Isotopes

An isotope is a variant of a particular chemical element which differs in neutron number, and consequently in atomic mass, but not in chemical properties. All isotopes of a given element have the same number of protons in each atom.

Key Points to Understand about Isotopes:

1. Atomic Number: The number of protons in the nucleus of an atom determines the element's atomic number.
2. Neutrons: Isotopes of an element have the same number of protons but different numbers of neutrons.
3. Atomic Mass: The sum of protons and neutrons in the nucleus gives the atomic mass of an isotope.
4. Nuclear Stability: Some isotopes are stable, while others are radioactive and decay over time.

Examples of Isotopes:

One common example of isotopes is carbon. Carbon-12, carbon-13, and carbon-14 are all isotopes of carbon, with 6 protons each but 6, 7, and 8 neutrons, respectively.

Study Guide Questions:

1. What is an isotope?
2. How do isotopes of an element differ from each other?
3. Explain the concept of atomic mass in relation to isotopes.
4. What is the difference between stable and radioactive isotopes?
5. Provide examples of isotopes and their differences in neutron numbers.

Understanding isotopes is important in various scientific fields, including chemistry, physics, and geology. Mastery of this topic will provide a strong foundation for understanding atomic structure and the behavior of elements in nature and in the laboratory.

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