For example, organic compounds include molecules with carbon rings and/or chains with hydrogen atoms (see picture below). These compounds are neutral overall. What is the correct formula for Calcium Carbonate? ThoughtCo, Aug. 28, 2020, thoughtco.com/ionic-compound-nomenclature-608607. How do you name alkanes with double bonds? Name metals that can have different oxidation states using roman numerals to indicate positive charge. Therefore, the proper name for this ionic compound is cobalt(III) oxide. Helmenstine, Anne Marie, Ph.D. "How to Name Ionic Compounds." Therefore, strong bases are named following the rules for naming ionic compounds. Which element comes first in a covalent compound? Why are prefixes not needed in naming ionic compounds. Do you use prefixes when naming ionic compounds? 4. Some polyatomic anions contain oxygen. Ionic compounds When a metal element reacts with a non-metal element an ionic compound is formed. )%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. The rules for naming binary molecular compounds are similar to A compound forms when two or more atoms of different elements share, donate, or accept electrons. The net charge of any ionic compound must be zero which also means it must be electrically neutral. By the Stock system, the names are iron(II) chloride and iron(III) chloride (Figure \(\PageIndex{2}\)). In naming ionic compounds, we always name the _____ first. What is chemical formula? This system recognizes that many metals have two common cations. Prefixes are not used to indicate the number of atoms when writing the chemical formula. To correctly specify how many oxygen atoms are in the ion, prefixes and suffixes are again used. 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 . 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 Can prefixes be used for covalent compounds and ionic? When do you use prefixes to name an element? 2. Example: KNO2 is potassium nitrite, while KNO3 is potassium nitrate. For example, copper can form "Cu"^(+)" ions and "Cu"^(2+)" ions. Dihydrogen dioxide, H2O2, is more commonly called hydrogen dioxide or hydrogen peroxide. Name the other non-metal by its elemental name and an -ide ending. Write the proper name for each ionic compound. 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. The number of atoms are written as subscripts to their chemical symbols. % , What errors can you come across when reading a thermometer, How many Hydrogen atoms in the formula 4H3O2. [4] To name them, follow these quick, simple rules: 1. Prefixes are not used in naming ionic compounds, but are used in naming binary molecular compounds. Carbon monoxide contains both carbon and oxygen, which is indicated by the prefix mono = 1. What is the correct name for Al(NO3)3? Using the names of the ions, this ionic compound is named calcium chloride. Thus, Na+ is the sodium ion, Al3+ is the aluminum ion, Ca2+ is the calcium ion, and so forth. The name of a monatomic anion consists of the stem of the element name, the suffix -ide, and then the word ion. The name of this ionic compound is aluminum fluoride. When naming ionic compounds, why do we not use prefixes (mono-di-, tri-, etc.) The name of this ionic compound is potassium chloride. Why are prefixes used in naming covalent compounds? Why are prefixes used in naming covalent compounds? Legal. How to Market Your Business with Webinars? naming ionic compounds, but are used in naming binary molecular If we were to use the stems and suffixes of the common system, the names would be ferrous chloride and ferric chloride, respectively (Figure \(\PageIndex{3}\)) . . Aluminum oxide is an ionic compound. These ions are named by adding the word hydrogen or dihydrogen in front of the name of the anion. How do you name alkenes using systematic names? She has taught science courses at the high school, college, and graduate levels. Prefixes are not used to indicate the number of atoms when writing the chemical formula. Which metals were used by the Indus Valley civilization? Ba3As2 is simply called barium arsenide. Note that arsenic gets the ide suffix because it is an element. There are two ways to make this distinction. to indicate the amount of each ion indie compound? In many cases, nonmetals form more than one binary compound, so prefixes are used to distinguish them. When naming binary ionic compounds, name the cation first (specifying the charge, if necessary), then the nonmetal anion (element stem + -ide). One example is the ammonium sulfate compound in Figure \(\PageIndex{6}\). For example, NaOH is sodium hydroxide, KOH is potassium hydroxide, and Ca(OH) 2 is calcium hydroxide. The prefixes are written at the beginning of the name of each element, with the exception of the prefix mono-, which is not used for the first element. Ionic compounds will follow set of rules, and molecular compounds will follow another. A chemical formula is written from the chemical symbols of elements which constitute the compound. The number of atoms of each element is written as the subscripts of the symbols for each atoms. For example, one Na+ is paired with one Cl-; one Ca2+ is paired with two Br-. Naming covalent molecular compounds: Left then right, use prefixes. Polyatomic anions have negative charges while polyatomic cations have positive charges. Rules for naming simple covalent compounds: Acids are named by the anion they form when dissolved in water. Dr. Helmenstine holds a Ph.D. in biomedical sciences and is a science writer, educator, and consultant. 