Sodium forms only a 1+ ion, so there is no ambiguity about the name sodium ion. Prefixes used for Covalent Compounds. The following table lists the most common prefixes for binary covalent compounds. 3 What are the rules for naming an ionic compound? Similarly, the formula of iron oxide containing 2 Fe and 3 O is written as FeO. Predict the charge on monatomic ions. Ionic compounds are made up of metal cations (positive ions) and non-metal anions (negative ions). An acid is a substance that dissociates into hydrogen ions (H+) and anions in water. Why is the word hydro used in the naming binary acids, but not in the naming of oxyacids? Common polyatomic ions. In this compound, the cation is based on nickel. In many cases, nonmetals form more than one binary compound, so prefixes are used to distinguish them. The metal is changed to end in ous or ic. When naming ionic compounds, why do we not use prefixes (mono-di-, tri-, etc.) To correctly specify how many oxygen atoms are in the ion, prefixes and suffixes are again used. 3H + N2 2NH3 1.C; Calcium + Carbonate --> Ca2+ + CO32- --> CaCO3, 2.D; FeO --> Fe + O2- --> Iron must have a charge of +2 to make a neutral compound --> Fe2+ + O2- --> Iron(II) Oxide, 3.A; Al(NO3)3 --> Al3+ + (NO3-)3 --> Aluminum nitrate, 4.B; Phosphorus trichloride --> P + 3Cl --> PCl3, 5.D, LiClO4; Lithium perchlorate --> Li+ + ClO4- --> LiClO4, 6. a. Beryllium Oxalate; BeC2O4 --> Be2+ + C2O42- --> Beryllium Oxalate, b. Ionic compounds have the simplest naming convention: nothing gets a prefix. The metal cation is named first, followed by the nonmetal anion as illustrated in Figure \(\PageIndex{1}\) for the compound BaCl2. The first step is to count the number of each element. Choose the correct answer: According to naming rules, the types of compound that use prefixes in their names are A) ionic compounds. For ionic, just add the Positive and negative charges must balance. The name of a monatomic anion consists of the stem of the element name, the suffix -ide, and then the word ion. Neo is used in the naming of the common nomenclature or organic A molecular compound consists of molecules whose formula represent the actual number of atoms bonded together in that molecule. to indicate the amount of each ion indie compound? FROM THE STUDY SET Chapter 3 View this set Naming Ionic Compounds Using hypo- and per- In the case where there is a series of four oxyanions, the hypo- and per- prefixes are used in conjunction with the -ite and -ate suffixes. Once you have determined each prefix, you need to add the ide suffix if the second name in the compound is an element (this is sometimes not the case for more complex molecules). How to Market Your Business with Webinars? Ionic compounds with transition metals will contain prefixes to denote oxidation states, but those are not prefixes. Prefixes for Ionic Compounds Ionic compounds have the simplest naming convention: nothing gets a prefix. In all cases, ionic compound naming gives the positively charged cation first, followed by the negatively charged anion. 2 0 obj When naming ionic compounds, it helps to first break down the formula into the cation(s) and the anion(s). Yes, the name for water using the rules for chemical nomenclature is dihydrogen monoxide. If both elements are in the same column (e.g. Use just the element name. x\KsF\fzFU50 hY/ $ii~?oO.N8FY3DBDO*y\?KqX!n=8Zh+2D1F~EB&|x\dTE^hgVSk^Xy/cbadOc)/p.R]8%FC+#abg U4V&2sCWbvq2rO6V&V")P]>JD| eP"~0z9bi\ q# vE2[zs^7-xZ|y'.2>j]y*=[ZdeC[%5|QrEneUduyZRpS:[\ Nitrogen triiodide is the inorganic compound with the formula NI3. Map: Chemistry & Chemical Reactivity (Kotz et al. Write the non-metal's name with an "-ide" ending. Thus, we need a different name for each iron ion to distinguish Fe2+ from Fe3+. The reactants contain a t Answers. { "5.01:_Sugar_and_Salt" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "5.02:_Compounds_Display_Constant_Composition" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "5.03:_Chemical_Formulas-_How_to_Represent_Compounds" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "5.04:_A_Molecular_View_of_Elements_and_Compounds" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "5.05:_Writing_Formulas_for_Ionic_Compounds" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "5.06:_Nomenclature-_Naming_Compounds" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "5.07:_Naming_Ionic_Compounds" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "5.08:_Naming_Molecular_Compounds" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "5.09:_Naming_Acids" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "5.10:_Nomenclature_Summary" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "5.11:_Formula_Mass-_The_Mass_of_a_Molecule_or_Formula_Unit" