1. AP Chemistry Chapter 1A Matter

2. Chemistry Study of atoms and molecules and their transformations.

3. Chemists

4. Haber Process process of producing ammonia (NH 3 ) for fertilizers, etc. (Approx. 17 million tons produced annually in United States.)

5. Nitrogen Cycle Cycle where Nitrogen is turned into useable forms by Plants  animals  soil  atmosphere 

7. Legumes Ex: beans. Plants that give off extra nitrogen (N 2 ) into soil.

8. Hypothesis tentative explanation or prediction of experimental observations.

9. Quantitative describes numerical data.

10. Qualitative describes information, details.

11. Law concise verbal or mathematical statement of a relation that seems always to be the same under the same condition.

12. Scientific Method a series of steps used to observe and test theories by experimentation.

13. Steps 1. State the Problem 2. Observe (5 senses) 3. Form a hypothesis 4. Experiment 5. Record and Analysis 6. Conclusion (Summing it all up)

14. Theory unifying principle that explains a body of facts and the laws based on them.

15. James Watson Francis Crick Maurice Wilkins 1962 Novel Prize in medicine and physiology for their work on structure of DNA. They recognized the need to know the structure of various elements and their role in the DNA molecule. James Francis Maurice

16. Alexander Fleming (1881-1955) discovered penicillin. (1928)

17. Bernard Courtois (1777-1838) discovered iodine.

18. Chemistry & Matter We can explore the MACROSCOPIC world — what we can see —We can explore the MACROSCOPIC world — what we can see — to understand the PARTICULATE worlds we cannot see.to understand the PARTICULATE worlds we cannot see. We write SYMBOLS to describe these worlds.We write SYMBOLS to describe these worlds.

19. A Chemist’s View of Matter

20. A Chemist’s View of Water H 2 O (gas, liquid, solid) MacroscopicMacroscopic SymbolicSymbolic ParticulateParticulate

21. A Chemist’s View 2 H 2 (g) + O 2 (g) --> 2 H 2 O(g) MacroscopicMacroscopic SymbolicSymbolic ParticulateParticulate

22. Macroscopic level tangible, visible.

23. Microscopic level atoms, ions, and molecules.

24. Symbolic level formulas and equations.

25. Matter anything that occupies space and has mass.

26. States of Matter a. solid - fixed shape and volume b. liquid - fixed volume that takes the shape of the container. c. gas - volume and shape of container varies with change in temperature and / or pressure.

28. States of Matter

29. Kinetic Energy energy of motion. The ball has kinetic energy. The roller coaster has kinetic energy.

30. Potential Energy Stored energy

31. Types of mixtures Heterogeneous

32. Heterogeneous Mixture- mixture in which uneven texture of the material can be detected. Ex: Salad, stew, blood, pizza, and whole milk.

33. Types of Mixtues cont. Homogeneous

34. Types of Mixtures cont. Homogeneous Mixtures mixture completely uniform at macroscopic level and consists of one or more substance in the same phase. Ex: Gold and jelly.

35. Solutions has properties of homogenous mixture. Appear the same everywhere in the sample. Ex: Oxygen (O 2 ), gasoline, and soft drinks.

36. Pure substance has unique properties that can be recognized and cannot be separated into two different species by any physical technique.

37. Purified When a mixture is separated into its pure components.

38. Periodic Table table of the elements that is organized by atomic numbers. Symbol are used to represent the elements. Symbols are always either a capital letter only or a capital letter followed by a lower case letter. Many of the earlier elements were named with a Greek or Latin name.

39. Periodic Table http://www.webelements.com/