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. What is the correct formula of lithium perchlorate? Example: The bleaching agent sodium hypochlorite is NaClO. It is still used for carbon monoxide due to the term being in use since early chemistry. compounds for easier identification. Naming Bases Most strong bases contain hydroxide, a polyatomic ion. 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. Please note that ionic compounds (Type I & II binary compound names) never use prefixes to specify how many times an element is present. Sodium forms only a 1+ ion, so there is no ambiguity about the name sodium ion. Sodium forms only a 1+ ion, so there is no ambiguity about the name sodium ion. What is the mass of 7.28 mol of copper (II) nitrate. Accessibility StatementFor more information contact us atinfo@libretexts.orgor check out our status page at https://status.libretexts.org. You'll get a detailed solution from a subject matter expert that helps you learn core concepts. The second component of an ionic compound is the non-metal anion. The process of naming ionic compounds with polyatomic ions is the same as naming binary ionic compounds. In many cases, the stem of the element name comes from the Latin name of the element. Example: FeCl3 is ferric chloride or iron(III) chloride. Therefore, HClO4 is called perchloric acid. Add an 'ide' to the end of the second compound's name. 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). Two ammonium ions need to balance the charge on a single sulfide ion. There is chemistry all around us every day, even if we dont see it. Some examples of molecular compounds are water (H2O) and carbon dioxide (CO2). We are going to focus our attention on ionic compounds. Legal. 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. You add. The method for naming polyatomic ionic compounds is the same as for binary ionic compounds. Remember that this rule only applies to the first element of the two. Name the non-metal furthest to the left on the periodic table by its elemental name. How do you write diphosphorus trioxide? 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. Chemical formula of a compound is used to identify a compound and distinguishes it from other compounds. Why is the word hydro used in the naming binary acids, but not in the naming of oxyacids? 1. Why did scientists decide to use prefixes to name molecular compounds, but not ionic compounds? 4 Which element comes first in a covalent compound? In the simpler, more modern approach, called the Stock system, an ions positive charge is indicated by a roman numeral in parentheses after the element name, followed by the word ion. An ionic compound is a chemical compound held together by ionic bonding. To make life easier, you dont need to include the prefix mono for the first element of the two. compounds. Thus, Fe2+ is called the iron(II) ion, while Fe3+ is called the iron(III) ion. These prefixes can be used to name just about any compound. Table \(\PageIndex{2}\) lists the names of some common monatomic ions. 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 Prefixes are only used for covalent compounds formed from non-metal elements. 2 Do you use prefixes when naming covalent compounds? However, the names of molecular Why are Greek prefixes not used in naming ionic compounds? Prefixes are not used in naming ionic compounds because two ions can combine in only one combination. For example, consider FeCl2 and FeCl3 . Aluminum Trioxide, it is an ionic compound. Find the formula for ionic compounds. 8. The reactants contain a t 2. (1990). Predict the charge on monatomic ions. Do NOT use prefixes to indicate how many of each element is present; this information is implied in the name of the compound. Ionic compounds are named differently. A molecular compound consists of molecules whose formula represent the actual number of atoms bonded together in that molecule. Aluminum Oxide. Sodium chloride is an ionic compound made up of sodium ions and chloride ions in a crystal lattice. For more information, see our tutorial on naming ionic compounds. If there is not a prefix before the first element, it is assumed that there is only one atom of that element. Explanation: Greek prefixes are used for binary (two element) molecular compounds. Chloride always has a 1 charge, so with two chloride ions, we have a total negative charge of 2. since iron can form more than one charge. Weak bases made of ionic compounds are also named using the ionic naming system. Regards. without charges, this is not possible in molecular compounds so prefixes are used. The -ide ending is added to the name of a monoatomic ion of an element. Generally, there are two types of inorganic compounds that can be formed: ionic compounds and molecular compounds. Name the nonmetal by its elemental name and an -ide ending. An ionic compound is named by its cation followed by its anion. In all cases, ionic compound naming gives the positively charged cation first, followed by the negatively charged anion. 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. 