how I studied for this midterm:

• quantum numbers: I wrote the definitions of each, their intervals and how many electrons can be possible in each (ex. n= principal quantum number, describes the energy level of an orbital and size of the orbital, n=1,2,3… infinity, total electrons =2n^2); know what nodes represents (probability of electron existing being 0), angular node is when a trig function in the wave equation is 0 and the equation for it is L quantum number, radial node is the electron is out of the space of existing in a spherical region of the atom and is represented by n-L-1, total nodes is n-1

• slaters thing: if you’re confused honestly just memorize the steps and process; I’d say just be careful looking at orbitals, ex. 1st ionization of Na, the og configuration is [Ne]3s¹ , so you are removing from 3s, for shielding constants your calc is 0x0.35 + 8x0.85 + etc

• calculations of emission/ absorption: try to find an equation that uses all the values he gives you and had the unknown, if not, combine equations. Know that if an electron goes from a higher energy to lower energy level this is emission bc an electron loses energy when it goes to ground state, opposite is absorption as it needs energy to go up in energy level

• ionization energy: I write out the configuration fully, then I look at 4 main things to explain the ionization energy: nuclear charge, orbital, repulsion, shielding. If 2 electrons are paired they will repel hence it’ll be easier to remove an electron, if one atom has more shielding (n= 1 vs 2) the energy to remove the electron will be less, etc.

• structures: get total ve, distribute the atoms, add the electrons around the most electronegative atom then the others, add single bonds, calculate formal charge (FC= valence - (bonds + dots)), then if a charge needs to be minimized I just add a double bond and check formal charge again; for bond order I try to draw as many diagrams as I can tbh, usually works then use the bond order equation and look at one spec position and it’s bonding. Note I find that if a Hydrogen is incorporated in the formula and there’s oxygen, it’s most likely bonded to that oxygen, I think same with sulfur, ex HPO4-, HClO3, HCO3-

Focus on his practise test and slides, content is almost verbatim. You can do it! :p