Unit 5 - Nomenclature Covalent Naming

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Unit 5 - NomenclatureCovalent NamingWriting chemical formulas is a fundamental skill in chemistry. Mastery of thisunit is REQUIRED as it will be used in EVERY subsequent unit. Chemistshave agreed in every nation on rules to name and write the chemical formulasof compounds. Chemists are able to communicate in a common languagebased on these rules and it is an important step in becoming a chemist.Chemical nomenclature is a set of rules to generate systematic names forchemical compounds. The nomenclature used most frequently worldwide isthe one created and developed by the International Union of Pure andApplied Chemistry (IUPAC).The IUPAC's rules for naming organic and inorganic compounds arecontained in two publications, known as the Blue Book and the Red Book,respectively.The primary function of chemical nomenclature is to ensure that a spoken orwritten chemical name leaves no ambiguity concerning which chemicalcompound the name refers to: each chemical name should refer to a singlesubstance.There are two types of nomenclature. The IUPAC has a set of rules fornaming organic chemicals and inorganic chemicals.Covalent Naming Binary covalent compounds are characterized by having two nonmetals.Naming these compounds involves the use of numerical xhexaheptaoctanonadecaNumber678910 If there is only ONE atom of the first element, you DON’T need a prefix.The FIRST element is named as a normal element. The SECOND element has an –IDE ending.1

o N2O4dinitrogen tetraoxideo XeF4xenon tetraflorideo N2O5dinitrogen pentaoxideo COcarbon monoxideo CBr4carbon tetrabromideo Diarsenic pentoxideAs2O5o Phosphorous pentabromidePBr5o Carbon tetraiodideCI4o Trisilicon tetranitrideSi3N4o Tetraphosphorous decoxideP4O10Naming Polyatomic IonsYou have memorized several polyatomic ions, but there are some you don’tknow, but can figure out: Use chlorate (ClO3-) as an example If the ion has 1 more oxygen atom than the base ion (ClO3-), it is namedby a prefix per- and a suffix –ate.o ClO4- is perchlorate If the ion has 1 less oxygen atom then the base ion (ClO3-), then it isnamed by the suffix –ite.o ClO2- is chlorite If the ion has 2 less oxygen atoms than the base ion (ClO3-), then it isnamed by the prefix hypo- and a suffix –ite.o ClO- is hypochloriteName the following:Sulfite1. SO32-3. SO22-Hyposulfite2. PO33-Phosphite4. CO22-Carbonite5. PO53-Perphosphate6. CrO32-Chromite2

Balancing ChargesOverall1. Balance charge with and – ions2. Write the positive ion of metal first, and the negative ion secondBa2 Cl Cl 3. Write the number of ions needed as subscriptsBaCl2Naming Binary Ionic Formulas1. The Cation is named and written first, then anion and the Monatomiccation name of the elementCa2 calcium ion2. The monatomic anion root and the ending is changed to -ideCl- chlorideSo CaCl2 Calcium ChlorideCriss-Cross rule1. Write out symbols and charge of elements2. Criss-Cross charges as subscripts(Swap and Drop)3. Combine as a formula unitEquation For Balancing Charges(Number of Cations)x(Cation Charge) (Number of Anions)x(Anion Charge) 0(1)( 3) (X)(-1) 0, x 3o EX: Aluminum and OxygenAl 3O-2 Al2O3 EX: Barium and OxygenBa 2 O-2 BaO3

