1.2 atomic orbitals, electronic configurations & the periodic table Flashcards
orbitals
stationary waves in an atom, vibrate in time
can hold a maximum of 2 electrons
spdf
principle quantum number
n
indicates an electron’s energy level
angular momentum quantum number
l
indicates the shape of the subshell
values from 0 to n-1
magnetic quantum number
Ml
indicates the orientation of the orbital
values between -l and +l
magnetic spin quantum number
Ms
indicates the direction of spin
values of either -1/2 or +1/2
s subshell
l = 0
holds 2 electrons maximum
1 value of Ml
spherical
p subshell
l = 1
holds 6 electrons maximum
3 values for Ml
dumbbell shaped
d subshell
l = 2
holds 10 electrons maximum
5 values for Ml
f subshell
l = 3
holds 14 electrons maximum
7 values for Ml
degenerate
orbitals of the same subshell have equal energy
pauli exclusion principle
no 2 electrons of the same atom can have the same set of 4 quantum numbers
what does the pauli exclusion principle mean?
orbitals hold a maximum of 2 electrons
each electron within an orbital must have opposite spins
aufbau principle
electrons fill orbitals in order of increasing energy
hund’s rule
when degenerate orbitals are available, electrons fill each singly, keeping their spins parallel before spin pairing starts
subshell stability
half-filled and fully-filled subshells are more stable than other incomplete subshells
vsepr theory step 1
take the number of valence electrons on the central atom
vsepr theory 2
add an electron for each attached atom
vsepr theory 3
add electrons for negative charges
subtract electrons for positive charges
vsepr theory 4
divide by 2 for the number of electron pairs
electron pair repulsion
negatively charged pairs repel each other so arrange to minimise repulsion and maximise separation
highest electron pair repulsion
lone pair-lone pair
lowest electron pair repulsion
bonding pair-bonding pair
dative covalent bonds
form when both electrons in a covalent bond are from the same atom
linear shaped molecules
2 bonding electron pairs
180° bond angle
trigonal planar shaped molecules
3 bonding electron pairs
120° bond angle
tetrahedral shaped molecules
4 bonding electron pairs
109.5° bond angle
angular shaped molecules
2 bonding electron pairs
2 lone electron pairs
104.5° bond angle
trigonal pyramidal shaped molecules
3 bonding electron pairs
1 lone electron pair
107° bond angle
trigonal bipyramidal shaped molecules
5 bonding electron pairs
· 120° equatorial bond angle
· 90° eq/ax bond angle
· 180° axial bond angle
octahedral shaped molecules
6 bonding electron pairs
90° bond angle
square pyramidal shaped molecules
5 bonding electron pairs
1 lone electron pair
82° bond angle
square planar shaped molecules
4 bonding electron pairs
2 lone electron pairs
90° bond angle