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Inorganic > 1A Atomic Structure > Flashcards

1A Atomic Structure Flashcards

1
Q

Berzelius In vs Org

A

Vitalism: life/organs needed to make organics

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2
Q

Who proved vitalism wrong

A

Wohler

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3
Q

Who made atom theory

A

Dalton

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4
Q

An atom consists of

A

One nucleus surrounded by an electron cloud

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5
Q

What determines the size/radius of an atom

A

Electron cloud

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6
Q

Role of the nucleus

A

Accommodate nucleons and determine weight

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7
Q

Electron mass in Coulumbs

A

1.602e-19 C

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8
Q

Mass of proton

A

1.673e-27 kg

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9
Q

Mass number

A

Protons + neutrons

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10
Q

Atomic number

A

Number of protons

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11
Q

What is an isotope

A

Nuclei with equal Z (atomic numbers)

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12
Q

What is an isobar

A

Nuclei with equal mass numbers (A)

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13
Q

What is an isotone

A

Nuclei with equal A - Z (mass - atomic)

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14
Q

What happens if there is high binding energy between nucleons

A

Significant mass defect

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15
Q

What is an electron to the Bohr model

A

Particles

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16
Q

What is an electron to the orbital models

A

Waves

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17
Q

Maximum occupancy in a shell for Bohr

A

2n^2 where n = 1 (K), 2 (L) etc

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18
Q

Bohr: Energy of electron depends on

A

Shell

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19
Q

Lyman series range

A

122 nm to 94 nm

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20
Q

Balmer series range

A

656 nm to 410 nm

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21
Q

Paschen series range

A

1875 nm to 1094 nm

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22
Q

Bohr: n is the…

A

She’ll number

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23
Q

What does the electron do in bohr

A

Circles in shells (orbits) around nucleus

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24
Q

Bohr: Can electrons exist between shells

A

Nope because they have discrete energy values

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25
Q

Bohr: Is it harder to remove an electron from K or L

A

4x harder to remove from K

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26
Q

Bohr: n can be interpreted as

A

Principal quantum number

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27
Q

Problems with the Bohr model

A
  1. Violates classic theories of electromagnetism
  2. Violates Heisenberg uncertainty principle
  3. Predictions for multi-e species wrong
  4. Struggles to explain relative emission intensities
  5. Fail to explain fine structure in spectral lines
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28
Q

Bohr: what happens to elements other than H

A

Splitting of lines in emission spectrum (fine structure)

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29
Q

Describe fine structure of alkali metal emission lines

A

Space, Principal, Diffuse, or Fundamental

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30
Q

De broglie said about electrons…

A

Each moving particle possess a wave character

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31
Q

Schrödinger came up with the

A

Wave function of a quantum mechanical system

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32
Q

Probability of density of finding a system in a given state when measured is proportional to

A

square of amplitude of the systems wave function at that state

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33
Q

Principal quantum number

A

N = 1, 2, 3…

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34
Q

Azimuthal quantum number

A

L = 0, … n- 1

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35
Q

Magnetic quantum number

A

Ml = -l, …, + l

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36
Q

Radial nodes in ns orbital

A

N - 1

37
Q

Radial nodes in np orbital

A

N - 2

38
Q

Radial nodes in nd orbitals

A

N - 3

39
Q

Radial nodes in nf orbitals

A

N - 4

40
Q

Abbreviation for angular nodes / nodal planes

A

l (that’s a lowercase L)

41
Q

No nodal plane

A

S orbital, l = 0

42
Q

One nodal plane

A

P orbital, l = 1

43
Q

Two nodal planes

A

D orbital, l = 2

44
Q

Three nodal planes

A

F orbital, l = 3

45
Q

Orbital: n =

A

Main energy level (aka shell)

46
Q

Orbital: azithmul l =

A

Subshell, shape

47
Q

Orbital: m =

A

Orbital orientation (2px etc)

48
Q

azithmul l values for each orbital

A

S is 0, P is 1, d is 2, f is 3

49
Q

Energy of every system is determined by

A

Net interaction

50
Q

Only attractive interaction btwn hydrogenic systems vs many e systems

A

Electron to nucleus: electrostatic attraction

51
Q

Electrostatic attraction

A

Electron to nucleus

52
Q

Electrostatic repulsion

A

Electron to electron

53
Q

Spin coupling

A

Two electrons in same orbital

54
Q

Is spin coupling attractive or repulsive

A

Attractive

55
Q

What’s wrong with the Schrödinger equation

A

Too complex for many electron systems so the only approximations are for non hydrogenic species

56
Q

Aufbau principle

A

Predict lowest energetic state (ground) of multi e systems

57
Q

Pauli exclusion principle

A

Two or more electrons cannot occupy same quantum state

58
Q

What is the point of magnetic spin quantum number

A

Differentiate between two electrons in the same orbital

59
Q

Ms =

A

-1/2, +1/2

60
Q

Madelung-Klechkovsky Rules

A
  1. Lowest n+l first
  2. For equal n+l, lowest n first
  3. Works only for atoms, not ions
61
Q

If n > 1

A

Multiple l values for the same shell; sub shells

62
Q

If l > 0

A

Multiple ml values for the same subshell, causing different orientations

63
Q

Degenerate subshell means the ml states are

A

Energetically equal

64
Q

Hunds rule

A

Every orbital in a sublevel is singly occupied before any orbital is doubly occupied

65
Q

Effects of hunds rule

A

Minimize spin coupling per subshell. Every degenerate ml must be filled with one electron before adding a second to any single occupied ml

66
Q

Slaters rule

A
  1. Inner electrons (lower n or lower) partially shield the attractive force of the nucleus from outer electrons (higher n or l)
  2. The effective nuclear charge Zeff experienced by outer electrons is lower than the absolute nuclear charge Z
  3. The semi empirical values for the shielding constant s are derived from electron excitation and ionization experiments
67
Q

Slaters rule equation

A

Zeff = Z - s

68
Q

Slaters rules for electrons in ns or np

A
  1. Each other ns or np electron shields 0.35 except for 1s which contribute 0.30
  2. Each electron in penultimate (n-1) shell shields. 0.85
  3. Each electron in lower shells shields 1
69
Q

Slaters rules for nd or nf

A
  1. Each other nd or nf electron shields 0.35
  2. Each electron in lower subshells shields
70
Q

azithmal number for s

A

0

71
Q

azithmal for p

A

1

72
Q

azithmal for d

A

2

73
Q

azithmal for f

A

3

74
Q

angular nodes =

A

azithmal number l

75
Q

radial nodes in 4f

A

0

76
Q

angular nodes in 5d

A

2

77
Q

mass of an electron

A

9.109e-31 kg

78
Q

speed of light

A

3e8 m/s

79
Q

planck’s constant

A

6.626 e-34 Js

80
Q

R in J/molK

A

8.314

81
Q

R in Latm/molK

A

0.08206

82
Q

Joules can also be written as

A

kgm2 / s2

83
Q

kilo

A

10^3

84
Q

deci

A

10^-1

85
Q

centi

A

10^-2

86
Q

milli

A

10^-3

87
Q

micro

A

10^-6

88
Q

nano

A

10^-9

89
Q

pico

A

10^-12

Inorganic (16 decks)

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