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Chapter 2: Problem 68

Give the chemical formula for each of the following ionic compounds: (a) sodium phosphate, (b) zinc nitrate, (c) barium bromate, (d) iron(II) perchlorate, (e) cobalt(II) hydrogen carbonate, (f) chromium(III) acetate, \((\mathrm{g})\) potassium dichromate.

Short Answer

Expert verified
The chemical formulas for the given ionic compounds are: (a) Sodium Phosphate: \(\text{Na}_{3}\text{PO}_{4}\) (b) Zinc Nitrate: \(\text{Zn}(\text{NO}_{3})_{2}\) (c) Barium Bromate: \(\text{Ba}(\text{BrO}_{3})_{2}\) (d) Iron(II) Perchlorate: \(\text{Fe}(\text{ClO}_{4})_{2}\) (e) Cobalt(II) Hydrogen Carbonate: \(\text{Co}(\text{HCO}_{3})_{2}\) (f) Chromium(III) Acetate: \(\text{Cr}(\text{C}_{2}\text{H}_{3}\text{O}_{2})_{3}\) (g) Potassium Dichromate: \(\text{K}_{2}\text{Cr}_{2}\text{O}_{7}\)

Step by step solution

01

(a) Sodium Phosphate

Sodium ion has a charge of \(+1\), and phosphate ion has a charge of \(-3\). To form the ionic compound sodium phosphate, we need 3 sodium ions to balance with the charge of 1 phosphate ion. The chemical formula is therefore given by \(\text{Na}_{3}\text{PO}_{4}\).
02

(b) Zinc Nitrate

Zinc ion has a charge of \(+2\), and nitrate ion has a charge of \(-1\). We need 2 nitrate ions to balance with the charge of 1 zinc ion. The chemical formula for zinc nitrate is given by \(\text{Zn}(\text{NO}_{3})_{2}\).
03

(c) Barium Bromate

Barium ion has a charge of \(+2\), and bromate ion has a charge of \(-1\). We need 2 bromate ions to balance with the charge of 1 barium ion. The chemical formula for barium bromate is given by \(\text{Ba}(\text{BrO}_{3})_{2}\).
04

(d) Iron(II) Perchlorate

Iron(II) ion has a charge of \(+2\), and perchlorate ion has a charge of \(-1\). We need 2 perchlorate ions to balance with the charge of 1 iron(II) ion. The chemical formula for iron(II) perchlorate is given by \(\text{Fe}(\text{ClO}_{4})_{2}\).
05

(e) Cobalt(II) Hydrogen Carbonate

Cobalt(II) ion has a charge of \(+2\), and hydrogen carbonate ion has a charge of \(-1\). We need 2 hydrogen carbonate ions to balance with the charge of 1 cobalt(II) ion. The chemical formula for cobalt(II) hydrogen carbonate is given by \(\text{Co}(\text{HCO}_{3})_{2}\).
06

(f) Chromium(III) Acetate

Chromium(III) ion has a charge of \(+3\), and acetate ion has a charge of \(-1\). We need 3 acetate ions to balance with the charge of 1 chromium(III) ion. The chemical formula for chromium(III) acetate is given by \(\text{Cr}(\text{C}_{2}\text{H}_{3}\text{O}_{2})_{3}\).
07

(g) Potassium Dichromate

Potassium ion has a charge of \(+1\), and dichromate ion has a charge of \(-2\). We need 2 potassium ions to balance with the charge of 1 dichromate ion. The chemical formula for potassium dichromate is given by \(\text{K}_{2}\text{Cr}_{2}\text{O}_{7}\).

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Most popular questions from this chapter

Write the chemical formulas for the following compounds: (a) aluminum hydroxide, (b) potassium sulfate, (c) copper(I) oxide, (d) zinc nitrate, (e) mercury(II) bromide, (f) iron(III) carbonate, (g) sodium hypobromite.

Name the following ionic compounds: (a) \(\mathrm{K}_{2} \mathrm{O}\), (b) \(\mathrm{NaClO}_{2},(\mathrm{c}) \mathrm{Sr}(\mathrm{CN})_{2},(\mathrm{~d}) \mathrm{Co}(\mathrm{OH})_{2},(\mathrm{e}) \mathrm{Fe}_{2}\left(\mathrm{CO}_{3}\right)_{3}\) (f) \(\mathrm{Cr}\left(\mathrm{NO}_{3}\right)_{3},(\mathrm{~g})\left(\mathrm{NH}_{4}\right)_{2} \mathrm{SO}_{3},(\mathrm{~h}) \mathrm{NaH}_{2} \mathrm{PO}_{4}\), (i) \(\mathrm{KMnO}_{4}\) (j) \(\mathrm{Ag}_{2} \mathrm{Cr}_{2} \mathrm{O}_{7}\)

Fill in the gaps in the following table, assuming each column represents a neutral atom: $$ \begin{array}{|l|l|l|l|l|l|} \hline \text { Symbol } & { }^{52} \mathrm{Cr} & & & & \\ \hline \text { Protons } & & 25 & & & 82 \\ \hline \text { Neutrons } & & 30 & 64 & & \\ \hline \text { Electrons } & & & 48 & 86 & \\ \hline \text { Mass no. } & & & & 222 & 207 \\ \hline \end{array} $$

Predict the chemical formulas of the compounds formed by the following paire of ions: (a) \(\mathrm{Cu}^{2+}\) and \(\mathrm{Br}^{-}\), (b) \(\mathrm{Fe}^{3+}\) and \(\mathrm{O}^{2-}\), (c) \(\mathrm{Hg}_{2}^{2+}\) and \(\mathrm{CO}_{3}^{2-}\), (d) \(\mathrm{Ca}^{2+}\) and \(\mathrm{AsO}_{4}{ }^{3-}\), (e) \(\mathrm{NH}_{4}{ }^{+}\) and \(\mathrm{CO}_{3}{ }^{2-}\)

How many protons, neutrons, and electrons are in the following atoms: (a) \({ }^{40} \mathrm{Ar}\), (b) \({ }^{65} \mathrm{Zn}\), (c) \({ }^{70} \mathrm{Ga}_{\text {, }}\) (d) \({ }^{80} \mathrm{Br}\), (e) \({ }^{184} \mathrm{~W},(\mathrm{f})^{243} \mathrm{Am} ?\)
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