Understanding Atomic Electron Binding Energy

In summary, the conversation is about a question regarding the first ionisation energy of chlorine and sulphur. The expert summarizer advises to get straight to the point and keep the answer short and concise in order to earn the full two marks. The expert also points out that understanding the subject is more important than simply answering test questions. The expert also provides a hint about considering nuclear charge and shielding effect when determining the binding energy of an atomic electron.
  • #1
rpatel
7
0
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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  • #2
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.
 
  • #3
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
 
  • #4
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
 
  • #5
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.
 

Related to Understanding Atomic Electron Binding Energy

1. What is ionisation energy?

Ionisation energy is the amount of energy required to remove an electron from an atom or molecule, resulting in the formation of an ion.

2. Why is ionisation energy important?

Ionisation energy is important because it helps us understand the chemical reactivity and stability of atoms and molecules. It also plays a crucial role in the formation of chemical bonds and the behavior of elements in different chemical reactions.

3. How is ionisation energy measured?

Ionisation energy is measured in units of energy such as joules (J) or electron volts (eV). It can be measured experimentally by using various techniques, such as spectroscopy, mass spectrometry, and electron impact ionisation.

4. What factors affect ionisation energy?

The main factors that affect ionisation energy include the atomic or molecular structure, the number of protons in the nucleus, and the distance between the outermost electron and the nucleus. Other factors such as shielding effect, electron configurations, and nuclear charge can also influence the ionisation energy of an atom or molecule.

5. How does ionisation energy vary across the periodic table?

Ionisation energy generally increases as you move from left to right across a period in the periodic table. This is because the number of protons and the nuclear charge increases, making it more difficult to remove an electron. It also decreases as you move down a group due to the shielding effect and the increasing distance between the outermost electron and the nucleus.

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