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Chapter 3: Problem 109
Name each of the following compounds: a. \(\mathrm{BaSO}_{3}\) b. \(\mathrm{NaNO}_{2}\) c. \(\mathrm{KMnO}_{4}\) \(\mathbf{d .} \mathbf{K}_{2} \mathrm{Cr}_{2} \mathbf{O}_{7}\)
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The designations \(1 \mathrm{A}\) through \(8 \mathrm{A}\) used for certain families of the periodic table are helpful for predicting the charges on ions in binary ionic compounds. In these compounds, the metals generally take on a positive charge equal to the family number, while the nonmetals take on a negative charge equal to the family number minus \(8 .\) Thus the compound between sodium and chlorine contains \(\mathrm{Na}^{+}\) ions and \(\mathrm{Cl}^{-}\) ions and has the formula NaCl. Predict the formula and the name of the binary compound formed from the following pairs of elements. a. Ca and N b. \(K\) and 0 c. \(\mathrm{Rb}\) and \(\mathrm{F}\) d. \(\mathrm{Mg}\) and \(\mathrm{S}\) e. Ba and I f. Al and Se g. Cs and \(P\) h. In and Br
A polyatomic ion is composed of \(\mathrm{C}, \mathrm{N},\) and an unknown element \(X\). The skeletal Lewis structure of this polyatomic ion is \([\mathrm{X}-\mathrm{C}-\mathrm{N}]^{-} .\) The ion \(\mathrm{X}^{2-}\) has an electron configuration of [Ar]4s^{2} 3 d ^ { 1 0 } 4 p ^ { 6 } . \text { What is element X? Knowing the identity of } X, complete the Lewis structure of the polyatomic ion, including all important resonance structures.
Order the following species with respect to carbon-oxygen bond length (longest to shortest). $$\mathrm{CO}, \quad \mathrm{CO}_{2}, \quad \mathrm{CO}_{3}^{2-}, \quad \mathrm{CH}_{3} \mathrm{OH}$$ What is the order from the weakest to the strongest carbonoxygen bond? \(\left(\mathrm{CH}_{3} \mathrm{OH} \text { exists as } \mathrm{H}_{3} \mathrm{C}-\mathrm{OH} .\right)\)
Without using Fig. \(3-4,\) predict the order of increasing electronegativity in each of the following groups of elements. a. \(C, N, O\) b. \(\mathbf{s}, \mathbf{S e}, \mathbf{C l}\) \(\mathbf{c}_{*} \mathrm{Si}, \mathrm{Ge}, \mathrm{Sn}\) d. \(\mathrm{TI}, \mathrm{S}, \mathrm{Ge}\)
For each of the following, write an equation that corresponds to the energy given. a. lattice energy of \(\mathrm{NaCl}\) b. lattice energy of \(\mathrm{NH}_{4} \mathrm{Br}\) c. lattice energy of \(\mathrm{MgS}\) d. \(O=O\) double bond energy beginning with \(O_{2}(g)\) as a reactant
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