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Name the nonmetal by its elemental name and an -ide ending. Prefixes are only used for covalent compounds formed from non-metal elements. Why are prefixes not used in naming ionic compounds. Naming ionic compounds. Put the two elements together, and dont forget the ide on the second element. Figure \(\PageIndex{1}\) is a synopsis of how to name simple ionic compounds. We do not call the Na+ ion the sodium(I) ion because (I) is unnecessary. Polyatomic anions sometimes gain one or more H+ ions to form anions of a lower charge. to indicate the amount of each ion indie compound? 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 common system uses two suffixes (-ic and -ous) that are appended to the stem of the element name. The transition metals may form more than one ion, thus it is needed to be specified which particular ion we are talking about. If we were to use the stems and suffixes of the common system, the names would be ferrous chloride and ferric chloride, respectively (Figure \(\PageIndex{3}\)) . Greek prefixes are used to name compounds based on the elemental subscript, which specifies the number of atoms present in the compound. To name acids, the prefix hydro- is placed in front of the nonmetal modified to end with ic. Common polyatomic ions. What is a the prefix we use to indicate 4 in covalent naming? If they combine with chlorine, we can have "CuCl" and "CuCl"_2". Which is the correct way to name a compound? Why is the word hydro used in the naming binary acids, but not in the naming of oxyacids? stream Remember that this rule only applies to the first element of the two. Legal. Prefixes are not used in 2. 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. 2. How do you name alkynes with two triple bonds. 4. The most common ones are shown in the table below: Several exceptions apply to the Roman numeral assignment: Aluminum, Zinc, and Silver. A chemical formula is written from the chemical symbols of elements which constitute the compound. When naming ionic compounds, why do we not use prefixes (mono-di-, tri-, etc.) Common Acid and Anion Names Explanation: Greek prefixes are used for binary (two element) molecular compounds. It is an ionic compound, therefore no prefixes Using the names of the ions, this ionic compound is named calcium chloride. The cation is the element name followed by a Roman numeral in parentheses if the element has multiple charges. In this compound, the cation is based on nickel. Why are prefixes not needed in naming ionic compounds. We do not call the Na + ion the sodium (I) ion because (I) is unnecessary. 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 . Using a maximum of ten sentences, respond to one of the two prompts. When naming binary ionic compounds, name the cation first (specifying the charge, if necessary), then the nonmetal anion (element stem + -ide). This system is used only for elements that form more than one common positive ion. two ions can combine in only one combination. The Roman numeral naming convention has wider appeal because many ions have more than two valences. Regards. 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. Ionic compounds with transition metals will contain prefixes to denote oxidation states, but those are not prefixes. Using a maximum of ten sentences, respond to one of the two prompts. Ionic compounds are named differently. suffix -ide. There is chemistry all around us every day, even if we dont see it. Two ammonium ions need to balance the charge on a single sulfide ion. An acid is a substance that dissociates into hydrogen ions (H+) and anions in water. The method for naming polyatomic ionic compounds is the same as for binary ionic compounds. Table \(\PageIndex{2}\) lists the names of some common monatomic ions. A compound forms when two or more atoms of different elements share, donate, or accept electrons. Non-metals, in general, share electrons, form covalent bonds, and form molecular compounds. Map: Chemistry & Chemical Reactivity (Kotz et al. Write the correct name for these compounds. to indicate the amount of each ion indie compound? You use a variety of different compounds in every day life! 7 Do you use Greek prefixes when naming a compound? For example- Ionic Compounds with Polyatomic Ions Ionic compounds are formed when metals combine with polyatomic ions. Yes, the name for water using the rules for chemical nomenclature is dihydrogen monoxide. In this tutorial, you will be introduced to the different types of chemistry prefixes. 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. Naming monatomic ions and ionic compounds. However, this -ous/-ic system is inadequate in some cases, so the Roman numeral system is preferred. The compounds name is iron(II) phosphate. two ions can combine in only one combination. Traditional naming Simple ionic compounds. since iron can form more than one charge. 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. Name the non-metal furthest to the left on the periodic table by its elemental name. In all cases, ionic compound naming gives the positively charged cation first, followed by the negatively charged anion. 