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90% of a worksheet must be completed to earn credit for that worksheet! Lewis Dot Structures: Diagrams that show electrons, bonding, and lone pairs of electrons. 4 0 obj Lewis Dot Diagrams Chemical Analysis Formulations Instrumental Analysis Pure Substances Sodium Hydroxide Test Test for Anions Test for Metal Ions Testing for Gases Testing for Ions Chemical Reactions Acid-Base Reactions Acid-Base Titration Bond Energy Calculations Decomposition Reaction Electrolysis of Aqueous Solutions configuration of 8 valence electrons. (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. S is a solid Lewis Dot Structures. 1. > To draw the Lewis structure for an odd-electron molecule like NO, we follow the same five steps we would for other molecules, but with a few minor changes: We will also encounter a few molecules that contain central atoms that do not have a filled valence shell. Students will learn how to display valence shells with Lewis Dot diagrams. But in reality, there are many exceptions when it comes to the structure in reality. more electrons. and neutrons. 4. Lewis Structures Notes 7. Lewis dot structures also called electron dot structures are diagrams that describe the chemical bonding between atoms in a molecule. We recommend using a diagram, total number of valence electrons, and Lewis dot structure. Multiple Dot Diagrams Possible-Resonance Structures Scientists can identify an element by its atomic number on the chart. Students can complete Bohr-Rutherford Diagrams for atoms and ions in this very organized table. 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. Ionic (EN is more than 2), Molecular Formula to Molecular Polarity The electrons found in the outer most energy level are collectively They also display the total number of lone pairs present in each of the atoms that constitute the molecule. including the ion charge . 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. achieves a stable octet. The tendency to form species that have eight electrons in the valence shell is called the octet rule. These worksheets have students explore the nature of atoms and their structure. The other halogen molecules (F2, Br2, I2, and At2) form bonds like those in the chlorine molecule: one single bond between atoms and three lone pairs of electrons per atom. Hypervalent molecules have a central atom that has more electrons than needed for a noble gas configuration. This portion of the quiz is all situational types of word problems. Carbon: 4 bonds, Nitrogen: 3 bonds and the molecular geometry (M.G. With all this usage came significant study, particularly with the emergence of organic chemistry. Since the spectator ions are not part of the product, we can choose not to show 4 precipitations These four electrons can be gained by forming four covalent bonds, as illustrated here for carbon in CCl4 (carbon tetrachloride) and silicon in SiH4 (silane). Page 2 of 10 WKS 6.2 - LDS for Ions/ Typical Charges Determine the common oxidation number (charge) for each of the following ions, and then draw their Lewis Dot Structure. Molecules formed from these elements are sometimes called hypervalent molecules. Lewis diagrams, or Lewis structures, are a way of drawing molecular structures and showing the present valence electrons and bonds. Ar Cl-S H-F-Mg 2+ Li + C P Al 3+ 2. Because hydrogen only needs two electrons to fill its valence shell, it is an exception to the octet rule. atoms The number of dots equals the number of valence electrons in the atom. By the end of this section, you will be able to: Thus far in this chapter, we have discussed the various types of bonds that form between atoms and/or ions. ii. Lets learn some interesting facts about these common atoms and how they impact the world around us. Connect the atoms A Lewis symbol consists of an elemental symbol surrounded by one dot for each of its valence electrons: Figure 7.9 shows the Lewis symbols for the elements of the third period of the periodic table. On the periodic table Carbon: 12 g/mole Same as the last worksheet, but you will see some different missing parts. It is possible to draw a structure with a double bond between a boron atom and a fluorine atom in BF3, satisfying the octet rule, but experimental evidence indicates the bond lengths are closer to that expected for BF single bonds. The four most common atoms are nitrogen, oxygen, carbon, and hydrogen. We use Lewis symbols to describe valence electron configurations of atoms and monatomic ions. The rows from left to right are termed periods, while the rows from top to bottom are called groups. We use Lewis symbols to describe valence electron configurations of atoms and monatomic ions. 2) Balancing chemical reactions and missing parts. Predict the products of the following nuclear reactions. An entire class of compounds, including spheres and tubes of various shapes, were discovered based on C60. Write the Lewis dot structure for the following atoms or ions: a. Mg b. Al3+ c. C d. N3- 2. 