EONS LEARNING

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    • Resources >
      • Study Skills
      • Periodic Table
      • Common Ion Sheet
      • The Scientific Method
      • Doing Background Research
    • Introduction and Course Philosophy
    • Unit 1: Beginning Chemistry >
      • Lesson 1: The Atom >
        • What is an Atom?
        • The Structure of Atoms
        • The Periodic Table
        • Modeling Atoms
      • Lesson 2: Chemical Bonding >
        • Why Do Atoms Form Bonds?
        • Ionic Bonding
        • Covalent Bonding
        • Intermolecular Attraction
      • Lesson 3: Chemical Nomenclature >
        • Octet Rule
        • Ionic Compounds
        • Covalent Molecules
      • Lesson 4: Molecular Molecules >
        • Modeling Ionic Compounds
        • Modeling Covalent Molecules
      • Lesson 5: States of Matter >
        • States of Matter
        • Phase Changes
      • Lesson 6: Density >
        • What is Density?
        • Calculating Density
      • Lesson 7: Thermodynamics >
        • Temperature
        • Heat
        • Gas Laws
      • Lesson 8: Solution Chemistry >
        • Diffusion
        • Solutions and Molarity
        • Semi-Permeable Membranes
      • Lesson 9: Thermal Expansion >
        • Thermal Expansion
    • Unit 2: Earth Science >
      • Lesson 10: Earth at a Glance >
        • Perspective
        • Maps
      • Lesson 11: Layers of the Earth >
        • Layers of the Earth
      • Lesson 12: Plate Tectonics >
        • Plate Tectonics
      • Lesson 13: Rocks and Minerals >
        • Rocks and Minerals
      • Lesson 14: Particle Sorting >
        • Differentiation
        • Deposition of Sediment
      • Lesson 15: The Atmosphere >
        • Composition of the Atmosphere
        • Layers of the Atmosphere
        • Change Over Time
        • Atmospheric Disruption
    • Unit 3: The Cell >
      • Lesson 16: Life >
        • What is Life?
        • Structural Hierarchy of Living Things
      • Lesson 17: Biochemistry >
        • Intro to Biochemistry
        • Water
        • Micromolecules
        • Energy, Carbohydrates, Lipids
        • Protein and Nucleic Acid
      • Lesson 18: Cells >
        • What are Cells?
        • Microscopy
        • Plant and Animal Cells
      • Lesson 19: Membrane Transport >
        • A Special Environment
        • The Structure of Membranes
        • Membrane Transport
      • Lesson 20: Energy and Cell Respiration >
        • Energy in Biology
        • Energy Diagrams
        • Glycolysis and Anaerobic Respiration
        • Aerobic Cellular Respiration
      • Lesson 21: Photosynthesis >
        • Plants Get Energy From The Sun
        • Photosynthesis Process
        • Energy, Ecosystems, and the Environment
    • Unit 4: Anatomy and Physiology >
      • Lesson 22: The Human Body >
        • What Are Bodies Made Of?
        • What Do Bodies Do?
      • Lesson 23: The Nervous System >
        • The Nervous System
        • Neuronal Communication
        • The Central Nervous System
      • Lesson 24: The Endocrine System >
        • The Endocrine System
        • Hormones
        • Hormones, Puberty, and Reproduction
      • Lesson 25: The Integumentary System >
        • The Integumentary System
      • Lesson 26: The Musculoskeletal System >
        • The Skeletal System
        • The Muscular System
        • Anatomy Of The Musculoskeletal System
      • Lesson 27: The Cardiovascular System >
        • Blood and Blood Vessels
        • The Heart
      • Lesson 28: The Respiratory System >
        • The Respiratory System
      • Lesson 29: The Digestive System >
        • The Digestive System
        • Nutrition
      • Lesson 30: The Excretory System >
        • The Excretory System
      • Lesson 31: The Immune System >
        • Disease and Infection
        • Immunity
    • Units 5-6 Coming Soon
  • Workbench
    • Unit 1 >
      • EIS >
        • Lesson 1: Atoms
        • Lesson 2: Chemical Bonding
        • Lesson 3: Chemical Nomenclature
        • Lesson 4: Molecular Models
        • Lesson 5: States of Matter
        • Lesson 6: Density
        • Lesson 7: Thermodynamics
        • Lesson 8: Solution Chemistry
        • Lesson 9: Thermal Expansion
      • Unit 1: Project
      • Unit 1: Exam Review
      • Unit 1: Exam
    • Unit 2 >
      • EIS >
        • Lesson 10: Earth at a Glance
        • Lesson 11: Layers of the Earth
        • Lesson 12: Plate Tectonics
        • Lesson 13: Rocks and Minerals
        • Lesson 14: Particle Sorting
        • Lesson 15: The Atmosphere
      • Unit 2: Project
      • Unit 2: Exam Review
      • Unit 2: Exam
    • Unit 3 >
      • EIS >
        • Lesson 16: Life
        • Lesson 17: Biochemsitry
        • Lesson 18: Cells
        • Lesson 19: Membrane Transport
        • Lesson 20: Energy and Cell Respiration
        • Lesson 21: Photosynthesis
      • Unit 3: Project
      • Unit 3: Exam Review
      • Unit 3: Exam
    • Unit 4 >
      • EIS >
        • 22: The Human Body
        • 23: The Nervous System
        • 24: The Endocrine System
        • 25: The Integumentary System
        • 26: The Musculoskeletal System
        • 27: The Cardiovascular System
        • 28: The Respiratory System
        • 29: The Digestive System
        • 30: The Excretory System
        • 31: The Immune System
      • Unit 4 Project
      • Unit 4 Exam Review
      • Unit 4 Exam
    • Units 5-6 Coming Soon
