Atoms with full outer electron shells are considered stable or unreactive. These atoms include the noble gases, which are helium (He), neon (Ne), argon (Ar), krypton (Kr), xenon (Xe), and radon (Rn).
Noble gases have a complete set of valence electrons, typically eight, except for helium, which has two valence electrons. The octet rule states that atoms are most stable when their outermost energy level is filled with eight electrons. Since noble gases already have a full outer electron shell, they do not readily gain, lose, or share electrons with other atoms, making them unreactive.
This stability arises from the arrangement of electrons in their orbitals. The outermost energy level in noble gases is completely filled, resulting in a stable electron configuration. This configuration provides a strong electrostatic force of attraction between the positively charged nucleus and the negatively charged electrons, making it energetically unfavorable for noble gases to react and form chemical bonds with other elements.
Which atoms are stable or unreactive? How many valence electrons do they have? Why do noble gasses not react with other atoms?
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