Chapter 5-7 Flashcards
Lattice
A three dimensional array of cations and anions
Lattice Energy
The amount of energy required to convert one mole of ionic solid to its constituent ions in the gas phase
Lattice Energy-
Trends
- Higher Charges = Higher Lattice Energy
- Smaller Ions = Higher Lattice Energy
Naming Ionic Compounds
(Cation) + (Anion) drop the -ion +ide
Naming Singular Ions
- Add -ide if it is an anion
- If the charge is more than one, add a roman numeral
Diatomic
A molecule containing two atoms/compounds
Homonuclear
Molecule containing two same atoms/compounds
Heteronuclear
Molecule containing two different atom/compound
Polyatomic
Molecule containing more than two atoms/compounds
Naming Molecular Compounds
- Add a prefix
- mono- is usually omitted for the cation
Naming Acids
hydro + element (drop -ide) + ic + acid
Oxoanions
Anions that have more than zero Oxygen atoms. Ends in -ate
Oxoacids
An acid consisting of one or more ionizable protons and oxoanion
Polar
Electrons not shared equally
Electronegativity
Ability of an atom in a compound to draw electrons to itself
Rules for Electronegativity
- delta E = 0.5 = non polar
- delta E = 0.5 - 2.0 = polar
- delta E = 2.0 + = ionic
Dipole Moment
Quantitative Measurement of the polarity of the bond
Dipole-Dipole Force
Attraction between two elements in a polar molecule
London Dispersion Force
A temporary dipole force.
The weakest Intermolecular force
Formal Charge
(Number of Valence Electrons) - (number of lone electrons) - (number of bonds)
Ion Dipole Force
Attraction between ions and polar molecules
Paramagnetic
A molecule that contains unpaired electrons (weakly attracted to magnetic forces)
diamagnetic
A molecule that does not contain unpaired electrons ( weakly repelled to magnetic forces)
Bond Order
{(# of bonding)-(# of anti-bonding)}/2
Localized
Fixed electrons that do not participate in resonance
Delocalized
Unfixed electrons that do participate in resonance
Hybridization Rules
2 = sp
3 = sp2
4 = sp3
5 = sp3d
6 = sp3d2
