GITIM 6th Ion (32S): Anion, Protons, Neutrons, Electrons?

Hey guys! Let's dive into a fascinating chemistry question about the 6th ion of GITIM Publications, specifically concerning sulfur-32 (32S). This question involves understanding the fundamental properties of ions, including anions, and the relationships between protons, neutrons, and electrons. We'll break down each statement to determine its accuracy, making sure we grasp the underlying concepts. So, buckle up and let’s unravel this chemical puzzle together!

Analyzing the Statements About the 32S Ion

Let's examine each statement about the 32S ion in detail. Understanding the properties of ions and their atomic structure is key to solving this problem. We'll look at what it means to be an anion, the relationship between protons and neutrons, and how to calculate the number of electrons in an ion. By carefully analyzing each point, we can determine which statements hold true.

I. It is an anion.

This first statement claims that the 6th ion of sulfur-32 (32S) is an anion. But what exactly is an anion? An anion is an ion with a negative charge, meaning it has more electrons than protons. To determine if this statement is true, we need to understand how sulfur becomes an ion. Sulfur has an atomic number of 16, which means a neutral sulfur atom has 16 protons and 16 electrons. The question mentions the “6th ion,” which implies that the sulfur atom has gained electrons to achieve a -2 charge (S2-). This is because sulfur typically gains two electrons to achieve a stable octet configuration in its outermost electron shell. Therefore, the sulfur ion with a -2 charge is indeed an anion. So, the first statement is correct.

Understanding the concept of ions is crucial here. Atoms are electrically neutral when the number of protons (positive charge) equals the number of electrons (negative charge). However, atoms can gain or lose electrons to achieve a more stable electron configuration. When an atom gains electrons, it becomes negatively charged and is called an anion. Conversely, when an atom loses electrons, it becomes positively charged and is called a cation. The charge of an ion indicates the number of electrons gained or lost. For example, a -2 charge means the atom has gained two electrons, while a +1 charge means the atom has lost one electron. The stability of an atom is often related to having a full outermost electron shell, which typically means having eight electrons (octet rule). Sulfur, with six valence electrons, tends to gain two electrons to achieve this stable configuration, hence forming the S2- anion. This drive to achieve stability is a fundamental principle in chemistry and explains why certain elements tend to form specific types of ions. Therefore, identifying sulfur as an anion is the first step in correctly assessing the statements in the question.

II. The total number of protons equals the total number of neutrons.

Now, let’s consider the second statement: “The total number of protons equals the total number of neutrons.” To evaluate this, we need to look at the given isotopic notation for sulfur, which is 32S. The number 32 represents the mass number of the isotope. What does the mass number tell us? The mass number is the sum of protons and neutrons in the nucleus of an atom. We already know that sulfur has an atomic number of 16, meaning it has 16 protons. To find the number of neutrons, we subtract the number of protons from the mass number: 32 (mass number) - 16 (protons) = 16 neutrons. In this specific isotope of sulfur (32S), the number of protons (16) does indeed equal the number of neutrons (16). However, this is not a universal rule for all atoms or isotopes. It just happens to be true for this particular isotope of sulfur. So, the second statement is also correct.

The relationship between protons and neutrons is a core concept in understanding atomic structure and isotopes. Protons, located in the nucleus, define the element; an atom with 16 protons is always sulfur. Neutrons, also in the nucleus, contribute to the mass of the atom but do not affect its charge. Isotopes are variants of an element that have the same number of protons but different numbers of neutrons. For instance, while 32S has 16 neutrons, other isotopes of sulfur exist, such as 34S, which has 18 neutrons. The mass number, which is the sum of protons and neutrons, distinguishes these isotopes. It's important to note that the number of protons determines the element's identity, while the number of neutrons can vary, leading to different isotopes of the same element. The fact that the number of protons and neutrons is equal in 32S is a specific case and not a general property of all elements or isotopes. Therefore, understanding the composition of the nucleus, the roles of protons and neutrons, and the concept of isotopes is crucial in analyzing the second statement.

III. The total number of electrons is 50.

Finally, let’s tackle the third statement: “The total number of electrons is 50.” We know that a neutral sulfur atom has 16 electrons (equal to the number of protons). However, as we determined in the first statement, the 6th ion implies a -2 charge (S2-), meaning the sulfur atom has gained two electrons. So, to calculate the total number of electrons in the S2- ion, we add the two gained electrons to the original 16 electrons: 16 (electrons in neutral S) + 2 (gained electrons) = 18 electrons. Therefore, the total number of electrons in the 32S2- ion is 18, not 50. This makes the third statement incorrect.

The process of calculating the number of electrons in an ion is fundamental to understanding its chemical behavior. In a neutral atom, the number of electrons is equal to the number of protons, ensuring a balanced charge. However, when an atom gains or loses electrons to form an ion, this balance is disrupted. Gaining electrons results in a negative charge (anion), and losing electrons results in a positive charge (cation). The magnitude of the charge indicates the number of electrons gained or lost. For instance, a -2 charge means the atom has gained two electrons, while a +1 charge means it has lost one electron. Applying this to the sulfur ion (S2-), we know that sulfur typically gains two electrons to achieve a stable electron configuration, resulting in 18 electrons (16 original electrons plus 2 gained electrons). This understanding of electron gain or loss and its impact on the ion's charge is crucial in determining the electron count and, consequently, the accuracy of the statement. Therefore, correctly calculating the number of electrons is essential for assessing the chemical properties and behavior of ions.

Conclusion: Which Statements Are True?

Alright, guys, we've dissected each statement about the 32S ion. To recap: Statement I is correct because the 6th ion of sulfur (S2-) is indeed an anion. Statement II is also correct for this specific isotope (32S), as the number of protons equals the number of neutrons. However, Statement III is incorrect because the total number of electrons in the S2- ion is 18, not 50. Therefore, the correct answer is that statements I and II are true.

In conclusion, understanding the basics of atomic structure, isotopes, and ions is crucial for tackling chemistry questions like this. Remember to consider the definitions of anions, the relationship between protons and neutrons, and how to calculate the number of electrons in an ion. By applying these concepts, you can confidently analyze and solve similar problems. Keep up the great work, guys, and happy learning!