Platinum has six isotopes: ^190 Pt,^192 Pt,^194 Pt,^195 Pt,^196 Pt, and ^198 Pt a. How many neut

step 1 Okay, so for Part A, we're asked to find how many neutrons are in each isotope. So we call that

Platinum has six isotopes: ^190 Pt,^192 Pt,^194 Pt,^195...

Platinum has six isotopes: $^{190} \mathrm{Pt},^{192} \mathrm{Pt},^{194} \mathrm{Pt},^{195} \mathrm{Pt},^{196} \mathrm{Pt},$ and $^{198} \mathrm{Pt}$ a. How many neutrons are there in each isotope? b. The natural abundances of the six isotopes are $0.014 \%^{190} \mathrm{Pt}(189.96 \mathrm{amu}) ; 0.782 \%^{192} \mathrm{Pt}(191.96 \mathrm{amu})$ $32.967 \%^{194} \mathrm{Pt}(193.96 \mathrm{amu}) ; 33.832 \%^{195} \mathrm{Pt}(194.97 \mathrm{amu})$ $25.242 \%^{196} \mathrm{Pt}(195.97 \mathrm{amu}) ;$ and $7.163 \%^{198} \mathrm{Pt}$ $(197.97 \mathrm{amu}) .$ Calculate the average atomic mass of platinum and compare it with the value in the periodic table on the inside front cover.

Platinum has six isotopes: $^{190} \mathrm{Pt},^{192} \mathrm{Pt},^{194} \mathrm{Pt},^{195} \mathrm{Pt},^{196} \mathrm{Pt},$ and
$^{198} \mathrm{Pt}$
a. How many neutrons are there in each isotope?
b. The natural abundances of the six isotopes are $0.014 \%^{190} \mathrm{Pt}(189.96 \mathrm{amu}) ; 0.782 \%^{192} \mathrm{Pt}(191.96 \mathrm{amu})$
$32.967 \%^{194} \mathrm{Pt}(193.96 \mathrm{amu}) ; 33.832 \%^{195} \mathrm{Pt}(194.97 \mathrm{amu})$
$25.242 \%^{196} \mathrm{Pt}(195.97 \mathrm{amu}) ;$ and $7.163 \%^{198} \mathrm{Pt}$
$(197.97 \mathrm{amu}) .$ Calculate the average atomic mass of platinum and compare it with the value in the periodic table on the inside front cover.

Key Concepts

Atomic Mass Unit

The atomic mass unit (amu) is a standard unit of mass that quantifies mass on an atomic or molecular scale. It is based on the mass of a carbon-12 atom and provides a convenient measure for expressing the masses of isotopes in atomic mass calculations.

Natural Abundance

Natural abundance refers to the relative proportion of each isotope of an element as it occurs in nature. These percentages are essential when calculating weighted averages, as they indicate the contribution of each isotope’s mass to the overall atomic weight.

Weighted Average Calculation

The average atomic mass of an element is computed as a weighted average using the masses of its isotopes and their natural abundances. Multiplying each isotope's mass by its fractional abundance and summing these products gives the average atomic mass, which is the value typically reported on the periodic table.

Isotopes

Isotopes are variants of a given chemical element that share the same number of protons (defining the element) but differ in the number of neutrons, resulting in different mass numbers. This concept is crucial because isotopes determine the atomic mass of an element based on the mix of these variants found in nature.

Neutron Number Calculation

The neutron number of an isotope is calculated by subtracting the atomic number (the number of protons) from the mass number (the total number of protons and neutrons). This method helps determine the composition of the nucleus for each isotope.

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