MIME-Version: 1.0 Content-Type: multipart/related; boundary="----=_NextPart_01C94A5D.8AE83EE0" This document is a Single File Web Page, also known as a Web Archive file. If you are seeing this message, your browser or editor doesn't support Web Archive files. Please download a browser that supports Web Archive, such as Microsoft Internet Explorer. ------=_NextPart_01C94A5D.8AE83EE0 Content-Location: file:///C:/D9286902/Fall08.Phys3650.exam2.SolutionWeb.htm Content-Transfer-Encoding: quoted-printable Content-Type: text/html; charset="us-ascii" TIME OF COMPLETION_______________

TIME OF COMPLETION_______________  &nb= sp;         NAME____SOLUTION= _________________________

 

 

<= span style=3D'font-family:"Times New Roman"'>&nb= sp;            =             &nb= sp;            =      DEPARTMENT OF NATURAL SCIENCES

 

PHYS 3650, Exam 2            =             &nb= sp;            =             &nb= sp;            =             &nb= sp;            =             &nb= sp;  Section 1

Version 1           &nb= sp;            =             &nb= sp;            =             &nb= sp;            =             &nb= sp;            =        October 31, 2008

Total Weight: 100 points

 

1.         = Check your examination for completeness prior to starting.  There are a total of nine (9) prob= lems on six (6) pages.

 

2.         = Authorized references include your calculator with calculator handbook, and the Refere= nce Data Pamphlet (provided by your instructor).

 

3.         = You will have 50 minutes to complete the examination.

 

4.         = The total weight of the examination is 100 points.

 

5.         = There are six (6) multiple choice and three (3) calculation problems. Work five (= 5) multiple choice and three (3) calculation problems.  Show all work; partial credit will= be given for correct work shown.

 

6.         = If you have any questions during the examination, see your instructor who will=

be located in the classroom.

 

7.         = Start:        &= nbsp;      10:00 a.m.

Stop:            &= nbsp;   10:50 a.m

 

 

 

&= nbsp;           &nbs= p; PROBLEM

 

&= nbsp;           &nbs= p;    POINTS

 

&= nbsp;           &nbs= p;   CREDIT

 

   &nbs= p;            &= nbsp;    1-6

 

   &nbs= p;            &= nbsp;    25

 

&= nbsp;

 

   &nbs= p;            &= nbsp;     7

 

   &nbs= p;            &= nbsp;    25

 

&= nbsp;

 

8

 

   &nbs= p;            &= nbsp;    25

 

&= nbsp;

 

   &nbs= p;            &= nbsp;     9

 

   &nbs= p;            &= nbsp;    25

 

&= nbsp;

 

&= nbsp;           &nbs= p;    TOTAL

 

&= nbsp;           &nbs= p;       100

 

 

 

 

 

&= nbsp;          PERCENTA= GE

 

 

 

 

 

CIRCLE THE SINGLE BEST ANSWER FOR ALL MULTIPLE CHOICE QUESTIONS. IN MULTIPLE CHOICE QUESTIONS WHICH REQUIRE A CALCULATION SHOW WORK FOR PARTIAL CREDIT.

 

 

1. Hydrogen atoms can emit lines with visible co= lors from red to violet. These four visible lines emitted by hydrogen atom are produced by electrons

 

  &nbs= p;         a. That start in the n =3D 2 level= .

 

  &nbs= p;         b. That end up the n =3D 2 level.

(5)

  &nbs= p;         c. That end up in the n =3D 3 leve= l.

 

  &nbs= p;         d. That start in the ground level.

 

 

2.   According to the Pauli’s exclusion principle, how many electro= ns in an atom may have a particular set of quantum numbers?

 

  &nbs= p;         a. 1.

 

  &nbs= p;         b. 2.

(5)

  &nbs= p;         c. 6.

 

  &nbs= p;         d. 10.

 

 

 

3.  The orbital angular momentum quantum number can take which of the following values for = any given value of the principal quantum number, n?

 

  &nbs= p;         a. l =3D 0, 1, 2,…..<= span style=3D'font-size:12.0pt;color:windowtext'>

 

  &nbs= p;         b. l =3D 0, 1, 2, …., n.

(5)

  &nbs= p;         c. l =3D 0, 1= , 2, …., n – 1. 

 

  &nbs= p;         d. l =3D 0, 1, 2, …., n + 1.

