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Published byErnest Tate Modified over 9 years ago
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AP BIOLOGY Chapter 2: Chemistry
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Chemistry Study of matter and its forms and interactions Important to Biology Themes of hierarchy and form fits function, as well as, emergent properties are all because of chemistry to some degree.
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Chemical Elements and Compounds Organisms are made of matter Matter Element Atom Compound Organic compound Molecule Organic macromolecule
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Life requires about 25 elements 92 naturally occurring CHNOPS = 96% of dry weight CHOPKINS CaFe, Mg NaCl = >99% Carbon, hydrogen, oxygen, phosphorus, potassium, iodine, nitrogen, sulfur, calcium, iron, magnesium, sodium and chlorine….. Trace elements are those required by an organism in quantities of <0.01% of body mass
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Atomic structure Proton Positive, central/nucleus Mass = 1 amu or Dalton Can not leave/add Atomic number Neutron Neutral, central/nucleus Mass = 1 amu or Dalton Neutron + proton = atomic mass Atomic weight vs. mass number Electron Negative, found in orbitals Can leave, add, transfer, move Creates charge as well as many properties of element
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Ions Elements that have a charge as a result of the proton number and the electron number being unequal. Positive ions are called cations and have more protons than electrons Negative ions are called anions and have more electrons than protons
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Isotopes These are atoms of the same element with varying numbers of neutrons, thus different masses. Many elements have naturally occurring isotopes (decimals in atomic mass are from averaging these) C12 and C14 are examples. Radioactive isotopes spontaneously decay, giving off energy and particles. Can be biologically harmful Can also be medically/scientifically useful as tracers
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Bonds Covalent Polar covalent Nonpolar covalent Ionic Hydrogen Van der Waals Interactions
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Covalent bonds Created when electrons are “shared” by several atoms. Orbitals overlap. Bond is tight (short) and strong. Nonpolar covalent bonds contain equally shared electrons and create no charged regions Polar covalent bonds share electrons UNEVENLY and create areas of CHARGE within the molecule.
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Ionic bonds Are created between atoms when electrons are transferred and ions are created. Ions of opposite charge then attract. Relatively distant (long) and weaker. Ionic bonds can “dissociate” or separate and re-bond with something else more attractive.
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Hydrogen Bonds Exist between two molecules because of regions of charge within the molecules. Water forms many H-bonds. Polar covalent water has negative regions near the oxygen and positive regions near the hydrogen. Oxygen region from one water attract hydrogen regions from other waters. Water beads because of this. Very, very, very weak, but collectively HUGE
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