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Properties are determined by
electrons
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That particles of matter have the same properties of waves & vice versa
deBroglie
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deBroglie's equation
- E=mc2 (einstein) E=hv (Planck) c=yv / v=c/y
- hv=mc2, so hc/y=mc2, so y=hc/mc2, c's cancel and y=h/mc
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Wave-particle duality
A stream of electrons acts the same as waves of light
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How was wave-particle duality proved
mathematically by deBroglie's equations
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C=3x10^8 in a VACUUM. But, how does it travel elsewhere?
It travels at different speeds and changes directions (refracts)
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Index of refraction
- specific to a substance
- Calculated by the bending of a light ray passing from a vacuum into a new substance.
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Momentum
- P
- mass x velocity
- Tells where an object is going
- Since y = h/mv, y = h/p
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As the momentum of an object increases,
y decreases
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As the momentum of an object decreases,
y increases.
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To see an object,
It must be hit by a photon of light & reflected to our eyes.
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Uncertainty Principle
you can't ever know the exact position and momentum of a moving object at any given instant.
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You can't ever see the exact position of an electron because
The photon is deflected, but the electron is so small that it causes the electron to move.
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Uncertainty Principle by
Heisenerg
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Who treated the electron as a particle?
Schrodinger
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Theory of Quantum Mechanics
- Schrodinger
- Studies the behavior of very small objects travelling at velocities at or near the speed of light
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Newtonian Mechanics
- Newton
- studies the behavior of VISIBLE objects travelling at ORDINARY velocities.
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Who proved the planetary theory wrong?
Schrodinger
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Orbitals
3-dimensional regions around the nucleus that give the probable location of the electron
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Quantum Numbers tell us
- The most likely position of the electron in an electron cloud
- Specific properties of the orbitals
- Properties of the electrons in the orbitals
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Primary Quantum Number
- n
- MAIN ENERGY LEVEL occupied by the electron
- values from 1-7, 1 is the smallest and closest to the nucleus
- as n increases, the energy of the electron it contains increases, as doesthe distance from the nucleus.
- 2xn^2 = maximum number of electrons an energy level can hold.
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Second Quantum Number
- cursive l/ribbon
- SUBLEVEL and SHAPE of the orbital
- Number of sublevels in an energy level = n
- Except in n=1, sublevels of different shapes exist in the same energy level
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Third Quantum Number (m)
ORBITALS and SPATIAL ORIENTATION of the orbitals in a sublevel
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n^2
number of orbitals in an atom
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Electron configurations are in what state?
ground
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Outermost energy level
atoms with full s and p levels (8e)
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Rules for filling energy levels with electrons
- 1. Aufbau Principle
- 2. Pauli Exclusion Principle
- 3. Hund's Rule
- 4. Diagonal Rule
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Aufbau Principle
electrons occupy the lowest energy orbital that can recieve it.
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Pauli Exclusion Principle
No 2 electrons in the same atom can have exactly the same 4 quantum numbers.
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Hund's Rule
Orbitals of equal energy are each occupied by 1 electron before any orbital is occupied by a second electron.
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All electrons in singly-occupied orbitals must have the (spin)
same spin
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Diagonal Rule
- After 18 electrons have been assigned to the orbitals, the normal filling under rule one doesn't apply.
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Notations to show how electrons are arranged
- Electron configuration notation
- Orbital notation
- Electron dot diagram
- Noble gas notation
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Electron configuration notation
- levels with exponent
- 1s^2 2s^2 2p^6, etc.
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Orbital notation
Levels with arrows
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Electron dot diagram
- Write the symbol for the element
- Identify elements in the HIGHEST ENERGY LEVEL
- Doesn't matter which order the dots are in
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Noble gas notation
- Write the symbol for the noble gas which PRECEDES the element in brackets & then list the additional electrons the element contains after.
- [AR]4s^2 3d^10 4p^4
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