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Chapter 2: Problem 55

Predict the chemical formula for the ionic compound formed by (a) \(\mathrm{Ca}^{2+}\) and \(\mathrm{Br}^{-},\) (b) \(\mathrm{K}^{+}\) and \(\mathrm{CO}_{3}^{2-},\) (c) \(\mathrm{Al}^{3+}\) and \(\mathrm{CH}_{3} \mathrm{COO}^{-}\) (d) \(\mathrm{NH}_{4}^{+}\) and \(\mathrm{SO}_{4}^{2-}\), (e) \(\mathrm{Mg}^{2+}\) and \(\mathrm{PO}_{4}^{3-}\).

Short Answer

Expert verified
The chemical formulas for the given ionic compounds are: (a) \(\mathrm{CaBr}_{2}\) (b) \(\mathrm{K}_{2}\mathrm{CO}_{3}\) (c) \(\mathrm{Al}(\mathrm{CH}_{3}\mathrm{COO})_{3}\) (d) \((\mathrm{NH}_{4})_{2}\mathrm{SO}_{4}\) (e) \(\mathrm{Mg}_{3}(\mathrm{PO}_{4})_{2}\)

Step by step solution

01

Identify the charges on the ions

The calcium ion carries a positive charge of 2 (\(\mathrm{Ca}^{2+}\)), and the bromide ion has a negative charge of 1 (\(\mathrm{Br}^{-}\)).
02

Balance the charges

To balance the charges, we need to find the lowest common multiple (LCM) of the charges, which is 2 in this case. This means we need 1 calcium ion and 2 bromide ions to balance the charges. Thus, the chemical formula is \(\mathrm{CaBr}_{2}\). (b) \(\mathrm{K}^{+}\) and \(\mathrm{CO}_{3}^{2-}\)
03

Identify the charges on the ions

The potassium ion has a positive charge of 1 (\(\mathrm{K}^{+}\)), and the carbonate ion has a negative charge of 2 (\(\mathrm{CO}_{3}^{2-}\)).
04

Balance the charges

The LCM of the charges is 2, so we need 2 potassium ions and 1 carbonate ion to balance the charges. The chemical formula is \(\mathrm{K}_{2}\mathrm{CO}_{3}\). (c) \(\mathrm{Al}^{3+}\) and \(\mathrm{CH}_{3}\mathrm{COO}^{-}\)
05

Identify the charges on the ions

The aluminum ion has a positive charge of 3 (\(\mathrm{Al}^{3+}\)), and the acetate ion has a negative charge of 1 (\(\mathrm{CH}_{3}\mathrm{COO}^{-}\)).
06

Balance the charges

The LCM of the charges is 3, so we need 1 aluminum ion and 3 acetate ions to balance the charges. The chemical formula is \(\mathrm{Al}(\mathrm{CH}_{3}\mathrm{COO})_{3}\). (d) \(\mathrm{NH}_{4}^{+}\) and \(\mathrm{SO}_{4}^{2-}\)
07

Identify the charges on the ions

The ammonium ion has a positive charge of 1 (\(\mathrm{NH}_{4}^{+}\)), and the sulfate ion has a negative charge of 2 (\(\mathrm{SO}_{4}^{2-}\)).
08

Balance the charges

The LCM of the charges is 2, so we need 2 ammonium ions and 1 sulfate ion to balance the charges. The chemical formula is \(($$\mathrm{NH}_{4})_{2}\mathrm{SO}_{4}\). (e) \(\mathrm{Mg}^{2+}\) and \(\mathrm{PO}_{4}^{3-}\)
09

Identify the charges on the ions

The magnesium ion has a positive charge of 2 (\(\mathrm{Mg}^{2+}\)), and the phosphate ion has a negative charge of 3 (\(\mathrm{PO}_{4}^{3-}\)).
10

Balance the charges

The LCM of the charges is 6, so we need 3 magnesium ions and 2 phosphate ions to balance the charges. The chemical formula is \(\mathrm{Mg}_{3}(\mathrm{PO}_{4})_{2}\).

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Most popular questions from this chapter

Write the empirical formula corresponding to each of the following molecular formulas: (a) \(\mathrm{Al}_{2} \mathrm{Br}_{6},\) (b) \(\mathrm{C}_{8} \mathrm{H}_{10},\) (c) \(\mathrm{C}_{4} \mathrm{H}_{8} \mathrm{O}_{2}\), (d) \(\mathrm{P}_{4} \mathrm{O}_{10}\) (e) \(\mathrm{C}_{6} \mathrm{H}_{4} \mathrm{Cl}_{2}\), (f) \(\mathrm{B}_{3} \mathrm{~N}_{3} \mathrm{H}_{6}\)

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: $$ \begin{array}{cc} \hline \text { Mass (amu) } & \text { Relative Size } \\ \hline 157.836 & 0.2569 \\ 159.834 & 0.4999 \\ 161.832 & 0.2431 \\ \hline \end{array} $$ (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.

Each of the following elements is capable of forming an ion in chemical reactions. By referring to the periodic table, predict (b) \(\mathrm{Al},(\mathbf{c}) \mathrm{K}\) the charge of the most stable ion of each: (a) \(\mathrm{Mg}\), (d) S, (e) \(\mathrm{F}\).

(a) What do ethane and ethanol have in common? (b) How does 1 -propanol differ from propane?

Fill in the blanks in the following table: $$ \begin{array}{|l|l|l|l|} \hline \text { Cation } & \text { Anion } & \text { Formula } & \text { Name } \\\ \hline & & & \text { Lithium oxide } \\ \hline \mathrm{Fe}^{2+} & \mathrm{PO}_{4}^{3-} & & \\ \hline & & \mathrm{Al}_{2}\left(\mathrm{SO}_{4}\right)_{3} & \\ \hline & & & \text { Copper(II) nitrate } \\ \hline \mathrm{Cr}^{3+} & \mathrm{I}^{-} & & \\ \hline & & \mathrm{MnClO}_{2} & \\ \hline & & & \text { Ammonium carbonate } \\ \hline & & & \text { Zinc perchlorate } \\ \hline \end{array} $$
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