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Bonding in Solids Bonding in Solids • There Are Four Types of Solid: 1

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Bonding in Solids Bonding in Solids • There Are Four Types of Solid: 1 Bonding in Solids Bonding in Solids • There are four types of solid: 1. Molecular (formed from molecules) - usually soft with low melting points and poor conductivity. 2. Covalent network -veryhardwithveryhigh melilting points and poor condiiductivity. 3. Ionic (formed form ions) - hard, brittle, high melting poitintsand poor condtiitductivity. 4. Metallic (formed from metal atoms) - soft or hard, high melting points, good conductivity, malleable and ductile. – NB: A solid with only one type of atom is also called ‘atomic’ Copyright © Houghton Mifflin Company. All rights reserved. 16a–1 Copyright © Houghton Mifflin Company. All rights reserved. 16a–2 Bonding in Solids Bonding in Solids Covalent Network Solids Covalent Network Solids • Intermolecular forces: dipole-dipole, London dispersion and H- bonds. • Atoms held together in large networks. • Exampp,gp,q(les: diamond, graphite, quartz (SiO2), silicon carbide ( SiC), and boron nitride (BN). • In diamond: – each C atom has a coordination number of 4; – each C atom is tetrahedral; – there is a three -dimensional array of atoms. – Diamond is hard, and has a high melting point (3550 °C). Copyright © Houghton Mifflin Company. All rights reserved. 16a–3 Copyright © Houghton Mifflin Company. All rights reserved. 16a–4 Diamond -Hard Structure - Tetrahedral atomic arrangement What hybrid state do you think the carbon has? Copyright © Houghton Mifflin Company. All rights reserved. 16a–5 Copyright © Houghton Mifflin Company. All rights reserved. 16a–6 Bonding in Solids Covalent Network Solids • In graphite – each C atom is arranged in a planar hexagonal ring; – layers of interconnected rings are placed on top of each other; – the distance between C atoms is close to benzene (1.42 ÅÅÅ vs. 1.395 Å in benzene); – the distance between layers is large (3.41 Å); – electrons move in delocalized orbitals (good conductor). Copyright © Houghton Mifflin Company. All rights reserved. 16a–7 Copyright © Houghton Mifflin Company. All rights reserved. 16a–8 Fullerene-C60 •Closely Related to GhitGraphite Graphite Structure •Both Six-membered and Five-membered Rings of Carbon are Found in the Fullerenes -Form planar sheets - actually more stable than diamond What hybrid state do you think the carbon has? Copyright © Houghton Mifflin Company. All rights reserved. 16a–9 Copyright © Houghton Mifflin Company. All rights reserved. 16a–10 Artists carbon nanotubes, multiwalled MWCNT Forming Carbon Nanotubes Copyright © Houghton Mifflin Company. All rights reserved. 16a–11 Copyright © Houghton Mifflin Company. All rights reserved. 16a–12 Real carbon nanotubes Examples of Three Types of Crystalline Solids Copyright © Houghton Mifflin Company. All rights reserved. 16a–13 Copyright © Houghton Mifflin Company. All rights reserved. 16a–14 Cubic Unit Cells There are 7 basic crystal systems, but we are only concerned with CUBIC. All sides equal length All angles are 90 degrees Copyright © Houghton Mifflin Company. All rights reserved. 16a–15 Copyright © Houghton Mifflin Company. All rights reserved. 16a–16 X-rays scattered from two different atoms may reinforce (constructive interference) or cancel (destructive interference) one another. Copyright © Houghton Mifflin Company. All rights reserved. 16a–17 Copyright © Houghton Mifflin Company. All rights reserved. 16a–18 Figure 16.11: Reflection of X rays of Reflection of X rays: Bragg equation wavelength n λ = 2 d sin θ Father and son Bragg – Nobel prize 1915 Copyright © Houghton Mifflin Company. All rights reserved. 16a–19 Copyright © Houghton Mifflin Company. All rights reserved. 16a–20 Crystal Lattices Cubic Unit Cells of Metals • Regular 3-3-DD arrangements of equivalent LATTICE Simple Body- POINTS in space. cubic (SC) centered • Lattice points define UNIT CELLS 1 atom/unit cell FaceFace-- cubic (BCC) – smallest reppgeating internal unit that has the s ymmetr y centered 2 atoms/unit cell characteristic of the solid. cubic (FCC) 4 atoms/unit cell Copyright © Houghton Mifflin Company. All rights reserved. 16a–21 Copyright © Houghton Mifflin Company. All rights reserved. 