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. What is the name of this molecule? The name of a monatomic anion consists of the stem of the element name, the suffix -ide, and then the word ion. The subscripts for each atom in the formula of an ionic compound is the charge of the other atom into which it is bonded. ClO - Hypochlorite ClO 2- Chlorite ClO 3- Chlorate ClO 4- Perchlorate Thus, as we have already seen, Cl is chlor- + -ide ion, or the chloride ion. Which metals were used by the Indus Valley civilization? Helmenstine, Anne Marie, Ph.D. "How to Name Ionic Compounds." The cation is named first, followed by the anion. Cations have positive charges while anions have negative charges. What is the correct formula of phosphorus trichloride? 3. How do you name alkanes from Newman projections? Refer to the explanation. Comment on the feasibility of a naming scheme where hydro is used. Why are prefixes not used in naming ionic compounds? Understandably, the rules for naming organic compounds are a lot more complex than for normal, small molecules. By the Stock system, the names are iron(II) chloride and iron(III) chloride (Figure \(\PageIndex{2}\)). For example, organic compounds include molecules with carbon rings and/or chains with hydrogen atoms (see picture below). molecule. When naming a binary molecular compound, the subscript for each element determines what prefix should be used. compounds for easier identification. Image credit: Wikipedia Commons, public domain. They have a giant lattice structure with strong ionic bonds. 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 in molecular compounds are decided by the number of atoms of each element in the compound. If both elements are in the same column (e.g. Nitrogen triiodide is the inorganic compound with the formula NI3. Ternary compounds are composed of three or more elements. Helmenstine, Anne Marie, Ph.D. "How to Name Ionic Compounds." 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). to indicate the number of that element in the molecule. ThoughtCo. Prefixes are not used in naming ionic compounds because two ions can combine in only one combination. For more information, see our tutorial on naming ionic compounds. 1 Do you use prefixes when naming ionic compounds? When naming ionic compounds, it helps to first break down the formula into the cation(s) and the anion(s). The number of atoms are written as subscripts to their chemical symbols. The prefix poly- means many, so a polyatomic ion is an ion that contains more than one atom. Upper Saddle River: Pearson Prentice Hall, 2007, Nomenclature of Inorganic Chemistry, Recommendations 1990, Oxford:Blackwell Scientific Publications. )%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. Ionic compounds consist of cations (positive ions) and anions (negative ions). When naming molecular compounds prefixes are used to dictate the number of a given element present in the compound. A quick way to identify acids is to see if there is an H (denoting hydrogen) in front of the molecular formula of the compound. Iron can also have more than one possible charge. Ionic compounds are made up of metal cations (positive ions) and non-metal anions (negative ions). Visit this website if you would like to learn more about how we use compounds every day! Naming ionic compound with polyvalent ion. The -ic suffix represents the greater of the two cation charges, and the -ous suffix represents the lower one. Aluminum Oxide. Please note that ionic compounds (Type I & II binary compound names) never use prefixes to specify how many times an element is present. Set your categories menu in Theme Settings -> Header -> Menu -> Mobile menu (categories), CO= carbon monoxide. However, the names of molecular We are going to focus our attention on ionic compounds. two ions can combine in. These ions are named by adding the word hydrogen or dihydrogen in front of the name of the anion. There is no space between the element name and the parenthesis. Find the formula for ionic compounds. Mono is not used to name the first element. To signify the number of each element contained in the compound, molecular compounds are named using a systematic approach of prefixes. We use cookies to ensure that we give you the best experience on our website. You can use a chart to see the possible valences for the elements. Prefixes are not used to indicate the number of atoms when writing the chemical formula. A binary ionic compound is a compound composed of a monatomic metal cation and a monatomic nonmetal anion. 3. Prefixes are used to denote the number of atoms. Prefixes are not used in Therefore, strong bases are named following the rules for naming ionic compounds. To distinguish the difference, Fe2+ would be named iron (II) and Fe3+ would be named iron (III). those for naming ionic compounds. You add prefixes ONLY to covalent. The metal is changed to end in ous or ic. 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:[\ The ClO- ion, for example, is the hypochlorite ion. The -ide ending is added to the name of a monoatomic ion of an 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. Names and formulas of ionic compounds. Ionic compounds are named by stating the cation first, followed by the anion. You add. Aluminum Trioxide, it is an ionic compound. Ionic compounds are named differently. Aluminum oxide is an ionic compound. 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. when naming ionic compounds those are only used in naming covalent molecular compounds. What is the correct formula for Calcium Carbonate? For example, NaOH is sodium hydroxide, KOH is potassium hydroxide, and Ca(OH) 2 is calcium hydroxide. 