Particles having the same atomic number but different mass numbers are called

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Examoogle · Accepted Answer

Isotopes

Explanation: Atoms of the same chemical element that possess the same atomic number (number of protons) but different mass numbers (sum of protons and neutrons) are known as isotopes. This variation arises solely from a difference in the number of neutrons within the atomic nucleus. Working Principle: In an atom, the atomic number $Z$ defines the identity of the element. Since isotopes maintain the same $Z$, their chemical properties remain nearly identical. However, the mass number $A$ changes because $A = Z + N$, where $N$ is the number of neutrons. Consequently, isotopes exhibit different physical properties such as atomic mass and nuclear stability (radioactivity). Key Formulas: $A = Z + N$ — representing the mass number $A$, atomic number $Z$, and neutron count $N$. Key Points: Isotopes have identical chemical properties due to the same electron configuration.; The presence of extra neutrons can make certain isotopes unstable (radioisotopes).; Isotopes are essential in nuclear power for fission reactions, such as $^{235}U$. Advantages: Used in medical imaging and radiotherapy.; Crucial for carbon dating and archaeological research.; Enables nuclear power generation via controlled fission. Disadvantages: Radioactive isotopes produce hazardous nuclear waste.; Requires complex enrichment processes for nuclear fuel. Applications: Nuclear power plants (e.g., Uranium-235).; Medical tracers and cancer treatment.; Industrial thickness gauging and sterilization. Additional Info: Option A (Positrons) are the antimatter counterparts of electrons.. Option B (Beta particles) are high-energy electrons or positrons emitted during radioactive decay.. Option D (Decayed particles) is a generic term not defining a nuclear configuration based on atomic numbers. Answer: C is correct — Isotopes are atoms sharing the same proton count but differing in neutron count, leading to distinct mass numbers. Exam Tip: Always remember: Isotopes change 'N' (neutrons), Isobars change 'Z' (protons), and Isotones maintain the same number of neutrons ($N$).

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