Overview of the Human Body
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Transcript of Overview of the Human Body
Overview of the Human BodyChapter 1
Overview• Anatomy and physiology: definitions• Form and Function• Homeostasis• Levels of organization
What is “Anatomy and Physiology”?
• Anatomy-
• Physiology-
Form (Structure) Fits Function
• Principle of Complementarity-
• You need to understand the parts and how they are put together before you can truly understand how they work
• If you know what a body structure does, you can usually predict how it is organized/structured to do its job
Homeostasis
• Homeostasis-
• The nervous system and endocrine system (hormones) play important roles in communication that promotes homeostasis throughout the body.
• Every cell of the body must also maintain homeostasis
Homeostasis and Feedback Loops• All systems involve three components: a ‘receptor’, a
control center and an effector
RECEPTOR (ie. free
nerve ending in the skin)
CONTROL CENTER(such as the brain)
EFFECTOR(such as a muscle,
or a gland)
Stimulus (input into the system)
The response to the stimulus leads to change. The change is ‘fed back’ to
the receptor.
Response(system’s output)
Homeostasis and Feedback Loops
• In negative feedback a stimulus causes a response which works to reduce/counteract the stimulus
– Examples?
• In positive feedback a stimulus causes a response which further increases the stimulus, so that output is accelerated
– Examples?
Levels of Organization
• How big is an atom?
~ 10,000,000 atoms lined up side by side
to measure 1 mm
OrganelleMoleculeAtoms
Chemical level Cellular level
Tissue levelTissues consist of similartypes of cells.
Organ levelOrgans are made up of different typesof tissues.
Organ system level Organismal level
Smooth muscle cell
Smooth muscle tissue
Connective tissue
Blood vessel (organ)
HeartBloodvessels
Epithelialtissue
Smooth muscle tissue
1 2
3
4
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Chemistry Chapter 2
Chemistry Basics• Element: unique substance that cannot be
broken down into a more simple substance by ordinary chemical methods.
Chemistry Basics• Atom: building block of an element
– Proton– Neutron– Electron
• Atomic Number• Atomic Mass
Chemistry Basics• Isotope: different # of neutrons (from a
standard atom of the same element)
• Ion: different # of electrons (from the standard atom of the same element)
Chemical Bonds• Chemical bonds: energy relationships between
electrons of reacting atoms• Electrons in valence shell (outermost electron shell)
– chemically reactive electrons• Octet rule (rule of eights)
– Except for the first shell (full with two electrons) atoms interact to have eight electrons in their valence shell
• 3 major bond types– Ionic– Covalent– Hydrogen
Sodium atom (Na)(11p+; 12n0; 11e–)
Chlorine atom (Cl)(17p+; 18n0; 17e–)
Sodium gains stability by losingone electron, and chlorine becomesstable by gaining one electron.
After electron transfer,the oppositely charged ionsformed attract each other.
Sodium ion (Na+) Chloride ion (Cl–)
Sodium chloride (NaCl)
+ —
Ionic Bonds
Figure 2.6a–b Formation of an ionic bond.
Reacting atoms
Hydrogen atoms Carbon atomFormation of four single covalent bonds:Carbon shares four electron pairs withfour hydrogen atoms.
+
Molecule of methane gas (CH4)
Structural formulashows single bonds.
or
Resulting molecules
Figure 2.7a Formation of covalent bonds.
Covalent Bonds
Types of Covalent Bonds• Non-Polar: Electrons shared equally
– Produces electrically balanced, nonpolar molecules
• Polar: unequal sharing of electrons produces polar – Atoms in bond have different electron-attracting
abilities
Electrons and chemical bonds
H2OH2
•Which molecule above is polar? Non-polar? How do you know?•Which molecule above has covalent bonds? Polar covalent bonds?•Are either of these molecules ions?
Other important terms
GLYC
EROLH2O
A triglyceride
• Hydrophilic-• Hydrophobic-
pH- Acids and Bases• Acids
– Have a sour taste– Release hydrogen ions, protons (H+) into
solution– HCl, HC2H3O2, H2CO3
• Bases– Have a bitter taste, feel slippery– Are proton acceptors (they take up H+s from
solution)– NaOH, HCO3
-, NH3
pH- Acid-Base Concentration• The concentration of H+ ions in solution is
measured in units of pH• The pH scale is logarithmic and runs from 0 to 14,
with a pH value of 7 indicating a neutral solution– Acidic solutions have pH values
from 0-6– Neutral solutions = pH 7– Basic (alkaline) solutions
have pH values from 8-14• The more hydrogen ions in a
solution, the more acidic it is, but the lower its pH value.
