Quantum Test Flashcards

1
Q

for emission the change in energy =

A

initial energy - final energy

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2
Q

large change in energy = _____ frequency and _______ wavelength

A

high frequency

short wavelength

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3
Q

small change in energy = ______ frequency and ______ wavelength

A

low frequency

high wavelength

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4
Q

in the balmer series n final =

A

2

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5
Q

balmer series color emitted when n initial=6

A

purple

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6
Q

balmer series color emitted when n initial =5

A

blue

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7
Q

balmer series color emitted when n initial =4

A

green

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8
Q

balmer series color emitted when n initial =3

A

red

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9
Q

principle quantum #

A

n

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10
Q

n determines

A

binding energy/shell

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11
Q

n =

A

1,2,3,…

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12
Q

angular momentum

A

l

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13
Q

l describes the

A

subshell/shape of the orbital

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14
Q

l =

A

0,1,2,3, … n-1

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15
Q

magnetic quantum #

A

mℓ

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16
Q

mℓ determines

A

behavior in the magnetic field, the specific orbital and orientation

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17
Q

mℓ =

A

-l, …. 0 … +l

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18
Q

what orbital when l = 0

A

s orbital

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19
Q

what orbital when l = 1

A

p orbital

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20
Q

what orbital when l = 2

A

d orbital

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21
Q

what orbital when l = 3

A

f orbital

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22
Q

when mℓ = -1 or 1 it is

A

x or y

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23
Q

when mℓ =0 it is

A

z

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24
Q

physical interpretation of a wave function

A

the probabbility of a finding an electron in a defined region is proportional to the square of the wave function

25
probability density =
[Ψnlm (r,θ,Φ)]^2 ▪probability/volume ▪likelihood of locating an electron in a given region of space
26
bohrs radius
a sub 0 | 52.9 pm for 1s
27
RPD
radial probability distribution
28
r sub mp
distance from the nucleus (r) you will most likely find an electron at
29
Ψnlm(r,θ,Φ)=
radial wave function x angular wave function
30
E subn
binding energy
31
radial node
▪where the radial wave function =0 | ▪means there is 0 possibility of measuring the particle at that value of r
32
nodal plane
arise from angular nodes in the wave function
33
of angular nodes =
l
34
angular node
where the angukar wave function changes signs
35
number of radial nodes
n-l-1
36
total # of nodes =
n-1
37
l=2 mℓ=0
dz^2
38
radial wave function (R)
probability of finding an electron at some distance from the nucleus and its energy
39
angular wave function (Y)
sets an orientation of the orbital in 3d space
40
energy of the electron increases as the distance from the nucleus ______
increases
41
shading depicts what?
different signs of the wave function
42
magnetic spin
ms
43
ms =
+ 1/2 (up) or -1/2 (down)
44
ms describes
electron, not orbital
45
Ψ(nl)mℓ(ms) describes
electron
46
how many p orbitals
e
47
how many d orbitals
5
48
how many s orbitals
1
49
how many quantum numbers define an electron
4
50
pauli exclusion principle
▪no 2 electrons can be in the same orbital and have the same spin ▪no 2 electrons in the same atom can have the samr 4 quantum numbers
51
as n increases the probability of finding an electron moves
farther away from the nucleus
52
energy of an electron in the hydrogen atom is determined by
n
53
energy of an electron in a mulrielectron system depends on
n and l
54
max # of electrons that can occupy an energy level descrubed by n is
2n^2
55
of f orbitals
7
56
wavelength associated with a moving particle
debroglie wavelength
57
degenerate orbitals
have the sams amount if energy
58
electron configuration
the arrangement of electeons in the orbitals of an atom