What Do I Need to Know for the EOC Chemistry?
*These are really important...
Reporting Category 3: Bonding and Reactions 14 Questions
*Name Ionic Compounds Containing Main Group or Transition
metals, covalent compounds, acids, bases, using IUPAC
nomenclature rules:
 Know your nomenclature rules! Identify the formula as either an—
Ionic compound: metal + nonmetal ions (NaCl, CaCO3, NH4Cl)
Covalent compound: nonmetals ONLY (CO2, CS3, SO3)
Acids: hydrogen + ion (HCl, H2SO4, HNO3, HF)
Bases: metal ion + hydroxide ion (OH-)—NaOH, KOH, Ca(OH)2
 If IONIC: Underline the two ions. Find their names on the periodic table or the
polyatomic ion chart (given to you!). Watch for multiple charge ions!
CaCl2 calcium chloride (note that both ions are monoatomic, and last ends in “ide)
FeCl3 iron III chloride (note that iron is a multiple charge ion, you must use “III”.)
KNO3 potassium nitrate (note that NO3 has the name “nitrate” from your polyatomic chart)

If COVALENT: Use prefixes to name the compounds. You will have to memorize
the prefixes. Memorize at least through 8! (mono, di, tri, tetra, penta, hexa, hepta,
octa). The suffix “ide” is added to the end of the name.
CCl4 carbon tetrachloride (1 carbon and 4 chlorine)
N2O dinitrogen oxide (2 nitrogen and 1 oxygen)
CO
carbon monoxide (don’t use “mono” for the first element, just for the
second one)
 If ACIDS: If there is H and one other element, this is a binary acid. If H and a
polyatomic ion, it is an oxyacid. There are different rules for each!
Binary acids: HCl, HF, H2S, HI, HBr
The name starts with “hydro” + stem of other element + “ide”
HCl = “hydro+chlor+ic”
H2S = “hydro+sulfur+ic”
Oxyacids: HNO3, H2SO4, H3PO4, HCN
Identify the name of the polyatomic ion. If the ion’s name ends in “ate”, or
“ide”, then the name of the acid ends in “ic”. If the ion’s name ends in “ite”, the
name of the acid ends in “ous”.
HNO3 (ion=nitrate), so acid name is = “nitric acid”
HCN (ion=cyanide), so acid name is = “cyanic acid”
H2SO3 (ion=sulfite), so acid name is = “sulfurous acid”
*Write the chemical formulas of common polyatomic ions, ionic
compounds containing main group or transition metals, covalent
compounds, acids, or bases:
 Ionic Compounds: Simple Binary (magnesium nitride)
Find the charge on each element from the Periodic Table and cross!
Remember: Equal and Opposite Charges—Put them together!
 Ionic Compounds: Multiple Charge Ions (Iron III sulfide)
Don’t forget that the Roman numeral is the charge!
Write the symbol and charge and cross: Fe+3 S2-  Fe2S3
 Ionic Compounds: Polyatomic Ions (Magnesium hydroxide)
Write the symbol and charge and cross: Mg+2 (OH)-1  Mg(OH)2
Watch for parentheses! (Ammonium nitrate)= (NH4)+ (NO3)-1 = NH4NO3
 Covalent (Molecular) Compounds: (made only of nonmetals!)
Use the prefixes to tell you how many of each atom. DON’T cross the numbers!
(Carbon disulfide = CS2) or (Trinitrogen dioxide = N3O2)
 Acids: Binary (hydrobromic acid, hydrosulfuric acid)
Identify the element other than hydrogen, and its charge. Hydrogen is
always H+.
Hydrobromic acid: H+1 Br-1 = HBr
Hydrosulfuric acid: H+1 S-2 = H2S
 Acids: Oxyacids (nitric acid, nitrous acid)
Remember: If the acid ends in “ic” and doesn’t start with “hydro”, then the
other ion ends in “ate”. If the acid name ends in “ous” , then the ion name
ends in “ite”. Find the ion on your polyatomic ion chart and write it and its
charge:
Nitric acid = H+ and the ion “nitrate”, so: H+ NO3- = HNO3
Nitrous acid = H+ and the ion “nitrite”, so: H+ NO2- = HNO2
Sulfuric acid = H+ and the ion “sulfate”, so: H+ SO4-2 = H2SO4
*Construct electron dot formulas to illustrate ionic and covalent bonds: