Atomic Structure/Amount of Substance Flashcards

1
Q

Relative mass of electron

A

0.0005 or 1/2000

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2
Q

Mass number

A

total number of nucleons (neutrons and protons)

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3
Q

Suggest points to consider when interpreting electron impact mass spectrum

A
  • greatest m/z value (of relatively high abundance) is from molecular ion and its m/z value gives relative molecular mass
  • exactly half m/z value could be 2+ ion, e.g. Cu+ (63 m/z) and Cu2+ (31.5 m/z)
  • ions slightly greater than greatest m/z value are due to molecular ions with 2H or 13C
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4
Q

Suggest points to consider when interpreting electrospray ionisation mass spectrum

A
  • greatest m/z value (of relatively high abundance) is from molecular ion and its relative molecular mass is m/z minus 1
  • always MINUS 1 from m/z to account for proton
  • ions slightly greater than greatest m/z value are due to molecular ions with 2H or 13C
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5
Q

Explain Cu and Cr electron configuration

A

copper - [Ar] 3d104s1
chromium - [Ar]3d54s1
- completely filled and half-filled subshells are more stable than partially filled ones
- electron from 4s orbital becomes excited and rises to 3d orbital

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6
Q

Describe process of electron impact/electrospray ToF mass spectrometry

A
  • sample vaporised and fired at by high speed electrons with electron gun
  • removes electrons from each particle to form ions with a single positive charge
    OR
  • sample dissolved in volatile solvent and injected through hypodermic needle attached to positive terminal of high voltage s]power supply
  • particles gain proton to form ions with a single positive charge
  • acceleration by electric field so particles have same kinetic energy but different velocity depending on mass
  • positive ions travel through a hole in a negatively charged plate into flight tube where time taken to hit detector is measured
  • positive ions gain electrons when they hit negatively charged detector plate
  • size of current gives measure of abundance of ion hitting plate
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7
Q

Give reasons why atoms are put into certain blocks

A
  • last electron found in that subshell

- highest energy subshell

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8
Q

Reason isotopes have the same chemical properties

A

same electron arrangement

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9
Q

Atomic number

A

number of protons in an element

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10
Q

Suggest why relative atomic mass calculated differs from the value in the Periodic Table

A

Periodic Table takes into account other isotopes/different amounts of isotopes

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11
Q

Suggest what information can be obtained from a mass spectrometer

A
  • m/z (relative isotopic mass)

- relative abundance of isotopes

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12
Q

Factors affecting ionisation energy

A
  • nuclear charge
  • shielding
  • atomic radius
  • whether electron is removed from neutral or charged species
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13
Q

What do electron arrows in orbitals represent

A

represent clockwise and anti-clockwise spin

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14
Q

Suggest why electrons in 2p sublevels have a higher energy than in 2s sublevels

A

further from nucleus so so more shielding

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15
Q

Explain why first ionisation energy of helium is very large

A

electron is not shielded from nucleus

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16
Q

How to calculate relative formula mass from mass spectrometer

A

sum of m/z multiplied by relative abundance divided by sum of relative abundances

17
Q

Reasons particles must be ionised before being analysed in a mass spectrometer

A
  • accelerated

- attracted to negative plate to be detected

18
Q

Term given to .xH20

A

waters of crystallisation

19
Q

Electron orbital

A

region around nucleus of an atom where electrons are most likely to be found

20
Q

Give mass spectrum for diatomic molecules with two isotopes and explain why

A

2A-2A (25%)
1A-1A (25%)
1A-2A or 2A-1A (so 50%)
molecule has two isotopes and is a diatomic molecule so there are three possible combinations of isotopes in molecule

21
Q

Suggest why there is a minimum energy for the electron gun used ionisation

A

so that only one electron is removed from atoms so ions with a single positive charge are formed

22
Q

Suggest a benefit of electrospray mass spectrometry

A

soft ionisation so larger molecules do not fragment as much

23
Q

Suggest which peak in mass spectrum is molecular ion peak

A

highest m/z value (but with relatively high abundance)

24
Q

Suggest how infrared mass spectrometry is used to differentiate between bonds in a molecule

A
  • different bonds vibrate at different discrete frequencies
  • infrared radiation absorbed by bonds excites them to a higher state of vibration
  • so different discrete frequencies of infrared radiation are absorbed based on bonds present
  • transmittance graph show peaks where infrared radiation is absorbed by bonds
25
Q

Fingerprint Region

A
  • between 1500-400cm-1
  • allows compounds with same functional groups to be distinguished
  • must have exact match to spectrum of known compound
26
Q

Relative atomic mass

A

ratio of the average mass of one atom of an element to one twelfth of the mass of an atom of carbon-12

27
Q

Suggest uses of a mass spectrometer

A
  • identify element
  • find mass and abundance of each isotope in element to determine relative atomic mass
  • find relative molecular mass of molecule
28
Q

Compare and contrast electron impact and electrospray ionisation ToF mass spectrometry

A
  • ionisation by electron gun vs dissolving in volatile solvent to protonate particles
  • elements and low Mr vs large molecules (e.g. proteins) and high Mr
  • electrospray referred to as soft ionisation since less fragmentation
  • Mr = greatest m/z vs greatest m/z minus 1
  • particles accelerated by an electric field for both
  • time measured for particles to travel through flight tube for both
  • abundance of each ion determined by size of current for both
29
Q

Suggest what peaks below greatest m/z value are due to for electron impact ionisation of molecules

A

fragmentation of molecular ion

30
Q

Explain why electrons in an orbital have opposite spin

A
  • electrons repel strongly

- opposite spin minimises repulsion

31
Q

Explain why 4s subshell is filled before 3d

A

lower energy level

32
Q

What does Avogadro’s constant tell us

A

number of particles in a mole

33
Q

State ideal gas equation and units for each variable

A
pV=nRT 
p - pressure in Pa
V - volume in m3
n - moles 
R - gas constant 
T - temperature in K (Celsius plus 273)
34
Q

Suggest what evidence there is from pattern in first ionisation energies across Period 3 to suggest 2 is maximum number of electrons in s-subshell

A

two elements before drop in ionisation energy

35
Q

Describe how to identify group or element from successive ionisation energies

A
  • calculate difference between each ionisation energy
  • any big jumps (above 1500-2000 kJmol-1) indicate electron is removed from a different energy level
  • smaller jumps refer to subshells (around 1000)
  • even smaller but still evident jumps are due to orbital pairing (unlikely to be obvious so ignore)
36
Q

How to use infrared spectroscopy to prove an aldehyde is definitely pentanal

A
  • compare with known spectrum for pentanal

- fingerprint regions should match exactly

37
Q

What needs to be true for molecular ions to have the same precise molecular mass

A

must contain same numbers of each atom not just same relative molecular mass