Light and Energy/Bohr Model of the atom TUESDAY, FEBRUARY 10, 2011

Mr Henderson started out the class by having us take out our packets and turn to page#13-14 to give us the correct answers to one of the webassigns due the previous day

(Pages 13-14)The answers to this webassign are:
1)a. Its predictions were inaccurate for atoms having more than one electron.
2)c. The best that one can know of an electron's location is to know the probability that it is in a given region of space.
3)d. Complex differential equations
4)b. Where an electron has a 90% probability of being located
5)b. The value of n cannot be negative AND c. The larger the n number, the higher the energy of the electron.
6)a. The value of l reveals information about the shape of the orbital housing the electron AND c. The value of l cannot be negative AND d. The value of l must be a whole number
7)b. The value of ml indicated the directional orientation of the orbital AND The value of ml must be a whole number
8)b. The value of ms indicated the spin direction
9)b. an l value of 1
10)a. TRUE b. TRUE c. TRUE d. TRUE e. TRUE
11)TRUE
12)b. 2
13)a. For every n value, there are just as many sublevels.
14)a. INVALID b. VALID c. INVALID d. INVALID
15)c. The 3s orbitals are larger than the 2s orbitals.

The class then looked at the blog from the previous day done by Dmitriy and Mr. Henderson had the class watch the video he added of the plane crashing into 12 feet of concrete.

Next the class took out their calculators and turned to page #1 to work on problem 4a. and 4b.
These problems will probably be the only time calculators will be needed to use for the rest of this unit.
The equation needed to remember for these equations is E=h*f=h*c/wavelength. f stands for frequency.

4a...red photon (f=4.80*10^14 Hz)

E=h*f=(6.62*10^-34)(4.80*10^14 Hz)=3.18*10^-19 Joules

4b...green photon (wavelength=5.43*10^-7)

E=h*c/wavelength=(6.62*10^-34)(2.998*10^8)/5.43*10^-7=3.66*10^-19 Joules

We continued the class period by turning to page #2 and started the problems in the chart at the bottom of the page.
Photon(Energy in Joules) use the equation from page #1
a. 3.03*10^-19
b. 4.09*10^-19
c. 4.55*10^-19
d. 4.85*10^-19
e. 5.00*10^-19
f. 1.64*10^-18
g. 1.93*10^-18
h. 1.06*10^-18
i. 1.55*10^-18

For these next problems use the equation En=Rh/n^2

• Rh is the constant called the Rydberg constant and its value is -2.180*10^-18 Joules.
• replace n with the number given in the problem.

E Initial(in Joules)
a.-2.42*10^-19
b. -1.36*10^-19

E Final(in Joules)
a. -5.45*10^-19
b. -5.45*10^-19

Change in E(in Joules)
a. -3.03*10^-19
b. -4.09*10^-19

The class was then given glasses that when put on revealed the true colors from white light included in roygbiv(red,orange,yellow,green,blue,indigo,violet)

We then also looked at different types of lighting which revealed different strengths of the colors from roygbiv.

At the end of the period the class ended the day by beginning a lab in the back of the room. The lab will be continued tomorrow

HW:next webassign not due till the 14th.