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Chapter 2: Problem 71

Name the following ionic compounds: (a) \(\mathrm{Li}_{2} \mathrm{O},\) (b) \(\mathrm{FeCl}_{3}\), (c) \(\mathrm{NaClO}\) (d) \(\mathrm{CaSO}_{3}\), (e) \(\mathrm{Cu}(\mathrm{OH})_{2}\) (f) \(\mathrm{Fe}\left(\mathrm{NO}_{3}\right)_{2}\), (g) \(\mathrm{Ca}\left(\mathrm{CH}_{3} \mathrm{COO}\right)_{2}\) (h) \(\mathrm{Cr}_{2}\left(\mathrm{CO}_{3}\right)_{3}\) (i) $\mathrm{K}_{2} \mathrm{CrO}_{4},(\mathbf{j})\left(\mathrm{NH}_{4}\right)_{2} \mathrm{SO}_{4}$.

Short Answer

Expert verified
(a) Lithium Oxide, (b) Iron(III) Chloride, (c) Sodium Hypochlorite, (d) Calcium Sulfite, (e) Copper(II) Hydroxide, (f) Iron(II) Nitrate, (g) Calcium Acetate, (h) Chromium(III) Carbonate, (i) Potassium Chromate, (j) Ammonium Sulfate.

Step by step solution

01

(a) Naming \(\mathrm{Li}_{2} \mathrm{O}\)

The compound \(\mathrm{Li}_{2} \mathrm{O}\) consists of two ions: lithium (Li) and oxygen (O). In the name, start with the cation, lithium. The anion oxygen exists as oxide. The name of this ionic compound is Lithium Oxide.
02

(b) Naming \(\mathrm{FeCl}_{3}\)

The compound \(\mathrm{FeCl}_{3}\) consists of iron (Fe) and chlorine (Cl). Iron is a transition metal that requires a Roman numeral in its name to indicate its charge. In this case, the charge on the iron ion is +3 (since there are 3 chlorides with a charge of -1 each). Call the ion Iron(III). Chlorine forms the chloride anion. The compound is named Iron(III) Chloride.
03

(c) Naming \(\mathrm{NaClO}\)

The compound \(\mathrm{NaClO}\) consists of sodium (Na) and the polyatomic anion called hypochlorite (ClO). The name of this ionic compound is Sodium Hypochlorite.
04

(d) Naming \(\mathrm{CaSO}_{3}\)

The compound \(\mathrm{CaSO}_{3}\) consists of calcium (Ca) and the polyatomic anion called sulfite (SO\(_3\)). The name of this ionic compound is Calcium Sulfite.
05

(e) Naming \(\mathrm{Cu}(\mathrm{OH})_{2}\)

The compound \(\mathrm{Cu}(\mathrm{OH})_{2}\) consists of copper (Cu) and the polyatomic anion called hydroxide (OH). Copper is a transition metal, and its charge is +2 (since there are two hydroxides with a charge of -1 each). The name of the copper ion is Copper(II). The name of this ionic compound is Copper(II) Hydroxide.
06

(f) Naming \(\mathrm{Fe}\left(\mathrm{NO}_{3}\right)_{2}\)

The compound \(\mathrm{Fe}\left(\mathrm{NO}_{3}\right)_{2}\) consists of iron (Fe) and the polyatomic anion called nitrate (NO\(_3\)). Iron, as a transition metal, has a charge of +2 in this compound (since there are two nitrates with a charge of -1 each). The name of the iron ion is Iron(II). This ionic compound is Iron(II) Nitrate.
07

(g) Naming \(\mathrm{Ca}\left(\mathrm{CH}_{3}\mathrm{COO}\right)_{2}\)

The compound \(\mathrm{Ca}\left(\mathrm{CH}_{3}\mathrm{COO}\right)_{2}\) consists of calcium (Ca) and the polyatomic anion called acetate (CH\(_3\)COO). The name of this ionic compound is Calcium Acetate.
08

(h) Naming \(\mathrm{Cr}_{2}\left(\mathrm{CO}_{3}\right)_{3}\)

