General Chemistry 1

Study Notes

General Chemistry 1 - Quiz 2

Chemical Bonding Stability: Dictated by Electronic Configuration
Valence Electron: Electrons in the outermost energy level, not atomic number, first, or second energy levels.
Octet Rule: Describes the stability of elements during chemical bonds. Many elements' stability is achieved by having eight valence electrons.
Lewis structures: Helps predict the bonding and arrangement.
Electrons surrounding an Oxygen atom (OF2): 2 lone pairs of electrons
Violates Octet Rule Element: AsF5
Completely Filled Valence Electron Atoms: Radium
Nitrogen's Octet Completion: Needs 3 electrons to gain an octet.
Octet Rule Completion for Reactants: Atoms react with each other to attain 8 electrons in their outermost energy level.
Octet Rule Formulator: Gilbert N. Lewis
Covalent Bonding: A type of chemical bonding where atoms share electrons to achieve stability.
Polar molecules: Have unequal sharing of electrons where the shared electrons are not equally shared.
Nonpolar molecules: Equal sharing of electrons where the shared electrons are equally shared.
Lone pairs/unshared pairs: Unshared electrons are on an atom in a molecule.
Number of covalent bonds (Carbon): 4
Shape (Methane): Tetrahedral
Shapes with 2 electron pairs: Linear & Angular
Shape with 2 electron pairs and 2 lone pairs (bond angle 109.5°): Trigonal Pyramidal
Octahedral Shape (bond angle): 90°
Trigonal Planar (bond angle): 120°
Molecular Structure of Water (H₂O): Bent shape, 104.5° bond angle.
Molecular shape with a bond angle of 120° (choose from 27 choices): Not possible for determination from the given text.
Drawing AB3E molecules: Use Lewis Electron Dot Diagram