Chapter 3: Problem 16
The common name for \(\mathrm{NH}_{3}\) is ammonia. What would be the systematic name for \(\mathrm{NH}_{3}\) ? Support your answer.
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Chapter 3: Problem 16
The common name for \(\mathrm{NH}_{3}\) is ammonia. What would be the systematic name for \(\mathrm{NH}_{3}\) ? Support your answer.
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Without using Fig. \(3-4,\) predict which bond in each of the following groups will be the most polar. a. \(C-F, S i-F, G e-F\) b. \(P-C\) or \(S-C\) \(\mathbf{c} . \mathbf{S}-\mathbf{F}, \mathbf{S}-\mathbf{C} \mathbf{l}, \mathbf{S}-\mathbf{B r}\) d. \(\mathrm{Ti}-\mathrm{Cl}, \mathrm{Si}-\mathrm{Cl}, \mathrm{Ge}-\mathrm{Cl}\)
Write Lewis structures that obey the octet rule (duet rule for H) for each of the following molecules. Carbon is the central atom in \(\mathrm{CH}_{4}\), nitrogen is the central atom in \(\mathrm{NH}_{3}\), and oxygen is the central atom in \(\mathrm{H}_{2} \mathrm{O}\). a. \(\mathrm{F}_{2}\) \(\mathbf{b} . \mathbf{O}_{2}\) c. CO d. \(\overline{\mathrm{CH}_{4}}\) \(\mathbf{e} . \mathrm{NH}_{3}\) \(\mathbf{f .} \quad \mathbf{H}_{2} \mathbf{O}\) g. IIF
Use the following data for potassium chloride to estimate \(\Delta E\) for the reaction: $$\mathrm{K}(s)+\frac{1}{2} \mathrm{Cl}_{2}(g) \longrightarrow \mathrm{KCl}(s) \quad \Delta E=?$$ Lattice energy Ionization energy for \(\mathbf{K}\) Electron affinity of Cl Bond energy of \(\mathrm{Cl}_{2}\) Energy of sublimation for \(\mathrm{K}\) \(-2913 \mathrm{kJ} / \mathrm{mol}\) \(735 \mathrm{kJ} / \mathrm{mol}\) \(1445 \mathrm{kJ} / \mathrm{mol}\) -328 kJ/mol \(154 \mathrm{kJ} / \mathrm{mol}\) 150\. kJ/mol
Oxidation of the cyanide ion produces the stable cyanate ion, OCN \(^{-}\). The fulminate ion, \(\mathrm{CNO}^{-}\), on the other hand, is very unstable. Fulminate salts explode when struck; \(\mathrm{Hg}(\mathrm{CNO})_{2}\) is used in blasting caps. Write the Lewis structures and assign formal charges for the cyanate and fulminate ions. Why is the fulminate ion so unstable? (C is the central atom in OCN - and \(\mathrm{N}\) is the central atom in \(\mathrm{CNO}^{-} .\) )
Each of the following compounds has three possible names listed for it. For each compound, what is the correct name and why aren't the other names used? a. \(\mathrm{N}_{2} \mathrm{O}\) : nitrogen oxide, nitrogen(I) oxide, dinitrogen monoxide b. \(\mathrm{Cu}_{2} \mathrm{O}:\) copper oxide, copper(I) oxide, dicopper monoxide c. \(\mathrm{Li}_{2} \mathrm{O}:\) lithium oxide, lithium(I) oxide, dilithium monoxide
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