Final answer:
The noble gases, found in group 18 of the Periodic Table, are historically known for being nonreactive due to their full valence shells. They are gases at room temperature and include helium, neon, argon, krypton, xenon, and radon. Despite their reknown stability, noble gases can form compounds, as proven by Dr. Neil Bartlett's research.
Step-by-step explanation:
The noble gases are located in group 18 of the Periodic Table. These elements, which include helium, neon, argon, krypton, xenon, and radon, are called noble because they were once thought to be completely nonreactive. This is due to their filled valence shells, which mean they generally do not need to gain or lose electrons to achieve a more stable configuration. However, in 1962, the assumption of their non-reactivity was challenged by Dr. Neil Bartlett who succeeded in forming a chemical compound with a noble gas.
All noble gases are monatomic and are in a gaseous state at room temperature. Their lack of reactivity makes these gases particularly useful in applications where a non-reactive atmosphere is needed, such as in welding, lighting, and in certain types of laboratory research.
The electron configuration of noble gases is significant because it provides them with a stable structure that rarely interacts with other elements to form compounds.