Using the Nomenclature Flowchart to Review Naming Compounds ANSWER KEY

Home , Oxyacid

You try #1: 1) For each compound, put a check () in the box for the appropriate class/subclass.

Compound Ionic, Ionic, Molecular Acid, Acid, Formula Type I Type II (covalent) Binary Oxyacid How did you know that?

CCl4  All nonmetals, no H in front

SnCl2  Sn is not a Type I metal HCl(aq)  H + one nonmetal

ZnCl2  Type I metal (always +2)

NH4Cl  NH4 belongs in Type I

H2CO3(aq)  H + 2 nonmetals (with O)

MgCO3  Type I metal (always +2)

MnCO3  Mn is not a Type I metal

CO2  All nonmetals, no H in front

You try #2: 2) Now, let’s apply these rules to each of the compounds that you categorized in question 1).

Compound Class/ Name Formula subclass How did you know that?

CCl4 Molecular carbon Don’t use mono with first element. Change ending of (covalent) tetrachloride second element to –ide.

SnCl2 Ionic, tin(II) chloride We need to figure out the charge on the Sn (since it Type II is a type II metal). The Sn must cancel the 2- charge on the Cl ions. HCl(aq) Acid, hydrochloric Binary acids are the only ones that start with Binary acid “hydro”.

SrCl2 Ionic, strontium Sr is always +2 so we don’t need roman numerals. Type I chloride

NH4Cl Ionic, ammonium NH4 is the one nonmetal that fits into the Type I Type I chloride ionic compound. 2- H2CO3(aq) Acid, carbonic acid Knowing that the base ion for this acid (CO3 ) is Oxyacid called “carbonate”, we can figure out that the ending changes to –ic.

MgCO3 Ionic, magnesium Mg is always +2 so we don’t need to use (II) to say Type I carbonate so.

MnCO3 Ionic, manganese(II) We need to figure out the charge on the Mn (since it Type II carbonate is a Type II metal). The Mn must cancel the 2- 2- charge on the CO3 ion.

CO2 Molecular carbon dioxide Don’t use mono with first element. Change ending of (covalent) second element to –ide.

1 Using the Nomenclature Flowchart to Review Naming Compounds ANSWER KEY

You try #3: 3) Let’s apply these rules to each of the compounds in the following table.

Compound name Class/ Formula subclass How did you know that?

Hydrosulfuric acid Acid, H2S(aq) . Starts with “hydro”, ends with “acid”. Binary . Must just be a single element after the H. S makes the most sense (related to root sulfur). Since S forms 2- ion, we need two H+ in front of the formula.

Sulfuric acid Acid, H2SO4(aq) . Ends with “acid”, but no “hydro”. Oxyacid . The base name of the anion was changed to “- ic”, so it must have been “-ate” originally. So the acid must be based on “sulfate” which is 2- + SO4 . We need two H in front of the formula to balance the -2 charge.

Sulfurous acid Acid, H2SO3(aq) . Ends with “acid”, but no “hydro”. Oxyacid . The base name of the anion was changed to “- ous”, so it must have been “-ite” originally. So the acid must be based on “sulfite” which is 2- + SO3 . We need two H in front of the formula to balance the -2 charge.

Sulfur dioxide Molecular SO2 . All nonmetals (no NH4 or H in front). (covalent) . Use the prefixes to figure out how many of each element is present.

Tin (IV) sulfite Ionic, Sn(SO3)2 . Roman numerals after the metal. Type II . Write down the ions for the two parts: Sn4+ 2- and SO3 . Use subscripts to combine the ions in the right ratio to cancel their charges. Here parenthesis are used because there is more than one polyatomic ion.

Cesium sulfate Ionic, Cs2SO4 . Metal without roman numerals. Cesium is Type I always +1. . Write down the ions for the two parts: Cs+ and 2- SO4 . Use subscripts to combine the ions in the right ratio to cancel their charges.

Silver sulfide Ionic, Ag2S . Metal without roman numerals. Silver is always Type I +1. . Write down the ions for the two parts: Ag+ and S2-. Use subscripts to combine the ions in the right ratio to cancel their charges.

2 Using the Nomenclature Flowchart to Review Naming Compounds ANSWER KEY

You try #4: 4) For each of the following compounds write the formula if you are given the name and the name if you are given the formula.

Name Formula

calcium sulfate CaSO4

nickel (III) acetate Ni(C2H3O2)3

zinc bisulfate (zinc hydrogen sufate) Zn(HSO4)2

cobalt (III) chromate Co2(CrO4)3

dinitrogen tetroxide N2O4

tin (II) phosphate Sn3(PO4)2

sulfurous acid H2SO3(aq)

phosphorus triiodide PI3

nickel (III) sulfite Ni2(SO3)3

ammonium carbonate (NH4)2CO3 barium sulfide BaS

potassium dichromate K2Cr2O7 cesium hydroxide CsOH

iron (II) cyanide Fe(CN)2

chlorous acid HClO2(aq)

triphosphorus tetroxide P3O4

ammonium hydroxide NH4OH silver chloride AgCl