
C8H10N4O2
NaCl
H2O
![Page 10: Unit 2: Nature of Matter and Kinetic Theory. Part 1: The Nature of Matter](https://reader034.vdocument.in/reader034/viewer/2022051214/56649e055503460f94af1f5d/html5/thumbnails/10.jpg)
Compounds Are More Than One Element
****The properties of the compound are different from the properties of the elements that compose the compound.
silver + bromine = silver bromide
![Page 11: Unit 2: Nature of Matter and Kinetic Theory. Part 1: The Nature of Matter](https://reader034.vdocument.in/reader034/viewer/2022051214/56649e055503460f94af1f5d/html5/thumbnails/11.jpg)
substance is not changed = no fixed composition
the basic identity of each
Mixture = made up of different kinds of matter
Pure Substance or Mixture?
![Page 12: Unit 2: Nature of Matter and Kinetic Theory. Part 1: The Nature of Matter](https://reader034.vdocument.in/reader034/viewer/2022051214/56649e055503460f94af1f5d/html5/thumbnails/12.jpg)
•Homogeneous mixtures are the same throughout.
• Also known as a solution.
Pure substance or a mixture?
![Page 13: Unit 2: Nature of Matter and Kinetic Theory. Part 1: The Nature of Matter](https://reader034.vdocument.in/reader034/viewer/2022051214/56649e055503460f94af1f5d/html5/thumbnails/13.jpg)
• When you dissolve sugar in water, sugar is the solute—the substance being dissolved.
• The substance that dissolves the solute is the solvent. in this case it is water
solute + solvent = solution
• When the solvent is water, the solution is called an aqueous solution.
![Page 14: Unit 2: Nature of Matter and Kinetic Theory. Part 1: The Nature of Matter](https://reader034.vdocument.in/reader034/viewer/2022051214/56649e055503460f94af1f5d/html5/thumbnails/14.jpg)
heterogeneous mixture is one with different compositions, depending upon where you look
Pure Substance or Mixture?
![Page 15: Unit 2: Nature of Matter and Kinetic Theory. Part 1: The Nature of Matter](https://reader034.vdocument.in/reader034/viewer/2022051214/56649e055503460f94af1f5d/html5/thumbnails/15.jpg)
![Page 16: Unit 2: Nature of Matter and Kinetic Theory. Part 1: The Nature of Matter](https://reader034.vdocument.in/reader034/viewer/2022051214/56649e055503460f94af1f5d/html5/thumbnails/16.jpg)
Pure Substance
Mixture
element
compound
homogenous
heterogeneous
Matter
![Page 17: Unit 2: Nature of Matter and Kinetic Theory. Part 1: The Nature of Matter](https://reader034.vdocument.in/reader034/viewer/2022051214/56649e055503460f94af1f5d/html5/thumbnails/17.jpg)
• a substance must be separated chemically
• a mixture can be separated physically
![Page 18: Unit 2: Nature of Matter and Kinetic Theory. Part 1: The Nature of Matter](https://reader034.vdocument.in/reader034/viewer/2022051214/56649e055503460f94af1f5d/html5/thumbnails/18.jpg)
An example of a pure substance in everyday life is _____.
a. pond water
b. a cola drink
c. sugar
d. concrete
c. sugar
![Page 19: Unit 2: Nature of Matter and Kinetic Theory. Part 1: The Nature of Matter](https://reader034.vdocument.in/reader034/viewer/2022051214/56649e055503460f94af1f5d/html5/thumbnails/19.jpg)
A soft drink is an example of a(n) _____.
a. compound
b. heterogeneous mixture
c. element
d. homogeneous mixture
d. homogenous mixture
![Page 20: Unit 2: Nature of Matter and Kinetic Theory. Part 1: The Nature of Matter](https://reader034.vdocument.in/reader034/viewer/2022051214/56649e055503460f94af1f5d/html5/thumbnails/20.jpg)
Identify each of the following as either a compound or a mixture.
