There are two stable isotopes of bromine. their masses are 78.9183 and 80.9163 amu. if the average atomic mass of bromine is 79.9091 amu, what is the natural abundance of the heavier isotope? percent abundance of 81br __%

The percent abundance of ₈₁Br = 49.59%

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

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

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

Element Bromine has two isotopes, 78.9183 and 80.9163 amu.

The average atomic mass of bromine is 79.9091 amu

For example isotopes 78.9183 = x% and isotopes 80.9163 amu = 100-x%

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

79.9091 amu = 78.9183 %x +80.9163. (100-x)%

79.9091 amu = 78.9183 %x + 80.9163 .100% - 80.9163 %x

79.9091 amu = -1.998 %x + 80.9163

-1.0072 amu = -1.998 %x

%x = 0.5041

x = 50,41%

So percent abundance of ₈₁Br = 100% - 50.41% = 49.59%

The subatomic particle that has the least mass

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element 2512X

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about subatomic particles statement

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Keywords: mass number, atomic mass, amu, isotope, Bromine

b.

the accuracy of the data.

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