University:
Georgia Southern University
Course:
CHEM 1310 | Comprehensive General Chemistry
Academic year:

2024
Views:

264

Pages:

1
Author:

Jalen W.

Electron Configurations I. Electron Configuration 1. To get the “noble/full shell look” elements form ions and/or bond with other elements. 2. Ion formation Metals form cations. Cations are positively charge elements because they have more protons than electrons. This is a result of the element LOSING electrons Nonmetals tend to form anions. Anions are negatively charged atoms because they have fewer protons than electrons. This is result of the element GAINING electrons. 3. An electron configuration represents how an atom’s electrons are arranged around the nucleus as dictated by their four quantum numbers (m, l, ml & ms). 4. Orbital arrangement in periodic table 5. Electron configuration/Electron Orbital Diagrams Filling of orbitals is from lowest empty energy level and orbitals upward (Aufbau principle) Inner Core: all electrons not in valance shell (which is the last level filled) Valance Electrons: a. The area where the outermost electrons reside. b. These are the electrons that participate in bonding or the electrons which are lost to form cations c. The valance shell is where electrons enter to form anions 6. When forming cations, which electrons are lost? a. Metals (alkali and alkaline earths) in “s” block loose “s” electrons. b. Metals in “p” block, loose “p” electrons first and the “s” electrons. i. “p” block metals NEVER lose any electrons from the “d” area c. Metals in the “d” block (transitions) loose “s” electrons first and the d” electrons.