  • Donate
  • Home
  • About Us
  • Classroom
    • Resources >
      • Study Skills
      • Periodic Table
      • Common Ion Sheet
      • The Scientific Method
      • Doing Background Research
    • Introduction and Course Philosophy
    • Unit 1: Beginning Chemistry >
      • Lesson 1: The Atom >
        • What is an Atom?
        • The Structure of Atoms
        • The Periodic Table
        • Modeling Atoms
      • Lesson 2: Chemical Bonding >
        • Why Do Atoms Form Bonds?
        • Ionic Bonding
        • Covalent Bonding
        • Intermolecular Attraction
      • Lesson 3: Chemical Nomenclature >
        • Octet Rule
        • Ionic Compounds
        • Covalent Molecules
      • Lesson 4: Molecular Molecules >
        • Modeling Ionic Compounds
        • Modeling Covalent Molecules
      • Lesson 5: States of Matter >
        • States of Matter
        • Phase Changes
      • Lesson 6: Density >
        • What is Density?
        • Calculating Density
      • Lesson 7: Thermodynamics >
        • Temperature
        • Heat
        • Gas Laws
      • Lesson 8: Solution Chemistry >
        • Diffusion
        • Solutions and Molarity
        • Semi-Permeable Membranes
      • Lesson 9: Thermal Expansion >
        • Thermal Expansion
    • Unit 2: Earth Science >
      • Lesson 10: Earth at a Glance >
        • Perspective
        • Maps
      • Lesson 11: Layers of the Earth >
        • Layers of the Earth
      • Lesson 12: Plate Tectonics >
        • Plate Tectonics
      • Lesson 13: Rocks and Minerals >
        • Rocks and Minerals
      • Lesson 14: Particle Sorting >
        • Differentiation
        • Deposition of Sediment
      • Lesson 15: The Atmosphere >
        • Composition of the Atmosphere
        • Layers of the Atmosphere
        • Change Over Time
        • Atmospheric Disruption
    • Unit 3: The Cell >
      • Lesson 16: Life >
        • What is Life?
        • Structural Hierarchy of Living Things
      • Lesson 17: Biochemistry >
        • Intro to Biochemistry
        • Water
        • Micromolecules
        • Energy, Carbohydrates, Lipids
        • Protein and Nucleic Acid
      • Lesson 18: Cells >
        • What are Cells?
        • Microscopy
        • Plant and Animal Cells
      • Lesson 19: Membrane Transport >
        • A Special Environment
        • The Structure of Membranes
        • Membrane Transport
      • Lesson 20: Energy and Cell Respiration >
        • Energy in Biology
        • Energy Diagrams
        • Glycolysis and Anaerobic Respiration
        • Aerobic Cellular Respiration
      • Lesson 21: Photosynthesis >
        • Plants Get Energy From The Sun
        • Photosynthesis Process
        • Energy, Ecosystems, and the Environment
    • Unit 4: Anatomy and Physiology >
      • Lesson 22: The Human Body >
        • What Are Bodies Made Of?
        • What Do Bodies Do?
      • Lesson 23: The Nervous System >
        • The Nervous System
        • Neuronal Communication
        • The Central Nervous System
      • Lesson 24: The Endocrine System >
        • The Endocrine System
        • Hormones
        • Hormones, Puberty, and Reproduction
      • Lesson 25: The Integumentary System >
        • The Integumentary System
      • Lesson 26: The Musculoskeletal System >
        • The Skeletal System
        • The Muscular System
        • Anatomy Of The Musculoskeletal System
      • Lesson 27: The Cardiovascular System >
        • Blood and Blood Vessels
        • The Heart
      • Lesson 28: The Respiratory System >
        • The Respiratory System
      • Lesson 29: The Digestive System >
        • The Digestive System
        • Nutrition
      • Lesson 30: The Excretory System >
        • The Excretory System
      • Lesson 31: The Immune System >
        • Disease and Infection
        • Immunity
    • Units 5-6 Coming Soon
  • Workbench
    • Unit 1 >
      • EIS >
        • Lesson 1: Atoms
        • Lesson 2: Chemical Bonding
        • Lesson 3: Chemical Nomenclature
        • Lesson 4: Molecular Models
        • Lesson 5: States of Matter
        • Lesson 6: Density
        • Lesson 7: Thermodynamics
        • Lesson 8: Solution Chemistry
        • Lesson 9: Thermal Expansion
      • Unit 1: Project
      • Unit 1: Exam Review
      • Unit 1: Exam
    • Unit 2 >
      • EIS >
        • Lesson 10: Earth at a Glance
        • Lesson 11: Layers of the Earth
        • Lesson 12: Plate Tectonics
        • Lesson 13: Rocks and Minerals
        • Lesson 14: Particle Sorting
        • Lesson 15: The Atmosphere
      • Unit 2: Project
      • Unit 2: Exam Review
      • Unit 2: Exam
    • Unit 3 >
      • EIS >
        • Lesson 16: Life
        • Lesson 17: Biochemsitry
        • Lesson 18: Cells
        • Lesson 19: Membrane Transport
        • Lesson 20: Energy and Cell Respiration
        • Lesson 21: Photosynthesis
      • Unit 3: Project
      • Unit 3: Exam Review
      • Unit 3: Exam
    • Unit 4 >
      • EIS >
        • 22: The Human Body
        • 23: The Nervous System
        • 24: The Endocrine System
        • 25: The Integumentary System
        • 26: The Musculoskeletal System
        • 27: The Cardiovascular System
        • 28: The Respiratory System
        • 29: The Digestive System
        • 30: The Excretory System
        • 31: The Immune System
      • Unit 4 Project
      • Unit 4 Exam Review
      • Unit 4 Exam
    • Units 5-6 Coming Soon
  • Donate

