Chapter 9: Problem 31
Why must all six atoms in \(\mathrm{C}_{2} \mathrm{H}_{4}\) lie in the same plane?
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Key Concepts
These are the key concepts you need to understand to accurately answer the question.
Chapter 9: Problem 31
Why must all six atoms in \(\mathrm{C}_{2} \mathrm{H}_{4}\) lie in the same plane?
These are the key concepts you need to understand to accurately answer the question.
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Get started for freeComplete the Lewis structures of the following molecules. Predict the molecular structure, polarity, bond angles, and hybrid orbitals used by the atoms marked by asterisks for each molecule. a. \(\mathrm{BH}_{3}\) b. \(\mathrm{N}_{2} \mathrm{~F}_{2}\) c. \(\mathrm{C}_{4} \mathrm{H}_{6}\)
Explain the difference between the \(\sigma\) and \(\pi\) MOs for homonuclear diatomic molecules. How are bonding and antibonding orbitals different? Why are there two \(\pi\) MOs and one \(\sigma\) MO? Why are the \(\pi\) MOs degenerate?
Values of measured bond energies may vary greatly depending on the molecule studied. Consider the following reactions: $$ \begin{array}{cc} \mathrm{NCl}_{3}(g) \longrightarrow \mathrm{NCl}_{2}(g)+\mathrm{Cl}(g) & \Delta H=375 \mathrm{~kJ} / \mathrm{mol} \\ \mathrm{ONCl}(g) \longrightarrow \mathrm{NO}(g)+\mathrm{Cl}(g) & \Delta H=158 \mathrm{~kJ} / \mathrm{mol} \end{array} $$ Rationalize the difference in the values of \(\Delta H\) for these reactions, even though each reaction appears to involve only the breaking of one \(\mathrm{N}-\mathrm{Cl}\) bond. (Hint: Consider the bond order of the NO bond in ONCl and in NO.)
Use the localized electron model to describe the bonding in \(\mathrm{H}_{2} \mathrm{CO}\) (carbon is the central atom).
Determine the molecular structure and hybridization of the central atom \(\mathrm{X}\) in the polyatomic ion \(\mathrm{XY}_{3}+\) given the following information: A neutral atom of \(\mathrm{X}\) contains 36 electrons, and the element \(Y\) makes an anion with a \(1-\) charge, which has the electron configuration \(1 s^{2} 2 s^{2} 2 p^{6}\).
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