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Paper 1 CHEM MMS EXAM > ✅1 - Atomic Structure and the Periodic Table > Flashcards

✅1 - Atomic Structure and the Periodic Table Flashcards

1
Q

What are the subatomic particles in an atom?

A

Neutron, Proton and Electron

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2
Q

What is the relative charge of a neutron?

A

0

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3
Q

What is the relative charge of a proton?

A

1+

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4
Q

What is the relative charge of a electron?

A

-

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5
Q

What is the atomic (proton) number?

A

The number of protons in the nucleus

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6
Q

What is the atomic mass number?

A

The number of protons + neutrons, also the relative atom mass

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7
Q

What are isotopes?

A

Atoms of the same element with different number of neutrons, but the same number of protons and electrons

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8
Q

What is relative atomic mass?

A

The weighted mean mass of an atom of an element relative to 1/12th of the mass of Carbon12

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9
Q

What is relative isotopic mass?

A

The mass of an isotope relative to 1/12th of the mass of Carbon12

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10
Q

What does a mass spectrometer measure?

A

The masses of atoms and molecules (as well as the fragments that make up the molecule)

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11
Q

What are Molecular Ion Peaks (M+) used to determine?

A

An exact Relative Molecular Mass

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12
Q

What peak is the M+?

A

The strongest peak furthest to the right

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13
Q

When should the term ‘Relative Formula Mass’ be used?

A

For compounds with giant structures

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14
Q

In a Mass Spectrum of an element, what does the number of peaks show?

A

The number of isotopes

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15
Q

In a Mass Spectrum of an element, what does the M/z of a peak show?

A

The mass number of the isotope

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16
Q

In a Mass Spectrum of an element, what does the size of a peak show?

A

The relative abundance of an isotope

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17
Q

What are the 4 processes in a mass spectrometer?

A

Ionisation, Acceleration, Deflection and Detection

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18
Q

Why must a vacuum be used in a mass spectrometer?

A
  • It means no interference from atoms or molecules in air

- Molecular fragments could not exist otherwise

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19
Q

What is M/z?

A

Mass to charge ration, mass divided by charge

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20
Q

What does the position of an atom on the Mass Spectra depend on?

A

The amount of deflection, therefore the mass of the atom.

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21
Q

What are quantum shells?

A

Defined energy levels, filled from the inside out

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22
Q

What are orbitals?

A

Subshells of the quantum shells, where electrons exist , a pattern of electron density

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23
Q

What shape is the S orbital?

A

Spherical

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24
Q

How many electrons can an S orbital hold?

A

2, with a 90% probability of finding them in its boundary

25
What shape are P orbitals?
'Dumbbell' shape
26
What are the names of the 3 P orbitals?
Px, Py ad Pz
27
How many electrons can the P orbitals hold in total?
6
28
Why is the 4s orbital filled before the 3d orbital?
Because it is slightly lower in energy
29
How many electrons do the D orbitals hold in total?
10
30
How many electrons fill the first quantum shell?
2
31
How many electrons fill the second quantum shell?
8
32
How many electrons fill the third quantum shell?
18
33
How many electrons fill the fourth quantum shell?
32
34
Two electrons in the same orbital must have opposite...
...spins
35
In what order do electrons fill subshells?
First singly, then pairing up
36
What does electronic configuration determine?
The chemical properties of an element
37
What provides evidence for the existence of quantum shells?
Atomic Emission Spectra
38
What provides evidence for the existence of quantum shells AND the group to which the element belongs?
Successive Ionisation Energies
39
What provides evidence for electron subshells?
First Ionisation Energies
40
If an electron takes in energy from its surroundings it is...
...excited to a higher energy level
41
When an electron drops down tot a lower energy level, it...
...releases this energy in the form of a photon with energy matching the gap.
42
When do the energy levels get closer together?
As energy/frequency increases
43
What suggests that electrons exist at very specific energy levels?
There is no 'inbetween' amount of energy, electrons exist at very specific energy levels
44
What is 'first ionisation energy'?
The energy needed to remove 1 electron from each atom in 1 mole of gaseous atoms to form one mole of gaseous 1+ ions
45
What is the equation for the first ionisation energy for sodium?
Na(g) -----> Na+(g) + e-
46
Why does Atomic Radius affect the First Ionisation Energy?
The more shells and atom has, and therefore the further away the outer electrons are from the nucleus, the less attraction they experience
47
Why does Nuclear Charge affect the First Ionisation Energy?
The more protons, the greater the nuclear charge, and the greater the attraction felt bu the electrons
48
Why does Electron Shielding affect the First Ionisation Energy?
As the number of electrons between the outer electrons and the nucleus increases, the outer electrons feel less attraction towards the nucleus
49
What happens to first ionisation energies going down a group?
It decreases
50
What happens to first ionisation energies going across a period?
They generally increase
51
What happens to first ionisation energies between Groups 5 + 6, and why?
They decrease because between Beryllium and Boron, a new energy level is begun, so less energy is required to remove the single electron form the new shell
52
What happens to first ionisation energies between Groups 2 + 3, and why?
They decrease because between Mg and Al, the 3p orbital is started, so less energy is required to remove the single electron in the new shell
53
What trends are there in the periodic table?
- melting and boiling points - atomic radius - ionisation energies
54
Why do metallic bonds get stronger across the metals?
Because there are more electrons per positive ion (2+ charge means there's 2 delocalised electrons for each positive ion
55
How does atomic radius change across a period?
It decreases, because as the nuclear charge of the atom increases, the outer shells are pulled inwards
56
How does electron shielding change across a period?
It doesn't, because they're still filling the same quantum shell
57
How does nuclear charge change across a period?
It increases, because the number of protons increases
58
How do melting/boiling points change across a period?
They increase until after the macro-molecular structures, London forces affect this.

Paper 1 CHEM MMS EXAM (12 decks)

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