1. Essentials of Human Anatomy & Physiology Copyright © 2003 Pearson Education, Inc. publishing as Benjamin Cummings A Refresher Seventh Edition Elaine N. Marieb Chapter 2 Basic Chemistry Lecture Slides in PowerPoint by Jerry L. Cook Modified by Marcia Sloan

2. Energy Slide 2.1 Copyright © 2003 Pearson Education, Inc. publishing as Benjamin Cummings The ability to do work; to act on matter Kinetic vs Potential Types Chemical Electrical Mechanical Radiant Energy Conversion

3. Matter Occupies space (volume) and has mass (weight) Three states Gas Liquid Solid

4. Composition of Matter Slide 2.2 Copyright © 2003 Pearson Education, Inc. publishing as Benjamin Cummings Elements Fundamental units of matter 96% of the body is made from four elements Carbon (C) Oxygen (O) Hydrogen (H) Nitrogen (N) Atoms Building blocks of elements

6. Atomic Structure Slide 2.3 Copyright © 2003 Pearson Education, Inc. publishing as Benjamin Cummings Nucleus Protons (p + ) Neutrons (n 0 ) Outside of nucleus Electrons (e - ) Figure 2.1

7. Identifying Elements Slide 2.4 Copyright © 2003 Pearson Education, Inc. publishing as Benjamin Cummings Atomic number Equal to the number of protons that the atoms contain Atomic mass number Sum of the protons and neutrons

8. Isotopes Slide 2.5 Copyright © 2003 Pearson Education, Inc. publishing as Benjamin Cummings Have the same number of protons Vary in number of neutrons

9. Atomic Weight Slide 2.5 Copyright © 2003 Pearson Education, Inc. publishing as Benjamin Cummings Atomic weight Close to mass number of most abundant isotope Atomic weight reflects natural isotope variation

10. Radioactivity Slide 2.6 Copyright © 2003 Pearson Education, Inc. publishing as Benjamin Cummings Radioisotope Heavy isotope Tends to be unstable Decomposes to more stable isotope Radioactivity Process of spontaneous atomic decay

11. Molecules and Compounds Slide 2.7 Copyright © 2003 Pearson Education, Inc. publishing as Benjamin Cummings Molecule – two or more atoms combined covalently Compound – two or more different atoms combined chemically

12. Mixtures Definition – substance composed of 2 or more substances NOT chemically bonded together. No properties of original substances are lost Can be separated by physical means Evaporation, filtration, distillation, centrifugation, etc.

13. Types of Mixtures Solutions Solvent + Solute Usually transparent Examples IV solutions Koolaid, tea, salt water

14. Types of Mixtures Colloids Solute particles are huge, but they form a mesh that does not settle out Tindel effect Sols (liquidy) and Gels (solidy) Examples Jello, cytoplasm

15. Types of Mixtures Suspensions Will settle out because solute has much larger particles than solvent Examples Sand in water, blood

16. Chemical Reactions Slide 2.8 Copyright © 2003 Pearson Education, Inc. publishing as Benjamin Cummings The creation and/or destruction of molecules The making and/or breaking of chemical bonds forming new combinations of the same atoms Metabolism All the chemical reactions in the body Anabolism – builds larger molecules Catabolism – breaks down molecules

17. Chemical Reactions Slide 2.8 Copyright © 2003 Pearson Education, Inc. publishing as Benjamin Cummings Metabolism All the chemical reactions in the body Anabolism Builds larger molecules Ex: Combining many amino acids to form protein Catabolism Breaks down molecules Ex: Digesting starches into sugars

18. Electrons and Bonding Slide 2.9 Copyright © 2003 Pearson Education, Inc. publishing as Benjamin Cummings Electrons occupy energy levels called electron shells Electrons closest to the nucleus are most strongly attracted Each shell has distinct properties Number of electrons has an upper limit Shells closest to nucleus fill first

19. Electrons and Bonding Slide 2.10 Copyright © 2003 Pearson Education, Inc. publishing as Benjamin Cummings Bonding involves interactions between electrons in the outer shell (valence shell) Full valence shells do not form bonds Noble Gases

20. Inert Elements Slide 2.11 Copyright © 2003 Pearson Education, Inc. publishing as Benjamin Cummings Have complete valence shells and are stable Rule of 8s Shell 1 has 2 electrons Shell 2 has 8 electrons Shell 3 has 8 electrons Figure 2.4a

21. Reactive Elements Slide 2.12 Copyright © 2003 Pearson Education, Inc. publishing as Benjamin Cummings Valence shells are not full and are unstable Tend to gain, lose, or share electrons Allows for bond formation, which produces stable valence Figure 2.4b

22. Chemical Bonds Slide 2.14 Copyright © 2003 Pearson Education, Inc. publishing as Benjamin Cummings Covalent Bonds Atoms become stable through shared electrons Single covalent bonds share one electron Double covalent bonds share two electrons Figure 2.6c

23. Examples of Covalent Bonds Slide 2.15 Copyright © 2003 Pearson Education, Inc. publishing as Benjamin Cummings Figure 2.6a, b

24. Chemical Bonds Slide 2.13 Copyright © 2003 Pearson Education, Inc. publishing as Benjamin Cummings Ionic Bonds Form when electrons are completely transferred from one atom to another Ions Charged atoms Anions are negative Cations are positive Either donate or accept electrons

25. Chemical Bonds Slide 2.13 Copyright © 2003 Pearson Education, Inc. publishing as Benjamin Cummings Ionic Bond Formation

26. Polarity Slide 2.16 Copyright © 2003 Pearson Education, Inc. publishing as Benjamin Cummings Covalently bonded molecules Some are non-polar e - are shared equally Some are polar e- are NOT shared equally Have a positive and negative side Figure 2.7

27. Chemical Bonds Slide 2.17 Copyright © 2003 Pearson Education, Inc. publishing as Benjamin Cummings Hydrogen bonds Weak chemical bonds Hydrogen is attracted to negative portion of polar molecule Provides attraction between molecules

28. Patterns of Chemical Reactions Slide 2.18 Copyright © 2003 Pearson Education, Inc. publishing as Benjamin Cummings Synthesis reaction (A+B  AB) Atoms or molecules combine Energy is absorbed for bond formation Anabolism Examples Combining amino acids to make proteins Combining glucose to make glycogen when blood sugar levels are too high

29. Patterns of Chemical Reactions Slide 2.18 Copyright © 2003 Pearson Education, Inc. publishing as Benjamin Cummings Decomposition reaction (AB  A+B) Molecule is broken down Chemical energy is released Catabolism Examples Digestion of foods Breaking down glycogen to restore blood sugar levels

30. Synthesis and Decomposition Reactions Slide 2.19 Copyright © 2003 Pearson Education, Inc. publishing as Benjamin Cummings Figure 2.9a, b

31. Patterns of Chemical Reactions Slide 2.20 Copyright © 2003 Pearson Education, Inc. publishing as Benjamin Cummings Exchange reaction (AB + C  AC + B) Involves both synthesis and decomposition reactions Switch is made between molecule parts and different molecules are made Example The terminal phosphate on ATP is exchanged for a hydroxyl group (OH) on glucose

33. Equilibrium All reactions are potentially reversible A + B ↔ AB Synthesis and decomposition occurring at the same rate

34. Factors Affecting Reaction Rates Temperature Surface area/particle size Concentration Catalysts Speed reactions without being used up Enzymes at Discovery Video Streaming Enzymes from Campbell’s Enzymes