Ionization energy: period trend | Atomic structure and properties | AP Chemistry | Khan Academy | Summary and Q&A

TL;DR

Ionization energy increases as you move across the periodic table due to the increase in effective nuclear charge.

Key Insights

• ❓ Ionization energy increases as you move across a period.
• 🧑‍🏭 Effective nuclear charge is the main factor affecting ionization energy.
• ❓ The electron configuration and orbital interaction can influence ionization energy.
• 😘 Boron has a lower ionization energy compared to beryllium due to extra shielding.
• 🤯 Oxygen has a lower ionization energy compared to nitrogen due to electron-electron repulsion in the two p orbital.
• 🛀 General trend shows an increase in ionization energy from nitrogen to neon.
• 😑 Ionization energy is the energy required to remove an electron from an atom or ion.

Transcript

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Questions & Answers

Q: What is ionization energy?

Ionization energy is the energy required to remove an electron from a neutral atom or ion.

Q: Why does ionization energy increase as you move across a period?

Ionization energy increases due to the increase in effective nuclear charge, which pulls the electrons closer to the nucleus, making it harder to remove them.

Q: How is effective nuclear charge calculated?

Effective nuclear charge is calculated by subtracting the average number of inner electrons from the number of protons.

Q: Why does boron have a lower ionization energy than beryllium?

Boron has a lower ionization energy because the electron in its two p orbital is shielded by the two s electrons, making it easier to remove.

Summary & Key Takeaways

• Going across a period from lithium to neon, there is a general increase in ionization energy.

• The increase in ionization energy is due to the increase in effective nuclear charge.

• Effective nuclear charge is calculated by subtracting the average number of inner electrons from the number of protons.