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Chem A Level > ✅1 - Atomic Structure and the Periodic Table > Flashcards

✅1 - Atomic Structure and the Periodic Table Flashcards

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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 proton?

A

+

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3
Q

What is the relative charge of a neutron?

A

0

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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
Q

What shape are P orbitals?

A

‘Dumbbell’ shape

26
Q

What are the names of the 3 P orbitals?

A

Px, Py ad Pz

27
Q

How many electrons can the P orbitals hold in total?

A

6

28
Q

Why is the 4s orbital filled before the 3d orbital?

A

Because it is slightly lower in energy

29
Q

How many electrons do the D orbitals hold in total?

A

10

30
Q

How many electrons fill the first quantum shell?

A

2

31
Q

How many electrons fill the second quantum shell?

A

8

32
Q

How many electrons fill the third quantum shell?

A

18

33
Q

How many electrons fill the fourth quantum shell?

A

32

34
Q

Two electrons in the same orbital must have opposite…

A

…spins

35
Q

In what order do electrons fill subshells?

A

First singly, then pairing up

36
Q

What does electronic configuration determine?

A

The chemical properties of an element

37
Q

What provides evidence for the existence of quantum shells?

A

Atomic Emission Spectra

38
Q

What provides evidence for the existence of quantum shells AND the group to which the element belongs?

A

Successive Ionisation Energies

39
Q

What provides evidence for electron subshells?

A

First Ionisation Energies

40
Q

If an electron takes in energy from its surroundings it is…

A

…excited to a higher energy level

41
Q

When an electron drops down tot a lower energy level, it…

A

…releases this energy in the form of a photon with energy matching the gap.

42
Q

When do the energy levels get closer together?

A

As energy/frequency increases

43
Q

What suggests that electrons exist at very specific energy levels?

A

There is no ‘inbetween’ amount of energy, electrons exist at very specific energy levels

44
Q

What is ‘first ionisation energy’?

A

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
Q

What is the equation for the first ionisation energy for sodium?

A

Na(g) —–> Na+(g) + e-

46
Q

Why does Atomic Radius affect the First Ionisation Energy?

A

The more shells and atom has, and therefore the further away the outer electrons are from the nucleus, the less attraction they experience

47
Q

Why does Nuclear Charge affect the First Ionisation Energy?

A

The more protons, the greater the nuclear charge, and the greater the attraction felt bu the electrons

48
Q

Why does Electron Shielding affect the First Ionisation Energy?

A

As the number of electrons between the outer electrons and the nucleus increases, the outer electrons feel less attraction towards the nucleus

49
Q

What happens to first ionisation energies going down a group?

A

It decreases

50
Q

What happens to first ionisation energies going across a period?

A

They generally increase

51
Q

What happens to first ionisation energies between Groups 5 + 6, and why?

A

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
Q

What happens to first ionisation energies between Groups 2 + 3, and why?

A

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
Q

What trends are there in the periodic table?

A
  • melting and boiling points
  • atomic radius
  • ionisation energies
54
Q

Why do metallic bonds get stronger across the metals?

A

Because there are more electrons per positive ion (2+ charge means there’s 2 delocalised electrons for each positive ion

55
Q

How does atomic radius change across a period?

A

It decreases, because as the nuclear charge of the atom increases, the outer shells are pulled inwards

56
Q

How does electron shielding change across a period?

A

It doesn’t, because they’re still filling the same quantum shell

57
Q

How does nuclear charge change across a period?

A

It increases, because the number of protons increases

58
Q

How do melting/boiling points change across a period?

A

They increase until after the macro-molecular structures, London forces affect this.

Chem A Level (19 decks)

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