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Chapter 2: Problem 133

Which of the following atoms is the most stable? A. nitrogen, because the elements in Group 15 can form anions B. argon, because the noble gases have full valence shells C. sodium, because alkali metals can form cations D. magnesium, because alkaline earth metals have a high melting point

Short Answer

Expert verified
B. argon, because the noble gases have full valence shells

Step by step solution

01

Understand Stability Criteria

Determine which characteristic among the given elements generally signifies the highest stability for an atom. Typically, full valence shells indicate a very stable electron configuration.
02

Examine Nitrogen

Elements in Group 15, such as nitrogen, can form anions by gaining extra electrons to complete their valence shell. However, this does not necessarily indicate maximum stability in its natural state.
03

Examine Argon

Noble gases like argon have completely filled valence shells, meaning they are very chemically inert and stable. This indicates a very high level of stability.
04

Examine Sodium

Alkali metals like sodium can lose an electron to form cations, but this process indicates less stability until the electron is lost.
05

Examine Magnesium

Although alkaline earth metals like magnesium have high melting points, this property does not directly correspond to having the most stable electron configuration.
06

Conclusion

Compare all the findings. Argon, with its full valence shell, represents the most stable electron configuration among the given elements.

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Key Concepts

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

Valence Shells
In atomic theory, a valence shell is the outermost shell of an atom. This is where the valence electrons are located. These electrons are the primary drivers behind both chemical bonding and the stability of atoms. Valence shells can either be partially filled or completely filled. When they are completely filled, the atom tends to be more stable. This is because a full valence shell means that the atom has reached a lower energy state.

Why Valence Shells Matter:
  • Determines Atom's Reactivity: The more incomplete the valence shell, the more reactive the atom.
  • Influences Bond Formation: Atoms will lose, gain, or share electrons to complete their valence shell, forming bonds in the process.
  • Impacts Stability: Atoms with full valence shells, like noble gases, are very stable.
A clear understanding of valence shells can help you predict how different atoms will behave in chemical reactions.
Noble Gases
Noble gases are elements located in Group 18 of the periodic table. These elements include helium, neon, argon, krypton, xenon, and radon. What sets noble gases apart is their completely filled valence shells, making them extremely stable and chemically inert.

Characteristics of Noble Gases:
  • Low Reactivity: Because their valence shells are full, noble gases rarely participate in chemical reactions.
  • Stable Electron Configuration: The full valence shell gives these elements a low-energy, stable state.
  • Exist as Monatomic Gases: Noble gases occur naturally as single atoms rather than molecules.
Noble gases serve as the benchmark for stability in other elements. Since they have full valence shells, they provide an ideal configuration that other elements strive to achieve, either by gaining, losing, or sharing electrons.
Electron Configuration
Electron configuration refers to the arrangement of electrons in an atom's various shells and subshells. The configuration follows specific rules such as the Aufbau principle, Pauli-exclusion principle, and Hund's rule. Understanding this concept is essential for predicting an atom's chemical behavior and its level of stability.

Important Principles:
  • Aufbau Principle: Electrons occupy the lowest energy orbitals available.
  • Pauli-Exclusion Principle: Each orbital can hold a maximum of two electrons with opposite spins.
  • Hund's Rule: Electrons fill degenerate orbitals singly before pairing up.


A stable electron configuration, often involving filled valence shells, is a key determinant in the chemical properties of an atom. For example, the electron configuration of argon (1s² 2s² 2p⁶ 3s² 3p⁶) shows that it has a full outer shell, making it extremely stable and less likely to react chemically.

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Most popular questions from this chapter

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