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-. Because these elements have only one oxidation state, you dont need to specify anything with a prefix. For ionic, just add the 5. Understandably, the rules for naming organic compounds are a lot more complex than for normal, small molecules. This occurs because the number of oxygen atoms are increasing from hypochlorite to perchlorate, yet the overall charge of the polyatomic ion is still -1. Retrieved from https://www.thoughtco.com/ionic-compound-nomenclature-608607. If they combine with chlorine, we can have "CuCl" and "CuCl"_2". a. Carbon monoxide is one of the few compounds that uses this prefix. Lastly, you will be given different examples to practice with naming chem prefixes. The prefix hypo - is used to indicate the very lowest oxidation state. When naming ionic compounds, it helps to first break down the formula into the cation(s) and the anion(s). two ions can combine in. 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. However, it is virtually never called that. A binary ionic compound is a compound composed of a monatomic metal cation and a monatomic nonmetal anion. The -ic suffix represents the greater of the two cation charges, and the -ous suffix represents the lower one. We do not call the Na+ ion the sodium(I) ion because (I) is unnecessary. Prefixes can be shortened when the ending vowel of the prefix "conflicts" with a starting vowel in the compound. The ClO- ion, for example, is the hypochlorite ion. To signify the number of each element contained in the compound, molecular compounds are named using a systematic approach of prefixes. Do you use prefixes when naming covalent compounds? They have a giant lattice structure with strong ionic bonds. Greek prefixes are used for binary (two element) molecular compounds. Non-metals, in general, share electrons, form covalent bonds, and form molecular 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. How do you name alkanes from Newman projections? According to the Wikipedia article IUPAC nomenclature of inorganic chemistry, he prefix bi- is a deprecated way of indicating the presence of a single hydrogen ion A very common example is the commonplace 'bicarb of soda', or sodium bicarbonate (or using its correct chemical name sodium hydrogen carbonate). 3. Zk2`ae|W/%EZ%{6|E6:P&*OH%3tmN'/$)dH dN bg|'q .WW?BN&!>FA`Z'P66`/hF]y$LA6$DFVHVN"(VSy[mFr
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& o`7f]--!- lOBNh! For example, #"O"_2"# is sometimes called dioxygen. Thanks. 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. Why are prefixes not needed in naming ionic compounds? Do you use prefixes when naming covalent compounds? For example, iron can form two common ions, Fe2+ and Fe3+. These are two different compounds that need two different names. 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. Aluminum oxide is an ionic compound. Why is the word hydro used in the naming binary acids, but not in the naming of oxyacids? The Roman numeral denotes the charge and the oxidation state of the transition metal ion. naming ionic compounds, but are used in naming binary molecular Ionic compound nomenclature or namingis based on the names of the component ions. 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. We know that cobalt can have more than one possible charge; we just need to determine what it is. 2003-2023 Chegg Inc. All rights reserved. Yes, the name for water using the rules for chemical nomenclature is dihydrogen monoxide. To find more on chemical formula, refer here: This site is using cookies under cookie policy . Example: Cu3P is copper phosphide or copper(I) phosphide. Sometimes prefixes are shortened when the ending vowel . This means that the one iron ion must have a 2+ charge. 7 Do you use Greek prefixes when naming a compound? This differentiates polyatomic ions from monatomic ions, which contain only one atom. $Lv*bz2;Z5G f94^]l880>xW;mnX\V sd"lZ]>9xy. 10. Oxide always has a 2 charge, so with three oxide ions, we have a total negative charge of 6. However, this -ous/-ic system is inadequate in some cases, so the Roman numeral system is preferred. Ionic compounds are made up of metal cations (positive ions) and non-metal anions (negative ions). Example: The classic example is the chemical name for water, H2O, which is dihydrogen monoxide or dihydrogen oxide. BINARY MOLECULAR COMPOUNDS Prefixes used to note how many atoms in a compound 1. mono- 6. hexa-2. For example, NO2 would be called nitrogen dioxide, not mononitrogen dioxide. https://www.thoughtco.com/ionic-compound-nomenclature-608607 (accessed March 5, 2023). Polyatomic anions are more common than polyatomic cations as shown in the chart below. Greek prefixes are used to name compounds based on the elemental subscript, which specifies the number of atoms present in the compound. When naming ionic compounds, why do we not use prefixes (mono-di-, tri-, etc.) You can use a chart to see the possible valences for the elements. Do you use Greek prefixes when naming a compound? 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#
