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Chapter 18: Q18.10-95 E (page 1047)
Oxygen forms double bonds in\({{\rm{O}}_2}\), but sulfur forms single bonds in \({{\rm{S}}_8}\). Why?
Due to its size, S-S \(\pi \) bonds are not possible.
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Write the Lewis structure for each of the following. You may wish to review the chapter on chemical bonding and molecular geometry.
(a)\(P{H_3}\).
(b)\(P{H_4} + \).
(c)\({P_2}{H_4}\).
(d)\(P{O_4}^3 - \)
(e)\(P{F_5}\)
Why is it necessary to keep the chlorine and sodium, resulting from the electrolysis of sodium chloride, separate during the production of sodium metal?
A hydride of silicon prepared by the reaction of \({\rm{M}}{{\rm{g}}_2}{\rm{Si}}\) with acid exerted a pressure of 306 torr at \({26^\circ }{\rm{C}}v\)in a bulb with a volume of\(57.0\;{\rm{mL}}\). If the mass of the hydride was\(0.0861\;{\rm{g}}\), what is its molecular mass? What is the molecular formula for the hydride?
Why does phosphorous acid form only two series of salts, even though the molecule contains three hydrogen atoms?
Write a balanced chemical equation for the reaction of an excess of oxygen with each of the following.
Remember that oxygen is a strong oxidizing agent and tends to oxidize an element to its maximum oxidation state.
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