Question

Name each of the following ions according to the Stock system: a. \({Fe}^{2+}\) d. \({Pb}^{4+}\) b.\({Fe}^{3+}\) e. \({Sn}^{2+}\) c.\({Pb}^{2+}\) f. \({Sn}^{4+}\)

Short answer

a. iron(II) d. lead(IV) b. iron(III) e. tin(II) c. lead(II) f. tin(IV)

Step-by-step solution

Identify the Element and its Common Oxidation States

For each ion, identify the element and its possible oxidation states. For example, iron (Fe) has common oxidation states of +2 and +3.

Apply the Stock System of Nomenclature

According to the Stock system, the oxidation state of the element is indicated by a Roman numeral in parentheses after the name of the element.

Name the Ion with its Oxidation State

Using the Stock system: * For \(Fe^{2+}\), the ion is called iron(II). * For \(Fe^{3+}\), the ion is called iron(III). * For \(Pb^{2+}\), the ion is called lead(II). * For \(Pb^{4+}\), the ion is called lead(IV). * For \(Sn^{2+}\), the ion is called tin(II). * For \(Sn^{4+}\), the ion is called tin(IV).

Key concepts

oxidation states

Oxidation states, also known as oxidation numbers, are used to indicate the degree of oxidation of an atom in a chemical compound. In simple terms, they tell us how many electrons an atom is losing, gaining, or sharing when it forms a bond.

For example, in the ions given in the problem: Fe can have oxidation states of +2 or +3, Pb can have +2 or +4, and Sn can have +2 or +4. These numbers are crucial for naming compounds using the Stock system.

To determine the oxidation state, you can look at the charge on the ion. For instance, in \(Fe^{2+}\), the oxidation state is +2 because the iron atom has lost two electrons.

transition metals

Transition metals are elements found in the middle of the periodic table, specifically in groups 3 through 12. They are known for having multiple oxidation states, making them quite versatile in chemical reactions.

Iron (Fe), lead (Pb), and tin (Sn) are all examples of transition metals. Because they can form ions with different charges, it is essential to specify the oxidation state when naming these ions.

This is especially important for understanding and applying the Stock system nomenclature, as the same element can have different names depending on its oxidation state (e.g., iron(II) vs. iron(III)).

Roman numerals

Roman numerals are used in the Stock system to denote the oxidation state of elements in their ionic form. Formulating the correct name requires the use of these numerals in parentheses right after the element's name.

Here’s a quick guide to Roman numerals: I, II, III, IV, V designate 1, 2, 3, 4, and 5, respectively. Thus, in the given problem: Fe(II) reads as iron(II) and Fe(III) as iron(III).

Accurately using these numerals helps chemists and students correctly identify and differentiate between ions of varying oxidation states.

ion naming

Ion naming follows specific conventions, particularly when dealing with transition metals, which can have multiple oxidation states. The Stock system is one such convention that helps in naming these ions precisely.

For the ions given in the problem, follow these steps:

• Identify the element and its charge.
• Apply the Stock system by using the element name followed by its oxidation state in Roman numerals in parentheses.

So, \(Fe^{2+}\) becomes iron(II) and \(Pb^{4+}\) becomes lead(IV). This systematic approach ensures that the ion names are clear and informative about their chemical properties.