Balancing Charges Practice:o Lithium Iodideo Strontium Chlorideo Aluminum Nitrideo Sodium SulfideLi ISrCl2Al NNa2SIonic Compound Naming Notes To name ionic compounds:o Name the Metal (cation) first.o Name the Non-Metal (anion) second- change the ending to ide.o Al2O3Aluminum Oxideo BaCl2Barium Chlorideo Ca3N2Calcium Nitrideo KFPotassium Fluoride Ionic Compounds with transition metals:o Transition metals and p-block metals can have multiple oxidationstates. Silver (Ag) is always 1 Zinc (Zn) is always 2 Cadmium (Cd) is always 2o Roman numerals are used in naming transition metals with more than one charge,we have to specify which charge is involved.Roman numeralIIIIIIIVCharge 1 2 3 4o Some elements, such as iron, form two or more cations withdifferent charges. We use Roman numerals to indicate the ion’s4

charge. For example, Fe 2 would be named Iron (II) and Fe 3would be named Iron (III). If an element does not form more thanone charge, then you do not use a Roman numeral in its name. Iron (III) Oxide PbO2 Fe2S3Fe2O3Lead (IV) OxideIron (III) Sulfide The one you are responsible for are as follows:Namelead (II)lead (IV)mercury (I)copper (I)copper (II)chromium (II)SymbolPb 2Pb 4Hg 1Cu 1Cu 2Cr 2Namemercury (II)tin (II)tin (IV)iron (II)iron (III)chromium (III)SymbolHg 2Sn 2Sn 4Fe 2Fe 3Cr 3Naming Acids If the compound begins with Hydrogen, it is an acid. If the acid does notcontain a polyatomic ion, write the prefix hydro-, then name the secondelement and change the ending to –ic.’o HClHydrochloric acido HBrHydrobromic acido H2 SHydrosulfuric acid5

Naming Acids with Polyatomic IonsThe polyatomic ions you have memorized have –ate as the ending, so youname the polyatomic ion and change the ending to –ic.Use sulfate (SO42-) as the example H2SO4 is sulfuric acid If the ion has one more oxygen atom than the base (SO42-), then the ion isnamed by adding the prefix per- and the suffix –icispersulfuric acido H2SO5 If the ion has one less oxygen atom than the base (SO42-), then the ion isnamed with the suffix –ous.issulfurous acido H2SO3 If the ion has two less oxygen atoms than the base (SO42-), then the ion isnamed with the prefix hypo- and the suffix –ous.ishyposulfurous acido H2SO2Name the following:1. H2CO3 Carbonic acid2. H3PO2Hypophosphorious acid3. HClO4Perchloric acid4. H3PO3Phosphorous acidHydrated Compounds These are Ionic compounds that produce water when decomposed byheating. The compounded is named using the ionic compound, a dot , H2O, andthe ending hydrate. The number of water molecules are indicate using previous prefixes of"di", "tri", etc.Practice Name Formula1. CuSO4 5H2O2. ZnCl2 6H2OCopper (II) sulfate pentahydrateZinc chloride hexahydrate6

Naming Summary Sheet:Naming Ionic Compounds: Metal and Nonmetal‐‐‐‐Transition Metals with Single Charges:-Cd 2-Zn 2-Ag 1Transition Metals with Multiple Charges:‐ Cu 1 or Cu 2‐ Cr 2 or Cr 3‐ Co 2 or Cr 3‐ Fe 2 or Fe 3‐ Pb 2 or Pb 4‐ Sn 2 or Sn 4Rules:1. The first element (the cation) is namedfirst, using the elements name.2. Second element (the anion) is namedchange the ending of the anion to –ide (unlessa polyatomic ion) (suffix "-ide")Example: CaF2 – calcium fluorideIf a metal has more than one possible charge,use roman numerals to describe the charge ofthe metal.‐ Fe2S3 – iron (III) sulfideNaming a Covalent Compounds: 2 NonmetalsRules:‐‐1. Prefixes are used to denote the number of atoms2. "Mono" is not used to name the first elementNote: when the addition of the Greek prefix places two vowels adjacent to one another, the "a" (orthe "o") at the end of the Greek prefix is usually dropped; e.g., "nonaoxide" would be written as"nonoxide", and "monooxide" would be written as "monoxide". The "i" at the end of the prefixes"di-" and "tri-" are never 10If there is only ONE atom of the first element, you DON’T need a prefix. The FIRST elementis named as a normal element. The SECOND element has an –IDE ending.Example: CBr4 – carbon tetrabromideNaming Polyatomics and Acids: Only NonmetalsBase hosphateChromateTo determine name, look at how the compound compares to the base, with an –ate ending.Number of Oxygen:1 more than baseBase1 less than base2 less than baseBinary (no oxygenpresentPolyatomicsPer –ate-ate-iteHypo-iteExampleAcidsExample-SO5 - persulfate-SO4 - sulfate-SO3 - sulfite-SO2 - hyposulfitePer –ic acid-ic acid-ous acidHypo-ous acid-ide-S - sulfideHydro-ic acidHClO4 – perchloric acidHClO3 - chloric acidHClO2 - chlorous acidHClO – hypochlorousacidHCl – hydrochloric acid7