45 neutrons and 36 electrons? It readily combines with a molecule containing an atom with a lone pair of electrons. For questions 1 and 2 predict the missing reactant or product and identify the form of radiation demonstrated in each Science Chemistry Draw a Lewis dot structure for the fictitious molecular ion [203]2. Recall that a Lewis dot symbol refers to an elemental symbol with dots used to represent the valence electrons. We dipped into, CHMY 121 - These are introduction notes. If all the criteria are met, then the molecule exists Browse lewis dot structure worksheet resources on Teachers Pay Teachers, a marketplace trusted by millions of teachers for original educational resources. Here's how: If it's an anion, add the negative charge to the number of valence electrons. Identify the element that corresponds to each of the following electron Write the chosen letter on a separate sheet of paper. 2 val e), expanded octet possible for n>3 (P and larger) The ion has 17 protons in the nucleus, with a Count total # of valence electrons 2. . 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$Bg^HOD}?. The Lewis dot structure consists of six silicon and six oxygen atoms in a ring each with single bonds. problem. This means that it will gain electrons until it Atoms were initially thought to be the smallest particle of matter, but they are actually composed of three smaller particles. Lewis structure of atoms worksheet answer key for very simple molecules and molecular ions, we can write the lewis structures by merely pairing up the unpaired electrons on the. Step 2 tells how many electrons are needed and Step 1 is how many electrons you have. properties of that compound? Never Change Subscripts Since valence electrons are typically represented as dots, these structural formulas sometimes are called Lewis dot stutctures. Practicing Ionic Bonding modifiedfromoriginal 5. Gain/Lose ___ e- Draw ion Name of ion Na 1 Cation Loses 1 Na+1 Sodium ion S 7 Anion Gains 2 S-2 Sulfide Cl In this section, we will explore the typical method for depicting valence shell electrons and chemical bonds, namely Lewis symbols and Lewis structures. Is the reaction product (sodium chloride) more or less stable than the reactants (sodium Molecular shape: Science. Place all remaining electrons on the central atom. Lewis dot structures Polyatomic ion Charges Hydrogen bonds Valence electrons Skills Practiced You will practice the following skills: Reading comprehension - ensure that you draw the most. 5. are not subject to the Creative Commons license and may not be reproduced without the prior and express written Most atoms tend to lose or gain electrons in. When one atom connects with another atom, they make up a chemical element. |LSp\:G7c|f (s9;6~X/#uhygM3nd[ekPsxx,%#g`U?t0=~j57DsSob(O{K443~2|Ho"$Q/jBb6#5@L7Lw_,\y/"f#zC<1fF/ xH~23H9OM!~pl!^D9w`Do )`6Sl4X>a}!`I:}O-ezaBmDFr$lm| }u V00lB,z!6:cdM(#N m9K&H=v0@D8!YX39az6ukQP)CQWx". We also use Lewis symbols to indicate the formation of covalent bonds, which are shown in Lewis structures, drawings that describe the bonding in molecules and polyatomic ions. Student will also write elements in standard atomic notation, write the Lewis Dot Diagrams for atoms and ions, identify how many electrons need to be gained or lost to to for an ion, determine whether a cation or anion has formed and write the atom in ion notation. Odd-electron molecules have an odd number of valence electrons, and therefore have an unpaired electron. The total number of electrons does not change. Students will learn how to predict the element formed based on the number of protons an atom has. Draw the dot diagram for an atom of bromine. Kroto sought to use a machine developed by Richard Smalley's team at Rice University to learn more about these structures. !We!can!always!distribute!the!electrons! Outer atoms first, then central atoms Our mission is to improve educational access and learning for everyone. In 2D the atoms in methane (CH4) can only get 90 degrees separation Chemistry. How much does one mole weigh? Can usually identify acids by looking to see if H is listed first in the formula The protons carry a positive charge, while the electrons have a negative charge. Since bonding involves the valance shell electrons only, it is only necessary to illustrate those outer electrons. atoms that can exceed the octet bonded to an atom with lone pairs. They tell us if one atom is donating extra electrons to another to give it an octet. OpenStax is part of Rice University, which is a 501(c)(3) nonprofit. These dots are arranged to the right and left and above and below the symbol . . Ionic compounds are often called salts A dashed line