8: Ionic and Metallic Bonding
- Page ID
- 53728
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\(\newcommand{\avec}{\mathbf a}\) \(\newcommand{\bvec}{\mathbf b}\) \(\newcommand{\cvec}{\mathbf c}\) \(\newcommand{\dvec}{\mathbf d}\) \(\newcommand{\dtil}{\widetilde{\mathbf d}}\) \(\newcommand{\evec}{\mathbf e}\) \(\newcommand{\fvec}{\mathbf f}\) \(\newcommand{\nvec}{\mathbf n}\) \(\newcommand{\pvec}{\mathbf p}\) \(\newcommand{\qvec}{\mathbf q}\) \(\newcommand{\svec}{\mathbf s}\) \(\newcommand{\tvec}{\mathbf t}\) \(\newcommand{\uvec}{\mathbf u}\) \(\newcommand{\vvec}{\mathbf v}\) \(\newcommand{\wvec}{\mathbf w}\) \(\newcommand{\xvec}{\mathbf x}\) \(\newcommand{\yvec}{\mathbf y}\) \(\newcommand{\zvec}{\mathbf z}\) \(\newcommand{\rvec}{\mathbf r}\) \(\newcommand{\mvec}{\mathbf m}\) \(\newcommand{\zerovec}{\mathbf 0}\) \(\newcommand{\onevec}{\mathbf 1}\) \(\newcommand{\real}{\mathbb R}\) \(\newcommand{\twovec}[2]{\left[\begin{array}{r}#1 \\ #2 \end{array}\right]}\) \(\newcommand{\ctwovec}[2]{\left[\begin{array}{c}#1 \\ #2 \end{array}\right]}\) \(\newcommand{\threevec}[3]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \end{array}\right]}\) \(\newcommand{\cthreevec}[3]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \end{array}\right]}\) \(\newcommand{\fourvec}[4]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \\ #4 \end{array}\right]}\) \(\newcommand{\cfourvec}[4]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \\ #4 \end{array}\right]}\) \(\newcommand{\fivevec}[5]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \\ #4 \\ #5 \\ \end{array}\right]}\) \(\newcommand{\cfivevec}[5]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \\ #4 \\ #5 \\ \end{array}\right]}\) \(\newcommand{\mattwo}[4]{\left[\begin{array}{rr}#1 \amp #2 \\ #3 \amp #4 \\ \end{array}\right]}\) \(\newcommand{\laspan}[1]{\text{Span}\{#1\}}\) \(\newcommand{\bcal}{\cal B}\) \(\newcommand{\ccal}{\cal C}\) \(\newcommand{\scal}{\cal S}\) \(\newcommand{\wcal}{\cal W}\) \(\newcommand{\ecal}{\cal E}\) \(\newcommand{\coords}[2]{\left\{#1\right\}_{#2}}\) \(\newcommand{\gray}[1]{\color{gray}{#1}}\) \(\newcommand{\lgray}[1]{\color{lightgray}{#1}}\) \(\newcommand{\rank}{\operatorname{rank}}\) \(\newcommand{\row}{\text{Row}}\) \(\newcommand{\col}{\text{Col}}\) \(\renewcommand{\row}{\text{Row}}\) \(\newcommand{\nul}{\text{Nul}}\) \(\newcommand{\var}{\text{Var}}\) \(\newcommand{\corr}{\text{corr}}\) \(\newcommand{\len}[1]{\left|#1\right|}\) \(\newcommand{\bbar}{\overline{\bvec}}\) \(\newcommand{\bhat}{\widehat{\bvec}}\) \(\newcommand{\bperp}{\bvec^\perp}\) \(\newcommand{\xhat}{\widehat{\xvec}}\) \(\newcommand{\vhat}{\widehat{\vvec}}\) \(\newcommand{\uhat}{\widehat{\uvec}}\) \(\newcommand{\what}{\widehat{\wvec}}\) \(\newcommand{\Sighat}{\widehat{\Sigma}}\) \(\newcommand{\lt}{<}\) \(\newcommand{\gt}{>}\) \(\newcommand{\amp}{&}\) \(\definecolor{fillinmathshade}{gray}{0.9}\)- 8.1: Electron Dot Diagrams
- This page explains electron dot diagrams that illustrate valence electrons, essential for understanding an atom's chemical properties and bonding behavior. These diagrams display valence electrons as dots around the element's symbol and highlight their role in reactivity, with specific counts dictated by group placement in the periodic table. Notably, Group 1 has one valence electron, Group 2 has two, and Group 18 has eight.
