Objective Sheet
2. Give the group names for the following:
a. IA h. VIIIA
b. IIA i. B Groups
c. IIIA j. Detached Top Row
d. IVA k. Detached Bottom Row
e. VA l. The Bottom Two Rows, Collectively
f. VIA
g. VIIA
3. Explain what the representative elements are.
4. Using your periodic table, determine whether an element is a metal, nonmetal, or metalloid.
5. List several properties of
a. metals
b. nonmetals
c. metalloids (also called semimetals)
6. Define ions, cations, and anions.
7. Explain how cations and anions are formed.
8. Tell which is more likely to form cations....metals, nonmetals, or metalloids.
9. Tell which is more likely to form anions...metals, nonmetals, or metalloids.
10. Give the charge of an atom that....
a. Gains 3 electrons
b. Loses 3 electrons
11. Explain the differences between molecular and ionic compounds. Include in your discussion the
type of elements that make up each as well as the differences in their physical properties.
12. Given the names of two elements, predict whether the compound that forms from their
chemical reaction would be molecular or ionic.
13. Based upon your knowledge of a compound's physical properties, determine whether it is more
likely to be a molecular compound or an ionic compound.
14. Define the following;
a. molecule
b. chemical formula
c. molecular formula
d. formula unit
15. Identify the number and kinds of atoms present in a molecule of a compound, such as
monosodium glutamate, C5H8O4NNa.
16. Using your periodic table, find the charge of any element. Remember, silver is always 1+,
cadmium and zinc are always 2+.
17. Be able to use the stock name or the classical name to identify the charge of any transition metal.
You may use the back of your periodic table for help with this.
18. Correctly name cations (name doesn't change) and anions (name ending changes to -ide.).
19. Define polyatomic ion.
20. Using your chart, identify the formula and charge of the polyatomic ions.
21. Explain the difference between the -ite and -ate ending for the polyatomic ions.
22. Note that two polyatomic ions have the -ide ending, simlar to the elemental anions. What are they?
23. Explain why a systematic method of naming chemical compounds is necessary and why it is
more useful that the common name system.
24. Define binary ionic compounds.
25. Write formulas for binary ionic compounds.
26. State the net charge on all binary ionic compounds.
27. When given a formula, write the name of the binary ionic compound.
28. Define ternary ionic compounds.
29. Write the formulas and give the names for ternary ionic compounds.
30. Explain when parentheses must be used when writing formulas.
31. Explain when Roman Numerals must be used when writing formulas.
32. Define binary molecular compounds.
33. Write the formulas for and name binary molecular compounds.
34. Give the formulas for the six common acids:
a. hydrochloric acid d. acetic acid
b. sulfuric acid e. phosphoric acid
c. nitric acid f. carbonic acid
35. State the diatomic elements.
36. Explain what is meant by diatomic elements.
37. When do these elements exist diatomically?