Chemistry 2213A/B Chapter 1: 1.1-1.7 COVALENT BONDING AND SHAPES OF MOLECULES

• School: Western University
• Department: Chemistry
• Course: Chemistry 2213A/B
• Professor: Nicholas Hudson

Document Summary

1. 1: how do we describe the electronic structure of atoms. Nucleus: composed of protons and neutrons, densely packed. Electrons: do not move freely in space, confined by principle energy levels (shells) Shells (1,2,3,4): divided into subshells s, p, d, f. Orbital: region of space that can hold 2 electrons. Ground-state electron configuration: the electron configuration of the lowest. Ground-state electron configuration: the electron configuration of the lowest energy for an atom, molecule, or ion. Rule 1: orbitals fill in order of increasing energy level. Rule 2: orbitals can hold up to two electrons with their spins paired (opposite spin) Rule 3: when orbitals of equivalent energy are available, but not enough electrons to fill them, we add one electron to each equivalent orbital before adding a second. Electron configuration: description of the orbitals electrons in the atom occupy. Valence electrons: electrons in the outermost shell of an atom. Valence shell: the outermost shell of an atom.