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37 Cards in this Set
- Front
- Back
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Problems with Bohr's Theory
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1. why are electrons not in the nucleus?
2. How can electrons quantum leap to different energy levels when they cant be between energy levels? 3. math only applies to hydrogen (equation gets changed to --> E=-kz((1/n1^2)-(1/n2^2)) |
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Constructive interference
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trough meets trough and crest meets crest
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Destructive interference
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trough meets crest
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Einstein
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- says that light is corpuscular (little pieces)
- light has momentum - red has less momentum - blue has more momentum - p=mv --> p=momentum -means the mass that blue light doesnt have is larger than the mass that red light doesnt have |
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Photoelectric Effect
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- light is energy
- blue light is seen while red light is not - seems okay because blue light must have more energy than red light |
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de Broglie
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- λ=h/mv
- h = Plancks constant (6.6262e-34) - m = kg - v = m/s - λ = wavelength - Dual nature of matter/light --> if you have momentum you can calculate wavelengths - light acts light particles - particles act light wavelengths - therefore light acts like wavelengths |
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Superposition
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something behaving as more than one thing at the same time
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Heisenberg
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- uncertainty principle
- making a measurement affects what your measuring - (Δx)(Δp) ≥ h - Δ = uncertainty in - p = momentum - h = plancks constant/2π - if you slow momentum down enough your Δx will get larger. |
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What we learned from Einstein, de Broglie, and Heisenberg
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- electrons can behave as waves
- can't know where something is and how it behaves |
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Schrodinger's Wave Equation
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- E(ψ) = H(ψ) --> E depends on ψ and H depends on ψ like f(x)
- E = energy - H = the hamiltonia - ψ = psi = wave function |
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Standing Waves
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don't more or transport energy
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Nodes
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- point between troughs and crests
- wavelengths can be measured at nodes |
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As energy increases
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frequency increases and wavelengths decrease
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As wavelength decreases
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number of nodes increase
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4 quantum numbers
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n = energy level (1, 2, 3, 4...)
l = orbital type/subshell (0,... n-1) ml = spatial orientation (-l...0...l) ms = spin (1/2 or -1/2) |
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n - 1
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number of nodes
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l
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number of angular nodes
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(n-1) - l
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number of spherical nodes
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l = 0
l = 1 l = 2 l = 3 |
S orbital
p orbital d orbital f orbital |
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n
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number of orbital types
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n = 1
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can be:
l=0 --> S |
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n = 2
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can be:
l=0 --> S l=1 --> Px, Py, Pz |
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n = 3
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can be:
l=0 --> S l=1 --> Px, Py, Pz l=2 --> dxy, dxz, dyz, dx^2y^2, dz^2 |
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Spin
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- makes electrons act like magnets
- there is an opposite spin so they attract and overcomes electric expulsion |
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Electron Configuration
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- can write Noble Gas of the electron that comes before it
- s^2 - p^6 - d^10 - f^14 |
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Orbitals are most stable when...
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it is full, half-filled, or empty
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Degenerate
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orbitals that are the same
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d4 and d9
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take 1 electron from S to make it more stable
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X^-y
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add y amount of electrons to the configuration of the element X
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isoelectronic
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elements that have the same amount of electrons --> F-1 is isoelectronic with Ne.
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X^+y
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subtract y amount of electrons from configuration of element X to make it more stable
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Boat Model
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- take away electrons from highest number orbital first
- 4s before 3d - P before S |
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Hund's Rule
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electrons sit alone when they can
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Pauli Exclusion Principle
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no more than 2 electrons in each orbital
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Aufbow Principle
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start at the bottom when filling orbitals
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Copenhagen Interpretation
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Both Bohr and Heisenberg believed that the electron can exist as both a particle and a wave at the same time
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How many orbital types in 3p are there?
How many orbitals in 3p are there? |
- orbital types= 3
- amount of orbitals = 3^2 = 9 |
