Chapter 8: Q4 E (page 451)
A typical barometric pressure in Redding, California, is about 750mm Hg. Calculate this pressure in atm and kPa.
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Draw the Lewis structures for \({\rm{C}}{{\rm{O}}_{\rm{2}}}\)and\({\rm{CO}}\), and predict the number of \({\rm{\sigma }}\) and \({\rm{\pi }}\) bonds for each molecule.
(a) \({\rm{C}}{{\rm{O}}_{\rm{2}}}\)
(b) \({\rm{CO}}\)
Consider nitrous acid, \({\rm{HN}}{{\rm{O}}_{\rm{2}}}{\rm{(HONO)}}\). (a) Write a Lewis structure. (b) What are the electron pair and molecular geometries of the internal oxygen and nitrogen atoms in the \({\rm{HN}}{{\rm{O}}_{\rm{2}}}\) molecule? (c) What is the hybridization on the internal oxygen and nitrogen atoms in \({\rm{HN}}{{\rm{O}}_{\rm{2}}}\)?
If molecular orbitals are created by combining five atomic orbitals from atom A and five atomic orbitals from atom B combine, how many molecular orbitals will result?
True or false: Boron contains \({\rm{2}}{{\rm{s}}^{\rm{2}}}{\rm{2}}{{\rm{p}}^{\rm{1}}}\)valence electrons, so only one \({\rm{p}}\)- orbital is needed to form molecular orbitals.
For many years after they were discovered, it was believed that the noble gases could not form compounds. Now we know that belief to be incorrect. A mixture of xenon and fluorine gases, confined in a quartz bulb and placed on a windowsill, is found to slowly produce a white solid. Analysis of the compound indicates that it contains \({\rm{77}}{\rm{.55\% }}\)Xe and \({\rm{22}}{\rm{.45\% \;F}}\)by mass.
(a) What is the formula of the compound?
(b) Write a Lewis structure for the compound.
(c) Predict the shape of the molecules of the compound.
(d) What hybridization is consistent with the shape you predicted?
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