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Physical Chemistry (Year 1) > Atomic Structure > Flashcards

Atomic Structure Flashcards

1
Q

Position of the proton in an atom?

A

Nucleus

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2
Q

Position of the neutron in an atom?

A

Nucleus

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3
Q

Position of the electron in an atom?

A

Orbitals

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4
Q

Relative mass of a proton?

A

1

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5
Q

Relative mass of a neutron?

A

1

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6
Q

Relative mass of a electron?

A

1/1840

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7
Q

Relative charge of a proton?

A

+1

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8
Q

Relative charge of a neutron?

A

0

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9
Q

Relative charge of a electron?

A

-1

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10
Q

What is the atomic number?

A

The number of protons in the nucleus.

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11
Q

What is the mass number?

A

The total number of protons and neutrons in the atom.

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12
Q

What is an isotope?

A

Atoms with the same number of protons but different number of neutrons.

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13
Q

Describe the chemical and physical properties of isotopes.

A

Isotopes have similar chemical properties because they have the same electronic structure.
Isotopes have different physical properties because they have different masses.

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14
Q

What are the 4 energy levels?

A

S
P
D
F

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15
Q

How many electrons does the s orbital hold?

A

2

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16
Q

How many electrons does the p orbital hold?

A

6

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17
Q

How many electrons does the d orbital hold?

A

10

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18
Q

How many electrons does the f orbital hold?

A

14

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19
Q

What is represented by the arrows spinning in opposite directions?

A

Different spins of the electrons in the orbital.

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20
Q

What shape is the s sublevel?

A

Spherical

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21
Q

What shape is the p sublevel?

A

Dumbbell

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22
Q

What does an arrow represent?

A

One electron.

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23
Q

What does the box holding two arrows represent?

A

One orbital

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24
Q

How do the boxes fill up?

A

One arrow for each box then put a second arrow after all boxes have atleast 1.

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25
When a positive ion forms, what happens to the outermost shell?
An electron is lost.
26
When a negative ion forms, what happens to the outermost shell?
An electron is gained.
27
Does 4s or 3d fill first?
4s
28
What is different about copper and chromium?
3d fills before 4s.
29
Define first ionisation energy.
The enthalpy change when 1 mole of electrons is removed from 1 mole of gaseous atoms.
30
Give the equation of the first ionisation energy for H.
H(g) -> H^+(g) + e-
31
Define second ionisation energy.
The amount of energy needed to remove a second mole of electrons from a gaseous ion with a 1+ charge to form a gaseous ion with a 2+ charge.
32
Give the equation of the second ionisation energy for H.
H^+ (g) -> H^2+ (g) + e-
33
3 factors affecting ionisation energy?
Nuclear charge Atomic Radius Shielding
34
What is the nuclear charge?
The attraction of the nucleus. The more protons in the nucleus, the greater the attraction.
35
What is the atomic radius?
The distance of the outermost electrons to the nucleus. The bigger the atom, the weaker the attraction to the nucleus.
36
What is shielding?
The effect where inner electrons reduce the attraction between the nucleus and outermost electrons.
37
Trend across a period for shielding.
Stays the same.
38
Trend down a group for shielding.
Increases.
39
Why do first ionisation energies decrease down a group?
As one goes down a group, the outer electrons are found in shells further from the nucleus and are more shielded so the attraction of the nucleus becomes smaller.
40
Why is there a general increase in first ionisation energy across a period?
As one goes across a period the electrons are being added to the same shell which has the same distance from the nucleus and same shielding effect. The number of protons increases, however, making the effective attraction of the nucleus greater.
41
What is a mass spectrometer used for?
It is used to determine all the isotopes present in a sample of an element and to therefore identify elements.
42
What condition must there be for a mass spectrometer?
It must be under a vacuum otherwise air particles would ionise and register on the detector.
43
What are the 4 steps in a mass spectrometer?
Ionisation Acceleration Ion drift Detection
44
What are the two ways of ionisation?
Electro spray ionisation Electron impact
45
When is electrospray ionisation used?
For larger organic molecules.
46
How come fragmentation doesn't occur for electrospray ionisation?
The conditions are softer in this technique.
47
When is electron impact used?
For elements and substances with a low formula mass.
48
What would happen if electron impact was used on larger molecules?
Fragmentation.
49
Describe the process of electrospray ionisation.
Sample is dissolved in a volatile solvent and injected through a needle at high voltage. Each molecule gains a proton.
50
Describe the process of electron impact.
A vaporised sample is injected at low pressure. An electron gun fires high energy electrons at the sample. This knocks out an outer electron. This forms a positive ion.
51
What happens during acceleration?
Positive ions are accelerated by an electric field. To a constant kinetic energy.
52
Describe the velocity of lighter and heavier particles.
Lighter particles = faster velocity Heavier particles = slower velocity
53
Describe flight tube.
The positive ions with a smaller m/z values will have the same kinetic energy as those with a larger m/z and will move faster. Heavier ions take long to move through the drift area.
54
Describe detection.
The ions reach the detector and generate a small current, which is fed to a computer for analysis. The current is produced by electrons transferring from the detector to the positive ions. The size of the current is proportional to the abundance of the species.
55
What is m/z
Mass to charge ratio
56
How is relative atomic mass calculated.
Sum of (isotopic mass x relative abundance) divided by total relative abundance.
57
What are the two isotopes of chlorine?
Chlorine 35 Chlorine 37
58
What is the percentage abundance of chlorine 35?
75%
59
What is the percentage abundance of chlorine 37?
25%
60
What are the two isotopes of bromine?
Br 79 Br 81
61
What is the percentage abundance of Br 79?
50%
62
What is the percentage abundance of Br 81?
50%

Physical Chemistry (Year 1) (8 decks)

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