All terms in this list:
Planck's constant: h = 6.626 x 10^-34 J-s
Speed of light: c = 2.998 × 10^8 m/s
Engery of a single quantum: E = hc/λ or E = hν
Frequency of wavelengths: ν = c/λ
Rydberg constant: R(∞) = I/hc = 1.10 x 10^7 m^-1
Ionization potential of H atom: I = 13.59 eV
Momentum: p=mv
De Broglie wavelength: λ=h/p The same formula gives the momentum of a photon or wavelength λ.
Heisenberg's principle: Δx * Δp GREATER THAN OR EQUAL TO h/4π Also known as uncertainty principle
Electron energy given orbit: E = (-hcR(∞)) x (1/n^2), where -hcR(∞) = -2.18 x 10^-18 and n = principle quantum number
ground state of atom: the lowest energy state (n = 1)
excited state of atom: any energy state higher than the ground state (n = 2, 3, ....)
Bohr equation: ΔE = hc/λ = -13.59 eV * ([1/n(f)^2] - [1/n(i)^2]); 2nd eqn. used to determine the transitions between the energy levels of the hydrogen atom as defined by their principle quantum numbers n(f) and n(i)
principle quantum number: designates the main energy level (shell); describes electron cloud size; n = 1, 2, 3, ....
azimuthal quantum number: designates the sub-level where the electrons can be found; determines shape of the orbital and angular momentum; coincides with s, p, d, f (s=0, p=1, d=2, f=3); ℓ = 0 LESS THAN ℓ LESS THAN n-1
magnetic quantum number: determines the projection of angular momentum; describes the orientation that the subshell takes; m( ℓ ) = -ℓ LESS THAN m( ℓ ) LESS THAN ℓ
spin projection quantum number: designates the spin of the electron; describes electron behavior, not the location; m(s) = -1/2 (counter-clockwise) or 1/2 (clockwise)
Angstrom: A very small unit of length, 10^-10 m, approximately the size of an atom, Å
distance: d = speed x time
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