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Noble gases

The elements that make up the family of noble gases include helium, neon, argon, krypton, xenon, and radon.

What are the similar properties of noble gases?

Noble gases share many similar properties including:
A full outer shell of electrons. Helium has two electrons in its outer shell and the rest have eight electrons.
Because of their full outer shells, they are very inert and stable. This means they don’t tend to react with other elements to form compounds.
They are gases under standard conditions.
They are colorless and odorless.
Their melting and boiling points are close together giving them a very narrow liquid range.
adapted from http://www.chem4kids.com/files/elem_noblegas.html

The noble gases are a family elements, in the far right column of the periodic table.  Group Zero, or Group eighteen (Group XVIII).

This family has the “happiest” elements of all. Why Are They Happy?

Using the Bohr description of electron shells, happy atoms have full electron shells. All of the noble gases have full outer shells with eight electrons.

Oh, wait! That’s not totally correct. At the top of the noble gases is little helium (He), with a shell that is full with only two electrons. The fact that their outer shells are full means they are quite happy and don’t need to react with other elements. In fact, they rarely combine with other elements. That non-reactivity is why they are called inert.
Who’s in the Family?

Neon is one of many inert gases used around you All of the elements in Group Zero are noble gases. The list includes helium, neon (Ne), argon (Ar), krypton (Kr), xenon (Xe), and radon (Rn). Don’t think that, because these elements don’t like to react, we don’t use them. You will find noble gases all over our world. Neon is used in advertising signs. Argon is used in light bulbs. Helium is used in balloons and to cool things. Xenon is used in headlights for new cars. Because of their chemical properties, these gases are also used in the laboratory to help stabilize reactions that would usually proceed too quickly. When you move down the periodic table, as the atomic numbers increase, the elements become rarer. They are not just rare in nature, but rare as useful elements, too.
But Wait, They Do Bond!

Some do. As of about 40 years ago, scientists have been able to make some compounds with noble gases. Some have been used in compounds to make explosives, and others just form compounds in a lab. The thing to remember is that they were forced. When going about their natural lives, you will never (well, never say never, because there may be an exception) find the noble gases bonded to other elements.

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