Which outer electron configurations would you expect to belong to a noble gas? a. ns² b. ns²np⁶ c. ns²np⁵ d. ns²np²

Verified step by step guidance

1. Understand that noble gases are elements in Group 18 of the periodic table, known for having a full valence shell of electrons.
2. Recall that the general electron configuration for noble gases is characterized by a completely filled outer shell, which is typically ns^2 np^6.
3. Analyze each given electron configuration option to determine if it represents a full valence shell.
4. Option a: ns^2 represents a filled s subshell, but does not include a filled p subshell, so it is not a noble gas configuration.
5. Option b: ns^2 np^6 represents a filled s and p subshell, indicating a full valence shell, characteristic of noble gases.

Key Concepts

Noble Gas Electron Configuration

Noble gases are elements in Group 18 of the periodic table, characterized by their complete outer electron shells. This configuration typically follows the pattern of ns²np⁶, where 'n' represents the principal quantum number. This stability is the reason noble gases are largely inert and do not readily form chemical bonds.

Electron Shells and Orbitals

Electron shells are regions around the nucleus of an atom where electrons are likely to be found. Each shell can hold a specific number of electrons, and they are filled according to the Aufbau principle. The outermost shell, or valence shell, determines an element's chemical properties and reactivity.

Periodic Table Groups

The periodic table is organized into groups (columns) and periods (rows). Elements in the same group share similar chemical properties due to their similar valence electron configurations. For example, Group 18 elements, the noble gases, have full outer shells, making them stable and unreactive compared to elements in other groups.