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Chapter 5: Problem 28

Why are there no rules for naming Group 18 ions?

Short Answer

Expert verified
There are no rules for naming Group 18 ions because these elements, also known as noble gases, are chemically stable under standard conditions due to having full electron shells. This means they do not easily form ions, making the need for such naming rules unnecessary.

Step by step solution

01

Understanding Group 18 Elements

First, it's crucial to understand what elements make up Group 18, otherwise known as the noble gases. These are helium, neon, argon, krypton, xenon, and radon. Noble gases are named as such because they are known to have full electron shells, making them chemically stable and largely unreactive.
02

Understanding Ions and their Naming Rules

An ion is a particle that has a charge due to the loss or gain of electrons. In the naming of ions, we generally specify if it is an anion (gained electrons, and thus, negatively charged), or a cation (lost electrons, and therefore, positively charged). As part of the naming convention, one would normally refer to the element name and append it with 'ion.' For instance, the sodium ion would refer to a sodium atom that has lost an electron and has become positively charged.
03

Applying Understanding of Naming Conventions to Group 18

Because Group 18 - the noble gases - are largely unreactive due to their full valence shells, this means they rarely gain or lose electrons - they rarely form ions. Hence, there are no established rules for naming Group 18 ions, because the formation of ions within this group is an event that is relatively rare in standard conditions.

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Most popular questions from this chapter

Why can't sodium gain a positive charge by acquiring a proton in its nucleus?

Graphing Calculator Calculating the Number of Valence Electrons The graphing calculator can run a program that can determine the number of valence electrons in an atom, given its atomic number. Go to Appendix C. If you are using a TI-83 Plus, you can download the program VALENCE and run the application as directed. If you are using another calculator, your teacher will provide you with keystrokes to use. After you have run the program, answer these questions. How many valence electrons are there in the following atoms? \begin{equation} \begin{array}{l}{\text { a. Rutherfordium, Rf, atomic number } 104} \\ {\text { b. Gold, Au, atomic number } 79} \\ {\text { c. Molybdenum, Mo, atomic number } 42} \\ {\text { d. Indium, In, atomic number } 49}\end{array} \end{equation}

Identify and name the cations and anions that make up the following ionic compounds and indicate the charge on each ion. \begin{equation} \begin{array}{ll}{\text { a. } \mathrm{NaNO}_{3}} & {\text { c. }\left(\mathrm{NH}_{4}\right)_{2} \mathrm{CrO}_{4}} \\ {\text { b. } \mathrm{K}_{2} \mathrm{SO}_{3}} & {\text { d. } \mathrm{Al}_{2}\left(\mathrm{SO}_{4}\right)_{3}}\end{array} \end{equation}

Why are most metals found in nature as ores and not as pure metals?

What is the difference between the chlorite ion and the chlorate ion?
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