Experiment #2 Chemical Nomenclature
Experiment #2Chemical NomenclatureFor this experiment, you will complete a series of worksheets. DO NOT USEGOOGLE OR ANY OTHER INTERNET SEARCHES TO DIRECTLYANSWER THE QUESTIONS ON THESE WORKSHEETS. You may use anyresources you need in order to learn how to write formulas and names, butyou may not look up answers directly. Only answers which are appropriatefor a first semester general chemistry course will be accepted. Any materialsfrom this class, this lab handout, OpenStax, or any other general chemistrytextbook will lead you to appropriate answers.IntroductionIn order to completely understand the science of chemistry you must first master the language ofchemistry. One of the most vital aspects of the language is being able to interpret chemicals both by nameand formula. While the first instinct is to simply start memorizing a plethora of names, a better approach isto step back and find the pattern or logic behind the nomenclature rules. The International Union of Pureand Applied Chemistry (IUPAC), has created a logical set of instructions for naming compounds, so as tocreate a universal language among chemists. While you will still be required to learn the names of thepolyatomic ions, learning the rules will minimize the amount of memorization necessary.In this exercise you will learn how to name four major classifications of compounds: covalentcompounds, ionic compounds, acids, and simple organic compounds. There are significant characteristicdifferences between these classes. The largest of these classes is ionic compounds. Because ioniccompounds are composed of strongly attracted charged particles called ions, all ionic compounds are highmelting point solids at normal room temperature and pressure. At the molecular level, the solid is composedof a periodic array of three-dimensionally assembled ions. The chemical formula of an ionic compound, forexample, NaCl, indicates the ratio of the ions in the array and not the specific number of ions in a molecule.On the other hand, covalent compounds are composed of nonmetal elements that are covalently bondedtogether. Covalent compounds can be solids at normal room temperature and pressure, but they can also beliquids or gases. Covalent compounds at the molecular level are composed of discrete molecules containingatoms arranged three-dimensionally with the exact number of each type of atom, which is indicated by thechemical formula. Acids are a uniquely defined class of compounds that contain hydrogen and in theaqueous form dissociate into a hydrogen cation and an anion in water. It is this hydrogen ion that isresponsible for the highly reactive nature of acids. Finally, to help you begin to become familiar with thevery important field of organic chemistry, we will start on the simple nomenclature of organic compounds.Each class of compounds can be separated into either a binary compound or a polyatomic compound.Binary compounds contain only 2 types of elements where polyatomic compounds contain more than 2types of elements. When naming each class of compound, there is a separate set of rules for binarycompounds and for polyatomic compounds.Therefore, the set of instructions presented below are organized in the following fashion.1
I.Binary CompoundsA. Covalent CompoundsB. Ionic Compounds1. Metals with a single chargea. alkali metals (1 charge)b. alkaline earth metals (2 charge)c. Aluminum ion (3 charge), Silver ion (1 charge), Zinc ion (2 charge),and Cadmium ion (2 charge)2. Metals with multiple chargesII. Polyatomic Ionic CompoundsIII. AcidsA. Binary AcidsB. Polyatomic AcidsIV. Common NamesV. Simple Organic MoleculesYou should also review nomenclature section 2.6 and 2.7 in your OpenStax textbook.I.Binary Compounds – Compounds that consist of only 2 elementsA. Covalent compounds – two nonmetals (The only compounds that use numeric prefixes below!)1. Molecular Formula to Namea. Only use a prefix on the first element if the first element has more than 1 atom exceptwith hydrogen.b. Name the first elementc. Always use a prefix for the second elementd. Name the second element, but change the suffix to ‘ide’Prefixmonoditritetrapentahexa-Number of ber of atoms789101112e. Examples:i. PCl3 – phosphorus trichlorideii. N2O5 – dinitrogen pentoxideiii. N2O – dinitrogen monoxideiv. CCl4 – carbon tetrachloride2. Name to Molecular Formulaa. Determine the symbols for the two elementsb. Name the nonmetal but change the suffix to ‘-ide’c. Examples:i. carbon dioxide – CO2ii. sulfur hexachloride – SCl62
