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Chemical Bonds: Ionic, Covalent, Metallic, and Hydrogen

This chapter discusses the different types of chemical bonds, including ionic, covalent, metallic, and hydrogen bonds. It explains the concepts of electronegativity, Lewis structures, and the octet rule. The text also covers the characteristics and properties of each bond type.

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Chemical Bonds: Ionic, Covalent, Metallic, and Hydrogen

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  1. Chapter 7 • Chemical Bonds

  2. Chemical bond • Link between atoms that results from attractions of their nuclei for e-

  3. 1. Ionic bond • Attraction between (+) and (-) ions, exchange of e- • Usually between metals and nonmetals

  4. Ion • Atom or group of atoms with a (+) or (-) charge • Cation: (+) chg • Anion: (-) chg

  5. e.g. sodium

  6. e.g. chlorine

  7. Na and Cl ions  ionic bond

  8. Polyatomic ions • Charged group of bonded atoms • e.g. phosphate ion (PO43-)

  9. 2. Covalent bonds • Sharing of e- • Usually between nonmetals

  10. Covalent bonding • Molecule- smallest unit quantity of matter that can exist by itself, e.g. atom of He, O2, H2O • Diatomic molecule-2 atoms, e.g. HCl, H2

  11. e.g. hydrogen molecule

  12. Bond types

  13. Chemical bonds are usually not completely ionic or covalent Difference in electronegativity 4.0 1.7 0.3 0.0 Polar covalent Non polar covalent ionic

  14. electronegativity • Measure of ability of an atom in a chem. cmpd. to attract electrons

  15. Chemical formula • Type and relative # of atoms in a chemical compound, e.g. H2O

  16. e- config.andbonding

  17. Octet rule • Atoms often gain, lose, or share electrons to achieve the same number of electrons as the noble gas closest to them in the periodic table • Because all noble gasses (except He) have filled s and p valence orbitals (8 electrons), many atoms undergoing reactions also end up with 8 valence electrons. • Octet Rule: Atoms tend to lose, gain, or share electrons until they are surrounded by 8 valence electrons • Note: there are exceptions to the octet rule, e.g.He

  18. Valence electrons • Electrons lost, gained, or shared in formation of chemical cmpds.

  19. Lewis structures • N2 (nitrogen) • Carbon tetrachloride

  20. Lewis structure • Structural formula

  21. Structural formula • Indicates the kind, number, arrangement, and bonds of atoms in molecules

  22. Single bonds • Sharing (1) pr. of e-

  23. Double bond • Sharing (2) pr. of e-

  24. Triple bond • Sharing (3) pr of e-

  25. 3. Metallic bonds • Metal-metal bonds, electron ‘sea’

  26. Metallic bonding • Results from attraction between (+) ions and surrounding mobile electrons (electron sea) • Motion of free electrons accounts for high conductivity of heat and electricity • Malleability and ducticity possible because bonding is not directional

  27. 4. Hydrogen bonds • Weak bonds between molecules due to partial charges on atoms • e.g. water

  28. Polarity of water molecule  hydrogen bonding

  29. Review: ionic or covalent? • Ca and Cl • Ionic • Na and F • Ionic • N and O • Covalent • H and H • Covalent

  30. Review: Lewis Structure • H + H + O • C2H4 (ethene)

  31. What kind of bonds?

  32. Define: • Covalent bond • Ionic bond • Metallic bond • Hydrogen bond • Diatomic molecule • Cation • Anion • Electronegativity

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