Radioactive Nuclide Symbol Ba-131 Explained Correct Statement Analysis

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In the realm of nuclear chemistry, understanding the symbols and notations used to represent radioactive nuclides is crucial. These symbols provide a wealth of information about the composition of an atom's nucleus, including the number of protons and neutrons. Let's delve into the specifics of the radioactive nuclide represented by the symbol \${}_{56}^{131}Ba\ to determine which statement about it is correct.

Decoding the Nuclide Symbol: \${}_{56}^{131}Ba\

The symbol \${}_{56}^{131}Ba\ represents a specific isotope of barium, a chemical element with the symbol Ba. To fully understand this notation, let's break it down:

  • Ba: This is the chemical symbol for barium, which identifies the element. All atoms of barium have the same number of protons in their nucleus.
  • 56: This subscript number is the atomic number (Z). The atomic number represents the number of protons in the nucleus of an atom. In this case, barium has 56 protons.
  • 131: This superscript number is the mass number (A). The mass number represents the total number of protons and neutrons in the nucleus of an atom. For this barium isotope, there are 131 protons and neutrons combined.

The Significance of Atomic Number

The atomic number is the defining characteristic of an element. It dictates the element's position on the periodic table and determines its chemical properties. All atoms with 56 protons are, by definition, barium atoms. Changing the number of protons would transform the atom into a different element altogether.

Understanding Mass Number and Isotopes

The mass number is crucial for identifying different isotopes of an element. Isotopes are atoms of the same element (same number of protons) but with different numbers of neutrons. While the number of protons remains constant for a given element, the number of neutrons can vary, leading to isotopes with different mass numbers. In the case of \${}_{56}^{131}Ba\, the mass number of 131 indicates the total count of protons (56) and neutrons.

Calculating the Number of Neutrons

To determine the number of neutrons in the nucleus, we can use the following formula:

Number of Neutrons (N) = Mass Number (A) - Atomic Number (Z)

For \${}_{56}^{131}Ba\:

N = 131 - 56 = 75

Therefore, this isotope of barium has 75 neutrons in its nucleus.

Evaluating the Statements

Now that we've decoded the nuclide symbol and understand the concepts of atomic number, mass number, and neutron number, we can evaluate the given statements:

A. The atomic number of the radioactive nuclide is 75.

This statement is incorrect. As we determined from the symbol \${}_{56}^{131}Ba\, the atomic number (number of protons) is 56, not 75.

B. The mass number of the radioactive nuclide is 131.

This statement is correct. The superscript in the symbol \${}_{56}^{131}Ba\ indicates that the mass number, which is the sum of protons and neutrons, is indeed 131.

C. The number of neutrons that are present in the…

This statement is incomplete, but based on our calculations, we know that the number of neutrons is 75.

Conclusion

Therefore, the correct statement is B. The mass number of the radioactive nuclide is 131. This exercise demonstrates the importance of understanding nuclide symbols and how they convey crucial information about the composition of an atom's nucleus. By correctly interpreting these symbols, we can determine the atomic number, mass number, and the number of neutrons in a given nuclide. This knowledge is fundamental to understanding nuclear chemistry and the behavior of radioactive isotopes. Understanding the concept of radioactive decay is also critical. Radioactive decay is the process where an unstable atomic nucleus loses energy by emitting radiation. This often involves the transformation of one element into another. The rate of decay is characterized by the half-life, which is the time it takes for half of the radioactive material to decay. These concepts are crucial in various applications, including medical imaging, cancer treatment, and carbon dating. The ability to accurately interpret nuclide symbols and understand the properties they represent is a cornerstone of nuclear chemistry and its applications.