B. Ionic compounds1. Metals with a single chargea. Chemical Formula to Namei. Name the metalii. Name the nonmetal but change the suffix to ‘-ide’iii. Examples:(1) NaCl – sodium chloride(2) AlP – aluminum phosphide(3) BaBr2 – barium bromide(4) Li2O – lithium oxide(5) AgCl – silver chlorideb. Name to Chemical Formulai. Determine the charge on the metal using a periodic tableii. Determine the charge on the nonmetal using a periodic tableiii. If charges are equal, write down the two elements as they areiv. If the charges are unequal, balance them using subscripts(1) lithium fluoride Li and FLi is an alkali metal and therefore has a charge of 1 Li1 F is a nonmetal, halide and has a charge of 1– F1(2)Both charges are equal, so: LiFzinc iodide Zn and IZn is a metal whose charge is always the same, 2 Zn2 I is a group 7 metal and has a charge of –1 I1Charges are not equal so I must have a subscript of 2 in order tobalance the charge and form the neutral compound: ZnI2(3)aluminum oxide Al and OAl is a group 3 metal and has a charge of 3 Al3 O is a group 6 nonmetal and has a charge of 2– O2Charges are not equal so Al must have a subscript of 2 and O asubscript of 3 to balance the charges and form the neutralcompound neutral compound: Al2O32. Metals with multiple charges and a NonmetalExperience is required to know which elements commonly exist in more than onecharge state. But here are some helpful hints. Transition metals, except for zinc,cadmium, and silver, form more than one charge state, plus the non-transitionmetals (also called post-transition metals), tin and lead. These metals are outlined inthe periodic table shown below.The most commonly used cations are listed below with their names. As you can see, thecation charges vary from 1 to 4 . You may think it necessary to memorize thecharges of these cations in order to name an ionic compound, but you will soonrealize that these charges are easily deduced if you know the charge of the anion.(Again, you will have to learn the names of the polyatomic anions and theircharges.)3
Element (English)iron (Fe)iron (Fe)tin (Sn)tin (Sn)lead (Pb)lead (Pb)copper (Cu)copper (Cu)mercury (Hg22 )mercury (Hg2 )chromium (Cr)chromium (Cr)manganese (Mn)manganese (Mn)cobalt (Co)cobalt (Co)Charge2 3 2 4 2 4 1 2 1 2 2 3 2 3 2 3 Stockiron (II)iron (III)tin (II)tin (IV)lead (II)lead (IV)copper (I)copper (II)mercury (I)*mercury (II)chromium (II)chromium (III)manganese (II)manganese (III)cobalt (II)cobalt icmanganousmanganiccobaltouscobaltic*Note: Hg22 consists of two Hg ions bonded into a single polyatomic iona. Chemical Formula to Name (classical system)i. Determine the charge on the metal(1) Look at the charge on the anion(2) Use the subscripts to determine what charge must be balancedii. Name the metal using the classical system (See the table above)(1) Metals of lower charge will have the suffix ‘-ous’(2) Metals of a higher charge will have the suffix ‘-ic’iii. Name the nonmetal as before changing the suffix to ‘ide’iv. Examples:(1) FeOO has a charge of 2–, therefore iron has a charge of 2 andthe name ferrous is used: ferrous oxide(2) PbCl4 Cl has a charge of 1– and there are 4 of them, therefore Pbhas a charge of 4 and the name plumbic is used:plumbic chloride(3) Hg2Se Se has a charge of 2–. Since there are two mercury ions thenthe charge on each ion is 1 and the name mercurous isused: mercurous selenide4
b. Chemical Formula to Name (stock system)i. Determine the charge on the metal(1) Look at the charge on the anion(2) Use the subscripts to determine what charge must be balancedii. Use the name of the metal plus a roman numeral in parenthesis indicating thecharge on the metal.iii. Name the nonmetal as before changing the suffix to ‘ide’iv. Examples:(1) FeOO has a charge of 2–, therefore iron has a charge of 2 andthe roman numeral (II) is used: iron (II) oxide(2) PbCl4 Cl has a charge of 1– and there are 4 of them, therefore Pbhas a charge of 4 and the roman numeral (IV) is used:lead (IV) chloride(3) Hg2Se Se has a charge of 2–. Since there are two mercury ions thenthe charge on each ion is 1 and the roman numeral (I) isused: mercury (I) selenidec. Name to Chemical Formula (classical and stock system)i. Determine charge on metal(1) Charge in classical needs to be memorized(2) Charge in stock gives the charge in Roman numeralsii. Write down the anions based on their names, consulting the periodic table forcharges.iii. Balance