Nitrogen (( 1s^2 2s^2 2p^3 )) has exactly one electron in each of the three 2p orbitals (Hund's Rule). This is a half-filled subshell , which is exceptionally stable. Oxygen (( 1s^2 2s^2 2p^4 )) has one 2p orbital with two electrons. The electron-electron repulsion in that paired orbital allows one electron to be removed more easily, lowering the IE.
Worksheet 12 Periodic Trends Ionization Electron Affinity.rar – Successfully decrypted and solved.
Today, we aren't just filling out a worksheet. We are going to visualize the atom as a battlefield. On one side: the (positive pull). On the other: the Electrons (negative shields). Ionization Energy and Electron Affinity are simply two sides of the same coin—measuring how badly an atom wants to hold onto its stuff. Nitrogen (( 1s^2 2s^2 2p^3 )) has exactly
Your worksheet likely touches on the "hiccups" in these trends. For example, groups with (like Nitrogen or the Noble Gases) are extra stable. They might buck the trend because they don't want to disrupt that stability by losing or gaining an electron. Pro-Tip for Worksheet 12
IE generally increases . This happens because the nuclear charge increases (more protons), pulling the electrons closer to the nucleus and making them harder to remove. We are going to visualize the atom as a battlefield
Remember that as atoms get smaller (top right of the table), both IE and EA typically increase.
If you think about the sun, it fuses Hydrogen (Low IE) into Helium (High IE). The worksheet is teaching you that chemistry is the art of moving electrons from places they are weak (Left/Bottom) to places they are strong (Right/Top). full outer shell.
EA generally becomes more negative (increases). Atoms like Halogens (Group 17) have a high "hunger" for electrons because adding one electron gives them a stable, full outer shell.