1. LS 2.1 Learning Goal: Understand how electrons behave in an atom
To be able to write electron configurations

2. Electron Configurations
So today we are going to be talking about orbitals and energy, and will be learning how to make energy diagrams for a different elements

3. Quantum Numbers location address
Describe the ______________ of the e-’s around the nucleus.
Quantum #’s are sort of like a home _____________ for the electron.
address

4. Quantum Numbers properties how why
This information about the location of the e-’s in an atom can be used to:
(1) determine chemical & physical _____________ for the elements.
(2) show how the _______________ __________ is organized.
(3) show _____ and _____ elements combine to form compounds.
properties
Periodic Table
how
why

5. Energy Levels Principle Energy Levels Quantum Number n
n = 1, 2, 3, ect
Not evenly spaced
Electrons with more
energy are further away
We have energy levels: the principle energy level and each sublevel associated with the principle energy level. The principle energy levels in an atom are designated by the quantum number: N. You guys learned a little bit about this with Bohr’s proposed model. It was something like this. (Draw circles)
is this accurate? …No. Why? We cant measure the orbit of an electron due to the Heisenberg Uncertainty Principle. Which is? Right, there is no way to know both where an electron is and its momentum or in other words knowing where its going next.
Here we have orbits, but an oribal is different than orbits,
So unlike the Bohr’s model, we have sublevels, the primary levels are divided into one or more of these sublevels. s, p, d, f.

6. Energy Levels Sublevels Orbital s, p, d, f
Principle Energy Levels
Quantum Number n
n = 1, 2, 3, ect
Sublevels
s, p, d, f
Quantum number n tells us HOW MANY sublevels
Orbital
Different from an orbit
Region of probability that can contain at most two electrons
We have energy levels: the principle energy level and each sublevel associated with the principle energy level. The principle energy levels in an atom are designated by the quantum number: N. You guys learned a little bit about this with Bohr’s proposed model. It was something like this. (Draw circles)
is this accurate? …No. Why? We cant measure the orbit of an electron due to the Heisenberg Uncertainty Principle. Which is? Right, there is no way to know both where an electron is and its momentum or in other words knowing where its going next.
Here we have orbits, but an oribal is different than orbits,
So unlike the Bohr’s model, we have sublevels, the primary levels are divided into one or more of these sublevels. s, p, d, f.

7. Heisenberg Uncertainty Principle – we cannot know both the position and the momentum of a particle at the same time
Heisenberg!

8. S Orbital Shape
1 S Orbital

9. P Orbital Shape
3 P Orbitals
P has more energy
than S

10. D & F Orbital Shape
5 D Orbitals 7 F Orbitals

11. Orbitals and Electrons
Sublevel
Number of Orbitals
Maximum Number of Electrons s 1 2 p 3 6 d 5 10 f 7 14
Each type of sublevel holds a different number or orbitals, and therefore, a different number of electrons. 
Each orbitals can hold, how many electrons? 2 right.
s sublevels has one orbital, which can hold up to two electrons. 
p sublevels have three orbitals, each of which can hold 2 electrons, for a total of 6. 
d sublevels have 5 orbitals, for a possible total of 10 electrons. 
f sublevels, with 7 orbitals, can hold up to 14 electrons. 

12. Periodic Table- S, P, D, F
Yesterday we learned about the orbital diagrams for atoms. Today we are going to learn how to write the electron configurations for each of them. Here are the blocks, the s block, the p block, the d block and f block. Using this information we can write out the electron configuration for a particular element.

13. Order of Energy Sublevels
Energy sublevels are filled in a specific order that is shown by the arrow diagram

14. Electron Configuration Layout
Find out the number of electrons
Go from Left to Right
1s1
Number of electrons in orbital
This is how it looks, we need to understand what each part of this means.
The large number 1 represents the energy level, n = 1
The s represents what type of orbital it is in
And the exponent 1 represents the number of electrons in the orbital or subshell
Type of orbital
Energy Level

15. Electron Configurations
Carbon (C)
__ electrons
1s2
2s2
2p2
Let’s try Carbon, In a neutral carbon, how many electrons do we have? \
Using our orbital diagram here, we can start writing our configuration. Write the first energy level and it’s orbital, 1s, how many electrons are in the orbital? 2. 1s2
Now we go to the next energy level, which is 2 and it’s an s orbital, so we have 2s, and how many electrons are in it? 2s2
We also have 2 in it, what orbital is it? P right. How many electronns? Right 2p2
So we have 1s22s22p2
And we can add up our electrons in our orbitals to see if it is the right amount, and here its which does equals 6.
Now we can also do it using this chart, by knowing which orbitals to fill in first.

16. Electron Configurations
Vanadium (V)
___ electrons
Add up electrons and it is 25
We can also do it using writing out this chart

17. Try writing configurations for:
Lithium
Sulfur
Tungsten (W)

18. Exit Slip
Write the electron configuration for Iron

19. Learning Goals
Understand how electromagnetic radiation is seen in our daily lives
Understand how light is produced

20. Video LInks http://www.youtube.com/watch?v=m4t7gTmBK3g

21. Electromagnetic Radiation

22. Electromagnetic Radiation
Electromagnetic radiation = energy being transmitted from one place to another by light
Each type has a specific wavelength and frequency

23. Electromagnetic Radiation

24. Types of Electromagnetic Radiation
Radio waves – transmit voices and music
X-rays - used to make image of bones
Microwaves – used to cook food
Infrared – we feel this as heat
Ultraviolet (UV) – gives you sunburn
*Snakes & Owls use infrared vision
*Some UV radiation blocked by the ozone layer

25. Infrared Vision

26. Types of Electromagnetic Radiation
Visible light – the only radiation we can detect with our eyes. It can be separated into colors with a prism
ROYGBIV

27. Types of Electromagnetic Radiation
7. Gamma rays – radioactive substances give it off

28. How light is produced
Atoms get hit with energy (by either being zapped with electricity or heated up) <picture a>
Electrons absorb this energy and jump to a higher energy level <picture b>
As they immediately fall back down to “the ground state,” they give off this energy in the form of light (or other electromagnetic radiation  photon) <picture c>

29. How light is produced
Ground State = lowest possible energy state Excited State = atom with excess energy

30. How light is produced Spectroscope
Each photon emitted has a specific color Since electrons are located in only certain energy levels (or orbitals) around the nucleus only certain specific colors of light are emitted.
Spectroscope
No two elements
produce the same
spectrum of colors

31. Exit Slip 1. Which electromagnetic radiation gives you sunburn?
2. What visible color has the longest wavelength?
3. What is a packet of energy called?