using subscriptsiv. Examples:(1) iron (II) chloride – FeCl2(2) plumbic oxide – PbO2II. Polyatomic Ionic CompoundsA polyatomic ion is a covalently bonded group of atoms that either gains or loses electrons to forman ion. While the majority of the common polyatomic ions are anions, there are two commonpolyatomic anions.The only two polyatomic cations that are commonly found in ionic compounds are the ammoniumion, NH4 and the mercury(I) ion, Hg22 . At first glance, the diatomic ion, Hg22 appears to beincorrectly named. However, it is considered to consist of two Hg ions giving an overallcharge of 2 , therefore the ion name is mercury(I) or if you use the Latin system it is called themercurous ion.There are many polyatomic anions that form, most of which you will need to memorize. There area few miscellaneous anion names, but most of the polyatomic anions can be organized in sucha way that their names can be learned in systematic fashion. As in any ionic compound, thecation is listed before the anion in the name and in the chemical formula.5
Tables of polyatomic ions.1. Polyatomic cations: 1 FormulaNH4 Hg22 Nameammoniummercury (I)**Note: Hg22 consists of two Hg ions bonded into a single polyatomic ion2. Polyatomic anions: hiocyanatehydrogen carbonate or bicarbonatehydrogen sulfite or bisulfitehydrogen sulfate or bisulfatedihydrogen phosphatepermanganate*Other halogens (except fluorine) also make oxoanions that are named similarly.**These (and peroxide) are the only polyatomic anions that end in –ide.3. Polyatomic anions: ulfitechromateperoxideoxalatehydrogen phosphate or biphosphatedichromatethiosulfate6
4. Polyatomic anions: Arsenic makes analogous compounds that are named similarly.5. Polyatomic anions: 4–FormulaSiO44–NamesilicateA. Chemical Formula to Name1. Locate the common groups of polyatomic ions in the formula2. Name the polyatomic cation or name the metal as before using the rules for binarycompounds.3. Name the polyatomic anion or name the monatomic anion as before using the rules forbinary compounds.4. Examples:Looking at the table, the only polyatomic ion in this formula isa. Na3PO4phosphate. It acts as the anion. The metal in this formula issodium, therefore, the compound is called sodium phosphate.Looking at the table, the only polyatomic ion in this formula is nitrite.b. Ba(NO2)2It acts as the anion. The metal in this formula is Barium, therefore,the compound is called barium nitrite.c. (NH4)2SO4 Looking at the tables, there are two polyatomic ions in this formula.Ammonium acts as the cation while sulfate acts as the anion. Thecompound is called ammonium sulfate.B. Name to Chemical Formula1. Write down the formula for any polyatomic ion using the tables on polyatomic ionsincluding the charge.2. Write down any monatomic ions given in the name of the formula with their chargeincluded.3. Balance the equation using subscripts, so that the total charge of the compound is 0.4. Examples:a. potassium dichromate The polyatomic ion in the name is dichromate, which isgiven as: Cr2O72–. It is acting as the anion. Potassium,or K , is acting as the cation and is monatomic.Balancing using subscripts gives KCr2O7.b. ammonium chlorideThe polyatomic ion in the name is ammonium, which isgiven as: NH4 . It is acting as the cation. Chloride, orCl–, is acting as the anion and is monatomic. Balancingusing subscripts gives NH4Cl.7
c. ammonium phosphiteThe polyatomic cation in the name is ammonium, which isgiven as: NH4 . The polyatomic anion in the formula isphosphite, which is given as: PO33–. Balancing usingsubscripts gives (NH4)3PO3.III. AcidsFor purposes of naming, each acid may be thought of as a neutral compound formed from ahydrogen ion and an anion. They exist in aqueous form. An aqueous compound is one that hasbeen dissolved in water. Binary acids have a different set of rules of naming than thepolyatomic acids, which are also known as oxoacids.A. Binary acids – Acids with only two elements.1. Add prefix hydro–2. Name anion by changing suffix to ‘–ic’3. Add the word acid4. Examples”a. HCl(aq) – hydrochloric acidb. H2S(aq) – hydrosulfuric acidc. HBr(aq) – hydrobromic acidd. H2Se(aq) – hydroselenic acidB. Polyatomic acids1. Acids derived from anions that end in ‘–ite’a. Name the anion by replacing the suffix ‘–ite’ with ‘–ous’b. Add the word acidc. Examples:i. H2SO3(aq) – sulfurous acidii. H3PO3(aq) – phosphorous acidiii. HNO2(aq) – nitrous acid2. Acids derived from anions that end in ‘–ate’a. Name the anion by replacing the suffix ‘–ate’ with ‘–ic’b. Add the word acidc. Examples:i. H2SO4(aq) – sulfuric acidii. H3PO4(aq) – phosphoric acidiii. HNO3(aq) – nitric acidiv. H2CO3(aq) – carbonic acid8
