The average atomic mass of naturally occurring rubidium is 85.4678 amu. There are two common isotopes of naturally occurring rubidium as indicated [Isotope Rb-85, Mass (amu) 84.91179; and Isotope Rb-87,Mass (amu) 86.90919) a. Using the information above i. Calculate the percent abundance of each isotope. Be sure to match each isotope with a percent. ii. Calculate the number of Rb-87 atoms in a 10.60 g sample of the naturally occurring isotope. b. A major line in the emission spectrum of rubidium has an energy value of 2.88X10-19 J. Calculate the wavelength, in nanometers, of light that corresponds to this line. c. In the upper atmosphere ozone molecules decompose as they absorb ultraviolet(UV) radiation, as shown by the equation below. Ozone serves to block harmful ultraviolet radiation that comes from the Sun, O3(g)=>O2(g) +O(g) A molecule of O3(g) absorbs a photon with a frequency of 1.00 X 1015 s-1. i. How much energy, in joules, does the O3(g) molecule absorb per photon? ii. The minimum energy needed to break an oxygen-oxygen bond in ozone is 387 kJ monl-1. Does a photon with a frequency of 1.00 X 1015 s-1 have enough energy to break the bond?