MATTER AND PROPERTIES

1. MATTER AND PROPERTIES Unit 3 Chemistry Langley

2. WHAT IS MATTER • Matter • Anything that has mass and occupies space • Anything that has mass and volume • 6 Phases of Matter • Bose-Einstein Condensates • Solid • Amorphous Solid • Liquid • Gas • Plasma Chem4kids.com

3. SOLID • A form of matter that has definite shape and volume • Particles are packed tightly together, in an orderly/rigid arrangement (crystalline) • Shape of a solid does not depend on the shape of the container (difficult to squeeze solid into a smaller volume), not easily compressed • Particles expand when heated • When shattered, fragments have same surface angles as original solid

4. AMORPHOUS SOLID • Lacks an ordered internal structure • Random arrangement of atoms • Definite volume • Can be molded into different shapes • Rubber, plastic, asphalt, glass • When shattered, fragments have irregular angles and jagged edges

5. LIQUID • Form of matter that has an indefinite shape (flows), but has a definite volume • Takes the shape of its container (due to the particles being free to flow from one location to another) • Volume of a liquid does not change has its shape changes • Particles expand slightly when heated • Due to the lack of space between particles, not easily compressed into smaller volumes

6. GAS • Indefinite shape, indefinite volume • Takes the shape and the volume of the container it is in • Can expand to fit any volume • Due to the space between the particles, gases are easily compressed into a smaller volume

7. PLASMA • Just like a gas • Exist only at extremely high temperatures • Does not occur naturally on Earth • Occurs naturally on the sun and stars, and in small quantities, surrounding a lightening bolt • Has enough energy for electrons to be separated from the nucleus • It consists of independently moving electrons and nuclei • Very good magnetic shield • Highest energy of all phases of matter

8. BOSE-EINSTEIN CONDENSATES • First predicted as a consequence of quantum mechanics by Einstein in 1925 • Produced in a lab in 1995 by Cornell and Wieman • Formed by a system of bosons confined in an external potential and cooled temperature (very near absolute zero) • Exists at extremely low temperatures, currently only created in a lab setting • Slowing of atomic movement • Lowest energy of all the forms of matter

9. PHASES OF MATTER LIQUID PLASMA GAS SOLID

10. Pure Substances Matter that has a uniform and definite composition A substance that cannot be broken down further Element Compound Mixture Physical blend of two or more substances that are not chemically combined Blend of two or more kinds of matter Homogeneous Heterogeneous 2 TYPES OF MATTER

11. PROPERTIES • Physical Properties • Any characteristic you can observe without changing the substance that make up the material • Color, size, state of matter, measurements, odor • Intensive or Extensive • Chemical Properties • Any characteristic of a substance that identifies how it reacts with other substances • Sodium reacts with water to produce a flame

12. PROPERTIES (cont.) • Extensive Properties • Property that depends on the amount of matter present, property changes with different amounts • Mass, volume, area • Intensive Properties • Properties that do not depend on the amount of matter present, depends on the type of matter present • Every sample of a given substance has identical intensive properties because every sample has the same composition • Density, Color, Hardness

13. CHANGES • Physical Change • Changes the outward appearance of a substance but does not change the actual substance/chemical • Classified as reversible or irreversible • All phase changes are physical changes • Chemical Change • Changes that produce matter with a different composition that the original matter • Mixing of two or more chemicals together to create a new one • 4 signs of a chemical change: gives off a gas, gives off a precipitate, absorbs or releases heat, color change

14. Endothermic Reactants absorb energy to create a new product Exothermic Reactants release energy to make a new product ENERGY CHANGES

15. Element Simplest form of matter that has a unique set of properties Cannot be broken down into simpler substances by chemical means Composed of only one kind of atom (hydrogen is only made of hydrogen atoms) Simplest form of matter than can exist at normal conditions Compound Substance that contains two or more elements chemically combined in a fixed proportion Salt = sodium atoms and chlorine atoms chemically combined H2 = hydrogen atoms chemically combined Can be broken down by chemical reactions Salt can be broken down into sodium and chlorine atoms when exposed to an electric shock 2 TYPES OF SUBSTANCES

16. Homogeneous Mixture that is uniform in composition Components are evenly distributed and not easily distinguished Individual parts cannot be seen (coffee) All solutions and alloys Heterogeneous Mixture that is not uniform in composition Components are not evenly distributed throughout the mixture Individual parts can be seen (pizza) Suspensions and colloids 2 TYPES OF MIXTURES

