NAMING COMPOUNDS

TYPES OF COMPOUNDS Molecular compound (covalent bonds) Compound made of two nonmetals NBr5 Ionic compound Compound made of a metal and a nonmetal NaCl Acid (ionic bonds) Compound that can donate a hydrogen ion HCl

MOLECULAR COMPOUND (TWO NONMETALS) To name a molecular compound, you have two parts: The first element in the compound and The second element in the compound NBr5 The first element is called by its normal name: N – nitrogen The second name is called by its name and ends in –ide: Br – bromine  bromide

PREFIXES In addition to naming the elements, you have to name how many they are. To do this you need prefixes. The prefix goes in the front of the name of the element

PREFIXES (CONT) One – mono Two – di Three – tri Four – tetra Five - penta Six – hexa Seven – hepta Eight – octa Nine – nona Ten - deca

MOLECULAR COMPOUND (CONT) Therefore if you start with NBr5: Mononitrogen pentabromide BUT wait, if you only have one element in the beginning part of the compound, you don’t have to put the prefix: Nitrogen pentabromide

TRY THESE SCl6 N2O4 P3F5 CCl4 XeO Trinitrogen hexaoxide Boron pentabromide Tetrasulfur decafluoride Phosphorus octaiodide

N3O6 BBr5 S4F10 PI8 ANSWERS Sulfur hexachloride Dinitrogen tetraoxide Triphosphorus pentafluoride Carbon tetrachloride Xenon monoxide N3O6 BBr5 S4F10 PI8

SPECIAL CASE When naming some compounds, it is implied that the compound is a DIATOMIC GAS There are only 7 diatomic molecules Hydrogen Nitrogen Oxygen Fluorine Chlorine Iodine Bromine

DIATOMIC MOLECULES If you ever see any of those molecules, you write them as a compound with two of the atoms Hydrogen – H2 Nitrogen – N2 Oxygen – O2 Fluorine – F2 Chlorine – Cl2 Iodine – I2 Bromine – Br2

IONIC COMPOUNDS (METAL AND NONMETAL) The two parts of naming an ionic compound: The first element is always the metal The second element is the nonmetal CaBr2 The first element is called by its normal name: Ca  Calcium The second element is named like a molecular compound: Br  bromide The only difference is that you do not use a prefix ever

IONIC COMPOUNDS Therefore if you start with CaBr2: Calcium Bromide There is no prefix for bromide even though there is a 2

IONIC COMPOUNDS Before we begin practice naming ionic compounds, look at your ion sheet Remember: To put ionic compounds together, you need to BALANCE THE CHARGE

EXAMPLE How would you show the following ionic compound: Strontium iodide Strontium  Sr (has a +2 charge: alkali earth metal) Iodide (has a -1 charge: halogen) Just like before, cancel swap the charges Sr+2 + 2I -  SrI2 Your ion sheet gives you the names of several ions with the many possible charges of the transition metals

BaCl2 K2O AlF3 CaO TRY THESE Magnesium oxide Potassium sulfide Sodium chloride Beryllium iodide

ANSWERS MgO K2S NaCl BeI2 Barium chloride Potassium oxide Aluminum fluoride Calcium oxide MgO K2S NaCl BeI2

POLYATOMIC IONS An ion that is composed of several atoms FORMAL DEFINITION Polyatomic ion: an electrically charged group of two or more chemically bonded atoms that function as a SINGLE ION

POLYATOMIC IONS Since the polyatomic ions are made of more than 1 atom, their names are complicated Example of some polyatomic ions: OH -  hydroxide ClO4 -  perchlorate CO3-2  carbonate NH4 +  ammonium

POLYATOMIC IONS IMPORTANT NOTE: When combining polyatomic ions, you still balance out the NET CHARGE: Example: If you have sodium hydroxide Sodium: Na+ Hydroxide: OH – Na+ + OH -  NaOH

POLYATOMIC ION What do you do if you have more than 1 polyatomic ion to balance out a charge? Example: If you have Magnesium acetate Magnesium: Mg+2 Acetate: C2H3O2 – Mg+2 + 2C2H3O2-  Mg(C2H3O2)2 You put the entire polyatomic ion in brackets with the number of ions as a subscript

TRY THESE K3BO3 Sr(NO2)2 Mg3(PO4)2 CaSO4 Lithium oxalate Barium bromate Sodium Phosphate Aluminum sulfate K3BO3 Sr(NO2)2 Mg3(PO4)2 CaSO4

ANSWERS Li2C2O4 Ba(BrO3)2 Na3PO4 Al2(SO4)3 Potassium borate Strontium nitrite Magnesium phosphate Calcium sulfate

IONIC COMPOUNDS (TRANSITION METALS) What do you do when you do not know the exact charge of the ion? In other words, some of the transition metals can have more than 1 ion Fe+2 Fe+3 You distinguish with Roman numerals

IONIC COMPOUNDS (TRANSITION METALS) Solution: The name of the compound tells you the charge. If you have a compound of iron and oxygen, an example would be: Iron (III) oxide This means that iron has a +3 charge 2Fe+3 + 3O-2  Fe2O3

