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Chapter 16: Problem 10

Fill in the blanks in the following table. (a) \(\mathrm{BaC}_{2} \mathrm{O}_{4}\) (b) \(\mathrm{Cr}(\mathrm{OH})_{3}\) (c) \(\mathrm{Pb}_{3}\left(\mathrm{PO}_{4}\right)_{2}\)

Short Answer

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Question: Identify the names, type of bond, and charge on each element for the following compounds: (a) \(\mathrm{BaC}_{2} \mathrm{O}_{4}\) (b) \(\mathrm{Cr} (\mathrm{OH})_{3}\) (c) \(\mathrm{Pb}_{3} \left(\mathrm{PO}_{4}\right)_{2}\)

Step by step solution

01

Name the compounds

For each of the compounds, we need to name them properly, following the rules of nomenclature for ionic and covalent compounds. (a) \(\mathrm{BaC}_{2} \mathrm{O}_{4}\): Barium chromate In this compound Barium (Ba) is a metal and Chromate (C2O4) is a polyatomic anion. (b) \(\mathrm{Cr} (\mathrm{OH})_{3}\): Chromium hydroxide In this compound, Chromium (Cr) is a metal and hydroxide (OH) is a polyatomic anion. (c) \(\mathrm{Pb}_{3} \left(\mathrm{PO}_{4}\right)_{2}\): Lead (II) phosphate In this compound, Lead (Pb) is a metal and phosphate (PO4) is a polyatomic anion.
02

Determine the type of bond in the compounds

All the given compounds have a metal and a polyatomic anion, which means they are ionic compounds. The bond in each compound is an ionic bond. (a) \(\mathrm{BaC}_{2} \mathrm{O}_{4}\): Ionic bond (b) \(\mathrm{Cr} (\mathrm{OH})_{3}\): Ionic bond (c) \(\mathrm{Pb}_{3} \left(\mathrm{PO}_{4}\right)_{2}\): Ionic bond
03

Identify the charge on each element

In ionic compounds, the charges on the elements can be determined from the oxidation numbers of the elements and the overall charge of the polyatomic ions. (a) \(\mathrm{BaC}_{2} \mathrm{O}_{4}\): Barium (Ba): +2 (from the periodic table) Chromate (C2O4): -2 (as a whole polyatomic ion) (b) \(\mathrm{Cr}(\mathrm{OH})_{3}\): Chromium (Cr): +3 (since it forms 3 OH- to become neutral) Hydroxide (OH): -1 (charge on O is -2 and H is +1, so overall charge on OH is -1) (c) \(\mathrm{Pb}_{3}\left(\mathrm{PO}_{4}\right)_{2}\): Lead (Pb): +2 (each lead ion, the roman numeral II is given) Phosphate (PO4): -3 (as a whole polyatomic ion)

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Most popular questions from this chapter

Lead azide, \(\mathrm{Pb}\left(\mathrm{N}_{3}\right)_{2}\), is used as a detonator in car airbags. The impact of a collision causes \(\mathrm{Pb}\left(\mathrm{N}_{3}\right)_{2}\) to be converted into an enormous amount of gas that fills the airbag. At \(25^{\circ} \mathrm{C}\), a saturated solution of lead azide is prepared by dissolving \(25 \mathrm{mg}\) in water to make \(100.0 \mathrm{~mL}\) of solution. What is \(K_{\mathrm{sp}}\) for lead azide?

Consider a \(1.50-\mathrm{L}\) aqueous solution of \(3.75 \mathrm{M} \mathrm{NH}_{3}\), where \(17.5 \mathrm{~g}\) of \(\mathrm{NH}_{4} \mathrm{Cl}\) is dissolved. To this solution, \(5.00 \mathrm{~g}\) of \(\mathrm{MgCl}_{2}\) is added. (a) What is \(\left[\mathrm{OH}^{-}\right]\) before \(\mathrm{MgCl}_{2}\) is added? (b) Will a precipitate form? (c) What is \(\left[\mathrm{Mg}^{2+}\right]\) after equilibrium is established?

What is the \(\mathrm{I}^{-}\) concentration just as \(\mathrm{AgCl}\) begins to precipitate when \(1.0 \mathrm{M} \mathrm{AgNO}_{3}\) is slowly added to a solution containing \(0.020 \mathrm{M} \mathrm{Cl}^{-}\) and \(0.020 M \mathrm{I}^{-}\)

Write a net ionic equation for the reaction with \(\mathrm{OH}^{-}\) by which (a) \(\mathrm{Sb}^{3+}\) forms a precipitate. (b) antimony(III) hydroxide dissolves when more \(\mathrm{OH}^{-}\) is added. (c) \(\mathrm{Sb}^{3+}\) forms a complex ion.

Fill in the blanks in the following table. (a) \(\mathrm{CoCO}_{3}\) (b) \(\mathrm{LaF}_{3}\) (c) \(\mathrm{Ba}_{3}\left(\mathrm{PO}_{4}\right)_{2}\)
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