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Chemistry /Edexcel A Level Chemistry: 1: Atomic Structure and the Periodic Table Part 2

Edexcel A Level Chemistry: 1: Atomic Structure and the Periodic Table Part 2

Chemistry28 CardsCreated 11 days ago

This deck covers key concepts related to atomic structure and the periodic table, including electron configurations, ionisation energies, and periodic trends.

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How many electrons fill the second quantum shell?

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Key Terms

Term
Definition
How many electrons fill the second quantum shell?
8
How many electrons fill the third quantum shell?
18
How many electrons fill the fourth quantum shell?
32
Two electrons in the same orbital must have opposite…
…spins
In what order do electrons fill subshells?
First singly, then pairing up
What does electronic configuration determine?
The chemical properties of an element
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Edexcel A Level Chemistry: 1: Atomic Structure and the Periodic Table Part 2
TermDefinition
How many electrons fill the second quantum shell?
8
How many electrons fill the third quantum shell?
18
How many electrons fill the fourth quantum shell?
32
Two electrons in the same orbital must have opposite…
…spins
In what order do electrons fill subshells?
First singly, then pairing up
What does electronic configuration determine?
The chemical properties of an element
What provides evidence for the existence of quantum shells?
Atomic Emission Spectra
What provides evidence for the existence of quantum shells AND the group to which the element belongs?
Successive Ionisation Energies
What provides evidence for electron subshells?
First Ionisation Energies
If an electron takes in energy from its surroundings it is…
…excited to a higher energy level
When an electron drops down to a lower energy level, it…
…releases this energy in the form of a photon with energy matching the gap.
When do the energy levels get closer together?
As energy/frequency increases
What suggests that electrons exist at very specific energy levels?
There is no 'inbetween' amount of energy, electrons exist at very specific energy levels
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
What is the equation for the first ionisation energy for sodium?
Na(g) -----> Na+(g) + e-
Why does Atomic Radius affect the First Ionisation Energy?
The more shells an atom has, and therefore the further away the outer electrons are from the nucleus, the less attraction they experience
Why does Nuclear Charge affect the First Ionisation Energy?
The more protons, the greater the nuclear charge, and the greater the attraction felt by the electrons
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
What happens to first ionisation energies going down a group?
It decreases
What happens to first ionisation energies going across a period?
They generally increase
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 from the new shell
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

What trends are there in the periodic table?

  • melting and boiling points

  • atomic radius

  • ionisation energies

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
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
How does electron shielding change across a period?
It doesn't, because they're still filling the same quantum shell
How does nuclear charge change across a period?
It increases, because the number of protons increases
How do melting/boiling points change across a period?
They increase until after the macro-molecular structures, London forces affect this.