why are prefixes not used in naming ionic compounds

6. Write the non-metal's name with an "-ide" ending. https://www.thoughtco.com/ionic-compound-nomenclature-608607 (accessed March 5, 2023). What are Rules for Prefix in a compound? + Example - Socratic.org For example, one Na+ is paired with one Cl-; one Ca2+ is paired with two Br-. Ionic compounds are made up of metal cations (positive ions) and non-metal anions (negative ions). 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. Experts are tested by Chegg as specialists in their subject area. Add an 'ide' to the end of the second compound's name. Example: The bleaching agent sodium hypochlorite is NaClO. The name of the compound is simply the name of the positive element followed by the name of the negative element adding the -ide suffix: MgF 2 (Magnesium Fluoride), AlCl 3 (Aluminum Chloride), or Al 2 O 3 (Aluminum Oxide) Notice that in ionic nomenclature you do not use the Greek prefixes to indicate the number of atoms in the molecule. The method for naming polyatomic ionic compounds is the same as for binary ionic compounds. Can prefixes be used for covalent compounds and ionic? )%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. Why are prefixes not needed in naming ionic compounds. Why is the word hydro used in the naming binary acids, but not in the naming of oxyacids? compounds for easier identification. What holds the packing in a stuffing box? a. When naming ionic compounds, it helps to first break down the formula into the cation(s) and the anion(s). Instead of using Roman numerals, the different ions can also be presented in plain words. An acid is a substance that dissociates into hydrogen ions (H+) and anions in water. Prefixes are not used to indicate the number of atoms when writing the chemical formula. What is chemical formula? The second system, called the common system, is not conventional but is still prevalent and used in the health sciences. 3 Ways to Name Ionic Compounds - wikiHow Which metals were used by the Indus Valley civilization? Comment on the feasibility of a naming scheme where hydro is used. Prefixes are used to denote the number of atoms. What is the correct name for Al(NO3)3? Rules for Naming Ionic Compounds - Video & Lesson Transcript - Study.com ThoughtCo. Generally, there are two types of inorganic compounds that can be formed: ionic compounds and molecular compounds. Regards. Naming Compounds | Boundless Chemistry | | Course Hero Pui Yan Ho (UCD), Alex Moskaluk (UCD), Emily Nguyen (UCD). Solved Using a maximum of ten sentences, respond to one of | Chegg.com This is indicated by assigning a Roman numeral after the metal. We know that cobalt can have more than one possible charge; we just need to determine what it is. The following are the Greek prefixes used for naming binary molecular compounds. For example, we might think to call C2H6 dicarbon hexahydride, but in reality its called ethane. Some examples of molecular compounds are water (H2O) and carbon dioxide (CO2). Common polyatomic ions. Name metals that can have different oxidation states using roman numerals to indicate positive charge. As indicated by the arrow, moving to the right, the following trends occur: Increasing oxidation state of the nonmetal, (Usage of this example can be seen from the set of compounds containing Cl and O). 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 The first compound is composed of copper 1+ ions bonded to choride 1 . However, these compounds have many positively and negatively charged particles. 5.7: Naming Ionic Compounds is shared under a CC BY-NC-SA 4.0 license and was authored, remixed, and/or curated by LibreTexts. Molecular compounds do not have such constraints and therefore must use prefixes to denote the number of atoms present. 2.10: Naming Binary, Nonmetal Compounds is shared under a CC BY-NC-SA 4.0 license and was authored, remixed, and/or curated by LibreTexts. These prefixes can be used to name just about any compound. Chemical formula of a compound is used to identify a compound and distinguishes it from other compounds. The NO 3- ion, for example, is the nitrate ion. We do not call the Na + ion the sodium (I) ion because (I) is unnecessary. Using the names of the ions, this ionic compound is named calcium chloride. This system recognizes that many metals have two common cations. However, it is virtually never called that. Upper Saddle River: Pearson Prentice Hall, 2007, Nomenclature of Inorganic Chemistry, Recommendations 1990, Oxford:Blackwell Scientific Publications. Write the proper name for each ionic compound. The -ic suffix represents the greater of the two cation charges, and the -ous suffix represents the lower one. 8 When do you use prefixes to name an element? Chemistry: What's in a Name? Ionic Nomenclature What is the correct formula of lithium perchlorate? penta- 10. deca- Rules for naming molecular compounds: Less-electronegative element is given first First element only gets a prefix if it has more than one Second element is named by combining These are two different compounds that need two different names. 