Understanding Atomic Electron Binding Energy

AI Thread Summary
The discussion centers on the higher first ionization energy of chlorine compared to sulfur, emphasizing the importance of understanding nuclear charge and the shielding effect. Participants stress that students should demonstrate their approach to the question before receiving help, highlighting the educational value of grasping concepts rather than just seeking answers. The conversation encourages a focus on atomic electron binding energy and the factors influencing it. Overall, the forum promotes a collaborative learning environment where effort and understanding are prioritized. Engaging with the material is essential for mastering the topic.
rpatel
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Why is the first ionisation energy of chlorine is higher than that of sulphur ?

i am having trouble with the questions above please help

thanks


:smile:
 
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Please show your approach to this question first, it's the policy here at PF for you to do so before any of us can help you out.
 
basically this is a 2 mark question. so really you want to get straight to the point. this isn't a long answers. just a short 2 sentence answer. which will earn you 2 marks.

regards
 
rpatel said:
basically this is a 2 mark question. so really you want to get straight to the point. this isn't a long answers. just a short 2 sentence answer. which will earn you 2 marks.

regards

wow what attitude :smile: compare nuclear charge and shielding effect. guess i can't tell you too much since you didnt even try the qn :-p
 
rpatel said:
basically this is a 2 mark question. so really you want to get straight to the point. this isn't a long answers. just a short 2 sentence answer. which will earn you 2 marks.
As semc indicated, the point of learning is to understand the subject, not simply to answer test questions! semc also points you in the right direction. What determines the binding energy of an atomic electron?

And as GCT indicated, we ask that students submit their work/understanding of the problem and we will then assist. Students are expected to show effort.
 

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