Thought Question• The presence of hydrogen ions
stimulates the brain to increase respiration rate.
• Johnny’s blood pH is 7.25. Normal blood pH is 7.4.
• Will Johnny likely be breathing faster or slower than normal? Why?
Chemical Reactions1. Synthesis or Anabolic reactions2. Decomposition or Catabolic reactions3. Exchange reactions (swapping
partners)
Chemical Reactions• Synthesis or Anabolic reactions A + B → AB • Decomposition/Catabolic
Reactions AB → A + B
• Exchange reactions AB + CD → AD + CB
What type of reaction is this?
OGlucose Fructose
SucroseGlucose
Fructose&
Reactant Products
FructoseFructose
A. Synthesis ReactionB. Decomposition ReactionC. Exchange ReactionD. All of the above
Chemical Reactions, Energy & Enzymes
• Most chemical reactions do not occur spontaneously, or they occur so slowly that they would be of little value to cells
• Activation energy-
• Enzymes promote chemical reactions by lowering activation energy
• Enzymes are biological catalysts, they are usually protein molecules
Mechanism of enzyme action
Substrates (S)e.g., amino acids
Enzyme (E)
Enzyme-substratecomplex (E-S)
Enzyme (E)
Product (P)e.g., dipeptide
Energy isabsorbed;bond isformed.
Water isreleased.
Peptidebond
1 Substrates bind at active site. Enzyme changes shape to hold substrates in proper position.
2 Internalrearrangements leading to catalysis occur.
3 Product isreleased. Enzyme returns to original shape and is available to catalyze another reaction.
Active site
+
Link- Enzyme animation
Sucrase is the enzyme that catalyzes this decomposition reaction
OGlucose Fructose
Sucrose
GlucoseFructose&
Reactant Products
sucraseFructose Fructose
What do you think? -Does the reverse reaction ever occur?-Is sucrose ever formed (synthesized) from glucose and fructose?
What are organic compounds?• In chemistry, an organic compound
must contain carbon and hydrogen
• Most biologically relevant, organic compounds are soluble in water– Why? – What group might be the exception?
• Many are polymers (large molecules) built from monomers (small subunits)
What are examples of inorganic compounds in the body?
What are some examples of these organic compounds in the body?
1. Carbohydrates2. Lipids3. Proteins4. Nucleic acids
Can you identify an example of each?
Carbohydrates
• Group of molecules that includes sugars, starches and fiber
• Account for less then 1-2% of body weight• In the body, primary function is as a readily
usable energy source (glucose)– Also as energy storage (glycogen)– Cellular surface markers
• Forms of carbohydrates– Monosaccharides, Disaccharides,
Polysaccharides
Glucose is a monosaccharide
= Fuel
• Glucose is a ‘single’ sugar. • Note that it is a ring structure with 6 carbon atoms. • Other monosaccharides- fructose, galactose
C6H12O6 =
glucose
=
Sucrose is a disaccharide
Other disaccharides- maltose, lactose
OGlucose FructoseFructose
Polysaccharides• Starch/Amylose• Glycogen• Cellulose
Linear chain
(a) Starch
Starch granules inpotato tuber cells
Glucosemonomer
(b) Glycogen
GlycogenGranulesIn muscletissue
(c) Cellulose
Cellulose molecules
Cellulose fibril ina plant cell wall
Polysaccharides
Monomer + Monomer + Monomer = Polymer
Lipids• Lipids, as a class, are a very diverse group of
molecules– What do you think is the unifying
characteristic of lipids? • Lipids are important energy stores• Lipids form essential structures in cells
Major types of lipids1. Triglycerides
- Comprised of fatty acids and glycerol; what we usually call ‘fats’ or ‘oils’
2. Steroids-Cholesterol derivatives
3. Eicosanoids-Cell signaling molecules
4. Phosopholipids- Amphipathic molecules that form cell
membranes
Triglycerides
• Triglycerides are three fatty acids linked to one glycerol molecule.
• Fatty acids are long, linear chains of carbon and hydrogens (hydrocarbon chains).
GLYC
EROL F A T T Y A C I D
F A T T Y A C I D
F A T T Y A C I D
TriglyceridesGL
YCER
OL
• In different triglycerides, the glycerol is the same, but the fatty acid chains vary, resulting in different types of fats and oils.
