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Part I. Introduction to Bonding (p. 161 – 163 in class)

Explore the basics of chemical bonding, including ionic, covalent, and metallic bonds. Learn about bond types, structures, properties, and bond polarity. Understand how differences in electronegativity determine bond characteristics.

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Part I. Introduction to Bonding (p. 161 – 163 in class)

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  1. Unit 4 Part 1 - Chemical Bonding Part I. Introduction toBonding(p. 161 – 163 in class)

  2. A. Vocabulary • Chemical Bond • attractive force between atoms or ions that binds them together as a unit • bonds form in order to… • decrease potential energy (PE) • increase stability

  3. A. Vocabulary CHEMICAL FORMULA Ionic Compounds Covalent Molecules Formula Unit Molecular Formula NaCl CO2

  4. A. Vocabulary COMPOUNDS more than 2 elements 2 elements Binary Compound Ternary Compound NaCl NaNO3

  5. A. Vocabulary ION 2 or more atoms 1 atom Monatomic Ion Polyatomic Ion Na+ NO3-

  6. B. Types of Bonds IONIC COVALENT e- are transferred from metal to nonmetal e- are shared between two nonmetals Bond Formation Type of Structure true molecules crystal lattice Physical State liquid or gas solid Melting Point low high Solubility in Water yes usually not yes (solution or liquid) Electrical Conductivity no Other Properties odorous Brittle solids C. Johannesson

  7. B. Types of Bonds METALLIC e- are delocalized among metal atoms Bond Formation Type of Structure “electron sea” Physical State solid Melting Point very high Solubility in Water no yes (any form) Electrical Conductivity malleable, ductile, lustrous Other Properties C. Johannesson

  8. B. Types of Bonds Metals and Nonmetals Electron transfer from sodium to chlorine C. Johannesson RETURN

  9. B. Types of Bonds Ionic Bonding - Crystal Lattice RETURN

  10. B. Types of Bonds Covalent Bonding - True Molecules Nonmetals Only Diatomic Molecule RETURN

  11. B. Types of Bonds in Metals Metallic Bonding - “Electron Sea” RETURN

  12. C. Bond Polarity • Most bonds are a blend of ionic and covalent characteristics. • Difference in electronegativity determines bond type.

  13. C. Bond Polarity • Electronegativity • Attraction an atom has for a shared pair of electrons. • higher e-neg atom  - • lower e-neg atom +

  14. C. Bond Polarity • Electronegativity Trend (p. 151) • Increases up and to the right.

  15. C. Bond Polarity • Nonpolar Covalent Bond • e- are shared equally • symmetrical e- density • usually identical atoms

  16. - + C. Bond Polarity • Polar Covalent Bond • e- are shared unequally • asymmetrical e- density • results in partial charges (dipole)

  17. C. Bond Polarity Examples: • Cl2 • HCl • NaCl 3.0-3.0=0.0 Nonpolar 3.0-2.1=0.9 Polar 3.0-0.9=2.1 Ionic

  18. https://courseware.e-education.psu.edu/courses/matse081hons/content/lesson07/05.htmlhttps://courseware.e-education.psu.edu/courses/matse081hons/content/lesson07/05.html • https://courseware.e-education.psu.edu/courses/matse081hons/content/lesson07/05.html C. Johannesson

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