Atom Structures And Orbitals Flashcards

1
Q

How do electrons move according to Bohr

A

In circles around the nucleus

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2
Q

Impossible to know both momentum and position at the same instant

A

Heisenberg’s uncertainty principle

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3
Q

In Bohr we are only able to describe…

A

Precise orbit of electron

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4
Q

Wave functions must be

A

Single valued

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5
Q

First derivatives must be

A

Continuous

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6
Q

Wave functions must approach — as r approaches —

A

0; infinity

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7
Q

Responsible for determining the overall energy of an atomic orbital

A

Quantum number n

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8
Q

Determines angular momentum and orbital shape

A

QN L

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9
Q

Determines orientation of angular momentum vector in a magnetic field or position of an orbital in space

A

QN ml

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10
Q

Determines orientation of electron magnetic moment and describes electron spin within orbital

A

Quantum number ms

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11
Q

A nodal surface is a space with…

A

No electron density

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12
Q

Build up of electrons in atom results from continuously increasing quantum numbers

A

Aufbau

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13
Q

Requires that each electron in atom have unique set of quantum numbers

A

Pauli exclusion

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14
Q

Electrons must be placed in orbitals to give max total possible spin

A

Hunds

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15
Q

Have the same energy

A

Degenerate orbitals

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16
Q

Lyman part of spectrum

A

UV

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17
Q

Balmer part of spectrum

A

VIS

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18
Q

Paschen part of spectrum

A

IR

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19
Q

Bohr’s two postulates

A

Stationary states exist in which energy of electron is constant and characterized by circular orbit around nucleus. Energy of absorbs or emits only when electron moves states

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20
Q

Region of space defined by wave function

A

Atomic orbital

21
Q

Constructive wave effect on probability of finding electron in the region

22
Q

Destructive wave effect on probability of finding electron in region

23
Q

Larger n means

A

Higher energy orbital

24
Q

Lower n means

A

More compact orbital

25
All orbitals with a given n value are
In the same shell
26
Orbitals with the same l value
Same subshell
27
What does ml do
Distinguishes the individual orbitals
28
Anticlockwise ms
+ 1/2
29
Clockwise ms
- 1/2
30
Radial nodes occur when
Radial component passes through zero
31
Number of type of node — with energy
Increases
32
Calculate number of radial nodes
N - l - 1
33
Radial nodes in 2s
1
34
Radial nodes in 2p
None
35
For any series of the same type of orbital, 1st has —- nodes, 2nd has —- etc
None, 1
36
Orbital with quantum number of l has what number of nodal planes
L number
37
Bohr radius
0.529 amps
38
Why was Bohr abandoned
Only works on hydrogen and electrons are not discrete particles
39
Wave functions can mean either electron is — OR electron is —
A discrete particle with relative probability of one point OR smeared distribution of negative charge with variations in density
40
Electrons will enter different orbitals for how long
As long as possible
41
2 electrons occupying different orbitals have
Parallel spins
42
Parallel spin means
Same direction
43
Most stable configuration has the largest number of unpaired electron spins
Hunds rule
44
Paramagnetic
1+ unpaired electrons so molecule is attracted to magnetic field
45
Diamagnetic
No unpaired electrons so there is weak repelling by magnetic field
46
Why measure magnetism
Bc it allows us to detect presence and number of unpaired electrons
47
Electronegativity determined by
Tendency of atoms to bind extra electrons and hold what it already has.
48
The ability to attract electrons from bonded neighbors
Electronegativity
49
Binding requires a
Net positive overlap of atomic orbitals