Atomic Structure Flashcards
Pauli’s Exclusion Principle
no two electrons in the same atom can have identical values for all four of their quantum numbers
Wave function
e value of the wave function of a particle at a given point of space and time is related to the likelihood of the particle’s being there at the time.
Hund’s rule
every orbital in a subshell is singly occupied with one electron before any one orbital is doubly occupied, and all electrons in singly occupied orbitals have the same spin
Additional electrons in inner orbitals
Inner electrons shield outer electrons more effectively than do electrons in the same sublevel.
Sizes of Atoms
The greater Zeff , the greater the attractive force between
the nucleus and its electrons and the smaller the average
distance between the nucleus and its valence electrons
(the atomic radius)
Changes in Zeff.
As the effective nuclear charge (Zeff)—the positive charge “felt” by an electron—increases, outer electrons are pulled closer to the nucleus; thus, the atoms are smaller.
Changes in n
As the principal quantum number (n) increases, the
probability that the outer electrons will spend more time farther from the nucleus increases as well; thus, the atoms are larger.
Zeff in terms of Ionisation energy
As Zeff increases, it requires more energy to remove the
outermost electron. Consequently, ionization energy is related to atomic radius, with ionization energy increasing as atomic radius decreases