1. Physical and Chemical Changes Pure Substances Mixtures States of Matter

2. Everything that has mass and volume is called matter.

3. All matter, regardless of state, undergoes physical and chemical changes. These changes can be microscopic or macroscopic.

5. A physical change occurs when the substance changes state but does not change its chemical composition. Examples: water freezing, cutting a piece of wood, glass shattering. Explanation: The form or appearance has changed, but the properties of that substance are the same

6. Melting point Boiling point Vapor pressure Color State of matter Density Electrical conductivity Solubility Adsorption to a surface Hardness

7. A chemical change occurs when a substance changes into something new. Many common signs of a chemical change can be seen: bubbling, precipitate forms, heat or light is given off.

8. Reaction with acids Reaction with bases (alkalis) Reaction with oxygen (combustion) Ability to act as oxidizing agent Ability to act as reducing agent Reaction with other elements Decomposition into simpler substances Corrosion

9. Physical and chemical properties may be intensive or extensive.

10. 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.

11. Extensive properties such as mass and volume do depend on the quantity of the sample.

12. Physical properties are those that we can determine without changing the identity of the substance we are studying.

13. The physical properties of sodium metal can be observed or measured. It is a soft, lustrous, silver-colored metal with a relatively low melting point and low density. Hardness, color, melting point and density are all physical properties.

14. Chemical properties describe the way a substance can change or react to form other substances. These properties, then, must be determined using a process that changes the identity of the substance of interest.

15. One of the chemical properties of alkali metals such as sodium and potassium is that they react with water. To determine this, we would have to combine an alkali metal with water and observe what happens. In other words, we have to define chemical properties of a substance by the chemical changes it undergoes.

18. Separation Techniques - Deal with the separation of mixtures to enhance purity of substances Are important to because most substances are needed in their pure state.

20. Some Types of Separation Techniques Filtration Chromatography Distillation

21. Filtration This is a technique used to separate mixtures of an insoluble solid and a liquid.

22. Examples of Mixtures You Can Separate Using Filtration Sand and water Broken glass and water Chalk suspensions and water

23. Chromatography Is the separation technique used to separate soluble substances using a media and a solvent. It is mostly applied in identifying mixtures that are coloured or pigments.

24. Types of Chromatography Radial chromatography Ascending chromatography Descending chromatography Gas chromatography

25. Radial Chromatography In this type of chromatography, as the pigment separates, the different colours move outwards.

26. Radial Chromatogram

27. Ascending Chromatography The solvent moves upwards on the separating media \

28. Descending Chromatography The solvent moves downwards on the separating media.

29. Gas Chromatography

30. Chromatograph

31. Distillation This is the separation technique where two miscible liquids are separated. It is made possible due to the fact that each liquid has its unique boiling point.

32. Types of Distillation Simple distillation Fractional distillation

34. Simple Distillation This is a technique used to separate a mixture of a soluble substance and a solvent. E.g salt and water

35. Fractional distillation This is the technique used to separate a mixture of two miscible liquids with different boiling points. E.g water and ethanol The boiling point for water is 100 while for ethanol it is 78.

36. Fractional Distillation Demonstration

37. Questions What is a mixture? Give three ways of separating a mixture. What kind of mixtures can you separate using the filtration method? Give an example of a mixture you can separate using the fractional distillation method.

38. Answers It is a substance made up of two or more substances which are physically combined. Filtration, Chromatography and Distillation. Mixtures of an insoluble substance and a liquid. Ethanol and water.

39. Substances can be identified as either an element, compound, or a mixture.

40. Classifying Matter

41. Fixed composition Cannot be separated into simpler substances by physical methods (physical changes) Can only be changed in identity and properties by chemical methods Properties do not vary

42. Compounds Can be decomposed into simpler substances by chemical changes, always in a definite ratio Elements Cannot be decomposed into simpler substances by chemical changes

43. Mixtures are two or more substances that are NOT chemically combined. Mixtures do not:  Have constant boiling points  Have constant melting points

44. Variable composition Components retain their characteristic properties May be separated into pure substances by physical methods Mixtures of different compositions may have widely different properties

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

46. Have the same composition throughout Components are indistinguishable May or may not scatter light Examples: milk, yogurt, etc.

47. Solutions are homogenous mixtures that do not scatter light. These mixtures are created when something is completely dissolved in pure water. Therefore, they are easily separated by distillation or evaporation. Examples: sugar water, salt water

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

49. Do not have same composition throughout Components are distinguishable Examples: fruit salad, vegetable soup, etc.

50. 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.

51. There is no observable change in the quantity of matter during a chemical reaction or a physical change. In other words, matter cannot be created nor destroyed. It is just converted from one form to another

52. Solids Liquids Gases Plasma Others (And how the Kinetic Molecular Theory affects each)

54. Have a definite shape Have a definite volume Molecules are held close together and there is very little movement between them. Kinetic Molecular Theory

55. Have an indefinite shape Have a definite volume Kinetic Molecular Theory: Atoms and molecules have more space between them than a solid does, but less than a gas (ie. It is more “fluid”.)

56. Have an indefinite shape Have an indefinite volume Kinetic Molecular Theory: Molecules are moving in random patterns with varying amounts of distance between the particles.

57. At 100°C, water becomes water vapor, a gas. Molecules can move randomly over large distances. Below 0°C, water solidifies to become ice. In the solid state, water molecules are held together in a rigid structure. Between 0°C and 100 °C, water is a liquid. In the liquid state, water molecules are close together, but can move about freely.

58. Changing states requires energy in either the form of heat. Changing states may also be due to the change in pressure in a system. Heat of formation, H f. Heat of vaporization, H v

59. Plasma is by far the most common form of matter. Plasma in the stars and in the tenuous space between them makes up over 99% of the visible universe and perhaps most of that which is not visible.

60. On earth we live upon an island of "ordinary" matter. The different states of matter generally found on earth are solid, liquid, and gas. We have learned to work, play, and rest using these familiar states of matter. Sir William Crookes, an English physicist, identified a fourth state of matter, now called plasma, in 1879.