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Analysis:- Look at the data carefully. Is any data left out? Based on the electron configuration, explain why this data was not included. Examine the graph carefully and describe the general trends in atomic radius. Describe the general trends in ionization energy. How easy is it to see trends and the “Atomic Radius” graph? Why is it so compressed to the IE line. List possible solutions for providing more detail in the atomic radius line. We want to be able to compare IE and atomic radii, would it be possible to do this if they were in on different graphs? What might be some of the challenges of comparing them on different graphs? 1) 2) According to the graph for the atomic radiuses of elements, the atomic radius decreases as we go from left to right of the period. This is because as we go across a period the number of electrons in the outer shell increases. Therefore, there is more attraction between the nucleus and the shells. Then a sudden rise of atomic radius is observed as we go down a group. This is because a new shell is added every group. Thus increasing the shielding effect. 3) From the graph we can infer that the ionization energy of the first two element, Hydrogen and Helium. There is a general trend of the ionization energy to increase as we go across the period and to decrease as we go down the group. “The ionization energy or ionization potential is the energy necessary to remove an electron from the neutral atom. It is a minimum for the alkali metals which have a single electron outside a closed shell. It generally increases across a row on the periodic maximum for the noble gases which have closed shells. For example, sodium requires only 496 kJ/mol or 5.14 eV/atom to ionize it while neon, the noble gas immediately preceding it in the periodic table, requires 2081 kJ/mol or 21.56 eV/atom. The ionization energy is one of the primary energy considerations used in quantifying chemical bonds.”...
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