KA 2: atomic orbitals, electronic configuration and the periodic table Flashcards
what are standing (stationary) waves?
waves that vibrate in time but do not move
what is an orbital?
different sizes and shapes of standing waves possible around the nucleus
What is the max. number of electrons that an orbital can hold
2
Name the four different shapes of orbitals
s,p,d,f
What is “quanta”?
the fixed amount of energy that electrons within an atom have
what can electrons be defined in terms of?
quantum number
For Principal Quantum Number:
-Name the symbol
-Say what values it can have
-What does it do
-What is it related to
-n
-can have values n=1,2,3,4…
-indicates main energy level for an electron
-is related to the size of the orbital
The higher the value of……
n, then the further the electrons are from the nucleus
For Angular Momentum Quantum Number:
-Name the symbol
-What does this determine
-What values can it have
-l
-can have values l=0,1,2,3 (up to n-1)
-it determines the shape of the subshell
For Magnetic Quantum Number:
-Name the symbol
-what values can it take
-what does it determine
-ml
-ml can take values of whole numbers (and zero) between -1 and +1
-determines the orientation of the orbital
How is the second shell organised?
one “s” orbital and three “p” orbitals
Three p orbitals are aligned along perpendicular axes.
For Spin Magnetic Quantum Number:
-what does it determine
-name the symbol
-what values can they take
-the direction of spin
-ms
-takes the values of -1/2 or +1/2
when an orbital contains two electrons they must…
be paired with spins opposed
In s orbitals:
-what is the value of l
-describe the trend
-l=0
-increasing size and energy as n increases
In p orbitals:
-what is the value of l
-what is it’s shape
-how many orbitals
-explain the trend
-l=1
-dumbbell shaped
-3 orbitals corresponding to ml= -1,0,1. These 3 orbitals have the same energy (degenerate)
-Energy and size increases with n(2p<3p<4p)
In d orbitals:
-what is the value of l
-what is it’s shape
-how many orbitals
-explain the trend
-l=2
-more complex dumbbell shapes
-5 orbitals (ml= -2,-1,0,1,2)(degenerate)
-energy and size increases with n (3d<4d)
describe the organisation of the third shell
max. 18 electrons
-2 in the s orbital
-6 in the 3 p orbitals
-10 remaining in the d orbitals (5 d orbitals)
What does degenerate mean?
orbitals that have the same energy
what is the periodic table subdivided into and what does that correspond to?
-s,p,d,f
-corresponds to the outer electronic configurations of these elements
what does each box in box notation represent?
an atomic orbital
what does box notation represent?
The relative energies corresponding to each orbital can be represented diagrammatically using orbital box notation for the first four shells of a multi-electron atom.
What is the order of filling?
1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s, 5f, 6d, 7p
what does each thing correspond to in spectroscopic notation?
leading numbers=> the n numbers i.e. the shell
letters=> the sub-shell (l numbers)
subscript=> the total number of electrons within that sub-shell
Name the three principles/rules
-The Aufbau Principle
-Hund’s rule
-The Pauli Exclusion Principle
