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AH Chemistry > 1.2 Atomic Orbitals, Electronic Configurations and the Periodc Table > Flashcards

1.2 Atomic Orbitals, Electronic Configurations and the Periodc Table Flashcards

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1
Q

What provide evidence of energy levels

A

Spectral lines

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2
Q

Quantum theory

A

Energy is emitted or absorbed in fixed amounts called quanta

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3
Q

Energy is emitted or absorbed in fixed amounts called quanta

A

Quantum theory

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4
Q

Atomic orbital

A

A region of high probability of finding electrons

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5
Q

A region of high probability of finding electrons

A

Atomic orbital

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6
Q

How many electrons can an orbital hold

A

2

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7
Q

3 p orbitals holds ___ electrons

A

6

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8
Q

5 d orbitals holds ___ electrons

A

10

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9
Q

The 1s orbital has _____ as the 2s orbital

A

Same shape

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10
Q

1 s orbital is smaller/larger and has a lower/higher energy than the 2s orbital

A

Smaller

Lower

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11
Q

Principle quantum number symbol

A

n

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12
Q

Principle quantum number defines..

A

Size and energy of shell

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13
Q

Principle quantum number typical values

A

1, 2, 3, 4

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14
Q

What quantum number had the symbol n

A

Principle quantum number

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15
Q

What quantum number defines the size and energy of shell

A

Principle quantum number

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16
Q

What quantum number had the values 1 2 3 4

A

Principle quantum number

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17
Q

Angular momentum quantum number symbol

A

l

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18
Q

Angular momentum quantum number defines

A

Shapes of sub shell

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19
Q

Angular momentum quantum number typical values

A

0 1 2 3

or

s p d f

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20
Q

What quantum number has the symbol l

A

angular momentum quantum number

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21
Q

What quantum number defines the shape of sub shell

A

angular momentum quantum number

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22
Q

What quantum number has the values 0 1 2 3 or s p d f

A

Angular momentum quantum number

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23
Q

Magnetic quantum number symbol

A

ml

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24
Q

Magnetic quantum number defines

A

Direction

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25
Q

Magnetic quantum number typical values

A

-2 -1 0 +1 +2

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26
Q

What quantum number had the symbol ml

A

Magnetic quantum number

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27
Q

What quantum number defines direction

A

Magnetic quantum number

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28
Q

What quantum number had the values -2 -1 0 +1 +2

A

Magnetic quantum number

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29
Q

Spin magnetic quantum number

A

ms

30
Q

Spin magnetic quantum number defines

A

Spin

31
Q

Spin magnetic quantum number typical values

A

-1/2 or +1/2

32
Q

What quantum number has the symbol ms

A

Magnetic quantum number

33
Q

What quantum number defines spin

A

Spin magnetic quantum number

34
Q

What quantum number has the symbol values -1/2 or +1/2

A

Spin magnetic quantum number

35
Q

Aufbau rule

A

Electrons occupy orbitals in order of increasing energy, eg the lowest energy orbital is filled first

36
Q

Electrons occupy orbitals in order of increasing energy, eg the lowest energy orbital is filled first

A

Aufbau rule

37
Q

Hunds rule

A

degenerate (equal energy) orbitals are occupied singularly before pairing

38
Q

degenerate (equal energy) orbitals are occupied singularly before pairing

A

Hunds rule

39
Q

Pauli exclusion principle

A

No two electrons can have the same 4 quantum numbers and if there are 2 electrons, their spin must be opposite

40
Q

No two electrons can have the same 4 quantum numbers and if there are 2 electrons, their spin must be opposite

A

Pauli exclusion principle

41
Q

Order of how orbitals fill

A

1s
2s
2p
3s
3p
4s
3d
4p

42
Q

when am element becomes an ion, what electrons are lost first

A

Electrons from the 4s orbital

43
Q

What elements are exceptions to the aufbau rule

A

Chromium and copper

44
Q

Why are chromium and copper exempt from the aufbau rule

A

They prefer half filled electrons

45
Q

Ionisation energy

A

When one mole of electrons is removed from one mole of atoms in their gaseous state

46
Q

When one mole of electrons is removed from one mole of atoms in their gaseous state

A

Ionisation energy

47
Q

Nuclear charge

A

An increase in the number of protons means there is a stronger attraction for electrons, so it requires more energy to remove

48
Q

An increase in the number of protons means there is a stronger attraction for electrons, so it requires more energy to remove

A

Nuclear charge

49
Q

Atomic size

A

The further away the electrons, the less attraction they have to the nucleus, so require less energy to remove

50
Q

Shielding

A

The inner electrons cancel out the increased nuclear charge, decreasing ionisation energy

51
Q

The inner electrons cancel out the increased nuclear charge, decreasing ionisation energy

A

Shielding effect

52
Q

What do copper and chromium file before the 4s orbital

A

The d orbitals

53
Q

Isoelectronic atoms

A

When particles have the same electron configuration

54
Q

When particles have the same electron configuration

A

Isoelectronic

55
Q

calculation for quantum number l

A

0 … n-1

eg, if n=2, l = 0

56
Q

calculation for quantum number ml

A

-l … 0 … +l

(l is letter L)

eg, if l=2, ml= -2, -1, 0, +1

57
Q

shape of orbital if l = 0

A

s

58
Q

shape of orbital if l = 1

A

p

59
Q

shape of orbital if l = 2

A

d

60
Q

shape of orbital if l = 3

A

f

61
Q

shape of s orbital

A
62
Q

shape of d orbital

A
63
Q

f orbital shape

A
64
Q

p orbital shape

A
65
Q

properties of half filled orbitals

A

have an unexpected stability that is preferable

66
Q

TMs with interesting electron configurations

A

chromium and copper

  • > half filled orbitals have an unexpected stability
67
Q

where are electrons removed from when ionising TMs

A

4s

68
Q

in empty orbitals, 3d has ____ energy than 4s of transition metals

A

more

69
Q

in filled orbitals, 3d has ____ energy than 4s of transition metals

A

less

70
Q

No of outer electrons….

A

No of group

71
Q

Ion electron configurations

A

Electrons removed from 4s before d orbitals

AH Chemistry (4 decks)

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