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Ionic and Metallic Bonding in Chemistry: A Comparative Study

Learn about the formation and properties of ionic and metallic bonds in chemistry, including electron interactions, structure, and conductivity. Understand the differences between these bond types. Dive into the world of atoms and molecules with detailed explanations and examples.

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Ionic and Metallic Bonding in Chemistry: A Comparative Study

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  1. Chapter 6B: Chemical Bonding General Chemistry Mr. Mata Cartoon courtesy of NearingZero.net

  2. 6-3 Ionic Bonding and Compounds • Ionic Compound- composed of + and - ions combined so charges are equal. (Metal + nonmetal) • Formula Unit- simplest group of atoms form an ionic compound.

  3. Cation Formation • Main group metals lose all their valence e-’s to form cations (+): • This loss of electrons is called oxidation. • Na .Na1+ +1e- sodium • Mg: Mg2+ + 2 e- magnesium • : Al. Al 3+ +3 e- aluminum

  4. Anion Formation • Non-metals gain e-’s to form anions (-). • This process is called reduction. Cl 1- chloride (gain 1 e-) O 2- oxide (gain 2 e-’s) N 3- nitride (gain 3 e-’s)

  5. Ionic Bond • - charges are attracted to + charges. • - anions are attracted to + cations. • The result is an ionic bond. • 3-D crystallattice of anions & cations formed.

  6. Structure of NaCl

  7. Properties of Ionic Compounds • Crystals form. • High melting point & boiling point. • Brittle (breaks easily). • Melt when heated (very high temps!) • Aqueous solutions conduct electricity. (solutions mixed in water)

  8. Electronegativity (EN) • Atoms to the right & top of Periodic Table have greater EN values. • F most EN of elements (EN = 4.0). • Fr least EN of elements (EN = O.7). • Cl =3.0 H = 2.1 S = 2.5 • O = 3.5 Na = 0.9 Br = 2.8 • C = 2.5 N = 3.0 I = 2.5

  9. Polar & Nonpolar Bonds • H-H is non-polar because H & H have the same EN’s. (EN diff. = 0) • Cl-Cl is non-polar because Cl & Cl have the same EN’s. (EN diff. = 0) • H-Cl is polar because H & Cl have different EN’s. ( H = 2.1, Cl = 3.0 )

  10. Predicting Bond Type • There is a continuum between non-polar covalent bonds to ionic bonds. • Non-polar bond; little difference in EN between atoms. (EN diff. = 0 – 0.3) • Ionic bonds; greatest EN diff between atoms. (ΔEN > 1.7) • Polar covalent bonds; in between EN diff between atoms. (EN diff. = 0.3 – 1.7)

  11. Ionic vs. Covalent Bonds Covalent Bonds • Sharing e-’s • non-metal + non-metal • Molecular (low mp/bp) • ex: CO2, Cl2 • Macromolecular (high mp/bp) • Ex: C(diamond), SiO2 • Non conductors Ionic Bonds • Exchange e-’s • Metal + non-metal • 3-D units (crystals) • high mp/bp • Brittle, melt • Ex: NaCl • conduct electricity

  12. Ionic Bonding in NaCl

  13. Ionic Bonding in NaCl

  14. 6-4 Metallic Bonding • Metals- conduct heat, have low ionization energy • Low EN; give up electrons easily. • Metals have luster (shine), are malleable (can be hammered into sheets) and are ductile (drawn into wires).

  15. Metallic Bonding • Metallic Bonding - type of bonding found in metallic crystals. • 3-D lattice of positive ions. • remain fixed in a crystal lattice. • loosely-held valence e-’s move freely throughout the crystal. • The fluid-like movements of valence e-’s make metals good conductors of heat and electricity.

  16. Metallic Bonding

  17. Metal Alloys • Alloys -metallic substances composed of two or more elements; at least one of these elements is a metal. • Alloys are important because the properties of an alloy are often superiorto those of its component elements.

  18. Chapter 6 SUTW Prompt • Describe the different properties of ionic bonds and metallic bonds by describing how the electrons interact with each bonding type. • Complete an 8-12 sentence paragraph using the SUTW paragraph format. Hilight using green, yellow, and pink. • Due Date: Monday, October 16, 2017 (start of class)

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