| A | B |
|---|
| each electron has been assigned | four quantum numbers "n", "l", "m", and 1/2 or -1/2 |
| the principal quantum number | indicates the main energy level occupied by electron, "n" positive integers 1-7 |
| the shell is a term | which represents the principal quantum number |
| the angular momentum quantum number | is represented by "l" which indicates shape or type of orbital |
| subshell is a term | which means the angular momentum quantum # |
| where "l" = 0 | the orbital is s shape( a sphere) |
| where "l" = 1 | the orbital is p shape (a dumbbell) |
| where "l"= 2 | the orbital is d shape (a cloverleaf) |
| where "l">or= to 3 | the orbital is f shape (complex) |
| the general defenition of quantum number is | a number that specifies the properties of electrons |
| the magnetic quantum # is | symbolized by "m" and indicates the tilt or orientation of an orbital |
| the magnetic quantum # is dependent on | the angular quantum # "l" |
| the spin quantum # is | symbolized by +1/2 or -1/2 |
| the spin quantum indicates | the orientation of an electron's magnetic field (relative to outside magnetic field) |
| Pauli determined that two, but no more than two | electrons can occupy a single orbital |
| No two electrons in the same atom can have the same 4 quantum #s | because they must always have opposite spins |
| there is 1 s orbital and that means | it can hold up to two electrons |
| there are three p orbital, and that means | they can hold up to six electrons |
| there are 5 d orbitals, and that means | they can hold up to ten electrons |
| there are 7 f orbitals, and that means | they can hold up to 14 electrons |
