3. (c) I (d) Ag An element has two naturally occurring isotopes. Isotope 1 has a mass of 120.9038 amu and a relative abundance of 57.4%, and isotope 2 has a mass of 122.9042 amu and a relative abundance of 42.6%. Find the atomic mass of this element and, referring to the periodic table, identify it. Show all mathematical calculations. Atomic c) Cs Se 4. Complete the table. Chemical Symbol Cl Ca Xe Na F mass = 126.9038 x 57.4 + 42.6*122.9042 /100 121.756 amu Group # 7A(17) Part B: Electron Configuration/lons (1) Write the electron configuration for each of the following: (a) Magnesium_ (b) Chlorine_ [Ne]35 [Ne] 353p [Ar] 45' 1525 2p5 (c) Potassium (d) Fluorine 2A 8A TA toses Ar) [XE] () Group Name halogen Alkaline earth Thert gas Alkali Metal (2) Determine the number of protons and electrons in each ion and write the electron dot symbol. (a) A1+ (Ne] I (b) s- (3) Predict how many electrons each element will most likely gain or lose. MOVE (a) I b) Ba M gain joses Meta