To further enhance our understanding, let's explore some related concepts in nuclear chemistry:

Isotopes and Nuclear Stability

As we mentioned earlier, isotopes are atoms of the same element with different numbers of neutrons. Not all isotopes are stable; some are radioactive and undergo decay. The stability of a nucleus depends on the balance between the number of protons and neutrons, as well as the nuclear forces that hold the nucleus together. Certain ratios of neutrons to protons are more stable than others. For instance, lighter nuclei tend to be stable when the number of neutrons is approximately equal to the number of protons. However, as the atomic number increases, stable nuclei tend to have more neutrons than protons. Nuclei that fall outside the band of stability are prone to radioactive decay, striving to reach a more stable configuration.

Types of Radioactive Decay

Radioactive decay occurs through various processes, each involving the emission of different particles or energy. The most common types of decay include:

  • Alpha Decay: This involves the emission of an alpha particle, which consists of two protons and two neutrons (equivalent to a helium nucleus). Alpha decay typically occurs in heavy nuclei and reduces both the atomic number and the mass number of the decaying nucleus.
  • Beta Decay: This type of decay involves the emission of a beta particle, which can be either an electron (β-) or a positron (β+). Beta-minus decay occurs when a neutron in the nucleus is converted into a proton, emitting an electron. Beta-plus decay occurs when a proton is converted into a neutron, emitting a positron. Beta decay changes the atomic number but does not significantly affect the mass number.
  • Gamma Decay: This involves the emission of gamma rays, which are high-energy photons. Gamma decay typically occurs after alpha or beta decay, as the nucleus releases excess energy to reach a more stable state. Gamma decay does not change the atomic number or the mass number.
  • Electron Capture: In this process, the nucleus captures an inner-shell electron, which combines with a proton to form a neutron. Electron capture decreases the atomic number by one but does not change the mass number.

Understanding Half-Life

Half-life is a fundamental concept in nuclear chemistry that describes the rate of radioactive decay. It is defined as the time required for half of the radioactive nuclei in a sample to decay. Half-life is a characteristic property of each radioactive isotope and can range from fractions of a second to billions of years. The decay of radioactive isotopes follows first-order kinetics, meaning that the rate of decay is proportional to the number of radioactive nuclei present. This allows us to predict the amount of radioactive material remaining after a certain period of time.

Applications of Radioactive Isotopes

Radioactive isotopes have numerous applications in various fields, including:

  • Medicine: Radioactive isotopes are used in medical imaging techniques, such as PET scans and SPECT scans, to diagnose diseases. They are also used in cancer therapy to target and destroy cancerous cells.
  • Industry: Radioactive isotopes are used in industrial radiography to inspect welds and other materials for defects. They are also used in gauging devices to measure the thickness of materials and the levels of liquids in containers.
  • Archaeology and Geology: Radioactive isotopes, such as carbon-14, are used in radiocarbon dating to determine the age of ancient artifacts and geological samples.
  • Research: Radioactive isotopes are used as tracers in research to study various processes in chemistry, biology, and other fields.

The Importance of Balancing Nuclear Equations

In nuclear chemistry, it is crucial to balance nuclear equations to ensure that the law of conservation of mass and charge is obeyed. A balanced nuclear equation shows the radioactive decay process, including the parent nucleus, the daughter nucleus, and the emitted particles. Balancing nuclear equations involves ensuring that the sum of the atomic numbers and the sum of the mass numbers are the same on both sides of the equation. This helps in predicting the products of nuclear reactions and understanding the transformations that occur during radioactive decay.

The study of radioactive nuclides and their properties is a fascinating and essential aspect of chemistry. By understanding the symbols, notations, and concepts discussed above, we can decipher the composition of atomic nuclei, predict their behavior, and appreciate the diverse applications of radioactive isotopes. From medical imaging to carbon dating, the principles of nuclear chemistry play a vital role in many areas of science and technology. Continued exploration of these concepts will undoubtedly lead to further advancements and discoveries in the field.

The symbol for a radioactive nuclide is \${}_{56}^{131}Ba\. Which of the following statements is correct regarding this nuclide?

Radioactive Nuclide Symbol Ba-131 Explained Correct Statement Analysis