Chemistry: Chapter 7
Unit Topic:
Chemical Formulas and
Bonding
Specific Resources/www sites
Unit Duration:
Weeks _____________________
Objectives: The student will be able to
7.1 Ionic Bonding
1. Define Ionic Bonding and state how it is related to static electricity.
2. Describe the ions (and molecules) that metals and nonmetals tend to form and give examples.
3. Describe ionic compounds in detail using the terms: cations and anions, electrically neutral and use chemical
symbols to show them.
4. Describe the physical properties of ionic compounds including their interaction with water.
5. Describe why sodium chloride is more stable than elemental sodium and chlorine; show this using the octet rule.
6. State the Octet Rule and its exceptions and describe how the octet rule is satisfied when Sodium and Chlorine
make sodium chloride.
7. Learn what ions are and how to predict ion charges from the periodic table (do not include transition and inner
transition metals).
8. Learn what is meant by oxidation state
a.) learn where the elements are which have only one possible oxidation state.
b.) Learn where are the metals with multiple oxidation states.
9. Describe which electrons in an electron configuration are essential in bonding.
10. Be able to draw Lewis Dot diagrams for elements.
11. Distinguish and give examples of monatomic and polyatomic ions.
12. State and give examples of which elements form more than one kind of cation and show how they are written
and read (said) to distinguish them.
13. Know the difference and give examples between a monatomic cation and monatomic anion
14. Know how “ide” is used to name monatomic anions.
15. Know how to name and write formulas for acids and their related salts using the chart provided by your teacher.
16. Learn how “ic” and “ous” are used to distinguish between differently charged ions of the same metal
17. Know how to name and write formulas for compounds which contain no metals.
18. Learn how to use the reference acids to determine charges found in ions.
19. Be able to name and write chemical equations for Binary Ionic Compounds.
20. Give examples of empirical formulas for Binary Ionic Compounds and how the criss-cross (crossover) method
works to make them electronically neutral.
21. Explain how you can use the criss-cross method for Polyatomic ions.
1
7.2 Covalent Bonding
22. Describe the physical differences between compounds with ionic and covalent bonds and give examples of those
compounds.
23. Define: Molecular Substance
24. Distinguish between a molecular formula and a structural formula using glucose as an example.
25. Explain the difference between single, double and triple covalent bonds using dots and lines.
26. Be able to draw dot structures with single, double and triple bonds.
27. Compare and contrast polar, nonpolar, and covalent bonds.
28. Use Lewis dots to show structural formulas and be able to change them to line structures.
29. Describe the octet rule for Lewis dot structures and its anomalies.
30. Be able to calculate valence electrons and oxidation numbers.
31. Be able to use the Electronegativity table and the chart on your help card to determine if a bond is ionic, covalent
or polar covalent.
32. Be able to use the Delta symbol ( δ ) in a polar bond to indicate the slightly negative and slightly positive
portions
7.3. Naming Chemical Compounds
33. Describe the steps how to name ionic compounds and molecular compounds.
34. Define the term hydrate and anhydrous substances, and explain how a hydrate is named such as
CuSO4 ● H20 as copper II sulfate pentahydrate.
36. Define the term acid and explain how an acid is named.
37. Describe how you can identify an Ionic and a molecular compound by the location of its elements on the
periodic table.
39. Describe a cation and an anion.
40. Describe how to determine the charge of a multivalent cation from the “ic-ous” chart.
41. Define Ionic substances called hydrates and anhydrous substances.
42. Define acid as a molecular substance that dissolves in water to produce hydrogen H+ ions (cation) and a
(reference) anion.
2