Use Slater's rules to calculate Zeff for the outermost electron of F (2p)

Explain why it is more difficult to ionize a fluorine atom than a boron atom.

"Write the ground state electron configuration (complete, no abbreviations or noble gas cores) of an atom ofKEnter the entire electron configuration with 1 space between each sublevel and no superscripts like this 1s2 2s2 2p6 . .

Briefly describe the Bohr atom. A drawing might be appropriate. Give its properties and assumptions. What physical/chemical phenomena and/or problems did it seek to explain or eliminate? What inadequacies does it have? 1.

Write equations corresponding to the first through fourth ionization energies for Mg. Between which two will the largest jump in ionization energy occur?

Specify all quantum numbers for the electrons in the 3p state in Zr. Do the same for the 4p state in Ba.

Use Slater's rule to calculate Zeff for the outermost electron of Si+

Which is higher in energy, the 2s or 2p orbitl, in hydrogen? Is this also true for helium? Explain.

Give the set of quantum numbers for Nitrogen (N).

22. Using the Bohr model, determine the energy of an electron with n = 6 in a hydrogen atom.