Ahypothetical element has two main isotopes with mass numbers of 62 and 65. if 66.00% of the isotopes have a mass number of 62 amu, what atomic weight should be listed on the periodic table for this element? answer in units of amu.

Answer is 63.04amu.

Explanation: We are given in the question that an element has two main isotopes 1 and 2.

Mass Number of isotope 1 = 62 amu

Mass Number of 2 isotope = 65 amu

% abundance of isotope 1 = 66%

Fractional abundance of isotope 1 = 0.66

Total fractional abundance = 1

Fractional abundance of isotope 2 = (1-0.66)

                                                          = 0.34

For calculating he atomic mass of element, we use

We have only 2 isotopes for an element, so the formula stops at isotope 2 only.

By putting the values in the above equation, we get

Atomic mass of element = 63.04amu

the electronic configuration of an atom with eight electrons is 1s²2s²2p⁴. the orbital diagrams are shown in the figure.

as per the hunds rule:

1. electrons tend to avoid being in the same orbital as per as practicable.

2. electrons in different orbitals of the same energy will have their spin parallel.

this can be illustrated from the multiplicity of the orbitals of the atom. as there are four electrons in the p orbital and p orbital has 3 sub-shells. the electrons can be fed in different ways as shown in the figure but the correct orbital diagram will be as per the hunds rule.

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