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d8RS-Mr4a5:^,oYu~>=?CEhVw_']eCa._]:jm;|1d =wbzwW_Pas3}M?-/Bt r_'/#+uZ(6}*iX/g-`yX%mXVhh2rq5>N{4NYUq%?5k30)t0z g=azu.( 8lua;n]ZYArI@gv{vi/O=A'wgk>l79$Bg^HOD}?. Bent (2 bonding groups, 1 lone pair on central atom) The Methodology of the Social Sciences (Max Weber) Civilization and its Discontents (Sigmund Freud) Lewis dot structures of atoms and ions University The City College of New York Course General Chemistry II (CHEM 10401) Uploaded by Maryann Gomes Academic year2022/2023 Helpful? Drawing 3D Ionic compounds are often called salts Lewis Dot Structure Worksheet Here are the basic steps involved in drawing the Lewis dot structure for a molecule: a) Calculate the total number of valence electrons in the molecule (take the number of valence . Chlorine needs an additional electron to attain the stable noble gas configuration of 8 Together with Robert Curl, who had introduced them, and three graduate studentsJames Heath, Sean OBrien, and Yuan Liuthey performed an intensive series of experiments that led to a major discovery. Atoms and ions worksheet answer key. Polar covalent Find those different elements and parts. Principal Energy Levels What I Know. Indicate whether the following species have a stable noble gas configuration. Science Worksheets > Atomic Structure. An atom is one of the most significant things in the world as it is the smallest unit of matter. Draw the Lewis dot structures for each of the following molecules: a. H 2 S c. SO 3 b. CH 2 Br 2 d. HCN 3. In Section 4.7, we demonstrated that ions are formed by losing electrons to make cations, or by gaining electrons to form anions. The word "atom" is derived from a Greek word for "uncuttable". Electrons in bonds and electrons in lone pairs will repel one another: get as far away Rearrange the electrons of the outer atoms to make multiple bonds with the central atom in order to obtain octets wherever possible. 2. POGIL - 2005 5/ Lewis Dot Structures and Molecule Geometries Worksheet Answer Key 3 4. Elemental substances (oxidation state same as charge) consent of Rice University. Ionic bonds are caused by electrons transferring from one atom to another. "^Z4!$}]M1\@F mQh UETI VI}SCfU?WD]9DP`@I="wIyMuV\7@iaxFd R X#rW@:>b^LKt`OZYW:l/ PK ! Determine the electron and molecular geometry of the produced molecules. What we need is a second Na atom to donate a second electron to the O atom: These three ions attract each other to give an overall neutral-charged ionic compound, which we write as Na2O. Draw three resonance structures for carbonate ion, CO32-, and assign formal charges on all the atoms. Lewis dot diagram worksheet use the bohr models to determine the number of. Basic facts to get us started. Place a check to identify the form of radiation demonstrated by each reaction below. Lewis Dot Structures Worksheet Answers Science Printable . Formal charges are an important book-keeping device that we use in Lewis structures. If the atoms are too close together, the repulsive forces are much stronger and the potential energy is at a maximum, and a bond will not form. An atom is composed of protons, neutrons, and electrons. Legal. Don't forget to show brackets and charge on your LDS for ions! then you must include on every digital page view the following attribution: Use the information below to generate a citation. Together they provide almost all of the mass for the element. Lewis dot diagrams and ionic bonding worksheet 2. 2 balancing This suggests the best Lewis structure has three BF single bonds and an electron deficient boron. Determine total # of valence electrons Draw the Electron dot structure. You will be given chemical symbols for elements, compounds, or a mixture and asked to state the phase of matter you find this at room temperature. Covalent bonds are formed when one electron from each atom forms an electron pair. Draw Lewis structures for atoms, ions and simple molecules. Complete the lewis structures of these molecules by adding multiple bonds and lone pairs. Central atom is listed first (unless hydrogen) and is the least electronegative Lewis symbols can also be used to illustrate the formation of cations from atoms, as shown here for sodium and calcium: Likewise, they can be used to show the formation of anions from atoms, as shown here for chlorine and sulfur: Figure 7.10 demonstrates the use of Lewis symbols to show the transfer of electrons during the formation of ionic compounds. polyatomic ions a nh 4 c po 4 3 b no 3 d co 3 2 4 for the following molecules or ions . Pyramidal (3 bonding groups, 1 lone pair on central atom) This may look a bit different than others. N _rels/.rels ( JAa}7 }O}}\mathbf{\: :}\right]^{2-}\; \; \; \; \; Mg^{2+}O^{2-}\; or\; MgO \nonumber \]. h26T0Pw/+Q0L)662)Is0i T$ 0 c. Give expanded octets to central atoms Identify the element that corresponds to each of the following electron configurations. Students will learn how to predict the element formed based on the number of protons an atom has. If atom doesnt have the right # of electrons: double bonds, triple bonds, etc Lewis Dot Structures It is pretty cool because how we mix up atoms up or together can make just about anything in the universe. 