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Chapter 2: Problem 73

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

Short Answer

Expert verified
The chemical formulas for the given compounds are: (a) Aluminum Hydroxide: Al(OH)₃ (b) Potassium Sulfate: K₂SO₄ (c) Copper(I) Oxide: Cu₂O (d) Zinc Nitrate: Zn(NO3)₂ (e) Mercury(II) Bromide: HgBr₂ (f) Iron(III) Carbonate: Fe₂(CO₃)₃ (g) Sodium Hypobromite: NaBrO

Step by step solution

01

(a) Aluminum Hydroxide

First, find the charges of aluminum (Al) and hydroxide (OH). Aluminum has a charge of +3, and hydroxide has a charge of -1. Combine them in the ratio that ensures a neutral compound: one aluminum for every three hydroxides. The chemical formula for aluminum hydroxide is: Al(OH)₃.
02

(b) Potassium Sulfate

First, find the charges of potassium (K) and sulfate (SO4). Potassium has a charge of +1, and sulfate has a charge of -2. Combine them in the ratio that ensures a neutral compound: two potassium ions for every sulfate ion. The chemical formula for potassium sulfate is: K₂SO₄.
03

(c) Copper(I) Oxide

First, find the charges of copper (Cu) and oxide (O). Since this is copper(I), its charge is +1, and oxide has a charge of -2. Combine them in the ratio that ensures a neutral compound: two copper ions for every oxide ion. The chemical formula for copper(I) oxide is: Cu₂O.
04

(d) Zinc Nitrate

First, find the charges of zinc (Zn) and nitrate (NO3). Zinc has a charge of +2, and nitrate has a charge of -1. Combine them in the ratio that ensures a neutral compound: one zinc ion for every two nitrate ions. The chemical formula for zinc nitrate is: Zn(NO3)₂.
05

(e) Mercury(II) Bromide

First, find the charges of mercury (Hg) and bromide (Br). Since this is mercury(II), its charge is +2, and bromide has a charge of -1. Combine them in the ratio that ensures a neutral compound: one mercury ion for every two bromide ions. The chemical formula for mercury(II) bromide is: HgBr₂.
06

(f) Iron(III) Carbonate

First, find the charges of iron (Fe) and carbonate (CO3). Since this is iron(III), its charge is +3, and carbonate has a charge of -2. Combine them in the ratio that ensures a neutral compound: two iron ions for every three carbonate ions. The chemical formula for iron(III) carbonate is: Fe₂(CO₃)₃.
07

(g) Sodium Hypobromite

First, find the charges of sodium (Na) and hypobromite (BrO). Sodium has a charge of +1, and hypobromite has a charge of -1. Combine them in the ratio that ensures a neutral compound: one sodium ion for every hypobromite ion. The chemical formula for sodium hypobromite is: NaBrO.

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Most popular questions from this chapter

The element chromium (Cr) consists of four naturally occurring isotopes with atomic masses 49.9460,51.9405,52.9407 , and \(53.9389 \mathrm{u}\). The relative abundances of these four isotopes are \(4.3,83.8,9.5,\) and \(2.4 \%\), respectively. From these data, calculate the atomic weight of chromium.

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