Though the common isotope of aluminum has a mass number of...

Though the common isotope of aluminum has a mass number of $27,$ isotopes of aluminum have been isolated (or prepared in nuclear reactors) with mass numbers of $24,25,26,28,29,$ and $30 .$ How many neutrons are present in each of these isotopes? Why are they all considered aluminum atoms, even though they differ greatly in mass? Write the atomic symbol for each isotope.

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Key Concepts

Nuclidic Notation

Nuclidic notation is the method used to represent isotopes by writing the element symbol with the mass number as a superscript, and sometimes the atomic number as a subscript. This format provides a clear depiction of the composition of the nucleus.

Isotopes

Isotopes are forms of the same chemical element that have an identical number of protons but different numbers of neutrons. This variance in neutron number results in different mass numbers while the chemical properties remain similar because they are determined by the proton count.

Atomic Number and Mass Number

The atomic number of an element represents the number of protons in its nucleus, defining the element's identity, while the mass number is the sum of protons and neutrons. This distinction is essential for determining the composition of an atom.

Neutron Number Calculation

The number of neutrons in an isotope can be calculated by subtracting the atomic number (protons) from the mass number. This calculation explains how isotopes with different mass numbers can be variants of the same element.

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