Explain why the noble gases are unreactive.

Noble gases are unreactive due to their electronic configuration. They have a complete outer shell of electrons, which makes them stable and unlikely to form chemical bonds with other elements. Here's a more detailed explanation:

Step 1: Define the Problem

Identify why noble gases are unreactive in terms of their atomic structure and properties.

Step 2: Break Down the Problem

1. Electronic Configuration: Noble gases have a full valence shell of electrons.
2. Stability: A full valence shell makes an atom stable and less likely to react.
3. Energy Considerations: Forming bonds would require energy to disrupt this stable configuration.

Step 3: Apply Relevant Concepts

• Octet Rule: Atoms tend to be more stable when they have eight electrons in their valence shell. Noble gases naturally have this configuration (except helium, which is stable with two electrons).
• Low Reactivity: Due to their full valence shells, noble gases have little tendency to gain, lose, or share electrons.

Step 4: Analysis, Verify and Summarize

• Helium (He): Has 2 electrons, filling its first and only shell.
• Neon (Ne), Argon (Ar), Krypton (Kr), Xenon (Xe), Radon (Rn): Each has a complete outer shell, following the octet rule.
• Chemical Inertness: This complete electron configuration results in minimal chemical reactivity.

Final Answer

Noble gases are unreactive because they have a complete outer electron shell, which makes them stable and unlikely to form chemical bonds. This stability is due to their adherence to the octet rule, resulting in low chemical reactivity.