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()" }, { "00:_Front_Matter" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "01:_The_Chemical_World" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "02:_Measurement_and_Problem_Solving" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "03:_Matter_and_Energy" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "04:_Atoms_and_Elements" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "05:_Molecules_and_Compounds" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "06:_Chemical_Composition" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "07:_Chemical_Reactions" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "08:_Quantities_in_Chemical_Reactions" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "09:_Electrons_in_Atoms_and_the_Periodic_Table" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "10:_Chemical_Bonding" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "11:_Gases" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "12:_Liquids,_Solids,_and_Intermolecular_Forces" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "13:_Solutions" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "14:_Acids_and_Bases" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "zz:_Back_Matter" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()" }, [ "article:topic", "showtoc:no", "license:ccbyncsa", "licenseversion:40" ], https://chem.libretexts.org/@app/auth/3/login?returnto=https%3A%2F%2Fchem.libretexts.org%2FCourses%2FCollege_of_Marin%2FCHEM_114%253A_Introductory_Chemistry%2F05%253A_Molecules_and_Compounds%2F5.07%253A_Naming_Ionic_Compounds, \( \newcommand{\vecs}[1]{\overset { \scriptstyle \rightharpoonup} {\mathbf{#1}}}\) \( \newcommand{\vecd}[1]{\overset{-\!-\!\rightharpoonup}{\vphantom{a}\smash{#1}}} \)\(\newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\) \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\) \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\) \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\) \( \newcommand{\Span}{\mathrm{span}}\) \(\newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\) \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\) \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\) \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\) \( \newcommand{\Span}{\mathrm{span}}\)\(\newcommand{\AA}{\unicode[.8,0]{x212B}}\), Example \(\PageIndex{3}\): Naming Ionic Compounds, Example \(\PageIndex{5}\): Naming Ionic Compounds, Naming Binary Ionic Compounds with a Metal that Forms Only One Type of Cation, Naming Binary Ionic Compounds with a Metal That Forms More Than One Type of Cation, Naming Ionic Compounds with Polyatomic Ions, 1.4: The Scientific Method: How Chemists Think, Chapter 2: Measurement and Problem Solving, 2.2: Scientific Notation: Writing Large and Small Numbers, 2.3: Significant Figures: Writing Numbers to Reflect Precision, 2.6: Problem Solving and Unit Conversions, 2.7: Solving Multistep Conversion Problems, 2.10: Numerical Problem-Solving Strategies and the Solution Map, 2.E: Measurement and Problem Solving (Exercises), 3.3: Classifying Matter According to Its State: Solid, Liquid, and Gas, 3.4: Classifying Matter According to Its Composition, 3.5: Differences in Matter: Physical and Chemical Properties, 3.6: Changes in Matter: Physical and Chemical Changes, 3.7: Conservation of Mass: There is No New Matter, 3.9: Energy and Chemical and Physical Change, 3.10: Temperature: Random Motion of Molecules and Atoms, 3.12: Energy and Heat Capacity Calculations, 4.4: The Properties of Protons, Neutrons, and Electrons, 4.5: Elements: Defined by Their Numbers of Protons, 4.6: Looking for Patterns: The Periodic Law and the Periodic Table, 4.8: Isotopes: When the Number of Neutrons Varies, 4.9: Atomic Mass: The Average Mass of an Elements Atoms, 5.2: Compounds Display Constant Composition, 5.3: Chemical Formulas: How to Represent Compounds, 5.4: A Molecular View of Elements and Compounds, 5.5: Writing Formulas for Ionic Compounds, 5.11: Formula Mass: The Mass of a Molecule or Formula Unit, 6.5: Chemical Formulas as Conversion Factors, 6.6: Mass Percent Composition of Compounds, 6.7: Mass Percent Composition from a Chemical Formula, 6.8: Calculating Empirical Formulas for Compounds, 6.9: Calculating Molecular Formulas for Compounds, 7.1: Grade School Volcanoes, Automobiles, and Laundry Detergents, 7.4: How to Write Balanced Chemical Equations, 7.5: Aqueous Solutions and Solubility: Compounds Dissolved in Water, 7.6: Precipitation Reactions: Reactions in Aqueous Solution That Form a Solid, 7.7: Writing Chemical Equations for Reactions in Solution: Molecular, Complete Ionic, and Net Ionic Equations, 7.8: AcidBase and Gas Evolution Reactions, Chapter 8: Quantities in Chemical Reactions, 8.1: Climate Change: Too Much Carbon Dioxide, 8.3: Making Molecules: Mole-to-Mole Conversions, 8.4: Making Molecules: Mass-to-Mass Conversions, 8.5: Limiting Reactant, Theoretical Yield, and Percent Yield, 8.6: Limiting Reactant, Theoretical Yield, and Percent Yield from Initial Masses of Reactants, 8.7: Enthalpy: A Measure of the Heat Evolved or Absorbed in a Reaction, Chapter 9: Electrons in Atoms and the Periodic Table, 9.1: Blimps, Balloons, and Models of the Atom, 9.5: The Quantum-Mechanical Model: Atoms with Orbitals, 9.6: Quantum-Mechanical Orbitals and Electron Configurations, 9.7: Electron Configurations and the Periodic Table, 9.8: The Explanatory Power of the Quantum-Mechanical Model, 9.9: Periodic Trends: Atomic Size, Ionization Energy, and Metallic Character, 10.2: Representing Valence Electrons with Dots, 10.3: Lewis Structures of Ionic Compounds: Electrons Transferred, 10.4: Covalent Lewis Structures: Electrons Shared, 10.5: Writing Lewis Structures for Covalent Compounds, 10.6: Resonance: Equivalent Lewis Structures for the Same Molecule, 10.8: Electronegativity and Polarity: Why Oil and Water Dont Mix, 11.2: Kinetic Molecular Theory: A Model for Gases, 11.3: Pressure: The Result of Constant Molecular Collisions, 11.5: Charless Law: Volume and Temperature, 11.6: Gay-Lussac's Law: Temperature and Pressure, 11.7: The Combined Gas Law: Pressure, Volume, and Temperature, 11.9: The Ideal Gas Law: Pressure, Volume, Temperature, and Moles, 11.10: Mixtures of Gases: Why Deep-Sea Divers Breathe a Mixture of Helium and Oxygen, Chapter 12: Liquids, Solids, and Intermolecular Forces, 12.3: Intermolecular Forces in Action: Surface Tension and Viscosity, 12.6: Types of Intermolecular Forces: Dispersion, DipoleDipole, Hydrogen Bonding, and Ion-Dipole, 12.7: Types of Crystalline Solids: Molecular, Ionic, and Atomic, 13.3: Solutions of Solids Dissolved in Water: How to Make Rock Candy, 13.4: Solutions of Gases in Water: How Soda Pop Gets Its Fizz, 13.5: Solution Concentration: Mass Percent, 13.9: Freezing Point Depression and Boiling Point Elevation: Making Water Freeze Colder and Boil Hotter, 13.10: Osmosis: Why Drinking Salt Water Causes Dehydration, 14.1: Sour Patch Kids and International Spy Movies, 14.4: Molecular Definitions of Acids and Bases, 14.6: AcidBase Titration: A Way to Quantify the Amount of Acid or Base in a Solution, 14.9: The pH and pOH Scales: Ways to Express Acidity and Basicity, 14.10: Buffers: Solutions That Resist pH Change, status page at https://status.libretexts.org. Aluminum Trioxide, it is an ionic compound. , The equation below represents a chemical reaction that occurs in living cells. A covalent compound is usually composed of two or more nonmetal elements. If you continue to use this site we will assume that you are happy with it. Why are Greek prefixes not used in naming ionic compounds? This is indicated by assigning a Roman numeral after the metal. When do you use prefixes for molecular compounds? Naming ionic compound with polyvalent ion. Legal. Which is the correct way to name a compound? For example, NO2 would be called nitrogen dioxide, not mononitrogen dioxide. Ions combine in only one ratio, so prefixes are not needed. Atom the smallest unit of a chemical element, made from protons, neutrons, and electrons, Prefixes the name that comes before the molecule, Compounds a chemical species composed of two or more elements, Periodic table a table of chemical elements that is arranged in order of atomic number, Oxidation State a number assigned to an element that represents the number of electrons lost or gained, Transition Metal elements from the d-block of the periodic table, which can have more than one configuration of valence electrons, Roman Numerals tells you the oxidation state of the transition metal ion, Element a substance that cannot be chemically broken down into simpler components. Using the names of the ions, this ionic compound is named calcium chloride. What is chemical formula? The following are the Greek prefixes used for naming binary molecular compounds. The process of naming ionic compounds with polyatomic ions is the same as naming binary ionic compounds. Yes, the name for water using the rules for chemical nomenclature is dihydrogen monoxide. This section begins the formal study of nomenclature, the systematic naming of chemical compounds. In most cases, the "mono-" prefix can be omitted, because it is implied when it is not present. Table \(\PageIndex{1}\) lists the elements that use the common system, along with their respective cation names. It is still common to see and use the older naming convention in which the prefix bi- is used to indicate the addition of a single hydrogen ion. In many cases, the stem of the element name comes from the Latin