Question

An atom that has an atomic number of 38 and a mass number of 88 is an isotope of an atom that has

Answer 1

The atomic number is the number of protons in the nucleus of the atom.

The mass number is the number of protons and neutrons in the nucleus of an atom.

Isotopes have the same atomic number but a different mass number.

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Answer 2

Answer: The isotopic representation of the atom is $_{38}^{50}\textrm{Sr}$

Explanation:

Atomic number is defined as the number of electrons or number of protons that are present in a neutral atom. It is represented as Z.

Z = Atomic number = Number of electrons = Number of protons

Mass number is defined as the sum of number of protons and number of neutrons present in an atom. It is represented as A.

A = Mass number = Number of protons + Number of neutrons

We are given:

Atomic number = Number of protons = 38

Mass number = 88

Number of neutrons = Mass number - Atomic number = 88 - 38 = 50

General isotopic representation of an element is $_Z^A\textrm{X}$

where,

Z = atomic number

A = Mass number

X = symbol of the element

Hence, the isotopic representation of the atom is $_{38}^{50}\textrm{Sr}$