means the atom sits behind the central atom [ Indicate whether the following species have a stable noble gas configuration. Lewis dot structure practice problems with answers and explanation youtube. The reactivity of the compound is also consistent with an electron deficient boron. Can usually identify bases by looking to see formula content OH As a result, there are two lone pairs in this molecule and two. Chemistry questions and answers. Draw the Electron dot structure. What will the resulting atom or ion symbol look like? In Section 4.7, we demonstrated that ions are formed by losing electrons to make cations, or by gaining electrons to form anions. charges on calcium ions and oxide ions to be when they form compounds. b. Linear (2 bonding groups, 0 lone pairs) Determine the total number of valence (outer shell) electrons. }O}}\mathbf{\: :} \nonumber \]. The transfer process looks as follows: The oppositely charged ions attract each other to make CaCl2. Exceptions to the octet rule: be (2 bonds 4 val e), B (3 bonds 6 val e), H (1 bond Home 1. If you are redistributing all or part of this book in a print format, Calculate formal charges and use the Electroneutrality Principle to determine which Lewis dot structure is the best, or which resonance structure makes the largest contribution to the resonance hybrid. Worksheet chemical bonding ionic and 3. electronegativity. Lewis Dot Diagrams are used to indicate the number of valence electrons and provide us with a quick form of short hand. C. Lewis dot structure for an atom of sodium is. How to draw simple Lewis structures (i.e. Acids produce H+ ions in solution where we have written the final formula (the formula for sodium chloride) as per the convention for ionic compounds, without listing the charges explicitly. They are the building blocks of all chemical structures. What reactants were needed to create these products. Note, in the Lewis structure there is a pair . Ionic Bonds are made of Ions. Depends on the substance For the Na atom to obtain an octet, it must lose an electron; for the Cl atom to gain an octet, it must gain an electron. Langmuir's Rule is sometimes useful in spotting resonance, too. In a Lewis structure of the compound, the carbon has a formal negative charge. - What is the formal charge on the central chlorine atom in the molecular ion [CIO4] ? Ions: Atoms that gain or lose electrons, forming a charge. Lewis Dot Structures to show the valance electrons of an element as dots. HCl+NaOHH2O+NaCl The neutrons have no charge. If the atoms are too far apart, the potential energy is zero, and a bond cannot form. PK ! w 1 [Content_Types].xml ( Ik0kPJCch*84}YL)Ibg{0dsI{W^e8v}~tYP8%wP$6\_?VRFj NO 3 - d. CO 3 2- 4. Considering that all living and non-living matter are made up of atoms, this is a significant concept to understand for scientific study. Bohr models (or Bohr diagram) are diagrams that show the number of protons and All of the substances described uses common names that most people will recognize. electronegativity and ionization energy. Step 3: Use two valence electrons to form each bond in the skeleton structure. citation tool such as, Authors: Paul Flowers, Klaus Theopold, Richard Langley, William R. Robinson, PhD. You will give 3 pieces of data and are asked to complete this here chart for us. Lewis structures are really helpful when it comes to learning about the oxidation states, valence, and the type of bonding. Draw a skeleton structure of the molecule or ion, arranging the atoms around a central atom. Draw the dot diagram for an atom of carbon. These worksheets have students explore the nature of atoms and their structure. The first unit was primarily based on solutions, Managing Engaging Learning Environments (D095), Perspectives in the Natural Sciences (SCI100), Statistical literacy in Psychology (Psy 260), Medical/Surgical Nursing Concepts (NUR242), Managing Organizations and Leading People (C200 Task 1), Differential Diagnosis & Primary Care Practicum (NR-511), Nursing B43 Nursing Care of the Medical Surgical (NURS B43), Professional Application in Service Learning I (LDR-461), Advanced Anatomy & Physiology for Health Professions (NUR 4904), Principles Of Environmental Science (ENV 100), Operating Systems 2 (proctored course) (CS 3307), Comparative Programming Languages (CS 4402), Business Core Capstone: An Integrated Application (D083), Bates Test questions The Thorax and Lungs, Chapter 15 Anxiety and Obsessive-Compulsive Disorders, Lesson 17 Types of Lava and the Features They Form, 1-2 Short Answer Cultural Objects and Their Culture, PDF Mark K Nclex Study Guide: Outline format for 2021 NCLEX exam. the formation of one formula unit of magnesium fluoride. Atom or Ion Electron Configuration # of valence electrons # of electrons gained or lost Quantum Numbers for last electron Lewis Dot Structure Li