2. If they combine with chlorine, we can have "CuCl" and "CuCl"_2". How do you name alkenes using systematic names? You will also learn the basics of these chemistry prefixes and how they are applicable in the real world today! The hypo- and per- prefixes indicate less oxygen and more oxygen, respectively. How do you name alkanes with double bonds? Thus, Fe2+ is called the iron(II) ion, while Fe3+ is called the iron(III) ion. To use the rules for naming ionic compounds. To add the "-ide" ending, just drop the 1 or 2 syllables ("-ine" in this case), and add "-ide" instead. Therefore, HClO4 is called perchloric acid. For example, NO2 would be called nitrogen dioxide, not mononitrogen dioxide. 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 Roman numeral naming convention has wider appeal because many ions have more than two valences. 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 prefix hypo - is used to indicate the very lowest oxidation state. 9th. These ions are named by adding the word hydrogen or dihydrogen in front of the name of the anion. since iron can form more than one charge. The following table lists the most common prefixes for binary covalent compounds. These compounds are neutral overall. Community Q&A Search Add New Question Question What is the difference between ionic compounds and covalent compounds? 4. Example: KNO2 is potassium nitrite, while KNO3 is potassium nitrate. 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. Retrieved from https://www.thoughtco.com/ionic-compound-nomenclature-608607. 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. compounds include prefixes that indicate the number of atoms in the The name of this ionic compound is aluminum fluoride. 2 0 obj Because these elements have only one oxidation state, you don't need to specify anything with a prefix. If you are given a formula for an ionic compound whose cation can have more than one possible charge, you must first determine the charge on the cation before identifying its correct name. Why aren't prefixes used in naming ionic compounds? Try these next 3 examples on your own to see how you do with naming compounds! The metal cation is named first, followed by the nonmetal anion as illustrated in Figure \(\PageIndex{1}\) for the compound BaCl2. 3H + N2 2NH3 Comment on the feasibility of a naming scheme where hydro is used when naming oxyacids and omitted when naming binary acids. To signify the number of each element contained in the compound, molecular compounds are named using a systematic approach of prefixes. 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. IUPAC nomenclature of inorganic chemistry - Wikipedia sulfur and oxygen), name the lower one first. Why are prefixes not needed in naming ionic compounds? The metal is changed to end in ous or ic. They have a giant lattice structure with strong ionic bonds. 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-. Why is the word hydro used in the naming binary acids, but not in the naming of oxyacids? The common system uses two suffixes (-ic and -ous) that are appended to the stem of the element name. Figure \(\PageIndex{1}\) is a synopsis of how to name simple ionic compounds. , The equation below represents a chemical reaction that occurs in living cells. The -ide ending is added to the name of a monoatomic ion of an element. 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). How to Name Binary Covalent Compounds - dummies Use the prefixes mono-, di-, tri-. Chemistry Prefixes | ChemTalk See polyatomic ion for a list of possible ions. 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. Prefixes are not used to indicate the number of atoms when writing the chemical formula. Greek prefixes are used to name compounds based on the elemental subscript, which specifies the number of atoms present in the compound. What is the correct formula of phosphorus trichloride? Polyatomic ions & Common polyatomic ions (article) | Khan Academy Prefixes should not be used to indicate how many of each element is present; this information is implied in the compound's name. naming ionic compounds, but are used in naming binary molecular The polyatomic ions have their own characteristic names, as discussed earlier. 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. Naming Bases Most strong bases contain hydroxide, a polyatomic ion. to indicate the amount of each ion indie compound? two ions can combine in only one combination. Helmenstine, Anne Marie, Ph.D. (2020, August 28). Why is it necessary to use prefixes in naming covalent compounds For both molecular and ionic compounds, change the name of the second compound so it ends in 'ide'; ex: fluorine = fluoride . Therefore, strong bases are named following the rules for naming ionic compounds. By the Stock system, the names are iron(II) chloride and iron(III) chloride (Figure \(\PageIndex{2}\)). Each element, carbon and. 4. However, this -ous/-ic system is inadequate in some cases, so the Roman numeral system is preferred. Naming monatomic ions and ionic compounds. Weak bases made of ionic compounds are also named using the ionic naming system. This section begins the formal