Question

K-41 is one of the naturally occurring isotopes of potassium. Use the periodic table to explain how the structure of K-41 differs from the normal K atom.

Answer 1

K-41 has the same number of protons and electrons as the most common isotope of potassium, K-39, but differs by having 22 neutrons instead of 20, leading to a different atomic mass and physical properties, while retaining the same chemical properties.

Step-by-step explanation:

K-41 is one of the naturally occurring isotopes of potassium. Potassium's atomic number is 19, which means a normal potassium atom contains 19 protons. The most abundant isotope of potassium is K-39, with 20 neutrons (since 39 minus 19 equals 20).

However, K-41 differs as it has 22 neutrons instead of the usual 20 found in K-39. Both isotopes have the same number of protons and electrons, and thus share the same chemical properties. The difference lies in the number of neutrons, which affects the atomic mass but not the chemical behavior. Since potassium's isotopes have the same electron configuration, with one electron in their valence shell, K-41, like K-39, is also likely to form a cation by losing its valence electron in chemical reactions. However, K-41 has a slightly different mass due to the extra neutrons, which can lead to different physical properties and is responsible for the isotope's contribution to background radiation through its decay process.