Note: When Group is used, it is referring to all of theelements in the groups on the periodic table.Condensed List of Common Ions and their charges1. Cations: 1 chargeGroup 1Ex:sodiumhydrogensilverhydroniumammoniumcopper (I)gold(I)Ex: Na 1H 1Ag 1H3O 1NH4 1Cu 1Au 1 2 chargeGroup 2Ex: calciumEx: Ca 2cadmiumzinccopper (II)chromium (II)cobalt (II)iron (II)lead (II)mercury (I)mercury (II)tin (II)Cd 2Zn 2Cu 2Cr 2Co 2Fe 2Pb 2Hg2 2Hg 2Sn 2 3 chargealuminumAl 3 4 chargechromium (III)cobalt (III)iron (III)Cr 3Co 3Fe 3lead (IV)Pb 4tin (IV)Sn 42. AnionsRequired Ions-1-2NameSymbolNameSymbolNameGroup 16Group 17Ex: ClCyanideCN-1Ex: OxideEx: *bicarbonate 3-1*nitriteNO2-1Optional Ions (May appear in extra credit or in AP ClO-1perbromate BrO4-1oxalate-1permanganate -1silicate-1-1iodateIO3hypobromite omatedichromateSymbolEx: O-2CO3-2SO4-2SO3-2-3NameSymbol*Group 15-3Ex: nitride Ex: Nphosphate iO3-2TeO4-2SeO4-2CrO4-2Cr2O7-2SymbolAsO4-3* -indicates ion can be determined by using additional information (see below).Bolded Ions- Indicates the most important of the required ions for students to know3. Additional Informationa. All cations not listed will use Roman numerals to indicate chargesb. Anions with different numbers of oxygens other than the “ate” form”i. 1 more O“per”-------“ate”Ex: FO4-1 perfluorateii. 1 less O---------------“ite”Ex: FO2-1 fluoriteiii. 2 less O“hypo”-----“ite”Ex: FO-1 hypofluorite8

c. Anions which have a hydrogen added to them take a “bi-“ or “hydrogen”prefix AND the charges increases by 1i. Ex. HCO3-1 bicarbonate or hydrogen carbonated. Some transition metals can be named in another ways, using their Latinname as a root.i. An “ous” ending has the lower possible oxidation stateii. An “ic” ending indicates the higher possible oxidation stateiii. This naming system is no longer commonly used and can be found onolder bottles of compounds.NameSymbolFYI onlyLatin Namelead (II)lead (IV)mercury (I)mercury (II)tin (II)tin (IV)copper (I)copper (II)iron (II)iron (III)chromium (II)chromium (III)Pb 2Pb 4Hg 1Hg 2Sn 2Sn 4Cu 1Cu 2Fe 2Fe 3Cr 2Cr prouscupricferrousferricchromouschromic9

2. Write the positive ion of metal first, and the negative ion second Ba2 Cl Cl 3. Write the number of ions needed as subscripts BaCl2 Naming Binary Ionic Formulas 1. The Cation is named and written first, then anion and the Monatomic cation name of the element Ca2 calcium ion 2. The monatomic anion root and the ending is changed to -ide

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