Lecture Day! Please get out: Line spectra packet (Exciting Salts) Lab notebook Get four pieces of paper on the back table Ask your table partner how their day is going.

Warm-Up In the flame test lab, you burned salts of sodium, calcium, strontium, copper, and potassium. In general, why did each salt give off a different color when placed in the flame? Draw a picture to support your answer. Take out your flame test lab for revision/collection

Warm-Up Answer EACH ATOM IS QUANTIZED. Each atom has only certain energy levels that are allowed. These energy levels are specific to that atom!

Flame Test Lab Revision (10 min.) Discuss with your table partners: 8c Your drawing in #9 Go through the Reflect and Connect questions Let’s discuss them together Turn in your revised lab to the turn in bin

Learning Targets I can write electron orbital configurations

If Bohr’s electron orbits were wrong, then….? Evolution of Atomic Theory If Bohr’s electron orbits were wrong, then….?

Edwin Schrodinger’s Electron Clouds Schrodinger proposed that we can’t predict exactly where electrons will be and when (1926) Developed “orbitals”- clouds where electrons have a high probability to be found An orbital IS NOT an orbit Picture is infrared spectra of orbitals.

Edwin Schrodinger’s Electron Clouds Schrodinger explained that electrons behave like particles AND waves (kind of like light photons! We can’t pin down exactly where the e- is because it acts like a wave with its orbital. An orbital IS NOT an orbit

Fan Blades = e-

So, where do electrons live? Let’s tour their home!

S orbital—First Two Energy Levels (1s, 2s) Sphere 1 orientation Each sphere holds 2 e- Holds 2 e- total Each energy level = sphere gets bigger http://player.discoveryeducation.com/index.cfm?guidAssetId=F6B8C2BB-FB87-472D-82D0-F9D21DE42161&blnFromSearch=1&productcode=US Quantum Theory – Bohr and some stuff about orbitals Spheres get bigger with a higher energy level. “S” stands for sharp

The next energy level: p Orbitals Dumbbell shaped 3 different orientations Each dumbbell holds 2 e- Holds 6 e- total Each energy level = dumbbells get bigger “P” stands for principle. Each dumbbell can hold 2 electrons and there are 3 different orientations so the p level can hold up to 6 electrons. Dumbbells will get bigger and bigger with each energy level.

Energy Levels

A third type! d orbitals Cloverleaf shaped 5 different orientations Each cloverleaf holds 2 e- Holds 10 e- total Each energy level = cloverleaf gets bigger “D” stands for diffuse. Mainly clover shaped with the exception of one orientation. Each orientation can hold 2 electrons and with five orientation they can hold up to 10 electrons. With each energy level the clover leaf gets bigger and bigger.

A fourth type! F orbitals Crazy shaped 7 different orientations Each shape holds 2 e- Holds 14 e- total Gets bigger with each energy level “F” stands for fundamental. Crazy shape, look kind of like the game jax with the bouncy balls? 7 different orientation, each one holding 2 electrons so this level can hold a total of 14 electrons.

Neon, with two filled shells (10 electrons) (a) Electron-distribution Fig. 2-10-2 Neon, with two filled shells (10 electrons) (a) Electron-distribution diagram First shell Second shell (b) Separate electron orbitals 1s orbital Figure 2.10 Electron orbitals

Neon, with two filled shells (10 electrons) (a) Electron-distribution Fig. 2-10-3 Neon, with two filled shells (10 electrons) (a) Electron-distribution diagram First shell Second shell (b) Separate electron orbitals x y z 1s orbital 2s orbital Three 2p orbitals Figure 2.10 Electron orbitals

Neon, with two filled shells (10 electrons) (a) Electron-distribution Fig. 2-10-4 Neon, with two filled shells (10 electrons) (a) Electron-distribution diagram First shell Second shell (b) Separate electron orbitals x y z 1s orbital 2s orbital Three 2p orbitals Figure 2.10 Electron orbitals (c) Superimposed electron orbitals 1s, 2s, and 2p orbitals

What orbital can…. …hold 2 e- total? …hold 6 e- total? Elements can be separated into “blocks” depending on what orbital their valence electrons live in- label your table! What orbital can…. …hold 2 e- total? …hold 6 e- total? …hold 10 e- total? …hold 14 e- total? This will help connect the orbitals to the periodic table. The periodic table is weirdly shaped…there are four different blocks AND we have four different orbitals. The s orbital can hold 2 electrons. The blue block can hold 2 electrons. The p orbital can hold 6 electrons and the red block is 6 blocks wide. The d orbital can hold 10 electrons so the green block can hold 10 and the f orbital can hold 14 electrons so the yellow block can hold 14

In what order do orbitals fill? Electrons are filled into orbitals in the order that keeps them at the LOWEST energy level! Start with the lowest energy level first. Notice the s and p blocks are the same as the period levels. We go down an energy level when we go to d block. In the 6th period we drop down into the f block. Let’s label energy levels!

How to write electron configurations… Orbital 1s2 # of electrons in that orbital Energy level

Let’s write the configuration for… Neon atom: 1s2 2s2 2p6 Double check! Start from the top? Yes! Correct number of electrons? Should have 10 e- since it is an atom, 2+2+6=10! Sodium atom: 1s2 2s2 2p6 3s1 Double check! Started from the top? YES! Correct number of electrons? Should have 11 e- since it is an atom 2+2+6+1=11! UGH! SO MUCH WORK! Let’s make this abbreviated! Sodium has all of Neon’s electrons plus 3s1 [1s2 2s2 2p6] 3s1 [Ne] 3s1 YOU CAN ONLY ABBREVIATE USING NOBLE GASES!

Let’s Practice by filling in the table! We will figure out the total # of electrons Then, start filling the orbitals until every electron has a home S orbitals hold 2 P orbitals hold 6 D orbitals hold 10 F orbitals hold 14!

Nice Job! On back, write the extended AND abbreviated electron configurations for: Calcium Tin Calcium: 1s2, 2s2, 2p6, 3s2, 3p6, 4s2 OR [Ar] 4s2 Tin: 1s2, 2s2, 2p6, 3s2, 3p6, 4s2, 3d10, 4p6, 5s2, 4d10, 5p2 OR [Kr] 5s2, 4d10, 5p2 Self Check: How many electrons does Tin have? 50! 2+2+6+2+6+2+10+6+2+10+2= 50!

Exit Task Draw a Bohr Model for Magnesium Write the long and abbreviated electron configuration for Magnesium How many valence electrons does Magnesium have? Circle the valence electrons in your Bohr Model and in both of your electron configurations 1s2 2s2 2p6 3s2  [Ne] 3s2 2 valence electrons