1. Ch. 11 Notes---Modern Atomic Theory
Atomic Models
(1) Model:
a ball of (+) charge containing a number of e-
no ________________
often described as the “________ _______________” atom.
(2) Model:
a ____________ of (+) charge surrounded by a number of e-
no _____________ and no e- orbitals
Thomson
nucleus
plum pudding
Rutherford
nucleus
neutrons

2. Atomic Models
(3) Model:
a nucleus of (+) charge that also contains ______________
nucleus is encircled by e-’s located in definite orbits (or paths).
e-’s have ___________ energies in these orbits
e-’s do not lose energy as they orbit the nucleus
(4) Mechanical Model ( Wave Mechanical Model)
no definite ____________ to the e- path (“fuzzy” cloud)
orbits of e-’s based on the _________________ of finding the e- in the particular orbital shape.
Bohr
neutrons
fixed
Quantum
shape
probability

3. Bohr Atomic Model

4. Bohr Atomic Model

5. Quantum Mechanical Model

6. Quantum Mechanical Model

7. Quantum Mechanical Model

8. Energy Levels Diagram: (Fig. 11.10)
The energy levels in an atom are sort of like _________ of a ladder.
The more energy an electron has, the __________ away from the nucleus it usually will be.
The energy levels are not evenly spaced. They get ___________ together as you travel farther away.
To move from one “rung” to another requires a “____________” of energy.
rungs
farther
“excited state”
closer
quantum
“groundstate”

9. continuous energy levels quantized energy levels
Figure 11.15: The difference between continuous and quantized energy levels.
continuous energy levels
quantized energy levels

10. most probable location
Quantum Numbers
Describe the ______________ of the e-’s around the nucleus.
Quantum #’s are sort of like a home _____________ for the electron.
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.
most probable location
address
properties
Periodic Table
how
why

11. The Four Quantum Numbers
Principal Q. # (n): Describes the _____________ that the electron is from the nucleus. The bigger the number, the ___________ away the electron is.
Example: (1=closest, 2, 3, 4...farther away)
These distances are sometimes called _______________
______________ ____________.
distance
farther
principal
energy levels 1 2 3
nucleus

12. Orbital Q. # (l ): Describes the __________ of the electron’s path around the nucleus with a letter: (s, p, d, & f) These are sometimes called “_____________”.
s=_____________ cloud; p=_____________ or a 3-D figure 8;
shape
sublevels
spherical
ellipsoid

13. d & f orbital shapes are complex ________- _______________ ellipsoids, and some d’s and f’s are an ellipsoid with a doughnut or two around the middle.
All of these orbital shapes are based on the probability of finding the electron in the cloud.
d - orbitals
criss
crossing
f - orbitals

14. Figure 11.22: How principal energy levels can be divided into sublevels.

15. A Way to Visualize s, p, d, and f sublevels

16. Magnetic Q. # (m): tells how many _________________ in 3-D there are about the nucleus for each orbital shape.
s=___ orientation p= ___ orientations... (x, y, and z)
d= ___ orientations f= ___ orientations
The orientations are represented with a line or a box.
Examples: ___ This means a __________ orbital at a distance of 1s “__” (close) to the nucleus. This orbital is centered about the x, y, and z axis.
□ □ □ This represents an ___________ orbital with its p ____ possible orientations at a distance of “___” from the nucleus.
orientations 3 1 5 7
spherical 1
ellipsoid 3 4

17. Figure 11.23: Principal energy level 2 shown divided into the 2s and 2p sublevels

18. Spin Q. # (s): describes how the electron in an orientation is spinning around the nucleus. This spin can be thought of as “____” or “________”. (Some like to imagine it spinning “clockwise” and “counterclockwise”.) The spin is represented as an ___________ in the direction of the spin.
Example: ↑ This represents one electron in a _________ s orbital with spin “____” at a distance of “___” from the nucleus.
Remember, the four quantum numbers tell us the location, or “address” of each electron in an atom.
This information is vital in understanding the layout of the Periodic Table and the reasoning behind why and how atoms form bonds. up
down
arrow
spherical up 2

19. Electron Configurations
Electron configurations are notations that represent the four Quantum #’s for all of the electrons in a particular atom. Here are the rules for these notations:
Rule #1 (Aufbau Principle): Electrons fill ________ energy orbitals first.
Examples: 1s would be filled before ____
3s would fill before ____
lowest 2s 3p

20. Electron Configurations
Silicon ↑ ↑ ↑ ↓ ↑ ↓ ↑ ↓ ↑ ↓ ↑ ↓
(Energy Level Diagram) ↑ ↓
1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s, 5f, 6d, 7p…

21. Rule #2: Only ___ electrons can fit into each orientation.
Example: ___ ___ not ____
1s s s
Rule #3 (Pauli Exclusion Principle): Electrons in the same orientation have ______________ spin.
Example: ___ not ___
1s s
Rule #4 (Hund’s Rule): “_______________ rule”---> Every “□” in an orbital shape gets an electron before any orientation gets a second e-.
Example: □□□ not □□□
2p p 2 ↑ ↓ ↑ ↑ ↓ ↑
opposite ↑ ↓ ↑ ↑
Monopoly ↑ ↑ ↑ ↑ ↓ ↑

