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Classification of Matter

Classification of Matter. Integrated Physic and Chemistry Fall 2013. CLASSIFICATION OF MATTER. 1. DISTINGUISH BETWEEN MASS AND MATTER. Mass - the quantity of matter in an object- measured in grams Matter - anything that has mass and occupies space - (anything that has mass and volume).

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Classification of Matter

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  1. Classification of Matter Integrated Physic and Chemistry Fall 2013

  2. CLASSIFICATION OF MATTER 1. DISTINGUISH BETWEEN MASS AND MATTER. • Mass - the quantity of matter in an object- measured in grams • Matter - anything that has mass and occupies space- (anything that has mass and volume)

  3. CLASSIFICATION OF MATTER • 2. STATE THE KINETIC THEORY OF MATTER. • - matter is made of tiny particles called atoms • - these atoms are in constant motion • - adding heat makes the atoms move faster and farther apart • - removing heat makes the atoms move slower and closer together

  4. CLASSIFICATION OF MATTER • 3. LIST THE FOUR STATES OF MATTER. • The four states of matter are solid, liquid, gas and plasma. • 4. IDENTIFY MAJOR CHARACTERISTICS OF SOLIDS, LIQUIDS AND GASES.

  5. CLASSIFICATION OF MATTER • 5. STATE THE LAW OF CONSERVATION OF MASS. • Matter cannot be created or destroyed in a chemical or physical change.  • 6. DEFINE AND DESCRIBE PHYSICAL PROPERTIES. • Physical Properties - characteristics which can be observed without changing the chemical composition of the substance • - size, shape, color, smell, density, melting point, freezing point, and boiling point • 7. DEFINE AND DESCRIBE PHYSICAL CHANGES. • Physical change - a change in the appearance or state of a substance but NOT it's chemical make-up • -Examples are the evaporation of water, melting of ice, dissolving of salt into water, and breaking a glass.

  6. CLASSIFICATION OF MATTER • 8. DEFINE AND CALCULATE DENSITY. • Density - a measure of mass per volume • - The formula is D = m v • m = mass (grams) • V = volume (ml or cm3) • D = density (g/ml or g/cm3)

  7. CLASSIFICATION OF MATTER • 9. DEFINE AND DESCRIBE CHEMICAL PROPERTIES • Chemical Properties - those characteristics which depend upon the reaction with another substance • - Examples are iron will rust, wood will burn, milk will sour, and sodium will explode in water (it all depends on what you mix it with). • 10. DEFINE AND DESCRIBE CHEMICAL CHANGES. • Chemical Changes - changes that produce new substances which are chemically different than the original substances • - Examples are burning, rusting, combustion, flammability, rotting, and digestion

  8. CLASSIFICATION OF MATTER • 11. LIST INDICATIONS OF A CHEMICAL CHANGE. • (a) production of a gas • (b) permanent color change • (c) formation of a precipitate • (d) change in energy • (1) endergonic - takes in energy • (2)exergonic - releases energy production of light energy

  9. CLASSIFICATION OF MATTER • 12. DESCRIBE AN ELEMENT. • Element - a pure substance in which all of its atoms are alike - refer to the periodic table of elements • 13. DESCRIBE A COMPOUND. • Compound - a pure substance made of two or more elements that are chemically combined in a definite proportion or ratio- compounds do not usually look or behave like the elements from which they are made • (water, salt, sugar)

  10. CLASSIFICATION OF MATTER • 14. DESCRIBE A MIXTURE. • Mixture - composed of two or more substances, simply mixed together. • - CAN be separated easily by filtration, evaporation, etc... • - substances are NOT chemically combined • Example are this class, tossed salad, and salt water • We will discuss in more detail in the next series of notes.

  11. CLASSIFICATION OF MATTER • 15. DEFINE AND GIVE EXAMPLES OF FLUIDS. • A fluid is any substance that can flow or be poured. • Gases and liquids are fluids. • 16. DEFINE VISCOCITY. • Viscosity is a fluid's resistance to flow. • The higher the viscosity, the slower it pours. (syrup, motor oil) • Temperature affects viscosity

  12. Mixtures Integrated Physic and Chemistry Fall 2013

  13. MIXTURES • 1. A pure substance is either an element or a compound.But a mixture is made up of two or more substances that can be separated by physical means. • 2. There are two types of mixtures. • A heterogeneous mixture differs from point to point. • A homogeneous mixture the same throughout.

  14. MIXTURES • 3. A solution is a homogeneous mixture of two or more substances. A solution consists of a solute and solvent. The solute isdissolved into the solvent. • The solute usually occurs in the smaller amount. • The solvent usually occurs in the larger amount. • Solutions form when particles of the solute spread out evenly in the solvent.

  15. MIXTURES • 4. Water is described as the universal solvent because more substances will dissolve in water than any other known solvent. There is no such thing as a true universal solvent!  • 5. Five physical properties of solutions are: • a. It is homogeneous. (evenly mixed) • b. Liquid solutions appear clear or transparent.(does not mean colorless) • c. Proportions may vary. (weak or strong) • d. The solute will not settle from the solvent. • e. The solute cannot be filtered from the solvent.

  16. MIXTURES • 6. The rate of solution depends upon 3 factors:(how quickly something dissolves) • a. Particle size (Crushing a sugar cube will dissolve it faster). • b. Stirring or shaking the mixture increases the rate of solution. (solid into a liquid - NOT gas into a liquid) • c. Temperature(solids dissolve faster in warmer solvents)

  17. MIXTURES • 7. Solubility is the amount of solute that can be dissolved in a given amount of solvent at a given temperature. Amount of solvent and temperature MUST be controls. • 8.The factors that determine IF something will dissolve. • a. Temperature - Solids dissolve more in warm liquid solvents.Gases dissolve less in warm liquid solvents. • b. Pressure -Increased pressure will cause more solute to stay in the solution (sodas) • c. Nature of the solvent and solute • Organic solvents dissolve organic solutes. Inorganic solvents dissolve inorganic solutes.Water is an exception.

  18. MIXTURES • 9. A solubility curve is a graph showing how much solute is dissolved in a solvent over a range of temperatures.

  19. MIXTURES • 10. The methods of separating mixtures are: • a. Evaporation is removing water from a solution or removing the liquid portion from a mixture without adding heat. • b. Distillation is the separation of two liquids because of a difference in boiling points. • c. Filtration is the removal of an insoluble solid from a liquid mixture. Filtrate is the portion of the mixture that passes through the filter. • Evaporation, distillation and filtration are all physical changes!

  20. MIXTURES • 11. The levels of concentration are unsaturated, saturated, or supersaturated. • An unsaturated solution will hold more solute. • A saturated solution will not dissolve more solute. • A supersaturated solution contains more solute than usual because it was • (a) heated • (b) more solute added and then • (c) cooled back to original temperature. • (dissolving sugar in warm tea, then adding ice)

  21. MIXTURES • 12. The addition of solute particles raises theboiling pointof a solution. (anti-freeze in radiator). The addition of solute particles lowers the freezing pointof a solution.(salt on ice for homemade ice cream or on sidewalks to melt ice).

  22. MIXTURE • 13. A comparison of solutions, colloids and suspensions.

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