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Accessibility StatementFor more information contact us atinfo@libretexts.orgor check out our status page at https://status.libretexts.org. 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. Answers. You can specify conditions of storing and accessing cookies in your browser. Table \(\PageIndex{1}\) lists the elements that use the common system, along with their respective cation names. tetra- 9. nona-5. An acid is a substance that dissociates into hydrogen ions (H+) and anions in water. In most cases, the "mono-" prefix can be omitted, because it is implied when it is not present. Refer to the explanation. Although there may be a element with positive charge like H+, it is not joined with another element with an ionic bond. The Roman numeral naming convention has wider appeal because many ions have more than two valences. 1.30 grams of H are reacted with an excess of N to produce 4.21 grams of NH3- Ionic compounds are named differently. This system is used only for elements that form more than one common positive ion. Using a maximum of ten sentences, respond to one of the two prompts. The number of atoms are written as subscripts to their chemical symbols. Set your categories menu in Theme Settings -> Header -> Menu -> Mobile menu (categories), CO= carbon monoxide. Thus, as we have already seen, Cl is chlor- + -ide ion, or the chloride ion. ThoughtCo. When naming a binary molecular compound, the subscript for each element determines what prefix should be used. 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. $%t_Um4hET2q4^
_1!C_ Community Answer The NO 3- ion, for example, is the nitrate ion. Ions combine in only one ratio, so prefixes are not needed. Why are prefixes not used in naming ionic compounds. c. Neither charge is an exact multiple of the other, so we have to go to the least common multiple of 6. two ions can combine in only one combination. For example, we might think to call C2H6 dicarbon hexahydride, but in reality its called ethane. Ionic compound base names contain two words: The first word is the name of the cation. They are named by first the cation, then the anion. 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. 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. Biochemical Nomenclature and Related Documents, London:Portland Press, 1992. However, it is virtually never called that. When naming molecular compounds prefixes are used to dictate the number of a given element present in the compound. For both molecular and ionic compounds, change the name of the second compound so it ends in 'ide'; ex: fluorine = fluoride . sulfur and oxygen), name the lower one first. When naming ionic compounds, why do we not use prefixes (mono-di-, tri-, etc.) The metal is changed to end in ous or ic. After learning a few more details about the names of individual ions, you will be one step away from knowing how to name ionic compounds. How do you name alkenes with two double bonds? The metal cation is named first, followed by the nonmetal anion as illustrated in Figure \(\PageIndex{1}\) for the compound BaCl2. It is also sometimes called the sodium salt of hypochlorous acid. The hypo- and per- prefixes indicate less oxygen and more oxygen, respectively. Focuses on when to use Greek prefixes and Roman numerals, and how to quickl. Nitrogen triiodide is the inorganic compound with the formula NI3. There are two rules that must be followed through: The cation (metal) is always named first with its name unchanged The anion (nonmetal) is written after the cation, modified to end in -ide Example 1 Na+ + Cl- = NaCl; Ca2+ + 2Br- = CaBr2 Sodium + Chlorine = Sodium Chloride; Calcium + Bromine = Calcium Bromide to indicate the number of that element in the molecule. The entire field of organic chemistry is devoted to studying the way carbon bonds. when naming ionic compounds those are only used in naming covalent molecular compounds. Ternary compounds are composed of three or more elements. These anions are called oxyanions. 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. Question: Using a maximum of ten sentences, respond to one of the two prompts. Use just the element name. 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. Dont worry about those rules for now its just something to keep in the back of your mind! Traditional naming Simple ionic compounds. Naming ionic compound with polyvalent ion. When an element forms two oxyanions, the one with less oxygen is given a name ending in -ite and the one with more oxygen are given a name that ends in -ate. Ionic compounds have the simplest naming convention: nothing gets a prefix. The following table lists the most common prefixes for binary covalent compounds. Each element, carbon and. suffix -ide. When naming a binary molecular compound, the subscript for each element determines what prefix should be used. Thus, we need a different name for each iron ion to distinguish Fe2+ from Fe3+. 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. First, you need to determine what type of compound it is. For example,magnesium chloride contains one magnesium and two chlorine atoms thus, its formula is MgCl. to indicate the amount of each ion indie compound? 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. Polyatomic ions. Why is the word hydro used in the naming binary acids, but not in the naming of oxyacids? 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. To use the rules for naming ionic compounds. Cations have positive charges while anions have negative charges. In addition, the prefix mono-is not used with the first element; for example, SO 2 is sulfur dioxide, not "monosulfur dioxide". Which is the correct way to name a compound? Helmenstine, Anne Marie, Ph.D. "How to Name Ionic Compounds." Prefixes are not used in naming ionic compounds, but are used in naming binary molecular compounds. Ba 3 As 2 is simply called "barium arsenide." Note that arsenic gets the "ide" suffix because it is an element. 1 Do you use prefixes when naming ionic compounds? { "5.01:_Sugar_and_Salt" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.
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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.
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