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Chemistry exam questions > Atomic theory 5 > Flashcards

Atomic theory 5 Flashcards

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1
Q

Write the electron configuration (s. p etc) for an iron atom.

A

1s₂ 2s₂ 2p₆ 3s₂ 3p₆

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2
Q

What term is used to refer to the condition of the hydrogen atom when its electron occupies the E1 level?

A

Ground state

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3
Q

What term is used for the condition of the hydrogen atom when its electron occupies any of the levels E2, E3 etc?

A

Excited state

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4
Q

What causes the electron to leave the E1 level?

A
  • It acquires energy

- It is heated

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5
Q

Why does the electron not remain in any of the levels E2, E3 etc?

A

Higher energy states unstable

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6
Q

The visible lines in the atomic emission spectrum of a sample of hydrogen are produced when electrons fall to a particular energy level. Identify this energy level.

A

E₂ / n = 2

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7
Q

Bohr’s theory considered electrons as tiny particles restricted to orbits. How does modern atomic theory describe the behaviour of electrons?

A

Electrons have both wave and particle properties.

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8
Q

What are orbitals?

A

An atomic orbital is a region in space around the nucleus of an atom in which there is a high probability of finding an electron.

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9
Q

Identify the main energy levels involved in the electron transition that gives rise to the first (red) line of the Balmer series in the emission spectrum of the hydrogen atom.

A

2 and 3

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10
Q

Define an atomic orbital.

A

An atomic orbital is a region in space around the nucleus of an atom in which there is a high probability of finding an electron.

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11
Q

Write the ground state s, electron configuration for a carbon atom. How many orbitals are occupied?

A

1s₂ 2s₂ 2p₂

4 orbitals occupied

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12
Q

Distinguish between the ground state and the excited states of the electron in a hydrogen atom.

A

Ground - n = 1

Excited - n = 2,3

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13
Q

How can the electron in a hydrogen atom become excited?

A

Add heat

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14
Q

Explain the origin of the series of visible lines in the emission spectrum of hydrogen. What name is given to this series?

A
  • Excited electrons fall back from n = 3,4 to n = 2, the energy lost is emitted as light of different frequencies.
  • Balmer series
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15
Q

Explain why there is no yellow line in the hydrogen emission spectrum.

A

No corresponding excited state

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16
Q

Describe how to carry out a flame test to confirm the presence of lithium in a salt sample.

A

Clean a platinum (nichrome) wire in concentrated hydrochloric acid
Dip rod in salt and hold salt in hot part of Bunsen flame
Red crimson colour is a positive result for lithium

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17
Q

Define an atomic orbital.

A

An atomic orbital is a region in space around the nucleus of an atom in which there is a high probability of finding an electron.

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18
Q

Distinguish between a 2p orbital and a 2p sublevel.

A

2p sublevel consists of three 2p orbitals of equal energy

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19
Q

Write the s, p electron configuration for a calcium atom.

A

1s₂ 2s₂ 2p₆ 3s₂ 3p₆ 4s₂

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20
Q

Explain in terms of energy sublevels why the arrangement of electrons I the main energy levels in a calcium atoms is 2, 8, 8, 2 and not 2, 8, 10.

A
  • 4s sublevel lower in energy than the 3d

- Electrons fill the 4s sublevel before the 3d

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21
Q

Explain how the line emission spectrum of hydrogen arises and provides evidence for the existence of energy levels.

A
  • In the ground state the hydrogen electron occupies the lowest available energy level.
  • The electron can jump to a higher energy level if it recieves a certain amount of energy
  • Excited state unstable
    Evidence - Energy emitted corresponds to difference between the two energy levels.
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22
Q

Suggest an element that gives a blue-green colour to a fireworks display.

A

Copper

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23
Q

Write the s, p configuration of a calcium atom in its ground state.

A

1s₂ 2s₂ 2p₆ 3s₂ 3p₆ 4s₂

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24
Q

Give one significant difference between an electron in the 2s orbital and an electron in the 3s orbital of a calcium atom.

A
  • Energy of 2s electron is less than 3s
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25
Q

State the famous principle published in 1927, which bears the name Werner Heisenberg.

A

Position and momentum of an electron cannot be found simultaneously.

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26
Q

Name the scientist whose work on energy levels in the hydrogen atom is depicted in the Google doodle reproduced above.

A

Bohr

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27
Q

Distinguish between the terms energy level and atomic orbital.

A

Energy level - Is the discrete amount of enegry an electron has when it is in an atom.
An atomic orbital - is a region in space around the nucleus of an atom in which there is a high probability of finding an electron.

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28
Q

Write the electron configuration (s, p) of an atom of silicon showing the distribution of electrons in atomic orbitals in the ground state.

A

1s₂ 2s₂ 2p₆ 3s₂ 3p₂

Distribution on marking scheme (2014)

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29
Q

State how many (i) main energy levels, (ii) atomic orbitals are occupied in the silicon atom in its ground state.

A

(i) 3

(ii) 8

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30
Q

Use Bohr’s atomic theory of 1913 to account for the emission spectrum of the hydrogen atom.

A
  • The electron in a hydrogen atom occupies fixed energy levels.
  • In the ground state electrons occupy the lowest available energy levels.
  • The electron can move to a higher energy level if it receives a certain amount of heat
  • Excited state unstable
  • Emitting excess energy in the form of a photon of light
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31
Q

Explain in terms of atomic structure, why different flame colours are observed in flame tests using salts of different metals.

A

Metal atoms of different elements have different sets of energy levels therefore they emit different frequencies.

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32
Q

What colour is observed in a flame test on lithium chloride?

A

Red

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33
Q

Describe the testing procedure in a flame test on lithium chloride.

A
  • Salt on platinum probe

- Hold in at top of flame

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34
Q

Explain the term uncertainty principle.

A

This states that it is impossible to know both the position and the speed of an electron at the same time as electrons move in a wave motion.

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35
Q

Give one factor that contributed to the need for modification of Bohr’s 1913 theory other than Heisenberg’s uncertainty principle.

A
  • Wave nature of electron
36
Q

What is an atomic orbital?

A

An atomic orbital is a region in space around the nucleus of an atom in which there is a high probability of finding an electron.

37
Q

Define atomic orbital.

A

An atomic orbital is a region in space around the nucleus of an atom in which there is a high probability of finding an electron.

38
Q

Write the electron configuration (s, p etc) of the element manganese (Mn).

A

1s₂ 2s₂ 2p₆ 3s₂ 3p₆ 4s₂ 3d₅

39
Q

What do the electron configurations of the series of elements from scandium to zinc have in common?

A

Electrons entering 3d sublevel / All end in 3d(x)

40
Q

State the number of (i) sub-levels, (ii) orbitals, occupied by electrons in an argon atom in its ground state.

A

(i) 5

(ii) 9

41
Q

Write the electron configuration (s, p) of an oxygen atom showing the arrangement of electrons in atomic orbitals.

A

1s₂ 2s₂

Arrangements in marking scheme (2012)

42
Q

Outline Bohr’s atomic theory based on the hydrogen emission spectrum.

A
  • The electron in a hydrogen atom occupies fixed energy levels
  • An electron in an energy level does not radiate energy
  • Electron occupies lowest energy levels available
  • The electron can move to a higher energy level if it receives an amount of energy
  • The photon must be exactly equal to the energy difference between the ground state and a higher energy level.
43
Q

State two limitations of Bohr’s theory that led to its modification.

A
  • Didn’t work for higher elements

- Did not allow for uncertainty

44
Q

Draw the shape of the p-orbital.

A

Dumbbell drawn

45
Q

Draw the shape of the s-orbital.

A

In notes

46
Q

State the maximum number of electrons that can be accommodated in a p-orbital.

A

2

47
Q

Write the s, p electron configuration for the potassium atom.

A

1s₂ 2s₂ 2p₆ 3s₂ 3p₆ 4s₁

48
Q

How many (i) energy sub-levels, (ii) individual orbitals, are occupied by electrons in a potassium atoms

A

(i) 6 sublevels

(ii) 10 orbitals

49
Q

Explain why there are electrons in the fourth main energy level of potassium although the third main energy level is incomplete.

A

4s sublevel lower in energy than 3d

50
Q

Write the electron configuration (s, p etc.) of the aluminium ion (Al³+)

A

1s₂ 2s₂ 2p₆

51
Q

Name the type of spectroscopy, based on absorptions within a particular range of electromagnetic frequencies, and used as a ‘fingerprinting’ technique to identify organic and inorganic compounds.

A

infra-red / IR

52
Q

Define energy level.

A

One of the discrete amounts of energy that an electron has when it is in an atom.

53
Q

Distinguish between ground state and excited state for the electron in a hydrogen atom.

A

Ground - in lowest energy state

Excited - higher energy state

54
Q

Name the series of lines in the visible part of the line spectrum of hydrogen.

A

Balmer series

55
Q

Explain how the expression E2 - E1 = hf links the occurrence of the visible lines in the hydrogen spectrum to energy levels in a hydrogen atom.

A
  • E2 - E1 : Energy difference between higher and lower level
  • f = frequency of line in spectrum
  • h is Plank’s constant
  • Energy difference divided by frequency equals a constant.
56
Q

Define energy level

A

One of the discrete amounts of energy that an electron has when it is in an atom.

57
Q

Write the electron configuration (s, p) for the sulphur atom in its ground state, showing the arrangement in atomic orbitals of the highest energy electrons.

A

1s₂ 2s₂ 2p₆ 3s₂ 3p₄

Arrangement in marking scheme (2007)

58
Q

State how many (i) energy levels, (ii) orbitals, are occupied in a sulphur atom in its ground state.

A

(i) 3

(ii) 9

59
Q

Describe how you would carry out a flame test on a sample of potassium chloride.

A

n

60
Q

Why do different elements have unique atomic spectra?

A

Each element has a different distribution of energy levels giving rise to different electron transitions.

61
Q

What instrumental technique is based on the fact that each element has a unique atomic spectra?

A

Atomic absorption spectrometry (AAS)

62
Q

Define atomic orbital.

A

An atomic orbital is a region in space around the nucleus of an atom in which there is a high probability of finding an electron

63
Q

What does Heisenberg’s uncertainty principle say about an electron in an atom?

A

It is not possible to measure the exact position and energy of an electron in an atom simultaneously.

64
Q

Write the electron configuration (s, p etc.) of a chromium atom in its ground state.

A

1s₂ 2s₂ 2p₆ 3s₂ 3p₆ 4s1 3d₅

65
Q

Name the series of coloured lines in the line emission spectrum of hydrogen corresponding to transitions of electron from higher energy levels to the second (n=2) energy level.

A

Balmer series

66
Q

Distinguish between atomic orbital and a sublevel.

A

Atomic orbital - a region in space around the nucleus of an atom in which there is a high probability of finding an electron.
Sublevel - A group of atomic orbitals within an atom, all of which have the same energy.

67
Q

Describe how Bohr used line emission spectra to explain the existence of energy levels in atoms.

A
  • electrons in ground state
  • fixed energies absorbed
  • excited state unstable
  • energy difference between levels gives specific frequency of light in spectrum
68
Q

Why does each element have a unique line emission spectrum?

A

Each element has a different distribution of energy levels giving rise to different electron transitions.

69
Q

Name the instrumental technique that can be used to detect heavy metals and to measure their concentrations in a soil or water sample.

A

Atomic absorption spectrometry (AAS)

70
Q

Bohr’s atomic theory was later modified. Give one reason why this theory was updated.

A

Only worked for simple atoms

71
Q

Define energy level

A

One of the discrete amounts of energy that an electron has when it is in an atom.

72
Q

Define atomic orbital

A

An atomic orbital is a region in space around the nucleus of an atom in which there is a high probability of finding an electron.

73
Q

Write the electronic configuration (s, p etc.) of nitrogen.

A

1s₂ 2s₂ 2p₃

74
Q

Describe how the electrons are arranged in the orbitals of the highest occupied sub-level of a nitrogen atom in its ground state.

A

One electron in each of the three p orbitals

75
Q

Write the electronic configuration of a neutral copper atom.

A

1s₂ 2s₂ 2p₆ 3s₂ 3p₆ 4s1 3d₁₀

76
Q

Define atomic orbital.

A

An atomic orbital is a region in space around the nucleus of an atom in which there is a high probability of finding an electron.

77
Q

What spectroscopic technique is used to detect heavy metals, e.g. lead, in environmental analysis?

A

atomic absorption spectrometry / AAS

78
Q

What is the colour of the light associated with the line spectrum of sodium?

A

yellow / orange

79
Q

Explain how line emission spectra occur.

A
  • electrons restricted to energy levels
  • jump to higher levels
  • fall back emitting energy as light
  • energy difference between levels gives specific frequency of light in spectrum.
80
Q

What evidence do line emission spectra provide for the existence of energy levels in atoms?

A
  • only fixed frequencies are emitted

- therefore electrons must be restricted to certain energy values

81
Q

Why is it possible for line emission spectra to be used to distinguish between different elements?

A
  • different elements have different spectra
82
Q

Different metals impart different colours to the Bunsen flame. In case of any two named metals, state the colour imparted.

A

Sodium - amber/yellow

Potassium - lilac

83
Q

Explain briefly why different metals produce different flame colours.

A

Metal atoms of different elements have different sets of energy levels therefore they emit different frequencies.

84
Q

Write the electronic configuration of the Al³+ ion. What neutral atom has the same configuration?

A

1s₂ 2s₂ 2p₆

85
Q

Use diagrams to distinguish between a p orbital and a p sub-level (p subshell).

A

You have to draw a normal p (infinity sign) and then the different variations of sublevel, when on the x,y and z axes.

86
Q

Write the electron configuration for nickel in its ground state.

A

1s₂ 2s₂ 2p₆ 3s₂ 3p₆

87
Q

State one piece of evidence that supports the existence of atomic energy levels.

A

The atomic emission spectrum.

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