Structure 1.3 Flashcards
(24 cards)
What is the high energy and frequency end of the EMS?
Violet end
What is the low energy and frequency end of the EMS?
Red end
Aufbau Principle
Electrons fill the lowest available energy levels before the higher levels
Hund’s Rule
If two or more orbitals of equal energy are available electrons will occupy them singularly before filling them in in pairs.
Pauli’s Exclusion Principle
No two electrons can have the same four electronic quantum numbers. (Each orbital can only contain a maximum of 2 electrons)
Cr electron config. exception
Its 3d orbital is half filled before its 4s orbital is completely filled
Cu electron config. exception
Its 3d orbital is filled before its 4s orbital is completely filled
Condensed Electrons Configurations build upon…
the last noble gas
What do emission spectra consist of?
Discrete lines at particular wavelengths corresponding to the distance between energy levels.
What happens to the electrons in an atom when they gain energy
They get excited and move to higher energy levels
What do electrons emit as they drop back down to lower levels
photons
Hydrogen emission spectra
Has discrete lines which converge toward the higher end of the spectrum. Has additional emission spectra in the uv and ir regions of the spectrum.
Electron transitions
Movement of electrons between shells
From what shells produces the visible spectrum
From n>2 to n=2
Convergence of energy levels
Energy levels get closer together as n increases
Max number of electrons in each energy level n=1-4
1- 2
2-8
3-18
4-32
How many electrons fit in an s sub-level
2
How many electrons fit in an p sub-level
6
How many electrons fit in an d sub-level
10
How many electrons fit in an f sub-level
14
How many electrons can each atomic orbital contain
A max of 2. They are spinning in opposite directions
Shape of s orbitals
spherical
Shape of s orbitals
Orthogonal and dumb-bell shaped
Shape of d orbitals
variety of shapes