 

 

 

 

 

 

4.  Which of the following values are associated with the electron spin quantum numbe= r, ms?

 

  &nbs= p;         a. ± 1/2.

 

  &nbs= p;         b. 0.

(5)

  &nbs= p;         c. ± 1.

 

  &nbs= p;         d. ± <= span style=3D'font-size:12.0pt'>2.

 

5.  Which ones of the atomic transition on the sodium energy level diagram below are = NOT allowed by the selection rules?

 
 
            a. a and c.

 

  &nbs= p;         b. b and f.

(5)

  &nbs= p;         c. c and d.

 

  &nbs= p;         d. d and g.

 

 

 

 

 

 

 

 

6.  Given the energy diagram above, es= timate the wavelength of a photon emitted by a sodium atom as the electron goes through the transition d.

            = a. 800 nm.

(5)       b. 620 nm.<= /span>

            = c. 450 nm.

            = d. 75 nm.  

 

  1. Titanium (Z =3D 22) is in its = ground state.

 

    1. What is its electronic configuration?

 

1s22s22p63s23p64s23d2

 

    1. List all the possible combina= tions of quantum numbers (n, l, ml, and ms)

an electron can have while in the subshell which is only partially filled in the  ground state.<= /span>

 

 

 3d subshell: n =3D 3, l =3D 2     

 

        =             &nb= sp;            =              l =3D 2        =       ml =3D -2        =        ms =3D +- 1/2        =              (3 2 -2 ½ )         (3 2 -2 -½ )  &nbs= p;

 

        =             &nb= sp;         =             &nb= sp;   l =3D 2      &= nbsp;       ml =3D -1        =        ms =3D +- 1/2        =              (3 2 -1 ½ )         (3 2 -1 -½ )      

 

        =             &nb= sp;            =              l =3D 2        =       ml =3D 0        =        ms =3D +- 1/2        =               (3 2 0 ½ )         (3 2 0 -½ )        

 

        =             &nb= sp;            =              l =3D 2        =       ml =3D 1        =        ms =3D +- 1/2        =             &nb= sp; (3 2 1 ½ )         (3 2 1 -½ )      

 

        =             &nb= sp;            =              l =3D 2             =  ml =3D 2        =        ms =3D +- 1/2        =             &nb= sp; (3 2 2 ½ )         (3 2 2 -½ )   

 

 

8.&n= bsp;    Using Bohr’s model, estimate the wavele= ngth of the Ka line  for

a.   &n= bsp;  calcium (Z =3D 20), and

&= nbsp;

EK =3D = - (Z-1)2 E0/12 =3D - (19)2 (13.6 eV)/12<= /sup> =3D - 4,910 eV

EL =3D = - (Z-1)2 E0/12 =3D - (19)2 (13.6 eV)/22<= /sup> =3D - 1.227 eV

DE =3D EL – EK =3D 3,683 eV

 l =3D hc/DE =3D 0.337 nm

       b. c= admium (Z =3D 48)

&= nbsp;

EK =3D = - (Z-1)2 E0/12 =3D - (47)2 (13.6 eV)/12<= /sup> =3D - 30,042 eV

EL =3D = - (Z-1)2 E0/12 =3D - (47)2 (13.6 eV)/22<= /sup> =3D - 7,510 eV

DE =3D EL – EK =3D 22,532 eV

 l =3D hc/DE =3D 0.0550 nm

 

&nb= sp;

9.     Find the energy of= the electron in the ground state of singly ionized helium (Z =3D 2).=

E1 =3D = - (Z)2 E0/12 =3D - (2)2 (13.6 eV)/12 =3D - 54.4 eV

 

What is the shortest possible wavelength which is emitted as a result of electron returning to the ground state?

Shorte= st wavelength corresponds to the transition from n =3D ∞:

DE =3D E∞ – E1 =3D 54.4 = eV

 l =3D hc/DE =3D 22.8 nm

What is the longest possible wavelength which is emitted as a result of electron returning to the ground state?

Lonest wavelength corresponds to the transision from n =3D 2:

E2 =3D = - (Z)2 E0/22 =3D - (2)2 (13.6 eV)/22 =3D - 13.6 eV

DE =3D E2 – E1 =3D 40.8 eV

 l<= span lang=3DEN-AU style=3D'font-size:12.0pt;line-height:200%'> =3D hc/DE =3D 30.4 nm

 

 

 

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PHYS 3650 Exam 2, Version 1

Fall 2008

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