n= l= ml= . valence electrons. total valence electrons = _____ Use two of these electrons to make a bond between the 2 oxygen atoms. Draw the Lewis dot structures of the following atoms ions Eiji Osawa predicted a spherical form based on observations of a similar structure, but his work was not widely known outside Japan. POGIL - 2005 5/ }Cl}}\mathbf{\: :}^{-} \nonumber \], \[\left [ Ne \right ]\; \; \; \; \; \left [ Ne \right ]3s^{2}3p^{6} \nonumber \]. Indium 114 g/mole Lewis structures (also known as Lewis dot structures or electron dot structures) are diagrams that represent the valence electrons of atoms within a molecule. Solubility and precipitation Authored by: Lizabeth M. Tumminello -Edited by: Erin Graham, Kelly Levy, Ken Levy and Rohini Quackenbush, The chemical properties of an element are based on the number of electrons in the, order to identify stable electron configurations. A solid line means that the atom is aligned with the central atom (in the same plane) Duration 45 minutes/1 class period Prerequisite Skills might be arranged in space to form the solid salt magnesium fluoride. We will advance on to looking further into the nucleus and explore nuclear chemistry of atoms that are not very stable. Write the complete electron configuration for each of the following elements. *ck=^]CU5 hLkAWPWJm 'zf*\H:{+e mM+&br &v:M%&;d]CgnpoLRM`fEO 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. Bent (2 bonding groups, 2 lone pairs on central atom) Each Cl atom interacts with eight valence electrons: the six in the lone pairs and the two in the single bond. Authored by: Lizabeth M. Tumminello -Edited by: Erin Graham, Kelly Levy, Ken Levy and Rohini Quackenbush, Copyright 2023 StudeerSnel B.V., Keizersgracht 424, 1016 GC Amsterdam, KVK: 56829787, BTW: NL852321363B01, Authored by: Lizabeth M. Tumminello -Edited by: Erin, . 1 mole = 6 x 10^23 (avogadros number) and you must attribute OpenStax. An atom is one of the most significant things in the world as it is the smallest unit of matter. The Lewis structure for the hydride ion is [H:] - For the main group atoms, an atom with many valence electrons (more than 4) will gain enough electrons to form a negative ion that has 8 valence electrons. Hydrogen: 1 bond We also acknowledge previous National Science Foundation support under grant numbers 1246120, 1525057, and 1413739. Di dlMts"6!cKDyKDHC_ The word "atom" is derived from a Greek word for "uncuttable". Provide the number of atoms in each molecule of the substances represented by the Authored by: Lizabeth M. Tumminello -Edited by: Erin Graham, Kelly Levy, Ken Levy and Rohini Quackenbush, A. Lewis dot structure for an atom of chlorine is. Atoms are thought to be the smallest particle of a single element. A similar process occurs between Mg atoms and O atoms, except in this case two electrons are transferred: The two ions each have octets as their valence shell, and the two oppositely charged particles attract, making an ionic bond: \[\mathbf{Mg\,}^{2+}\; + \; \left[\mathbf{:}\mathbf{\ddot{\underset{.\: . We look at the function of each of the subatomic particles and how they interact to form molecules and ions. neutrons are found in the nucleus. answer. % - Draw the Lewis Dot Diagram for each of the ions involved ! We peek into the true anatomy of these buggers. f?3-]T2j),l0/%b c. Give expanded octets to central atoms G is gas In 3D they can spread out a little further (109 degrees) 2. 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.) Resonance structures Determine which atoms are bonded together and put two electrons between them to represent the bond 3. Draw orbital diagrams for the following choices. B. Lewis dot structure for a chloride ion is. It is stated in orbital notation. 6 lewis, geometry, polarity In 1916, American chemist, Gilbert N. Lewis, introduced bond lines to electron dot structures. Note lone pair electrons and bonding electrons in HCl Steps for writing Lewis dot structures Sum the valence e-'s from all the atoms. Lewis Dot Structures Objectives: 1. You will across note the directionals. Lewis electron dot diagram. Place remaining valence electrons to . We ask you to tell us about what it composed of. 3 0 obj Carbon atoms can link together to make some of the longest, most durable chains. Law of Conservation of Matter: Matter cannot be created or destroyed Sodium has an electron configuration of 2-8-1, therefore it has one valence electron, 2D vs 3D . 2 0 obj What is the force of attraction that holds the magnesium and fluoride ions together? 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. Atoms are essential pieces of matter, with matter being anything you can physically touch. Dot one dot represents one valence electron (found on odd-electron particles). 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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.