Supply the missing information in the following table:

Verified step by step guidance

1. Identify the atomic number from the isotopic symbol, which is the subscript number (79) next to the element symbol (Au).
2. Recognize that the atomic number (79) is equal to the number of protons in the atom.
3. Identify the mass number from the isotopic symbol, which is the superscript number (198) next to the element symbol (Au).
4. Calculate the number of neutrons by subtracting the atomic number (79) from the mass number (198).
5. Fill in the table with the atomic number (79), mass number (198), number of protons (79), and the calculated number of neutrons.

Key Concepts

Isotopic Symbol

The isotopic symbol represents a specific isotope of an element, denoted by the element's chemical symbol along with its mass number as a superscript and atomic number as a subscript. For example, in the symbol 19879Au, 'Au' stands for gold, '79' is the atomic number indicating the number of protons, and '198' is the mass number, which is the total number of protons and neutrons.

Atomic Number

The atomic number is a fundamental property of an element that defines its identity, representing the number of protons in the nucleus of an atom. It determines the element's position in the periodic table and its chemical behavior. For instance, gold (Au) has an atomic number of 79, meaning it has 79 protons and, in a neutral atom, 79 electrons.

Mass Number

The mass number is the total count of protons and neutrons in an atom's nucleus, providing a measure of the atom's mass. It is crucial for distinguishing between different isotopes of the same element, which have the same number of protons but different numbers of neutrons. In the case of 19879Au, the mass number is 198, indicating that the isotope has 79 protons and 119 neutrons (198 - 79 = 119).