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A Level Chemistry - Physical Chemistry > 3.1.1 Atomic Structure > Flashcards

3.1.1 Atomic Structure Flashcards

1
Q

Definition of an isotope

A

Same number of protons different number of neutrons

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2
Q

Relative mass of an electron

A

1/1836

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3
Q

Is the mass number the top or bottom number

A

Top

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4
Q

Is the atomic number the top or bottom number

A

Bottom

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5
Q

What is the mass number

A

Number of protons and neutrons

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6
Q

What is the atomic number

A

The number of protons
& Electron if the element is neutral

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7
Q

What holds an atom together

A

Electrostatic attraction between the positive nucleus and the negatively charged electrons orbiting around it

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8
Q

How is an ions formed

A

When atoms gain or lose electrons

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9
Q

Chemical properties of isotopes + why

A

Isotopes of the same element have the SAME CHEMICAL CHARACTERISTICS because the have the same number of electrons on OUTER SHELL.
( electrons take part in chemical reactions and therefore determine the chemistry of an atom)

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10
Q

Isotopes physical properties + why
(Compared to the same element)

A

Different mass and density
Different number of neutrons

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11
Q

How to calculate relative atomic mass from a mass spectra

A

(Relative abundance x mass)+(relative abundance x mass) etc / total abundance aka percentage (usually adds to 100 but check)

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12
Q

The abundance tells us….

A

How common each isotope is

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13
Q

What do you use a mass spectrometer for

A

Determining mass number and abundance of isotopes

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14
Q

What is in the sample chamber in a mass spectrometer

A

All the different isotopes of that element

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15
Q

Samples need to be…. before it enters the mass spectrometer

A

Ionised

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16
Q

What are two ways to ionise a sample

A

Electron spray ionisation
Electron impact ionisation

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17
Q

How does electrons spray ionisation work

A

Sample dissolved in a volatile solvent
Injectedthrough small nozzle at high pressure and voltage
Each Particles gain H+ ion

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18
Q

How does electron impact ionisation work

A

Sample is vaporised
Electron gun fires high energy electrons at it
Electron knocked off forming +1 ion

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19
Q

Definite relative atomic mass

A

The average mass of one atom of an element compared with 1/12 of the mass of an atom of carbon-12

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20
Q

Why is TOF kept in a vacuum

A

To prevent ions from colliding with air molecules

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21
Q

Through which form of ionisation is fragmentation most likely to occur

A

Electron impact ionisation

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22
Q

Ions are all accelerated to have the same ….

A

Kinetic energy

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23
Q

Equation for kinetic energy

A

KE= 1/2 x m x v^2

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24
Q

Definition first ionisation energy

A

The energy needed to remove one mole of electrons from one mole of atoms in their gaseous state to form one mole of 1+ ions

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25
Define second ionisation energy
The energy needed to remove one mole of electrons from one mole of 1+ ions in their gaseous state to form one mole of 2+ ions.
26
What did John dalton do x2
Atoms were solid spheres Difference spheres made different elements (:
27
What did JJ Thompson do
- plum pudding model - discovered electrons
28
What is Rutherford do + model
Alpha scattering experiment Nuclear model + discovered nucleus
29
What did Bohr do x3
Electrons in fixed orbits Each shell fixed energy When electrons move between shells electromagnetic radiation is emitted or absorbed
30
Definition of relative atomic mass
Average mass of one atom of an element compared with 1/12 of the mass of an atom of carbon-12
31
Explain how ions are accelerated, detected and have their abundance determined in a time of flight (TOF) mass spectrometer
Attraction to negatively charged plate Ions detected by gaining electrons Abundance determined by current flowing in the detector
32
2 difference between model used now and plum pudding model
Nucleus contains protons AND neutrons Electrons are arranged in energy levels
33
Ionisation energy equations 1st 2nd 3rd
E(g) —> E+(g) + E- E(g)+ —> E2+(g) + E- E2+ (g) —-> E3+(g) + E-
34
Abundance is …… to the size of the current
Proportional
35
How to calculate the mass of an ion in kg
Atomic number x 10^-3 / 6.022x10^23
36
Which shell empties first 4s or 3d
4S PLEASE REMBER
37
Why does aluminium not fit ionisation trend
Electron in 3p orbital higher in energy level than 3s orbital in magnesium
38
Why does sulphur not fit the trend of ionisation
Outer electron in 3p sub shell begin to pair So they repel
39
What is the little line in a mass spectrometer due to
Presence of 2H or 13C
40
How to find the relative molecular mass from a mass spectrometer
Where the peak is Greatest m/z ratio
41
Which is the one where you take off one for the relative molecular mass
Electron spray ionisation They gain a H+
42
Which two element are the exception to the electron configuration
Cr and Cu
43
Electron configuration of cr
1s2 2s2 2p6 3s2 3p6 3d5 4s1
44
Electron configuration of cu
1s2 2s2 2p6 3s2 3p6 3d10 4s1
45
In a mass spectrometer the ions travel at a ….
Constant speed
46
Relative molecular mass
The average mass of a molecule when measured on a scale on which the mass of an atom of carbon 12 is exactly 12
47
Relative isotopic mass
The mass of an atom of an isotope of an element when measured in a scale on which the mass of an atom of carbon 12 is exactly 12
48
What does the last peak on a mass spectra for molecules indicates
It is the molecular ion peak It is the same as the relative molecular mass of the molecule
49
What’s key to remember about the electron configuration order
4s comes before 3d It empties and fills first
50
Ionisations energy always have a positive/negative charge + why
Positive Endothermic as the process requires energy
51
What 3 things effect the ionisation energy
Shielding Nuclear charge Atomic size
52
Why is ionisation necessary in time of flight x2
- they can be accelerated by magnetic field - ions create a current when hitting the detector
53
Isotopes have the same/different chemical properties
Same
54
Ionisation energy increase/decreases across period 2 or 3 +why
Increases because number of protons increasing but SHIELDING is the similar. Stronger attraction between outer most electron and nucleus
55
As you move down group 2 the first ionisation energies
Decreases.
56
Which ionisation means the m/z ratio is one higher than the relative mass + what do you do
Electron spray ionisation means the m/z ration is +1 than it should be because it gained H+ Take away 1 then do
57
Acceleration in TOF is done by…
ELECTRIC field
58
Why does radius decrease/increase across period 2
Decrease Increase nuclear traction as the number of protons increase with the same shielding. So the electrons in outer shell are more strongly attracted in.
59
The ion that reaches the detector forts in TOF would have the highest/lowest m/z ratio
Lowest
60
2 difference between Rutherford model and current model
current neutrons AND PROTONS ELECTRONS IN DIFFERENT ENERGY LEVELS
61
In terms of ionisation energy do all the periods follow the same trend
Yes
62
Although not on spec can ask about trend in ionisation energies across period 2. What do you say…?
The exact same pattern as for period 3 with the same reasons. Just don’t say 3p orbitals etc because it’s two. If in doubt don’t say which letter.
63
Which has a greater first ionisation energy H or He
Helium The electron is begin removed from the same orbital as hydrogen but there are more protons 2 instead of 1 so the is a grate attraction + ionisation energy increases top right of periodic table
64
Technique for doing electron configuration of ions
Do original elements first then ion DO THIS

A Level Chemistry - Physical Chemistry (8 decks)

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