CHEM 1E03 Lecture Notes - Lecture 6: Diamagnetism, Noble Gas, Paramagnetism

• School: McMaster University
• Department: Chemistry
• Course: CHEM 1E03
• Professor: Randall Dumont; Linda Davis

Document Summary

See if there are unpaired electrons in electron configuration. When you ionize it you take an electron away. Therefore it is harder to take an electron from n. Upon ionization you create a half-filled subshell from a full. Atoms that go from half-filled to filled are less likely to be ionized: all energies correspond to a scale that at zero results ionization e. **groups 1/13 and 15/16 this trend is reversed. Ca (filled), as (half) therefore this order is correct. S < p is correct (half), mg < al (incorrect - filled: each ionization energy takes more energy, as there becomes a greater jump. I1 < i2 << i3 < i4 < i5 < i6: a group 2 element because there is a much larger jump after the second ionization (from the s orbital to the p). Electron affinity adding electrons to atoms (always negative) General trend is the same as ionization energy.