1. Unit 1 continued… 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.

3. Types of Matter  Pure Substance - a particular kind of matter - pure  Mixture - more than one kind of matter, not chemically combined

5. What are Pure Substances?  Substances which have a single composition throughout. These can be elements or compounds  The simplest forms of matter are the elements. There are nearly 120 different elements currently known on the earth.  The smallest particles of an element are atoms.  Atoms of an element are unique. For example lead atoms are completely different from gold atoms.

6. Pure 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 Salt –Made of molecules - two or more atoms bonded together

7.  A molecule is the smallest particle of a compound that acts as a unit. Molecules are made of a fixed ratio of atoms.

8. What is a chemical formula?  A chemical formula tells the kind and number of atoms in a molecule.  The formula uses the symbols of the element to identify the elements present and subscripts (lowered numbers beside the symbol) to indicate how many atoms are present.

9. Compound or Mixture CompoundMixture 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 of particle Variable composition

10. Which is it? Element

11. Which is it? Compound

12. Which is it? Mixture

13. 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.  Both physical and chemical properties can be used to help identify a substance

14. Physical Properties Melting Boiling Color

15. Chemical Properties Flammability Reactivity Radioactivity

16. 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  Both intensive and extensive properties can be used to help identify a substance

17. Extensive Properties Mass Volume

18. Intensive Properties Luster Density Color

19. States of matter  Solid - matter 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

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

21. States of Matter Low Kinetic Energy - molecules barely move Moderate Kinetic Energy - molecules move around more than in solids High Kinetic Energy – molecules in rapid, constant motion

22. Solid Liquid Gas Melt Evaporate Condense Freeze

23. States of Matter  There are more than 3…  Plasma –high temperature, low pressure –electrons separate from nucleus –Most common in the universe  More at very low temp –Bose- Einstein condensate –Quantum superfluids

24. 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 Silly PuttySilly Putty  Will also turn gas to liquid- –Compressor in refrigerator and AC

25. Changes  Physical Change - a change that changes appearances, without changing the composition. –Examples »cutting hair, melting ice

26. Changes  Chemical Change - a change where a new form of matter is formed. –Also called chemical reaction. –Examples »Bleaching fabric, burning paper –Not phase changes »Ice is still water.

27. 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.

28. What are homogeneous mixtures? Solutions Solutions are homogeneous mixtures. Solution particles are very small and composed of molecules, atoms, or ions. Colloids Colloids are homogeneous mixtures. Colloid particles are larger than solution particles, but do not settle as suspensions do. Examples of colloids are fog, mayonnaise, jell-o, whipped cream.

29. heterogeneous mixtures What are heterogeneous mixtures? Heterogeneous mixtures Heterogeneous mixtures (suspensions) are made of larger particles than that of homogeneous mixtures. These particles remain suspended temporarily and will eventually settle or separate. Examples are chocolate milk, orange juice, muddy water.

30. What are liquid mixtures?  Liquids which evenly mix are said to be miscible. Gasoline, antifreeze and water.  Liquids which do not mix are said to be immiscible. Oil and water; oil and vinegar. Can gases mix with liquids? How do fish breathe? What are carbonated soft drinks?

31. Phases  A part of a sample with uniform composition, therefore uniform properties  Homogeneous mixtures have 1 phase  Heterogeneous mixtures have more than 1 phase

32. Separating mixtures Only a physical change - no new matter formed  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

33. Chromatography

34. physical changes How can physical changes be used to separate mixtures? distillation Impurities mixed with water can be separated by distillation. distillation What is distillation? Distillation Distillation is a process of separating parts of a mixture by differences in boiling points.

35. Solutions  Type of 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

36. Solutions  Like all mixtures, they keep the properties of the components.  Can be separated by physical means –Not easily separated, but can be separated without creating anything new.

37. 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  Products have NEW PROPERTIES

38. Indications of a chemical reaction  Energy absorbed or released  Color change  Odor change  Precipitate - solid that separates from solution Precipitate  Action is not easily reversed  These are only clues, not certainty

39. Chemical symbols  There are 116 elements  Each has a 1 or two letter symbol – often first letter (or first two letters) of element name  First letter always capitalized, second never capitalized  Some are from other languages so symbol may not always match name (Ag = Silver)

40. Chemical symbols  Used to write chemical formulas  Subscripts tell us how many of each atom –H2O–H2O–H2O–H2O –C3H8–C3H8–C3H8–C3H8 –HBrO 3

41. 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

42. The Law of Conservation of Matter  Matter cannot be created or destroyed.

43. Energy  The ability to do work. –Work - cause a change or move an object.

44. 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

45. 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.

46. Conservation of Energy  Energy can be neither created nor destroyed in ordinary changes (not nuclear), it can only change form.  Its not just a good idea, its the law.

47. What about nuclear reactions?  E = mc 2 –energy = mass x (speed of light) 2 –speed of light = 3 x 10 8 m/s  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 chemical change