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0 bond order is not stable if positive charge one

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0 bond order is not stable if positive charge, one less electron, if negative charge, one more electron 14.3 bonding in homonuclear diatomic molecules two identical atoms order of MO: sigma2s, sigma2s anti, sigma2p, 2 pi2p, 2 pi2p anti, sigma2p anti paramagnetism-causes substance to be attracted toward the induced magnetic field unpaired electrons diamagnetism- substance to be repelled from the inducing magnetic field paired electrons for B2, C2, and N2, the sigma2p and the 2 pi2p orbitals are switched p-s mixing sigma2s orbital will repel any electrons placed in the sigma2p orbital, thus making this  orbital less attractive (higher in energy) to electrons sigma2s orbitals are pushed to a higher energy level than the pi2p orbitals which do not  have electron probability between the nuclei and are not affected by electrons in the  sigma2s orbital diatomic molecules definite correlations between bond order, bond energy, and bond length as MO model increases, bond energy increases, and bond length decreases correlation of bond energies of B2 and F2 molecules indicate the bond order cannot  automatically be associated with a particular bond energy large bond energy with N2 because of triple bond, thus very stable O2 molecule is known to be paramagnetic 14.4 bonding in heteronuclear diatomic molecules slightly tilted, but acts the same way 14.5 combining the localized electron and molecular orbital models localized- restricted to the space between a given pair of atoms sigma electrons can be described as localized with no problems but the pi electrons  must be treated as being delocalized
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03:14 Chapter 15:Chemical Kinetics
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03:14 Spontaneous does not mean fast Chemical kinetics- area of chemistry that is concerned with reaction rates Steps by which a reaction takes is called the reaction mechanism 15.1 reaction rates speed  or rate of a process is defined as the change in a given quantity over a specified  period of time volume remains constant, it is the change in the number of moles per unit of volume per  unit of time reaction rate- (concentration of A at time t2 – concentration of A at time t1)/(t2-t1) change in concentration/change in time add negative because the rates are positive -change in conc/change in time instantaneous rate- value of rate at particular time can be obtained by computing the slope of a line tangent to the curve at that point 15.2 introduction to rate laws chemical reactions are reversible the reaction rates ONLY depend on the concentration, not time rate law=k[concentration(reactants)]^n k is proportionalirt constant n is order of reactant concentrations of products do not appear in rate law n must be determined by experiment
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