How is an electron able to change energy levels? Q of the Day How is an electron able to change energy levels? Day 1 1-7

Objective / Essential Question How do we define / describe an electron’s location in the atom?

Revisiting the Electron Cloud Notes Page 7 Revisiting the Electron Cloud Electron Position: probability orbitals uncertainty Electron Distribution Properties of element

How can the whereabouts of an electron compare to an apartment building? Floor/story of building Suite/apartment Bedroom Female / Male Energy level Sublevel Orbital for e- couple Spin

The Address of the Electrons Just like people in an apartment, electrons have an address. The most probable location of an electron is described using quantum numbers. Each electron has 4 quantum numbers which each relays a different piece of information about the electron’s possible whereabouts in the atom.

The Address of the Electrons Pauli exclusion- no 2 electrons can have the same address!!! – same 4 quantum numbers

Describing Atomic Structure Energy level – regions of space where there is a high probability of finding electrons Energy levels - break into - Sublevels - break into - Orbitals

Describing Atomic Structure Sublevels First sublevel – 2 electrons 3 Second sublevel – 6 electrons 2 1 Third sublevel – 10 electrons

Describing Atomic Structure – Building an Address Energy levels – designated by - # 1st Level = 1, 2nd Level = 2, etc. … Sublevels – designated by – letter (s, p, d, f) 1st Sublevel = s 2nd Sublevel = p 3rd Sublevel = d 4th Sublevel = f

Describing Atomic Structure # of energy level = # of sublevels in that energy level Energy level 1 = 1 sublevel Energy level 2 = 2 sublevels Energy level 3 = 3 sublevels …

Describing Atomic Structure Sublevels f d p s E n e r g y Energy still Increases away from the nucleus

Q of the Day Day 2 1-8 Why is it impossible to determine the speed and location of an electron at the same time?

Do you think Bohr was right or wrong? The New Atom? Do you think Bohr was right or wrong? Pauli exclusion? Energy levels - break into - Sublevels - break into - Orbitals

Electron Arrangement Energy level 1, sublevel s, orbital 1s Energy level 2, has two sublevels s and p, 2s orbital and 2p orbitals 2 3 1 Energy level 3, 3 sublevels s, p, and d, 3s orbital, 3p orbitals, and 3d orbitals

Electron Arrangement Quantum #s – specify the properties of atomic orbitals and the properties of electrons in those orbitals Principle quantum # (n) – main energy level = 1, 2, 3… Angular momentum quantum # (l) –shape of the orbital = 0, 1, 2… (n-1) 0 = s, 1 = p, 2 = d, 3 = f Magnetic quantum # (ml) – orientation of the orbital around the nucleus

Electron Arrangement Quantum #s – specify the properties of atomic orbitals and the properties of electrons in those orbitals Magnetic quantum # (ml) – orientation of the orbital around the nucleus Spin quantum # – indicate the two possible spin states (+1/2, -1/2)

Electron Arrangement Energy levels – designated by - # (n the principle quantum #) Sublevels – designated by – letter (s, p, d, f) (l the angular momentum quantum #) s = 0 p = 1 d = 2 f = 3 E n e r g y Energy still Increases away from the nucleus

Electron Arrangement How many electrons in an orbital? 2 electrons fit in an orbital one spinning in the +1/2 orientation and one spinning in the -1/2 orientation

Prelab Notebook Checks

Q of the Day 1. What is an atomic emission spectra (use your lab handout if necessary)? Day 3 1-11

Q of the Day NO ATB today. Sit with your partner(s) for lab and get out your lab. Wait for instructions. Day 5 1-13

LAB Day 3 1-11 Day 4 1-12 Day 6 1-13

COMPLETED LAB PACKETS ARE DUE TOMORROW!!!

QUARTERLY WILL BE NEXT WEDNESDAY

Quantum Theory Quanta’s Ability: Did not do 2012-2013. Quanta’s Ability: Light energy hits the electrons in metal- the light must be powerful enough. Electrons in the metal absorb the energy. The electrons become excited, and they jump out of the metal.

Quantum Theory Did not do 2012-2013. The electrons become excited, and they jump out of the metal. The electrons fall down again, and create a spark or current. Examples: The luster of a shiny metal, Photoelectric cells (solar power)

Q of the Day How many electrons fit in an orbital?  How is their movement different (from each other)? Day 1 1-15

COMPLETED LAB PACKETS ARE DUE TODAY!!!

Q of the Day How many sig figs: 4020 4020.00 0.004020 Day 2 1-19

QUARTERLY WILL BE NEXT WEDNESDAY

QUARTERLY REVIEW NOTEBOOK CHECKS

Q of the Day There are 4 quantum numbers for each electron. Each one tells you something about the electron’s location within the atom. What do they tell you? Energy level, sublevel, orbital, spin Day 4 1-21

NOTES

Electron Arrangement s = 1 p = 3 d = 5 f = 7 How many orbitals in each sublevel? s = 1 p = 3 d = 5 f = 7

Electron Arrangement How many sublevels in each energy level? 1 = _____ (__) 2 = _____ (____) 3 = _____ (______) 4 = _____ (__________) 3 2 1

Electron Arrangement Each x = an electron Each xx = an orbital Energy Level 4 3 2 1 xx xx xx xx xx xx xx xx xx xx xx xx xx xx xx xx f d p s Each x = an electron Each xx = an orbital

Review Energy levels  number Sublevel  letter s, p, d, f

Taking a Look at Orbitals D P Notes Page 10

Taking a Look at Orbitals

Taking a Look at Orbitals Why does the ring model work? p – orbitals always occur in 3’s (one for each dimension)

Q of the Day Get out your electron acrostic from yesterday. You have 2 minutes to finish!!! Today’s ATB = What shape is an s sublevel? What shape is a p sublevel? Day 5 1-22

Electron Acrostic E L C T R O N

Electron Arrangement Recall that atoms like to stay in their most stable (lowest energy) state. - Sublevels fill from the nucleus outward 3 2 1 Handouts

Electron Arrangement Recall that atoms like to stay in their most stable (lowest energy) state = electron configuration electron configuration – notation used to show electron placement within sublevels

Electron Arrangement electron configuration – notation used to show electron placement within orbitals electron Configuration for: Si 1s22s22p63s23p2 C 1s22s22p2

Electron Configurations Practice: 1s22s22p63s23p4 F 1s22s22p5 1s22s22p63s23p3 P http://www.youtube.com/watch?v=Vb6kAxwSWgU http://www.youtube.com/watch?v=rcKilE9CdaA Practice

The most likely location of an electron is described by a wave of probability. This type of wave is actually a set pattern that forms a 3-D shape within the space of the atom. This wave pattern does not overlap itself and is known as a standing wave. http://www.youtube.com/watch?v=-gr7KmTOrx0 http://www.youtube.com/watch?v=3BN5-JSsu_4 http://www.youtube.com/watch?v=18BL7MKjtZM

Define: quantized wavelength electron cloud model radiant energy Plank’s constant Bohr excited state electromagnetic radiation quantized wavelength electron cloud model radiant energy Speed of light 48

Objective / Essential Question How do we define / describe an electron’s location in the atom?

Quick Talk Compton quanta excited state continuous particle or wave Ground state radiant energy Bohr photon frequency 50

Ask your discussion partner a question.

Electron Acrostic E L C T R O N

Electron Acrostic E L C T R O N

Element Electron Configuration Noble Gas Notation # of Valence electrons Mn C