principles of anatomy and...
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CHAPTER 2The Chemical Level of
Organization
Copyright © 2014 John Wiley & Sons, Inc. All rights reserved.
Principles of Anatomy and Physiology
14th Edition
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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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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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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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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Trace Elements of the Human Body
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Chemical elements are composed of units of matter of the same type called atomsAtoms are the smallest units of matter that retain the properties and characteristics of an element
� Atoms are composedof protons, neutrons,and electrons
Atoms
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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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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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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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Chemical Bonding
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Interactions Animation:
Chemical Bonds
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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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Cations vs. Anions
Ionic Bonds
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Single, double, and triple bonds
Covalent Bonds
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Covalent Bonds
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In a hydrogen bond, 2 other atoms associate with a hydrogen atom
Hydrogen Bonds
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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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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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Exergonic vs. endergonicreactions
Activation energy
Energy Transfer
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Catalysts
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1. Synthesis
2. Decomposition
3. Exchange
4. Reversible
5. Oxidation-reduction
Types of Chemical Reactions
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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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Properties of Water
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Interactions Animation:
� Polarity and Solubility of Molecules
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Water as a Polar Molecule
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Water as a Solvent
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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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Water has a:� High heat capacity
� High heat of vaporization
Water’s Thermal Properties
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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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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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Percentage & Molarity
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Acids, Bases, & Salts
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pH
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pH and Buffers
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Interactions Animation:
� Acids and Bases
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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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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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Functional Groups of Carbon
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Functional Groups of Carbon
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Functional Groups of Carbon
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Functional Groups of Carbon
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Functional Groups of Carbon
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Carbohydrates
Carbohydrates provide most of the energy needed for life
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Monosaccharides
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Disaccharides
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Polysaccharides
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Lipids
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Fatty acids can be saturated or unsaturated
Fatty Acids
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Triglycerides proved protection, insulation, and energy
Triglycerides
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Phospholipids are an important component of cell membranes
Phospholipids
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Steroids
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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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Amino Acids
Proteins are formed by combining various amino acids
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Polypeptides
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Organization of Proteins
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An enzyme is a catalyst in a living cell
Enzymes are:� Highly specific
� Extremely efficient
� Subject to cellular controls
Enzymes
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Enzymes
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Enzymes
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Interactions Animation:
� Enzyme Functions and ATP
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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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DNA vs. RNA
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ATP is the principal energy-storing molecule in the body
Adenosine Triphosphate (ATP)
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End of Chapter 2
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