Question

Naturally occurring magnesium consists primarily of three isotopes, of mass numbers $24,25,$ and 26 How many protons does each of these nuclides contain? How many neutrons does each of these nuclides contain? Write nuclear symbols for each of these isotopes.

Short answer

All magnesium isotopes have 12 protons. The isotope with mass number 24 has 12 neutrons, mass number 25 has 13 neutrons, and mass number 26 has 14 neutrons. Their nuclear symbols are ${}_{12}^{24}\text{Mg}$, ${}_{12}^{25}\text{Mg}$, and ${}_{12}^{26}\text{Mg}$.

Step-by-step solution

Determine the number of protons in magnesium isotopes

To find the number of protons in an element, we need its atomic number (Z). The atomic number is unique for each element and is the number of protons in its nucleus. Magnesium has an atomic number (Z) of 12, which means that all isotopes of magnesium will have 12 protons in their nucleus.

Determine the number of neutrons in magnesium isotopes

To find the number of neutrons (N) in an isotope, we use the mass number (A) and the atomic number (Z). Number of neutrons (N) = Mass number (A) - Atomic number (Z) Let's calculate the number of neutrons for each magnesium isotope: Isotope with mass number 24: Number of neutrons (N) = 24 - 12 = 12 Isotope with mass number 25: Number of neutrons (N) = 25 - 12 = 13 Isotope with mass number 26: Number of neutrons (N) = 26 - 12 = 14

Write the nuclear symbols for each magnesium isotope

A nuclear symbol is represented as: ${}_Z^A\text{Element Symbol}$ where Z = atomic number (number of protons) A = mass number (sum of protons and neutrons) Using this format, we can write the nuclear symbols for the magnesium isotopes: Isotope with mass number 24: ${}_{12}^{24}\text{Mg}$ Isotope with mass number 25: ${}_{12}^{25}\text{Mg}$ Isotope with mass number 26: ${}_{12}^{26}\text{Mg}$ In conclusion, the three isotopes of magnesium have 12 protons each, and their respective neutron counts are 12, 13, and 14. Their nuclear symbols are ${}_{12}^{24}\text{Mg}$, ${}_{12}^{25}\text{Mg}$, and ${}_{12}^{26}\text{Mg}$.

Key concepts

Magnesium Isotopes

Magnesium isotopes are versions of the magnesium element that have the same number of protons but different numbers of neutrons. Naturally occurring magnesium is composed mainly of three isotopes: those with mass numbers of 24, 25, and 26. These numbers represent the sum of protons and neutrons within the atom's nucleus.

In terms of real-world applications, magnesium isotopes are significant in fields such as geology and medicine. For example, the ratios of these isotopes in rocks can provide insights into the Earth's history and the processes that formed its layers.

Understanding these isotopes helps chemists and researchers make informed predictions and analyses based on their distinct physical and chemical properties.

Protons and Neutrons

In all elements, protons and neutrons are the particles that reside in the atom's nucleus. Protons carry a positive charge, while neutrons are neutral, carrying no charge. The number of protons in an atom is defined by its atomic number, making it unique to each element. This atomic number also determines the element's place on the periodic table.

For magnesium, the atomic number is 12, meaning every magnesium atom contains 12 protons. The presence of protons gives the element its identity, while neutrons, in varying numbers, result in different isotopes.

To determine the number of neutrons in an isotope, the atomic number (number of protons) is subtracted from the mass number. For example, in magnesium isotope with a mass number of 24, there are 12 neutrons because 24 - 12 equals 12. As you explore isotopes, remember that while the number of protons remains constant, the varying number of neutrons creates diverse isotopic forms.

Nuclear Symbols

Nuclear symbols provide a concise way to represent specific isotopes of an element. These symbols include essential information about the atomic number (number of protons), mass number (total protons and neutrons), and the element itself.

The format for a nuclear symbol is $${}_Z^A\text{Element Symbol}$$where:

• $Z$ is the atomic number.
• $A$ is the mass number.
• The element symbol is the one or two-letter abbreviation from the periodic table.

For magnesium isotopes:

• Mass number 24: ${}_{12}^{24}\text{Mg}$
• Mass number 25: ${}_{12}^{25}\text{Mg}$
• Mass number 26: ${}_{12}^{26}\text{Mg}$

Understanding nuclear symbols allows for quick and accurate communication of an atom's specifics. These symbols strip complex isotopic information down to a basic, understandable form, benefitting students and professionals alike in the sciences.