unit 1 ~ intro zchapter 1: themes in the study of life zchapter 2: chemical context of life zchapter...
TRANSCRIPT
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Unit 1 ~ Intro
Chapter 1: Themes in the Study of Life
Chapter 2:Chemical Context of Life
Chapter 3:Water and the Fitness of the Environment
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Unifying Themes in Biology
Evolution~ biology’s core theme; differential reproductive success
Emergent Properties~ hierarchy of life
The Cell~ all organism’s basic structure
Heritable Information~ DNA
Structure & Function~ form and function
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Environmental Interaction~ organisms are open systems
Regulation~ feedback mechanismsUnity & Diversity~ universal genetic codeScientific Inquiry~ observation; testing;
repeatabilityScience, Technology & Society~ functions
of our world
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AP - Biochemistry
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Chemical Context of Life
Matter (space & mass)
Element; compoundThe atomAtomic number (# of
protons); mass number (protons + neutrons)
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Isotopes (different # of neutrons); radioactive isotopes (nuclear decay)
Energy (ability to do work); energy levels (electron states of potential energy)
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Chemical Bonding
Covalent Double covalent Nonpolar covalentPolar covalentIonicHydrogenvan der Waals
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Covalent Bonding
Sharing pair of valence electrons
Number of electrons required to complete an atom’s valence shell determines how many bonds will form
Ex: Hydrogen & oxygen bonding in water; methane
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Polar/nonpolar covalent bonds
Electronegativityattraction for electrons
Nonpolar covalent •electrons shared
equally •Ex: diatomic H and O
Polar covalent•one atom more electronegative than the other (charged)•Ex: water
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Polar/nonpolar bonds
Animation chapter 3 - Campbell
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Ionic bonding
High electronegativity difference strips valence electrons away from another atom
Electron transfer creates ions (charged atoms)
Cation (positive ion); anion (negative ion)
Ex: Salts (sodium chloride)
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Hydrogen bonds – weak bond
Hydrogen atom covalently bonded to one electronegative atom is also attracted to another electronegative atom (oxygen or nitrogen)
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van der Waals interactions
Weak interactions between molecules or parts of molecules that are brought about by localized change fluctuations
Due to the fact that electrons are constantly in motion and at any given instant, ever-changing “hot spots” of negative or positive charge may develop
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Water
Polar~ opposite ends, opposite charges
Cohesion~ H+ bonds holding molecules together
Adhesion~ H+ bonds holding molecules to another substance
Surface tension~ measurement of the difficulty to break or stretch the surface of a liquid
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Specific heat~ amount of heat absorbed or lost to change temperature by 1oC
Heat of vaporization~ quantity of heat required to convert 1g from liquid to gas states
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Bozeman: Water
http://www.bozemanscience.com/water-a-polar-molecule
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Density
Less dense as solid than liquid
Due to hydrogen bonding
Crystalline lattice keeps molecules at a distance
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Acid/Base & pH
Dissociation of water into a hydrogen ion and a hydroxide ion
Acid: increases the hydrogen concentration of a solution
Base: reduces the hydrogen ion concentration of a solution
pH: “power of hydrogen” Buffers: substances that
minimize H+ and OH- concentrations (accepts or donates H+ ions)