study of nomenclature, the systematic naming of chemical compounds. We use common names rather than systematic names for some simple covalent compounds. Enter a Melbet promo code and get a generous bonus, An Insight into Coupons and a Secret Bonus, Organic Hacks to Tweak Audio Recording for Videos Production, Bring Back Life to Your Graphic Images- Used Best Graphic Design Software, New Google Update and Future of Interstitial Ads. BINARY MOLECULAR COMPOUNDS Prefixes used to note how many atoms in a compound 1. mono- 6. hexa-2. Naming Acids and Bases | Introduction to Chemistry | | Course Hero Find the formula for ionic compounds. It is an ionic compound, therefore no prefixes Prefixes for Ionic Compounds Ionic compounds have the simplest naming convention: nothing gets a prefix. 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. two ions can combine in only one combination. Pls Upvote. without charges, this is not possible in molecular compounds so prefixes are used. For ionic, just add the Why aren't prefixes used to name ionic compounds? - Quora two ions can combine in. The ammonium ion has a 1+ charge and the sulfide ion has a 2 charge. What was the percent yield for ammonia in this reactio , What errors can you come across when reading a thermometer, How many Hydrogen atoms in the formula 4H3O2. Aluminum oxide is an ionic compound. Traditional naming Simple ionic compounds. Most studied answer Answer: The charges on the ions dictate how many must be present to form a neutral unit. If there is not a prefix before the first element, it is assumed that there is only one atom of that element. 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. Covalent compounds are named with number prefixes to identify the number of atoms in the molecule. 1. Then, assign a prefix based on the list at the beginning of this article (mono for 1, di for 2, et cetera). Naming Ionic Compounds - Nomenclature Rules - Science Notes and Projects Do you use prefixes when naming ionic compounds? It is still used for carbon monoxide due to the term being in use since early chemistry. In many cases, nonmetals form more than one binary compound, so prefixes are used to distinguish them. When naming ionic compounds, why do we not use prefixes (mono-di-, tri-, etc.) Carbonyl Compounds - Reactants, Catalysts and Products How do you write diphosphorus trioxide? Naming ionic compounds with -ide and -ate - BBC Bitesize Sodium forms only a 1+ ion, so there is no ambiguity about the name sodium ion. Do NOT use prefixes to indicate how many of each element is present; this information is implied in the name of the compound. In naming ionic compounds, we always name the _____ first. You can use a chart to see the possible valences for the elements. Why are prefixes used in naming covalent compounds? di- 7. hepta-3. When naming molecular compounds prefixes are used to dictate the number of a given element present in the compound. Helmenstine, Anne Marie, Ph.D. "How to Name Ionic Compounds." Naming Covalent Compounds - Rules for Naming Covalent Compounds - BYJUS For example, in NaCl, Na is sodium and Cl is chlorine. Explanation: Greek prefixes are used for binary (two element) molecular compounds. 55: Naming compounds: When to use Greek prefixes or Roman - YouTube Names and formulas of ionic compounds. 8. Positive and negative charges must balance. With a little bit of practice, naming compounds will become easier and easier! Predict the charge on monatomic ions. Example Fe2+ is Iron(II). When naming a binary molecular compound, the subscript for each element determines what prefix should be used. An overview of naming molecular and ionic compounds common to general chemistry. to indicate the number of that element in the molecule. The transition metals may form more than one ion, thus it is needed to be specified which particular ion we are talking about. An ionic compound is named by its cation followed by its anion. Similarly, O2 is the oxide ion, Se2 is the selenide ion, and so forth. Because the rules of nomenclature say so. Accessibility StatementFor more information contact us atinfo@libretexts.orgor check out our status page at https://status.libretexts.org. FROM THE STUDY SET Chapter 3 View this set Prefixes are used to denote the number of atoms 4. Is prefixes a compound? Explained by Sharing Culture Ionic and Covalent Bonding - Department of Chemistry & Biochemistry For example,magnesium chloride contains one magnesium and two chlorine atoms thus, its formula is MgCl. 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. When naming ionic compounds, list the cation first and the anion second. Ionic compounds are named differently. 4. Ions combine in only one ratio, so prefixes are not needed. Name the nonmetal by its elemental name and an -ide ending. The second system, called the common system, is not conventional but is still prevalent and used in the health sciences. b. The -ate ending indicates a high oxidation state. The name of a monatomic anion consists of the stem of the element name, the suffix -ide, and then the word ion. { "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.