the number listed is the average atomic mass, which represents the weighted average of all the naturally…

the number listed is the average atomic mass, which represents the weighted average of all the naturally occurring isotopes of that element. this weighted average takes into account the relative abundance of each isotope. for example, carbon - 12 is the most abundant of all carbon isotopes, which is why the average atomic mass of carbon is so close to 12.\ninstructions: use the reading on the first page to complete the questions below.\n1.) what is an isotope?\n2.) what do different isotopes of the same element have in common? what is different between them?\n3.) what is the difference between a stable isotope and a radioactive isotope?\n4.) briefly explain how isotopes play a role in cancer treatment.\n5.) what is the difference between the mass number and the average atomic mass of an element?\n6.) complete the chart below:\n| |chromium - 48|chromium - 50|chromium - 63|\n|----|----|----|----|\n|protons| | | |\n|neutrons| | | |\n|electrons| | | |

the number listed is the average atomic mass, which represents the weighted average of all the naturally occurring isotopes of that element. this weighted average takes into account the relative abundance of each isotope. for example, carbon - 12 is the most abundant of all carbon isotopes, which is why the average atomic mass of carbon is so close to 12.\ninstructions: use the reading on the first page to complete the questions below.\n1.) what is an isotope?\n2.) what do different isotopes of the same element have in common? what is different between them?\n3.) what is the difference between a stable isotope and a radioactive isotope?\n4.) briefly explain how isotopes play a role in cancer treatment.\n5.) what is the difference between the mass number and the average atomic mass of an element?\n6.) complete the chart below:\n| |chromium - 48|chromium - 50|chromium - 63|\n|----|----|----|----|\n|protons| | | |\n|neutrons| | | |\n|electrons| | | |

Answer

Brief Explanations:

  1. Isotopes are atoms of the same element with the same number of protons but different numbers of neutrons.
  2. Different isotopes of the same element have the same number of protons and electrons (in neutral state), thus the same atomic number and chemical - behavior. They differ in the number of neutrons and mass number.
  3. A stable isotope does not undergo radioactive decay spontaneously. A radioactive isotope emits radiation as it decays to a more stable form over time.
  4. Radioactive isotopes can be used in cancer treatment. For example, they can be used in radiation therapy to target and destroy cancer cells by emitting radiation that damages the DNA of the cancer cells, preventing them from growing and dividing.
  5. The mass number is the sum of protons and neutrons in a single isotope. The average atomic mass is a weighted - average of the masses of all naturally occurring isotopes of an element, taking into account their relative abundances.
  6. Chromium has an atomic number of 24. So for all its isotopes:
    • Protons: 24 for Chromium - 48, Chromium - 50, and Chromium - 63.
    • Neutrons: For Chromium - 48, 48 - 24 = 24; for Chromium - 50, 50 - 24 = 26; for Chromium - 63, 63 - 24 = 39.
    • Electrons: In a neutral atom, the number of electrons is equal to the number of protons, so 24 for all three isotopes.

Answer:

  1. Atoms of the same element with the same number of protons but different numbers of neutrons.
  2. Have the same number of protons and electrons (same atomic number and chemical - behavior); differ in the number of neutrons and mass number.
  3. Stable isotopes do not decay spontaneously; radioactive isotopes emit radiation as they decay.
  4. Radioactive isotopes are used in radiation therapy to damage cancer - cell DNA, preventing growth and division.
  5. Mass number is for a single isotope (sum of protons and neutrons), average atomic mass is a weighted - average of all isotopes' masses.
Chromium - 48 Chromium - 50 Chromium - 63
Protons 24 24 24
Neutrons 24 26 39
Electrons 24 24 24