A. sand
B. water
C. juice
mixture
compound
mixture
![Page 21: Unit 2: Nature of Matter and Kinetic Theory. Part 1: The Nature of Matter](https://reader034.vdocument.in/reader034/viewer/2022051214/56649e055503460f94af1f5d/html5/thumbnails/21.jpg)
In ocean water, salt is a(n) _____.
a. alloy
b. solution
c. solute
d. solvent
c. solute
![Page 22: Unit 2: Nature of Matter and Kinetic Theory. Part 1: The Nature of Matter](https://reader034.vdocument.in/reader034/viewer/2022051214/56649e055503460f94af1f5d/html5/thumbnails/22.jpg)
pure substance?element or compound?
a mixture?Heterogeneous or
homogenous Aluminum foil
Pure substance, element
![Page 23: Unit 2: Nature of Matter and Kinetic Theory. Part 1: The Nature of Matter](https://reader034.vdocument.in/reader034/viewer/2022051214/56649e055503460f94af1f5d/html5/thumbnails/23.jpg)
pure substance?element or compound?
a mixture?Heterogeneous or homogenous
• bowl of cereal
mixture, heterogeneous
![Page 24: Unit 2: Nature of Matter and Kinetic Theory. Part 1: The Nature of Matter](https://reader034.vdocument.in/reader034/viewer/2022051214/56649e055503460f94af1f5d/html5/thumbnails/24.jpg)
pure substance?element or compound?
a mixture?Heterogeneous or homogenous
• whipped cream
Mixture, homogenous
![Page 25: Unit 2: Nature of Matter and Kinetic Theory. Part 1: The Nature of Matter](https://reader034.vdocument.in/reader034/viewer/2022051214/56649e055503460f94af1f5d/html5/thumbnails/25.jpg)
pure substance?element or compound?
a mixture?Heterogeneous or homogenous
• oil and vinegar dressing
Mixture, heterogeneous
![Page 26: Unit 2: Nature of Matter and Kinetic Theory. Part 1: The Nature of Matter](https://reader034.vdocument.in/reader034/viewer/2022051214/56649e055503460f94af1f5d/html5/thumbnails/26.jpg)
pure substance?element or compound?
a mixture?Heterogeneous or homogenous
• aspirin - acetylsalicylic acid
Pure substance, compound
![Page 27: Unit 2: Nature of Matter and Kinetic Theory. Part 1: The Nature of Matter](https://reader034.vdocument.in/reader034/viewer/2022051214/56649e055503460f94af1f5d/html5/thumbnails/27.jpg)
pure substance?element or compound?
a mixture?Heterogeneous or homogenous
• orange juice with pulp
Mixture, heterogeneous
![Page 28: Unit 2: Nature of Matter and Kinetic Theory. Part 1: The Nature of Matter](https://reader034.vdocument.in/reader034/viewer/2022051214/56649e055503460f94af1f5d/html5/thumbnails/28.jpg)
pure substance?element or compound?
a mixture?Heterogeneous or homogenous
• gold
Pure substance, element
![Page 29: Unit 2: Nature of Matter and Kinetic Theory. Part 1: The Nature of Matter](https://reader034.vdocument.in/reader034/viewer/2022051214/56649e055503460f94af1f5d/html5/thumbnails/29.jpg)
pure substance?element or compound?
a mixture?Heterogeneous or homogenous
• salt
Pure substance, compound
![Page 30: Unit 2: Nature of Matter and Kinetic Theory. Part 1: The Nature of Matter](https://reader034.vdocument.in/reader034/viewer/2022051214/56649e055503460f94af1f5d/html5/thumbnails/30.jpg)
pure substance?element or compound?
a mixture?Heterogeneous or homogenous
• peanut butter
Mixture, homogenous
![Page 31: Unit 2: Nature of Matter and Kinetic Theory. Part 1: The Nature of Matter](https://reader034.vdocument.in/reader034/viewer/2022051214/56649e055503460f94af1f5d/html5/thumbnails/31.jpg)
Chemical Properties• Chemical properties are those that can
be observed only when there is a change in the composition of the substance.
