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45 Cards in this Set
- Front
- Back
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Whats is the Plum Pudding model? |
By JJ Thompson Spherical atom Uniformly distributed positive charge Negative charge resided in positive charge |
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Pros to plum pudding model |
Spherical presence of positive and negative atoms |
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Cons to plum pudding |
No nucleus could not explain the gold foil exp. |
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What is the nuclear model? |
By Ernest Rutherford contains a nucleus |
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What is a nucleus |
A dense region at the center Contains the atom's positive charge |
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Pros to the nuclear model |
atomic mass is concentrated in the nucleus explains gold foil exp. neutral nature of matter |
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Cons to the nuclear model |
fails to account for all the atom's mass electron arrangement negatively charged electrons are not pulled into positively charged nucleus |
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Planetary model |
By Neils Bohr fixed energy level paths quantum and quantum jump |
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Quantum |
specific amount of energy |
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Quantum Jump |
electron jumps from ground state to excited state |
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Pros to planetary model |
energy levels electron arrangement |
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Cons to planetary |
Failed to predict line spectra of atoms larger than Hydrogen |
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Quantum Mechanical Model (Q.M.M.) |
By Louis De Broglie electrons have dual properties wave functions predict 3D region |
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Dual properties of electrons |
behaves like particles wave like |
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Pros for Q.M.M. |
accounted for fixed energy levels wave like motion certain uncertainty |
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Cons for Q.M.M. |
limitation: uncertainty |
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Electrons |
negatively charged |
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Neutrons |
Neutrally charged |
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Protons |
positively charged |
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Isotopes |
Atoms with same number of protons but different number of neutrons |
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How to get the mass number of isotopes |
Protons + Neutrons in the nucleus |
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Electron Configuration |
how electrons are arranged around the nuclei atoms |
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n |
main energy level |
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l |
sublevel |
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x |
number of electrons |
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Noble gases |
He, Ne, Ar, Kr, Xe, Rn |
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Aufbau Principle |
electrons enter orbitals of the lowest available energy level |
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Pauli Exclusion Principle |
each electron has an associate spin |
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Hund's rule |
same spin must occupy each equal energy orbital |
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Heisenberg uncertainty
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it is impossible to know precisely the velocity and location of an electron at a specific given time |
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Quantum numbers |
defines the region in space where electrons are most probably located |
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Principle Quantum Numbers (n) |
Main energy level or period cannot be negative |
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Azimuthal Quantum numbers (l) |
Sublevel L= 0 to (n-1) |
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Magnetic Quantum # (Ml) |
number of orbitals/boxes Ml= -l to +l (including zero) |
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Spin Quantum # (Ms) |
Ms= -1/2 (downwards) and +1/2 (upwards) |
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Ammonium |
NH4 |
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Acetate |
C2H3O2 |
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Chlorate |
Clo3 |
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Hydroxide |
OH |
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Nitrate |
NO3 |
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Carbonate |
CO3 |
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Chromate |
CrO4 |
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Sulfate |
SO4 |
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Arsenate |
AsO4 |
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Phosphate |
PO4 |
