Question

Supply the Latin system name for each of the following monoatomic cations: (a) \(\mathrm{Cu}^{+}\) (b) \(\mathrm{Fe}^{3+}\) (c) \(\mathrm{Sn}^{4+}\) (d) \(\mathrm{Pb}^{4+}\)

Short answer

(a) Cuprous, (b) Ferric, (c) Stannic, (d) Plumbic.

Step-by-step solution

Identify the Element and Charge

First, identify the elements and their oxidation states based on the given cations. (a) Copper (Cu) with a +1 charge. (b) Iron (Fe) with a +3 charge. (c) Tin (Sn) with a +4 charge. (d) Lead (Pb) with a +4 charge.

Understand the Latin System

The Latin system uses the element's Latin name and can involve a suffix to indicate the oxidation state. The lesser oxidation number (lower charge) uses the suffix '-ous,' and the higher oxidation number (higher charge) uses the suffix '-ic.'

Assign Latin Names with Correct Suffix

Based on each element's charge, use the appropriate suffix:(a) For \(Cu^+\), use 'cuprous' (from 'cuprum').(b) For \(Fe^{3+}\), use 'ferric' (from 'ferrum').(c) For \(Sn^{4+}\), use 'stannic' (from 'stannum').(d) For \(Pb^{4+}\), use 'plumbic' (from 'plumbum').

Write the Latin System Names

Finally, list the Latin system names for each cation:(a) Cuprous for \(Cu^+\).(b) Ferric for \(Fe^{3+}\).(c) Stannic for \(Sn^{4+}\).(d) Plumbic for \(Pb^{4+}\).

Key concepts

Understanding Oxidation States

The concept of oxidation states is fundamental in chemistry, especially when you are dealing with monoatomic cations. Oxidation state, also known as oxidation number, is a measure of the degree of oxidation of an atom within a compound. It can be thought of as the charge of an atom if all bonds were ionic. When an atom loses or gains electrons, it forms ions with positive or negative charges, respectively. For example:

• In \( \mathrm{Cu}^{+} \), copper has lost one electron, resulting in a +1 charge.
• In \( \mathrm{Fe}^{3+} \), iron has lost three electrons, leading to a +3 charge.
• In \( \mathrm{Sn}^{4+} \), tin lost four electrons, giving it a +4 charge.
• In \( \mathrm{Pb}^{4+} \), lead also lost four electrons, yielding a +4 charge.

Knowing the oxidation state helps us identify the electron configuration of an atom and analyze its chemical behavior. In the naming of ions and compounds, the oxidation state can indicate how elements interact with each other.

Monoatomic Cations: A Simple Breakdown

Monoatomic cations are ions consisting of single atoms that have a positive charge. This positive charge occurs because the atom has lost one or more electrons. Monoatomic cations are typically metals, especially those in the transition metals category. Some characteristics include:

• They are denoted by the element symbol followed by the charge in superscript; for instance, \( \mathrm{Cu}^{+} \).
• Metals in groups 1 and 2 usually form cations that correspond to their group number (e.g., \( \mathrm{Na}^{+} \), \( \mathrm{Ca}^{2+} \)).
• Transition metals, however, can have multiple possible charges depending on the chemical environment, which leads to different cations, like \( \mathrm{Fe}^{2+} \) and \( \mathrm{Fe}^{3+} \).

Understanding these ions is crucial in predicting the types of compounds they can form and their roles in chemical reactions.

Nomenclature for Transition Metals

Transition metals, a group of elements found in the d-block of the periodic table, are known for having multiple oxidation states. The nomenclature of transition metals requires understanding their unique naming system. Unlike group 1 and group 2 metals, transition metals can exhibit more than one stable oxidation state. Therefore, to distinguish between them, a systematic naming approach is used that often involves their Latin-derived names with suffixes.In the Latin system of nomenclature:

• The lower oxidation state is represented using the suffix '-ous.' For example, \( \mathrm{Cu}^{+} \) is called 'cuprous.'
• The higher oxidation state uses the suffix '-ic.' Hence, \( \mathrm{Fe}^{3+} \) is 'ferric.'

This Latin-rooted naming system helps in identifying the specific oxidation state of a metal in a compound, which is important for predicting the compound's properties and reactivity. Additionally, understanding these naming conventions allows chemists to communicate effectively about compounds that may have multiple forms.