Understanding Isotopes
* Isotopes are atoms of the same element (same number of protons) but with different numbers of neutrons. This difference in neutrons leads to different mass numbers.
Drawing Carbon Isotopes
1. Carbon-12 (¹²C)
* Protons: 6 (all carbon atoms have 6 protons)
* Neutrons: 6 (mass number - number of protons = 12 - 6 = 6)
* Electrons: 6 (atoms are neutral, so they have the same number of protons and electrons)
* Drawing:
* Nucleus: Draw a circle representing the nucleus. Inside, write "6p" for the protons and "6n" for the neutrons.
* Electron Shells: Draw two concentric circles around the nucleus to represent the electron shells. In the first shell, place 2 dots. In the second shell, place 4 dots.
2. Carbon-14 (¹⁴C)
* Protons: 6 (all carbon atoms have 6 protons)
* Neutrons: 8 (mass number - number of protons = 14 - 6 = 8)
* Electrons: 6 (atoms are neutral, so they have the same number of protons and electrons)
* Drawing:
* Nucleus: Draw a circle representing the nucleus. Inside, write "6p" for the protons and "8n" for the neutrons.
* Electron Shells: Draw two concentric circles around the nucleus to represent the electron shells. In the first shell, place 2 dots. In the second shell, place 4 dots.
Important Notes:
* Mass Number: The mass number is the total number of protons and neutrons in an atom's nucleus. It's written as a superscript to the left of the element symbol.
* Electron Configuration: Both isotopes of carbon have the same electron configuration because they have the same number of electrons. This means they have the same chemical properties.
* Radioactivity: Carbon-14 is a radioactive isotope, meaning its nucleus is unstable and decays over time. Carbon-12 is a stable isotope.
