The iodine isotope with 72 neutrons Enter the isotopic symbol in the form X-A . For example, C-13. he phosphorus isotope with 14 neutrons Enter the isotopic symbol in the form X-A . For example, C-13. The uranium isotope with 145 neutrons Enter the isotopic symbol in the form X-A . For example, C-13. the argon isotope with 22 neutrons Enter the isotopic symbol in the form X-A . For example, C-13.
The Correct Answer and Explanation is:
To find the isotopic symbols of the specified elements, we need to know two key pieces of information for each isotope: the chemical symbol of the element and the total number of nucleons (protons + neutrons). The isotopic symbol is expressed in the form (X-A), where (X) is the element symbol and (A) is the mass number (the sum of protons and neutrons).
1. Iodine Isotope with 72 Neutrons
- Atomic Number of Iodine (I): 53 (iodine has 53 protons).
- Neutrons: 72.
- Mass Number (A): (A = \text{protons} + \text{neutrons} = 53 + 72 = 125).
- Isotopic Symbol: I-125.
2. Phosphorus Isotope with 14 Neutrons
- Atomic Number of Phosphorus (P): 15 (phosphorus has 15 protons).
- Neutrons: 14.
- Mass Number (A): (A = 15 + 14 = 29).
- Isotopic Symbol: P-29.
3. Uranium Isotope with 145 Neutrons
- Atomic Number of Uranium (U): 92 (uranium has 92 protons).
- Neutrons: 145.
- Mass Number (A): (A = 92 + 145 = 237).
- Isotopic Symbol: U-237.
4. Argon Isotope with 22 Neutrons
- Atomic Number of Argon (Ar): 18 (argon has 18 protons).
- Neutrons: 22.
- Mass Number (A): (A = 18 + 22 = 40).
- Isotopic Symbol: Ar-40.
Summary of Isotopic Symbols
- Iodine: I-125
- Phosphorus: P-29
- Uranium: U-237
- Argon: Ar-40
Explanation
Each element on the periodic table has a unique atomic number, which corresponds to the number of protons in its nucleus. The number of neutrons can vary, leading to different isotopes of the same element. The mass number is the total count of protons and neutrons in an isotope. In the case of iodine, phosphorus, uranium, and argon, we calculated their isotopic symbols by adding the number of protons (which is fixed for each element) to the given number of neutrons. This method allows us to identify isotopes accurately, providing insight into their stability, nuclear properties, and potential applications in various fields such as medicine, energy, and research. Isotopes can behave differently in chemical reactions and decay processes, which is why precise identification is critical in chemistry and related sciences.