2021-22, Chapter 01 - Fundamentals of Nursing 9th edition - test bank, Leadership class , week 3 executive summary, I am doing my essay on the Ted Talk titaled How One Photo Captured a Humanitie Crisis https, School-Plan - School Plan of San Juan Integrated School, SEC-502-RS-Dispositions Self-Assessment Survey T3 (1), Techniques DE Separation ET Analyse EN Biochimi 1. The Lewis dot structure consists of six silicon and six oxygen atoms in a ring each with single bonds. Since atoms are part of all living and non-living things, they are crucial to scientific study. answer. 3 0 obj Cross), Brunner and Suddarth's Textbook of Medical-Surgical Nursing (Janice L. Hinkle; Kerry H. Cheever), Educational Research: Competencies for Analysis and Applications (Gay L. R.; Mills Geoffrey E.; Airasian Peter W.), Civilization and its Discontents (Sigmund Freud), The Methodology of the Social Sciences (Max Weber), Campbell Biology (Jane B. Reece; Lisa A. Urry; Michael L. Cain; Steven A. Wasserman; Peter V. Minorsky), Principles of Environmental Science (William P. Cunningham; Mary Ann Cunningham), Psychology (David G. Myers; C. Nathan DeWall), Chemistry: The Central Science (Theodore E. Brown; H. Eugene H LeMay; Bruce E. Bursten; Catherine Murphy; Patrick Woodward), Biological Science (Freeman Scott; Quillin Kim; Allison Lizabeth), Give Me Liberty! <> Acids produce H+ ions in solution In the compound potassium bromide, determine the charge on the potassium ion and the Consider sodium: in its elemental form, it has one valence electron and is stable. For example, consider the ammonium ion, NH 4+, which contains 9 (5 from N and 1 from each of the four H atoms) -1 = 8 electrons. Oxygen and other atoms in group 16 obtain an octet by forming two covalent bonds: As previously mentioned, when a pair of atoms shares one pair of electrons, we call this a single bond. The attraction of oppositely charged ions caused by electron transfer is called an ionic bond. Let's find the valence electrons for OH-: 0xygen: 1 atom x 6 valence electrons = 6 valence electrons. Outer atoms first, then central atoms If all the criteria are met, then the molecule exists Thus we need two \(Cl\) atoms to accept the two electrons from one \(Ca\) atom. The total number of valence electrons in the ion is: n valence electrons = [ ( 4 6) + ( 6 18) + 12] e = ( 24 + 108 + 12) e = 144 e . This means that sodium loses an electron to achieve the stable noble gas All of the substances described uses common names that most people will recognize. Nitrogen is the fourth most common atom, making up about seventy-five percent of the Earths atmosphere. Trigonal planar (3 bonding groups, 0 lone pairs on central atom) Aq is aqueous 3. The atom is the unit of matter that forms all elements in the universe. Background: Scientists often create models to represent either a physical or . wZ5Aae The strength of ionic bonding depends on the magnitude of the charges and the sizes of the ions. We break down the anatomy of these structures to display this for students and we will explore the Bohr model of this structure. Can usually identify bases by looking to see formula content OH You will also diagram the electron configuration in an orbital diagram. Tetrahedral (4 bonding groups, 0 lone pairs on central atom) PK ! Notes: Remember that Metals tend to lose their electrons, falling back to their . Every atom (except the hydronium ion) has two main components, a NUCLEUS with (or electron dot diagram or a Lewis diagram or a Lewis structure) is a representation of the valence electrons of an atom that uses dots around the symbol of the element. This will test two skills: 1) Your ability to indicate if the item presented is an element, compound, or mixture. 5. Solve any question of Chemical Bonding and Molecular Structure with:-. Chemistry questions and answers. Charge it all up. Write the electron configuration, orbital Connect atoms using single bonds Atoms, the tiniest unit of matter, make up all things. Is the reaction product (sodium chloride) more or less stable than the reactants (sodium Soot has been used as a pigment (often called carbon black) for thousands of years. Atoms were initially thought to be the smallest particle of matter, but they are actually composed of three smaller particles. Cross), Principles of Environmental Science (William P. Cunningham; Mary Ann Cunningham), Forecasting, Time Series, and Regression (Richard T. O'Connell; Anne B. Koehler), Campbell Biology (Jane B. Reece; Lisa A. Urry; Michael L. Cain; Steven A. Wasserman; Peter V. Minorsky), Civilization and its Discontents (Sigmund Freud), Give Me Liberty! In 1916, American chemist, Gilbert N. Lewis, introduced bond lines to electron dot structures. C. Lewis dot structure for an atom of sodium is. F3 L word/_rels/document.xml.rels ( N0EHC=qR. The parts of the atom are the proton, neutron, and electron. Use Lewis structures as a guide to construct three-dimensional models of small molecules. We dipped into, CHMY 121 - These are introduction notes. 