States of Matter

In this lesson, you will learn about the states of matter. As you’ve learned, matter is stuff. It is you, me, and everything else in the universe. And, like a shapeshifting alien or a Transformer, matter can change forms. These forms are called states, as in “a way of being.” You can imagine matter getting very introspective and asking itself, “What am I? Why am I the way I am? How do I change? How do I become?” In this lesson, we will journey inward with matter on it’s introspective journey of self-discovery as we answer these important questions. 

The States of Matter

One day the air looked to the ocean. He thought, “Wow, I wonder what it takes to become so vast, yet so powerful and fluid.” Then he thought, “All I can do is make wind.” And, as he started to make wind, the ocean rose and crashed its waves and thrashed every which way, all the while wondering, “I wonder what it’s like to be air, so light, so unassuming and spacious, and yet so strong and capable of causing me so much change without even realizing it.” But the air didn’t see what it was doing to the ocean. All it saw was waves dancing and frolicking and having a good time—which just made the air want to be ocean more. The air wanted to be ocean so badly, and it couldn’t understand why it was that they were so different anyhow. The air started to cry. And as air cried, its tears became ocean.

What is the point of this story? Well, mostly it’s just nice poetry, and maybe it’s supposed to teach you something about not comparing yourself to others (I mean, maybe). It also goes to show you that all matter can be found in different states, or ways of being, that these states have different properties, and that matter can change between states. Bye-bye emotion story, it’s science time.

The three common states of matter are solid, liquid, and gas. A fourth state is plasma, which we’ll talk a bit about because it’s cool, but won’t worry too much about for this class.

Solids

The way molecules are structured is very important in determining the state an object will be in. In a solid, molecules are bonded into very compact departments. Under this umbrella, there are two main configurations atoms can have. The first is called a geometric lattice. In a geometric lattice, atoms are well organized into a specific type of structure. Most solids are found in a geometric lattice. Solids in a geometric lattice are called crystalline solids; examples include metals, ionic compounds, minerals (like diamonds), and ice cubes.
Not all solids are organized into a geometric lattice. Some solids are considered amorphous. Amorphous solids aren’t nicely structured like crystals; they’re more like a bunch of molecules just got smushed together.  Examples include glass, gels, thin films, and nanostructures. 
Seeing what a broad range of structures are encompassed by the term "solid," it may seem like a bit of a challenge for chemists to define. Peeling away from the microscope, however, it is really simple. A solid is a structure with a definite shape and volume. That is, if you stick a round solid into a square box, it will still be round. It will also still be the same size. This definition implies a certain structural rigidity about solids, making them a fascinating field of study because of the numerous practical applications--like building bridges, or making a lightweight cell phone.

