Title: Anatomy and Physiology by Rod R Seeley 6th edition chapter 2 power-point
1 Anatomy and Physiology, Sixth Edition
Rod R. SeeleyIdaho State University Trent D.
StephensIdaho State University Philip
TatePhoenix College
Chapter 02 Lecture Outline
See PowerPoint Image Slides for all figures and
tables pre-inserted into PowerPoint without notes.
Copyright The McGraw-Hill Companies, Inc.
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2Chapter 2
- The Chemical Basis of Life
3Basic Chemistry
- Matter, Mass, and Weight
- Matter Anything that occupies space and has mass
- Mass The amount of matter in an object
- Weight The gravitational force acting on an
object of a given mass - Elements and Atoms
- Elements The simplest type of matter with unique
chemical properties - Atoms Smallest particle of an element that has
chemical characteristics of that element
4Atomic Structure
- Atoms composed of subatomic particles
- Neutrons no electrical charge
- Protons positive charge
- Electrons negative charge
- Nucleus
- Formed by protons and neutrons
- Most of volume of atom occupied by electrons
5Atomic Number and Mass Number
- Atomic Number Equal to number of protons in each
atom which equals the number of electrons - Mass Number Number of protons plus number of
neutrons
6Isotopes and Atomic Mass
- Isotopes Two or more forms of same element with
same number of protons and electrons but
different neutron number - 3 types of hydrogen
- Denoted by using symbol of element preceded by
mass number as 1H, 2H, 3H - Atomic Mass Average mass of naturally occurring
isotopes
7Electrons and Chemical Bonding
- Ion When an atom loses or gains electrons and
become charged - Cation Positively charged ion
- Anion Negatively charged ion
- Ionic Bonding
- Cations and anions are attracted to each other
8Covalent Bonding
- Atoms share one or more pairs of electrons
- Single covalent Electron pair between 2 atoms
- Double covalent Two atoms share 4 electrons
- Nonpolar covalent Electrons shared equally
- Polar covalent Electrons not shared equally
9Molecules and Compounds
- Molecules Two or more atoms chemically combine
to form and independent unit - Example Water
- Compounds A substance composed of two or more
different types if atoms chemically combined - Example Hydrogen Molecule
- Molecular Mass Determined by adding up atomic
masses of its atoms or ions - Example NaCl (22.99 35.45)
10Intermolecular Forces
- Result from weak electrostatic attractions
between oppositely charged parts or molecules, or
between ions and molecules - Weaker than forces producing chemical bonding
11Intermolecular Forces
- Hydrogen Bonds
- Water Positively charged hydrogen atoms bond
with negatively charged oxygen atoms of other
water molecules - Important role in determining shape of complex
molecules
12Intermolecular Forces
- Solubility Ability of one substance to dissolve
in another - Example Sugar dissolves in water
- Dissociation or Separation
- Ionic compounds
- Cations are attracted to negative end and anions
attracted to positive end of water molecules
13Intermolecular Forces
- Electrolytes Cations () and anions (-) that
dissociate in water - Capacity to conduct an electric current
- Currents can be detected by electrodes
- Nonelectrolytes Molecules that do not dissociate
form solutions that do not conduct electricity
14Chemical Reactions
- Chemical Reactions Atoms, ions, molecules or
compounds interact to form or break chemical
bonds - Metabolism All anabolic and catabolic reactions
in the body - Catabolism Decomposition reactions
- Hydrolysis Reactions that use water
- Anabolism Growth, maintenance, and repair of
the body in synthesis reactions - Produce molecules characteristic of life ATP,
proteins, carbohydrates, lipids, and nucleic acids
15Synthesis and Decomposition Reactions
- Synthesis Reactions
- Two or more reactants chemically combine to form
a larger product - Anabolism All bodys synthesis reactions
- Decomposition Reactions
- Reverse of synthesis reactions
- Catabolism Reactions of decomposition in body
16Oxidation-Reduction Reactions
- Oxidation
- Loss of an electron by an atom
- Reduction
- Gain of an electron by an atom
- Oxidation-Reduction Reactions
- The complete or partial loss of an electron by
one atom is accompanied by the gain of that
electron by another atom
17Speed of Chemical Reactions
- Activation Energy Minimum energy reactants must
have to start a chemical reaction - Catalysts Substances that increase the rate of
chemical reactions without being permanently
changed or depleted - Enzymes Increase the rate of chemical reactions
by lowering the activation energy necessary for
reaction to begin
18Water
- Inorganic
- Stabilizes body temperature
- Protection
- Necessary for many chemical reactions of life
- Mixing Medium
- Mixture Substance physically but not chemically
combined - Solution Liquid, gas, or solid uniformly
distributed - Solvent What dissolves the solute
- Solute What is to be dissolved
19Acids and Bases Salts and Buffers
- Acid A proton donor or any substance that
releases hydrogen ions - Bases A proton acceptor or any substance that
binds to or accepts hydrogen ions - Salts A cation consisting of other than a
hydrogen ion and other than an anion or hydroxide
ion - Buffers A solution of a conjugate acid-base pair
in which acid and base component occur in similar
concentrations
20The pH Scale
- Refers to the Hydrogen ion concentration in a
solution - Neutral pH of 7 or equal hydrogen and hydroxide
ions - Acidic a greater concentration of hydrogen ions
- Alkaline or basic a greater concentration of
hydroxide ions
21Organic Chemistry
- Carbohydrates
- Composed of carbon, hydrogen, oxygen
- Lipids
- Composed mostly of carbon, hydrogen, oxygen
- Proteins
- Composed of carbon, hydrogen, oxygen,nitrogen
- Nucleic Acids DNA and RNA
- Composed of carbon, hydrogen, oxygen, nitrogen,
phosphorus - Adenosine Triphosphate (ATP)
- Composed of adenosine and three phosphate groups
22Carbohydrates
- Monosaccharides
- Simple sugars glucose, fructose, galactose
- Disaccharides
- Two simple sugars bound together by dehydration
sucrose, lactose, maltose - Polysaccharides
- Long chains of many monosaccharides glycogen in
animals starch and cellulose in plants
23Lipids
- Lipids Can be dissolved in nonpolar organic
solvents as alcohol or acetone but relatively
insoluble in water - Fats Ingested and broken down by hydrolysis
- Triglycerides composed of glycerol and fatty
acids - Phospholipids Important structural component of
cell membranes - - Steroids Cholesterol, bile salts, estrogen,
testosterone
24Proteins
- Amino acids The building blocks of protein
- Peptide bonds Covalent bonds formed between
amino acids during protein synthesis - Enzymes Protein catalysts
25Nucleic Acids DNA and RNA
- DNA Deoxyribonucleic acid
- Genetic material of cells copied from one
generation to next - Composed of 2 strands of nucleotides
- Each nucleotide contains one of the organic bases
of adenine or guanine which are purines and
thymine or cystosine which are pyrimidines - RNA Ribonucleic acid
- Similar to a single strand of DNA
- Four different nucleotides make up organic bases
except thymine is replaced with uracil
(pyrimidine)
26Adenosine Triphosphate (ATP)
- Energy currency of the body
- Provides energy for other chemical reactions as
anabolism or drive cell processes as muscle
contraction - All energy-requiring chemical reactions stop when
there is inadequate ATP