1. Essentials of Human Anatomy & Physiology Copyright © 2003 Pearson Education, Inc. publishing as Benjamin Cummings Slides 2.1 – 2.20 Seventh Edition Elaine N. Marieb Chapter 2 Basic Chemistry Lecture Slides in PowerPoint by Jerry L. Cook

2. Matter and Energy Slide 2.1 Copyright © 2003 Pearson Education, Inc. publishing as Benjamin Cummings Matter – anything that occupies space and has mass (weight) Energy – the ability to do work Chemical Electrical Mechanical Radiant

3. 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

4. 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

5. 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 Sum of the protons and neutrons

6. Atomic Weight and Isotopes Slide 2.5 Copyright © 2003 Pearson Education, Inc. publishing as Benjamin Cummings Isotopes Have the same number of protons, but vary in number of neutrons Atomic weight Close to mass number of most abundant isotope Atomic weight reflects natural isotope variation

7. 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

8. Molecules and Compounds Slide 2.7 Molecule – two or more like atoms combined chemically. Compound – two or more different atoms combined chemically. molecule, molecule, molecule & compound

9. Chemical Reactions Slide 2.8 Copyright © 2003 Pearson Education, Inc. publishing as Benjamin Cummings Atoms are united by chemical bonds Atoms dissociate from other atoms when chemical bonds are broken

10. 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

11. 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

12. 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 10 electrons 10 = 2 + 8 Shell 3 has 18 electrons 18 = 2 + 8 + 8 Figure 2.4a

13. 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

14. 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

15. Chemical Bonds Slide 2.13 Copyright © 2003 Pearson Education, Inc. publishing as Benjamin Cummings Ions Charged particles Anions are negative Cations are positive Either donate or accept electrons

16. 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

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

18. Polarity Slide 2.16 Copyright © 2003 Pearson Education, Inc. publishing as Benjamin Cummings Covalent bonded molecules Some are non-polar Electrically neutral as a molecule Some are polar Have a positive and negative side Figure 2.7

19. 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

20. Patterns of Chemical Reactions Slide 2.18 Synthesis reaction (A+B  AB) Anabolic- atoms or molecules combine Endergonic- energy is required/ used for bond formation Ex: Dehydration synthesis

21. Patterns of Chemical Reactions Slide 2.18 Copyright © 2003 Pearson Education, Inc. publishing as Benjamin Cummings Decomposition reaction (AB  A+B) Catabolic- Molecule is broken down Exergonic- Chemical energy is given off Ex: Hydrolysis- using water to split a bond

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

23. Patterns of Chemical Reactions Slide 2.20 Copyright © 2003 Pearson Education, Inc. publishing as Benjamin Cummings Exchange reaction (AB  AC+B) Involves both synthesis and decomposition reactions Switch is made between molecule parts and different molecules are made