Lecture 3

Lecture 3 - Lecture 3 Guide September 1 (HOME) Starting...

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Lecture 3 Guide (HOME) September 1 Starting with this lecture, the Study Guides will be in a form that you will need to add to during lecture. Readings: pages 32-46 Basics Of Biological Molecules Atomic And Molecular Structure Matter – anything that takes up space and has mass (weight) Element – a substance that cannot be broken down to a simpler substance by ordinary chemical means Compound – a substance that consists of two or more elements combined in a fixed ratio Atom – the smallest particle of an element that retains the property of the element (see Fig. 2.4) Atomic number - the number of protons in an atom Mass number - the number of protons and neutrons in an atom Atomic mass - approximately the mass number of an atom in daltons. Isotopes – atoms with the same atomic number but different mass numbers Radioactive Isotopes – unstable isotope that decays giving off particles and energy Natural Carbon Isotopes (Atomic number = 6) Isotope Abundance
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12 C 98% 13 C 1% 14 C trace (radioactive) Natural Potassium Isotopes (Atomic number = 19) Isotope Abundance 39 K 93.3% 40 K trace (radioactive) 41 K 6.7% Radioactive Isotopes – important tools in experimental studies Examples: 1. Trace biochemical pathways 2. Determine rates of synthesis 3. Identify cellular locations Electron Configuration in Atoms Electrons fill sequential "shells" around atoms Electron Configuration & Chemical Properties (Fig. 2.8)
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Chemical Bonds Depend on Electrons in the Outer Shell and Electronegativity of an Atom Valence Shell - outermost shell containing electrons Valence Electrons - electrons in outer shell Electronegativity
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Lecture 3 - Lecture 3 Guide September 1 (HOME) Starting...

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