• Rusting is a chemical reaction in which iron combines with oxygen to form a new substance, iron oxide.
Examples of chemical property:
• flammability
• reactivity
![Page 32: Unit 2: Nature of Matter and Kinetic Theory. Part 1: The Nature of Matter](https://reader034.vdocument.in/reader034/viewer/2022051214/56649e055503460f94af1f5d/html5/thumbnails/32.jpg)
Chemical Changes
chemical change - the change of one or more substances into other substances.
• A chemical property always relates to a
chemical change = chemical reaction.
![Page 33: Unit 2: Nature of Matter and Kinetic Theory. Part 1: The Nature of Matter](https://reader034.vdocument.in/reader034/viewer/2022051214/56649e055503460f94af1f5d/html5/thumbnails/33.jpg)
- production of bubbles- release or absorption of energy
- color change
***only way to be sure is to check the composition of the sample before and after the change.
Clues that a chemical change has occurred:
![Page 34: Unit 2: Nature of Matter and Kinetic Theory. Part 1: The Nature of Matter](https://reader034.vdocument.in/reader034/viewer/2022051214/56649e055503460f94af1f5d/html5/thumbnails/34.jpg)
Below are listed changes that can be observed in everyday life. Tell whether it is a physical change or a chemical change.
1.an icicle melting
2.charcoal burning
3.magnetizing a piece of steel
4.iron rusting
5.rubbing alcohol evaporating from the skin
physical change
chemical change
physical change
chemical change
physical change
![Page 35: Unit 2: Nature of Matter and Kinetic Theory. Part 1: The Nature of Matter](https://reader034.vdocument.in/reader034/viewer/2022051214/56649e055503460f94af1f5d/html5/thumbnails/35.jpg)
chemical change involves only a rearrangement of the atoms. Atoms DO NOT just appear or disappear.
******Law of Conservation of Mass****** In a chemical change, matter is neither created nor destroyed.
Chemical Reactions
![Page 36: Unit 2: Nature of Matter and Kinetic Theory. Part 1: The Nature of Matter](https://reader034.vdocument.in/reader034/viewer/2022051214/56649e055503460f94af1f5d/html5/thumbnails/36.jpg)
Chemical Reactions and Energy
• All chemical changes also involve some sort of energy change.
• Energy is either taken in or given off as the chemical change takes place. Energy is the capacity to do work.
• Work is done whenever something is moved.
![Page 37: Unit 2: Nature of Matter and Kinetic Theory. Part 1: The Nature of Matter](https://reader034.vdocument.in/reader034/viewer/2022051214/56649e055503460f94af1f5d/html5/thumbnails/37.jpg)
Chemical Reactions and Energy
• Energy is also produced and released in the form of heat and light.
Chemical reactions that GIVE OFF heat energy are called exothermic reactions.
![Page 38: Unit 2: Nature of Matter and Kinetic Theory. Part 1: The Nature of Matter](https://reader034.vdocument.in/reader034/viewer/2022051214/56649e055503460f94af1f5d/html5/thumbnails/38.jpg)
• Chemical reactions that ABSORB heat energy are called endothermic reactions.
Chemical Reactions and Energy
![Page 39: Unit 2: Nature of Matter and Kinetic Theory. Part 1: The Nature of Matter](https://reader034.vdocument.in/reader034/viewer/2022051214/56649e055503460f94af1f5d/html5/thumbnails/39.jpg)
Classify each of the following as a chemical or physical property.
