Question

Determine the average atomic mass of boron. The natural abundance of 10B (weighing 10.0129 amu) is 19.9% and the natural abundance of 11B (weighing 11.0093 amu) is 80.1%. Show all your work.

Answer 1

The atomic mass of boron with a natural abundance of 19.9% of 10 B and 80.1%  of 11 B is 10.801 amu

Boron has 2 isotopes.

First isotopes

mass = 10

% abundance = 19.9%

Second Isotopes

mass = 11

% abundance = 80.1%

Therefore,

Atomic mass = (19.9% of 10) + (80.1% of 11)

Atomic mass = (19.9 / 100 × 10) + (80.1 / 100 × 11)

Atomic mass = 199 / 100 + 881.1 / 100

Atomic mass = 1.99 + 8.811

Atomic mass = 10.801

Atomic mass = 10.801 amu

Although the kilogramme is the SI measure of mass, the unified atomic mass unit, or dalton, is a common way to represent atomic mass. An unbound carbon-12 atom in its ground state has a mass of 112 of a Da.

The total amount of protons and neutrons in an atom makes up the mass number. A whole number, that is. The average number of protons and neutrons among an element's natural isotopes is known as the atomic mass. It has a decimal form.

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