No, I do not have a chart of trends in my text.

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Discussion Overview

The discussion revolves around the properties of ionic compounds KF, NaF, and RbCl, specifically focusing on ionic bond lengths, lattice energy, and melting points. Participants explore the relationships between these properties and the periodic trends that influence them.

Discussion Character

  • Homework-related
  • Conceptual clarification
  • Debate/contested

Main Points Raised

  • One participant questions whether NaF has the shortest ionic bonds and highest lattice energy, while RbCl has the lowest melting point.
  • Another participant suggests that the original poster has not demonstrated sufficient effort in their inquiry and encourages them to refer to their chemistry textbook for trends.
  • A participant expresses confusion about the relationship between bond length and lattice energy, suggesting that shorter bonds correlate with higher lattice energy.
  • Another participant reiterates the reasoning that as one moves up and to the right on the periodic table, ionic bonds become stronger, leading to the choice of NaF.
  • There is a mention that melting points are related to intermolecular forces, with the implication that stronger bonds result in higher melting points.
  • One participant acknowledges a lack of understanding regarding the provided resources and expresses gratitude for assistance.

Areas of Agreement / Disagreement

Participants do not reach a consensus on the relationships between ionic bond lengths, lattice energy, and melting points. There are competing views on how these properties are determined and interpreted.

Contextual Notes

Some participants reference periodic trends and factors influencing bond lengths and melting points, but there are unresolved assumptions regarding the definitions and relationships of these properties.

lorka150
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Out of KF, NaF, and RbCl, does NaF have the shortest ionic bonds as well as highest lattice energy, and RbCl have the lowest melting point?

Thanks
 
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It doesn't look like you've done much work on this... Read your chemistry book it will tell you all of these trends in the corresponding sections. You need to show at least some effort even if its not the correct answer.
 
I did, sorry. I just didn't type it all. I read through the trends, and just want to make sure I interpreted them correctly. I was under the impression tha the shorter bonds and highest lattice energy would be the same, because the increased lattice = stronger bonds, and the strong bonds are a high energy, and the shorter they are, the stronger they are.

Sorry that it was taken that way. GOsh, I feel stupid!
 
lorka150 said:
Out of KF, NaF, and RbCl, does NaF have the shortest ionic bonds as well as highest lattice energy, and RbCl have the lowest melting point?

Thanks
What do you think, and why? Show your attempt to solve this problem.
 
Hi Geoff
I explained my reasoning in the message above you. I thought that the highest lattice and shortest bonds correspond, and I know that as you move up and to the right that they are at the strongest - therefore because F is the farthest and Na is higher than K, I chose NaF.

For the lowest melting point, I was under the impression it would be the opposite (descendig and towards the left).
 
lorka150 said:
Hi Geoff
I explained my reasoning in the message above you. I thought that the highest lattice and shortest bonds correspond, and I know that as you move up and to the right that they are at the strongest - therefore because F is the farthest and Na is higher than K, I chose NaF.

For the lowest melting point, I was under the impression it would be the opposite (descendig and towards the left).
Bond length is determined by a number of factors, which, as Steve said, should be detailed in your text. Consider bond lengths of each ion and electronegativities. This page might aid your understanding.

Melting point is directly proportional to intermolecular forces. The more energy it takes to break the bonds between molecules, the higher the melting point.
 
Thanks for the link. I do not understand it, but thank you for your help.
 
lorka150 said:
Thanks for the link. I do not understand it, but thank you for your help.
Well, we'll do what we can until you do understand. First of all, do you have a chart of trends in your text?
 

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