Chemistry Part B Final Exam Review Topics
Chapters 3 & 4
Temperature – a measure of the average kinetic energy of the particles
To convert from Celsius to Kelvin add 273
Qualitative Quantitative –
Accuracy –
Precision Volume units
Mass units
Conversions: Know the following prefixes: micro – u – 1/1000000
milli – 1/1000th
Centi – 1/100th
deci - 1/10th
kilo – 1000 times bigger
Chapter 6
Oxidation numbers (be able to determine the charge by using the Periodic
table) Example: Na +
Be able to find oxidation numbers for polyatomic ions by using a chart
Example: hydroxide is OHWriting correct chemical formulas
Roman numerals tell the oxidation number for a metal because some metals
may have more than one oxidation number Example: Pb(II) is Pb2+ while
Pb(IV) is Pb 4+
Naming compounds properly: ie: cation (metal) goes first, anion (negative
ion goes second). Change ending to “ide” if the anion is a single element.
If the anion is a polyatomic ion, it keeps its name as all polyatomic ions keep
their names.
For nonmetals, use prefixes since they can share bonds in different ways
1 – mono 2 – di 3 – tri 4 - tetra 5 – penta 6- hexa 7- hepta
8 – octa 9 – nona 10 –deca
Chapter 7
Molar mass
Moles and mole conversions
Avogadro’s number 6.02 x 1023 units
1 mole of any substance has 6.02 x 1023 units (atoms, molecules, etc)
Moles to grams, etc.
Moles to liters, etc
1 mole of any gas at STP has a volume of 22.4 L
Molarity is all about the concentration of a solution
A 1M solution of HCl has one mole of HCl (36.5 grams) dissolved in 1 Liter
solution of water. A 2 M solution has 2 moles per liter of solution, etc. 500
mL of a 1M solution of HCl would have ½ of 36.5 grams (18.25 g) of solute
because 500 mL is ½ L.
% Composition – be able to calculate
Chapter 8
Reactants Products Skeleton equations – writing them properly
Balancing chemical equations by using coefficients
5 Types of chemical reactions (be able to recognize them when looking at a
chemical equation)
Chapter 15
Ion Ionic bonds Melting and boiling points are higher in ionic compounds compared with
molecular compounds
Know the difference between a formula unit (has ionic bonds) and a
molecular compound (has covalent bonds and lower melting points)
Chapter 16
Covalent bonds Single vs. double vs. triple bond
Lewis dot structures for molecules
Electronegativity –
Polar bonds and nonpolar bonds
Table of electronegativity and bond types on page 462 will help
Polar molecules and nonpolar molecules
Intermolecular forces: London dispersion forces, dipole – dipole, Hydrogen
bonds (strongest)
Acids have hydrogen in them. Example: HCl dissolved in water is
hydrochloric acid.
Diatomic molecule -
Example: Cl2