Test 4 Flashcards
Structure of an atom
Hard, dense (+) nucleus in the center
There are energy levels that are composed of sublevels which are composed of a set number of orbitals which contain 2 electrons each (spin up and spin down)
Excited State
An electron absorbs energy and is bumped up an energy level, leaves a “gap” (a subshell or shell that has been skipped)
Most Stable
full s and p shells (noble gases)
Bohr
Rejected Rutherford’s idea of electrons orbiting the nucleus (because they would have to be going faster than the speed of light if that was the case). Instead, he proposed that electrons exist in energy levels that contain subshells/sublevels each containing a certain number of orbitals that contain 2 electrons each. Electrons can move between energy levels but they must have the exact amount of energy in order to do so (nothing more, nothing less).
Order of Electron Configuration
1s2s2p3s3p4s3d4p5s4d5p6s4f5d6p
Electron Configuration
The coordinates for the electrons of an element in ground state
Second most stable
Full subshells, s or p
Least stable
half filled subshells
Octet Rule
By saying full n= shell, stability is determined only by the 8 electrons in the s and p shells to be full
Quantum Numbers
Numerical values that represent unique electrons and are used to calculate different properties of the electrons (all quantum mechanical probabilities)
(n, l, m, s)
n (quantum number)
principle quantum number
= to the energy level (shell number)
l (quantum number)
angular momentum quantum number
corresponds to the subshell
0 = s, 1 = p, 2 = d, 3 = f
varies up to n - 1
m (quantum number)
magnetic quantum number
corresponds to the orbital
varies between -l and l
s (quantum number)
spin quantum number
corresponds to spin up or spin down
+/- 1/2
valence electron
highest n value/energy, most reactive electrons, the electron that gives the element its chemical identity
the same thing as the outer shell