17. Solution Has 2 parts: solute (what you want to dissolve) and solvent (what does the dissolving) Kool-Aid: powder and sugar = solute and the water = the solvent 3 types: saturated, unsaturated, and supersaturated Alloy Combining one or more metals to maximize the benefits of each 14 Karat gold: gold + silver = shine of gold and the strength of silver HOMOGENEOUS MIXTURES

18. Suspension Mixture where the particles are so large they settle to the bottom unless constantly stirred Example: When you add sugar to cold tea Colloid Mixture where the particles are average size and do not dissolve and do not settle to the bottom as they remain “stuck” in the middle of the liquid Tyndall Effect is used to tell the difference between a solution and a colloid Scattering of light by particles which causes a beam of light to become visible Example: glue, milk, smoke, whipped cream, mayo, fog, egg, paint HETEROGENEOUS MIXTURES

19. PROPERTIES OF MIXTURES • Solutions • 2 parts: solute and solvent • Solute dissolves completely in solvent • Cannot separate solute from solvent • Saturated, unsaturated, supersaturated • Colloids • Cloudy appearance • Particles are intermediate in size so they will not settle out and will not dissolve • Filter will not separate particles • Emulsion is a specific type of colloid, where a liquid gets stuck in a solid

20. PROPERTIES OF MIXTURES (cont.) • Suspension • Cloudy appearance • Large particles • Particles “suspended” in the liquid • Particles eventually settle to the bottom unless there is constant stirring • Particles can be separated by a filter

21. CLASSIFICATION OF MIXTURES • Electrolytes • When a mixture is able to conduct an electric current • Nonelectrolytes • When a mixture is not able to conduct an electric current

22. WAYS TO SEPARATE A MIXTURE • Filtration • Mixture passes through filter paper and only traps large particles • Decanting • Solid and liquid are mixed together and parts of the solid dissolves, but most go to the bottom; liquid off the top of the solid is poured off

23. WAYS TO SEPARATE A MIXTURE (cont.) • Chromatography • Used to separate dyes or pigments • Based off on the fact that different dyes move at different speeds up chromatography paper • Centrifuge • Place a test tube filled with a mixture into a machine • Machine spins rapidly and pushes solids to the bottoms

24. WAYS TO SEPARATE A MIXTURE (cont.) • Distillation • Based off the fact that each substance has its own characteristic boiling point • To distill water, heat mixture up to 100°C, trap the vapor that comes off at that temperature. Cool the vapor back to a liquid, you have pure water

25. SOLUBILITY • 4 factors that affect the rate of dissolving • Surface area • Increase surface area = longer time to dissolve • Agitation • Stirring/Shaking up a solution speeds up the rate of dissolving • Heat • Higher the temperature, faster the particles move and therefore faster they dissolve • Pressure • Increase in pressure increases solubility of gases

26. SOLUBILITY (cont.) • Like dissolves like • Bases dissolve bases • Acids dissolve acids • Miscible liquids are liquids that freely dissolve one another • Immiscible are solutes and solvents that will not dissolve one another (Oil and water)

27. 3 TYPES OF SOLUTIONS • Unsaturated Solution • Solution contains less than the maximum amount of solute • Can still add more solute that can be dissolved • Saturated Solution • Solution contains the maximum amount of solute • If you add more solute, it will not dissolve, it will fall to the bottom

28. 3 TYPES OF SOLUTION (cont.) • Supersaturated Solution • Solution contains more than the maximum amount of solute • Large amounts of solute fall to the bottom

29. PROPERTIES OF ELEMENTS AND THE PERIODIC TABLE • Elements are pure substances • Some symbols come from the Latin name, some are made up by scientist who discovers element • Periodic table: • All known elements are organized onto periodic table • Vertical columns – groups/families • Horizontal rows – periods

30. PROPERTIES OF ELEMENTS AND THE PERIODIC TABLE (cont.) • Groups of Elements: • Metals • Good conductors of heat and electricity • Malleable – hammered into sheets • Ductile – drawn into wires • High tensile strength – resist breaking • Luster – high shine • Tend to be positive • Nonmetals • Poor conductors of heat and electricity • Many are gases • Form brittle solids – break easily • Tend to be negative

31. PROPERTIES OF ELEMENTS AND THE PERIODIC TABLE (cont.) • Metalloids • On the zigzag line • B, Si, Ge, As, Sb, Te, Po, At • Semi conductors • Noble gases • Group 18 • Un-reactive