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. Nitrogen triiodide is the inorganic compound with the formula NI3. They are named by first the cation, then the anion. Cations have positive charges while anions have negative charges. 2. Nomenclature is the process of naming chemical compounds with different names so that they can be easily identified as separate chemicals. Set your categories menu in Theme Settings -> Header -> Menu -> Mobile menu (categories), CO= carbon monoxide. are used in naming. To name acids, the prefix hydro- is placed in front of the nonmetal modified to end with ic. Figure \(\PageIndex{1}\) is a synopsis of how to name simple ionic compounds. 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:[\
ThoughtCo, Aug. 28, 2020, thoughtco.com/ionic-compound-nomenclature-608607. Note: when the addition of the Greek prefix places two vowels adjacent to one another, the "a" (or the "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 . Aluminum oxide is an ionic compound. A quick way to identify acids is to see if there is an H (denoting hydrogen) in front of the molecular formula of the compound. Chlorine becomes chloride. What is the correct name for Al(NO3)3? Thanks. When naming molecular compounds prefixes are used to dictate the number of a given element present in the compound. Dihydrogen dioxide, H2O2, is more commonly called hydrogen dioxide or hydrogen peroxide. Dont get frustrated with yourself if you dont understand it right away. Example: Cu3P is copper phosphide or copper(I) phosphide. It is still used for carbon monoxide due to the term being in use since early chemistry. Remember that this rule only applies to the first element of the two. The name of this ionic compound is potassium chloride. Understandably, the rules for naming organic compounds are a lot more complex than for normal, small molecules. We do not call the Na+ ion the sodium(I) ion because (I) is unnecessary. How do you name alkenes using systematic names? In most cases, the "mono-" prefix can be omitted, because it is implied when it is not present. The prefix per - (as in hyper-) is used to indicate the very highest oxidation state. If you continue to use this site we will assume that you are happy with it. CO = carbon monoxide BCl3 = borontrichloride, CO2 = carbon dioxide N2O5 =dinitrogen pentoxide. In this compound, the cation is based on nickel. Why are prefixes not needed in naming ionic compounds? You use a variety of different compounds in every day life! The -ide ending is added to the name of a monoatomic ion of an element. Question: 3.24 Determine the charge on copper in each of the following ionic compounds: (a) CuCl2 (b) CuzN (c) Cuo (d) Cu 3.25 Determine the charge on iron in each of the following ionic compounds: (a) Fe 0; (b) FeCl, (c) Fe (d) FeN SECTION 3.3: NAMING IONS AND BINARY IONIC COMPOUNDS 3.26 Why do we not use Greek prefixes to specify the number of ions of each type when Now that we're familiar with polyatomic ions, let's learn how to name ionic compounds when given their chemical formulas by using the following steps: Step 1 Determine the "base name" of the ionic compound. When naming ionic compounds, why do we not use prefixes (mono-di-, tri-, etc.) Write the correct name for these compounds. In all cases, ionic compound naming gives the positively charged cation first, followed by the negatively charged anion. Prefixes are used to denote the number of atoms 4. 4. Dont worry about those rules for now its just something to keep in the back of your mind! Legal. Biochemical Nomenclature and Related Documents, London:Portland Press, 1992. For example- Ionic Compounds with Polyatomic Ions Ionic compounds are formed when metals combine with polyatomic ions. For example, one Na+ is paired with one Cl-; one Ca2+ is paired with two Br-. For both molecular and ionic compounds, change the name of the second compound so it ends in 'ide'; ex: fluorine = fluoride . It is also sometimes called the sodium salt of hypochlorous acid. The number of atoms of each element is written as the subscripts of the symbols for each atoms. In the first compound, the iron ion has a 2+ charge because there are two Cl ions in the formula (1 charge on each chloride ion). Pui Yan Ho (UCD), Alex Moskaluk (UCD), Emily Nguyen (UCD). The naming system is used by determining the number of each atom in the compound. What is the correct formula of phosphorus trichloride? The metal is changed to end in ous or ic. This is indicated by assigning a Roman numeral after the metal. FROM THE STUDY SET Chapter 3 View this set The hypo- and per- prefixes indicate less oxygen and more oxygen, respectively. { "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. According to Table 2.6 Prefixes for Indicating the Number of Atoms in Chemical Names, the prefix for two is di-, and the prefix for four is tetra-. Ionic compounds have the simplest naming convention: nothing gets a prefix. How do you name alkynes with two triple bonds. What is the name of this molecule? two ions can combine in. Traditional naming Simple ionic compounds. Prefixes are not used in naming ionic compounds because two ions can combine in only one combination. sulfur and oxygen), name the lower one first. Some examples of molecular compounds are water (H2O) and carbon dioxide (CO2). Because these elements have only one oxidation state, you don't need to specify anything with a prefix. When naming a binary molecular compound, the subscript for each element determines what prefix should be used. We are going to focus our attention on ionic compounds. On the other hand, the anion is named by removing the last syllable and adding -ide. A molecular compound consists of molecules whose formula represent the actual number of atoms bonded together in that molecule. molecule. Thus, we need a different name for each iron ion to distinguish Fe2+ from Fe3+. Compounds that consist of a nonmetal bonded to a nonmetal are commonly known as Molecular Compounds, where the element with the positive oxidation state is written first. 8. 