Lecture 2 Atomic Theory II Tutorial - AP...
Transcript of Lecture 2 Atomic Theory II Tutorial - AP...
Lecture 2 Atomic Theory II
Tutorial
1) A photon travels with a frequency of 8.57 x 1014 Hz.
a. Find the wavelength of this photon in nm?
8
1 4 1
7
2
3 1 0 m /s8.5 7 10 s3 .5 0 1 0 m3 .5 0 1 0 n m
ccλ ν
λν
λ
λ
λ
−
−
=
=
×=
×= ×
= ×
b. Find the energy contained by a single photon. Put your answer in kJ.
34 14 1
19
16
= = (6.63x10 Js) (8.57 x 10 s ) = 5.68 x 10 J = 5.68 x 10 kJ
E hEEE
ν− −
−
−
2) An electron drops from n = 5 to n = 3 in a hydrogen atom.
a. Find the energy contained by the photon that is released during this transition.
18
5 2
205
2.178 10 J5
8.712 10 J
E
E
−
−
− ×=
= − ×
18
3 2
193
2.178 10 J3
2.420 10 J
E
E
−
−
− ×=
= − ×
3 5
19 20
19
=
= 2.420 10 J ( 8.712 10 J)= 1.549 10 J
E E E
EE
− −
−
Δ −
Δ − × − − ×
Δ − ×
b. Find the frequency of the electromagnetic radiation that is released.
1914 1
34
1.549 10 J 2.34 10E s
6.63 10 Js
E h
h
ν
ν−
−−
×= = = ×
=
×
c. At what speed does this electromagnetic radiation travel?
(3x108 m/s) The speed of electromagnetic waves (light) is a constant.
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d. What is the wavelength of this electromagnetic radiation?
8
1 4 1
6
3
3 .0 0 1 0 m /s2 .3 4 1 0 s
1 .2 8 1 0 m1 .2 8 1 0 n m
ccλ ν
λν
=
=
λ
λ
λ
−
−
×=
×= ×
×
=
3) An electron is traveling with a velocity of 3.92 x 106 m/s. (mass e- = 9.11 x 10-31 kg)
a. What is its wavelength in nm?
347 2
34
6.63 10 Js 1.86 10 m 1.86 10 nm(9.11 10 kg)(3.92
hmv
λ−
−−
×= = = × = ×
× 6 /s)10 m×
b. What is its frequency?
8
-7
1 5 1
3 1 0 m /s1 .8 6 × 1 0 m1 .6 1 1 0 s
ccλ ν=
=νλ
ν
ν −×
×
=
=
4) Find the momentum of an electron with a wavelength of 232 nm.
3427
9
6.63 10 Js 2.86 10 kg m/s232 10 m
mvh h
mv
ρ
λρ
hρλ
−−
−
=
= = = × ⋅ii
= =
5) How many possible orientations exist in a p-sublevel?
The angular momentum quantum number (l) for a p-sublevel is 1. The magnetic
uantum numbers range from - l to + l . For a p-sublevel the magnetic quantum ientations in the
-sublevel.
qnumbers are -1, 0, and +1. Thus, there are THREE possible orp
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6) What is the lowest principal quantum number that can have p-orbitals?
n-1 = l n = l +1
n = 2
n = 1 + 1
7) If n=5: a. What are the possible angular momentum numbers?
The angular momentum numbers range from 0 to n-1. If n = 5 the possible angular momentum numbers are:
0, 1, 2, 3, and 4.
b. What do these numbers represent? The angular momentum numbers rep r type of orbital. 0 is an s-orbital, is a p-orbital, 2 is a d-orbital, and 3 is an f-orbital.
resent the shape o1
8) If l = 3:
-3, -2, -1, 0, 1, 2, and 3
a. What are the possible magnetic quantum numbers?
These numbers define th e-dimensional space. In this ase, there are seven different orientations (an f-sublevel).
b. What do these numbers represent?
e orientation of the orbital in threc
9) What are the possible angular momentum, magnetic, and electron spin quantum
= 0 (An s-orbital is defined by l = 0) m =ms= + ½
numbers associated with a single electron in the s-orbital of n = 2.
l - l to + l , so m = 0 (there is only one orientation for an s-orbital)
or – ½ (the one electron could be spin up or spin down.)
omentum, magnetic, and electron spin quantum .
= 3 (l = 3 defines an f-orbital) m =for f-orms= + ½ or – ½ (the one electron could be spin up or spin down.)
10) What are the possible angular mnumbers associated with a single electron in an f-orbital of n = 5
l
- l to + l , so m = -3, -2, -1, 0, +1, +2, or +3 (there are seven possible orientations bitals)
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