Write the atomic symbol for the isotope with each of the...

Write the atomic symbol for the isotope with each of the following characteristics:
a. an oxygen atom with 10 neutrons
b. 4 protons and 5 neutrons
c. 25 electrons and 28 neutrons
d. a mass number of 24 and 13 neutrons
e. a nickel atom with 32 neutrons

Key Concepts

Isotopes

Isotopes are forms of an element that have the same number of protons but different numbers of neutrons. This variation in neutron count leads to differences in the mass numbers of the isotopes while maintaining the same chemical properties because the number of protons (and thus electrons in a neutral atom) remains unchanged.

Atomic Number

The atomic number of an element, which is equal to the number of protons in its nucleus, uniquely identifies the element. This number is usually written as a subscript to the left of the element’s chemical symbol and is fundamental for determining its position on the periodic table.

Mass Number

The mass number of an isotope is the total count of protons and neutrons in the nucleus. It is typically placed as a superscript to the left of the element’s symbol. The mass number is used to distinguish between different isotopes of the same element.

Isotopic Notation

Isotopic notation is a standardized method of writing the symbol for an isotope where the mass number is shown as a superscript at the top left and the atomic number is shown as a subscript at the bottom left of the element symbol. This notation succinctly conveys both the identity of the element and the specific isotope by indicating its nuclear composition.

Neutron Calculation

To determine the number of neutrons in an atom, subtract the atomic number (number of protons) from the mass number (total nucleons). This relationship is often used when the characteristics of an isotope are described in terms of its neutrons, protons, or electrons.

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