Chapter 5 Covalent Bonds and Molecular Structure
A bond that results from the sharing of electrons between atoms (valence electrons)
The unit of matter held together by covalent bonds. The electrons from 1 atom are attracted to the protons of another atom.
Graphic representation of a molecule showing atoms, bonds and their relative arrangement.
Written representation of a molecule's atoms.
Bond Dissociation Energy
The energy needed to completely break a covalent bond in a molecule in the gaseou state.
Ionic Compound Properties
High melting point in solids, dissolve in water to form ions, solutions of ions are good conductors of electricity
Covalent Compound Properties
Low melting points, contains solids liquids and gases, strong internal covalent bonds but weak intermolecular bonds.
How hard an atom "pulls" on the electrons. Has to do with the atoms affinity for electrons.
Periodic Trends of Electronegativity
F pulls hardest (top right), Cs pulls least (bottom left)
If the electrons are pulled to one side more than the other, one side of a bond has more negative (d-) while the other has more positive (d+)
Naming Molecular Compounds
1. Cation like comes first, then anion like.
2. Cation like keeps elemental name
3. Anion like gets "ide" ending
4. Prefixes are used to specify number of each atom (anion)
Lewis Dot Structures
Drawing of molecules where electrons are shown as dots around elemental symbols
Lone pairs of electrons around their respective atom.
When one Lewis structure is not enough. Example O3
Square brackets around molecule with double-sided arrow to signify resonance
A convenient way of assigning charges to individual atoms in a molecule. =column - things
Valence Shell Electron Pair Repultion Theory
VSEPR. All pairs of electrons get the maximum amount of space available.
Two charge system
Three charge system
Four charge system
Five charge system
Six charge system
Three charge system with two atoms around central atom and one lone pair of electrons
Four charge system with three atoms around central atom and one lone pair of electrons
Four charge system with two atoms around center atom and two lone pairs of electrons
Five charge system with four atoms around central atom and one lone pair of electrons
Five charge system with three atoms around central atom and two lone pairs of electrons
Five charge system with two atoms around central atom and three lone pairs of electrons
Six charge system with five atoms around central atom and one lone pair of electrons
Six charge system with four atoms around central atom and two lone pairs of electrons
Six charge system with three atoms around central atom and three lone pairs of electrons
Six charge system with two aroms around central atom and foour lone pairs of electrons
Valence Bond Theory
Used to describe the way electrons are shared in covalent bonds
Result from head-on overlap of atomic orbital between 2 nuclei
Result from edge on (sideways) overlap of atomic orbitals (d or p orbitals)
Molecular Orbital Theory
Atomic orbitals combine to form these orbitals. Has two types: bonding and anti bonding