why are noble gas monoatomic?
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Inert gases, also known as noble gases, are monoatomic in nature. The simple reason for this is that they have completely filled octet which accounts for their high stability on their own. They don't have the necessity to bind with other atoms of their own kind to gain stability.
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Noble gases have large positive electron gain enthalpy. This is because the extra electron is placed in the next higher principal quantum energy levels. Thus, a highly unstable electronic configuration is produced.
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Argon is a noble gas so as such it does not form any compounds as it is very stable . It is monoatomic in the elemental state. Argon is an element belonging to group 18.
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Because noble gases' outer shells are full, they are extremely stable, tending not to form chemical bonds and having a small tendency to gain or lose electrons. ... Noble gas atoms, like the atoms in other groups, INCREASE steadily in atomic radius from one period to the next due to the INCREASING number of electrons.
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All noble gases have full s and p outer electron shells (except helium, which has no p sublevel), and so do not form chemical compounds easily. Their high ionization energy and almost zero electron affinity explain their non-reactivity. ... The first binary noble gas compounds were reported later in 1962.
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noble gas form compounds with oxygen and fluorine only because they are most electronegative elements. So they can ionise noble gases also.
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The noble gases (helium, neon, argon, krypton, xenon, and radon) are also gases at STP, but they are monatomic. The homonuclear diatomic gases and noble gases together are called "elemental gases" or "molecular gases", to distinguish them from other gases that are chemical compounds.
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The group 0 elements, the noble gases, are all unreactive non-metal gases. They show trends in their physical properties. Their uses depend on their inertness, low density and non-flammability.
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Noble gases have zero electron gain enthalpy because they contain all paired electrons and there is no place to accept another electron. All the orbitals are completely filled in them. So, they can't accept an electron and so the enthalpy is zero.
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The Chemical Properties The full valence electron shells of these atoms make noble gases extremely stable and unlikely to form chemical bonds because they have little tendency to gain or lose electrons. Although noble gases do not normally react with other elements to form compounds, there are some exceptions.
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For a long time noble gases with completely filled electron shells were considered to be simple. Under normal conditions they are monoatomic inert gases. Their behavior, however, depends on such conditions as density, temperature and pressure. ... When cooled or compressed, noble gases become liquid or solid.
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Noble gas. The noble gases are the chemical elements in group 18 of the periodic table. They are the most stable due to having the maximum number of valence electrons their outer shell can hold.
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In other words, they have the perfect number of electrons already, and don't need to form alliances with anything. This quality makes noble gases (also called "inert gases") intriguing, but their disdain for interacting with regular matter makes them very hard to detect.
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Octet Rule. The noble gases are unreactive because of their electron configurations. The noble gas neon has the electron configuration of 1 s 2 2 s 2 2 p 6 . It has a full outer shell and cannot incorporate any more electrons into the valence shell.
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Chemical Properties of Noble Gases Noble gases are the least reactive of all known elements. That's because with eight valence electrons, their outer energy levels are full. The only exception is helium, which has just two electrons.
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They are helium, neon, argon, krypton, xenon, and radon. They were once called inert gases because they were thought to be completely inert—unable to form compounds. This is a reasonable belief because the noble gases have a complete octet, making them very stable and unlikely to gain or lose any electrons.
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Noble gases have large positive electron gain enthalpies because the electron has to enter the next-higher principal quantum level leading to a very unstable electronic configuration. How do atomic radius vary in a period and in a group? ... As a result, atomic radii must increase.