Inorganic Chemistry - 1)b) Atomic orbitals, electronic configurations and the periodic table Flashcards
(22 cards)
what is principal quantum number?
(n) indicates the electrons main energy level
what is angular momentum quantum number?
(l) determines the shape of the subshell and has values 0 to n-1
what is magnetic quantum number?
(ml) determines the orientation in space of the electron, values between -l and +l
what is spin magnetic quantum number?
(ms) indicates the direction in which the electron is spinning, 1/2 or -1/2
Pauli Exclusion principle:
no two electrons in the same atom can have the same set of four quantum numbers
Aufbau principle
electrons fill subshells in order of increasing energy
Hund’s Rule
electrons fill degenerate orbitals singly with parallel spins before pairing up to fill the orbitals
what term is used to describe electrons in their lowest possible energy levels?
ground state
what term is used to describe particles which have the same electronic configurations?
isoelectronic
why does electron-electron repulsion lower the ionisation energy?
it lowers the attraction between the fourth electron and the nucleus, so despite the increased nuclear charge, the electron is easier to remove and less energy is required to remove the electron
dative covalent bond:
when one atom provides both the electrons that form the bond
state an example of a molecule/ion that contains a dative covalent bond:
ammonium
what is the shape and bond angle acquired by two filled orbitals, both bonding pairs?
linear
180°
what is the shape and bond angle acquired by three filled orbitals, all bonding pairs?
trigonal planar
120°
what is the shape and bond angle acquired by four filled orbitals all bonding pairs?
tetrahedral
109.5°
what is the shape and bond angle acquired by five filled orbitals all bonding pairs?
trigonal bipyramidal
120° and 90°
what is the shape and bond angle acquired by six filled orbitals all bonding pairs?
octahedral
90°
what is the shape and bond angle acquired by three filled orbitals, two bonding and one lone pair?
angular
120°
what is the shape and bond angle acquired by four filled orbitals, three bonding and one lone pair?
trigonal pyramidal
107.5°
what is the shape and bond angle acquired by four filled orbitals, two bonding and two lone pairs?
angular
104.5°
what is the shape and bond angle acquired by five filled orbitals, three bonding and two lone pairs?
T-shaped
86°
what shape and bond angle is acquired by six filled orbitals, 4 bonding and 2 lone pairs?
square planar
90°
