Chem Study Guide #3
Logan Rafferty
ChemH
Bonding and Nomenclature
Intermolecular Forces- a force between molecules
Intramolecular Force- a force between atoms
Van der Waals Forces
Dispersion- interaction of the electron clouds of
neighboring molecules that produce temporary
oppositely charged regions in neighboring
molecules (holds nonpolar molecules)
Hydrogen Bonding
Bond between hydrogen in one molecule and a
highly electronegative nonmetal(N,F,O) from a
neighboring molecule (very strong)
Dipole-dipole- attraction between the positive end
of one polar molecule and the negative end of a
neighboring polar molecular (hold polar
molecules) (stronger than dispersion)
Naming compounds- Ionic Compounds- Metal + Nonmetal (cation-metal) (anion-non-metal)
Type 1: metal present only forms one type of cation(one oxidation state)
1.Write the name of the metal
2. Take the first part of the nonmetal’s name and add ideType 2: metal present can form two (or more) cations that have different charges (more than one oxidation
states)
1.Wrtie the name of the metal first
2.Specify the charge of the cation by a Roman numeral in parentheses (oxidation state)
3. Take the first part of the nonmetals name and add ide
Type3: compound contains a polyatomic ion (metal () __ polyatomic ion)
1. See if the cation has more than one oxidation state
2. Name of polyatomic ions are in Table E
3. Write the same of the polyatomic ion followed by a space then the name of anion ending in ide
(most of the time the polyatomic ion is anion but if it’s the cation do this)
Molecular Compounds- two nonmetals (P4O6)
1. Name the first element using full name
2. Name the second element but change ending to “-ide”
3. Use prefixes to denote the number of atoms
Molecular Geometry
How to use VSEPR
1.Draw the Lewis structure of molecule
2.Locate Central Atom
3. Count the number of shared and unshared pairs
of electrons (double and triple bonds= one share
pair)
4. Use Chart
Molecular Lewis Structure and Structural Formula
1.Count the total # of valance electrons for each
atom and add together
2.Each atom must have 8 (or 2) electrons
surrounding it
3.Every bond represents 2 electrons
4. If electrons are shared between 2 atoms than
those electrons count for both atoms