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Embed code for: PT unit day 3 MILES NOTES
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Bell Work 10-18 Tuesday 10-19 Wednesday
Describe in your own words an excited state of an atom.
Explain why different colors are visible from different metals when they are heated.
- Turn in Pogil extension questions
Split a half-sheet of paper with your shoulder partner
Put everything away except the piece of paper and something to write with. (NO RED PENS)
The questions will be on the slides.
I will read each question twice and give your time to answer.
Once we have gone through each question I will go back through.
What is a common property of the groups on the periodic table?
Given the equation, E=hv. If the frequency is doubled what will happen to the energy?
If the wavelength of a wave is 562nm, what is the frequency of the wave? (c= 3.00*10^8 m/s)
Explain, In your words, the limitations to the Bohr model.
Draw an orbital diagram of neon in an excited state.
Aufbau’s Principle states that the __________ energy level must be filled first.
Bohr Model – energy levels house a specific number of electrons
Quantum mechanical Model changed from the circular rings for electrons to the electron cloud.
Each level of energy has a number of sub levels, which have different shapes
Energy Sub Levels
Electrons are at different distances from the nucleus based on their energy level.
Every major energy level is called the Principal Energy Level
1st Principal energy level has one sub level
2nd Principal energy level has two sublevels
3rd Principal energy level has three sub levels
4th Principal energy level has four sub levels
4 different sub levels
S sub level
Shape is a sphere
Can hold up to 2 electrons
P sub level
Shape is a dumbbell
3 different orbitals. On the x-axis, y-axis, and z-axis
Can hold up to 6 electrons ( 2 each )
Energy sub levels
D sub level
Double barbell like shape
5 orbitals, 4 are identical on the x, y, and z axis and one different one
Can hold up to dumbbell10 electrons total ( 2 each )
F Sub level
7 different multilobed shaped orbitals
Can hold up to 14 electrons total ( 2 each )
The major rules
Aufbau Principle- electrons occupy the lowest energy levels first.
Pauli exclusion Principle- states that a max of two electrons can occupy a single orbital. Both electrons have different spins. This is why there is more than one of the different p orbitals.(px,py,pz)
Hunds rule- single electrons with the same spin must occupy each equal-energy orbital before opposite spin electrons can be added
Like charges repel each other
Orbital arrangement can be displayed with boxes and arrows
Nobel Gas Configuration
Accounts for full inner shells ( 8 electrons )
Go back and put in the energy levels:
Lewis Dot Diagrams
Diagram what shows VALENCE ELECTRONS of the specific element.
Valence electrons – electrons in the atoms outer most energy level
Carbon – 1s22s22p2
Fluorine – 1s22s22p5
Neon - 1s22s22p6
Lithium – 1s22s1
Electron Configuration Activity
Working with your shoulder partner
Read all statements and determine TRUE or FALSE
Correct the false statements
Cut out the statements and place them into 2 groups, true and false.
Take the corrected statements and place them into groups
Glue the slips of paper down in their groups
*Why does 4s fill before 3d?
Because it is lower in energy…