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Chapter 2: Problem 105

Because many ions and compounds have very similar names, there is great potential for confusing them. Write the correct chemical formulas to distinguish between (a) calcium sulfide and calcium hydrogen sulfide, (b) hydrobromic acid and bromic acid, (c) aluminum nitride and aluminum nitrite, (d) iron(II) oxide and iron(III) oxide, (e) ammonia and ammonium ion, (f) potassium sulfite and potassium bisulfite, (g) mercurous chloride and mercuric chloride, (h) chloric acid and perchloric acid.

Short Answer

Expert verified
The correct chemical formulas for the given ions and compounds are: (a) Calcium sulfide: \(CaS\); Calcium hydrogen sulfide: \(Ca(HS)_2\) (b) Hydrobromic acid: \(HBr\); Bromic acid: \(HBrO3\) (c) Aluminum nitride: \(AlN\); Aluminum nitrite: \(Al(NO2)_3\) (d) Iron(II) oxide: \(FeO\); Iron(III) oxide: \(Fe2O3\) (e) Ammonia: \(NH3\); Ammonium ion: \(NH4^+\) (f) Potassium sulfite: \(K2SO3\); Potassium bisulfite: \(KHSO3\) (g) Mercurous chloride: \(Hg2Cl2\); Mercuric chloride: \(HgCl2\) (h) Chloric acid: \(HClO3\); Perchloric acid: \(HClO4\)

Step by step solution

01

(a) Calcium sulfide and calcium hydrogen sulfide

Calcium sulfide has one calcium ion (Ca^2+) and one sulfide ion (S^2-). To write its formula, we simply combine these ions together and balance them by their charges: Ca^2+ + S^2- -> \(CaS\) Calcium hydrogen sulfide contains one calcium ion (Ca^2+) and one hydrogen sulfide ion (HS^-). To write its formula, we combine the ions together and balance them by their charges: Ca^2+ + 2(HS^-) -> \(Ca(HS)_2\)
02

(b) Hydrobromic acid and bromic acid

Hydrobromic acid is formed when a hydrogen ion (H^+) combines with a bromide ion (Br^-): H^+ + Br^- -> \(HBr\) Bromic acid is formed when a hydrogen ion (H^+) combines with a bromate ion (BrO3^-): H^+ + BrO3^- -> \(HBrO3\)
03

(c) Aluminum nitride and aluminum nitrite

Aluminum nitride has one aluminum ion (Al^3+) and one nitride ion (N^3-). To write its formula, we simply combine these ions together and balance them by their charges: Al^3+ + N^3- -> \(AlN\) Aluminum nitrite contains one aluminum ion (Al^3+) and one nitrite ion (NO2^-). To write its formula, we combine the ions together and balance them by their charges: Al^3+ + 3(NO2^-) -> \(Al(NO2)_3\)
04

(d) Iron(II) oxide and iron(III) oxide

Iron(II) oxide has one iron(II) ion (Fe^2+) and one oxide ion (O^2-). To write its formula, we simply combine these ions together and balance them by their charges: Fe^2+ + O^2- -> \(FeO\) Iron(III) oxide has one iron(III) ion (Fe^3+) and one oxide ion (O^2-). To write its formula, we combine the ions together and balance them by their charges: 2(Fe^3+) + 3(O^2-) -> \(Fe2O3\)
05

(e) Ammonia and ammonium ion

Ammonia is a neutral molecule with the chemical formula: \(NH3\) Ammonium ion is formed when ammonia molecule gains a hydrogen ion (H^+): \(NH3\) + H^+ -> \(NH4^+\)
06

(f) Potassium sulfite and potassium bisulfite

Potassium sulfite contains one potassium ion (K^+) and one sulfite ion (SO3^2-). To write its formula, we combine the ions together and balance them by their charges: 2(K^+) + SO3^2- -> \(K2SO3\) Potassium bisulfite contains one potassium ion (K^+) and one hydrogen sulfite ion (HSO3^-). To write its formula, we combine the ions together and balance them by their charges: K^+ + HSO3^- -> \(KHSO3\)
07

(g) Mercurous chloride and mercuric chloride

Mercurous chloride (also known as mercury(I) chloride) has one mercury(I) ion (Hg2^2+) and two chloride ions (Cl^-). To write its formula, we combine the ions together and balance them by their charges: Hg2^2+ + 2(Cl^-) -> \(Hg2Cl2\) Mercuric chloride (also known as mercury(II) chloride) has one mercury(II) ion (Hg^2+) and two chloride ions (Cl^-). To write its formula, we combine the ions together and balance them by their charges: Hg^2+ + 2(Cl^-) -> \(HgCl2\)
08

(h) Chloric acid and perchloric acid

Chloric acid is formed when a hydrogen ion (H^+) combines with a chlorate ion (ClO3^-): H^+ + ClO3^- -> \(HClO3\) Perchloric acid is formed when a hydrogen ion (H^+) combines with a perchlorate ion (ClO4^-): H^+ + ClO4^- -> \(HClO4\)

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Most popular questions from this chapter

Complete the table by filling in the formula for the ionic compound formed by each pair of cations and anions, as shown for the first pair. $$ \begin{array}{|l|c|c|c|c|} \hline \text { Ion } & \mathrm{K}^{+} & \mathrm{NH}_{4}^{+} & \mathrm{Mg}^{2+} & \mathrm{Fe}^{3+} \\ \hline \mathrm{Cl}^{-} & \mathrm{KCl} & & & \\ \hline \mathrm{OH}^{-} & & & & \\ \hline \mathrm{CO}_{3}^{2-} & & & & \\ \hline \mathrm{PO}_{4}{ }^{3-} & & & & \\ \hline \end{array} $$

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) \(\mathrm{K}_{2} \mathrm{CrO}_{4},(\mathrm{j})\left(\mathrm{NH}_{4}\right)_{2} \mathrm{SO}_{4}\)

The element oxygen has three naturally occurring isotopes, with \(8,9,\) and 10 neutrons in the nucleus, respectively. (a) Write the full chemical symbols for these three isotopes. (b) Describe the similarities and differences between the three kinds of atoms of oxygen.

Naturally occurring magnesium has the following isotopic abundances: $$ \begin{array}{ccc} \hline \text { Isotope } & \text { Abundance } & \text { Atomic mass (amu) } \\\ \hline{ }^{24} \mathrm{Mg} & 78.99 \% & 23.98504 \\ { }^{25} \mathrm{Mg} & 10.00 \% & 24.98584 \\ { }^{26} \mathrm{Mg} & 11.01 \% & 25.98259 \\ \hline \end{array} $$ (a) What is the average atomic mass of \(\mathrm{Mg}\) ? (b) Sketch the mass spectrum of \(\mathrm{Mg}\).

A chemist finds that \(30.82 \mathrm{~g}\) of nitrogen will react with \(17.60 \mathrm{~g}\), \(35.20 \mathrm{~g}, 70.40 \mathrm{~g},\) or \(88.00 \mathrm{~g}\) of oxygen to form four different compounds. (a) Calculate the mass of oxygen per gram of nitrogen in each compound. (b) How do the numbers in part (a) support Dalton's atomic theory?
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