unit 1 – the chemistry of life zchapter 2: chemical context of life zchapter 3: water and the...
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Unit 1 – The Chemistry 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 Environmental Interaction~ organisms are
open systems Regulation~ feedback mechanisms Unity & Diversity~ universal genetic code Scientific Inquiry~ observation; testing;
repeatability Science, Technology & Society~ functions
of our world
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Chemical Context of Life
Matter (space & mass)
Element vs. compound The atom Atomic number (# of
protons); mass number (protons + neutrons)
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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Electron configurations of the first 18 elements.
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Polar/nonpolar covalent bonds
Electronegativityattraction for electrons
Nonpolar covalent •electrons shared equally•Ex: methane (CH4)
Polar covalent•one atom more electronegative than the other (charged)•Ex: water (H20)
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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
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 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 Density……….
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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)