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Chapter 3: Problem 30

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

Short Answer

Expert verified
The correct names for the given compounds are: a. Dinitrogen monoxide: the other names are incorrect as they either do not specify the number of atoms or inappropriately use oxidation states for nitrogen. b. Copper(I) oxide: transition metals like copper have different oxidation states, making it necessary to indicate the oxidation state. The other names either lack this detail or use inappropriate naming conventions. c. Lithium oxide: lithium has a fixed oxidation state of +1, making the use of Roman numerals unnecessary, and the IUPAC naming convention does not involve "di" or "mono" prefixes for such ionic binary compounds.

Step by step solution

01

a. Correct name for \(\mathrm{N}_{2} \mathrm{O}\)

The correct name for \(\mathrm{N}_{2} \mathrm{O}\) is dinitrogen monoxide. The reason behind this choice is that the IUPAC nomenclature rules for inorganic compounds require the use of prefixes denoting the number of atoms of each element present in the compound. In this case, we have two nitrogen atoms, thus the prefix "di" for nitrogen, and one oxygen atom, leading to the prefix "mono" for oxygen.
02

a. Incorrect names for \(\mathrm{N}_{2} \mathrm{O}\) and why

1. Nitrogen oxide: This name is incorrect because it does not specify the number of nitrogen and oxygen atoms, making it ambiguous. 2. Nitrogen(I) oxide: This name is not appropriate because the Roman numeral "(I)" represents the oxidation state of nitrogen. However, in this compound, nitrogen has an oxidation state of +1 while the other nitrogen has an oxidation state of -1, so using the oxidation state in the name would not be suitable here.
03

b. Correct name for \(\mathrm{Cu}_{2} \mathrm{O}\)

The correct name for \(\mathrm{Cu}_{2} \mathrm{O}\) is copper(I) oxide. Copper is a transition metal, and its compounds can have different oxidation states. In this case, copper has an oxidation state of +1 (due to only one oxygen atom), which is represented by the Roman numeral (I) in the compound's name.
04

b. Incorrect names for \(\mathrm{Cu}_{2} \mathrm{O}\) and why

1. Copper oxide: This name is incorrect because it does not indicate the oxidation state of copper, which is necessary for transition metal compounds. 2. Dicopper monoxide: This name would be used if Cu had a fixed oxidation state like Li in \(\mathrm{Li}_{2} \mathrm{O}\). However, it is not used in this context as copper has variable oxidation states, and the IUPAC naming convention relies on indicating the oxidation states of these elements.
05

c. Correct name for \(\mathrm{Li}_{2} \mathrm{O}\)

The correct name for \(\mathrm{Li}_{2} \mathrm{O}\) is lithium oxide. Lithium is an alkali metal, and it always has a fixed oxidation state of +1 in its compounds. In this compound, there are two lithium atoms, and they form an ionic bond with one oxygen atom, which has an oxidation state of -2. Since lithium only has one possible oxidation state, there is no need to include the oxidation state in the compound's name.
06

c. Incorrect names for \(\mathrm{Li}_{2} \mathrm{O}\) and why

1. Lithium(I) oxide: This name is incorrect because including the Roman numeral (I) is unnecessary, as lithium has only one possible oxidation state in its compounds, which is +1. 2. Dilithium monoxide: This name is not used because the IUPAC naming convention for ionic binary compounds formed by metals with a fixed oxidation state does not involve inserting "di" or "mono" prefixes for the involved elements.

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Most popular questions from this chapter

Indicate the bond polarity (show the partial positive and partial negative ends) in the following bonds. a. \(C-O\) b. \(P-H\) \(\mathbf{c} . \quad \mathbf{H}-\mathbf{C l}\) d. \(\mathrm{Br}-\mathrm{Te}\) \(\mathbf{e} . \mathbf{S e}-\mathbf{S}\)

Predict the empirical formulas of the ionic compounds formed from the following pairs of elements. Name each compound. a. Al and Cl b. Na and O c. Sr and F d. Ca and Se

For each of the following groups, place the atoms and/or ions in order of decreasing size. a. \(\mathrm{V}, \mathrm{V}^{2+}, \mathrm{V}^{3+}, \mathrm{V}^{5+}\) b. \(\mathrm{Na}^{+}, \mathrm{K}^{+}, \mathrm{Rb}^{+}, \mathrm{Cs}^{+}\) c. \(\mathrm{Te}^{2-}, \mathrm{I}^{-}, \mathrm{Cs}^{+}, \mathrm{Ba}^{2+}\) d. \(P, P, P^{2}, P^{3}\) e. \(\mathrm{O}^{2-}, \mathrm{S}^{2-}, \mathrm{Se}^{2-}, \mathrm{Te}^{2-}\)

Write Lewis structures for the following. Show all resonancestructures where applicable.a. \(\mathrm{NO}_{2}^{-}, \mathrm{NO}_{3}^{-}, \mathrm{N}_{2} \mathrm{O}_{4}\left(\mathrm{N}_{2} \mathrm{O}_{4} \text { exists as } \mathrm{O}_{2} \mathrm{N}-\mathrm{NO}_{2} .\right)\) b. \(\mathrm{OCN}^{-}, \mathrm{SCN}^{-}, \mathrm{N}_{3}^{-}\) (Carbon is the central atom in \(\mathrm{OCN}^{-}\) and \(\mathrm{SCN}^{-} .\) )

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
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