1. Chapter Two Part 1 Properties of Matter Classifying Matter

2. The Nature of Matter The Nature of Matter You can observe matter easily with your senses... rocks, trees, bicycles, air... Basically everything and anything! Matter is anything that takes up space and has mass. Examples of Matter: The word matter comes from the Latin word materia, meaning “material” or “stuff” First we need to ask... The only thing that wouldn’t be matter would be energy (sunlight, heat, electricity). - no mass or volume so they can’t be matter! What is matter?

3. Elements, Molecules, and Compounds Elements and compounds make up all the different kinds of matter in the universe. Elements are the simplest form of matter C Cannot be broken down into simpler substances. E Each element is made of atoms of the same type. ach has a unique set of physical and chemical properties. 1 117 known elements in the universe. A Approximately 92 are found naturally on Earth. Examples of Elements: gold gold silver silver oxygen oxygen hydrogen hydrogen aluminum aluminum nitrogen nitrogen tin tin calcium calcium Six elements make up 99% of all living matter! Sulfur Sulfur Potassium Potassium Oxygen Oxygen Nitrogen Nitrogen Carbon Carbon Hydrogen Hydrogen

4. Compounds are two or more elements combined chemically together. Properties are different from the properties of the elements that make them up. Properties are different from the properties of the elements that make them up. Elements in a compound have a fixed ratio. Elements in a compound have a fixed ratio. Example: Na (Sodium) Soft metal explodes in H 2 0 + Cl (chlorine) Poisonous greenish gas =Salt Most matter in the universe is in the form of compounds! Compounds, Molecules, and Elements H (hydrogen) Explosive gas + O 2 (oxygen) Explosive gas =Water

5. Molecules, Elements, and Compounds When two or more atoms combine, they form a molecule. Most molecules are made of two or more atoms Most molecules are made of two or more atoms A molecule is the smallest particle of a substance with the same properties of thesubstance. A molecule is the smallest particle of a substance with the same properties of thesubstance. NOTE:Compounds are different than molecules because compound is used to describe the substance in general, while molecule describes the smallest particle of the substance. NOTE: Compounds are different than molecules because compound is used to describe the substance in general, while molecule describes the smallest particle of the substance.

6. Mixtures, Solutions, and Suspensions A mixture is a combination of two or more substances NOT combined chemically. May be a mixture of both elements and compounds May be a mixture of both elements and compounds Substances keep their unique properties and can be separated by physical means. Substances keep their unique properties and can be separated by physical means.

7. There are two types of mixtures... Homogeneous – the parts (substances) are evenly distributed. It is difficult to tell one substance from another. Heterogeneous – the parts of the mixture are noticeably different from one another. Mixtures, Solutions, and Suspensions

8. A solution is a mixture that looks like a single substance and has the same properties throughout. solution Solute ~ The substance that dissolves in a solution. Solvent ~ The substance into which the solute dissolves. Solutions, and Suspensions and Colloids

9. A colloid is a mixture that contains both small particles in solution and larger particles in suspension. Colloids do not separate into layers. Colloids do not separate into layers. Colloids, like suspensions scatter light. Colloids, like suspensions scatter light. Milk is an example of a colloid. In a suspension components are dispersed, but large enough to see and settle out.

10. Chapter Two Part 2 Properties of Matter Physical Properties

11. Physical property is a property that can be observed without changing the identity of the substance. Physical Properties Examples: viscosity viscosity conductivity conductivity malleability malleability hardness hardness magnetism magnetism melting point melting point boiling point boiling point density density color color

12. Examples of Physical Properties Viscosity of a substance is its resistance to flow. Examples: water = low viscosity Examples: water = low viscosity honey = high viscosity Conductivity is a material’s ability to allow heat to flow. Examples: metal = high conductivity wood = poor conductivity Examples: metal = high conductivity wood = poor conductivity

13. Examples of Physical Properties Malleability of a substance is its ability to be hammered into a thin sheet Melting and Boiling points are the temperatures at which a solid becomes a liquid and a liquid becomes a gas. Density of a substance is the ratio of its mass compared to its volume.

14. Next Time...

15. Physical Properties to separate mixtures Two common separation methods: Filtration – process that separates materials based on the size of their particles. Distillation – process that separates the substances in a solution based on their boiling points.

16. Physical Change A change in the appearance, without changing the composition of the material. Can be reversible, or irreversible Can be reversible, or irreversible Substance may seem different, but the way the atoms link up is the same. Substance may seem different, but the way the atoms link up is the same. It is a physical change if... It changes shape or size It changes shape or size Or the substance changes phase. Or the substance changes phase. It dissolves. It dissolves.

