Rohan Kubba Dis 4B wrote:Why is it that when we are dealing with energy levels, as the energy levels increase, they get closer together? Does this also affect our calculations with the Bohr frequency condition or the E=-hR/n^2 formula in any way?
As of now, the Rydberg formula (E=-hR/n^2), and the concepts of Balmer and Lyman Series applies ONLY to atomic hydrogen.
And typically, the trend across the periodic table is that the atomic radius of atoms decreases from left to right. This is due to an increase in attraction forces (coulombic attraction) coming from the nucleus. As for your question, you seem to have the trend backwards...as energy levels increase down the periodic table, atomic radius tends to increase, so electrons (that is what I am assuming "they" means) are pushed further away from the nuclease due to an increase in electron shielding. Hope that helps!