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Nomenclature of Inorganic Compounds
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0. review
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Diatomic Molecules Hydrogen H2 Nitrogen N2 Oxygen O2 Fluorine F2
Chlorine Cl2 Bromine Br2 Iodine I2
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Polyatomic Molecules Sulfur S8 Phosphorous P4
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Outline 1. Common Names 2. Ions 3. Ionic Formulas 4. Polyatomic Ions
5. Halogen Compounds 6. Acids 7. Covalent Compounds
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Chemical names are either:
common or systematic Common names are inconsistent but often come from stories, people’s names, important characteristics of a compound, history. They continue to be used in spite of their lack of consistency. Systemic names are regulated by the IUPAC: International Union of Pure and Applied Chemistry
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1. common names
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Common Name Chemical Name acetone
dimethyl ketone; 2-propanone (usually known as acetone) alcohol, grain ethyl alcohol alcohol, wood methyl alcohol aqua regia A mixture of nitric acid and hydrochloric acid aspirin acetylsalicylic acid baking soda sodium bicarbonate pencil lead graphite (carbon) bone ash crude calcium phosphate brimstone sulfur brine aqueous sodium chloride solution Calamine lotion zinc oxide and iron (III) oxide caustic lime calcium hydroxide Epsom salts magnesium sulfate laughing gas nitrous oxide lye sodium hydroxide milk of magnesium magnesium hydroxide quicksilver mercury rubbing alcohol isopropyl alcohol salt, table sodium chloride sugar, table sucrose vinegar impure dilute acetic acid vitamin C ascorbic acid
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2. ions
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If one or more electrons are removed from a neutral atom a positive ion is formed. A positive ion is called a cation. remove e- → neutral atom cation
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The charge of a cation depends on the atom.
Na Na e- Ca Ca e- Al Al e-
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cations have the same name as their parent atoms
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If one or more electrons are added to a neutral atom a negative ion is formed. A negative ion is called an anion. add e- → neutral atom anion
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anions made from one element have names that end in -ide
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Ions are always formed by adding or removing electrons from an atom
Ions are always formed by adding or removing electrons from an atom. Protons are NOT added or removed except in NUCLEAR reactions.
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elements of Group 6A have a -2 charge
6.2
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Chemical compounds have a NET charge of zero
Chemical compounds have a NET charge of zero. The charge of all the cations must be equal to the charge of all the anions.
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Write the formula of calcium chloride.
Step 1. Write down the formulas of the ions. Ca2+ Cl- Step 2. Combine the smallest numbers of Ca2+ and Cl- so that the sum of the charges equals zero. (Ca2+) + 2(Cl-) = 0 (2+) (1-) = 0 The correct formula is CaCl2
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Write the formula of barium phosphide.
Step 1. Write down the formulas of the ions. Ba2+ P3- Step 2. Combine the smallest numbers of Ba2+ and P3- so that the sum of the charges equals zero. 3(Ba2+) + 2(P3-) = 0 3(2+) (3-) = 0 The correct formula is Ba3P2
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Write the formula of magnesium oxide.
Step 1. Write down the formulas of the ions. Mg2+ O2- Step 2. Combine the smallest numbers of Mg2+ and O2- so that the sum of the charges equals zero. (Mg2+) + (O2-) = 0 (2+) (2-) = 0 The correct formula is MgO
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3. ionic formulas
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Binary compounds contain only two different elements
Binary compounds contain only two different elements. Binary ionic compounds consist of a metal combined with a non-metal.
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NaCl name of metal sodium chloride nonmetal stem
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MgCl2 name of metal magnesiumchloride nonmetal stem
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K2O potassium oxide
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Na3P sodium phosphide
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Some metals form more than one type of cation.
These metals are said to have variable oxidation states. 6.2
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Different compounds are formed with different oxidation states of the cation.
FeS Fe3+ Fe2S3 6.2
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In the Stock System the charge on a cation with variable oxidations states is designated by a Roman numeral placed in parentheses immediately following the name of the metal. Cation Charge +1 +2 +3 +4 +5 Roman Numeral (I) (II) (III) (IV) (V)
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Stock System Copper Cu+ copper (I) Cu2+ copper (II)
Iron Fe2+ iron(II) Fe3+ iron(III) Lead Pb2+ lead (II) Pb4+ lead(IV) Mercury Hg22+ mercury(I) Hg2+ mercury(II) Tin Sn2+ tin(II) Sn4+ tin (IV)
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+2 -1 -1 +3 iron(II) chloride FeCl2 chloride iron(II) compound name
ion charge ion name iron(III) chloride FeCl3 -1 +3 iron(III) chloride
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+2 -1 -1 +4 tin(II) bromide SnBr2 bromide tin(II) compound name
ion charge ion name tin(IV) bromide SnBr4 -1 +4 tin(IV) bromide
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Classical System Cu+ Cu2+ Fe2+ Fe3+ Pb2+ Pb4+ Hg Hg2+ Sn2+ Sn4+ 2+ 2
Element Formula Name Copper Cu+ cuprous Cu2+ cupric Iron Fe2+ ferrous Fe3+ ferric Lead Pb2+ plumbous Pb4+ plumbic Mercury Hg mercurous Hg2+ mercuric Tin Sn2+ stannous Sn4+ stannic 2+ 2
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4. polyatomic ions
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A polyatomic ion is an ion that contains two or more elements.
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The names, formulas and charges of polyatomic ions must be committed to memory.
