Title | Periodic Trends - Notes |
---|---|
Course | Concepts In Physics & Chem |
Institution | Emory University |
Pages | 2 |
File Size | 50.7 KB |
File Type | |
Total Downloads | 86 |
Total Views | 161 |
Notes...
Atomic Radius (size of neutral atom)
Periodic Trend: o Decreases from left to right across a period o Protons are added to the nucleus and electrons are added to the same principal energy level o As force of attraction between nuclei and electrons increases, the size of the atoms decreases. Group Trend: o Increases as you go down o Caused by more energy levels of electrons and therefore more electron shielding
Ionic Radius (size of charged ion)
Periodic Trend: o Decreases from left to right across a period o Cation radius decreases As you go left to right, cations have more attraction (smaller size because more protons than electrons) o Anion radius decreases The anions have a larger size than the cations, but also decrease left to right Group Trend: o Increases as you go down o Each row adds a new electron shell
First Ionization Energy (amount of energy needed to remove an outer electron from an atom and make it into an ion)
Periodic Trend: o Increases from left to right o More protons in the nucleus pulling in electrons, so it requires more energy to remove an outer electron o Outer electrons have more attraction to the nucleus Group Trend: o Decreases as you move down o More energy levels and more shielding o Outer electrons have less attraction to the nucleus
Effective Nuclear Charge (positive charge felt by the outermost/valence electrons)
Periodic Trend: o Increases across a period
o More protons with no accompanying increase in shielding Group Trend: o Decrease down a group o The number of protons increases but more shielding down a group...