Question

an unknown element has two primary isotopes, one with a relative abundance of 99.63 percent and a mass of 14.00307 u, and another with a relative abundance of 0.37 percent and a mass of 15.0011 u. what is the atomic weight of this element?

Answer 1

Protons and neutrons make up the compact, dense nucleus of an atom, which is positively charged and comparatively hefty.

How do you determine an element's Amu?

The total number of protons and neutrons in an isotope's nucleus is referred to as the mass number. This is due to the fact that each proton and neutron has a mass of one atomic mass unit (amu). You may get the mass of the atom by multiplying the total number of protons and neutrons by 1 amu.

What does "1 amu" or "1u" mean to you?

An element's atomic mass is expressed in terms of the atomic mass unit (AMU or amu) also referred to as the unified atomic mass unit or the Dalton (Da) (u)both atomic and molecular masses through the AMU. AMU is described as being one-twelfth the mass of a carbon-12 atom (12C).

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