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MATTER

Discover the four states of matter - solid, liquid, gas, and plasma - and learn about their properties, changes, and physical and chemical properties.

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MATTER

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  1. MATTER Does it Really MATTER? YES

  2. STATES OF MATTER The Four States of Matter • Solid • Liquid • Gas • Plasma • Based upon particle arrangement • Based upon energy of particles • Based upon distance between particles

  3. States of Matter

  4. States of Matter A. The Kinetic Theory 1. All matter is composed of small particles (atoms, molecules, or ions). 2. They are in constant, random motion. 3. They constantly collide with each other and with the walls of their container.

  5. STATES OF MATTERSOLIDS • Particles of solids are tightly packed, vibrating about a fixed position. • Solids have a definite shape and a definite volume.

  6. STATES OF MATTERLIQUID • Particles of liquids are tightly packed, but are far enough apart to slide over one another. • Liquids have an indefinite shape and a definite volume.

  7. STATES OF MATTERGAS • Particles of gases are very far apart and move freely. • Gases have an indefinite shape and an indefinite volume.

  8. B. Phase Properties Particle Properties Phase Proximity Energy Motion Volume Shape Solid close little vibrational definite definite Liquid close moderate rotational definite indefinite Gas far apart a lot translational indefinite indefinite

  9. PHASE CHANGES

  10. PHASE CHANGES

  11. Chemistry Joke • A small piece of ice which lived in a test tube fell in love with a Bunsen burner. "Bunsen! my flame! I melt whenever I see you" said the ice. The Bunsen burner replied : "It's just a phase you're going through".

  12. Thermal E x p a n s i o n 1. Particles in any state expand when heated (generally). 2. Examples of solids: a. Expansion joints b. Power lines c. Thermostats 3. Different materials expand at different rates.

  13. 4. Mercury and alcohol are liquids that expand in thermometers 5. Air expands when heated (becoming less dense) 6. Water reaches maximum density at about 4 C. Ice particles are farther apart than liquid water (so it floats).

  14. But 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?

  15. Plasma a. Hot, ionized gas particles. b. Electrically charged. c. Most common state in universe.

  16. Some places where plasmas are found… 1.Flames

  17. 2. Lightning

  18. 3. Aurora (Northern Lights)

  19. The Sun is an example of a star in its plasma state

  20. Plasma

  21. STATES OF MATTER LIQUID PLASMA SOLID GAS Tightly packed, in a regular pattern Vibrate, but do not move from place to place Close together with no regular arrangement. Vibrate, move about, and slide past each other Well separated with no regular arrangement. Vibrate and move freely at high speeds Has no definite volume or shape and is composed of electrical charged particles

  22. Physical Properties What are some physical properties? • color • melting and boiling point • odor

  23. Physical Changes • can be observed without changing the identity of the substance Some physical changes would be • boiling of a liquid • melting of a solid • dissolving a solid in a liquid

  24. Chemical Properties and Chemical Change • Burning hydrogen (H2) in oxygen (O2) gives H2O. • Chemical change or chemical reaction — transformation of one or more atoms or molecules into one or more different molecules.

  25. Sure Signs of a Chemical Change • Heat • Light • Gas Produced (not from boiling!) • Precipitate – a solid formed by mixing two liquids together

  26. Physical vs. Chemical physical chemical physical physical chemical • Examples: • melting point • flammable • density • magnetic • tarnishes in air

  27. MIXTURE PURE SUBSTANCE yes Is the composition uniform? no yes no Can it be chemically decomposed? Colloids Suspensions Matter Flowchart MATTER yes no Can it be physically separated? Homogeneous Mixture (solution) Heterogeneous Mixture Compound Element

  28. What Are Substances ?? Substances can be identified as either an element, compound, or a mixture.

  29. A substance cannot be further broken down or purified by physical means. • A substance is matter of a particular kind. • Each substance has its own characteristic properties that are different from the set of properties of any other substance.

  30. Pure substances Elements • The simplest form of matter that has a unique set of properties. • Cannot be decomposed into simpler substances by chemical changes Compounds • Can be decomposed into simpler substances by chemical changes, always in a definite ratio • A compound is a substance that contains two or more elements chemically combined in a fixed proportion

  31. Elements, Molecules and Compounds Some elements, such as the noble gases, exist as individual atoms. Often, elements consist of two or more atoms joined together. We call these molecules. If more than one type of atom is in a molecule, we call it a compound.

  32. Definitions • A solution is a homogeneous mixture • A soluteis dissolved in a solvent. • A saturated solution is one where the concentration is at a maximum - no more solute is able to dissolve. • A saturated solution represents an equilibrium: the rate of dissolving is equal to the rate of crystallization. The salt continues to dissolve, but crystallizes at the same rate so that there “appears” to be nothing happening.

  33. solute - is the substance being dissolved • Solvent - is the liquid in which the solute is dissolved • an aqueous solution has water as solvent

  34. Types of Mixtures • Variable combination of 2 or more pure substances. Heterogeneous –visibly separate phases Homogeneous – Same throughout

  35. Mixtures This is a mixture of elements made up of atoms, elements made up of molecules, and compounds. In a mixture, the particles are not joined together. Atom, molecule or compound? atom molecule compound

  36. HOMOGENEOUS MIXTURES Homogenous mixtures look the same throughout but can be separated by physical means (dissolution, centrifuge, gravimetric filtering, etc.). Examples: milk, yogurt

  37. INDICATORS OF A HOMOGENEOUS MIXTURE • Have the same composition throughout • Components are indistinguishable • May or may not scatter light Examples: milk, yogurt, etc.

  38. HETEROGENEOUS MIXTURES Heterogeneous mixtures are composed of large pieces that are easily separated by physical means (ie. density, polarity, metallic properties).

  39. INDICATORS OF A HETEROGENEOUS MIXTURE • Do not have same composition throughout • Components are distinguishable Examples: fruit salad, vegetable soup, etc.

  40. WHAT ARE COLLOIDS? Colloids are solutions. They can be described as a substance trapped inside another substance. They can be identified by their characteristic scattering of light. For example: air trapped inside the fat molecules in whipped cream.

  41. TYNDALL EFFECT

  42. Intensive and Extensive Properties • Physical and chemical properties may be intensive or extensive.

  43. What are intensive properties? • Intensive properties such as density, color, and boiling point do not depend on the size of the sample of matter and can be used to identify substances.

  44. What are extensive properties? • Extensive properties such as mass and volume do depend on the quantity of the sample.

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