What are Isotopes?
* Isotopes are atoms of the same element (like carbon) that have the same number of protons but a different number of neutrons.
* Since the number of protons defines the element, isotopes behave chemically almost identically but have slightly different masses due to the varying number of neutrons.
Carbon Isotopes
Carbon has two main naturally occurring isotopes:
1. Carbon-12 (¹²C): This is the most common isotope, making up about 98.9% of all carbon found on Earth. It has 6 protons and 6 neutrons. Its atomic mass is exactly 12 amu by definition.
2. Carbon-13 (¹³C): This isotope is less abundant, making up about 1.1% of carbon. It has 6 protons and 7 neutrons. Its atomic mass is approximately 13 amu.
Key Points
* Definition of amu: The atomic mass unit (amu) is defined as 1/12th the mass of a single carbon-12 atom.
* Mass Difference: The difference in amu between carbon isotopes is primarily due to the extra neutron in ¹³C compared to ¹²C. This difference is relatively small but measurable.
Why Does the Difference Matter?
* Radioactive Isotopes: Some isotopes of carbon, like Carbon-14 (¹⁴C), are radioactive and have applications in dating archaeological artifacts.
* Mass Spectrometry: Instruments like mass spectrometers can differentiate between isotopes based on their mass, helping scientists study their relative abundance and use them in various applications.
Let me know if you'd like more details about a specific carbon isotope or its applications!
