Atomic Structure Flashcards

1
Q

Define Isotope

A

Same number of protons but a different number of neutrons

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2
Q

Define ion

A

A charged particle with more/fewer electrons than protons

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3
Q

In the periodic table symbols what are A and Z

A

A is the mass number
Z is the atomic number

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3
Q

Define Nucleon

A

Particles in the nucleus

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4
Q

Define Element

A

A chemical (molecule or atoms) made up of 1 type of atom, all with the same number of protons

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5
Q

What’s the equation to calculate the number of neutrons?

A

N = A - Z

Where A is the mass number and Z is the atomic number

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6
Q

What’re the 2 points you need to make for the model answer about the models of the atom

A

The current model has:

Neutrons and Protons in the nucleus,

Electrons orbit the nucleus in different energy levels

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7
Q

Define Relative Molecular Mass

A

The average weighed mass of one molecule compared to 1/12th the mass of one atom of carbon 12

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7
Q

Define Relative Atomic Mass

A

The average weighed mass of one atom compared to 1/12th the mass of one atom of carbon 12

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7
Q

What’s the equation to calculate relative atomic mass?

A

𝑅𝐴𝑀= (∑(𝑚𝑎𝑠𝑠 𝑥 𝑎𝑏𝑢𝑛𝑑𝑎𝑛𝑐𝑒))/(𝑡𝑜𝑡𝑎𝑙 𝑎𝑏𝑢𝑛𝑑𝑎𝑛𝑐𝑒)

Total abundance is all abundances added together

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8
Q

What should be done if there are 2 unkown abundances in a RAM calculation?

Scaffold

A

Solve simultaneously, by creating an equation showing the left over %s in terms of x+y and rearranging

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9
Q

Model Answer describing Electron Impact

A

(for atoms/small molecules)
High energy electrons
From electron gun.
Fired at sample.
Knocks off one electron.
Has to happen in the gas phase.

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10
Q

Equation for electron impact with state symbols

A

M(g) –> M(g)+ + e-

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11
Q

Model Answer for Electrospray

A

Sample dissolved in volatile polar solvent
Injected as an aerosol through needle
Needle has a high positive charge
Sample gains a H+ ion

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12
Q

Equation for Electrospray

With state symbols

A

M(g)+ H^+(g) –> MH^+(g)

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13
Q

Model Answer describing Acceleration

A

Positive ions are accelerated by a negative electric field
To a constant kinetic energy

14
Q

Ion Drift Model Answer

A

The positive ions with smaller m/z values will have the same kinetic energy as those with larger m/z and so will move faster as they have less mass, so have more velocity. The heavier particles move slower. The ions are separated by different flight times.

15
Q

Detection model Answer

A

For each isotope the mass spectrometer can measure a m/z (mass/charge ratio) and an abundance. Each ion of the same mass hits the detector plate at the same time.
Each ion gains an electron.
This generates a current that is measured. The current is proportional to abundance

16
Q

What is a molecular ion peak? What do they show?

A

Molecular ion peak is the peak furthest to the right that isn’t tiny.
Molecular ion peak’s m/z=molecules Mr

17
Q

What does Time of Flight mass spectrometry measure?

A

ToF mass spec measures 2 properties of compounds (and their ions) mass/charge ratio, called m/z and abundance

Mass/charge ratio is the relative mass of the ionised chemical compared to the positive charge of the molecule

In ToF mass spec the charge of the ions involved is often +1 and there is little fragmentation

18
Q

What’s the equation that links v, d and t?

A

v=d/t

19
Q

What’s the substitution equation for KE and d and t?

A
20
Q

What’s the equation to calculate the mass of an atom?

A

mass of 1 atom = (Ar/1000)/L

21
Q

Equation for calculating the time of 2 different particles with different masses?

A

mx/tx^2=my/ty^2

22
Q

What are the 4 types of orbital?

A

s, p, d, f

23
Q

Where are the s, p, d and f blocks?

A
24
Q

Model Answer describing s and d orbitals

A

s fills and empties before d

25
Q

What are the rules for filling orbitals?

A

Electrons enter the lowest available energy level

When in orbitals of equal energy, electrons will try to remain unpaired

No two electrons can have the same four quantum numbers.

26
Q

Define First Ionisation Energy

A

The minimum energy required to remove 1 mole of electrons from 1 mole of gaseous ions

27
Q

What three factors affect ionisation energy?

A

Distance from nucleus,
Nuclear Charge,
Shielding by electrons,

28
Q

What is shielding?

A

When the number of inner electrons is greater, they shelter the outermost electron from the nucleus, allowing it to neglect the nuclear pull to some extent.

29
Q

Model Answer describing atomic radius down a group

A

Down a group atomic radius increases because, whilst the nuclear charge (number of protons) increases, the energy levels and shielding increase more

30
Q

Model answer describing atomic radius trends across a period

A

Across a period the atomic radius decreases because the nuclear charge increases and the energy level and shielding stay the same.

31
Q

Model Answer - First ionisation energy down a group

A

larger atomic radius

More shielding

Therefore weaker attraction from nucleus to electron in outer shell

32
Q

Model Answer first ionisation energy general trend across a period

A

Across a period:
Increased nuclear charge (i.e. more protons)
Smaller atomic radius
No change in Shielding
Therefore stronger attraction from nucleus to electron in outer shell

33
Q

First ionisation energy trend, Graph

A
34
Q

Model answer reason for deviation between Mg and Al in first ionisation energy

A

First electron in 3p which is higher in
energy

35
Q

Model Answer - Reason for deviation for S and P in first ionisation energy

A

S is lower than expected because it has the first spin pair repulsion in 3p

36
Q

Model Answer - Describing identifying an element from successive ionisation energy

Use X and Y as the numbers of the ionisation

A

There is a large jump between X and Y. This is because the lower energy level are much closer to the nucleus and less shielded so have a stronger attraction to nucleus requiring more energy to remove them.