I'm having a hard time understanding the first ionization energy exception between the s and p block. My book tries to explain it but I feel like it is a poor explanation. It states that the ionization energy for Boron is actually lower than Beryllium because of the fact that the p block is higher in energy. Is there another explanation someone can provide because this doesn't really explain why. If this was the case then the entire p block should have a lower ionization energy. I understand why ionization energy increases as you approach the right side of the periodic table due to an increase in Zeff, but I'm not sure what is creating this exception between the s and p block. Also I'm not sure why a higher energy would result in less energy required to remove an electron. Wouldn't something with more energy be more difficult to remove?