Chem final- Exam 2 Flashcards
diamagnetic
-Only paired electrons
-Slightly repelled
paramagnetic
-Unpaired electrons
-Attracted
Isoelectronic
-Atoms that have the same number of electrons
-Diff protons
Ions electronic configuration
-S electrons removed first
Effective nuclear charge
-Actual nuclear charge experienced by an electron
-Charge of nucleus + charge of shielding electrons
Shielding
-Electrons in lower energy orbitals screen it from full effects of nuclear charge
Penetrance
-Electron in an orbital might penetrate to get closer to the nucleus
Atomic radius trend
-Bottom left: Biggest
-Top right: Smallest
Ionization energy trend
-Bottom left: Lowest
-Top right: Highest
Ionization energy
-Energy required to remove an electron from an atom in gas state (+ values)
Lattice energy
-Energy of forming a lattice
-Higher charges = Higher lattice energy
-Bigger distance = Lower lattice energy
-Smaller ions can get closer together
-negative = good (all top)
Higher effective nuclear charge (IA)
Higher Ionization energy
Electron affinity
-Energy change that occurs when an electron is added to an atom in gas state (- values)
Electron affinity trend
-Becomes more negative as you go from left to right
Higher effective electron affinity (EA)
More negative electron affinity