Question

A newly discovered element has two isotopes. one has an atomic weight of 120.9038 amu with 57.25% abundance. the other has an atomic weight of 122.8831 amu. what is the atomic weight of the element?

Answer 1

the atomic weight of the element : 122.22 amu

Further explanation

The elements in nature have several types of isotopes

Isotopes are atoms whose no-atom has the same number of protons while still having a different number of neutrons.

So Isotopes are elements that have the same Atomic Number (Proton)

Atomic mass is the average atomic mass of all its isotopes

In determining the mass of an atom, as a standard is the mass of 1 carbon-12 atom whose mass is 12 amu

So the atomic mass obtained is the mass of the atom relative to the 12th carbon atom

Mass atom X = mass isotope 1 . % + mass isotope 2.%

An atomic mass unit = amu is a relative atomic mass of 1/12 the mass of an atom of carbon-12.

The 'amu' unit has now been replaced with a unit of 'u' only

for example, Carbon has 3 isotopes, namely ₆¹²C, ₆¹³C, and ₆¹⁴C

Element has two isotopes. 120.9038 amu with 57.25% abundance and the other has an atomic weight of 122.8831 amu

Mass atom element X = mass isotope 1 . % + mass isotope 2.%

Mass atom element X = 120.9038 . 57.25% + 122.8831. 42.75%

Mass atom element X = 69.22 + 52.53 = 122.22 amu

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Keywords: mass number, atomic mass, amu, isotope

Answer 2

Atomic weight of the element = atomic weight of isotope 1 * abundance of isotope 1 +  atomic weight of isotope 2 * abundance of isotope 2

Atomic weight of the element = 120.9038 amu * 57.25% + 122.8831 amu * (1 - 57.25%)

Atomic weight of the element = 69.2174255 + 52.53252525 = 121.74995075

=> ~ 121.7500 <--------- answer