Question | Answer |
Aufbau procedure | "building up"; adding electrons to one subshell until it's full before moving to the next subshell |
Pauli Exclusion Principle | a max of 2 electrons per orbital as long as they have opposite spin; no two electrons in an atom can have the same four quantum numbers |
Hund's Rule | parallel before paired; when filling degenerate orbitals, electrons occupy them singly (one at a time) with parallel spin before pairing up |
ground state | the lowest energy state |
excited state | not the lowest energy state |
degenerate | equal in energy |
node | a region in space where there is zero probability of finding an electron |
shell | n (1, 2, 3, ...) |
subshell | n & l (1s, 2s, 2p, ...) |
Where is the "s" block found? | the left side |
Where is the "p" block found? | the right side |
Where is the "d" block found? | the middle |
Where is the "f" block found? | the bottom |
The s block starts with what? | 1s |
The p block starts with what? | 2p |
The d block starts with what? | 3d |
The f block starts with what? | 4f |
Special electron configurations occur when what are involved? | 1. filled outermost subshells
2. half-filled subshells |
Which electrons are removed in cations? | the electrons from the outermost shell (which is not necessarily the outermost subshell) |
isoelectronic | having the same electron configuration |
paramagnetic | attracted into a magnetic field; having unpaired electrons |
diamagnetic | slightly repelled by a magnetic field; having all electrons paired |
valence electrons | outer shell electrons |
core electrons | inner shell electrons |
For abbreviated electron configurations... | Put the proceeding noble gas symbol in brackets before writing the valence electrons |
shielding | the ability of other electrons, especially inner core electrons, to decrease the nuclear attraction for an outer electron |
effective nuclear charge | the nuclear charge that an electron experiences |
atomic size trend | increases toward the lower left and decreases toward the upper right |
ionization energy trend | increases toward the upper right and decreases toward the lower left |
What is the relationship in size between a cation and its parent atom? | smaller than their parent atom |
What is the relationship in size between an anion and its parent atom? | larger than their parent atom |
In an isoelectronic series, what is the trend in size? | size decreases with increasing nuclear charge |
ionization energy | the energy required to remove an electron from a gaseous atom or ion |
What are the exceptions in ionization energy? | 1. between column 2 and 13 because it is easier to remove the higher energy p electron than the lower energy s electron.
2. between column 15 and 16 because column 15 has a half-filled subshell |
When does a "huge jump" occur in ionization energies? | when an inner core electron is removed |
electron affinity | the energy change (delta E) the occurs when an electron is added to a gaseous atom; some negative and some positive |
The more electronegative the element, | the more the atom "wants" the electron |
What groups have positive or near-positive electron affinities? | Groups 2 and 18 |
What group has the most negative/most exothermic electron affinities? | Group 17 (halogens) |
What do you use to make individual predictions? | electron configuration and nuclear charge |