Elements of group 6A, compared to 5A, require less ionization energy due to the paired electrons of 6A.

But a question arises: why does group 7A, compared to group 6A, require more ionization energy in spite of the paired electrons in group 7a too.

Regardless of the general trend that the ionization energy increases as we go from left to right in periods, why didn't we apply the same procedure as the first comparison?


Question: What are the best tips for saving money as a university student?
Answer: Get a decent job while at university - it will make all the difference. And calculate your budget and don't spend more than your budget allows

Worked for me. That was the time when I had the greatest disposable income - all gone downhill since :-)