Why don't noble gases react with other chemicals?

Answer 1

Noble or inert gases don't react with other elements because their outer electron shells are completely full. It's all about the electron configuration in the outer shell (or valence shell or valence band) of a given atom. When the outer electron shell in an atom is full, the electrons there are "happy with their arrangement" and the atom does not want to either loan out or borrow electrons. The very basis of chemistry is the loaning out or borrowing of electrons to make a given atom "feel like its outer electron shell is full" so it can be "happy" with things. There is "balance" achieved when an atom has or can "simulate" having a full outer electron shell. Let's have a quick look at the electrostatics that make up an atom. An atom has protons and neutrons bound together in the nucleus, and the positive charge on the nucleus attracts electrons, which "form up" around it in energy levels or shells. That's atomic structure. Remember that the electrons don't like each other because like charges repel, and the electrons are negatively charged. Whatever the arrangement the electrons arrive at, they have to arrange some kind of "deal" amongst themselves to "stay out of each other's way" as it were. They form up in shells and subshells, and they have spin components that allow them to "get along with each other" in a given subshell. That's the basic electrostatics that give the atom structure. (The electrons have too much kinetic energy to "fall into" the nucleus, so they orbit atoms.) When the electron configuration is "set up" by an atom, the electrons decide how "happy" they are with a given structure. And an atom will then behave in a way to try to emulate or simulate an atom with a full outer shell if it doesn't have one. If it lacks an electron or two from having a full shell, it will want to borrow those electrons. If it has only an electron or two in its outer shell, it will want to loan those out to achieve that "magic configuration" and feel like it's an inert gas. In an inert or noble gas, the outer electron shell, the valence shell or valence band, is full. That atom will, because the outer shell is "maxed out" and cannot hold any more electrons, wander around by itself steering clear of any borrowing or loaning out activities (any chemical reactions) 'cause it's "happy" like it is.
The noble gases (helium, neon, argon, krypton, xenon and radon) have full valence electron shells, and as such are already in the lowest possible energy state. They do not need to react and gain or lose more, so are completely inert.

However, the heavier noble gases actually can be forced to react with very electronegative elements like oxygen and fluorine. However, they don't do so readily.
Noble gases have completely filled orbitals / energy levels. They generally have 8 valence electrons (helium has only 2) and have stable electronic configuration. Hence they are chemically inert and generally donot form compounds under normal conditions.

Answer 2

Noble gases have a full outer electron shell, making them stable and unreactive. This stability means they do not need to gain, lose, or share electrons with other elements, so they do not readily form chemical bonds.

Answer 3

Noble gases have completely filled valence electrons. hence they are stable and chemically inert.