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Chemistry > 1.5 & 1.6: Electronic Configuration Of Atom > Flashcards

1.5 & 1.6: Electronic Configuration Of Atom Flashcards

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1
Q

What are the 2 important concepts of the Quantum Theory?

A
  1. Electrons can be described as waves by the Schrondinger equation
  2. Uncertainty principle
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2
Q

What is the Schrondiger equation?

A

An equation that describes an electron’s properties in terms of quantum numbers

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3
Q

What is the uncertainty principle?

A

The idea that both the exact location and velocity of a subatomic particle can never be known at the same time

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4
Q

What are the 3 observations that quantum theory shows and classical mechanisms can’t?

A
  1. Spectra of light emitted by atoms
  2. Stability of atoms
  3. Wave-particle duality
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5
Q

What does measuring the energy of a photon allow us to determine?

A

The energy difference between levels - this indicates energy levels are not equally spaced

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6
Q

What is ionisation energy?

A

The measure of the amount of energy needed to remove electrons from atoms/ions

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7
Q

Define ‘First Ionisation Energy’

A

The amount of energy required to remove one mole of electrons from one mole of gaseous atoms to form one mole of gaseous positive ions

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8
Q

What gives us evidence for the arrangement of electrons within an atom?

A

Patterns in ionisation energies

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9
Q

What is electron affinity?

A

The amount of energy needed to add electrons to atoms/ions

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10
Q

Define ‘First Electron Affinity’

A

The amount of energy required to add one mole of electrons to one mole of gaseous atoms to form one mole of gaseous negatively charged ions

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11
Q

Why are first electron affinities always negative?

A

Energy is released on addition of the electron

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12
Q

What shows the stability of a negative ion?

A

Electron affinity - the more negative = more stable ion formed

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13
Q

What is the trend in Atomic size:
1. Down a group
2. Across a period

A

Atomic size increases down a group

Atomic size decreases across a period

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13
Q

What is the trend in first ionisation energy:
1. Down a group
2. Across a period

A

First ionisation energy decreases down a group

First ionisation energy increases across a period

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14
Q

What is the trend in Atomic size:
1.

A
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14
Q

What is the trend in Atomic size:
1.

A
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15
Q

What is the trend in First electron affinity:
1. Down a group
2. Across a period

A

First electron affinity becomes less negative down a group - less stable ion

First electron affinity becomes more negative across a period - more stable ion

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16
Q

What is an orbital?

A

A region in space where there is a given (usually 95%) probability of finding a particular electron

Cannot specify the exact position of an electron in an atom

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17
Q

What are quantum numbers?

A

The various energy levels available within an atom in which electrons can reside

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18
Q

What 3 things do quantum numbers show?

A
  1. The position of an electron in an atom
  2. The direction of spin of the electron
  3. The energy and angular momentum of an electron
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19
Q

What are the 4 quantum numbers required to specify the character of an atom?

A
  1. Principle Quantum Numbers (n)
  2. Azimuthal or subsidiary Quantum Numbers (l)
  3. Magnetic Quantum Numbers (m)
  4. Spin Quantum Numbers (s)
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20
Q

What do principle energy levels/ shells correspond to?

A

The Principle Quantum Number (n)

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21
Q

What are Principle Quantum Numbers traditionally referred to?

A

Letters K, L, M …..

Where the K shell n =1
L shell n =2 etc

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22
Q

What happens to energy levels in complex atoms when n increases?

A

They get closer

23
Q

What do Principle Quantum Numbers (n) indicate?

A
  1. Distance of electrons from nucleus
  2. Energy of electron
  3. Number of electrons a shell can hold : 2n²
24
Q

What is the formula used to determine how many electrons a shell can hold?

A

2n²

25
Q

What is a subshell?

A

A group of orbitals with the same energy

26
Q

What are subshells described by?

A

The azimuthal or subsidiary quantum number (l)

27
Q

What range of values is l always between?

A

0 to n-1

28
Q

What letters do the azimuthal or subsidiary quantum numbers correspond to?

A

Letters s, p ,d, f ……

29
Q

What 4 things do azimuthal quantum numbers indicate?

A
  1. Which subshell an electron is in
  2. Energy of the subshell
  3. Shape of the orbitals in the subshell
  4. Maximum number of electrons a subshell can hold
30
Q

How can the maximum number of electrons a subshell can hold be worked out?

A

By equation: 2(2l+1)

Eg. l for d-subshell = 2
Therefore, the number of electrons it can hold = 2(4+1)=10

31
Q

What shape is an s-orbital (l=0)?

A

Spherical

32
Q

What

A
33
Q

What shape is a p-orbital (l=1)?

A

Dumbbell

34
Q

What shape is a d-orbital (l=2)?

A

More complex

35
Q

What shape is a f-orbital (l=3)?

A

Still more complex

36
Q

What can the combination of n and l be used for?

A

To identify a particular subshell and thus describe the location of an electron in the atomic energy level

37
Q

What do Magnetic Quantum Numbers (m) represent?

A

The orbitals in a given subshell

38
Q

What do Magnetic Quantum Numbers (m) indicate and don’t indicate?

A

Indicate the direction of a particular orbital relative to the magnetic field/axis
Don’t indicate energy

39
Q

‘m’ can have integral value ranging from –l through 0 to +l. Therefore,
for a given value of l, total number of m value is (2l+1)????????

A

LEARN THIS

40
Q

What does the Spin Quantum Number (s) describe?

A

How an electron, moving around the nucleus, spins about
its own axis (self rotation) either in a clockwise or
anticlockwise direction

(also described as spin up and spin
down)

41
Q

What are the two possible spin quantum values?

A

+1/2 (clockwise spinning)
-1/2
(anticlockwise spinning)

42
Q

What do clockwise and anti-clockwise spinning
electrons produce?

A

Opposite magnetic fields

43
Q

What is AUFBAU PRINCIPLE?

A

Electrons enter the lowest available energy level first

44
Q

What is MADELUNG’S RULE?

A

The energy of an atomic orbital increases with increasing n+l. For
identical values of n+l, energy increases with increasing n

45
Q

What is HUND’S RULE OF MAXIMUM MULTIPLICITY?

A

When in orbitals of equal energy, electrons will try to remain unpaired.

46
Q

What is PAULI EXCLUSION PRINCIPLE?

A

No two electrons can have the same four quantum numbers.
Only two electrons can go in each orbital, providing they are of opposite
spin.

47
Q

PAGE 21

A

Look over

48
Q

MEMORISE PAGE 23

A
49
Q

What are the electronic configurations of Cr and Cu?

A

Cr Z = 24 1s2 2s2 2p6 3s2 3p6 4s1 3d5
Cu Z = 29 1s2 2s2 2p6 3s2 3p6 4s1 3d10

50
Q

How are anions (negative ions) formed?

A

By adding electrons to atoms

51
Q

How are cations (positive ions) formed?

A

By removing electrons from atoms

52
Q

Where is an electron removed from first and what is an exception to this rule?

A

The highest occupied orbitals

Transition metals lose s electrons first

53
Q

What does a large jump between successive ionisation energy indicate

A

A change in energy level from which the electron has been removed.

54
Q

What does Diamagntic mean?

A

There are no unpaired electrons - slightly repelled by magnetic field

55
Q

What does Paramagnetic mean?

A

There is at least 1 unpaired electron

Spins align to external magnetic fields

56
Q

Give an example of a contrast agent used in medical imaging ?

A

GD3+ (commonly used - 7 unpaired electrons)
Used in MRI scanning image enhancement

Chemistry (13 decks)

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