- 8.2: Octet Rule
- This page explains the organization of electrons in atoms, comparing it to seating arrangements at graduation. It discusses the octet rule by Gilbert Lewis, which states that atoms aim for eight valence electrons for stability, reminiscent of noble gases, which are generally unreactive. While noble gases have full outer shells, exceptions exist for hydrogen and lithium. Atoms achieve stability by sharing or transferring electrons, with metals losing electrons and nonmetals gaining them.
- 8.3: Cation Formation
- This page explains that cations are positively charged ions formed by the loss of electrons, allowing atoms to mimic noble gas configurations. It provides examples like sodium (Na+), magnesium (Mg2+), and aluminum (Al3+). Additionally, it mentions that high cation concentrations in hard water can cause problems, and that ion exchange resins can be used to reduce these minerals, enhancing water quality.
- 8.4: Anion Formation
- This page discusses the dangers of chlorine gas and its reaction with sodium to form safe sodium chloride. It explains the formation of anions, negatively charged ions that achieve stability by gaining electrons. The concept of isoelectronic species, where different ions have the same electron configuration, is highlighted to illustrate the differences between ions like sodium and neon. The summary emphasizes the importance of anions in ion formation.
- 8.5: Transition Metal Ion Formation
- This page discusses transition metals, focusing on their complex electron configurations in the d block. These metals can lose electrons from both s and d sublevels, resulting in various ion charges. For example, iron typically forms Fe²⁺ and Fe³⁺. While some transition metals reach noble-gas configurations, others like zinc and copper achieve a stable pseudo noble-gas configuration. The process of forming these ions involves intricate electron rearrangements.
- 8.6: Ionic Bonding
- This page discusses ionic compounds using sodium chloride as a main example. It explains that table salt can be obtained from salt mines or oceans, emphasizing that dissolved salt exists as separate ions until water is evaporated. The text covers ionic bonds, which arise from the attraction between oppositely charged ions, with bond strength depending on charge and distance.
- 8.7: Ionic Crystal Structure
- This page discusses the value of crystals, especially ruby, for their beauty, utility, and magical attributes. It explains that ionic compounds like sodium chloride create extended three-dimensional structures, maximizing attractive forces between cations and anions. Additionally, it highlights the use of visual models, such as ball-and-stick and space-filling diagrams, to represent these structures, which can be analyzed at the atomic level with modern techniques.
- 8.8: Coordination Number
- This page discusses the color variation of cobalt salts based on surrounding species and water influence. It defines coordination number, exemplified by sodium chloride (NaCl) with a coordination number of 6 and cesium chloride (CsCl) with 8 due to larger ions. Additionally, it notes the coordination values in titanium(IV) oxide (TiO2) and the structural representation in iron(III) chloride (FeCl3), emphasizing how crystal structures correspond to formula units.
- 8.9: Physical Properties of Ionic Compounds
- This page discusses the distinct physical properties of ionic compounds, highlighting their high melting points, hardness, brittleness, and inability to conduct electricity in solid form, while emphasizing their conductivity when dissolved or melted. It also provides examples of colored ionic crystals, such as amethyst and azurite, explaining that their colors often arise from transition metal ions.
- 8.10: Metallic Bonding
- This page explains that metals possess unique properties due to metallic bonding, characterized by positive ions in a sea of delocalized electrons. This structure facilitates efficient electrical and thermal conductivity, imparts luster through light interaction, and allows metals to be ductile and malleable, enabling shaping without breaking, in contrast to brittle ionic compounds. Overall, these properties are closely tied to the nature of metallic bonds.
- 8.11: Crystal Structure of Metals
- This page explains the stacking of cannonballs and its relevance to metallic crystal structures. It highlights how pyramidal arrangements mirror the close-packed configurations of atoms in metals, emphasizing body-centered cubic (bcc) and face-centered cubic (fcc) structures. The bcc structure has a coordination number of 8, while fcc and hexagonal close-packed (hcp) structures have a coordination number of 12, showcasing their efficient packing with minimal empty space.
- 8.12: Alloys
- This page discusses the significance of alloys in guitar strings, noting that electric guitars utilize steel strings for magnetic detection, while acoustic guitars prefer bronze and titanium for tone quality. It outlines the benefits of alloys like bronze and brass in musical instruments and underscores the strength and corrosion resistance of steel alloys in construction, facilitating the development of tall structures such as skyscrapers.