EMR and the atom: Part Deux EMR and the atom: Part Deux on to electron configurations from wave information http://imagers.gsfc.nasa.gov/ems/waves3.html

What you’ve seen so far…. Model of a Nitrogen (z=7) atom

Which is really not true- why? Because orbitals- the “electron cloud” are 3-D, not flat are not round in most cases e-s are spread out as much as possible (e-s are moving very rapidly)

Sublevels and Orbitals The electrons are spread out in orbitals that have varying Shapes Energy (distance from nucleus) The orbitals are described in regards to their quantum numbers

The value of “n” The first number (1, #, #,±#) Describe the The first number (1, #, #,±#) Describe the distance from the nucleus of the orbital The energy of the orbital Values for n are integers The smallest possible value is 1 As the distance from the nucleus (and therefore energy) increases, the number increases

Quantum numbers

There periodic table and n The 7 periods on the periodic table correspond to n values Each period has a unique n value For the 1st period, n=1 For the 2nd period, n=2 And so on….

The “shape” of things Is the shape of the sublevel can change The “shape” of things Is the shape of the sublevel can change There are 4 shapes (although we only deal with the first 3) s p d f

The s sublevel http://www.sfu.ca/~nbranda/28xweb/images/s_orbital.gif

p sublevel

d sublevel

Another look at d sublevel

f sublevel

Orbitals Denote the _________________ that is filled s sublevel has one orbital; a sphere has 1 orientation in space p sublevel has three orbitals; 3 orientations in space d sublevel has five orbitals; 5 orientations in space f sublevel has seven orbitals; 7 orientations in space

General tutorials for electron configuration stuff some slides in this PowerPoint are from this site already http://www.wwnorton.com/chemistry/overview/ch3.htm See key equations and concepts (select from menu on the left), as well as the looking through the overview where to the tutorials are listed (links for just those are on the left, too)

How we use this…. There is a specific order to how the e- fill the orbitals; it is not random Although there are exceptions to the rules (last thing we do)

The principles of e- configuration The Aufbau (next) Principle: That e- fill the lowest energy sublevel before going to the next sublevel The Pauli Exclusion Principle: That e-s are paired according to opposite spins Hund’s Rule: e-s spread out in equal energy sublevels before placing electrons

The first level to fill is the 1s level It is the lowest energy sublevel It holds two electrons They are oppositely paired (up and down- ↑↓) Each sublevel (each __) holds 2 electrons

Next… The second sublevel is the 2s sublevel It also holds 2 electrons (because s holds 2, not because of the number), also oppositely paired ↑↓

1s2, 2s2,then comes 2p6 So, as it states above 1s fills, 2s fills ,then comes 2p It holds up to six electrons Because p orbitals hold 6 electrons

Next… From 2p, Notice, you follow the arrows From 2p, 3s fills with 2e-, then onto 3p, with 6e- then 4s with 2e- followed by 3d with 10e- (because d holds 10e-) Then 4p with 6e- Notice, you follow the arrows Remember, the number of electrons comes from the letter (the orbital’s momentum, m)

The sublevels of the orbitals are first filled, then you continue onto the next level (Aufbau) Also be sure to place one electron in each sublevel prior to filling the level (↑ ↑ ↑ and not ↑↓ ↑ _) (Hund) e-s must be paired with e-s of opposite spin (↑↓, not ↑↑ or ↓↓) (Pauli)

Putting it all together… Carbon (neutral, so 6 electrons) What this would look like: ↑↓ ↑↓ ↑ ↑ _ 1s 2s 2p (notice there are 6 arrows for 6 electrons) This can also be written as 1s2 2s2 2p2 Notice the superscripts add up to 6