Week Five Lecture Notes
Week Five Lecture Notes Chem 105
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Popular in Chemistry
This 3 page Class Notes was uploaded by Marisa Loken on Monday October 19, 2015. The Class Notes belongs to Chem 105 at University of Wisconsin - Stevens Point taught by Dr. Riha in Fall 2015. Since its upload, it has received 19 views. For similar materials see Fundamental Chemistry in Chemistry at University of Wisconsin - Stevens Point.
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Date Created: 10/19/15
Week Five Notes September 28Wednesday September 30 Pauli Exclusion Only 2 electron per orbital o S 1 orientation 1 orbital 2e only 0 P 3 orientations 3 orbitals 6e only 0 D 5 o F 7 Aufbom ll e starting with lowest energy and working up in energy Hund39s rue Spread out the electrons in degenerate orbita to maximize spin Condensed electron con gurations Use previous noble gas and then ll remaining eecton orbitals that follow Ions Charged particles different numbers of electrons and protons Ca on More protons than electrons 0 Positive charge Anion More electrons than protons Neutral 0 2 core electrons 6 electron valence electrons Neutral S 6 valence electrons Neutral Mg 2 valence electrons Neutral Ca 2 valence electrons Periodic Groups 1A alkali metals 2A alkaline earth metals 6A haocegns 7A Halides 8A nobe gasses 0 Completely ed outer shell Effective nuclear charge Net positive charge felt by an electron Down periodic table Zeff increases 0 Electron is further from nucleus in outermost shell Zeff increases across the row of period of periodic table Core electrons remain the same 0 Number of protons increase which increases nucleus charge 0 Number of electrons increase which increases charge of valence shell Bonding atomic radii Down periodic table atomic radii increases 0 Electrons spread out Across periodic table atomic radii decreases o Stronger action between the nucleus and electrons Wednesday Cations have greater number of protons than electrons Anions have less protons than electrons Canns Remove electrons from outer shell when electrons ll into d orbitals the energy of the d orbital drops below the orbital remove electrons from the orbital with the highest n value than the highest I value Anions Add electrons to the outer shell 0 Atomic radii increase Canns Take electrons out of the outer shell 0 Gets smaller in radius Ionization energy Minimum energy to remove an electron from an atom in ground state as Zeff increases ionization energy also increases ionization energy increases across periodic table and decreases down a group For np less energy is needed to remove that electron drops overall energy of the atom From no decrease in ionization energy Atoms prefer empty half lled or full orbital shells 2nCI ionization energies are larger than the rst ionization energy