17. Chapter Two Part 3 Properties of Matter Chemical Properties

18. Chemical property is any ability to produce a change in the composition of matter. Chemical Properties flammability reactivity Material’s ability to burn in the presence of oxygen. How readily a substance combines chemically with other substances. Examples of chemical properties...

19. Chemical Changes Chemical changes occur when a substance reacts and forms one or more new substances. Formation of a precipitate. A change in color. Production of a gas. You know a chemical change has occurred when...

20. physical What kind of change is it?

21. chemical

22. physical

23. physical

24. chemical

25. physical

26. The 5 Branches of Chemistry InorganicOrganicAnalyticalPhysicalBiochemistry

27. Inorganic Chemistry The study of chemicals that do not contain carbon.

28. Organic Chemistry The study of chemicals that contain carbon. Origin: study of chemicals in living organisms.

29. Organic or Inorganic ? Sulfuric Acid H 2 SO 4 Methane CH 4 Hydrochloric Acid HCl EthaneC 2 H 6

30. Analytical Chemistry Composition of matter. http://besg.group.shef.ac.uk/Facilities/Images/gcms.JPG Ex: Mass Spectrometer Gas Chromatograph

31. Physical Chemistry The study of : The mechanism The mechanism The rate The rate The energy transfer The energy transfer that happens when matter undergoes change.

32. Biochemistry Study of processes that take place in organisms.

33. Science What?Why?How?When?

34. Science and Technology Science  Pure Does not necessarily have an application. Does not necessarily have an application. Technology  Applied Has practical applications in society. Has practical applications in society. Engineering. Engineering.

35. Question: Science or Technology? Studying or forming aspirin in a lab in small scale (small amounts).

36. Producing aspirin tablets so that consumers can use them. Producing aspirin tablets so that consumers can use them. Question: Science or Technology?

37. Example: Discovery of Nylon by Wallace Carothers in 1930’s http://www.chemheritage.org/EducationalServices/nylon/nylon.html http://heritage.dupont.com/touchpoints/tp_1935-2/depth.shtml

38. Microscopic- Macroscopic Micro –(small) Microscopic- objects can be seen with a microscope. Microscopic- objects can be seen with a microscope. Macro-(from afar) Macroscopic- objects are seen without a microscope. Macroscopic- objects are seen without a microscope.

39. Aristotle (Greece, 4 th Century BC) Philosopher who believed that: Philosopher who believed that: There are 4 elements: earth, water, air, fire. Matter is perpetually divisible.

40. Democritus (Greece, 4th Century BC) First atomic theory Atom (indivisible).

41. Alchemists (~300BC-1650 AD) China, India, Arabia, Europe, Egypt Aiming to:  Change common metals to gold.  Develop medicines. Developed lab equipment. Mystical.

42. Antoine Lavoisier (France 1743-1794) Regarded as the Father of Chemistry. Designed equipment. Used observations and measurements. and measurements. Discovered nitrogen.

43. Antoine Lavoisier (cont’d) Discovered the Law of Conservation of Mass: In a chemical reaction mass is conserved. In a chemical reaction mass is conserved.

44. Explained burning as reaction with oxygen. Old theory: release of “phlogiston”. Antoine Lavoisier (cont’d)

45. Question: Does an iron nail gain mass or lose mass when it rusts (a form of burning)?

46. John Dalton (England 1766-1844) Atomic theory

47. Amedeo Avogadro (Italy, 1776-1856) Avogadro’s Number 6.02x10 23 One mole of any substance contains 6.02x10 23 particles.

48. Dmitri Mendeléev (Russia, 1834-1907) First Periodic Table of elements.

49. Part III Math and Chemistry Math- the language of Science

50. Units SI Units – International System Basic Units Basic Units mks mks Length(meter) m Mass (kilogram)kg Time (second)s National Bureau of Standards

51. Solving Word Problems Analyze List knowns and unknowns. List knowns and unknowns. Devise a plan. Devise a plan. Write the math equation to be used. Write the math equation to be used.Calculate If needed, rearrange the equation to solve for the unknown. If needed, rearrange the equation to solve for the unknown. Substitute the knowns with units in the equation and express the answer with units. Substitute the knowns with units in the equation and express the answer with units.Evaluate Is the answer reasonable? Is the answer reasonable?