name of the element. To make life easier, you dont need to include the prefix mono for the first element of the two. For example, consider FeCl2 and FeCl3 . What is the name of this molecule? Key Terms There are two rules that must be followed through: Na+ + Cl- = NaCl; Ca2+ + 2Br- = CaBr2, Sodium + Chlorine = Sodium Chloride; Calcium + Bromine = Calcium Bromide. The -ic suffix represents the greater of the two cation charges, and the -ous suffix represents the lower one. $Lv*bz2;Z5G f94^]l880>xW;mnX\V sd"lZ]>9xy. When naming ionic compounds, why do we not use prefixes (mono-di-, tri-, etc.) Just like the other nomenclature rules, the ion of the transition metal that has the lower charge has the Latin name ending with -ous and the one with the the higher charge has a Latin name ending with -ic. The net charge of any ionic compound must be zero which also means it must be electrically neutral. 1. What are the rules for naming an ionic compound? We are going to focus our attention on ionic compounds. Then, assign a prefix based on the list at the beginning of this article (mono for 1, di for 2, et cetera). Retrieved from https://www.thoughtco.com/ionic-compound-nomenclature-608607. The metals that form more than one ion are the transition metals, although not all of them do this. When naming molecular compounds prefixes are used to dictate the number of a given element present in the compound. The entire field of organic chemistry is devoted to studying the way carbon bonds. Subscripts in the formula do not affect the name. The polyatomic ions have their own characteristic names, as discussed earlier. The NO 3- ion, for example, is the nitrate ion. How do you write diphosphorus trioxide? two ions can combine in. In polyatomic ions, polyatomic (meaning two or more atoms) are joined together by covalent bonds. C6H12O6 + 6O2 ------> 6CO2 + 6H2O + energy HF (g) = hydrogen fluoride -> HF (aq) = hydrofluoric acid, HBr (g) = hydrogen bromide -> HBr (aq) = hydrobromic acid, HCl (g) = hydrogen chloride -> HCl (aq) = hydrochloric acid, H2S (g) = hydrogen sulfide -> H2S (aq) = hydrosulfuricacid. Name the second element as if it were an anion that uses the -ide ending. These compounds are neutral overall. Name the nonmetal by its elemental name and an -ide ending. By the Stock system, the names are iron(II) chloride and iron(III) chloride (Figure \(\PageIndex{2}\)). Cations have positive charges while anions have negative charges. Categorize each statement as a naming property for molecular compounds, ionic compounds, or polyatomic ions.-cations with a fixed or variable charge-greek prefix may be on first or second element-positively charged chemical names end in -onium -roman numerals used to denote charges-no charge indicated in the formula-suffixes usually end in -ite or -ate-no prefix on the first or second element . For example, we might think to call C2H6 dicarbon hexahydride, but in reality its called ethane. In naming ionic compounds, we always name the _____ first. The hypo- and per- prefixes indicate less oxygen and more oxygen, respectively. Put the two elements together, and dont forget the ide on the second element. How do you name alkanes with double bonds? https://www.thoughtco.com/ionic-compound-nomenclature-608607 (accessed March 5, 2023). You use a variety of different compounds in every day life! Molecular compounds do not have such constraints and therefore must use prefixes to denote the number of atoms present. The -ide ending is added to the name of a monoatomic ion of an element. Prefixes should not be used to indicate how many of each element is present; this information is implied in the compound's name. Common Acid and Anion Names If they combine with chlorine, we can have "CuCl" and "CuCl"_2". To distinguish the difference, Fe2+ would be named iron (II) and Fe3+ would be named iron (III). Here are the principal naming conventions for ionic compounds, along with examples to show how they are used: A Roman numeral in parentheses, followed by the name of the element, is used for elements that can form more than one positive ion. Because these elements have only one oxidation state, you dont need to specify anything with a prefix. For example, a compound that has 5 atoms of a particular element would have the penta prefix before that element in the compounds name. The number of atoms are written as subscripts to their chemical symbols. Although HF can be named hydrogen fluoride, it is given a different name for emphasis that it is an acid. This means that the one iron ion must have a 2+ charge. The cation is the element name followed by a Roman numeral in parentheses if the element has multiple charges. When two or more elements share electrons in a covalent bond, they form molecular compounds.