22. Example: ___ ___ ___ ___ ___ ___ 5s 4d becomes ___ ___ ___ ___ ___ ___
Rule #5: The Exceptions
Half-filled or completely filled d & f sublevels have ________ energies and are more stable than partially filled d’s and f’s.
This means that an atom can “borrow” one of its “s” electrons from the previous orbital to become more stable.
Example: ___ ___ ___ ___ ___ ___
5s d
becomes ___ ___ ___ ___ ___ ___
5s d
Because the 4d sublevel is now full, the atom is at a ________ energy state and therefore _________ stable.
lower ↑ ↓ ↑ ↓ ↑ ↓ ↑ ↓ ↑ ↓ ↑ ↑ ↓ ↑ ↓ ↑ ↓ ↑ ↓ ↑ ↓ ↑
lower
more

23. Electron Configurations
Practice Problems:
Write the electron configuration notation for each of the following
atoms:
Hydrogen
Carbon
Iron
Bromine
Shorthand Method: Assumes we already know about the # of □. H C Fe Br

24. How Electron Configurations Relate to the Organization of the Periodic Table

25. Figure 11.31: Orbitals being filled for elements in various parts of the periodic table.

26. Electron Configurations & Properties
How do electron configurations relate to the chemical and physical properties of an element?
All elements with the _________ outer shell e- configurations have ________ properties.
This means that elements in the same ____________ group have similar properties.
Examples: (1) Li, Na, K, Rb, and Cs all have __ lone “__” e- for their last orbital... (_____, _____, _____, etc.) This makes all of them ___________ reactive. They all react with __________ to produce hydrogen gas.
(2) Ne, Ar, Kr, Xe, and Rn all have the outer energy level completely __________ with electrons...(________, ________, ________, etc.) This makes all of them ______________. They do not produce __________________!
same
similar
vertical 1 s
2s1
3s1
4s1
very
water
filled
2s2 2p6
3s2 3p6
4s2 4p6
inert
compounds

27. More Practice Problems
(1) Which element has its last electron as a 4p5? ___________
(2) Which elements are similar in properties as Bromine? __________
(3) What would the outer shell electron configuration look like for the element underneath Radon, (Rn)?
(4) Which electron is added after 6s2? ________
(5) Which element would “borrow” a 5s electron to get a half-filled “d” sublevel? ___________
(6) What is the shape of the last orbital filled in Calcium, (Ca)? _____
(7) How many electrons are in the last “p-orbital” of Sulfur, (S)? ____
Bromine
F, Cl, I, At
…7s2 5f14 6d10 7p6
4f1 Mo
sphere 4

28. Electromagnetic Radiation
Any wave of energy traveling at a speed of ___________ is called electromagnetic radiation.
There are many types of electromagnetic radiation and each type has a different _______________ and _______________.
Here are the types of electromagnetic radiation from longest to shortest wave or lowest to highest frequency. These are also in order from lowest to highest energy.
light
frequency
wavelength

29. Electromagnetic Radiation

30. Electromagnetic Radiation
(1) Radio Waves -- used in __________________
(2) Microwaves-- broadcasts TV signals and used to _____ _______.
(3) Infrared (IR) -- we feel this as _____; _________ & ______ can “see” this.
communications
cook food
heat
Snakes
owls
infrared image of a cat
infrared image of heating pipes under a floor

31. Infrared Vision

32. Electromagnetic Radiation
(4) Visible Light -- the only radiation we can detect with our eyes. It can be separated into the colors of the spectrum with a __________.
ROYGBIV
(5) Ultraviolet (UV) -- gives you a _____________; _________ can “see” this; some of this radiation from the sun gets blocked by the ___________ layer
prism
sunburn
Bees
ozone
flower photo under normal light
flower photo under UV light

33. Electromagnetic Radiation
(6) X-rays -- used in medicine
Ouch!

34. Electromagnetic Radiation
(7) Gamma Rays-- some radioactive substances give it off
The last type of radiation is sometimes grouped with gamma rays…
(8)_______________Rays -- highest energy radiation; almost all of this
radiation from the sun is blocked by the ozone layer and the air.
Cosmic
Interesting superhero facts:
Superman has x-ray vision.
The Incredible Hulk was “created” by an accidental overdose of gamma radiation.
The Fantastic Four were “created” by cosmic rays.

35. How Light is Produced
When atoms get hit with energy (by _____________ them with electricity or by ____________ them up), the electrons absorb this energy and __________ to a higher energy level. Figure (a)
As they immediately fall back down to the “____________ state”, they give off this energy in the form of a particle of ___________ (or other types of electromagnetic radiation) called a _____________. Figure (b)
zapping
heating
jump
ground
light
photon

36. How Light is Produced
Each photon emitted has a specific ___________ (or frequency).
The color of the light that is given off depends on how _____ the electron _______ (which depends on how big of a jump it originally made.) The farther the fall, the ___________ energy the photon has.
color
far
fell
greater

37. Figure 11.6: Photons of red and blue light.

38. How Light is Produced energy
Since electrons are located only in certain __________ levels (or orbitals) around the nucleus, only certain specific _________ of light are emitted.
Scientists use a _________________ to separate these colors into bands of light. These bands of color look like a ______ code of color which is characteristic of that element. No two elements produce the same ______________ of colors. This can be used to distinguish one element from another contained in a sample. (See Fig )
color
spectroscope
bar
spectrum

39. Emission Spectrum
Hydrogen Spectrum
Neon Spectrum

40. How hydrogen produces the four visible photons

41. All the Photons Produced by Hydrogen