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Atomic Theory Unit Study Guide CP Chemistry Spring 2012 Terms to Know absorption spectrum continuous spectrum electromagnetic spectrum emission spectrum energy level excitation excited state frequency ground state The “Big Idea” I. Our understanding of the structure of matter has changed and continues to change as new data contradicts existing theories. line spectrum photon relaxation wavelength Aufbau principle angular momentum quantum number Hund's rule magnetic quantum number Pauli exclusion principle principle quantum number quantum theory spin quantum number Uncertainty Principle wave mechanical theory group halogen lanthanide main group elements noble gas actinide orbital alkali metal alkaline earth metal period transition metals What you need to know about it. 1. Describe the major theories of the structure of matter from the ancient Greeks through the present and name the principal theorist. 2. Arrange the major atomic models in chronological order, describe the evidence that supported the model and explain why the model was modified or abandoned. 3. Describe why Rutherford's metal foil experiments forced Dalton’s and Thomson’s models of atomic structure to be replaced with a nuclear model of the atom. 4. Describe the uses and limitations of the Bohr model, particularly as it related to the quantization of electron energies. 5. Use examples from the history of the development of atomic theory to explain how scientific theories are modified or replaced, and identify two or more barriers to acceptance of new theories. 1. Describe the structure of the atom in terms of protons, neutrons, and electrons and identify the charge and relative mass of each particle. 2. Use ZAX notation to determine number of protons, neutrons, and electrons and identify the element from a periodic table. II. All neutral atoms of an element have the same number of electrons and protons, but the number of neutrons varies. 3. Write the ZAX notation of any isotope. 4. Calculate the average atomic mass of a naturally occurring element given the relative abundance of each isotope. 5. Calculate the relative abundance of isotopes given the average atomic mass. 6. Write the balanced nuclear equations for the nuclear decay processes of α particle production, β particle production, γ ray production, positron production and electron capture. 7. Calculate the half-life of an isotope given the time it takes for the isotope to decay, or the amount of the starting amount of an isotope remaining given the half-life. Page 1 Atomic Theory Unit Study Guide The “Big Idea” CP Chemistry Spring 2012 What you need to know about it. 1. Write the equations that relate wavelength, frequency, amplitude, and velocity of electromagnetic radiation. 2. Label regions of the electromagnetic spectrum as radio waves, infrared, visible, ultraviolet, x-ray and gamma radiation and identify the frequency, wavelength and energy of light for each region identified above. 3. Contrast the following pairs of terms III. Electromagnetic radiation is the result of energy transitions at the atomic level. a. b. c. d. e. ground state vs. excited state excitation vs. relaxation absorption vs. emission line spectra vs. and continuous spectra absorption vs. emission spectra. 4. Calculate the energy of absorption and emission spectral lines of the hydrogen atom, and identify the electron transitions that caused the lines. 5. Describe the concept of wave-particle duality, and relate the DeBroglie wavelength of a wave or particle to its momentum. 6. Describe the photoelectric effect, including what changes in the effect result from variation of the incident light frequency and intensity and how it provides evidence for photons. 7. Calculate the energy of an emitted or absorbed photon from the initial and final energy levels of a molecule or atom. IV. Each electron in an atom has a unique quantum number, which describes its probable position and energy. 1. Describe the nature and relationship of the principal (n), azimuthal (l), and magnetic (ml) quantum numbers to solutions of the Schrödinger Wave Equation, and identify which orbital properties are determined by each of these numbers. 2. Name orbitals given its quantum numbers, or identify quantum numbers for given orbital. 3. Sketch the relative shapes, sizes, and spatial orientations of s, p, and d orbitals of the hydrogen atom. 4. Apply the concept of effective nuclear charge, Zeff, to describe the difference in orbital energies between single and multi-electron systems. 5. Define the Pauli Exclusion Principle, the Aufbau Principle, and Hund’s Rule and explain the accepted scientific rationale for each. 1. Apply the Aufbau principle to predict the ground state electronic configuration of any element. V. The periodic table of elements is organized based on electron structure. 2. Locate any unknown element on the periodic table based on its electron configuration. 3. Identify alkali metals, alkaline earth metals, halogens, noble gases, main group elements, transition metals, and lanthanides & actinides on a blank periodic table. 4. Describe the electron configuration of elements that belong to each of the groups identified above. Page 2