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IB Chemistry > Structure 1.3 Electron configurations > Flashcards

Structure 1.3 Electron configurations Flashcards

1
Q

What can light be described as?

A

An electromagnetic wave

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2
Q

What is the formula for the energy of an electromagnetic wave?

A

Energy = Planck’s constant x frequency = (Planck’s constant x speed of light) / wavelength

OR
E = hv = (hc) / wavelength

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3
Q

What does a shorter wavelength correspond to?

A

Higher frequency. High energy

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4
Q

What does a longer wavelength correspond to?

A

Less frequency. Less energy

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5
Q

What is frequency?

A

Number of waves that pass a point per second (s^-1)

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6
Q

What is wavelength?

A

The distance between two neighbouring peaks of a wave

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7
Q

What are the wavelengths of radiation that correspond to visible light?

A

380-780nm / 10^-9m

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8
Q

Which region of the electromagnetic spectrum borders on the higher energy side of the visible light region?

A

Ultraviolet borders on blue/violet

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9
Q

Which region of the electromagnetic spectrum borders on the lower energy side of the visible light region?

A

Infrared borders on orange/red

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10
Q

What does sunlight contain in terms of visible light?

A

All wavelengths of visible light

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11
Q

What occurs when sunlight passes through a prism?

A

Different wavelengths are refracted by different amounts, resulting in a rainbow (continuous spectrum of colours)

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12
Q

What happens when other sources of light (not sunlight) pass through a prism?

A

Split into discrete coloured lines with each coloured line = a specific wavelength of light within the visible region

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13
Q

What is the ground state?

A

Electrons are at their lowest energy arrangement (most stable)/closest to the nucleus

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14
Q

Why is light emitted during a flame test?

A

Energy is given to atom in the form of heat. Excited electrons absorb the amount of energy that corresponds to the difference between two energy levels in the atom, thus jumping to a higher energy level. They return to the groundstate by emitting this energy absorbed, in the form of electromagnetic waves. The different frequencies correspond to different colours

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15
Q

What happens to the energy difference between successful energy levels as they get further from the nucleus?

A

The energy difference between successful energy levels decreases as they get further from the nucleus.

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16
Q

What happens when an electron drops to its original orbital?

A

Energy, as a photon of light, will be emitted.

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17
Q

In the hydrogen emission spectrum, what energy level must the drop be to in order to produce visible light?

A

To n = 2.

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18
Q

In the hydrogen emission spectrum, what energy levels corresponds to infared light when dropped to?

A

= to or greater than 3

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19
Q

In the hydrogen emission spectrum, what energy level correspond to ultraviolet light when dropped to?

A

N = 1

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20
Q

What colour of visible light has the most energy?

A

Violet

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21
Q

What colour of visible light has the least energy?

A

Red

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22
Q

What is a photon?

A

Packet of light energy

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23
Q

What is the ionisation energy?

A

Minimum amount of energy requried to remove an electron from an atom in gaseous state

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24
Q

What is the formula for ionisation energy?

A

n = infinity -> n = 1

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25
Q

What is a bigger energy difference: n = 2 -> n = 1 OR n = infinity => n = 2?

A

n =2 -> n =1.
No bigger drop than this

26
Q

What features of an energy level diagram should be included?

A

Converging energy levels
Labeled energy levels
Show what is emitted
arrow for increasing energy

27
Q

What is the formula for maximum number of electrons in each main energy level of an atom?

A

2n^2

28
Q

When do electrons begin to fill the next shell?

A

When the shell is full / has 8 electrons in it

29
Q

What is an atomic orbital?

A

Region in space where there is a high probability that an electron of a specific energy level may be found

30
Q

How can shells be subdivided?

A

Shells -> subshells -> orbitals

31
Q

What is the relationship between the shell number and the number of subshells?

A

They are the same

32
Q

What are the subshell types for shell number 1?

A

S

33
Q

What are the subshell types for shell number 2?

A

s p

34
Q

What are the subshell types for shell number 3?

A

s p d

35
Q

What are the subshell types for shell number 4?

A

s p d f

36
Q

How many electrons can subshell type s hold?

A

2

37
Q

How many electrons can subshell type p hold?

A

6

38
Q

How many electrons can subshell type d hold?

A

10

39
Q

How many electrons can subshell type f hold?

A

14

40
Q

How many orbitals does subshell s have?

A

1 (2 electrons)

41
Q

How many orbitals does subshell p have?

A

3

42
Q

How many orbitals does subshell d have?

A

5

43
Q

How many orbitals does subshell f have?

A

7

44
Q

What is the shape of an s orbital?

A

Spherical shape

45
Q

What is the shape of a p orbital?

A

Dumbell-shaped spaces that align with x/y/z axis

46
Q

What is the relationship between shell number and energy level?

A

Higher shell number = higher energy

47
Q

Do all subshells have the same energy?

A

Similar.
S < p < d < f
2s and 2p have similar

48
Q

Do all orbitals have the same energy?

A

Within a sub shell, all orbitals have the same energy

49
Q

What is the Aufbau principle?

A

Subshells and orbitals are filled from the lowest energy to highest energy

50
Q

What is the Paull exclusion principle?

A

Each orbital may hold maximum 2 electrons. Both electrons must have a different spin

51
Q

What is Hund’s rule?

A

Each orbital in a subshell must be filled with one electron with parallel spin before an orbital is filled with a second electron

52
Q

What is the order of subshells being filled?

A

1s 2s 2p 3s 3p 4s 3d 4p 5s 4d 5p 6s 4f 5d 6p 7s 5f 6d 7p 8s

53
Q

According to Hund’s rule, how should electrons fill the orbital?

A

Every orbital must be filled with one electron with parallel spin before a 2nd electron is added

54
Q

How can electron configuration be condensed?

A

[Symbol of nearest noble gas]Additional subshells

55
Q

What is the electron configuration of Chromium?

A

1s2 2s2 2p6 3s2 3p6 3d5 4s1

56
Q

What is the electron configuration of Copper?

A

1s2 2s2 2p6 3s2 3p6 3d10 4s1

57
Q

What does it mean if an atom is in an excited state?

A

One or more electrons are found in higher energy subshells

58
Q

What is the subshell configuration that all atoms want?

A

p6

59
Q

In ions, how is the atomic electron configuration written?

A

Remove from the further shell possible first from nucleus OR add to p orbital

60
Q

In transition metals, what electrons are lost first?

A

Ones in the 4s subshell then the next level

IB Chemistry (7 decks)

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