Isotopes

Isotopes are atoms of the same element that have the same number of protons but different numbers of neutrons. This means that isotopes have the same atomic number, representing the element, but different atomic masses due to the varying number of neutrons. For example, the most common form of carbon is carbon-12, with 6 protons and 6 neutrons, but there is also a rarer form called carbon-14, which has 6 protons and 8 neutrons.

Key Points to Remember:

1. Isotopes have the same number of protons but different numbers of neutrons.
2. Isotopes of an element have the same chemical properties but different physical properties due to their differing atomic masses.
3. Isotopes are used in various scientific fields, including medicine (for radioactive isotopes in imaging and treatment) and archaeology (for carbon dating).

Study Guide Questions:

1. What are isotopes?
2. How do isotopes of an element differ from each other?
3. Give an example of an isotope and explain its composition.
4. What are some practical applications of isotopes in different scientific fields?

[Isotopes] Related Worksheets and Study Guides:

• Atomic Structure - Set IIChemistry • High School
• Atomic Structure - Set IChemistry • High School
• Elements and the periodic tableChemistry • High School