chemical bonding
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The art of balancing equations in chemistry!
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Professor Sylvia Ceyer discusses bond enthalpy and the enthalpy of endothermic/exothermic chemical reactions. The heat of formation is defined as Professor Ceyer explains Hess's Law which is used to predict the enthalpy change and conservation of energy, regardless of the path through which it is to be determined. The lecture concludes with a discussion of thermodynamics and spontaneous chance, specifically Gibbs free energy and the concep...more
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Environmental Politics and Law (EVST 255) The lecture critiques the U.S. Green Building Council's (USGBC) certification system, LEED (Leadership in Energy and Environmental Design). The criteria for being highly rated under LEED emphasize energy efficiency and minimizing waste, but do not prioritize environmental health and limiting use of dangerous plastics and chemicals. USGBC is a non-profit organization, not a government agency, and...more
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This lecture brings experiment to bear on the previous theoretical discussion of bonding by focusing on hybridization of the central atom in three XH3 molecules. Because independent electron pairs must not overlap, hybridization can be related to molecular structure by a simple equation. The "Umbrella Vibration" and the associated rehybridization of the central atom is used to illustrate how a competition between strong bonds and stable at...more
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Professor Sylvia Ceyer discusses the nature of chemical equilibrium as it relates to free energy, the reaction quotient, and the relationship between K and Q. The meaning of K is further clarified and the external effects on K are identified, from adding and removing reagents to changes associated with the Principle of Le Chatelier.
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Professor Sylvia Ceyer continues her discussion on chemical equilibrium and external effects such as a change in volume, adding inert gas, and a change in temperature. Parameters are set for maximizing the yield of a reaction, and the Principle of Le Chatelier's is returned to. Hemoglobin is used as an example involved in a series of equilibrium reactions in response to oxygen pressure.
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Professor McBride begins by using previous examples of "pathological" bonding and the BH3 molecule to illustrate how a chemist's use of localized bonds, vacant atomic orbitals, and unshared pairs to understand molecules compares with views based on the molecule's own total electron density or on computational molecular orbitals. This lecture then focuses on understanding reactivity in terms of the overlap of singly-occupied molecular orbit...more
