Key Equations

energy of hydrogen electron in an orbital	$E_{n} = - \frac{13.6 eV}{n^{2}} (n = 1, 2, 3, ...)$
energy of any hydrogen-like electron in orbital	$E_{n} = \frac{Z^{2}}{n^{2}} E_{o} (n = 1, 2, 3, ...)$
wavelength of light emitted by an electron changing states	$\frac{1}{λ} = R (\frac{1}{n_{f}^{2}} - \frac{1}{n_{i}^{2}})$
wavelength of an orbital	$n λ_{n} = 2 π r_{n} (n = 1, 2, 3, ...)$
heisenberg’s uncertainty principle	$Δ x Δ p \geq \frac{h}{4 π}$

radioactive half-life

N = N_{O} e^{- λ t}

energy–mass conversion	$E = m c^{2}$
proton-proton chain	$2 e− + 4^{1} H \to 4 He + 2 v_{e} + 6 γ$

roentgen equivalent man

rem = rad \times RBE

Resources