Molly Johnson Obituary,
Aubrey Paige Ryan Seacrest,
Articles W
The number of atoms are written as subscripts to their chemical symbols. 3 What are the rules for naming an ionic compound? A compound forms when two or more atoms of different elements share, donate, or accept electrons. uddPlBAl(|!n
mEUCUCqXZD:0r>gGd`\' ]$"jA2,MT`1~YvR"2IuNr:;q 2 2 Shubham Choudhary Using the names of the ions, this ionic compound is named calcium chloride. What is the mass of 7.28 mol of copper (II) nitrate. naming ionic compounds, but are used in naming binary molecular Helmenstine, Anne Marie, Ph.D. (2020, August 28). Ionic compounds with transition metals will contain prefixes to denote oxidation states, but those are not prefixes. They have a giant lattice structure with strong ionic bonds. We encounter many ionic compounds every. Experts are tested by Chegg as specialists in their subject area. CO = carbon monoxide BCl3 = borontrichloride, CO2 = carbon dioxide N2O5 =dinitrogen pentoxide. 3H + N2 2NH3 Prefixes are not used to indicate the number of atoms when writing the chemical formula. 3. Some elements, like carbon, bond differently than most others. 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. Ionic compounds will follow set of rules, and molecular compounds will follow another. 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 . Ionic compounds are named differently. Map: Chemistry & Chemical Reactivity (Kotz et al. The hypo- and per- prefixes indicate less oxygen and more oxygen, respectively. A lot of energy is needed to. Which is the correct way to name a compound? Why are Greek prefixes not used in naming ionic compounds? Refer to the explanation. sulfur and oxygen), name the lower one first. A molecular compound consists of molecules whose formula represent the actual number of atoms bonded together in that molecule. Because the rules of nomenclature say so. Then, assign a prefix based on the list at the beginning of this article (mono for 1, di for 2, et cetera). If they combine with chlorine, we can have "CuCl" and "CuCl"_2". When you have a polyatomic ion with one more oxygen than the -ate ion, then your acid will have the prefix per- and the suffix -ic. For example, the chlorate ion is ClO3. To use the rules for naming ionic compounds. Put the two elements together, and dont forget the ide on the second element. Answers. This occurs because if the atoms formed an ionic bond, then it would have already become a compound, thus not needing to gain or loose any electrons. ThoughtCo, Aug. 28, 2020, thoughtco.com/ionic-compound-nomenclature-608607. However, it is virtually never called that. Prefixes are not used in https://www.thoughtco.com/ionic-compound-nomenclature-608607 (accessed March 5, 2023). Because these elements have only one oxidation state, you don't need to specify anything with a prefix. 9th. " mono-" indicates one, "di-" indicates two, "tri-" is three, "tetra-" is four, "penta-" is five, and "hexa-" is six, "hepta-" is seven, "octo-" is eight, "nona-" is nine, and "deca" is ten. Name the second element as if it were an anion that uses the -ide ending. It is just like an ionic compound except that the element further down and to the left on the periodic table is listed first and is named with the element name. Covalent bonds are molecules made up of non-metals that are linked together by shared electrons. You'll get a detailed solution from a subject matter expert that helps you learn core concepts. When do you use prefixes for molecular compounds? For example, one Na+ is paired with one Cl-; one Ca2+ is paired with two Br-. Common polyatomic ions. di- 7. hepta-3. 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:[\
Sometimes prefixes are shortened when the ending vowel . Do you use Greek prefixes when naming a compound? Ammonium Permanganate; NH4MnO4 --> NH4+ + MnO4- --> Ammonium Permanganate, c. Cobalt (II) Thiosulfate; CoS2O3 --> Co + S2O32- --> Cobalt must have +2 charge to make a neutral compund --> Co2+ + S2O32- --> Cobalt(II) Thiosulfate. FROM THE STUDY SET Chapter 3 View this set By clicking Accept All Cookies, you agree to the storing of cookies on your device to enhance site navigation, analyze site usage, and assist in our marketing efforts. The ClO- ion, for example, is the hypochlorite ion. 4. Table \(\PageIndex{1}\) lists the elements that use the common system, along with their respective cation names. Covalent Bonds: When it comes to atoms and how they interact with one another, it is important to understand the type of bond that. However, some of the transition metals' charges have specific Latin names. Set your categories menu in Theme Settings -> Header -> Menu -> Mobile menu (categories), CO= carbon monoxide. Why is the word hydro used in the naming binary acids, but not in the naming of oxyacids? mono- indicates one, di- indicates two, tri- is three, tetra- is four, penta- is five, and hexa- is six, hepta- is seven, octo- is eight, nona- is nine, and deca is ten. The second system, called the common system, is not conventional but is still prevalent and used in the health sciences. 