6 redox Lewis Dot Structures to show the valance electrons of an element as dots. one!particular!side!of!the!chemical!symbol.! However, a pair of atoms may need to share more than one pair of electrons in order to achieve the requisite octet. Duration 45 minutes/1 class period Prerequisite Skills POGIL - 2005 2/ A step-by-step explanation of how to draw the O2- Lewis Dot Structure.For the O 2- structure use the periodic table to find the total number of valence elect. This allows each halogen atom to have a noble gas electron configuration. In 3D they can spread out a little further (109 degrees) Atoms in general, try and seek to half-fill or fully-fill their valence electron shell. In Section 4.7, we demonstrated that ions are formed by losing electrons to make cations, or by gaining electrons to form anions. 372 0 obj <>stream We look at the function of each of the subatomic particles and how they interact to form molecules and ions. Place all remaining electrons on the central atom. Most atoms tend to lose or gain electrons in. O: O 3. seven valence electrons and needs to have seven dots drawn around its symbol. Chapter 5 Electrons In Atoms Answers To. Resonance structures For example, when two chlorine atoms form a chlorine molecule, they share one pair of electrons: The Lewis structure indicates that each Cl atom has three pairs of electrons that are not used in bonding (called lone pairs) and one shared pair of electrons (written between the atoms). Connect the atoms It is a colorless, weightless gas. It turns out that the Na+ ion has a complete octet in its new valence shell, the n = 2 shell, which satisfies the octet rule. 1999-2023, Rice University. Ar Cl-S H-F-Mg 2+ Li + C P Al 3+ 2. The significance of atoms is that without them, nothing could exist. What is missing in here? The need for the number of electrons lost being equal to the number of electrons gained explains why ionic compounds have the ratio of cations to anions that they do. There are one hundred and eighteen elements on the table and scientists will add two more soon. Now consider an Na atom in the presence of a Cl atom. The two atoms have these Lewis electron dot diagrams and electron configurations: \[\mathbf{Na\, \cdot }\; \; \; \; \; \; \; \; \; \; \mathbf{\cdot }\mathbf{\ddot{\underset{.\: . are not subject to the Creative Commons license and may not be reproduced without the prior and express written Amount of H+ and OH- produced determines the strength of an acid/base Each Si-atom has two other oxygen atoms linked to it as side . are licensed under a, Measurement Uncertainty, Accuracy, and Precision, Mathematical Treatment of Measurement Results, Determining Empirical and Molecular Formulas, Electronic Structure and Periodic Properties of Elements, Electronic Structure of Atoms (Electron Configurations), Periodic Variations in Element Properties, Relating Pressure, Volume, Amount, and Temperature: The Ideal Gas Law, Stoichiometry of Gaseous Substances, Mixtures, and Reactions, Shifting Equilibria: Le Chteliers Principle, The Second and Third Laws of Thermodynamics, Representative Metals, Metalloids, and Nonmetals, Occurrence and Preparation of the Representative Metals, Structure and General Properties of the Metalloids, Structure and General Properties of the Nonmetals, Occurrence, Preparation, and Compounds of Hydrogen, Occurrence, Preparation, and Properties of Carbonates, Occurrence, Preparation, and Properties of Nitrogen, Occurrence, Preparation, and Properties of Phosphorus, Occurrence, Preparation, and Compounds of Oxygen, Occurrence, Preparation, and Properties of Sulfur, Occurrence, Preparation, and Properties of Halogens, Occurrence, Preparation, and Properties of the Noble Gases, Transition Metals and Coordination Chemistry, Occurrence, Preparation, and Properties of Transition Metals and Their Compounds, Coordination Chemistry of Transition Metals, Spectroscopic and Magnetic Properties of Coordination Compounds, Aldehydes, Ketones, Carboxylic Acids, and Esters, Composition of Commercial Acids and Bases, Standard Thermodynamic Properties for Selected Substances, Standard Electrode (Half-Cell) Potentials, Half-Lives for Several Radioactive Isotopes. Accessibility StatementFor more information contact us atinfo@libretexts.orgor check out our status page at https://status.libretexts.org. Source: www.chegg.com. Element Lewis Dot # of Valance e- Cation or anion? Lewis theory (Gilbert Newton Lewis, 1875-1946) focuses on the valence