A new element, “Marshmallowium,” was discovered which had an atomic number of 110, and an atomic symbol of Mm. This element is very unstable and had a ½ life of only 15 seconds. Luckily we were able to get a fairly large sample of this delicious but rare element. But we must study it quickly because it will not last long.
Directions: Once everyone has a sample, Mm will begin its nuclear decay. Every 15 seconds half of the Mm will decay (we will eat half of it). After one minute we will mass how much Mm is remaining and enter that in the space below.
Original mass of Mm __________ Mass after 4 half lives __________
What should the theoretical mass of the Mm be after 1 minute?
How much of the sample would theoretically remain after 2 minutes?
In the most abundant isotope which is Mm – 270, how many neutrons are present? (Read the introduction paragraph at the top for the atomic number)
If Mm formed ions with a charge of -2, how many electrons would be present in those ions?
There are three different isotopes of this element.
Here are the weights and relative abundances: 88.00% 270.00 Mm, 10.40% 272.00 Mm, 1.60% 274.00 Mm. Before doing any calculations, estimate which number the average atomic mass will be closest to and explain your reasoning.
Calculate the average atomic mass of Mm using the numbers from the previous question. Express your answer to one decimal place.
Mm actually goes through a series of nuclear decay. It undergoes 2 alpha emissions and 1 beta emission. Show these balanced emissions as well as the final element.
Considering Mm emits alpha particles, why is it especially unwise to eat? (Think in terms of penetrating power).