NOTE:

YOU WILL ONLY WRITE IUPAC NOMENCLATURE IN THIS CLASS. 

THE INSTRUCTOR CAN PROVIDE EITHER SYSTEM FOR NAMING.

Description

Rule

Example

Type I

Metal + Nonmetal

(Metal only has one type of charge)

1.  Always write cation then anion.

 Cation = metal with (+) charge.

Anion = nonmetal with (-) charge.

2.  Hydrogen can be anion or cation. 

3.  Name cation as noted on periodic table.

4.  Change anion name, add “ide” suffix.

5.  # (+)  charges = # (-) charges

6.  This is an ionic bond.

LiCl  = lithium chloride

BaO = barium oxide

MgCl₂ = magnesium chloride

Type II a

Metal + Nonmetal

(Metal has more than one type of charge)

1.  Same rules as with Type I.

2.  Tell charge on metal by using Roman Numbers in ( ).  (I = +1 charge on metal; II = +2 charge on metal, etc…)

3.  This is ionic bonding.

Fe₂O₃ = iron (III) oxide  (IUPAC System)

                          or

                ferric oxide  (Classical System)

CuF = copper (I) fluoride 

            (IUPAC System)

                      or

            cuprous fluoride 

          (Classical System)

Type II b

Metal + Polyatomic Ion

(Metal has only one type of charge)

1.  Name the cation (metal) first.

2.  Then name the polyatomic ion

3.  If more than one polyatomic ion, put it in ( ) and then tell how many as subscript after ( ).

4.  This is ionic bonding between metal and polyatomic ion.

5.  Covalent bonding holds the polyatomic ion together.

NaNO₃ = sodium nitrate

Mg(OH)₂ = magnesium hydroxide

Ba(NO₃)₂ = barium nitrate

Ca(HCO₃)₂ = calcium hydrogen carbonate

                               (IUPAC System)

                                         or

                         calcium bicarbonate

                            (Classical System)  

Type II c

Metal + Polyatomic Ion

(Metal has more than one type of charge)

1.  Name the cation (metal) first but follow rules as listed in Type II above.

2.  Follow rules as in Type III a.  If more than one polyatomic ion, put it in ( ) and tell how many as a subscript after ( ).

3.  This is ionic bonding between metal and polyatomic ion.

4.  Covalent bonding holds the polyatomic ion together.

Cu₂SO₄ =  copper (I) sulfate (IUPAC System)

                                 or

                   cuprous sulfate (Classical System)

Ni₃(PO₄)₂ =  nickel (II) phosphate

                            (IUPAC System)

                                      or

           nickelous phosphate(Classical System)                          

Type II d

Polyatomic Ion + Polyatomic Ion

(NH₄⁺  = ammonium ion)

1.  Name polyatomic ions as memorized.

2.  Place ( ) around polyatomic ion ONLY IF more than one, then tell how many as subscript outside ( ).

3.  This is ionic bonding between metal and polyatomic ion.

4.  Covalent bonding holds the polyatomic ion together.

NH₄ClO= ammonium  hypochlorite

(NH₄)₂SO₃ = ammonium sulfite

Type II e

Polyatomic Ion + Nonmetal

1.  Name polyatomic ion them nonmetal,

2.  Nonmetal name is changed to the “ide” suffix since it is the anion.

NH₄F  = ammonium fluoride

(NH₄)₂O = ammonium oxide

Type III

Nonmetal + Nonmetal

1.  Name as though ionic, even though it is not.  This is covalent bonding.

2.  Do not try to solve using metal + nonmetal rules.  JUST NAME IT USING GREEK PREFIXES.

mono =1, di=2, tri=3, tetra =4,

penta =5, hexa =6, hepta =7, octa =8, nona =9 deca =10

3.  Never use mono for the first element.

SO₃ = sulfur trioxide

P₂O₅ = diphosphorus pentoxide

Acids & Bases

1.  Acids have H written first in the formula.  These are the transferable hydrogens.  Acids should be denoted by the (aq) state.  Acids without oxygen are named hydro___ ic acid.  Acids with oxygen are named by looking at the ending of their polyatomic names.  If “ate”, then “___ic  acid” and if “ite”, then “___ous acid”.  Hydro is not used with acids with oxygen in it.

