ChemistryMonday, 11-3-14• Go to my web page and click on the link for "Modern Atomic Theory PPT".• Use this PowerPoint to complete the notes handout.

• Tuesday 11-4-14• Go to my web page and open the link for Chem Textbook Ch 5• Read pgs. 125-126.• In your journal, answer Section Assessment questions 7-10.

ChemistryWednesday 11-5-14 Copy the following notes in your journal.

Quantum Numbers

• Every electron in an atom has its own unique set of quantum numbers, like its own

“address”.

Four quantum values:

• n (principal) ---> energy level (1-7; this coincides with the number of rows on the

periodic table.)

• L (orbital) ---> shape of orbital (We will be studying the first 3 orbital shapes.)

• mL (magnetic) ---> designates a particular suborbital (the x,y,z, orientation of the

orbital)

• s (spin) ---> spin of the electron (clockwise or counterclockwise: ½ or – ½)

Chemistry

• All electrons exist in distinct energy states, that is, they all have a very well defined energy associated with them.

• If an electron absorbs a particular amount of energy from outside the atom, it may temporarily “jump” up to a higher energy state.

• But it will usually very quickly return to its original energy level.

• When the electron returns to its original level, it gives back the energy it absorbed in the form of light (a photon).

Electrons returning from a higher energy level to a lower one.

The atoms of every element emit their own unique spectrum, as their electrons move between many combinations of energy levels. The energy levels for hydrogen – the simplest element – are as follows. 

Electron Excitation & Transition

ChemistryThursday 11-6-14• Find the handout, "Atomic Spectra Questions" that you were

given last week.• In your journal, write the answers to these questions.• Attach the handout in your journal also.• You may want to refer to the textbook (Ch. 5) as well as the

notes you took yesterday to determine the answers.

Chemistry: Friday 11-7-14; Atomic Spectra Activity

Hold the spectrometer right side up.While looking through the eyepiece, point the slit toward the light source.Without moving the spectrometer, shift your eye to the right.You should be able to see the spectrum superimposed on the wavelength scale.

Reading the Wavelength Scale

Multiply these values by 100 to get wavelength in nanometers, nm.

Examples: Blue line is at 450 nm; red line is at 630 nm.

Sketch the different spectra that you observe on your Data Sheet.https://onedrive.live.com/view.aspx?cid=0171D4F305BF14BE&resid=171D4F305BF14BE%213204&app=Word