A. density
B. reactivity
C. color
D. melting point
physical property
chemical property
physical property
physical property
![Page 40: Unit 2: Nature of Matter and Kinetic Theory. Part 1: The Nature of Matter](https://reader034.vdocument.in/reader034/viewer/2022051214/56649e055503460f94af1f5d/html5/thumbnails/40.jpg)
Part 2: The Kinetic Theory
• States of Matter–solid–liquid–gas–plasma
![Page 41: Unit 2: Nature of Matter and Kinetic Theory. Part 1: The Nature of Matter](https://reader034.vdocument.in/reader034/viewer/2022051214/56649e055503460f94af1f5d/html5/thumbnails/41.jpg)
Intermolecular Forces (IMF)
• Attractive forces between molecules.
Much weaker than chemical bonds within molecules.
![Page 42: Unit 2: Nature of Matter and Kinetic Theory. Part 1: The Nature of Matter](https://reader034.vdocument.in/reader034/viewer/2022051214/56649e055503460f94af1f5d/html5/thumbnails/42.jpg)
The Kinetic Theory of Matter
1. Matter is composed of PARTICLES.
2. Particle movement is rapid, constant, and random (Brownian motion)
![Page 43: Unit 2: Nature of Matter and Kinetic Theory. Part 1: The Nature of Matter](https://reader034.vdocument.in/reader034/viewer/2022051214/56649e055503460f94af1f5d/html5/thumbnails/43.jpg)
The Kinetic Theory of Matter
3.All collisions are perfectly ELASTIC (NO energy lost).
![Page 44: Unit 2: Nature of Matter and Kinetic Theory. Part 1: The Nature of Matter](https://reader034.vdocument.in/reader034/viewer/2022051214/56649e055503460f94af1f5d/html5/thumbnails/44.jpg)
Kinetic theory of matter
Kinetic energy (K.E.) = energy of motion
• gases have the least restriction on motion– have the most K.E.
• solids have the most restriction on motion– have the least K.E.
![Page 45: Unit 2: Nature of Matter and Kinetic Theory. Part 1: The Nature of Matter](https://reader034.vdocument.in/reader034/viewer/2022051214/56649e055503460f94af1f5d/html5/thumbnails/45.jpg)
Kinetic model of gases
• Gases: matter with variable shape and variable volume
• Gas particles move in a straight line until they collide with container or each other
![Page 46: Unit 2: Nature of Matter and Kinetic Theory. Part 1: The Nature of Matter](https://reader034.vdocument.in/reader034/viewer/2022051214/56649e055503460f94af1f5d/html5/thumbnails/46.jpg)
Kinetic model of liquids• Liquids: matter with variable
shape and definite volume
• Particles slide past each other but are so close together they do not move in a straight line
![Page 47: Unit 2: Nature of Matter and Kinetic Theory. Part 1: The Nature of Matter](https://reader034.vdocument.in/reader034/viewer/2022051214/56649e055503460f94af1f5d/html5/thumbnails/47.jpg)
Kinetic model of solids
• solids: matter with definite shape and definite volume
• Particles cannot move past each other, they are in constant motion bouncing off neighbors
![Page 48: Unit 2: Nature of Matter and Kinetic Theory. Part 1: The Nature of Matter](https://reader034.vdocument.in/reader034/viewer/2022051214/56649e055503460f94af1f5d/html5/thumbnails/48.jpg)
Other forms of matter• Plasmas - gaseous mixture of ions
-exists at high temperatures
• most common form of matter in the universe but least common on Earth itself
![Page 49: Unit 2: Nature of Matter and Kinetic Theory. Part 1: The Nature of Matter](https://reader034.vdocument.in/reader034/viewer/2022051214/56649e055503460f94af1f5d/html5/thumbnails/49.jpg)
Plasmas continued
• an ionized gas that conducts electricity -forms at very high temps when matter absorbs energy and breaks apart
• The sun is made of plasma- also found in fluorescent lights
![Page 50: Unit 2: Nature of Matter and Kinetic Theory. Part 1: The Nature of Matter](https://reader034.vdocument.in/reader034/viewer/2022051214/56649e055503460f94af1f5d/html5/thumbnails/50.jpg)
Temperature and kinetic energy
• temperature—the measure of the average K.E. of particles in a sample
• Kelvin (K) – SI base unit of temperature; measures average K.E.