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. When naming a binary molecular compound, the subscript for each element determines what prefix should be used. Prefixes should not be used to indicate how many of each element is present; this information is implied in the compound's name. Ionic compound nomenclature or namingis based on the names of the component ions. The following are the Greek prefixes used for naming binary molecular compounds. compounds. To indicate different polyatomic ions made up of the same elements, the name of the ion is modified according to the example below: To combine the topic of acids and polyatomic ions, there is nomenclature of aqueous acids. Use the prefixes mono-, di-, tri-. For example, NaOH is sodium hydroxide, KOH is potassium hydroxide, and Ca(OH) 2 is calcium hydroxide. Yes, the name for water using the rules for chemical nomenclature is dihydrogen monoxide. Key Terms 8 When do you use prefixes to name an element? One example is the ammonium sulfate compound in Figure \(\PageIndex{6}\). , What errors can you come across when reading a thermometer, How many Hydrogen atoms in the formula 4H3O2. Prefixes are not used in 1.6K views In most cases, the "mono-" prefix can be omitted, because it is implied when it is not present. , The equation below represents a chemical reaction that occurs in living cells. For example- Ionic Compounds with Polyatomic Ions Ionic compounds are formed when metals combine with polyatomic ions. molecule. Add the name of the non-metal with an -ide ending. For example, iron can form two common ions, Fe2+ and Fe3+. C6H12O6 + 6O2 ------> 6CO2 + 6H2O + energy To correctly specify how many oxygen atoms are in the ion, prefixes and suffixes are again used. Prefixes are not used in naming ionic compounds, but are used in naming binary molecular compounds. suffix -ide. Retrieved from https://www.thoughtco.com/ionic-compound-nomenclature-608607. It is also sometimes called the sodium salt of hypochlorous acid. Therefore, strong bases are named following the rules for naming ionic compounds. Name the non-metal furthest to the left on the periodic table by its elemental name. They are named by first the cation, then the anion. When naming molecular compounds prefixes are used to dictate the number of a given element present in the compound. Prefixes are used to denote the number of atoms 4. Iron, for example, can form two cations, each of which, when combined with the same anion, makes a different compound with unique physical and chemical properties. Biochemical Nomenclature and Related Documents, London:Portland Press, 1992. These ions are named by adding the word hydrogen or dihydrogen in front of the name of the anion. In addition, the prefix mono-is not used with the first element; for example, SO 2 is sulfur dioxide, not "monosulfur dioxide". What is the correct formula for Calcium Carbonate? Aluminum oxide is an ionic compound. $%t_Um4hET2q4^
_1!C_ Prefixes are not used in naming ionic compounds because two ions can combine in only one combination. Some anions have multiple forms and are named accordingly with the use of roman numerals in parentheses. Write the proper name for each ionic compound. Why are prefixes not needed in naming ionic compounds. Community Q&A Search Add New Question Question What is the difference between ionic compounds and covalent compounds? Aluminum Oxide. Rules for naming simple covalent compounds: Acids are named by the anion they form when dissolved in water. When naming molecular compounds prefixes are used to dictate the number of a given element present in the compound. Yes, the name for water using the rules for chemical nomenclature is dihydrogen monoxide. The first compound is composed of copper 1+ ions bonded to choride 1 . You will also learn the basics of these chemistry prefixes and how they are applicable in the real world today! Common Acid and Anion Names The same issue arises for other ions with more than one possible charge. A chemical formula is written from the chemical symbols of elements which constitute the compound. Aluminum Trioxide, it is an ionic compound. On the other hand, the anion is named by removing the last syllable and adding -ide. Naming covalent molecular compounds: Left then right, use prefixes. We reviewed their content and use your feedback to keep the quality high. When naming binary ionic compounds, name the cation first (specifying the charge, if necessary), then the nonmetal anion (element stem + -ide). When do you use prefixes to name an element? The rules for naming binary molecular compounds are similar to Do you use prefixes when naming ionic compounds? This notation is usually seen with metals since they commonly display more than one oxidation state or valence. The most common ones are shown in the table below: Several exceptions apply to the Roman numeral assignment: Aluminum, Zinc, and Silver. Why is the word hydro used in the naming binary acids, but not in the naming of oxyacids? Similarly, O2 is the oxide ion, Se2 is the selenide ion, and so forth. Covalent or Molecular Compound Properties, Empirical Formula: Definition and Examples, Why the Formation of Ionic Compounds Is Exothermic, The Difference Between a Cation and an Anion, Properties of Ionic and Covalent Compounds, Compounds With Both Ionic and Covalent Bonds, Ph.D., Biomedical Sciences, University of Tennessee at Knoxville, B.A., Physics and Mathematics, Hastings College. The second system, called the common system, is not conventional but is still prevalent and used in the health sciences. Prefixes are only used for covalent compounds formed from non-metal elements. Iron can also have more than one possible charge. Comment on the feasibility of a naming scheme where hydro is used when naming oxyacids and omitted