Question | Answer |
Electromagnetic spectrum | -series of waves including visible and invisible light
-visible: ROYGBIV
-invisible: everything else |
Wavelength | -lambda
-distance between two crests
-measured in nm, m, cm |
Frequency | -v
-number of waves
-1/s, s to the neg. 1st, Hz |
Speed of light | -3.00 x 10 to the 8th m/s |
Finding speed of light (equation) | c=λv |
Finding wavelength (equation) | λ=c/v |
Finding frequency (equation) | v=c/λ |
Finding energy (equation) | E=h*v (h=Planck's constant) (v=frequency) |
Planck's Constant | 6.6262 x 10 to the -34 J/S |
What did Max Planck propose? | -proposed that light was emitted is "packets" of energy called quanta |
What is excited state? | -when an electron gains energy |
What is the Heisenberg Uncertainty Principle? | -declares that it is impossible to know the velocity and position of a particle at the same time |
Who proposed the Quantum Mechanical Model and what did it conclude? | -Schrodinger and Heisenberg
-concluded that electrons are not found in orbits, but rather in atomic orbitals |
What is a quantum? | -the amount of energy needed to move an electron away from the nucleus |
What are quantum numbers? | -regions in space where electrons are found |
Sublevels | S, P, D, F |
S | -spherical
-1 orbital
-maximum # of electrons: 2 |
P | -dumbbell
-3 orbitals
-maximum # of electrons: 6 |
D | -clover
-5 orbitals
-maximum # of electrons: 10 |
F | -forget about it
-7 orbitals
-maximum # of electrons: 14 |
Aufbau Principle | -electrons enter orbitals at the lowest energy level first |
Pauli Exclusion Principle | -no more than 2 electrons can occupy an orbital
-electrons in the same orbital must have opposite spins |
Hund's Rule | -when electrons occupy orbitals of equal energy, one electron enters each orbital until all the orbitals contain one electron with parallel spins |
Exceptional configurations | -only applies to elements that end in d4 and d9
-exception: a half-full d sublevel is more stable than a partially-filled d sublevel
-(ex) elements go from: 4s2 3d4 to 4s1 3d5 |