CHEM 101 Lecture Notes - Lecture 13: Atomic Radius, Fluorine, Electron Configuration

• School: University of Victoria
• Department: Chemistry
• Course: CHEM 101
• Professor: Neil Burford

Document Summary

Size increases moving down a group due to the increasing number of energy levels. Size decreases across a period because the nuclear charge increases and the electrons are pulled closer to the nucleus. Ionic size because they have less electron repulsion. Cations (positively charged ions) are smaller than their corresponding atom. Anions (negatively charged ions) are smaller than their corresponding atom. The greater the magnitude of the ion"s charge, the greater the difference in size because they have more electron repulsion. Ionization energy values are positive , because the removal of an electron is an. Ionization energy decreases moving down a group because the electrons are endothermic reaction farther away from the nucleus, and experience less attractive nuclear force. Ionization energy increases across a period because the electrons experience a higher nuclear charge and are more attracted to the nucleus. Exceptions: beryllium has a higher ionization energy than boron, and nitrogen has a higher ionization energy than oxygen.