Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

Inorganic > 1A Atomic Structure > Flashcards

1A Atomic Structure Flashcards

1
Q

Berzelius In vs Org

A

Vitalism: life/organs needed to make organics

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

Who proved vitalism wrong

A

Wohler

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

Who made atom theory

A

Dalton

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

An atom consists of

A

One nucleus surrounded by an electron cloud

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

What determines the size/radius of an atom

A

Electron cloud

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

Role of the nucleus

A

Accommodate nucleons and determine weight

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

Electron mass

A

1.602e-19 C

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

Mass of proton

A

1.673e-27 kg

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

Mass number

A

Protons + neutrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

Atomic number

A

Number of protons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

What is an isotope

A

Nuclei with equal Z (atomic numbers)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

What is an isobar

A

Nuclei with equal mass numbers (A)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

What is an isotone

A

Nuclei with equal A - Z (mass - atomic)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

What happens if there is high binding energy between nucleons

A

Significant mass defect

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

What is an electron to the Bohr model

A

Particles

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

What is an electron to the orbital models

A

Waves

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

Maximum occupancy in a shell for Bohr

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

Bohr: Energy of electron depends on

A

Shell

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

Lyman series range

A

122 nm to 94 nm

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

Balmer series range

A

656 nm to 410 nm

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

Paschen series range

A

1875 nm to 1094 nm

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

Bohr: n is the…

A

She’ll number

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

What does the electron do in bohr

A

Circles in shells (orbits) around nucleus

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

Bohr: Can electrons exist between shells

A

Nope because they have discrete energy values

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Q

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

A

4x harder to remove from K

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
26
Q

Bohr: n can be interpreted as

A

Principal quantum number

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
28
Q

Bohr: what happens to elements other than H

A

Splitting of lines in emission spectrum (fine structure)

29
Q

Describe fine structure of alkali metal emission lines

A

Space, Principal, Diffuse, or Fundamental

30
Q

De broglie said about electrons…

A

Each moving particle possess a wave character

31
Q

Schrödinger came up with the

A

Wave function of a quantum mechanical system

32
Q

Probability of density of finding a system in a given state when measured…

A

Is proportional to square of amplitude of the systems wave function at that state

33
Q

Principal quantum number

A

N = 1, 2, 3…

34
Q

Azimuthal quantum number

A

L = 0, … n- 1

35
Q

Magnetic quantum number

A

Ml = -l, …, + l

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 orbital 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

For equal n and l, the lowest energy state has the highest
Σms bc unpaired e less shielded

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

Inorganic (11 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions