Helium is known for its unique properties including its low density and non-reactivity. It was first discovered in 1868 by French astronomer Jules Janssen and British astronomer Joseph Norman Lockyer, who observed a yellow spectral line in the light of the sun during a solar eclipse.

Atomic Number2
Electron Configuration1s^2
Electrons Per Shell2

You will note that there is no bond length listed above. This is because the 1s shell can only hold a maximum of two electrons. Thus, He is stable entirely on its own without any bonding and exists naturally in this way. Two He atoms will generally find thtemselves approximately 50 Å apart. At the atomic scale, this is a significant distance!

Helium atoms visualized using VESTA. Note that the blue dashed line indicates a separation distance, not a bond.
Helium atoms visualized using VESTA. Note that the blue dashed line indicates a separation distance, not a bond.

One of the most common uses of helium is for balloons and blimps, due to its low density and ability to make objects lighter than air. It’s also used in a variety of scientific and industrial applications, including cooling MRI machines, welding, and as a coolant in nuclear reactors.

Helium exists in two forms: Helium-4, which is the most common isotope and makes up almost all natural helium, and Helium-3, which is much rarer and is used in a variety of scientific applications. Helium-4 is also used in cryogenics and as a cooling agent for rocket fuel.

Want to learn about other elements? Visit our page on the Periodic Table here!

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