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Honors Chem 1320 > Quantum Test > Flashcards

Quantum Test Flashcards

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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
Q

probability density =

A

[Ψnlm (r,θ,Φ)]^2

▪probability/volume
▪likelihood of locating an electron in a given region of space

26
Q

bohrs radius

A

a sub 0

52.9 pm for 1s

27
Q

RPD

A

radial probability distribution

28
Q

r sub mp

A

distance from the nucleus (r) you will most likely find an electron at

29
Q

Ψnlm(r,θ,Φ)=

A

radial wave function x angular wave function

30
Q

E subn

A

binding energy

31
Q

radial node

A

▪where the radial wave function =0

▪means there is 0 possibility of measuring the particle at that value of r

32
Q

nodal plane

A

arise from angular nodes in the wave function

33
Q

of angular nodes =

A

l

34
Q

angular node

A

where the angukar wave function changes signs

35
Q

number of radial nodes

A

n-l-1

36
Q

total # of nodes =

A

n-1

37
Q

l=2 mℓ=0

A

dz^2

38
Q

radial wave function (R)

A

probability of finding an electron at some distance from the nucleus and its energy

39
Q

angular wave function (Y)

A

sets an orientation of the orbital in 3d space

40
Q

energy of the electron increases as the distance from the nucleus ______

A

increases

41
Q

shading depicts what?

A

different signs of the wave function

42
Q

magnetic spin

A

ms

43
Q

ms =

A

+ 1/2 (up) or -1/2 (down)

44
Q

ms describes

A

electron, not orbital

45
Q

Ψ(nl)mℓ(ms) describes

A

electron

46
Q

how many p orbitals

A

e

47
Q

how many d orbitals

A

5

48
Q

how many s orbitals

A

1

49
Q

how many quantum numbers define an electron

A

4

50
Q

pauli exclusion principle

A

▪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
Q

as n increases the probability of finding an electron moves

A

farther away from the nucleus

52
Q

energy of an electron in the hydrogen atom is determined by

A

n

53
Q

energy of an electron in a mulrielectron system depends on

A

n and l

54
Q

max # of electrons that can occupy an energy level descrubed by n is

A

2n^2

55
Q

of f orbitals

A

7

56
Q

wavelength associated with a moving particle

A

debroglie wavelength

57
Q

degenerate orbitals

A

have the sams amount if energy

58
Q

electron configuration

A

the arrangement of electeons in the orbitals of an atom

Honors Chem 1320 (8 decks)

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