P1: Atomic Structure Flashcards

1
Q

What are protons and neutrons sometimes called, and why?

A

Nucleons, because they are in the nucleus.

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2
Q

What is relative atomic mass relative to?

A

Carbon 12, weighing 12

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3
Q

What is 1 mass unit equal to (relative atomic mass)?

A

1/12 mass of Carbon 12

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4
Q

What is mass (kg) of a proton?

A

1.673 x 10^(-27)

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5
Q

What is the charge (c) of a proton?

A

+1.602 x 10^(-19)

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6
Q

What is the mass (kg) of a neutron?

A

1.675 x 10^(-27)

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7
Q

What is the charge (c) of a neutron?

A

0

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8
Q

What is the mass (kg) of an electron?

A

0.911 x 10^(-30)

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9
Q

What is the charge (c) of an electron?

A

-1.602 x 10^(-19)

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10
Q

What are the Mr’s of a proton, neutron, and an electron?

A

P: 1
N: 1
E: 1/1840

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11
Q

What do we use Time of Flight Mass Spectrometry for?

A

To find the abundance mass of each isotope in an element, allowing us to determine its relative atomic mass.
- Can also do molecular

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12
Q

What are the 3 stages of Time of Flight Mass Spectrometry?

A
  1. Ionisation- make it a +ion, there are two methods
  2. Acceleration- Using an electric field so they all have the same kinetic energy
  3. Flight Tube- Ions travel through a hole in the negative plate, a current is detected and time is taken.
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13
Q

Explain the ‘electron impact’ method for ionisation in ToF

A
  • Sample is vaporised
  • An electron gun, hot wire filament, fires high energy electrons at the sample
  • This knocks off one electron from each particle, forming 1+ ions
    -These are attracted to the negative plate and are accelerated

(fragmentation may occur)

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14
Q

Explain the ‘electrospray ionisation’ method for ToF

A
  • Sample is dissolved in volatile solvent (e.g water) and injected into a fine hypodermic needle
  • This creates a fine mist
  • The needle is attached to a positive terminal of high voltage power supply
  • The particles gain a proton (e.g H+ ion) and are now positive ions
  • The solvent evaporates and leaves the + ions to be attracted to the negative plate where they are accelerated.
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15
Q

Why do some ions reach the detector before the other ions? (in ToF)

A

Lighter ions travel faster as they have more velocity (isotopes) so reach the detector first.

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16
Q

(ToF) What is the kinetic energy formula?

A

KE= 1/2mv^2

becomes…

KE=1/2m d^2/t^2 when combined with the velocity calc d/t

17
Q

(ToF) What is the time equation?

A

t= d⎷m/2KE

or if not given enough values for that, use the KE equation and rearrange

m/t=m/t (t^2)

18
Q

What are the two ionisation equations? (ToF)

A

Electrospray:

X(g) + H+ → XH+(g)

Electron impact:

X(g) + e- → X+(g) + 2e-

19
Q

What are some other names for electron shells?

A

-Main energy levels
-Orbitals
-Shells

20
Q

What are the main energy levels labelled as?

A

1, 2, and 3…

1 being the closest to the nucleus and the lowest energy.

21
Q

Where are the sub-levels of orbitals found?

A

Level 1: s
Level 2: s + p
Level 3: s + p + d

also f (not needed)

22
Q

Explain the ‘ s ‘ sub-unit

A
  • All orbitals have them
  • Hold up to 2 electrons, with only one group (so just 2)
  • The first two groups of the periodic table.

The diagram is a circle around the origin in a graph.

23
Q

Explain the ‘p’ sub-unit

A
  • Starts at level 2 and carries on
  • Holds 2 electrons in each, with 3 groups (so 6 altogether)
  • Begins after the transition metals on the periodic table.

There are 3 diagrams, all have a figure of 8 shape in these directions on the axis ↑ → and diagonal right.

24
Q

Explain the ‘d’ sub-unit

A
  • Starts at level 3 and so on, however although it belongs to the level 3 group, it comes after 4s as this has lower energy (and follows the periodic table structure)
  • Hold 2 electrons each, with 5 groups (so 10 altogether)
  • The transition metals on the periodic table.

We don’t need to know the diagrams.

25
Q

How are the main energy levels arranged with the sub-units (☐) in a diagram?

A
  |
  |          5p☐☐☐
  |                         4d☐☐☐☐☐
  | 5s☐
  |          4p☐☐☐
  |                         3d☐☐☐☐☐
  | 4s☐
  |          3p☐☐☐
  | 3s☐
  |          2p☐☐☐
  | 2s☐
  |
  | 1s☐ ^Energy

*notice how the 4s is below the 3d as 4s is lower in energy, even though 3d is technically still level 3

26
Q

What is a spin?

A

A property that electrons have within an orbital.
- There is and up spin and a down spin
- Two electrons in the same orbital must have opposite spins

Represented by half arrows (like in an equilibria reaction)

27
Q

What are the 3 rules of allocating electrons to orbitals?

A
  1. Low energy orbitals must be filled first, so the lowest main energy level, with the lowest sub unit (s).
  2. Orbitals with the same energy levels (e.g p and d) must fill singularly before paired (otherwise repulsion occurs) so 3d: 3 up arrows before any down arrows are added.
  3. No orbital can have more than two electrons in it, so only two arrows.
28
Q

How do you write electron shell configurations?

A

e.g 10 electrons
1s^2 , 2s^2 , 2p^6

1= energy level
s= sub-unit
^x= how many electrons

29
Q

Define ionisation energy

A

The energy required to remove an electron from an atom

-From one singular atom, so may need to be in vapour form

30
Q

Why does the ionisation energy increase as we go down an energy level and each electron?

A

-Energy level 3 is the furthest away from the nucleus therefore has the least attraction, as you go down levels, the energy required increases
-A slight increase in energy occurs as each electron is taken in one energy level because the ion gets increasingly positive, therefore the attraction is greater.

31
Q

These are the fist ionisation energies of period 3:
Na- 496
Mg- 738
*Al- 578
Si- 789
P- 1012
*S- 1000
Cl- 1251
Ar- 1521

These should increase as the nuclear charge increases, but why are there anomalies in Al and S?

A

Al- has an electron in the p sub-unit, slightly higher than the s sub-unit in Mg, therefore further away from the nucleus so less energy needed.

S- has 2 electrons in one p sub-unit (one box) so ‘spin-pair repulsion’ occurs, easier to take away as they are repelling anyway.

32
Q

Why does the 1st ionisation energy decrease going down group 2?

A

The number of shells increase, so better atomic shielding and larger atomic radius

33
Q

Why do we use time of flight mass spectrometry?

A

Helps work out the mass of an atom

34
Q

Kinetic energy =?

A

1/2 m v^2

35
Q

Velocity=?

A

distance/ time

36
Q

Kinetic energy combined with velocity equation?

A

KE= 1/2 m d^2/t^2

37
Q

Time with kinetic energy equation?

A

t= d Square root: m/ 2KE