Trends in the sizes of ions (ionic radii) Q1. What is the trend as we go down a group? Q2. How can...
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Transcript of Trends in the sizes of ions (ionic radii) Q1. What is the trend as we go down a group? Q2. How can...
![Page 1: Trends in the sizes of ions (ionic radii) Q1. What is the trend as we go down a group? Q2. How can we explain the trend?](https://reader035.fdocuments.net/reader035/viewer/2022081603/5697bfc11a28abf838ca418e/html5/thumbnails/1.jpg)
Trends in the sizes of ions (ionic radii)
Q1. What is the trend as we go down a group?
Q2. How can we explain the trend?
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Q3. How would the atomic radius compare with the ionic radius for a CATION and its’ parent atom?
E.g. Na+ ionic radius and the Na atomic radius
Q4. How would the atomic radius compare with the ionic radius for an ANION and its’ parent atom?
E.g. Br- ionic radius and the Br atomic radius
Data on next slide.
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Q5. What trend would you expect in ionic radii across a period?
Eg. Period 3 Na Ar
Use the extract from the Edexcel Data Booklet to find the ionic radii of the elements in Period 3:
Ion: Na+ Mg2+ Al3+ Si4+ P3- S2- Cl-1
Radius:(nm)
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Excel chart on next slide
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How can we explain this trend?
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Comparing ionic radii of isoelectronic ions
E.g. Al3+ and N3-
Both have the electron configuration: 1S2 2S2 2P6
Which would be the largest ion? Why?
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Use the data booklet extract to find the ionic radii of three more isoelectronic ions.
Explain the trend in the ionic radii of the ions you choose.
AflAfl
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Typical exam question on trends in ionic radii:
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IONIC BONDING PPQs