Atomic Orbitals, Electronic Configurations and the Periodic Table Flashcards
Unit 1
what are regions of high probability of finding a electron called?
Atomic Orbitals
what are the four orbital shapes?
s,p,d,f
why is the s orbital in the first shell smaller than that of the s orbital in the second shell?
their diameter increases as the shell number increases
how many electrons can each s orbital hold?
can only hold two electrons of opposite spins
what term can be used to describe p orbitals?
degenerate
what does the term degenerate mean?
orbitals of equal energy
principal quantum number (n):
this number indicates the electrons main energy level
angular momentum quantum number (l):
determines the shape of the orbital
(n-1)
magnetic quantum number (ml):
determines the orientation of the orbital
values between -l and +l
spin magnetic quantum number (ms):
indicates the direction in which the electron is spinning.
Either clockwise or anti-clockwise (-1/2, +1/2)
Pauli Exclusion Principle:
“no two electrons in the same atom can have the same four quantum numbers, so no orbital can contain more than two electrons, and the two electrons must have opposite spins”
think can’t live at same address, Pauli/Paula
Aufbau Principle:
“electrons fill the subshells in order of increasing energy”
Hund’s Rule:
“when the degenerate orbitals are available, electrons fill each degenerate orbital singly and with parallel spins, before pairing to fill the orbitals”
what is the rule with the electronic configuration of atoms to ions?
atoms form ions which have the electronic configuration of the nearest noble gas
what is meant by the term isoelectronic?
particles which have the same electronic configuration
what is meant by the ground state?
when the electrons are in their lowest possible energy level
how are covalent bonds formed?
when two atomic orbitals combine to form a molecular orbital
how do atomic orbitals combine to forma molecular orbital?
usually, both orbitals are half-filled and overlap to form a molecular orbital
when is a dative covalent bond formed?
when one atom provides both the electrons that form the bond
what formula can be used to calculate the number of electron pairs?
electrons of central atom+atoms attached/2
what is the shape/bond angle of a molecule with two bonding pairs?
linear shape
180°
what is the shape/bond angle of a molecule with three bonding pairs?
trigonal planar shape
120°
what is the shape/bond angle of a molecule with four bonding pairs?
tetrahedral
109.5°
what is the shape/bond angles of a molecule with five bonding pairs?
trigonal bipyramidal
120° and 90°