1. Cl is chlorine. The metal cation is named first, followed by the nonmetal anion as illustrated in Figure \(\PageIndex{1}\) for the compound BaCl2. Some examples of molecular compounds are water (H2O) and carbon dioxide (CO2). 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. For example, iron can form two common ions, Fe2+ and Fe3+. How do you write diphosphorus trioxide? Ionic compounds will follow set of rules, and molecular compounds will follow another. Choose the correct answer: According to naming rules, the types of compound that use prefixes in their names are A) ionic compounds. However, some of the transition metals' charges have specific Latin names. The prefix mono- is not used for the first element. The Roman numeral denotes the charge and the oxidation state of the transition metal ion. When naming binary ionic compounds, name the cation first (specifying the charge, if necessary), then the nonmetal anion (element stem + -ide). 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). This section begins the formal study of nomenclature, the systematic naming of chemical compounds. There are two ways to make this distinction. Write the proper name for each ionic compound. compounds. Subscripts in the formula do not affect the name. In general, the prefix mono- is rarely used. The following table lists the most common prefixes for binary covalent compounds. The naming system is used by determining the number of each atom in the compound. The first step is to count the number of each element. How to Market Your Business with Webinars? . The NO 3- ion, for example, is the nitrate ion. compounds. BINARY MOLECULAR COMPOUNDS Prefixes used to note how many atoms in a compound 1. mono- 6. hexa-2. Chlorine becomes chloride. Greek prefixes are used for binary (two element) molecular compounds. Prefixes can be shortened when the ending vowel of the prefix "conflicts" with a starting vowel in the 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 prefix hypo - is used to indicate the very lowest oxidation state. If there is not a prefix before the first element, it is assumed that there is only one atom of that element. CO = carbon monoxide BCl3 = borontrichloride, CO2 = carbon dioxide N2O5 =dinitrogen pentoxide. You'll get a detailed solution from a subject matter expert that helps you learn core concepts. Accessibility StatementFor more information contact us atinfo@libretexts.orgor check out our status page at https://status.libretexts.org. 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. The hypo- and per- prefixes indicate less oxygen and more oxygen, respectively. 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. Why are prefixes not needed in naming ionic compounds? Worked example: Finding the formula of an ionic compound. Table \(\PageIndex{1}\) lists the elements that use the common system, along with their respective cation names. Yes, the name for water using the rules for chemical nomenclature is dihydrogen monoxide. Do NOT use prefixes to indicate how many of each element is present; this information is implied in the name of the compound. 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 . 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-. An ionic compound is named by its cation followed by its anion. This means that the one iron ion must have a 2+ charge. It is also sometimes called the sodium salt of hypochlorous acid. 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. To make life easier, you dont need to include the prefix mono for the first element of the two. Why aren't prefixes used in naming ionic compounds? When naming a binary molecular compound, the subscript for each element determines what prefix should be used. 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,. , The equation below represents a chemical reaction that occurs in living cells. A lot of energy is needed to. For example, NO2 would be called nitrogen dioxide, not mononitrogen dioxide. We know that cobalt can have more than one possible charge; we just need to determine what it is. , What errors can you come across when reading a thermometer, How many Hydrogen atoms in the formula 4H3O2. You add prefixes ONLY to covalent. To get 6+, three iron(II) ions are needed, and to get 6, two phosphate ions are needed . without charges, this is not possible in molecular compounds so prefixes are used. Name metals that can have different oxidation states using roman numerals to indicate positive charge. The following are the Greek prefixes used for naming binary molecular compounds. 2. Zk2`ae|W/%EZ%{6|E6:P&*OH%3tmN'/$)dH dN bg|'q .WW?BN&!>FA`Z'P66`/hF]y$LA6$DFVHVN"(VSy[mFr TnEI4Qmo%*CJ2 z )(H; ~DRX\z] & o`7f]--!- lOBNh! The second component of an ionic compound is the non-metal anion. 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 second system, called the common system, is not conventional but is still prevalent and used in the health sciences. 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. A covalent compound is usually composed of two or more nonmetal elements. Covalent bonds are molecules made up of non-metals that are linked together by shared electrons. 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. Because these elements have only one oxidation state, you don't need to specify anything with a prefix. 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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.