Exam 2 Lecture 7 Flashcards

1
Q

The deBroglie wavelength of matter The deBroglie wavelength of matte

A

h=6.62607004 × 10-34 m2 kg / s

lower case v is “velocity”

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2
Q

Who is this guy?

What did he discover?

A

Werner Heisenberg

The dual nature of matter (a particle and a wave) places limitations on the preciseness with which we can know both the location and the momentum (mass x velocity) of an object

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3
Q

IF you can Know location precisely,

A

then momentum is uncertain

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4
Q

If you can Know momentum precisely,

A

then location is uncertain

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5
Q

Earth Wavelength

A

miniscule

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6
Q

baseball wavelength

A

moderate

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7
Q

electron wavelength

A

relatively moderate

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8
Q

Who is this guy?

What does he say about electrons?

A

Erwin Schrodinger

The behavior of the electron is better described b y g focusin g on it’s wavelike p p ro perties

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9
Q

An orbit:

A

a defined, known pathway

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10
Q

An orbital:

A

a probability function; “the probability that the probability that an electron will be found in a given location”

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11
Q

An orbital: A description of….

A

the distribution of electron density in space

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12
Q

Orbitals have a characteristic ……

A

shape and energy

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13
Q

What do the dots represent?

A

Each dot represents a position where an electron may be found at any given moment with respect to the nucleus, which is at the center of the axes

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14
Q

Orbitals of a given shape (within a subshell)….

A

have a specific orientation in space

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15
Q

Orbital quantum numbers

A

n, l, ml, ms

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16
Q

n lables…

A
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17
Q

n possible values…

A
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18
Q

n notes

A
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19
Q

n name

A
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20
Q

l name

A
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21
Q

ml​ name

A
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22
Q

ml​ labels….

A
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23
Q

ml​ possible values

A
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24
Q

ml​ notes

A
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25
l labels....
26
l possible values....
27
l notes....
28
ms name
29
ms labels...
30
ms possible values...
31
ms notes...
32
n describes the....
energy of the orbital of the orbital n=1,2,3,4 "shells"
33
l describes the...
3-dimensional shape of the orbital | (subshells)
34
ml describes the
orientation of an orbital in space (values are integers from “- l” to “ + l”)
35
A specific orbital is defined by
specific and unique values for n, l, and ml
36
Quantum numbers for n=1 orbital
37
Quantum numbers for n=2 orbitals
38
sherical
39
Elipsoid
40
2p orbital ml=1 spacial orientation
along the x axis
41
2p orbital ml=0 spacial orientation
along the z axis
42
2p orbital ml=-1 spacial orientation
along the y axis
43
n refers to the ____ of the \_\_\_\_
44
l refers to the ____ of the \_\_\_\_
45
ml refers to the ____ of the \_\_\_\_
46
define node
a point at which a harmonic function has the value zero, especially a point of zero electron density in an orbital.
47
n=3 orbitals quantum numbers
48
Allowed values for l
integers from 0 to n 1
49
•Allowed values for ml
integers from -l to +l
50
How many orbitals are there in n=3?
51
Pears
52
2 pears to one torus
53
shape of s orbital
spherical
54
shape of p orbital
dumbell (elipsoid)
55
shape of d orbitals
pear and toris
56
d orbital spacial orientation
57
What are those?
58
n=4 orbital quantum numbers
59
How many orbitals in n=4?
60
Shapes of f orbitals
Intense
61
62
Subshell names: n=1
63
Subshell names: n=2
64
Subshell names: n=3
65
Subshell names: n=4
66
Subshell names: n=5
67
number of orbitals in s
68
number of orbitals in p
69
number of orbitals in d
70
number of orbitals in f
71
Name Irregular Electron Configurations in periods 4 and 5
Cr, Cu, Mo, Ag 1
72
Explain what is Cr's electron configuration? Why is it different?
migh predict: [Ar]4s23d4 actually: [AR]4s13d5 Cr would rather have a full spin party than a ful s orbital.
73
Explain what is Cu's electron configuration? Why is it different?
migh predict: [Ar]4s23d9 actually: [AR]4s13d10 Cr would rather have a full spin party than a full s orbital.