Some types of intermolecular forces that could be going on in a solid include ionic bonding, covalent network bonding, and metallic bonding. Dipole-dipole interactions, hydrogen bonding, and dispersion forces are generally not strong enough to keep particles together in solid form. Ice is a special case where hydrogen bonding will hold it in a solid, and this only occurs because of the low temperature (which means molecules aren’t moving around much, so they don’t have the energy to escape hydrogen bonds). Sometimes, dispersion forces can be very strong if the molecule is just the right shape and size. This is what happens in fats. See the sub-lesson on intermolecular attraction for more information.

This is a great video if you’d like to learn more about solids:

Liquids

In liquid form, molecules are loosely bonded together; while liquids have definite volume, they do not have definite shape. For example, when you pour water from a beaker to a tub, the amount of water you pour is the same, but the shape is different. This is because molecules can move (relatively) freely in a liquid, whereas in a solid they're pretty much stuck in one place.

Note that you can pour a liquid. This is because the attraction between molecules is strong enough to hold the particles together (unlike in a gas), but not quite so strong that they are fixed in one spot (as they are in a solid). So, when you pour a liquid, the bonds are just sliding past each other, allowing the molecules to cascade down like a fountain. It's pretty cool.
Common types of intermolecular forces between the molecules in a liquid include dipole-dipole interactions and hydrogen bonding. These are strong, but not so strong that they aren’t flexible. Dispersion forces can hold a liquid together if the molecules are pretty long and can pack together pretty well (if they pack together really well they could even make solids). This is what happens in oils. See the sub-lesson on intermolecular attraction for more information.

The stronger the intermolecular attraction between particles in a liquid, the more viscous, or thick, it will be (think about pouring molasses as compared to water). The density of the liquid also influences the viscosity, but you'll learn more about this later.

Solids can become liquids by adding heat, like in melting. Since heat is adding energy, this causes the molecules to move faster, which allows them to escape their bonds and get away from each other.

This is a great video on liquids, if you’d like to know more:
(Mandatory disclaimer: Please do not put gallium in your mouth. I mean, it’s not particularly toxic, but, like, why?)

Gases

If solids are held together by strong bonds and liquids weak ones, gases, then, contain molecules that do not bond with one another. As a result, gas particles are free to float around wherever they want, taking up as much space as they want. They do not have a definite volume or shape. In other words, they will spread out (expand, or increase in volume) or condense to fill the container they are in, and they'll take on it's shape, too. Gas molecules are also very far apart from each other. To understand this, try grabbing a fistful of air--rather hard, isn't it? (Air is mostly empty space). So, basically, gases are just loners who do whatever they want—or at least try.
Picture
When there are lots of gas molecules in a small space, it is said to have a high pressure. If the container isn't strong enough to withstand this pressure, it might burst! (Think of an overfull balloon).  If we decrease the volume of a rigid enough container, the gas just gets squished together and ends up very high pressure. So, maybe gases don’t so much do what they want as what their container wants. That somehow seems less cool.
Picture
Since gases don't have a definite volume, they can be easily compressed (pushed into a smaller volume). This causes an increase in pressure.

Likewise, gases take up more space when we remove pressure, as demonstrated in this video:
If any intermolecular attraction exists between gases, it is very weak (for example, weak dispersion forces). 

Liquids can become gases when significant heat is added, like when we boil water. This happens for the same reason as the transition from solid to liquid: added kinetic energy means molecules can escape their bonds. Liquids can also become gases when significant pressure is removed, like in this video of boiling water in a vacuum:
This is a great video on the properties of gases:
We’ll talk more about gases later.

Plasma

Plasma is cool, and not very common. You may have heard of plasma in some other context. Plasma T.V.’s, neon signs, etc. But what exactly is plasma?

Well, plasma is an ionized gas. By heating up the gas, atoms/molecules gain energy. This causes gas to form intermolecular bonds (because of the ions participating in electrostatic interactions, like two ends of a magnet), creating plasma. 

Plasma is similar to gases in that both have neither a definite shape nor a definite volume. 
This is a nice video on plasma:

Summary

You should understand:
  • That molecules are closest together and bound by the strongest intermolecular forces in solids. Solids have definite shape and volume.
  • That molecules are medium-close together and bound by medium-strong intermolecular forces in liquids. Liquids have definite volume, but not shape.
  • That molecules are far apart and bound by weak or no intermolecular forces in gases. Gases have neither definite volume nor shape.
That substances can transition between solid, liquid, and gas depending on external factors, especially temperature and pressure. Higher temperature means more movement and more gas-like properties, and more pressure means less space between molecules and more solid-like properties.
Picture

Learning Activity

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Next: Phase changes

Content contributors: Rebecca Deng, Emma Moulton
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