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. , The equation below represents a chemical reaction that occurs in living cells. There are two ways to make this distinction. This means that the one iron ion must have a 2+ charge. This system is used commonly in naming acids, where H2SO4 is commonly known as Sulfuric Acid, and H2SO3 is known as Sulfurous Acid. the ions in ionic compounds have known charges that have to add to zero, so the numbers of each ion can be deduced. Answers. Add the name of the non-metal with an -ide ending. Ionic compounds are made up of metal cations (positive ions) and non-metal anions (negative ions). You'll get a detailed solution from a subject matter expert that helps you learn core concepts. An ionic compound is named by its cation followed by its anion. The net charge of any ionic compound must be zero which also means it must be electrically neutral. The metal cation is named first, followed by the nonmetal anion as illustrated in Figure \(\PageIndex{1}\) for the compound BaCl2. 6 When do you use prefixes for molecular compounds? However, it is virtually never called that. In many cases, nonmetals form more than one binary compound, so prefixes are used to distinguish them. Inorganic compounds are compounds that do not deal with the formation of carbohydrates, or simply all other compounds that do not fit into the description of an organic compound. In many cases, the stem of the element name comes from the Latin name of the element. We do not call the Na + ion the sodium (I) ion because (I) is unnecessary. Predict the charge on monatomic ions. How do you name alkanes with double bonds? Weak bases made of ionic compounds are also named using the ionic naming system. The common system uses two suffixes (-ic and -ous) that are appended to the stem of the element name. We also acknowledge previous National Science Foundation support under grant numbers 1246120, 1525057, and 1413739. A compound forms when two or more atoms of different elements share, donate, or accept electrons. Although there may be a element with positive charge like H+, it is not joined with another element with an ionic bond. Ionic compounds are named differently. Community Q&A Search Add New Question Question What is the difference between ionic compounds and covalent compounds? When naming binary ionic compounds, name the cation first (specifying the charge, if necessary), then the nonmetal anion (element stem + -ide). 3. Sodium chloride is an ionic compound made up of sodium ions and chloride ions in a crystal lattice. Pls Upvote. 9th. The first step is to count the number of each element. 10. Accessibility StatementFor more information contact us atinfo@libretexts.orgor check out our status page at https://status.libretexts.org. When naming binary ionic compounds, name the cation first (specifying the charge, if necessary), then the nonmetal anion (element stem + -ide). The number of atoms are written as subscripts to their chemical symbols. You add prefixes ONLY to covalent. The subscripts for each atom in the formula of an ionic compound is the charge of the other atom into which it is bonded. Please note that ionic compounds (Type I & II binary compound names) never use prefixes to specify how many times an element is present. For example, iron can form two common ions, Fe2+ and Fe3+. What holds the packing in a stuffing box? to indicate the amount of each ion indie compound? 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. When naming ionic compounds, why do we not use prefixes (mono-di-, tri-, etc.) The name of a monatomic anion consists of the stem of the element name, the suffix -ide, and then the word ion. ClO - Hypochlorite ClO 2- Chlorite ClO 3- Chlorate ClO 4- Perchlorate The second system, called the common system, is not conventional but is still prevalent and used in the health sciences. Write the proper name for each ionic compound. For example, consider FeCl2 and FeCl3 . In polyatomic ions, polyatomic (meaning two or more atoms) are joined together by covalent bonds. Ba3As2 is simply called barium arsenide. Note that arsenic gets the ide suffix because it is an element. Can prefixes be used for covalent compounds and ionic? Although they belong to the transition metal category, these metals do not have Roman numerals written after their names because these metals only exist in one ion. When do you use prefixes for molecular compounds? c. Neither charge is an exact multiple of the other, so we have to go to the least common multiple of 6. There are a few easy steps that you can use for chemistry prefixes. Prefixes are not used in naming ionic compounds, but are used in naming binary molecular compounds. The Roman numeral naming convention has wider appeal because many ions have more than two valences. Do you use prefixes when naming covalent compounds? suffix -ide. stream A covalent compound is usually composed of two or more nonmetal elements. In general, the prefix mono- is rarely used. What was the percent yield for ammonia in this reactio 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. It is important to include (aq) after the acids because the same compounds can be written in gas phase with hydrogen named first followed by the anion ending with ide. Two ammonium ions need to balance the charge on a single sulfide ion. Because these elements have only one oxidation state, you dont need to specify anything with a prefix. To use the rules for naming ionic compounds. 4 Which element comes first in a covalent compound? The prefix mono- is not used for the first element. We have seen that some elements lose different numbers of electrons, producing ions of different charges (Figure 3.3). suffix -ide. The polyatomic ions have their own characteristic names, as discussed earlier. Do NOT use prefixes to indicate how many of each element is present; this information is implied in the name of the compound. The following are the Greek prefixes used for naming binary molecular compounds. 3 What are the rules for naming an ionic compound?