• All fatty acid (hydrocarbon chains) are non-polar.
FATTY ACID #1
Functions and locations of triglycerides in the body
• Functions of triglycerides?
• Where can we find stores of triglycerides?
GLYC
ERO
L
F A T T Y A C I D F A T T Y A C I D F A T T Y A C I D
1.
2.
3.
Steroids• All consist of a complex
ring structure• Cholesterol is the precursor
for all steroid hormones– Estrogen– Testosterone– Cortisol
• Signaling molecules– Sexual function– Tissue metabolism
• Component of animal cell membranes
cholesterol
estrogen testosterone
Eicosanoids
• Non-Steroidal Anti-Inflammatory Drugs(NSAIDs) inhibit prostaglandin synthesis
Cell Cell membranae
• Diverse group of lipids derived from fatty acids of cell membranes–Prostaglandins
• Powerful signaling molecules, synthesized by nearly all tissues of the body
• Tend to act locally• Pain/inflammation • Labor
Phospholipids
A triglyceride
A phospholipid
Phospholipids are modified triglycerides. Phospholipids have TWO fatty acids chains, and a phospho-group in place of the third!
GLYCEROL
F A T T Y A C I D
F A T T Y A C I D
F A T T Y A C I D
GLYCEROL
F A T T Y A C I D
F A T T Y A C I D =
PhosphateGroup
Non-lipidGroup
PhospholipidChemist’s version Anatomist/Biologist’s
version
Phospholipid molecules are amphipathic. One part of the molecule is polar, while the other end is non-polar.
Which end interacts readily with water?
Yikes!
Phospholipid bilayer
Chemist’s version
Biologist’s version Sesame Street
versionH20
Two layers of phospholipids, stacked on each other, with the hydrophobic tails of each layer
facing one another.Phospholipid animationhttp://telstar.ote.cmu.edu/biology/MembranePage/index2.html
All cell membranes are a phosophlipid bilayer
• Forms the boundary between a cell and its environment• Hydrophobic core, with hydrophilic ends
Proteins• Proteins are polymers (chains)
of amino acids (AA)
• A single, generalizedamino acid
- + +-
•Amino acids are linked together via peptide bonds. •Two linked amino acids = dipeptide•10-50 linked together = polypeptide•50+ = protein
Heidi’s Protein Cartoon- Each shape in the chain represents
one amino acid
Peptide bonds
Protein FunctionsThe over 2 million proteins in our bodies do an
amazing variety of tasks
• Enzymes (control metabolism)• Support• Movement• Transport• Cell Receptors for communication• Buffering• Hormonal Regulation• Defense
The 20 Amino Acids
Protein Structure
The hydrogen bonds between amino acids
(not the peptide bonds) are easily
disrupted by changes in temperature and
pH. What happens to protein structure
when pH is abnormal?
LINK
Nucleic acids
• DNA- deoxyribonucelic acid and RNA- ribonucleic acid
-Store and process information-Your genetic code-Provide the directions for building proteins
• DNA is a double stranded molecule that resides in the cell nucleus
• RNA is single stranded molecule that is found mainly outside of the nucleus, usually serving as a ‘copy’ of DNA
Nucleic Acids are Polymers, too!
• The monomers/units of nucleic acids are nucleotides
• A nucleotide consists of– Sugar– Phosphate group– Nitrogenous base (A, C, T, G or U)
Phosphate
Base
Sugar
Nucleotide monomer
DNA and RNA•DNA is two long strands of nucleotides, held together by hydrogen bonds between the nucleotide bases
-Exhibits complementary base pairing along double helix
•RNA is a single stranded nucleic acid; serves as a template for protein synthesis
RNA
DNA
Adenosine
Adenosine Triphosphate- ATP
• Storable “energy packets” for cells
---
Link http://faculty.ccbcmd.edu/biotutorials/energy/adpan.html
Solute
Membraneprotein
Relaxed smoothmuscle cell
Contracted smoothmuscle cell
+
+
+
Transport work: ATP phosphorylates transportproteins, activating them to transport solutes(ions, for example) across cell membranes.
Mechanical work: ATP phosphorylates contractile proteins in muscle cells so the cells can shorten.
Chemical work: ATP phosphorylates key reactants, providing energy to drive energy-absorbing chemical reactions.
(a)
(b)
(c)
Cellular work driven by ATP energy
• Hydrolysis of ATP provides energy for cellular needs
• ATP transfers its terminal phosphate, and ‘energizes’ another molecule