There are three naturally occurring stable isotopes of magnesium: 24MB, 25MB, and 26Mg, which haverelative abundances on Earth of 79%, 10%, and 11% respectively. Note that the atomic number ofmagnesium is 12.a) Describe what is meant by an isotope with reference to atomic and mass numbers. Determine thenumber of protons and neutrons for each of the three isotopes of naturally occurring stablemagnesium.b) i)A magnesium-24 nucleus can be considered as nucleons uniformly distributed in a sphericalvolume. Calculate the energy required to construct a uniformly charged sphere, using the following2Q2equation: U =where Q is the total charge and R is the radius.20πεο R 'ii) Calculate the binding energy (in eV) of magnesium-24, which has an atomic mass of 23.9850 AMU.The mass of a neutron is 1.0087 amu and the mass of a proton is 1.0073 amu.iii) Using your results from parts (i) and (ii) discuss how the nucleus is held together.c) The radioisotope of magnesium with the longest half-life is magnesium-28, with a half-life of 20.9hrs. Magnesium-28 decays through B- decay into aluminium-28. With reference to fundamentalparticles, describe the process which occurs in beta minus decay. Hence determine the equation forthe decay of magnesium-28 into aluminum-28.

According to Q&A guidelines of Bartleby, we are supposed to answer only the first question out…

There are three naturally occurring stable isotopes of magnesium: 24Mg, 25M., and 2°Mg, which have relative abundances on Earth of 79%, 10%, and 11% respectively. Note that the atomic number of magnesium is 12. a) Describe what is meant by an isotope with reference to atomic and mass numbers. Determine the number of protons and neutrons for each of the three isotopes of naturally occurring stable magnesium.

There are three naturally occurring stable isotopes of magnesium: 24Mg, 25M., and 2°Mg, which have relative abundances on Earth of 79%, 10%, and 11% respectively. Note that the atomic number of magnesium is 12. a) Describe what is meant by an isotope with reference to atomic and mass numbers. Determine the number of protons and neutrons for each of the three isotopes of naturally occurring stable magnesium.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

How to arrange this isotopes? according to its increasing stability
An atom has a diameter of 3.00 Å and the nucleus of that atom has a diameter of 7.50 × 10-5 Å. Determine the fraction of the volume of the atom that is taken up by the nucleus. Assume the atom and the nucleus are a sphere. fraction of atomic volume: Calculate the density of a proton, given that the mass of a proton is 1.0073 amu and the diameter of a proton is 1.69 × 10-¹5 m. density: g/cm³
1.)fluorine-20 Express your answers as integers separated by a comma. 2.)cobalt-63 Express your answers as integers separated by a comma. 3.)iron-59 Express your answers as integers separated by a comma. Give the number of protons and number of neutrons in the nucleus for all 3 I need help
An element has the following natural abundance and isotopic masses: 90.92% abundance with 19.99amu, 0.26% abundance with 20.99amu and 8.82% abundance with 21.99amu. Calculate the average atomic mass of this element.
Need help on part C and part D
Diane, Timothy and Ira were having a discussion about isotopes and the tendency to react. Which do you suggest offers the best explanation? Diane felt that isotopes would react the same as the atoms of the same element since they had the same number of valence electrons. Timothy suggested that they would react the same since the isotope and the atom of the same element would have the same number of total electrons. Ira said that the isotopes would react different since the number of neutrons would vary and therefore the atomic mass of the isotopes versus the atom of the same element would be different.
An unknown element is determined to have two naturally occurring isotopes. Isotope 1 is 68.11% abundant and has a mass of 68.925580 amu, and isotope 2 has a mass of 70.9247005 amu. Determine the atomic mass of the unknown element. Express your answer to four significant figures.
6. The atomic mass of an element is found as the decimal number on the periodic table. For example, the atomic mass of Vanadium is 50.94 amu. Using this atomic mass, predict which isotope of vanadium is most abundant in nature. Vanadium-23 Vanadium-51 Vanadium-50
Carbon, nitrogen, and oxygen have 6, 7 and 8 protons in their nucleus. How many neutrons are in their nucleus as well, for the normal stable isotopes of these elements.
the atom bromine79 has an isoptopic mass of 78.91 while bromine 81 has an isotopic mass of 80.91. determine the percentage of each bromine isotope.
A certain element consists of two stable isotopes. The first has a mass of 113 amu and a percent natural abundance of 4.28 %. The second has a mass of 115 amu and a percent natural abundance of 95.7 %. What is the atomic weight of the element? amu
1. explain what happens to an atom when the number of protons, neutrons, or electrons changes, while the number of the other two particles remains the same. 2. Are there different ways to make an oxygen atom?