1. Atomic structure Flashcards
Principal vs azithumal/angular momentum vs magnetic vs spin quantum number
Energy level/shell, n, max # of e- w/in a shell: 2n^2 vs subshell, l, max # of e- w/in a subshell: 4l + 2, ranges from 0 to n-1 (ie. In the first shell, you have one subshell which is l=0; in the second shell, you have two subshells which are l=0 and l=1; etc); energy of subshells inc with increasing l values (ex: 3d has more energy than 4s, but lower than 4p) vs # of orbitals, ranges b/w l and -l including 0 vs spin and momentum, either +1/2 or -1/2
Balmer series vs Lyman series vs Paschen series in atomic emission spectrum of hydrogen from Bohr model
H+ emission lines transitioning from n>2 to n=2 vs n>1 to n=1 vs n>/=4 to n=3
Heisenberg uncertainty principle
Can’t find e-‘s momentum and position simultaneously; if one of them has more certainty, then the other has more uncertainty
How to find energy of e- going b/w energy levels
E = -RH(1/n^2 initial minus 1/n^2 final)
-RH (Rydberg unit of energy aka energy of e-) is a constant: 2.18E-18 J/e-
Energy of e- b/w energy levels corresponds to EXACT energy of a photon —> can use Planck’s eqn
Avogadro’s number
6.02E23
Planck’s eqn and constant
Describes energy of a quantum
E = hf
h = 6.626E-34 J*s
Ground state vs excited state
State of lowest energy (usually closest to nucleus) vs state of higher than nml energy (usually farther from nucleus)
As e- move from lower to higher energy levels, they get AHED: absorbs energy, higher potential, excited, distant from nucleus
How to find electromagnetic energy of photons
E = hc/lambda
Pauli exclusion principle vs Aufbau principle/building up principle
No 2 e- can have same set of 4 quantum numbers (ie. Only max of 2 e- in each orbital and the 2 e- in the orbitals must have opposite spins) vs e- full from lower to higher energy subshells
Paramagnetic vs diamagnetic vs ferromagnetic
Magnetic field will cause parallel spins in unpaired e- —> weak attraction (ex: gold, aluminum, copper) vs material that only has paired e- and has no net magnetic field —> repelled by magnetic field (ex: wood, plastic, glass) vs have unpaired e- and magnetic dipoles oriented randomly —> no net magnetic dipole, BUT is still strongly attracted to a magnetic field (ex: iron, nickel and cobalt)
Spectroscopic notation
It’s electron config; s represents l=0 subshell, p represents l=1 subshell, d represents l=2 subshell, and f represents l=3 subshell
Mass number vs atomic number symbols
A vs Z
n + l rule
The lower the sum of n+l —> the lower the energy of subshell (ie. the closer the e- is to the nucleus). If 2 subshells have same n+l value —> the lower n value has lower energy. This rule determines which e-or subshell = closer to nucleus
Electron config for cations
When you move back an element —> you remove a subshell with highest n value first (ex: nml e- config for Mn is [Ar]4s^23d^5, for Mn+ is [Ar]4s^13d^5)
Bohr model vs Quantum mechanical model
e- = in fixed orbit outside of nucleus vs e- in orbitals or clouds outside of nucleus
