There are four naturally occurring isotopes of strontium: ^8438 Sr, 38^86 Sr, 38^87 Sr, 38^88 Sr

step 1 The question here has, A, how many protons neutrons, electrons are in strontium 87? So it's goin

There are four naturally occurring isotopes of strontium:...

There are four naturally occurring isotopes of strontium: $^{84}_{38} \mathrm{Sr}$, $_{38}^{86} \mathrm{Sr}, _{38}^{87} \mathrm{Sr}, _{38}^{88} \mathrm{Sr}.$ a. How many protons, neutrons, and electrons are in $\mathrm{Sr}-87 ?$ b. What is the most prevalent isotope in a strontium sample? c. How many neutrons are in Sr-84? d. Why don't any of the isotopes of strontium have the atomic mass of 87.62 amu listed on the periodic table?

There are four naturally occurring isotopes of strontium: $^{84}_{38} \mathrm{Sr}$, $_{38}^{86} \mathrm{Sr}, _{38}^{87} \mathrm{Sr}, _{38}^{88} \mathrm{Sr}.$
a. How many protons, neutrons, and electrons are in $\mathrm{Sr}-87 ?$
b. What is the most prevalent isotope in a strontium sample?
c. How many neutrons are in Sr-84?
d. Why don't any of the isotopes of strontium have the atomic mass of 87.62 amu listed on the periodic table?

Key Concepts

Atomic Structure

This concept involves understanding that an atom consists of protons, neutrons, and electrons. The number of protons, determined by the atomic number, defines the element, while the protons and neutrons form the nucleus. Electrons orbit the nucleus and balance the positive charge of protons in a neutral atom.

Isotopes

Isotopes are variants of a particular chemical element that have the same number of protons but differ in the number of neutrons. This difference in neutron count leads to varying mass numbers for the isotopes of an element without affecting its chemical properties.

Mass Number vs Atomic Mass

The mass number of an isotope is the sum of its protons and neutrons and is always a whole number, whereas the atomic mass listed on the periodic table is a weighted average of the masses of all the naturally occurring isotopes of an element. This average takes into account the relative abundance and the individual mass numbers of the isotopes.

Natural Abundance

Natural abundance refers to the relative proportions of the different isotopes of an element found in nature. The average atomic mass on the periodic table is calculated based on these natural isotopic abundances, meaning that the most abundant isotope will have a greater influence on this value, even though none of the isotopes individually has that exact mass.

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