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Inorganic > Atom Structures And Orbitals > Flashcards

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

A

Increases

22
Q

Destructive wave effect on probability of finding electron in region

A

Decreases

23
Q

Larger n means

A

Higher energy orbital

24
Q

Lower n means

A

More compact orbital

25
Q

All orbitals with a given n value are

A

In the same shell

26
Q

Orbitals with the same l value

A

Same subshell

27
Q

What does ml do

A

Distinguishes the individual orbitals

28
Q

Anticlockwise ms

A

+ 1/2

29
Q

Clockwise ms

A
  • 1/2
30
Q

Radial nodes occur when

A

Radial component passes through zero

31
Q

Number of type of node — with energy

A

Increases

32
Q

Calculate number of radial nodes

A

N - l - 1

33
Q

Radial nodes in 2s

A

1

34
Q

Radial nodes in 2p

A

None

35
Q

For any series of the same type of orbital, 1st has —- nodes, 2nd has —- etc

A

None, 1

36
Q

Orbital with quantum number of l has what number of nodal planes

A

L number

37
Q

Bohr radius

A

0.529 amps

38
Q

Why was Bohr abandoned

A

Only works on hydrogen and electrons are not discrete particles

39
Q

Wave functions can mean either electron is — OR electron is —

A

A discrete particle with relative probability of one point OR smeared distribution of negative charge with variations in density

40
Q

Electrons will enter different orbitals for how long

A

As long as possible

41
Q

2 electrons occupying different orbitals have

A

Parallel spins

42
Q

Parallel spin means

A

Same direction

43
Q

Most stable configuration has the largest number of unpaired electron spins

A

Hunds rule

44
Q

Paramagnetic

A

1+ unpaired electrons so molecule is attracted to magnetic field

45
Q

Diamagnetic

A

No unpaired electrons so there is weak repelling by magnetic field

46
Q

Why measure magnetism

A

Bc it allows us to detect presence and number of unpaired electrons

47
Q

Electronegativity determined by

A

Tendency of atoms to bind extra electrons and hold what it already has.

48
Q

The ability to attract electrons from bonded neighbors

A

Electronegativity

49
Q

Binding requires a

A

Net positive overlap of atomic orbitals

Inorganic (16 decks)

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