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Understanding Ionic and Covalent Bonds in Chemistry

Learn about ionic, covalent, and metallic bonds in chemistry, including properties of ionic compounds, naming conventions, molecular structures, and the formation of alloys. Get insights on chemical bonding with clear examples and explanations.

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Understanding Ionic and Covalent Bonds in Chemistry

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  1. Chapter 6 Chemical Bonds

  2. Show second one http://science.howstuffworks.com/periodic-table-videos-playlist.htm

  3. Ionic Bonds Sec. 6.1 • When elements react they tend to transfer electrons to become stable • Ex. Na and Cl • When ions form the charge changes from neutral because of a change in the number of protons or electrons. • Ex. Na+ and Cl-

  4. 1 2 3 4 5 6 7 Lose e- Gain/ Lose e- Gain e-

  5. Anion • Negative charge • Have the ending –ide • Ex. Cl- becomes chloride

  6. Cation • Positive charge • The name is the same as the element • Ex. Na+ is sodium

  7. Ionic Compounds • Shows the ratio of the atoms in the compound • Ex. NaCl • Ex. MgCl2 (2 Cl atoms needed)

  8. Properties of Ionic Compounds • Strong attraction of ions • High melting point • Not malleable

  9. Ionic Compounds • The name of the compound must distinguish it from other compounds of the same elements • The formula describes the ratio of the elements that make up the compound

  10. Naming Binary Compounds • They follow a predictable pattern of the cation followed by the anion • Remember: the anion will end in –ide • Ex. Figure 16 Common Anions

  11. Practice with compounds • Write the chemical formulas for the following compounds using their valence electrons to assist you… • Li and N K and P H and F • Al and P C and S Al and Br • C and Sn B and N Rb and Se • Answers • Li3N K3P HF • Al3P3(AlP) C2S4(CS2) AlBr3 • C4Sn4 (CSn) B3N3 (BN) Rb2Se

  12. Naming the compounds from previous slide • Li and N K and P H and F • Al and P C and S Al and Br • C and Sn Ba and C Rb and Se • Lithium nitride Potassium phosphide • Hydrogen fluoride Aluminum phosphide • Carbon sulfide Carbon Tinide • Aluminum Bromide Boron Nitride • Rubidium selenide

  13. Multiple Ions • The transition metals form more than one type of ion • Ex. Cu (I) with a 1+ charge and Cu (II) with a 2+ charge • The other elements have positive charges that are equal to their group number

  14. Polyatomic Ions • Many ions • Positive or negatively charged • Figure 19

  15. Writing Formulas for Ionic Compounds • Determine the ratio of elements needed in the compound by using the charges given. • Ex. Na has a 1+ charge and S has a 2- charge = Na2S • Practice Page 174

  16. Covalent Bonding 6.2 • Sharing electrons (Co) means to share • Ex. Hydrogen • Single bond between the elements H-H • H2 describes a molecule of Hydrogen • Many nonmetals exist as diatomic molecules • Ex. Cl2

  17. Multiple Covalent Bonding • Sharing multiple pairs of electrons • Ex. N2 has a triple bond Page 167

  18. Polar or Nonpolar Molecule? • If it has only two atoms, it is polar • If there are more than two atoms, the type of atoms and the shape determine whether the molecule is polar or nonpolar • H2O is polar because it has a bent shape • Polar attractions are greater than nonpolar

  19. Naming Molecular Compounds6.3 • The most metallic element appears first in the name • The name of the second will end in –ide • Ex. N2O4 – dinitrogen tetraoxide • NO2 – nitrogen dioxide • Prefixes for naming compounds is figure 20

  20. Metallic Bonds 6.4 • Metals become cations with a pool of shared electrons surrounding it • The attraction between the cation and the surrounding electrons is the metallic bond

  21. Properties of Metal • The ability to conduct and malleability are two properties of metal that are explained by the structure of the electrons around the metal • Figure 22 - malleability

  22. Alloys • Mixture of metals • Copper – when mixed with tin will produce bronze, and when mixed with zinc will produce brass • Steel – a mixture of iron and small amounts of carbon

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