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Chapter 2: Problem 106

Name each of the following chlorides. Assuming that the compounds are ionic, what charge is associated with the metallic element in each case? (a) \(\mathrm{AgCl},(\mathbf{b}) \mathrm{TiCl}_{4},(\mathbf{c}) \operatorname{Ir} \mathrm{C} 1_{3},\) (d) \(\mathrm{LiCl}\).

Short Answer

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The chlorides given are: (a) Silver Chloride (AgCl), (b) Titanium(IV) Chloride (TiCl\(_{4}\)), (c) Iridium(III) Chloride (IrCl\(_{3}\)), and (d) Lithium Chloride (LiCl). The charges associated with the metallic elements are: (a) Ag has a charge of +1, (b) Ti has a charge of +4, (c) Ir has a charge of +3, and (d) Li has a charge of +1.

Step by step solution

01

Name each chloride

Naming the compounds involves identifying the metallic element and the non-metallic element (in this case, chlorine) and adding the suffix "-ide" to the non-metallic element. For some compounds, it is important to mention the oxidation state of the metallic element. (a) \(\mathrm{AgCl}\): Silver Chloride (b) \(\mathrm{TiCl}_{4}\): Titanium(IV) Chloride (c) \(\mathrm{IrCl}_{3}\): Iridium(III) Chloride (d) \(\mathrm{LiCl}\): Lithium Chloride
02

Determine charge associated with metallic elements

The charge associated with the metallic element can be determined by understanding the charges present on the non-metallic element (in this case, chlorine) and using the oxidation state of the metallic element. (a) Silver Chloride (AgCl): Chlorine has a charge of -1, so silver (Ag) must have a charge of +1 to balance the charges. The charge associated with Ag is +1. (b) Titanium(IV) Chloride (TiCl\(_{4}\)): Chlorine has a charge of -1, and there are four chlorine atoms, resulting in a total charge of -4. The oxidation state of titanium is IV (4), resulting in a charge of +4. The charge associated with Ti is +4. (c) Iridium(III) Chloride (IrCl\(_{3}\)): Chlorine has a charge of -1, and there are three chlorine atoms, resulting in a total charge of -3. The oxidation state of iridium is III (3), resulting in a charge of +3. The charge associated with Ir is +3. (d) Lithium Chloride (LiCl): Chlorine has a charge of -1, so lithium (Li) must have a charge of +1 to balance the charges. The charge associated with Li is +1.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Oxidation States
Every atom in a chemical compound has an electric charge, known as an oxidation state. This oxidation state indicates how many electrons an atom has gained or lost when forming a compound. For example, in the compound Titanium(IV) Chloride (\(\text{TiCl}_4\)), the Roman numeral IV represents the oxidation state of titanium, which in this case is +4. This number helps us to understand the nature of the bonding in chemical compounds.
  • Oxidation states help determine the charge needed to balance a compound, ensuring its neutrality.
  • For metals like silver (\(\text{AgCl}\)), the oxidation state of chlorine is -1. Therefore, silver must be +1 to maintain a balanced compound.
Understanding oxidation states is crucial for naming ionic compounds, as sometimes the metal can exist in multiple oxidation states, each forming different compounds with various properties.
Metallic Elements
Metallic elements often form ionic bonds with non-metallic elements by donating electrons and forming positive ions, known as cations. These cations carry a positive charge, which is balanced by the negative charge of the anions, typically formed by non-metals such as chlorine.
  • In \(\text{LiCl}\), lithium donates one electron to chlorine, forming \(\text{Li}^+\) and \(\text{Cl}^-\).
  • Across different compounds, the same metal can have different charges or oxidation states, like titanium in \(\text{TiCl}_4\) having a +4 charge.
This property makes metallic elements highly versatile in forming compounds and is a key factor in understanding and predicting the behavior of ionic compounds.
Chemical Formulas
Chemical formulas give us insight into the composition and proportions of elements in a compound. Each formula represents the elements involved, with subscripts indicating the number of atoms or ions partaking in the makeup of the compound. In ionic compounds, these formulas also reflect the balance of total charges.
  • For example, in \(\text{IrCl}_3\), the subscript 3 next to chlorine indicates that three chloride ions are needed to balance the charge of one iridium ion, which has an oxidation state of +3.
  • The formula \(\text{TiCl}_4\) signifies four chloride ions balancing a single titanium ion with a charge of +4.
These formulas are essential for understanding the stoichiometry of reactions and predicting the products and reactants involved in chemical processes.

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Most popular questions from this chapter

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