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Chapter 2: Problem 73

Write the chemical formula for each substance mentioned in the following word descriptions (use the front inside cover to find the symbols for the elements you don't know). (a) Zinc carbonate can be heated to form zinc oxide and carbon dioxide. (b) On treatment with hydrofluoric acid, silicon dioxide forms silicon tetrafluoride and water. (c) Sulfur dioxide reacts with water to form sulfurous acid. (d) The substance phosphorus trihydride, commonly called phosphine, is a toxic gas. (e) Perchloric acid reacts with cadmium to form cadmium(II) perchlorate. (f) Vanadium(III) bromide is a colored solid.

Short Answer

Expert verified
(a) ZnCO3 → ZnO + CO2 (b) SiO2 + 4HF → SiF4 + 2H2O (c) SO2 + H2O → H2SO3 (d) PH3 (e) HClO4 + Cd → Cd(ClO4)2 (f) VBr3

Step by step solution

01

(a) Zinc carbonate forming zinc oxide and carbon dioxide

To write the chemical formula for zinc carbonate, we need to find the symbols for zinc and carbonate ions. Zinc (Zn) forms a 2+ ion and carbonate (CO3) forms a 2- ion. Therefore, the formula for zinc carbonate is ZnCO3. When heated, zinc carbonate decomposes into zinc oxide (ZnO) and carbon dioxide (CO2). So the overall reaction is: ZnCO3 (s) → ZnO (s) + CO2 (g)
02

(b) Silicon dioxide and hydrofluoric acid forming silicon tetrafluoride and water

The chemical formula for silicon dioxide is SiO2, and for hydrofluoric acid, it is HF. When silicon dioxide reacts with hydrofluoric acid, it forms silicon tetrafluoride (SiF4) and water (H2O). The balanced chemical equation for this reaction is: SiO2 (s) + 4HF (aq) → SiF4 (g) + 2H2O (l)
03

(c) Sulfur dioxide and water forming sulfurous acid

Sulfur dioxide (SO2) reacts with water (H2O) to form sulfurous acid (H2SO3). The balanced chemical equation for this reaction looks like this: SO2 (g) + H2O (l) → H2SO3 (aq)
04

(d) Phosphorus trihydride

Phosphorus trihydride is more commonly referred to as phosphine. The chemical formula for phosphorus trihydride (phosphine) is PH3.
05

(e) Perchloric acid and cadmium forming cadmium(II) perchlorate

Perchloric acid has the formula HClO4, and cadmium (Cd) forms a 2+ ion. When cadmium reacts with perchloric acid, it forms cadmium(II) perchlorate, which has the formula Cd(ClO4)2, since perchlorate has a 1- charge.
06

(f) Vanadium(III) bromide

Vanadium(III) means that vanadium (V) has a 3+ charge. Bromide (Br) has a 1- charge. Therefore, the chemical formula for vanadium(III) bromide is VBr3 since it requires three bromide ions to balance the 3+ charge of vanadium.

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Most popular questions from this chapter

The first atoms of seaborgium (Sg) were identified in 1974 . The longest-lived isotope of Sg has a mass number of \(266 .\) (a) How many protons, electrons, and neutrons are in an \({ }^{266} \mathrm{Sg}\) atom? (b) Atoms of Sg are very unstable, and it is therefore difficult to study this element's properties. Based on the position of Sg in the periodic table, what element should it most closely resemble in its chemical properties?

Many familiar substances have common, unsystematic names. For each of the following, give the correct systematic name: (a) saltpeter, \(\mathrm{KNO}_{3}\); (b) soda ash, \(\mathrm{Na}_{2} \mathrm{CO}_{3}\); (c) lime, \(\mathrm{CaO}\); (d) muriatic acid, \(\mathrm{HCl}\); (e) Epsom salts, \(\mathrm{MgSO}_{4}\); (f) milk of magnesia, \(\mathrm{Mg}(\mathrm{OH})_{2}\)

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. $$ \begin{array}{|l|c|c|c|c|} \hline \text { Ion } & \mathrm{K}^{+} & \mathrm{NH}_{4}^{+} & \mathrm{Mg}^{2+} & \mathrm{Fe}^{3+} \\ \hline \mathrm{Cl}^{-} & \mathrm{KCl} & & & \\ \hline \mathrm{OH}^{-} & & & & \\ \hline \mathrm{CO}_{3}^{2-} & & & & \\ \hline \mathrm{PO}_{4}{ }^{3-} & & & & \\ \hline \end{array} $$

Two compounds have the same empirical formula. One substance is a gas, whereas the other is a viscous liquid. How is it possible for two substances with the same empirical formula to have markedly different properties?

The element lead (Pb) consists of four naturally occurring isotopes with atomic masses 203.97302,205.97444,206.97587 , and 207.97663 amu. The relative abundances of these four isotopes are 1.4,24.1,22.1 , and \(52.4 \%\), respectively. From these data, calculate the atomic weight of lead.
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