The compound \(\mathrm{Cr}_{2}\left(\mathrm{CO}_{3}\right)_{3}\) consists of chromium (Cr) and the polyatomic anion called carbonate (CO\(_3\)). Chromium is a transition metal and has a charge of +3 in this compound (since there are three carbonates with a charge of -2 each). The name of the chromium ion is Chromium(III). This ionic compound is Chromium(III) Carbonate.
09

(i) Naming \(\mathrm{K}_{2} \mathrm{CrO}_{4}\)

The compound \(\mathrm{K}_{2} \mathrm{CrO}_{4}\) consists of potassium (K) and the polyatomic anion called chromate (CrO\(_4\)). The name of this ionic compound is Potassium Chromate.
10

(j) Naming \(\left(\mathrm{NH}_{4}\right)_{2} \mathrm{SO}_{4}\)

The compound \(\left(\mathrm{NH}_{4}\right)_{2} \mathrm{SO}_{4}\) consists of the polyatomic cation ammonium (NH\(_4\)) and the polyatomic anion called sulfate (SO\(_4\)). The name of this ionic compound is Ammonium Sulfate.

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Most popular questions from this chapter

Predict whether each of the following compounds is molecular or ionic: $(\mathbf{a}) \mathrm{BI}_{3}(\mathbf{b}) \mathrm{N}\left(\mathrm{CH}_{3}\right)_{3}(\mathbf{c}) \mathrm{Zr}\left(\mathrm{NO}_{3}\right)_{2}\( (d) \)\mathrm{N}_{2} \mathrm{H}_{4}(\mathbf{e})\( \)\mathrm{OsCO}_{3}(\mathbf{f}) \mathrm{H}_{2} \mathrm{SO}_{4}(\mathbf{g}) \mathrm{HgS}(\mathbf{h}) \mathrm{IOH}$

What fraction of the \(\alpha\) particles in Rutherford's gold foil experiment are scattered at large angles? Assume the gold foil is two layers thick, as shown in Figure \(2.9,\) and that the approximate diameters of a gold atom and its nucleus are 270 \(\mathrm{pm}\) and \(1.0 \times 10^{-2} \mathrm{pm}\), respectively. Assume that the gold nuclei in each layer are offset from each other.

The oxides of nitrogen are very important components in urban air pollution. Name each of the following compounds: (a) \(\mathrm{N}_{2} \mathrm{O}\) \(,(\mathbf{b}) \mathrm{NO}\) (c) \(\mathrm{NO}_{2}\) (d) \(\mathrm{N}_{2} \mathrm{O}_{5}\) (e) $\mathrm{N}_{2} \mathrm{O}_{4}$

From the following list of elements $-\mathrm{Mg}, \mathrm{Li}, \mathrm{T}, \mathrm{Pb}, \mathrm{Se}, \mathrm{Cl}, \mathrm{Xe}, \mathrm{Si},$ C-pick the one that best fits each description. Use each element only once: (a) an alkali metal, \((\mathbf{b})\) an alkaline earth metal, \((\mathbf{c})\) a noble gas, (d) a halogen, \((\mathbf{e})\) a metalloidin group \(14,(\mathbf{f})\) a nonmetal listed in group \(14,(\mathbf{g})\) a metal that forms a \(3+\) ion, \((\mathbf{h})\) a nonmetal that forms a 2 - ion, (i) an element that is used as radiation shielding.

There are two different isotopes of bromine atoms. Under normal conditions, elemental bromine consists of \(\mathrm{Br}_{2}\) molecules, and the mass of a \(\mathrm{Br}_{2}\) molecule is the sum of the masses of the two atoms in the molecule. The mass spectrum of \(\mathrm{Br}_{2}\) consists of three peaks: $$ \begin{array}{lc} \hline \text { Mass (u) } & \text { Relative Size } \\ \hline 157.836 & 0.2569 \\ 159.834 & 0.4999 \\ 161.832 & 0.2431 \\ \hline \end{array} $$ (a) What is the origin of each peak (of what isotopes does each consist)? (b) What is the mass of each isotope? (c) Determine the average molecular mass of a \(\mathrm{Br}_{2}\) molecule. (d) Determine the average atomic mass of a bromine atom. (e) Calculate the abundances of the two isotopes.
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