/*! This file is auto-generated */ .wp-block-button__link{color:#fff;background-color:#32373c;border-radius:9999px;box-shadow:none;text-decoration:none;padding:calc(.667em + 2px) calc(1.333em + 2px);font-size:1.125em}.wp-block-file__button{background:#32373c;color:#fff;text-decoration:none} Problem 37 Give formulas for the following.... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 20: Problem 37

Give formulas for the following. a. potassium tetrachlorocobaltate(II) b. aquatricarbonylplatinum(II) bromide c. sodium dicyanobis(oxalato)ferrate(III) d. triamminechloroethylenediaminechromium(III) iodide

Short Answer

Expert verified
a. \[K_2CoCl_4\] b. \[[Pt(CO)_3(H_2O)]Br_2\] c. \[Na_3[Fe(CN)_2(C_2O_4)_2]\] d. \[[Cr(NH_3)_3Cl(en)]I_3\]

Step by step solution

01

a. potassium tetrachlorocobaltate(II)

First, we identify the cations and anions in the compound. Here, potassium is the cation (K^+) and tetrachlorocobaltate(II) is the anion. Cobalt has an oxidation state of +2, so the formula for the tetrachlorocobaltate(II) anion is CoCl4^2-. Now, we determine the number of each ion to balance their charges: one potassium ion (K^+) and one tetrachlorocobaltate(II) anion (CoCl4^2-). So, the chemical formula of potassium tetrachlorocobaltate(II) is \[K_2CoCl_4\].
02

b. aquatricarbonylplatinum(II) bromide

Here, we have aquatricarbonylplatinum(II) as the cation and bromide as the anion. The cation has platinum with an oxidation state of +2 along with three carbonyl ligands (CO) and one water ligand (H2O). Therefore, the formula for aquatricarbonylplatinum(II) cation is [Pt(CO)3(H2O)]^2+. Bromide anion has the formula Br^-. Now, we determine the number of each ion to balance their charges: one aquatricarbonylplatinum(II) cation [Pt(CO)3(H2O)]^2+ and two bromide anions Br^-. So, the chemical formula of aquatricarbonylplatinum(II) bromide is \[[Pt(CO)_3(H_2O)]Br_2\].
03

c. sodium dicyanobis(oxalato)ferrate(III)

In this compound, sodium is the cation (Na^+) and dicyanobis(oxalato)ferrate(III) is the anion. Ferrate(III) has an oxidation state of +3, so we have Fe(CN)2(C2O4)2^3-. Now, we determine the number of each ion to balance their charges: three sodium ions (Na^+) and one dicyanobis(oxalato)ferrate(III) anion (Fe(CN)2(C2O4)2^3-). So, the chemical formula of sodium dicyanobis(oxalato)ferrate(III) is \[Na_3[Fe(CN)_2(C_2O_4)_2]\].
04

d. triamminechloroethylenediaminechromium(III) iodide

Here, triamminechloroethylenediaminechromium(III) is the cation and iodide is the anion. The cation consists of chromium with an oxidation state of +3, three ammonia ligands (NH3), one chloro ligand (Cl), and one ethylenediamine ligand (en, which is C2H4(NH2)2). Therefore, the formula for triamminechloroethylenediaminechromium(III) cation is [Cr(NH3)3Cl(en)]^3+. Iodide anion has the formula I^-. Now, we determine the number of each ion to balance their charges: one triamminechloroethylenediaminechromium(III) cation [Cr(NH3)3Cl(en)]^3+ and three iodide anions I^-. So, the chemical formula of triamminechloroethylenediaminechromium(III) iodide is \[[Cr(NH_3)_3Cl(en)]I_3\].

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Over 30 million students worldwide already upgrade their learning with 91影视!

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

The ferrate ion, \(\mathrm{FeO}_{4}^{2-},\) is such a powerful oxidizing agent that in acidic solution, aqueous ammonia is reduced to elemental nitrogen along with the formation of the iron(III) ion. a. What is the oxidation state of iron in \(\mathrm{FeO}_{4}^{2-},\) and what is the electron configuration of iron in this polyatomic ion? b. If \(25.0 \mathrm{mL}\) of a \(0.243 \mathrm{M} \mathrm{FeO}_{4}^{2-}\) solution is allowed to react with \(55.0 \mathrm{mL}\) of \(1.45 \mathrm{M}\) aqueous ammonia, what volume of nitrogen gas can form at \(25^{\circ} \mathrm{C}\) and 1.50 atm?

Oxalic acid is often used to remove rust stains. What properties of oxalic acid allow it to do this?

Name the following coordination compounds. a. \(\mathrm{Na}_{4}\left[\mathrm{Ni}\left(\mathrm{C}_{2} \mathrm{O}_{4}\right)_{3}\right]\) b. \(\mathrm{K}_{2}\left[\mathrm{CoCl}_{4}\right]\) c. \(\left[\mathrm{Cu}\left(\mathrm{NH}_{3}\right)_{4}\right] \mathrm{SO}_{4}\) d. \(\left[\mathrm{Co}(\mathrm{en})_{2}(\mathrm{SCN}) \mathrm{Cl}\right] \mathrm{Cl}\)

Iron is present in the earth's crust in many types of minerals. The iron oxide minerals are hematite \(\left(\mathrm{Fe}_{2} \mathrm{O}_{3}\right)\) and magnetite \(\left(\mathrm{Fe}_{3} \mathrm{O}_{4}\right) .\) What is the oxidation state of iron in each mineral? The iron ions in magnetite are a mixture of \(\mathrm{Fe}^{2+}\) and \(\mathrm{Fe}^{3+}\) ions. What is the ratio of \(\mathrm{Fe}^{3+}\) to \(\mathrm{Fe}^{2+}\) ions in magnetite? The formula for magnetite is often written as \(\mathrm{FeO} \cdot \mathrm{Fe}_{2} \mathrm{O}_{3} .\) Does this make sense? Explain.

The \(\mathrm{CrF}_{6}^{4-}\) ion is known to have four unpaired electrons. Does the \(\mathrm{F}^{-}\) ligand produce a strong or weak field?
See all solutions

Recommended explanations on Chemistry Textbooks

Chemistry Branches

Read Explanation

Chemical Analysis

Read Explanation

Physical Chemistry

Read Explanation

Kinetics

Read Explanation

Inorganic Chemistry

Read Explanation

Making Measurements

Read Explanation
View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.