Bohr Model l , n l x n Light hn Matter A.P. CHEM. CH. 7 ATOMIC STRUCTURE Background Info Duality Particle Wave-Mechanical Model Bohr Model Wave mass l , n It explained Duality of matter U.V. catastrophe/ photelelectric effect Atom doesn’t collapse DeBroglie Planck / Einstein Young Double Slit Dalton Bright-Line Spectra DeBroglie Equations H Wave ** Equation l x n = c Named: Quantum model Schroedinger Light hn Matter P E= Characteristics E E= mc2 m = h/cl Discrete energy levels l = h/mv Uncert. Princ. Electron transitions Heisenberg USE SPECIAL PENS OR PENCILS IN THE BINS TO FILL IN OVERVIEW! Equation: En=-2.178x10-18J(Z2/n2) Observer affects the observed Flaw: Bohr didn’t know why Dx • Dmv ≥ h/4p

H Y E Y I.E.= Zeff Zact - repulsive effects Z2eff penetration s aufbau position High prob. region in space where the electron is likely to be found. Wave function ** H Y E Y = Defined: orbital Can be applied to atoms other than hydrogen by finding: Zeff Zact - repulsive effects = Repulsions/ core shielding Can be found by knowing I.E. equation Z2eff I.E.= 1310 kJ mole e- n2 Config. Not. Orbital. Not. evidence Not as low as could be in certain instances due to: PHOTOELECTRON SPRECTOSCOPY Hydrogen like orbitals penetration Representations s Rules for multielectronic atoms: I.E. aufbau Relate to Chart E.A. Know the trends of this p Pauli size d Hund’s f

This is the photoelectron spectrum for _______________________ phosphorous 1000 5000 100 1000 100 (eV) The peak on the spectrum to which the arrow is pointing would be associated with electrons in which sublevel? A.) 1s B.) 2s C.) 3s D.) 3p

A.) shift more to the right than in phosphorous. This is the photoelectron spectrum for _______________________ phosphorous 1000 5000 100 1000 100 (eV) If the photoelectron spectrum for sulfur was shown above, the peak for the 1s orbital would A.) shift more to the right than in phosphorous. B.) shift more to the left than in phosphorous. C.) not shift compared to phosphorous. D.) not be able to be compared to phosphorous. Due to more protons in the nucleus…no change in core shielding or repulsions!

A.) shift more to the right than in phosphorous. This is the photoelectron spectrum for _______________________ phosphorous 1000 5000 100 1000 100 (eV) If the photoelectron spectrum for sulfur was shown above, the peak for the 3p orbital would A.) shift more to the right than in phosphorous. B.) shift more to the left than in phosphorous. C.) not shift compared to phosphorous. D.) not be able to be compared to phosphorous. Due to significant repulsion when an electron is added to an orbital in a set of degenerate orbitals that had previously had only one!

…nearly violet 1s22s2 1757.1 kJ/mol 14848.7 kJ/mol 4 Practice Problem: Chapter 7 A.P. Chemistry Let’s look at the atom beryllium. Write out the ground state configuration notation for Be: _____________________ Record the second and third ionization energies for Be: I.E.2= ________________ I.E.3= ________________ Predict a value for I.E.1 = _________________ (the actual value = _____________) Zeff ( ) = _______________ One of the emission spectral lines for Be3+ [that’s nearly a color we can see] results from an electronic transition from n=5 to n=4. Is the transition’s associated “color” nearly red or nearly violet? 1s22s2 1757.1 kJ/mol 14848.7 kJ/mol <1757.1 kJ/mol 899.5 kJ/mol 4 For the remaining electron E4 = (-2.178x10-18 J)(42/42) = -2.178x10-18 J Find the difference E5 = (-2.178x10-18 J)(42/52)= -1.394x10-18 J E (released) =7.84x10-19 J - 7.84x10-19 J E =h n n = 1.18x1015/s …nearly violet c/n = l l = 2.54x10-7 m