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Chapter 2

Chapter 2. Matter and Change. What is Matter?. Matter is anything that takes up space and has mass. Mass is the amount of matter in an object. Mass is resistance to change in motion along a smooth and level surface. Examples. Properties. Words that describe matter (adjectives)

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Chapter 2

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  1. Chapter 2 Matter and Change

  2. What is Matter? • Matter is anything that takes up space and has mass. • Mass is the amount of matter in an object. • Mass is resistance to change in motion along a smooth and level surface. • Examples

  3. Properties • Words that describe matter (adjectives) • Physical Properties- a property that can be observed and measured without changing the substance. • Chemical Properties- a property that can only be observed by changing the type of substance.

  4. Study of how matter reacts • Chemical Rxns- chemicals interacting and rearranging to form new substances Reactant(s)  Product(s) Sometimes reactions need energy added to them to get going, called activation energy Evidence of a Chemical Reaction • Color change • Formation of a precipitate • Production of Gas • Temperature change- either increase (exothermic) or decrease (endothermic) • Production of Light

  5. Characteristics of Matter Properties - Characteristics that help identify matter Physical Properties: Can be measured without changing its chemical composition. Also can be changed back to original form. Chemical Properties: Can be observed only when substances interact with each other. Changes:phy – does not affect composition chem- produces new substances

  6. Properties • Words that describe matter (adjectives) • Extensive Properties- only depends on the amount of matter • Intensive Properties- only depends on the type of matter, not the amount • Used to identify a substance

  7. Physical Properties Color Shape Hardness Texture Tearing Grinding Mass Volume Weight Length Density Boiling pt./melting pt. Conductivity Taste Odor Malleability Ductility Elasticity Tensile strength Viscosity Luster Cooking

  8. Chemical Properties Combustion/Flammability Corrosion (rust) Respiration Photosynthesis Decomposition Cooking

  9. States of matter • Solid- mater that can not flow and has definite volume. • Liquid- definite volume but takes the shape of its container (flows). • Gas- a substance without definite volume or shape and can flow. • Vapor- a substance that is currently a gas but normally is a liquid or solid at room temperature.

  10. States of Matter Definite Volume? Definite Shape? Temp. increase Com-pressible? Small Expans. Solid YES YES NO Small Expans. Liquid NO NO YES Large Expans. Gas NO NO YES

  11. Condense Freeze Evaporate Melt Gas Liquid Solid

  12. Phase Changes- Energy is involved either in or out (endothermic or exothermic) Solid  Liquid Melting Liquid  Solid Freezing Liquid  Gas Vaporization (forced) Evaporation (natural Gas Liquid Condensation Solid  Gas Sublimation Gas  Solid Deposition

  13. States of Matter • There are more • Plasma • high temperature low pressure • electrons separate from nucleus • Most common in the universe • More at very low temp • Bose- Einstein condensate • Quantum superfluids

  14. Another Way to Change States • Pressure • For some substances it will turn solids to liquids • For others it will turn liquids to solids • Silly putty • Will turn gas to liquid- • Compressor in refrigerator and AC

  15. Types of Matter • Substance- a particular kind of matter - pure • Mixture- more than one kind of matter

  16. Matter breakdown matter / \ pure substances mixtures l / \ compounds heterogeneous homogeneous l l / \ elements suspension solution colloid / l \ saturated unsat.supersat.

  17. Mixtures • Made up of two substances. • Variable composition. • Heterogeneous- mixture is not the same from place to place. • Chocolate chip cookie, gravel, soil. • Homogeneous- same composition throughout. • Kool-aid, air. • Every part keeps its properties.

  18. Phases • A part of a sample with uniform composition, therefore uniform properties • Homogeneous- 1 phase • Heterogeneous – more than 1

  19. Solutions • Homogeneous mixture • Mixed molecule by molecule • Can occur between any state of matter. • Solid in liquid- Kool-aid • Liquid in liquid- antifreeze • Gas in gas- air • Solid in solid - brass • Liquid in gas- water vapor

  20. Solutions • Like all mixtures, they keep the properties of the components. • Can be separated by physical means • Not easily separated- can be separated without creating anything new.

  21. Substances • Elements- simplest kind of matter • Cannot be broken down into simpler • All one kind of atom. • Compounds are substances that can be broken down by chemical methods • When they are broken down, the pieces have completely different properties than the compound. Salt • Made of molecules- two or more atoms stuck together

  22. Compound or Mixture Compound Mixture One kind of piece- Molecules More than one kind - Molecule or atoms Making is a chemical change Making is a physical change Only one kind Variable composition

  23. Element Compound Mixture Which is it?

  24. Chemical Reactions • Another name for chemical change • When one or more substances are changed into new substances. • Reactants- stuff you start with • Products- What you make • NEW PROPERTIES • Because each substance has its own properties

  25. Indications of a chemical reaction • Energy absorbed or released • Color change • Odor change • Precipitate- solid that separates from solution • Not easily reversed • Only clues not certainty

  26. Chemical symbols • There are 116 elements • Each has a 1 or two letter symbol • First letter always capitalized second never • Don’t need to memorize • Some from Latin or other languages

  27. Chemical symbols • Used to write chemical formulas • Subscripts tell us how many of each atom • H2O • C3H8 • HBrO3

  28. Conservation of Mass • Mass can not be created or destroyed in ordinary (not nuclear) changes. • All the mass can be accounted for. • Mass at the start = mass at end

  29. Separating mixtures • Only a physical change- no new matter • Filtration- separate solids from liquids with a barrier • Distillation- separate because of different boiling points • Heat mixture • Catch vapor in cooled area • Chromatography- different substances are attracted to paper or gel, so move at different speeds

  30. Chromatography

  31. Energy • The ability to do work. • Work - cause a change or move an object. • Many types- all can be changed into the other.

  32. Types of energy • Potential- stored energy • Kinetic Energy- energy something has because its moving • Heat- the energy that moves because of a temperature difference. • Chemical energy- energy released or absorbed in a chemical change. • Electrical energy - energy of moving charges

  33. Types of Energy • Radiant Energy- energy that can travel through empty space (light, UV, infrared, radio) • Nuclear Energy – Energy from changing the nucleus of atoms • All types of energy can be converted into others. • If you trace the source far enough back, you will end up at nuclear energy.

  34. Conservation of Energy • Energy can be neither created or destroyed in ordinary changes (not nuclear), it can only change form. • Its not just a good idea, its the law.

  35. What about nuclear? • E = mc2 • energy = mass x (speed of light)2 • speed of light = 3 x 108 • A little mass can make a lot of energy • Law of Conservation of Mass - Energy the total of the mass and energy remains the same in any change

  36. Density Lab For each of the cubes and each of the cylinders record the mass then, calculate volume using two techniques: A) using measured units Block V= l x w x h Cylinder V= π x r2 x h B) using volume displacement, place them in the appropriate graduated cylinder and then measure. Calculate Densities Then use volume displacement to calculate densities of the five odd items. Question: Which of the methods for measuring volume is more accurate and why?

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