16a–22 Atom Sharing Atoms in unit cell at Cube Faces and Corners 1 ½ ¼ Atom shared in corner Atom shared in face --> 1/8 inside each unit cell --> 1/2 inside each unit cell 1/8 Copyright © Houghton Mifflin Company. All rights reserved. 16a–23 Copyright © Houghton Mifflin Company. All rights reserved. 16a–24 Number of Atoms per Unit Cell Simple Ionic Compounds Unit Cell Type Net Number Atoms SC 1 CsCl has a SC lattice of + - BCC 2 Cs ions with Cl in the cente r. FCC 4 1 unit cell has 1 Cl- ion plus (8 corners)(1/8 Cs+ per corner) = 1 net Cs+ ion. Copyright © Houghton Mifflin Company. All rights reserved. 16a–25 Copyright © Houghton Mifflin Company. All rights reserved. 16a–26 Two Views of CsCl Unit Cell Simple Ionic Compounds Either arrangement leads to formula of 1 Cs+ and 1 Cl - per unit cell Salts with formula MX can have SC structure — but not salts with formula MX 2 or M2X Copyright © Houghton Mifflin Company. All rights reserved. 16a–27 Copyright © Houghton Mifflin Company. All rights reserved. 16a–28 NaCl Construction Na+ in FCC lattice of Cl- with octahedral Na+ in holes holes Copyright © Houghton Mifflin Company. All rights reserved. 16a–29 Copyright © Houghton Mifflin Company. All rights reserved. 16a–30 Your eyes “see” 14 Cl- ions and 13 Na+ The Sodium Chloride Lattice ions in the figure Many common salts have FCC arrangements of anions with cations in OCTAHEDRAL HOLES — e. g., salts such as CA = NaCl • FCC lattice of anions -------->> 4 A-/unit cell ••CC+ in octahedral holes ------>> 1 C+ at center + [12 edges • 1/4 C+ per edge] = 4 C+ per unit cell + - Ion Count for the Unit Cell: 4 Na and 4 Cl Na4Cl4 = NaCl Can you see how this formula comes from the unit cell? Copyright © Houghton Mifflin Company. All rights reserved. 16a–31 Copyright © Houghton Mifflin Company. All rights reserved. 16a–32 Bonding in Solids Comparing NaCl and CsCl Ionic Solids – NaCl Structure • Each ion has a coordination number of 6. • Face-centered cubic lattice. • Cation to anion ratio is 1:1. • Even though their formulas have one • Examples: LiF, KCl, AgCl and CaO. cation and one anion, the lattices of CsCl – CsCl Structure and NaCl are different. • Cs+ has a coordination number of 8. • Different from the NClNaCl structure (Cs+ is larger than • The different lattices arise from the fact Na+). that a Cs+ ion is much larger than a Na + • Cation to anion ratio is 1:1. ion. Copyright © Houghton Mifflin Company. All rights reserved. 16a–33 Copyright © Houghton Mifflin Company. All rights reserved. 16a–34 The CsCl and NaCl Structures CsCl NaCl Copyright © Houghton Mifflin Company. All rights reserved. 16a–35 Copyright © Houghton Mifflin Company. All rights reserved. 16a–36 Figure 16.13: The closet packing arrangement of uniform spheres. Copyright © Houghton Mifflin Company. All rights reserved. 16a–37 Copyright © Houghton Mifflin Company. All rights reserved. 16a–38 Figure 16.14: When spheres are closest packed so that the spheres in the third layer are directlly over those in the first layer (aba), the unit cell is the hexagonal prism illustrated here in red. Copyright © Houghton Mifflin Company. All rights reserved. 16a–39 Copyright © Houghton Mifflin Company. All rights reserved. 16a–40 Figure 16.37: (a) The octahedral hole (shown in yellow) lies at the center of six spheres that touch along the edge Figure 16 . 36: (e) of the square . The holes that exist among closest packed uniform spheres Copyright © Houghton Mifflin Company. All rights reserved. 16a–41 Copyright © Houghton Mifflin Company. All rights reserved. 16a–42 Figure 16.37: (a) The octahedral hole (shown in yellow) lies at the center of six spheres that touch along the edge Figure 16.38: (e) of the square . ()Th(a) The tetrahedral hole (b) The d = 2R√2 center of the 2r = 2R√2 – 2R tetrahedral r = R(√2 – 1) hole = R()(0.414) r = R(0.225) Copyright © Houghton Mifflin Company. All rights reserved. 16a–43 Copyright © Houghton Mifflin Company. All rights reserved. 16a–44 Figure 16.39: One packed sphere and its (a) A simple cubic array with X- ions, with an M+ ion in the center (in the cubic hole). relationship to the tetrahedral hole (b) The body diagonal b equals r = R(0.732) r = R(0.732) Copyright © Houghton Mifflin Company. All rights reserved. 16a–45 Copyright © Houghton Mifflin Company. All rights reserved. 16a–46 Copyright © Houghton Mifflin Company. All rights reserved. 16a–47.
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