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What is Biology?
Study of life & characteristics of life
Expectations/learning outcomes:– Understand, explain, describe, & integrate the
natural world of living things– Focusing on:
• How life works… rather than the “meaning of life”
Characteristics of Life?
In other words… what are the essential properties/functions of “living” systems?
• DNA• Cells• Acquire & use energy• Highly complex & organized• Growth & development• Metabolize chemicals• Reproduce• Evolve by natural selection
Levels of organization• Biosphere• Ecosystem• Community• Population• Organism• Organ system• Organ• Tissue• Cell -------functional units of life• Organelle• Molecule• Atom• Subatomic particle
How can we study: all these characteristics, diversity, complexity… and, try to make sense of it?
• Scientific Method– What?
– Why?
– How?
Inductive approach: from specific observations to the general
Deductive approach: use general principles in predicting specific outcomes
Scientific Method
Complexity builds from the atomic level up (Ch. 2)
• Atoms– Chemical unit – Made up of subatomic particles
• Nucleus of an atom– Protons positive charge– Neutrons neutral charge
• Electrons– negative charge– Orbit around nucleus in energy shells (2,8,8…)– Determine chemical nature, reactivity, and interactions with other
elements …incomplete shells create potential for interactions.
Lets make an atom of Carbon…• Symbol for Carbon element• Atomic number
6 protons
• Nucleus w/ 6 protons & 6 neutrons• 1st shell with 2 electrons• Second shell with only 4 electrons
…has space for 4 more e-
• Atomic mass?6 protons6 neutrons6 electrons= 12.011 (electrons negligible mass)
6
C12.011
1
H1
Relationships between atoms & molecules or, Bonds
• Interactions of outer shells or valence electrons
• Form molecules of multiple atoms• Form compounds of multiple molecules
• Covalent bonds– Atoms share
electrons (e-) between pairs to satisfy each of their valence shells
Example
• Ionic bonds– Unequally charged ions…
e- transferred from one ion to another (gain/loss of e-)
1
H1
17
Cl35.4
11
Na22
1
H1
+
+
Although the strongest bonds are Covalent, it is the weak Hydrogen bonds that are perhaps
the most significant to cell functions.
• Polar molecules– Covalent bonds of unequal
sharing (H20)
– O is more electronegative than H
• Hydrogen bonds include H• Opposites (+ & -) attract
creating H-bonds between water molecules
What else do we know about water?• Naturally occurs in 3 forms with varying levels of energy
and density.– Solid, liquid, gas
• Which is the most dense?
• Molecules in constant motion– Breaking & making H-bonds
• Varies with temperature, density, and dissolved particulates
Water is a common solvent that dissolves substances (solutes) to form an aqueous solution
• Additional water molecules dissociate leaving some hydrogen ions (H+) and some hydroxide ions (OH-)
• These ions are very reactive
• [H+] in solution = acidic Therefore a lower pH
• [OH-] in solution = basic Therefore a higher pH
The importance of Organic chemicals… (Ch. 3)
• contain at least one C atom– 4 electrons in outer shell
– in need of 4 more
– covalent bonds with H, O, N, or other C
• Molecules of only C and H are called hydrocarbons
• Bonding determines shape• Functional groups
– determine properties & functions of organic compounds
– Are usually polar, thus soluble in water, thus more reactive than carbon backbone by itself
Most of a cells molecules are variations and extensions of a small set of small molecules.
Making Macromolecules• Many repeating smaller
molecules• Polymers of monomers• Built by dehydration
synthesis reaction (rxn)
Classes of Macromolecules
• Carbohydrates– Simple & complex sugars– Monosaccharides & Polysaccharides
• Lipids– Fats, oils, waxes, etc.
• Proteins– Made of 20 Amino acids
• Nucleic Acids– DNA made of only 4 monomers (nucleotides)
Carbohydrates
• E.g. glucose, fructose, lactose, sucrose, starch, glycogen, cellulose…
• Fuel to do work• Raw material for bigger
molecules• 2 sugars linked =
disaccharide via dehydration synthesis
• More sugars = polysaccharides
Note: Animals can’t hydrolyze cellulose very well, therefore use bacteria to do it for us -- Byproduct is methane gas
Lipids• Fats, oils, waxes, steroids
• Polymers of fatty acids and glycerol
• Energy storage molecules
• Hydrophilic heads (w / polar functional group(s); interacts easier with water)
• & hydrophobic tails (nonpolar; insoluble)
• Saturated fats– Very few double bonds– Lots of H’s– Solid at room temperature (butter, lard, and
most animal fats)
• Unsaturated fats– Kinked due to double bonds, less H’s, take up
more space– Liquid at room temperature– E.g. oils, margarine, and most plants fats– Hydrogenating unsaturated fats make them
solid (margarine); trans fats
Steroids
• Lipids with backbones bent into rings
• Cholesterol– functions in digestion of fats– Important component in cell
membranes (see ch 5)– Starting material of other
steroids like sex hormones
Note: Anabolic steroids (synthetics) mimic testosterone (see ch 12)
Proteins – have many roles
Made from 20 different amino acids monomers• Structural – hair, cell, cytoskeleton• Contractile – muscles, motile cells• Storage – sources of amino acids (egg whites)• Defense – antibodies, membrane proteins• Transport – hemoglobin, membrane proteins• Signaling – hormones, membrane proteins• Catalyst – free enzymes, membrane proteins
Protein properties…
• Amino group• Carboxyl group• Variable R group
– Could be a single H– Or, C’s with functional
groups– Determines specific
properties and protein diversity
• Linked to form polymer proteins by peptide bonds– Specific covalent bond between amino acids– Two aminos bonded = dipeptide– More aminos = polypeptides
Protein’s shape determines function
• 1o structure: unique sequence of amino acids
• 2o structure: coils or folds via H-bonding
• 3o structure: 3-D globular or fibrous subunit via bonds of R-groups
• 4o structure: multiple subunits