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hydroxide OH1-
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cyanide CN1-
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thiocyanate SCN1-
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carbonate CO32-
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bicarbonate HCO31-
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sulfate SO42-
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sulfite SO32-
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phosphate PO43-
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phosphite PO33-
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nitrate NO31-
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nitrite NO21-
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ammonium NH41+
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acetate C2H3O21-
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chromate CrO42-
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dichromate Cr2O72-
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There are three common positively charged polyatomic ions.
mercury(I) ammonium hydronium
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When naming a compound containing a polyatomic ion, name the cation first and then name the anion. The cations must neutralize the charge on the anions. sodium carbonate
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sodium carbonate
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potassium permanganate
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Anions ending in -ate always contain more oxygen than ions ending in -ite.
nitrate nitrite
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-ate and –ite do not indicate the number of oxygen atoms.
sulfate sulfite -ate and –ite do not indicate the number of oxygen atoms.
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phosphate phosphite
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Ba(OH)2 barium hydroxide
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MgCO3 magnesium carbonate
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K2SO3 potassium sulfite
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NaSCN sodium thiocyanate
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Al2(CrO4)3 aluminum chromate
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aluminum phosphate AlPO4
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sodium sulfate Na2SO4
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magnesium nitrate Mg(NO3)2
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calcium cyanide Ca(CN)2
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ammonium nitrate NH4NO3
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5. halogen compounds
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per is a short form of hyper, meaning more
Per- denotes anions with more oxygen than the -ate form. chlorate perchlorate per is a short form of hyper, meaning more
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hypo- denotes anions with less oxygen than the -ite form.
hypochlorite chlorite -hypo means less
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Ba(ClO3)2 barium chlorate
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Ca(ClO2)2 calcium chlorite
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KIO4 potassium periodate
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NaClO4 sodium perchlorate
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Al(BrO4)3 aluminum perbromate
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lithium bromate LiBrO3
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sodium hypoiodite NaIO
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magnesium chlorite Mg(ClO2)2
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calcium perchlorate Ca(ClO4)2
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ammonium chlorite NH4ClO2
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6. acids
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Certain binary hydrogen compounds, when dissolved in water, form solutions that have acid properties. The aqueous solutions of these compounds are given acid names. The acid names are in addition to their –ide names and only apply to the compounds when they are in the aqueous solution. Hydrogen is typically the first element of a binary acid formula.
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HCl HCl(aq) The pure compound hydrogen chloride
dissolved in water becomes hydrochloric acid HCl(aq)
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For binary acid formulas write the symbol of hydrogen first.
After hydrogen write the symbol of the second element. HCl To assign a name to the acid place the prefix hydro- in front of the stem of the nonmetal name. hydrochlor- Place the suffix –ic acid after the stem of the nonmetal name. hydrochloric acid
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HI hydrogen iodide Pure Compound
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HI(aq) hydroiodic acid Dissolved in Water
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H2S hydrogen sulfide Pure Compound
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H2S(aq) hydrosulfuric acid Dissolved in Water
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H2Se hydrogen selenide Pure Compound
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H2Se(aq) hydroselenic acid Dissolved in Water
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Oxy-acids contain hydrogen, oxygen and one other element.
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sulfuric acid indicates hydrogen contains hydrogen contains sulfur
contains oxygen sulfuric acid
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Naming the Acid Based on the Name of the Polyatomic Ion
Ending of Polyatomic Ion Ending of Acid ite ous less oxygen ate ic more oxygen
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sulfite sulfurous acid
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sulfate sulfuric acid
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nitrite nitrous acid
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nitrate nitric acid
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7. covalent compounds
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Compounds between nonmetals are molecular, not ionic.
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In a compound formed between two nonmetals or metalloids, the element that occurs first in this series is named first. Si B P H C S I Br N Cl O F
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A Greek prefix is placed before the name of each element to indicate the number of atoms of the element that are present.
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Mono is rarely used when naming the first element.
mono = 1 di = 2 tri = 3 tetra = 4 penta = 5 hexa = 6 hepta = 7 octa = 8 nona = 9 deca = 10 Mono is rarely used when naming the first element.
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N2O3 dinitrogen trioxide indicates two nitrogen atoms
indicates three oxygen atoms
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PCl5 phosphorous pentachloride indicates one phosphorous atom
indicates five chlorine atoms
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Cl2O7 dichlorine heptaoxide indicates two chlorine atoms
indicates seven oxygen atoms
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Determine the Name of PCl5
Analysis There are 2 elements present. The compound is binary. Phosphorous and chlorine are nonmetals so the rules for naming binary compounds of two nonmetals apply. Phosphorous is named first. Therefore the compound is a chloride.
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Determine the Name of PCl5
No prefix is needed for phosphorous because each molecule of PCl5 has only one phosphorous atom. The prefix penta- is used with chloride because there are 5 chlorine atoms present in one molecule. The name is phosphorous pentachloride.
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Cl2O3 dichlorine trioxide
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N2O3 dinitrogen trioxide
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CCl4 carbon tetrachloride
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CO carbon monoxide
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CO2 carbon dioxide
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phosphorous triiodide
PI3 phosphorous triiodide
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summary
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6.5
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Fe(NO3)2 iron (II) nitrate
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CuCl2 copper (II) chloride
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N2O5 dinitrogen pentoxide
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NH4ClO4 ammonium perchlorate
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AgNO2 silver nitrite
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tin(IV) bromate Sn(BrO3)4
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hydrosulfuric acid H2S(aq)
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nitric acid HNO3(aq)
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hypochlorous acid HClO(aq)
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mercury (I) chlorite Hg2(ClO2)2
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