3: Ionic Bonding and Simple Ionic Compounds
- Page ID
- 15922
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\(\newcommand{\avec}{\mathbf a}\) \(\newcommand{\bvec}{\mathbf b}\) \(\newcommand{\cvec}{\mathbf c}\) \(\newcommand{\dvec}{\mathbf d}\) \(\newcommand{\dtil}{\widetilde{\mathbf d}}\) \(\newcommand{\evec}{\mathbf e}\) \(\newcommand{\fvec}{\mathbf f}\) \(\newcommand{\nvec}{\mathbf n}\) \(\newcommand{\pvec}{\mathbf p}\) \(\newcommand{\qvec}{\mathbf q}\) \(\newcommand{\svec}{\mathbf s}\) \(\newcommand{\tvec}{\mathbf t}\) \(\newcommand{\uvec}{\mathbf u}\) \(\newcommand{\vvec}{\mathbf v}\) \(\newcommand{\wvec}{\mathbf w}\) \(\newcommand{\xvec}{\mathbf x}\) \(\newcommand{\yvec}{\mathbf y}\) \(\newcommand{\zvec}{\mathbf z}\) \(\newcommand{\rvec}{\mathbf r}\) \(\newcommand{\mvec}{\mathbf m}\) \(\newcommand{\zerovec}{\mathbf 0}\) \(\newcommand{\onevec}{\mathbf 1}\) \(\newcommand{\real}{\mathbb R}\) \(\newcommand{\twovec}[2]{\left[\begin{array}{r}#1 \\ #2 \end{array}\right]}\) \(\newcommand{\ctwovec}[2]{\left[\begin{array}{c}#1 \\ #2 \end{array}\right]}\) \(\newcommand{\threevec}[3]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \end{array}\right]}\) \(\newcommand{\cthreevec}[3]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \end{array}\right]}\) \(\newcommand{\fourvec}[4]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \\ #4 \end{array}\right]}\) \(\newcommand{\cfourvec}[4]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \\ #4 \end{array}\right]}\) \(\newcommand{\fivevec}[5]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \\ #4 \\ #5 \\ \end{array}\right]}\) \(\newcommand{\cfivevec}[5]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \\ #4 \\ #5 \\ \end{array}\right]}\) \(\newcommand{\mattwo}[4]{\left[\begin{array}{rr}#1 \amp #2 \\ #3 \amp #4 \\ \end{array}\right]}\) \(\newcommand{\laspan}[1]{\text{Span}\{#1\}}\) \(\newcommand{\bcal}{\cal B}\) \(\newcommand{\ccal}{\cal C}\) \(\newcommand{\scal}{\cal S}\) \(\newcommand{\wcal}{\cal W}\) \(\newcommand{\ecal}{\cal E}\) \(\newcommand{\coords}[2]{\left\{#1\right\}_{#2}}\) \(\newcommand{\gray}[1]{\color{gray}{#1}}\) \(\newcommand{\lgray}[1]{\color{lightgray}{#1}}\) \(\newcommand{\rank}{\operatorname{rank}}\) \(\newcommand{\row}{\text{Row}}\) \(\newcommand{\col}{\text{Col}}\) \(\renewcommand{\row}{\text{Row}}\) \(\newcommand{\nul}{\text{Nul}}\) \(\newcommand{\var}{\text{Var}}\) \(\newcommand{\corr}{\text{corr}}\) \(\newcommand{\len}[1]{\left|#1\right|}\) \(\newcommand{\bbar}{\overline{\bvec}}\) \(\newcommand{\bhat}{\widehat{\bvec}}\) \(\newcommand{\bperp}{\bvec^\perp}\) \(\newcommand{\xhat}{\widehat{\xvec}}\) \(\newcommand{\vhat}{\widehat{\vvec}}\) \(\newcommand{\uhat}{\widehat{\uvec}}\) \(\newcommand{\what}{\widehat{\wvec}}\) \(\newcommand{\Sighat}{\widehat{\Sigma}}\) \(\newcommand{\lt}{<}\) \(\newcommand{\gt}{>}\) \(\newcommand{\amp}{&}\) \(\definecolor{fillinmathshade}{gray}{0.9}\)There are only 118 known chemical elements but tens of millions of known chemical compounds. Compounds can be very complex combinations of atoms, but many important compounds are fairly simple. Table salt, as we have seen, consists of only two elements: sodium and chlorine. Nevertheless, the compound has properties completely different from either elemental sodium (a chemically reactive metal) or elemental chlorine (a poisonous, green gas). We will see additional examples of such differences in this chapter as we consider how atoms combine to form compounds.