![Page 51: Unit 2: Nature of Matter and Kinetic Theory. Part 1: The Nature of Matter](https://reader034.vdocument.in/reader034/viewer/2022051214/56649e055503460f94af1f5d/html5/thumbnails/51.jpg)
Temperature and kinetic energy
• When temp increases, particle motion increases.
• When temp decreases, particle motion decreases.
A temp of 300 K has twice the kinetic energy as 150 K.
![Page 52: Unit 2: Nature of Matter and Kinetic Theory. Part 1: The Nature of Matter](https://reader034.vdocument.in/reader034/viewer/2022051214/56649e055503460f94af1f5d/html5/thumbnails/52.jpg)
Temperature and kinetic energy
• 0 Kelvin = absolute zero = no molecular motion
• No degrees sign ( ° ) is used with Kelvin numbers
• There will never be negative numbers for Kelvin temperatures!.
![Page 53: Unit 2: Nature of Matter and Kinetic Theory. Part 1: The Nature of Matter](https://reader034.vdocument.in/reader034/viewer/2022051214/56649e055503460f94af1f5d/html5/thumbnails/53.jpg)
density compressibility
intermolecular forces
solid most dense difficult to compress
strong
liquid
gas least dense easily compressed
weak
Comparing solids, liquids, and gases
![Page 54: Unit 2: Nature of Matter and Kinetic Theory. Part 1: The Nature of Matter](https://reader034.vdocument.in/reader034/viewer/2022051214/56649e055503460f94af1f5d/html5/thumbnails/54.jpg)
Kinetic energy
space between particles
organization
solid least amount of kinetic energy
very little space between particles
most organized
liquid
gas most amount of kinetic energy
a lot of space between particles
least organized
Comparing solids, liquids, and gases
![Page 55: Unit 2: Nature of Matter and Kinetic Theory. Part 1: The Nature of Matter](https://reader034.vdocument.in/reader034/viewer/2022051214/56649e055503460f94af1f5d/html5/thumbnails/55.jpg)
Changing states and energy changes
• Going from a more energetic state (gas) to a less energetic state (solid) requires a release of energy–exothermic
![Page 56: Unit 2: Nature of Matter and Kinetic Theory. Part 1: The Nature of Matter](https://reader034.vdocument.in/reader034/viewer/2022051214/56649e055503460f94af1f5d/html5/thumbnails/56.jpg)
• Going from less energetic (solid) to more energetic (gas) requires absorption of energy -- endothermic
![Page 57: Unit 2: Nature of Matter and Kinetic Theory. Part 1: The Nature of Matter](https://reader034.vdocument.in/reader034/viewer/2022051214/56649e055503460f94af1f5d/html5/thumbnails/57.jpg)
Vapor Pressure and boiling
• Vapor PressureVapor Pressure - pressure of vapor above a liquid at equilibrium
•high vapor pressure = volatile•volatile = easily evaporates
•The greater the fraction of molecules which can escape the liquid, the greater the vapor pressure
![Page 58: Unit 2: Nature of Matter and Kinetic Theory. Part 1: The Nature of Matter](https://reader034.vdocument.in/reader034/viewer/2022051214/56649e055503460f94af1f5d/html5/thumbnails/58.jpg)
• What happens to the vapor pressure if you increase the temperature of a liquid in a closed container?
–causes the vapor pressure above the liquid to increase.