electrons, since the outermost electrons are the ones that are highest in energy and farthest from the nucleus, and are therefore the ones that are most exposed to other atoms when bonds form. hdA@`naIt(:ti-)DE]w@xEC6ab\( $_7GrX>C*Z,d0y}F/r0%[=~;2RL7TQ[W3c@k7*eE` H Displaying all worksheets related to - Lewis Structure Of Ions. Trade pairs of electrons for bond between atoms The astute reader may have noticed something: many of the ions that form have eight electrons in their valence shell. The Periodic Table Part 2 Answer Key. We saw this in the formation of NaCl. Science. Before!anyone!gets!wrong!ideas;!the!electrons!aren't!permanently!fixed!to! Worksheet 6 - Lewis structures Determine the Lewis structure of O2 oxygen gas. fluorine can transfer electrons to form ions of each element with stable octets. 8. charge of an ion that contains 35 protons, total valence electrons = _____ Use two of these electrons to make a bond between the 2 oxygen atoms. hydrogen: 1 atom x 1 valence electron = 1 valence electron. and needs one dot. They have a negative charge and provide very little mass to the overall element. neutrons are found in the nucleus. Worksheet - Lewis Dot Arkansas State University Department of Chemistry and Physics Worksheets Lewis Dot Structures For each of the following, draw the Lewis Dot Structure, give the electron arrangement (E.A.) You may need to balance a reaction or two. Dash each dash represents two electrons that are shared between two atoms as a covalent bond. In Lewis dot structure all atoms have their octet complete. }Cl}}\mathbf{\: :}^{-}\rightarrow Na^{+}Cl^{-}\; \; or\; \; NaCl \nonumber \]. Nitric oxide, NO, is an example of an odd-electron molecule; it is produced in internal combustion engines when oxygen and nitrogen react at high temperatures. Chlorines electron configuration is 2-8-7; therefore it has Solubility and precipitation 2. Lewis structure of atoms worksheet answer key 1. What is the force of attraction that holds the magnesium and fluoride ions together? }O}}\mathbf{\: :} \nonumber \]. 1. The Lewis Structure also denotes the number of lone pairs of electrons present around the central atom. Scientists can identify an element by its atomic number on the chart. and you must attribute OpenStax. A Lewis Dot Structure is drawn by a series of dots, lines, and atomic symbols and provides a structure for the way that the atom or molecule is arranged. Intact-compound Equation Worksheet chemical bonding ionic and 3. *ck=^]CU5 hLkAWPWJm 'zf*\H:{+e mM+&br &v:M%&;d]CgnpoLRM`fEO Strong= 100% Dissociative For the species in the problem above that do not have a noble gas configuration, identify how they can obtain a noble gas configuration of 8 electrons. Bent (2 bonding groups, 2 lone pairs on central atom) Valence Shell: The outer electron shell of any atom. Note lone pair electrons and bonding electrons in HCl Steps for writing Lewis dot structures Sum the valence e-'s from all the atoms. The number of protons is the atomic number and the mass number is the sum of the protons The ion has 17 protons in the nucleus, with a M SoU]SSpX[@xN4~|OhX#>nzwx:c5HH?:oq"&pf|\t2P? { "10.01:_Bonding_Models_and_AIDS_Drugs" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "10.02:_Representing_Valence_Electrons_with_Dots" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "10.03:_Lewis_Structures_of_Ionic_Compounds-_Electrons_Transferred" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "10.04:_Covalent_Lewis_Structures-_Electrons_Shared" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "10.05:_Writing_Lewis_Structures_for_Covalent_Compounds" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", 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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%2F10%253A_Chemical_Bonding%2F10.03%253A_Lewis_Structures_of_Ionic_Compounds-_Electrons_Transferred, \( \newcommand{\vecs}[1]{\overset { \scriptstyle \rightharpoonup} {\mathbf{#1}}}\) \( \newcommand{\vecd}[1]{\overset{-\!-\!\rightharpoonup}{\vphantom{a}\smash{#1}}} \)\(\newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\) \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\) \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\) \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\) \( \newcommand{\Span}{\mathrm{span}}\) \(\newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\) \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\) \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\) \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\) \( \newcommand{\Span}{\mathrm{span}}\)\(\newcommand{\AA}{\unicode[.8,0]{x212B}}\), Example \(\PageIndex{1}\): Synthesis of Calcium Chloride from Elements, 10.2: Representing Valence Electrons with Dots, 10.4: Covalent Lewis Structures- Electrons Shared, 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, 10.3: 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.