when naming binary acids. compounds include prefixes that indicate the number of atoms in the Prefixes in molecular compounds are decided by the number of atoms of each element in the compound. The word ion is dropped from both parts. naming ionic compounds, but are used in naming binary molecular 3. Roman numerals are used in naming ionic compounds when the metal cation forms more than one ion. For example, NO2 would be called nitrogen dioxide, not mononitrogen dioxide. For example,magnesium chloride contains one magnesium and two chlorine atoms thus, its formula is MgCl. Thanks. For more information, see our tutorial on naming ionic compounds. Thus, as we have already seen, Cl is chlor- + -ide ion, or the chloride ion. Ionic compound base names contain two words: The first word is the name of the cation. The net charge of any ionic compound must be zero which also means it must be electrically neutral. 8. Each element, carbon and. In the second compound, the iron ion has a 3+ charge, as indicated by the three Cl ions in the formula. The number of atoms of each element is written as the subscripts of the symbols for each atoms. Using a maximum of ten sentences, respond to one of the two prompts. To add the "-ide" ending, just drop the 1 or 2 syllables ("-ine" in this case), and add "-ide" instead. stream Example: The classic example is the chemical name for water, H2O, which is dihydrogen monoxide or dihydrogen oxide. See polyatomic ion for a list of possible ions. The -ic suffix represents the greater of the two cation charges, and the -ous suffix represents the lower one. An ionic compound is named by its cation followed by its anion. By adding oxygens to the molecule in number 9, we now have H3PO4? Sodium forms only a 1+ ion, so there is no ambiguity about the name sodium ion. In this tutorial, you will be introduced to the different types of chemistry prefixes. An acid is a substance that dissociates into hydrogen ions (H+) and anions in water. Greek prefixes are used for binary (two element) molecular compounds. If you continue to use this site we will assume that you are happy with it. Choose the correct answer: According to naming rules, the types of compound that use prefixes in their names are A) ionic compounds. 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. Ionic compounds are made up of metal cations (positive ions) and non-metal anions (negative ions). Atoms are electrically neutral because the number of protons, which carry a 1+ charge, in the nucleus of an atom is equal to the number of electrons, which carry a 1- charge, in the atom. compounds. We use cookies to ensure that we give you the best experience on our website. Therefore, HClO4 is called perchloric acid. In naming ionic compounds, we always name the _____ first. A binary ionic compound is a compound composed of a monatomic metal cation and a monatomic nonmetal anion. How do you name alkenes with two double bonds? We also acknowledge previous National Science Foundation support under grant numbers 1246120, 1525057, and 1413739. What is chemical formula? How do you name alkenes with double bonds? 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. The polyatomic ions have their own characteristic names, as discussed earlier. The cation is the element name followed by a Roman numeral in parentheses if the element has multiple charges. The -ate ending indicates a high oxidation state. When naming ionic compounds, why do we not use prefixes (mono-di-, tri-, etc.) For both molecular and ionic compounds, change the name of the second compound so it ends in 'ide'; ex: fluorine = fluoride . Name the nonmetal by its elemental name and an -ide ending. 1. First name the element that is leftmost on the periodic table. The following are the Greek prefixes used for naming binary molecular compounds. Greek prefixes are used to name compounds based on the elemental subscript, which specifies the number of atoms present in the compound. To find more on chemical formula, refer here: This site is using cookies under cookie policy . Ba 3 As 2 is simply called "barium arsenide." Note that arsenic gets the "ide" suffix because it is an element. When naming ionic compounds, list the cation first and the anion second. For example, a compound that has 5 atoms of a particular element would have the penta prefix before that element in the compounds name. Therefore, the proper name for this ionic compound is iron(II) chloride. The prefix per - (as in hyper-) is used to indicate the very highest oxidation state. Such acids include sulfuric acid (H2SO4) or carbonic acid (H2CO3). How do you name alkanes from Newman projections? Two ammonium ions need to balance the charge on a single sulfide ion. The common system uses two suffixes (-ic and -ous) that are appended to the stem of the element name. Common exceptions exist for naming molecular compounds, where trivial or common names are used instead of systematic names, such as ammonia (NH 3) instead of nitrogen trihydride or water (H 2 O) instead of dihydrogen monooxide. The prefix mono- is not used for the first element. The name of the second element loses one or two syllables and ends in the suffix -ide. These are two different compounds that need two different names. 