Ionic Radius: Ordering Cl-, Be2+, Li+, F-, H-

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SUMMARY

The discussion centers on the ordering of ionic radii for the ions Cl-, Be2+, Li+, F-, and H-. The proposed order from largest to smallest is Cl-, H-, F-, Li+, Be2+. However, there is contention regarding the placement of H- due to its unique properties as a hydride. The chemistry teaching assistant (TA) suggests that H- should be ranked last, indicating a need for further clarification on ionic radius trends.

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  • Understanding of ionic radius and periodic trends
  • Familiarity with the concepts of cations and anions
  • Knowledge of hydride properties in chemistry
  • Basic grasp of the periodic table and element positioning
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  • Research the ionic radius of hydrides and their placement in periodic trends
  • Study the differences between cationic and anionic radii
  • Examine the factors affecting ionic size, including charge and electron configuration
  • Learn about the methods used to measure ionic radii in various compounds
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ubiquinone
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Hi I have a question involving periodic trends. This time the trend is on ionic radius. I'm not sure I got this right so I was wondering if anyone here may please offer their advice. Thank you!

Question:
Order each of the following ions according to largest to smallest.
A. [tex]Cl^-[/tex]
B. [tex]Be^{2+}[/tex]
C. [tex]Li^+[/tex]
D. [tex]F^-[/tex]
E. [tex]H^-[/tex]
 
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Well have you read about the trend? It will make a lot more sense if you have read the information.
 
I have read the trend and I think the answer should be Cl-, H-, F-, Li+, Be2+.

However, I am not sure about this, because of the hydride. I heard that there is some controversy as what is the actual ionic radius. I just wanted to see if anyone here came up with the same order.

However, my chem TA disagreed and thinks the hydride should be last. What do you guys think?
 

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