The elements in Group 18 are known as noble gases.In terms of their electron configurations, explain what the noble gases all have in common.

Noble gases, which are the elements in Group 18 of the periodic table, all have full electron shells. This means that the outermost energy level of each atom is completely filled with electrons.

Here's a step-by-step explanation:

1. Electron configuration refers to the arrangement of electrons in an atom's electron shells.

2. The electron shells of an atom are filled according to the Aufbau principle, which states that electrons occupy the lowest energy level first.

3. The outermost electron shell of an atom is known as the valence shell. The chemical properties of an element are largely determined by the number of electrons in its valence shell.

4. Noble gases are unique because their valence shells are full. For example, helium has two electrons in its first and only shell, and neon has eight electrons in its second shell.

5. Because their valence shells are full, noble gases are stable and do not readily form chemical bonds with other elements. This is why they are called "noble" - they are 'unreactive' and do not easily engage with other elements.

6. This full electron configuration is what all noble gases have in common.