02 [chapter 2 the chemical level of organization]

Principles of Anatomy & Physiology 14th edition [Gerard J Tortora/ Bryan Derrickson]

1. CHAPTER 2
The Chemical Level of
Organization
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Principles of
Anatomy and
Physiology
14th Edition

2. The purpose of the chapter is to:
1.Introduce the language and fundamental
concepts of chemistry
2.Discuss how matter is organized
3.Discuss how chemical bonds form and how
chemical reactions occur
4.Compare and contrast organic and inorganic
compounds
Introduction
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3. 1.Chemistry is the science of structure and
interactions of matter
2.Matter is anything that has mass and
takes up space
3.Mass is the amount of matter a
substance contains, whereas weight is
the force of gravity acting on a mass
Basic Principles of Chemistry
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4. Matter exists in 3 forms:
1.Solid
2.Liquid
3.Gas
All forms of matter are composed of
chemical elements
Chemical Elements
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5. Elements are given chemical symbols such
as:
O = oxygen
C = carbon
H = hydrogen
N = nitrogen
These elements make up the majority of our
bodies
Elements
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6. Trace Elements of the Human Body
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7. Chemical elements are composed of units
of matter of the same type called atoms
Atoms are the smallest units of matter that
retain the properties and characteristics of
an element
Atoms are composed
of protons, neutrons,
and electrons
Atoms
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8. Atomic number is the number of protons in
the nucleus of an atom
Mass number is the number of protons and
neutrons in an atom
Isotopes
Atomic Number and Mass Number
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9. Atomic mass assumes the mass of a:
Neutron = 1.008 daltons
Proton = 1.007 daltons
Electron = 0.0005 daltons
The atomic mass/weight of an element is
the average mass of all its naturally
occurring isotopes
Atomic Mass
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10. Ion – an atom that has lost or gained an
electron
Molecule – 2 or more atoms sharing
electrons
Compound – a substance that can be
broken down into 2 or more different
elements
Ions, Molecules, and Compounds
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11. Chemical Bonding
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Interactions Animation:
Chemical Bonds
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12. A chemical bond occurs when atoms are
held together by forces of attraction
The number of electrons in the valence shell
determines the likelihood that an atom will form a
chemical bond with another atom
Chemical Bonds
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13. Cations vs. Anions
Ionic Bonds
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14. Single, double, and triple bonds
Covalent Bonds
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15. Covalent Bonds
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16. In a hydrogen bond, 2 other atoms
associate with a hydrogen atom
Hydrogen Bonds
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17. A chemical reaction occurs when new bonds
are formed or old bonds are broken
Reactants – starting substances
Products – ending substances
Metabolism
Law of conservation of mass
Chemical Reactions
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18. Energy is the capacity to do work
Potential energy
Kinetic energy
Chemical energy
Law of conservation of energy
Forms of Energy & Chemical
Reactions
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19. Exergonic vs.
endergonic
reactions
Activation
energy
Energy Transfer
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20. Catalysts
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21. 1.Synthesis
2.Decomposition
3.Exchange
4.Reversible
5.Oxidation-reduction
Types of Chemical Reactions
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22. Inorganic compounds usually lack carbon
and are simple molecules
Water is the most important and abundant
inorganic compound in all living things
Organic compounds always contain H,
usually contain O, and always have covalent
bonds
Inorganic vs. Organic Compounds
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23. Properties of Water
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Interactions Animation:
Polarity and Solubility of Molecules
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24. Water as a Polar Molecule
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25. Water as a Solvent
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26. Water is the ideal medium
In a hydrolysis reaction, water is added to break
bonds
In a dehydration synthesis reaction, water is
removed to make bonds
Water in Chemical Reactions
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27. Water has a:
High heat capacity
High heat of vaporization
Water’s Thermal Properties
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28. Water is a major component of our body
fluids and helps reduce friction as
membranes and organs slide over one
another
Water as a Lubricant
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29. Mixture – a combination of elements or
compounds that are physically blended
together but not bonded together
3 types of mixtures:
1.Solution
2.Colloid
3.Suspension
Solutions, Colloids, and Suspensions
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30. Percentage & Molarity
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31. Acids, Bases, & Salts
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32. pH
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33. pH and Buffers
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Interactions Animation:
Acids and Bases
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34. Maintenance of body fluid homeostasis is
critical
Buffer systems help to regulate pH by converting
strong acids or bases into weak acids or bases
H+ + HCO3-  H2CO3
Buffer Systems
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35. Organic compounds always contain carbon
Many carbons can combine in a variety of
shapes
Carbon compounds do not dissolve easily in
water
Carbon compounds are a good source of
energy
Carbon
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36. Functional Groups of Carbon
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37. Functional Groups of Carbon
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38. Functional Groups of Carbon
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39. Functional Groups of Carbon
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40. Functional Groups of Carbon
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41. Carbohydrates
Carbohydrates
provide most of
the energy
needed for life
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42. Monosaccharides
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43. Disaccharides
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44. Polysaccharides
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45. Lipids
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46. Fatty acids can be saturated or unsaturated
Fatty Acids
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47. Triglycerides proved protection, insulation,
and energy
Triglycerides
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48. Phospholipids are an important component
of cell membranes
Phospholipids
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49. Steroids
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50. Proteins give structure to the body, regulate
processes, provide protection, assist in
muscle contraction, transport substances,
and serve as enzymes
Proteins
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51. Amino Acids
Proteins are formed by
combining various
amino acids
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52. Polypeptides
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53. Organization of Proteins
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54. An enzyme is a catalyst in a living cell
Enzymes are:
Highly specific
Extremely efficient
Subject to cellular controls
Enzymes
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55. Enzymes
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56. Enzymes
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Interactions Animation:
Enzyme Functions and ATP
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57. DNA & RNA
DNA forms the
genetic code in the
nuclei of body cells
and it regulates
most of the cell’s
activities
RNA guides protein
formation
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58. DNA vs. RNA
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59. ATP is the principal energy-storing molecule
in the body
Adenosine Triphosphate (ATP)
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60. Copyright 2014 John Wiley & Sons, Inc.
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End of Chapter 2
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