IV. Some Common NamesYou will frequently encounter common names for widely used compounds. H2O, for instance,could be systematically named dihydrogen oxide (among others), but you know it simply aswater. Sodium hydrogen carbonate or sodium bicarbonate is another compound that has thecommon name of baking soda. Below is a table that contains the common names of somehousehold or industrial 2ONa2S2O3Chemicalcalcium oxidecalcium hydroxidesodium hydroxidepotassium carbonatesodium bicarbonatesodium chloridehydrochloric aciddinitrogen monoxidesodium thiosulfateCommon Namelimeslaked limelyepotashbaking soda, bicarbonate sodatable saltmuriatic acidlaughing gashypoV. Simple Organic NomenclatureOrganic Chemistry is an important branch of chemistry that deals with compounds made up ofcarbon and hydrogen, and sometimes oxygen and/or nitrogen. Throughout organic chemistry,the same root names are consistently used to represent chains and branches of a given numberof carbon atoms. The table below lists the ten simple organic molecules along with their rootnames. Try to note how the number of hydrogen atoms relates to the number of carbon atoms in thelist.Compound 4C7H16C8H18C9H20C10H229
2 I. Binary Compounds A. Covalent Compounds B. Ionic Compounds 1. Metals with a single charge a. alkali metals (1 charge) b. alkaline earth metals (2 charge) c. Aluminum ion (3 charge), Silver ion (1 charge), Zinc ion (2 charge), and Cadmium ion (2 charge) 2. Metals with multiple charges I
4.3 More complex nomenclature systems, 49 4.4 Coordination nomenclature, an additive nomenclature, 51 4.5 Substitutive nomenclature, 70 4.6 Functional class nomenclature, 96 5 ASPECTS OF THE NOMENCLATURE OF ORGANOMETALLIC COMPOUNDS, 98 5.1 General, 98 5.2 Derivatives of Main Group elements, 98 5.3 Organometallic derivatives of transition .
Nomenclature and the Nomenclature Committee of IUBMB. He was involved with the work of these two bodies from their inception and made many valued contributions to biochemical nomenclature. Nomenclature, just like chemistry, is a subject that develops continually. New classes of compound require new adaptations of nomenclature and
(2) Nomenclature of alkyl halides Generally, alkyl halides are named based on both the substitutive nomenclature and radicofunctional nomenclature. Common names are already introduced. haloalkane, haloarene (substitutive nomenclature) alkyl halide, aryl halide (radicofunctional nomenclature)
Nomenclature of carbohydrates 1923 Preamble These Recommendations expand and replace the Tentative Rules for Carbohydrate Nomenclature [ 11 issued in 1969 jointly by the IUPAC Commission on the Nomenclature of Organic Chemistry and the TUB-IUPAC Commission on Biochemical Nomenclature (CBN) and reprinted in [2].They also replace other published
1 Unit 6 Covalent Naming Nomenclature Chemical nomenclature is a set of rules to generate systematic names for chemical compounds.The nomenclature used most frequently worldwid
Experiment 15Diodes Lab – Part 1 Experiment 16Diodes Lab – Part 2 Experiment 17Transistor Lab 1 Experiment 18Transistor Lab 2 Experiment 19Transistor Lab 3 Experiment 20Induction, Magnet and Coil Additional Equipment needed: Please refer to the Equipment Needed section in the beginni
Chemical Formulas and Equations continued How Are Chemical Formulas Used to Write Chemical Equations? Scientists use chemical equations to describe reac-tions. A chemical equation uses chemical symbols and formulas as a short way to show what happens in a chemical reaction. A chemical equation shows that atoms are only rearranged in a chemical .
Levenspiel (2004, p. iii) has given a concise and apt description of chemical reaction engineering (CRE): Chemical reaction engineering is that engineering activity concerned with the ex-ploitation of chemical reactions on a commercial scale. Its goal is the successful design and operation of chemical reactors, and probably more than any other ac-File Size: 344KBPage Count: 56Explore further(PDF) Chemical Reaction Engineering, 3rd Edition by Octave .www.academia.edu(PDF) Elements of Chemical Reaction Engineering Fifth .www.academia.eduIntroduction to Chemical Engineering: Chemical Reaction .ethz.chFundamentals of Chemical Reactor Theory1www.seas.ucla.eduRecommended to you b