2. We do not call the Na+ ion the sodium(I) ion because (I) is unnecessary. The name of a monatomic anion consists of the stem of the element name, the suffix -ide, and then the word ion. $Lv*bz2;Z5G f94^]l880>xW;mnX\V sd"lZ]>9xy. This differentiates polyatomic ions from monatomic ions, which contain only one atom. 2 0 obj Thus, Na+ is the sodium ion, Al3+ is the aluminum ion, Ca2+ is the calcium ion, and so forth. Ba3As2 is simply called barium arsenide. Note that arsenic gets the ide suffix because it is an element. to indicate the number of that element in the molecule. )%2F02%253A_Atoms_Molecules_and_Ions%2F2.10%253A_Naming_Binary_Nonmetal_Compounds, \( \newcommand{\vecs}[1]{\overset { \scriptstyle \rightharpoonup} {\mathbf{#1}}}\) \( \newcommand{\vecd}[1]{\overset{-\!-\!\rightharpoonup}{\vphantom{a}\smash{#1}}} \)\(\newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\) \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\) \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\) \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\) \( \newcommand{\Span}{\mathrm{span}}\) \(\newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\) \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\) \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\) \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\) \( \newcommand{\Span}{\mathrm{span}}\)\(\newcommand{\AA}{\unicode[.8,0]{x212B}}\), --> Cobalt must have +2 charge to make a neutral compund --> Co, Compounds between Metals and Nonmetals (Cation and Anion), Compounds between Nonmetals and Nonmetals, International Union of Pure and Applied Chemistry, status page at https://status.libretexts.org, Pettrucci, Ralph H. General Chemistry: Principles and Modern Applications. Which metals were used by the Indus Valley civilization? The transition metals may form more than one ion, thus it is needed to be specified which particular ion we are talking about. Carbon monoxide contains both carbon and oxygen, which is indicated by the prefix mono = 1. The compounds name is iron(II) phosphate. 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. Dr. Helmenstine holds a Ph.D. in biomedical sciences and is a science writer, educator, and consultant. To name them, follow these quick, simple rules: 1. The hypo- and per- prefixes indicate less oxygen and more oxygen, respectively. are used in naming. In this compound, the cation is based on nickel. Naming Ionic Compounds Using-ous and -ic, Naming Ionic Compounds Using-ite and -ate, Naming Ionic Compounds Using hypo- and per-, Ionic Compounds Containing bi- and di- Hydrogen. What is the name of this molecule? Chlorine becomes chloride. In all cases, ionic compound naming gives the positively charged cation first, followed by the negatively charged anion. These endings are added to the Latin name of the element (e.g., stannous/stannic for tin) to represent the ions with lesser or greater charge, respectively. Prefixes are used to denote the number of atoms. Nitrogen triiodide is the inorganic compound with the formula NI3. Weak bases made of ionic compounds are also named using the ionic naming system. 6 When do you use prefixes for molecular compounds? Although HF can be named hydrogen fluoride, it is given a different name for emphasis that it is an acid. You add prefixes ONLY to covalent. Name the other non-metal by its elemental name and an -ide ending. The prefix hypo - is used to indicate the very lowest oxidation state. Molecular compounds do not have such constraints and therefore must use prefixes to denote the number of atoms present. The following table lists the most common prefixes for binary covalent compounds. The ammonium ion has a 1+ charge and the sulfide ion has a 2 charge. Prefixes for Ionic Compounds Ionic compounds have the simplest naming convention: nothing gets a prefix. The Roman numeral naming convention has wider appeal because many ions have more than two valences. Visit this website if you would like to learn more about how we use compounds every day! For example, we might think to call C2H6 dicarbon hexahydride, but in reality its called ethane. The entire field of organic chemistry is devoted to studying the way carbon bonds. Legal. The first step is to count the number of each element. In polyatomic ions, polyatomic (meaning two or more atoms) are joined together by covalent bonds. The above list shows the 10 most basic chemistry prefixes for naming compounds, which come from Greek. The method for naming polyatomic ionic compounds is the same as for binary ionic compounds. When naming molecular compounds prefixes are used to dictate the number of a given element present in the compound. Question: Using a maximum of ten sentences, respond to one of the two prompts. Ternary compounds are composed of three or more elements. For example, organic compounds include molecules with carbon rings and/or chains with hydrogen atoms (see picture below). 4. 10. Write the non-metal's name with an "-ide" ending. B) ionic compounds involving transition metals. How to Market Your Business with Webinars? Dihydrogen dioxide, H2O2, is more commonly called hydrogen dioxide or hydrogen peroxide. when naming ionic compounds those are only used in naming covalent molecular compounds. Naming monatomic ions and ionic compounds. The metal cation is named first, followed by the nonmetal anion as illustrated in Figure \(\PageIndex{1}\) for the compound BaCl2. However, it is virtually never called that. Traditional naming Simple ionic compounds. The -ide ending is added to the name of a monoatomic ion of an element. { "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.