Chapter 1: Atomic Structure Flashcards
Principle Quantum Number
n
Describes the average energy and the shell, shape.
Higher n= higher energy level= greater radius.
Azimuthal Quantum Number
l
describes the subshells within a given principle energy level (s,p,d, and f).
Magnetic Quantum Number
ml
specifies the orbital within a subshell where an electron can be located
Spin Quantum Number
ms
Designates the spin orientation (+-1/2) of an electron orbital.
l=0 subshell
s
l=1 subshell
p
l=2 subshell
d
l=3 subshell
f
Maximum number of electrons in orbital
2 electrons
Maximum number of electrons in subshell
4l+2
How many orbitals in s?
1 orbital
How many orbitals in p?
3 orbitals
How many orbitals in d?
5 orbitals
How many orbitals in f?
7 orbitals
Quantum
The energy difference between energy levels
Ground State
the lowest energy state, the energy of the ground state is known as the zero-point energy of the system, the state in which all e-s are in lowest possible orbitals
Excited State
A state in which at least one e- has moved to a subshell of higher than normal energy
As electrons go from a lower energy level to a higher energy level, they…
…get AHED:
Absorb Light
Higher potential
Excited
Distant (from the nucleus)
Lyman Series
the group of hydrogen emission lines corresponding to transition from energy levels n>2 to n=1
Balmer Series
the group corresponding to transition from energy levels n>3 to n=2 and includes four wavelengths in the visible region (the shorter photon wavelengths in the UV region).
Paschen Series
corresponds to transition from n>4 to n=3.
Orbitals
The localized regions of space that electrons are likely to be found in.
Heisenberg uncertainty principle
It is impossible to simultaneously know both the location and momentum of an electron.
Pauli exclusion principle
no two electrons in a given atom can posses the same set of four quantum numbers.
Aufbau principle
aka building-up principle.
Electrons fill from lower to higher energy subshells and each subshell will completely fill before electrons enter the next one.
Hund’s rule
subshells with multiple orbitals fill electrons so there is a maximum number of 1/2 filled orbitals first because of electron repulsion
Exceptions to electron configuration?
Chromium (Z=24)
Copper (Z=29)
Chromium should have EC: [Ar]4s2 3d4
Instead has = [Ar]4s1 3d5
Copper should have EC: [Ar] 4s2 3d9
Instead has: [Ar] 4s1 3d10
stability of full d or f shell outweighs the energetically unfavorable cost of removing an electron from an s orbital. Doesn’t work for p subshell.
Paramagnetic materials
Materials that have unpaired electrons that align with the magnetic field, attracting the material to the magnet.
Diamagnetic
Materials that have all paired electrons, which can not be easily realigned; they are repelled by magnets.