- 3.0: Prelude to Ionic Bonding and Simple Ionic Compounds
- This page discusses the importance of table salt (sodium chloride) for health, its historical value as a payment medium (salary for Roman soldiers), and the health implications of salt consumption. While necessary for bodily functions, the average salt intake in the U.S. is high, potentially leading to health risks. Doctors often recommend low-salt diets for hypertension, urging the use of potassium substitutes despite taste preferences.
- 3.1: Two Types of Bonding
- This page discusses how atoms bond to achieve stability, primarily through the octet rule for most elements and the duet rule for smaller atoms like hydrogen and helium. It explains that ionic bonds form when electrons are transferred, creating attractive oppositely charged ions. The summary highlights the tendency of elements to lose or gain electrons to reach electroneutrality and stability via ionic or covalent bonds.
- 3.2: Ions
- This page discusses the formation of cations and anions through electron loss or gain for achieving an octet, using sodium and chlorine to exemplify the creation of sodium chloride. It explains ionic compounds formation via Lewis diagrams, detailing charge balance in compounds like LiBr and MgO. The text also addresses predicting ion charges from the periodic table and includes exercises to reinforce understanding of charge acquisition and electron configurations through Lewis diagrams.
- 3.3: Formulas for Ionic Compounds
- This page covers the fundamentals of writing chemical formulas for ionic compounds, highlighting the structure of ions, charge balance, and conventions for formula construction. It explains the classification and naming of polyatomic ions, detailing suffixes that indicate oxygen levels and rules for naming ionic compounds. The text emphasizes the role of hydrogen carbonate ions in blood regulation compared to other ions found in seawater.
- 3.4: Ionic Nomenclature
- This page outlines the rules for naming ionic compounds, detailing how to name monatomic cations and anions, and polyatomic ions. It discusses the Stock system for variable charge cations and the order of naming (cation before anion). The text provides examples and exercises for practice, helping to clarify the application of these naming conventions in chemical nomenclature.
- 3.5: Formula Mass
- This page explains how to calculate the formula mass of ionic compounds by summing the atomic masses of their atoms, including examples like sodium chloride and calcium fluoride. It also discusses hydrates and their notation. Additionally, it includes a list of ion pairs and chemical compounds for practice, providing calculated formula masses in atomic mass units (amu) to reinforce the concept of determining the sum of atomic masses for both ionic and molecular compounds.
- 3.6: Characteristics of Ionic Compounds
- This page discusses ionic compounds, highlighting their properties such as high melting points, hardness, and brittleness due to strong ionic bonds in a crystal lattice. It notes that they form colorful crystals, are non-conductive in solid form but conduct electricity when melted or dissolved in water, and can shatter under force. Examples provided include sodium chloride and ammonium nitrate, emphasizing their ability to dissociate into ions in solution.
- 3.E: Ionic Bonding and Simple Ionic Compounds (Exercises)
- This page contains exercises and answers on electron configurations and valence shells of atoms and ions, including sodium and bromine. It examines differences between neutral atoms and their ions, ionic compound formation, and calculates formula mass. Additionally, it discusses periodic trends in ion size and specific ion electron configurations, with examples such as sodium losing electrons and potential cations of mercury.
- 3.S: Ionic Bonding and Simple Ionic Compounds (Summary)
- This page explains how atoms form compounds via chemical bonds, focusing on the octet rule. It describes ionic bonding, formed by cations and anions, and outlines the representation and naming conventions for chemical formulas. The chapter also details the naming of ionic compounds, their formula mass calculations, and describes the unique physical properties of ionic compounds, such as hardness and high melting points.