IONIC COMPOUNDS (TRANSITION METALS) This means that if you’re given the formula, you have to figure out the charge of the metal ion: Example: MnO2 What you know: O has a -2 charge Therefore the total negative is -4 This means that you need a +4 to balance You get Manganese (IV) oxide

TRY THESE W(PO4)2 AuBO3 Tl3PO4 Sn(NO3)4 Nickel (III) iodate Lead (II) chloride Gold (I) Sulfate Vanadium (III) chlorate W(PO4)2 AuBO3 Tl3PO4 Sn(NO3)4

Ni(IO3)3 PbCl2 Au2SO4 V(ClO3)3 ANSWERS Tungsten (VI) phosphate Gold (III) borate Thallium (I) phosphate Tin (IV) nitrite

ACIDS What is an acid? For now: An acid is a compound that will donate a proton (H+) How do you recognize an acid Any compound that begins with H+ There are two basic types of acids for naming Binary acid Polyatomic acid

BINARY ACID A binary acid has a hydrogen ion and a single halide Examples: HCl, HF, HBr, HI Naming these acids takes the following format: Hydro-(root of the name of the halide)-ic acid Therefore HCl becomes Hydrochloric acid

BINARY ACID What would be the names of the following: HF HBr HI

ANSWERS Hydrofluoric acid Hydrobromic acid Hydroiodic acid

POLYATOMIC ACIDS Similar convention to binary acids (Base name of the polyatomic ion)-ic acid HC2H3O3 This is an H+ with a C2H3O3- The name of the polyatomic ion is acetate The name is Acetic acid

POLYATOMIC ACIDS The differences What if you have H2SO4 and H2SO3 What’s the difference in these two names?: only one can be sulfuric acid

POLYATOMIC ACIDS If the ion ends in the name “-ate” Sulfate, nitrate, chlorate The name of the acid is (root of ion)-ic acid Sufuric acid, nitric acid, chloric acid If the ion ends in the name “-ite” Sulfite, nitrite, chlorite The name of the acid is (root of ion)-ous acid Sulfurous acid, nitrous acid, chlorous acid

H2CO3 HNO2 HIO3 H3PO4 TRY THESE Oxalic acid Sulfurous acid Sulfuric acid Bromic acid

H2C2O4 H2SO3 H2SO4 HBrO3 ANSWERS Carbonic acid Nitrous acid Iodic acid Phosphoric acid H2C2O4 H2SO3 H2SO4 HBrO3

SUMMARY Before you start naming, determine the type of compound Molecular, ionic or acid Naming molecular compounds (nonmetal and nonmetal) Name of the first element Base name of the second element + ide Make sure you use the prefix indicating number of atoms

SUMMARY (CONT) Naming ionic compounds (metal and nonmetal) Name of the first element Name of the second element + ide or Name of the second polyatomic ion Make sure you balance the charges of each ion If the metal has more than 1 possible charge, indicate the charge with a Roman numeral

SUMMARY (CONT) Acids (the compound has a hydrogen ion H+) Binary acids Hydro (base name of the halogen)-ic acid Polyatomic acids (Base name of the polyatomic ion w/ “-ate”) – ic acid (Base name of the polyatomic ion w/ “-ite”) – ous acid

WRITE THE SYMBOL OR NAME Calcium chloride Lead (IV) sulfate Carbon tetrachloride Hydroiodic acid Sulfuric acid Dinitrogen hexachloride HBr NH4NO3 S3Br8 NO HNO2 Mn(C2H3O2)3 Pb(SO3)2

ANWERS CaCl2 Pb(SO4)2 CCl4 HI H2SO4 N2Cl6 Hydrobromic acid Ammonium nitrate Trisulfur octabromide Nitrogen monoxide Nitrous acid Manganese (III) acetate Lead (IV) sulfite

PUTTING THIS IN A CHEMICAL REACTION General Format: Reactants  Products Steps Translate the chemical into its symbol and then put the state of matter AFTER the chemical symbol Put a “+” between each set of reactants and products

STATES OF MATTER Symbols for states of matter: Solid (s) Liquid (l) Gas (g) Aqueous (aq)

EXAMPLE Solid sodium is mixed with chlorine gas to form aqueous sodium chloride Solid sodium = ? is mixed with = ? chlorine gas = ? to form = ? aqueous sodium chloride = ?

Na(s) + Cl2(g)  NaCl(aq) FINAL ANSWER Na(s) + Cl2(g)  NaCl(aq)

TRY THESE Solid iron is combined with oxygen gas to produce solid iron(III) oxide. Aqueous magnesium nitrate is combined with solid zinc to form aqueous zinc nitrate and solid magnesium.

Mg(NO3)2(aq) + Zn(s)  Zn(NO3)2(aq) + Mg(s) ANSWERS Fe(s) +O2(g)  Fe2O3(s) Mg(NO3)2(aq) + Zn(s)  Zn(NO3)2(aq) + Mg(s)