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Unformatted text preview: of metals and nonmetals ‐ Location on Periodic Table and properties atomic # (Z): # of protons=# of electrons • Know which elements exist as solids, liquids, gases at room temperature (25˚C) • Determine # of protons, neutrons, and electrons for any given isotope. • Know the names and symbols for all elements included on p. 10 in the Ch. 4 lecture notes, Ti (titanium), and Sr (strontium), and uranium (U). Spelling counts! • Give atomic notation for any element given element name/symbol and mass number Chapter 9 wavelength (λ): distance between peaks frequency (ν): number of crests passing by a given point in 1 s CHEM121 Exam 1 Study Guide Wavelength (λ) is inversely related to frequency (ν) and energy (E): – As λ↑ → ν↓, Ε↓ or As λ↓ → ν↑, Ε↑ page 3 of 4 Chapter 9 (Continued) Electromagnetic Spectrum: – continuum of radiant energy – gamma (γ) rays to radio waves – The visible spectrum makes up a small portion – Red light at 700 nm is lower in energy than blue light at 400 nm. Know the people and ideas associated with the Classical Model of Matter – John Dalton, JJ Thomson, Ernest Rutherford, James Maxwell Max Planck and Quantum Theory – Planck proposed energy is absorbed and emitted as bundles = quanta – single bundle of energy = quantum Einstein and the Photoelectric Effect – Be able to describe the Photoelectric Effect – Experimental evidence for light existing as particles = photons Bohr Theory of the Atom – Electrons move in quantized orbits called “energy levels” around the nucleus. – ground state: electron(s) fill the lowest energy level(s) before filling higher level(s) – When an atom absorbs energy, electron jumps from lower energy to higher energy level. – When an electron drops from a higher energy to lower energy level, it releases energy, in some cases as light → atomic emission spectra – Know the limitations of the...
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This document was uploaded on 03/22/2014 for the course CHEM 12 at Seattle Central Community College.

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