ELAINE N. MARIEB EIGHTH EDITION 2 Copyright © 2006 Pearson Education, Inc., publishing as Benjamin Cummings PowerPoint ® Lecture Slide Presentation by Jerry L. Cook, Sam Houston University ESSENTIALS OF HUMAN ANATOMY & PHYSIOLOGY PART A Basic Chemistry

Copyright © 2006 Pearson Education, Inc., publishing as Benjamin Cummings Introduction 1) Why review chemistry in Anatomy? a) The entire body is made up of chemicals continuously interacting with one another. b) All body processes are chemical reactions 2) What is Matter? Identify Chemical and Physical changes 3) What is Energy? a) Types 1. Kinetic: energy in motion 2. Potential: Stored energy b) Living things require a continual supply of energy

Copyright © 2006 Pearson Education, Inc., publishing as Benjamin Cummings 4) Forms of energy: a) Chemical: Stored in the bonds of chemical substances b) Electrical: Results from the movement of charged particles c) Mechanical: Directly involved in moving matter d) Radiant: (electromagnetic spectrum) travels in waves

Copyright © 2006 Pearson Education, Inc., publishing as Benjamin Cummings 5) Energy can be changed from one form to another (Conservation of energy), but in each conversion part of the energy degrades into heat (1 st Law of Thermodynamics)

Copyright © 2006 Pearson Education, Inc., publishing as Benjamin Cummings II. Composition of Matter 1) Element: a) Substance that cannot be broken down into simpler substances by ordinary chemical methods b) There are 92 naturally occurring elements c) Carbon, oxygen, hydrogen and nitrogen make up about 96% of the body weight d) Appendix B: Periodic table of elements

Copyright © 2006 Pearson Education, Inc., publishing as Benjamin Cummings 3) Atomic structure: a) Protons: Positive particle in the nucleus b) Neutron: Neutral particle in the nucleus c) Electron: Negative particle orbiting the nucleus

Copyright © 2006 Pearson Education, Inc., publishing as Benjamin Cummings Atomic Structure Figure 2.1

Copyright © 2006 Pearson Education, Inc., publishing as Benjamin Cummings 5) Ion: charged atom formed when electrons are lost or gained. 6) Planetary model: Used to represent the subatomic particles, not accurate 7) Orbital Model: Shows the area where electrons are likely to be found around the nucleus forms an electron cloud 8) Identifying elements

Copyright © 2006 Pearson Education, Inc., publishing as Benjamin Cummings a) Using the atomic number and mass you should be able to determine the number of protons, neutrons and electrons b) Isotope: Atoms that differ in the number of neutrons

Copyright © 2006 Pearson Education, Inc., publishing as Benjamin Cummings c) Radioisotopes: Unstable isotopes that release particles and energy (radioactivity) to become more stable isotopes (used medically see Pet scans PP ) 9) Molecules and compounds: a) Molecule: formed when 2 or more atoms combine chemically b) Compound: Formed when 2 or more different atoms combine c) Compound properties are always different from the atom properties

Copyright © 2006 Pearson Education, Inc., publishing as Benjamin Cummings III. Chemical Bonds 1) Chemical reaction: Occur when atoms combine or dissociate 2) Chemical bond: Attraction between atoms forming compounds 3) Electron’s role a) In a reaction, only the valence (outer level) electrons interact b) Each energy level can only hold a specific number of valence electrons 1 st : 2 electrons All others: 8

Copyright © 2006 Pearson Education, Inc., publishing as Benjamin Cummings c) Octet rule: Atoms tend to gain, lose or share electrons to get 8 in the outer level 4) Ionic bond: form when ions are attracted to each other 5) Covalent bond: a) form by the sharing of electrons b) Non-polar : electrons are shared evenly c) Polar: uneven sharing of electrons causing positive and negative ends e) Polar molecules will attract each other or ions

Copyright © 2006 Pearson Education, Inc., publishing as Benjamin Cummings COVALENT BONDS ANIMATION Examples of Covalent Bonds Figure 2.6a–b

Copyright © 2006 Pearson Education, Inc., publishing as Benjamin Cummings 6) Hydrogen bond a) Occurs between hydrogen of one molecule to a charged end of another b) Water is an example of hydrogen bonding You should be able to compare, contrast and identify the different types of bonds

Copyright © 2006 Pearson Education, Inc., publishing as Benjamin Cummings IV. Biochemistry: 1) Two major classes of compounds a) Inorganic: small, lack carbon b) Organic: Carbon compounds including 2) Inorganic compounds a) Water: 1. About 2 thirds of the body weight 2. Properties: (Page 39) A. High heat capacity B. Polarity/Solvent properties C. Chemical reactivity D. Cushioning

Copyright © 2006 Pearson Education, Inc., publishing as Benjamin Cummings b) Salts 1. Ionic compounds 2. Form Electrolytes c) Acids & Bases 1. Acid properties: sour taste, dissolve metals, proton donors, have a hydrogen ion 2. Base properties: Bitter, accept protons, many have hydroxide ions 3. Neutralization reaction: When an acid and base combine, they form water & a salt

Copyright © 2006 Pearson Education, Inc., publishing as Benjamin Cummings 4. pH: Scale used to measure the acidity of a solution 7=neutral Below= acid Above = base 5. Buffers: maintain pH stability by taking up excess H and OH ions

Copyright © 2006 Pearson Education, Inc., publishing as Benjamin Cummings 3) Organic compounds a) Carbohydrates 1. Include sugars and starches and contain C, H and O 2. Classes: Mono, di & polysaccharides

Copyright © 2006 Pearson Education, Inc., publishing as Benjamin Cummings b) Lipids: 1. Large and diverse group of organic compounds (Pg 44 Table 2.2) 2. Consist of C,H & O, not soluble in water 3. Important types A.Triglycerides (neutral fats): Composed of fatty acid and glycerol forming an E- shaped molecule (Saturated = solid fats & Unsaturated = liquid oils) used as energy storage, cushioning & insulation

Copyright © 2006 Pearson Education, Inc., publishing as Benjamin Cummings B. Phospholipid: Similar to triglyceride with one fatty acid replaced by a phosphate group making it polar. Form membranes C. Steroids: 4 interlocking fat rings including cholesterol used in forming cell membranes, vitamin D and some hormones

Copyright © 2006 Pearson Education, Inc., publishing as Benjamin Cummings Lipids Figure 2.14a–b movie

Copyright © 2006 Pearson Education, Inc., publishing as Benjamin Cummings c) Proteins: 1. 50% of the organic matter in the body 2. Formed from amino acids 3. Types: A. Fibrous: Structural proteins (collagen) B. Globular: mobile, spherical molecules functional proteins C. Enzymes: Catalyst for reactions in the body (suffix –ase) necessary for the body reactions to occur at normal body temp.

Copyright © 2006 Pearson Education, Inc., publishing as Benjamin Cummings d) Nucleic acids: 1. Formed from a nucleotide (sugar, phosphate and nitrogenous base) 2. Types: A. DNA: forms the genetic material of the cell B. RNA: used to carry protein codes, amino acids and form ribosomes

Copyright © 2006 Pearson Education, Inc., publishing as Benjamin Cummings

e) ATP: 1. Adenine base with additional phosphates 2. This is the energy molecule for all reactions 3. ADP: molecule formed when ATP is broken down to release energy

Copyright © 2006 Pearson Education, Inc., publishing as Benjamin Cummings How ATP Drives Cellular Work Figure 2.20