Helium Atomic Mass

Atomic Mass of Helium. Atomic mass of Helium is 4.0026 u. The atomic mass is the mass of an atom. The atomic mass or relative isotopic mass refers to the mass of a single particle, and therefore is tied to a certain specific isotope of an element. Helium is a chemical element with atomic number 2 which means there are 2 protons and 2 electrons in the atomic structure. The chemical symbol for Helium is He. It is a colorless, odorless, tasteless, non-toxic, inert, monatomic gas, the first in the noble gas group in the periodic table. Helium, chemical element, inert gas of Group 18 (noble gases) of the periodic table. The second lightest element, helium is a colorless, odorless, and tasteless gas that becomes liquid at -268.9 degrees Celsius. The boiling and freezing points of helium are lower than those of any other known substance.

Question #1d260

2 Answers

Helium Ka Atomic Mass

Because that is the average atomic mass of its two stable isotopes.

Explanation:

The average atomic mass of an element is determined using the atomic masses and the abundances of its stable natural isotopes.

As you know, the identity of a chemical element is given by its atomic number, i.e. by the number of protons it has in its nucleus.

Rounded Atomic Mass Helium

For a given element, the number of neutrons it has in its nucleus can vary quite a lot. Atoms that have the same number of protons but different numbers of neutrons in their nucleus are called isotopes.

Each isotope will contribute to the average atomic mass of the element proportionally to its abundance.

Helium only has two stable isotopes, helium-3 and helium-4.

The atomic masses and abundances for these two isotopes are

#'^3'He' -> '3.0160293 u' '# and #' '0.000137%# abundance
#'^4'He' -> '4.002602 u' '# and #' '99.999863%# abundance

So, what will the average atomic mass of helium be? Deck building 101highlander: the card game. Notice that helium-3 has a very, very small abundance, which means that its atomic mass will contribute very, very little to the average.

#'avg. atom. mass' = sum_i ('isotope'_i xx 'abundance'_i)#

In helium's case, you have - I'll use decimal abundances, which are percent abundances divided by #100#

#m_a = '3.0160293 u' xx 0.00000137 + '4.002602 u' xx 0.99999863#

#m_a = '0.000004132 u' + '4.0025965 u'#

#m_a = '4.002601 u' ~~ '4.00 u'#

The average atomic mass of helium can thus be approximated to be #'4.00 u'#.

The atomic weight (mean relative mass) is not #'4.00 u'#. It is #'4.002602 u'# as reported on the periodic table published by the National Institute of Standards and Technology (NIST), the Webelements Periodic Table with full significant figures, and Vertex42.

Explanation: