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Chemistry > W2 > Flashcards

W2 Flashcards

1
Q

What year did Niels Bohr solve Rutherford’s problem?

A

1913.

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2
Q

What is Bohr’s model based on?

A

Experimental data of the emission line spectra for hydrogen.

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3
Q

Is emission spectra continuous?

A

No because electrons can only exist in discrete energy levels and not in between them.

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4
Q

How many lines did Hydrogen have in Bohr’s experiement on the emission spectra?

A

4

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5
Q

What did Bohr determine in relation to atom structure?

A

That electrons move in orbits or fixed energy levels, called shells.

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6
Q

What’s a principal quantum number?

A

A number given for a level of shell.

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7
Q

What pronumeral represents principal quantum numbers?

A

n

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8
Q

Expand on n = 1.

The shell closest to nucleus. Orbit? Energy? AKA?

A

Smallest orbit and least energy. Referred to as ‘ground state’.

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9
Q

What is ground state?

A

n = 1, or the closest shell to the nucleus.

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10
Q

What happens to the orbit and energy as electrons are further away from the nucleus?

A

Larger orbit and more energy.

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11
Q

What did Bohr predict?

A

That electrons can only ‘jump’ and ‘fall’ between fixed energy levels, and that each shell has limits to the amount of electrons it can hold.

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12
Q

How was radiation involved in Bohr’s work?

A

Radiation is absorbed and emitted when an electron moves from one orbit to another.

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13
Q

What’s a spectrometer?

A

An instrument that seperates components of light, which have different wavelengths.

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14
Q

What form does the sample have to be in to see line spectrum?

A

Elemental form.

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15
Q

What units do spectrometers measure in?

A

Nanometres (nm).

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16
Q

What’s the wavelength of a red light?

A

Larger, 659nm.

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17
Q

What’s the wavelength of a blue light?

A

Smaller, 434nm.

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18
Q

What’s the energy like in a blue light?

A

High.

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19
Q

What’s the energy like in a red light?

A

Low.

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20
Q

What’s the frequency like of a red light?

A

Small.

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21
Q

What’s the frequency like of a blue light?

A

High.

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22
Q

In what quantities can atoms emit energy?

A

Only in precise ones.

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23
Q

What is the energy level also known as?

A

Shell.

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24
Q

What was Bohr’s conclusion?

A

When an atom is heated it absorbs energy, exciting electrons so they jump to the NEXT shell. When they fall back to ground state, they release fixed amount of energy called quanta. This is seen as wavelengths of light and different colours.

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25
Q

What is quanta?

A

The fixed amount of energy released by electrons when they fall back to ground state.

26
Q

How is quanta seen?

A

As wavelengths of light in different colours.

27
Q

Is the ultraviolet range visible to humans?

A

No.

28
Q

What’s the formula for the max. amount of electrons on the outer shell?

A

2n squared.

29
Q

What’s the max. number of electrons in n = 1, n = 2, n = 3 and n = 4?

A

2, 8, 8/18 and 32.

30
Q

What are the pronumerals for shells n = 1, n = 2, n = 3 and n = 4?

A

K, L, M and N.

31
Q

What are valence electrons?

A

Electrons in the outer most shell.

32
Q

How are groups connected?

Hint: valence.

A

Same group = same valence (amount of electrons in the outer shell). This means they have similar properties.

33
Q

What are the limitations of Bohr’s findings?

A

With some elements other than Hydrogen, more than one line of a certain colour occurs on the emission line spectra. He couldn’t explain this, the 2n(2) rule or why the fourth shell can accept electrons when the third isn’t full.

34
Q

What state are electrons represented in by the electron configuration?

A

Their ground state.

35
Q

What’s the colour with the shortest wavelength and highest frequency?

A

Violet.

35
Q

Are the line patterns of emission line spectra unique? Why?

A

Yes, they’re different with every element because of their electron configuration.

35
Q

What was Erwin Schrodinger’s background?

A

An Austrian physicist.

36
Q

Which model did Erwin Schrodinger refine?

A

Bohr model.

37
Q

Where are subshells?

A

In each shell.

38
Q

How many subshells in each shell?

A

The principal quantum number corresponds to the amount of subshells. Eg. Shell 2 = 2 subshells.

39
Q

What are the subshell names/pronumerals?

A

s, p, d, f.

40
Q

What’s the Pauli Exlusion Principle?

A

Max number of electrons per orbital = 2.

41
Q

What are orbitals?

A

Regions of probability in each subshell where an electron can be found.

42
Q

Describe the K shell: quantum number, max number of electrons it can hold, number of subshells and how many electrons can each subshell hold/number of orbitals?

A

n = 1
Max. electrons = 2
1s (1 subshell)
1s(2) = subshell holds 2 electrons

43
Q

Describe the L shell: quantum number, max number of electrons it can hold, number of subshells and how many electrons can each subshell hold/number of orbitals?

A

n = 2
Max. electrons = 8
2s and 2p (two subshells)
2s(2) = subshell holds two electrons
2p(6) = subshell holds six electrons

44
Q

Describe the M shell: quantum number, max number of electrons it can hold, number of subshells and how many electrons can each subshell hold/number of orbitals?

A

n = 3
Max. electrons = 8/18
3s, 3p and 3d (three subshells)
3s(2) = subshell holds two electrons
3p(6) = subshell holds six electrons
3d(10) = subshell holds ten electrons

45
Q

Describe the N shell: quantum number, max number of electrons it can hold, number of subshells and how many electrons can each subshell hold/number of orbitals?

A

n = 4
Max. electrons = 32
4s, 4p, 4d and 4f (four subshells)
4s(2) = subshell holds two electrons
4p(6) = subshell holds six electrons
4d(10) = subshell holds ten electrons
4f(14) = subshell holds fourteen electrons

46
Q

What does the L shell tell you?

A

It describe the shape of the atom.

47
Q

Are electrons particles, waves, or both?

A

Both.

48
Q

What’s the exception when filling the orbitals in the ‘d’ subshell of transition elements?

A

If the last subshell is ‘d10’ then you can half fill it by dividing by 2, also halving the subshell before it. This will make it more stable. Remember to then switch these two around when writing electronic configuration.

49
Q

When writing electronic configuration using the Bohr model, do you have to use all the orbitals in the last subshell?

A

No.

50
Q

Do you have to fully fill a shell to make it stable? Eg. when writing the element symbol.

May need to use isotopes.

A

Yes.

51
Q

What’s a real life example of flame tests?

A

Fireworks.

52
Q

What do flame tests help you identify?

A

Metal ions M+ (cations).

53
Q

How do flame tests help you identify metal ions?

A

By the unique colour that’s emitted from the movement of electrons between shells, when heated up.

54
Q

What colour is emitted from sodium in a flame test?

A

Yellow/orange.

55
Q

What colour is emitted from potassium in a flame test?

A

Lilac.

56
Q

What colour is emitted from calcium in a flame test?

A

Brick red.

57
Q

What colour is emitted from strontium in a flame test?

A

Red.

58
Q

What colour is emitted from copper in a flame test?

A

Blue.

59
Q

What colour is emitted from barium in a flame test?

A

Light green.

Chemistry (7 decks)

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