![Page 59: Unit 2: Nature of Matter and Kinetic Theory. Part 1: The Nature of Matter](https://reader034.vdocument.in/reader034/viewer/2022051214/56649e055503460f94af1f5d/html5/thumbnails/59.jpg)
equilibrium vapor pressure - when the number of vapor molecules rejoining the water equals the number leaving to go into the vapor phase
![Page 60: Unit 2: Nature of Matter and Kinetic Theory. Part 1: The Nature of Matter](https://reader034.vdocument.in/reader034/viewer/2022051214/56649e055503460f94af1f5d/html5/thumbnails/60.jpg)
• If there is equilibrium between the liquid state and the gas state, what is true about the rate of evaporation and the rate of condensation?
• They are equal
![Page 61: Unit 2: Nature of Matter and Kinetic Theory. Part 1: The Nature of Matter](https://reader034.vdocument.in/reader034/viewer/2022051214/56649e055503460f94af1f5d/html5/thumbnails/61.jpg)
Vapor pressure and boiling point
• Boiling Point - temp at which v.p. of liquid equals external pressure
-depends on atmospheric
pressure & IMF
Normal B.P. - b.p. at 1 atm
![Page 62: Unit 2: Nature of Matter and Kinetic Theory. Part 1: The Nature of Matter](https://reader034.vdocument.in/reader034/viewer/2022051214/56649e055503460f94af1f5d/html5/thumbnails/62.jpg)
Effects of Intermolecular Forces (IMF)
• When IMF’s are weak–vapor pressure is high–volatility is high–boiling point is low
![Page 63: Unit 2: Nature of Matter and Kinetic Theory. Part 1: The Nature of Matter](https://reader034.vdocument.in/reader034/viewer/2022051214/56649e055503460f94af1f5d/html5/thumbnails/63.jpg)
Heat of Fusion
• Melting point – temp of a solid when it becomes a liquid= freezing point (temp when liquid
becomes a solid)
![Page 64: Unit 2: Nature of Matter and Kinetic Theory. Part 1: The Nature of Matter](https://reader034.vdocument.in/reader034/viewer/2022051214/56649e055503460f94af1f5d/html5/thumbnails/64.jpg)
B. Heating Curves
Freezing/Melting point
Solid
Liquid
Boiling point
Gas
![Page 65: Unit 2: Nature of Matter and Kinetic Theory. Part 1: The Nature of Matter](https://reader034.vdocument.in/reader034/viewer/2022051214/56649e055503460f94af1f5d/html5/thumbnails/65.jpg)
Heating Curves• IMPORTANT: temp does not change
during the actual phase change.• Increasing the temp will only make
the change happen faster.
![Page 66: Unit 2: Nature of Matter and Kinetic Theory. Part 1: The Nature of Matter](https://reader034.vdocument.in/reader034/viewer/2022051214/56649e055503460f94af1f5d/html5/thumbnails/66.jpg)
Phase Diagrams• Shows the phases of a
substance at different temps and pressures.
![Page 67: Unit 2: Nature of Matter and Kinetic Theory. Part 1: The Nature of Matter](https://reader034.vdocument.in/reader034/viewer/2022051214/56649e055503460f94af1f5d/html5/thumbnails/67.jpg)
triple point -the point (temperature and pressure) on a phase diagram at which three phases of a substance can coexist.
All six phase changes can occur at the triple point: freezing and melting, evaporation and condensation, sublimation and deposition.
![Page 68: Unit 2: Nature of Matter and Kinetic Theory. Part 1: The Nature of Matter](https://reader034.vdocument.in/reader034/viewer/2022051214/56649e055503460f94af1f5d/html5/thumbnails/68.jpg)
Phase Diagrams
critical point -at extremely high temperatures and pressures, the liquid and gaseous phases become indistinguishable, in what is known as a supercritical fluid
![Page 69: Unit 2: Nature of Matter and Kinetic Theory. Part 1: The Nature of Matter](https://reader034.vdocument.in/reader034/viewer/2022051214/56649e055503460f94af1f5d/html5/thumbnails/69.jpg)
The End!