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A-level Chemistry: 3.1.1 Atomic Structure Part 2

Chemistry27 CardsCreated 2 months ago

This deck covers key concepts in atomic structure, focusing on mass spectrometry, electron configuration, and ionisation energy. It includes detailed questions and answers to help students understand and retain important chemistry principles.

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Describe the step ion drift in mass spectrometry (TOF)


  • Ions enter region with no electric field so they just drift through it

  • Lighter ions will drift faster than heavier ions

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Key Terms

Term
Definition

Describe the step ion drift in mass spectrometry (TOF)


  • Ions enter region with no electric field so they just drift through it

  • Lighter ions will drift faster than heavier ions<...

Describe the step detection in mass spectrometry (TOF) & state how abundance is measured

  • Lighter ions travel at higher speeds = reach detector in less time than heavier ions

  • Positive ions collected at detector

    ...
Describe the step data analysis in mass spectrometry (TOF)
Signal from detector is sent to a computer which generates a mass spectrum
What does the y-axis of mass spectrum represent?
Abundance of ions
What does the height of each peak give on the mass spectrum?
Relative isotopic abundance
If the sample is an element, what does each line represent on the mass spectrum?
A different isotope of the element
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A-level Chemistry: 3.1.1 Atomic Structure Part 2
TermDefinition

Describe the step ion drift in mass spectrometry (TOF)


  • Ions enter region with no electric field so they just drift through it

  • Lighter ions will drift faster than heavier ions

Describe the step detection in mass spectrometry (TOF) & state how abundance is measured

  • Lighter ions travel at higher speeds = reach detector in less time than heavier ions

  • Positive ions collected at detector

  • Causing current to flow / detected electrically

  • Abundance measured: idea that current depends on number of ions hitting detector

Describe the step data analysis in mass spectrometry (TOF)
Signal from detector is sent to a computer which generates a mass spectrum
What does the y-axis of mass spectrum represent?
Abundance of ions
What does the height of each peak give on the mass spectrum?
Relative isotopic abundance
If the sample is an element, what does each line represent on the mass spectrum?
A different isotope of the element
What does the x-axis on the mass spectrum represent?
'mass/charge' ratio (m/z)

Describe how to work out the relative atomic mass from mass spectrum (4)

  1. Spectrum gives relative abundance (of isotopes) & m/z (mass/charge ratio)

  2. Multiply m/z by relative abundance for each isotope

  3. Sum these values

  4. Divide by the sum of the relative iostopic abundances

Why do elements with isotopes produce more than one line in a mass spectrum?
∵ isotopes = different masses
Describe how you can use mass spectrometry to identify elements
You can see if the sample being analysed has the same relative abundances of isotopes
Explain how you use mass spectrometry to identify molecules
mass/charge ratio (of peak) = relative molecular mass of molecule
Electrons have ____ ______ & move around nucleus in certain regions of atom called ____________
Electrons have fixed energies & move around nucleus in certain regions of atom called shells/energy levels
Each shell is given a number called ____ ____ _____
principal quantum number
What is the principal quantum number?
2(n2)
The further away a shell is from nucleus, the _ its energy & the ____ its principal quantum number
higher its energy + larger its principal quantum number
Electrons in same the shell ___ have same energy
DON'T
Shells divided up into sub-shells which have ____ ______ energies
slightly different
Sub-shells have different no. of orbitals which can hold up to ___ electrons
2
2 electrons in each orbital…
spin in opposite directions
Electrons fill up ___ energy sub-shell 1st
Electrons fill up lowest energy sub-shell 1st
Why do electrons fill orbitals singly before they start sharing?
∵ electrons repel each other
Electron configuration: Give 2 examples of transition metals behaving unusually
Chromium (Cr) & copper (Cu) = donate 1 of their 4s electrons to 3d sub-shell
Electron configuration: what happens when transition metals become an ion?
They lose 4s electrons before their 3d electrons
Groups 4-7 can electrons when they form ____
Groups 4-7 can share electrons when they form covalent bonds
Why are the gases in Group 0 inert?
∵ completely filled s & p sub-shells
Why does Chromium (Cr) & copper (Cu) donate 1 of their 4s electrons to 3d sub-shell?
∵ they're happier with a more stable full or half-full d sub-shell
Define first ionisation energy
Enthalpy change when 1 mole of gaseous 1+ ions is formed from 1 mole of gaseous atoms