Chapter 1 - Structure, Bonding, Hybridization Flashcards
Ionic Compound
Elements achieve an octet configuration by gaining or losing electrons. Ions form when an electron is gained or lost from a neutral atom. Ions are held together by electrostatic attraction.
Ionic Bond
Ions are held together by an electrostatic attraction.
Covalent Bond
Bond formed by sharing electrons between atoms.
Coavlent Molecule
Neutral collection of atoms held together by covalent bonds.
Lewis Structures
Electron-Dot Structures
Valence shell electrons of an atom are represented as dots. Dots represent covalent bonds.
Kekule Structures
Line-Bond Structures
Two-electron covalent bond is represented by a line.
Lone-Pair Electrons
Valence-shell electron pairs not used for bonding.
Valence Bond Theory
Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals. Electrons are paired in overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together.
Sigma Bond
Bond formed by a head-on overlap of two atomic orbitals along a line drawn between the nuclei.
sp3 Hybrid Orbitals
A hybrid orbital derived from the combination of an s atomic orbital with three p atomic orbitals. Form equivalent atomic orbitals with a tetrahedral orientation.
Bond Angle
The angle formed between two adjacent bonds.
Approximate Tetrahedral Bond Angle
109.5 Degrees
Approximate Planar Bond Angle
120 Degrees
sp2 Hybrid Orbitals
A hybrid orbital derived by combination of an s atomic orbital with two 2p atomic orbitals. One p orbital remains non-hybridized.
Bond Strength (Single vs. Double)
Carbon-carbon double bond is shorter and stronger than carbon-carbon single bond.