2.  Bases can be easily recognized when the hydroxide ion (OH^-) is observed.  Ammonia (NH₃) is also a base.

HCl (aq)  =  hydrochloric acid

H₂SO₄ (aq) = sulfuric acid

HNO₂ (aq) = nitrous acid

HYDRATES

(hydrate =  H₂O associated with complex)

1.  Name the compound as noted above.

2.  Tell how many hydrates using Greek prefixes. 

3.  Place a dot ( ^. ) between complex and hydrate.

3.  Mono is used to indicate only one hydrate.

NaNO₃ ^. H₂O  =  sodium nitrate monohydrate

Sn(ClO₃) ^. 5 H₂O =tin (II) chlorate pentahydrate

                                (IUPAC System)

                                                        or

                     stannous chlorate pentahydrate

                               (Classical System)

DOUBLE DISPLACEMENT REACTIONS

(example)

AB  +  CD  ®  AD  +  CB

(Remember to always write the cation 1st then the anion)

(solution)

Type I - Precipitation Reactions

(refer to the solubility tables)

(aq)  +  (aq)  ®  (s)  +  (aq)

lead(II) nitrate reacts with

potassium iodide to form (you know)

Pb(NO₃)₂ (aq)  +  2 KI (aq)  ®

PbI₂ (s)  +  2  KNO₃ (aq)

Type II - Neutralization Reactions

acid + base ® water  +  salt  +  heat

hydrochloric acid  reacts with

sodium hydroxide  to yield

( you know)

HCl   +  NaOH  ®   H₂O  +  NaCl

Type III - Gaseous Reactions

Formation of CO₂ gas

Carbonate (CO₃ ^2- ) reacts with an acid

NaHCO₃  +  HCl  ®  2 CO₂  +  H₂O  + NaCl

(via an intermediate reaction)

Formation of SO₂ gas

Sulfite (SO₃ ^2- ) reacts with an acid

Na₂SO₃  +  HNO₃  ®  SO₂  +  H₂O  + 

2 NaNO₃

(via an intermediate reaction)

Formation of H₂S gas

(the rotten egg smell)

Sulfide (S ^2- ) reacts with an acid

Na₂S  +  H₂SO₄  ®  H₂S  +  Na₂SO₄

(directly)

Formation of HCN gas

Cyanide (CN^-)  reacts with an acid

LiCN  +  HCl  ®  HCN  +  LiCl

SINGLE REPLACEMENT REACTIONS

(example)

A  +   BC  ®  AC  +  B

metal or nonmetal replaces another element

(refer to the activity series)

(solution)

a piece of sodium metal is placed into a test tube containing

lead (II) nitrate

2 Na  +  Pb(NO₃)₂  ®  2 NaNO₃  +  Pb

COMBUSTION

(example)

CH or CHO  +  O₂  ®  CO₂  +  H₂O  + Heat

hydrocarbon or hydrocarbon with oxygen forms carbon dioxide and water vapor  and heat

(YOU ARE EXPECTED TO KNOW THE PRODUCTS)

(solution)

Methane Burns

CH₄  +  2 O₂ (g)  ®  CO₂ (g) +  2 H₂O (g)  + Heat

COMBINATION REACTION

(example)

A  +   B  ®  AB

two or more substance forms only ONE substance

(solution)

nitrogen reacts with hydrogen to form ammonia

N₂  +  3 H₂  ®  2 NH₃

DECOMPOSITION REACTION

(example)

AB  ®  A  +   B

ONE substance breaks down to two or more substances

(solution)

sodium nitrate when heated to form

sodium nitrite and oxygen

2 NaNO₃  ®  2 NaNO₂  +  O₂

SOLUBILITY RULES FOR IONIC COMPOUNDS

1.       Compounds containing Group IA metals, ammonium, acetates and nitrates are all soluble. 

2.       Most halides (Group 7A - chlorides etc.) are soluble. Exceptions include Ag⁺¹, Pb⁺², and Hg₂⁺² halides.

3.       Most sulfates are soluble.  Exceptions include Ba⁺², Sr⁺², Ag⁺¹, Pb⁺², and Ca⁺² sulfates.

4.       Most hydroxides insoluble.  Exceptions include hydroxides of Group 1A metals, ammonium, Ca⁺², Sr⁺², and Ba⁺².

5.       Most phosphates, carbonates, chromates, and sulfides are insoluble.  Exceptions include those compounds containing Group 1A metals and ammonium. 

6.       In addition, all acids are soluble!

ACTIVITY SERIES FOR METALS (and HYDROGEN)