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Atomic Energy Transitions: Ultraviolet and Visible Spectrum, Assignments of Chemistry

The relationship between atomic energy transitions and the resulting emission and absorption of photons in the ultraviolet and visible regions of the electromagnetic spectrum. Topics include the effects of frequency and wavelength changes on atomic energy levels, the role of the ground state atom, and the significance of the principal quantum number (n) and orbital angular momentum quantum number (l) in determining permissible energy levels and electron configurations.

Typology: Assignments

Pre 2010

Uploaded on 08/18/2009

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CHM 115 E & G Ch. 7
19. The yellow light whose frequency is doubled would be in the ultraviolet region. The beam
whose wavelength is doubled would be in the infrared region.
22. The absorbed photon must be in the ultraviolet region, while the emitted photon is in the red
portion of the visible region. The ground state atom absorbs a photon raising it to a high lying
excited state. The atom then loses energy in the form of the red photon falling to a lower lying
excited state. If the ground state atom absorbed a red photon, it would be impossible for it to
emit an ultraviolet photon.
27.
c
2
.
998
x
10
8
s
1
1
.
365
x
10
6
s
1
219
.
6
m
31.
56
x
10
6
km
x
10
3
m
1
km
2
.
998
x
10
8
m
s
1
1
.
9
x
10
2
s
35.
E
h
6
.
626
x
10
34
J
s
x
1
.
365
x
10
6
s
1
9
.
044
x
10
28
J
39.
c
2
.
998
x
10
8
m
s
1
3
.
84
x
10
14
s
1
7
.
81
x
10
7
m
781
nm
This is just at the extreme red end of the visible spectrum.
43.
E
ph
R
H
(
1
n
2
u
1
n
2
l
)
2
.
179
x
10
18
J
(
1
2
2
1
1
2
)
1
.
634
x
10
18
J
hc
E
ph
(
6
.
626
x
10
34
J
s
)
(
2
.
998
x
10
8
m
s
1
)
1
.
634
x
10
18
J
1
.
216
x
10
7
m
121
.
6
nm
This wavelength is in the UV portion of the EM spectrum.
49.
h
mv
6
.
626
x
10
34
J
s
(
1
.
6749286
x
10
27
kg
)
(
4
.
15
x
10
3
m
s
1
)
9
.
53
x
10
11
m
95
.
3
pm
remember
1
J
1
kg
m
2
s
2
53.
h
mv
6
.
626
x
10
34
J
s
(
0
.
145
kg
)
(
30
.
0
m
s
1
)
1
.
52
x
10
34
m
(This is much, much smaller than the diameter of an atom)
55. When n = 4, l may have the values 0, 1, 2 or 3 (l = 0, 1, 2,...(n -1) ).
If l is 3, ml may be -3, -2, -1, 0, 1, 2 or 3 (ml = -l to +l).
57. The M shell is the n = 3 shell, so there are 3 subshells, s (l = 0), p (l = 1) and d (l = 2). An f
subshell has l =3, so there are 2l +1 = 7 orbitals in an f subshell (ml = -3, -2, -1, 0, 1, 2, 3)
pf2

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CHM 115 E & G Ch. 7

  1. The yellow light whose frequency is doubled would be in the ultraviolet region. The beam whose wavelength is doubled would be in the infrared region.
  2. The absorbed photon must be in the ultraviolet region, while the emitted photon is in the red portion of the visible region. The ground state atom absorbs a photon raising it to a high lying excited state. The atom then loses energy in the form of the red photon falling to a lower lying excited state. If the ground state atom absorbed a red photon, it would be impossible for it to emit an ultraviolet photon.

c

2. 998 x 10^8 m s ^1

1. 365 x 10^6 s ^1

  1. 6 m

56 x 106 km x 103 m 1 km

2. 998 x 108 ms ^1

  1. 9 x 102 s

35. E  h  6. 626 x 10  34 J s x 1. 365 x 106 s ^1  9. 044 x 10  28 J

c  2. 998 x 108 m s ^1

3. 84 x 1014 s ^1

7. 81 x 10 ^7 m  781 nm

This is just at the extreme red end of the visible spectrum.

43. Eph  RH (

n 2 u

n 2 l

) 2. 179 x 10 ^18 J (

) 1. 634 x 10  18 J

 hc

Eph

( 6. 626 x 10  34 J s)( 2. 998 x 108 m s ^1 )

1. 634 x 10  18 J

1. 216 x 10  7 m 121. 6 nm

This wavelength is in the UV portion of the EM spectrum.

h mv

6. 626 x 10  34 J s

( 1. 6749286 x 10  27 kg)( 4. 15 x 103 m s ^1 )

9. 53 x 10 ^11 m 95. 3 pm

remember 1 J 1 kg m 2 s ^2

h mv

6. 626 x 10 ^34 J s

( 0. 145 kg)( 30. 0 m s ^1 )

1. 52 x 10  34 m

(This is much, much smaller than the diameter of an atom)

  1. When n = 4, l may have the values 0, 1, 2 or 3 ( l = 0, 1, 2,...(n -1) ). If l is 3, m l may be -3, -2, -1, 0, 1, 2 or 3 (m l = - l to + l ).
  2. The M shell is the n = 3 shell, so there are 3 subshells, s ( l = 0), p ( l = 1) and d ( l = 2). An f subshell has l =3, so there are 2 l +1 = 7 orbitals in an f subshell (m l = -3, -2, -1, 0, 1, 2, 3)
  1. (a) 6d (b) 5g (c) 4f (d) 6p
  2. (a) m s = +1/2 or -1/2 only. +1 is not a valid value for the m s quantum number. (b) If n = 1, the only permissible value for l is 0. The maximum value for l is n - 1. (c) If l = 2, the only permissible values for m l are -2, -1, 0, 1 and 2. (d) n is restricted to positive integers. n = 0 is not a valid principal quantum number. (e) m s = +1/2 or -1/2 only. +3/2 is not a valid value for the m s quantum number.

67. Emin  h  4. 34 x 10  19 J min 

4. 34 x 10 ^19 J

6. 626 x 10 ^34 J s

6. 55 x 1014 s ^1

71. Eph  RH (

n (^) u^2

n (^) l^2

)   2. 179 x 10 ^18 J (

)  4. 576 x 10  19 J

hc

Eph 

( 6. 626 x 10  34 J s)( 2. 998 x 108 m s ^1 )

4. 576 x 10  19 J

4. 341 x 10  7 m  434. 1 nm

75. Eph  Z 2 RH (

n 2 u

n 2 l

)   22 x 2. 179 x 10 ^18 J (

)  1. 211 x 10 ^18 J

hc

Eph 

( 6. 626 x 10  34 J s)( 2. 998 x 108 m s ^1 )

1. 211 x 10  18 J

1. 640 x 10  7 m  164. 0 nm

This occurs in the ultraviolet region of the spectrum.

  1. (a) 3d 5 orbitals (b) 4f 7 orbitals (c) 4p 3 orbitals (d) 5s 1 orbital

83. Eph  239 kJ mol ^1 x

1000 J

1 kJ x 1 mol

  1. 022 x 1023

^3.^97 x^10 

19 J

hc

Eph 

( 6. 626 x 10  34 J s)( 2. 998 x 108 m s ^1 )

3. 97 x 10 ^19 J

5. 00 x 10 ^7 m  500. nm

87. Eph 

hc

( 6. 626 x 10 ^34 J s)( 2. 998 x 108 m s ^1 )

4. 25 x 10 ^7 m

4. 67 x 10 ^19 J

Ee 

mv 2 

( 9. 109 x 10 ^31 kg) x ( 4. 88 x 105

m s

)^2  1. 08 x 10 ^19 J

Ee  Eph  w where w  the energy required to remove the e 

w  Eph  Ee  4. 67 x 10 ^19 J  1. 08 x 10 ^19 J  3. 59 x 10  19 J

3. 59 x 10 ^19 J x

  1. 022 x 1023 1 mol x 1 kJ

1000 J 

216 kJ mol ^1