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6

There are two ways to look at the $\ce{SO2}$ molecule. The valence bond way is this: $\ce{SO2}$ is a bent molecule with C2v symmetry point group. A valence bond theory approach considering just s and p orbitals describes the bonding in terms of resonance between two resonance structures: The sulfur–oxygen bond has a bond order of 1.5 and does not invoke d ...


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What you have calculated is the energy required to make two separated ions out of two separated $\ce{Na}$ ad $\ce{Cl}$ atoms. When they are separated, these ions do not make a molecule or a crystal of salt. Separated ions attract one another and are able to release a huge amount of Coulomb energy when approaching each other. Anyhow your calculation should ...


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The kinetic energy is not ignored. Each quantized state (labeled by the vibrational quantum number) has a total energy given by the expectation value of the Hamiltonian operator for the wavefunction. The contribution of the kinetic energy can be computed as the expectation value of the QM kinetic energy operator, or as the difference between the expectation ...


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Getting to know the superoxide anion radical Hayyan et al. (2016) have studied and characterized the formation of the superoxide anion radical, $\ce{O2^.-}$. This chemical entity forms as a result of the reduction of diatomic oxygen $\ce{O2 + e^- -> O2^.-}$ There is some conflicting data on the reactivity of this radical, however it can be isolated: A ...


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Greg is quite correct: no clear question. But sometimes you don't know enough to define a question clearly. The implicit question is: "Is this mechanism helpful or even correct?" The second, clear, question, is why does rusting take time to happen. I think the answer to the first, implicit, question is that it is a start, but far from helpful and ...


2

The curves labelled Harmonic/Morse show how the potential energy changes with internuclear separation, and the horizontal lines are the allowed total energies, potential plus kinetic. The potential energy is a maximum at the turning points (end of the horizontal lines in your picture) and zero at the $r_e$ value but because the total energy is constant the ...


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For many of the compounds that you encounter in a first-year chemistry course, yes, this is the case, as satisfying the octet rule usually results in stability through full s- and p-orbitals. However, this is definitely not a guarantee Some common examples include nitrogen compounds due to its odd number of electrons in its ground state, such as $\ce{NO}$ ...


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There are two factors here to consider. First, the energy released by a given reaction is (partly) due to the difference between the bond strength in the product vs reactant, not the absolute bond strength, unless the reaction involves just breaking a bond and not forming a new one. Second, even if your reaction is just a bond breaking, there are multiple ...


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First of all, multiple intermolecular forces could be present between molecules, and, yes, all forces influence attraction, binding and etc. However, if you study any chemical system, you will see that is usually dynamic. It all depends on conditions like temperature, pH and especially compound properties, etc. For example, the drug captopril (an ...


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In principle, when studying a structure like HCl, CH3COOH, or any other compound, the first thing to do is drawing the symbol of the atoms in a reasonable geometry on a sheet of paper. Then consider the outer electron layers : put enough points around each symbol to get a reasonable Lewis structure. For example, one point near $\ce{H}$ and six points around $...


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I have carried out a calculation of NO43- (B3LYP/ccpVTZ) followed by the ELF population analysis. This method provides a partition of the electron density which is consistent with the Lewis's picture. The valence shell of N is the union of 4 V(N,O) basins each with a population of 1.375 e-, the total population of the nitrogen valence shell is, accordingly 5....


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