CHEM 1030- Midterm Exam Guide - Comprehensive Notes for the exam ( 13 pages long!)

• School: Auburn University
• Department: Chemistry
• Course: CHEM 1030
• Professor: Allie Brandriet

Document Summary

Electron configuration: each orbital can take on two electrons, practice problem: br = 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p5, however!!!! Quantum numbers: spin quantum number (ms): either +1/2 or -1/2 depending on if (in orbital notation) the electron has more positive spins (up arrows) or negative spins (down arrows) Ions: cation, remove from the highest n-value first, remove electrons, anion, add electrons, add to next orbital. Increases as you go left on a row: effective nuclear charge increases as move left to right, electrons feel positive charge shrinking the size. Ionic size: cations are smaller because they feel the positive charge more (less electrons, anions are larger because there are more electron-electron repulsions expanding the atom. Ionization energy: takes energy to break attraction and move an electron out, energy required is positive. Chem 1030 lecture 12 finishing chapter 3 and starting chapter 4.