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Chapter 20: Problem 28

Thallium and indium form \(+1\) and \(+3\) oxidation states when in compounds. Predict the formulas of the possible compounds between thallium and oxygen and between indium and chlorine. Name the compounds.

Short Answer

Expert verified
The possible compounds between thallium and oxygen are TlO (Thallium(I) oxide or Thallium monoxide) and Tl₂O₃ (Thallium(III) oxide or Thallium trioxide). The possible compounds between indium and chlorine are InCl (Indium(I) chloride or Indium monochloride) and InCl₃ (Indium(III) chloride or Indium trichloride).

Step by step solution

01

Identify the charges of the elements

Thallium has oxidation states of \(+1\) and \(+3\), and oxygen has an oxidation state of \(-2\). Indium also has oxidation states of \(+1\) and \(+3\), while chlorine has an oxidation state of \(-1\).
02

Determine the possible compounds between thallium and oxygen

We will balance charges in order to create neutral compounds. There are two possible scenarios for the thallium and oxygen compound: 1. Thallium with \(+1\) oxidation state, forming a compound with one oxygen atom: \[ \textrm{Tl}^{+1} \qquad \textrm{O}^{-2} \] 2. Thallium with \(+3\) oxidation state, forming a compound with multiple oxygen atoms: \[ \textrm{Tl}^{+3} \qquad \textrm{O}^{-2} \]
03

Create formulas for the thallium and oxygen compounds

By charging the balancing process for each scenario: 1. Thallium with \(+1\) oxidation state and one oxygen atom: \[ \textrm{Tl}_{1}\textrm{O}_{1} \] 2. Thallium with \(+3\) oxidation state and multiple oxygen atoms: \[ \textrm{Tl}_{1}\textrm{O}_{\frac{3}{2}} \] However, this formula contains a fractional value for oxygen, which is not correct. Therefore, we will multiply the entire formula by 2 to get whole number ratios: \[ 2\times\left(\textrm{Tl}_{1}\textrm{O}_{\frac{3}{2}}\right)=\textrm{Tl}_{2}\textrm{O}_{3} \] The possible compounds between thallium and oxygen are TlO and Tl₂O₃.
04

Determine the possible compounds between indium and chlorine

We will balance charges in order to create neutral compounds. There are two possible scenarios for the indium and chlorine compound: 1. Indium with \(+1\) oxidation state, forming a compound with one chlorine atom: \[ \textrm{In}^{+1} \qquad \textrm{Cl}^{-1} \] 2. Indium with \(+3\) oxidation state, forming a compound with multiple chlorine atoms: \[ \textrm{In}^{+3} \qquad \textrm{Cl}^{-1} \]
05

Create formulas for the indium and chlorine compounds

By charging the balancing process for each scenario: 1. Indium with \(+1\) oxidation state and one chlorine atom: \[ \textrm{In}_{1}\textrm{Cl}_{1} \] 2. Indium with \(+3\) oxidation state and multiple chlorine atoms: \[ \textrm{In}_{1}\textrm{Cl}_{3} \] The possible compounds between indium and chlorine are InCl and InCl₃.
06

Name the compounds

Using the IUPAC naming conventions, the compounds and their names are as follows: 1. Thallium and oxygen compounds: - TlO: Thallium(I) oxide or Thallium monoxide - Tl₂O₃: Thallium(III) oxide or Thallium trioxide 2. Indium and chlorine compounds: - InCl: Indium(I) chloride or Indium monochloride - InCl₃: Indium(III) chloride or Indium trichloride

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Most popular questions from this chapter

Tin forms compounds in the \(+2\) and \(+4\) oxidation states. Therefore, when tin reacts with fluorine, two products are possible. Write balanced equations for the production of the two tin halide compounds and name them.

Elemental boron is produced by reduction of boron oxide with magnesium to give boron and magnesium oxide. Write a balanced equation for this reaction.

Beryllium shows some covalent characteristics in some of its compounds, unlike the other alkaline earth halides. Give a possible explanation for this phenomenon.

Lewis structures can be used to understand why some molecules react in certain ways. Write the Lewis structure for the reactants and products in the reactions described below. a. Nitrogen dioxide dimerizes to produce dinitrogen tetroxide. b. Boron trihydride accepts a pair of electrons from ammonia, forming \(\mathrm{BH}_{3} \mathrm{NH}_{3}\). Give a possible explanation for why these two reactions occur.

Compare the Lewis structures with the molecular orbital view of the bonding in \(\mathrm{NO}, \mathrm{NO}^{+}\), and \(\mathrm{NO}^{-}\). Account for any discrepancies between the two models.
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