1. To Do… OWL Lectures Discussion Chapter 11 (Part 1) due Friday, April 6
Chapter 11 (Part 2) due Wednesday, April 11
Lectures
Continue reading Chapter 12
Discussion
Chapter 11 text homework
Chapter 12 text homework

2. Figure 11. 18 A representation of the photo of the firefly experiment
Figure A representation of the photo of the firefly experiment. Remember that a picture is brightest where the film has been exposed to the most light. Thus the intensity of the color reflects how often the firefly visited a given point in the room. Notice that the brightest area is in the center of the room near the source of the sex attractant.
Figure p247

3. Electrons Electrons are most likely to be found near the nucleus
Electrons could be anywhere (very far even)
We do not know how the electron moves
ORBITALS = regions of 90% probability

4. Figure 11. 20 (a) The hydrogen 1s orbital
Figure (a) The hydrogen 1s orbital. (b) The size of the orbital is defined by a sphere that contains 90% of the total electron probability. That is, the electron can be found inside this sphere 90% of the time. The 1s orbital is often represented simply as a sphere. However, the most accurate picture of the orbital is the probability map represented in (a).
Figure p248

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6. Figure 11.24 The relative sizes of the 1s and 2s orbitals of hydrogen.
Figure p249

7. Figure 11. 25 The three 2p orbitals: (a) 2px, (b) 2pz, (c) 2py
Figure The three 2p orbitals: (a) 2px, (b) 2pz, (c) 2py. The x, y, or z label indicates along which axis the two lobes are directed. Each orbital is shown both as a probability map and as a surface that encloses 90% of the electron probability.
Figure p250

8. Figure 11.28 The shapes and labels of the five 3d orbitals.
Figure p251

9. Figure The orbitals being filled for elements in various parts of the periodic table. Note that in going along a horizontal row (a period), the (n + 1)s orbital fills before the nd orbital. The group label indicates the number of valence electrons (the number of s plus the number of p electrons in the highest occupied principal energy level) for the elements in each group.
Figure p257

10. Figure The electron configurations in the sublevel last occupied for the first eighteen elements.
Figure p255

11. Valence Electrons Highest or outermost energy level electrons
Where the chemistry “happens”!
Look at principal quantum level n
Sulfur: 1s22s22p63s23p4
Valence electrons are in n = 3 level
Valence electrons = = 6 electrons

12. Clicker Question
How many unpaired electrons does sulfur contain in its ground state? (Hint: Draw an orbital diagram.)
A) 0
B) 1
C) 2
D) 3
E) 6

13. Clicker Question
Which of the following (a-c) does not correctly match the species with the expected electron configuration?
a) A ground state calcium atom [Ar] 4s2
b) The most stable ion for bromine [Ar] 4s23d104p6
c) An excited state of sulfur [Ne] 3s23p34s1
d) At least two of the above (a-c) are incorrectly matched.
e) All of the above (a-c) are correctly matched.