Honors Chemistry
Review Packet 2016
Name: ________________________________
Section I: Reading the Periodic Table
Define the following terms:
Period –
Group (or Family) –
Periodic Function –
What do elements in the same group or family have in common with each other?
Label the groups by number on the periodic table below, then identify the columns of the families below:
Alkali metals
Noble Gases
Alkaline Earth Metals
Transition Metals
Halogens
Inner-Transition Metals
Draw the staircase on the periodic table above. How can you tell whether an element is a metal, a non-metal, or
a metalloid based on its location on the periodic table?
Atomic Number –
Average Atomic Mass –
What are valence electrons?
Label the number of valence electrons for each column on the periodic table below:
Section II: Types of Bonding

A cation is a ______________ charged ion that forms when an atom ____________ one or more electrons.

An anion is a ______________ charged ion that forms when an atom ____________ one or more electrons.

Ionic compounds are held together by ionic bonds formed from the ________________________between
positively charged ______________ cations and negatively charged ______________ anions. Because
ionic compounds consist of large numbers of ions held together in a lattice structure, they do not exist as
individual molecules. Instead, a _________________ indicates the simplest ratio of atoms in an ionic
compound.

Molecular compounds are held together by ______________ bonds that are formed when electrons are
shared between two or more _____________________atoms. The simplest unit of a molecular compound
is called a(n) ___________
_____.
Label the following compounds as either ionic or molecular:
How can you tell? _______________________________________________________
1. CaF2
6. Cu2O
2. CO2
7. N2O3
3. MgO
8. ClF
4. AlCl3
9. LiCl
5. H2O
10. Ca3N2
What does the octet rule state?
Use the octet rule to predict the charges of the s-block and p-block elements on the periodic table below.

Different elements can form different types of ions, based on the number of _____________________they
have. The charge an element has in a compound is sometimes known as its ____________________.

Note that hydrogen forms the hydrogen ion (H+) in compounds with _______________ and the hydride ion
(H–) in compounds with ________________.

Many elements, including most of the _______________ metals, have oxidation states that are difficult to
predict from their location on the periodic table. These elements can often form more than one type of ion.
For instance, iron may form a +2 ion or a +3 ion in an ionic compound.
Determining Oxidation States Practice Wkst
Determine the oxidation number of the underlined element in each example:
1. BrCl
11. NaAuCl4
2. Au2O3
12. K2W4O13
3. KMnO4
13. NbOF63–
4. NaClO4
14. ZrO2
5. Li2CO3
15. Mg(BF4)2
6. ClO–
16. Cs2TeF8
7. K4P2O7
17. NH4+
8. SeO32–
18. NaIO3
9. OF2
19. Cr2O72–
10. KAl(SO4)2
20. Na3VO4
Section IV: Nomenclature Practice I
Notes: First decide whether to use the Ionic or Covalent naming rules. (If the first element is a metal or a
polyatomic ion than follow the rules for Ionic compounds)
Next – If covalent then write the subscript on each element as a prefix in front of the elements chemical
name
Ex: S3 would be written as trisulfur
The second element in the compound has its ending changed to –ide (unless on polyatomic list)
However – if the compound is Ionic – you need to identify oxidation states on both the cations and anions
before you proceed – and you should not use prefixes.
Name the following compounds:
1. K2O
11. Cr(OH)3
2. Mg3N2
12. RbCl
3. NaNO2
13. SnO2
4. CF4
14. AgCl
5. Ni3(PO4)2
15. Cu(NO3)2
6. Ca(OH)2
16. NaClO2
7. FeS
17. CO2
8. Cu2O
18. SeH2
9. P4O10
19. Mn(NO3)2
10. Al2(SO4)3
20. (NH4)2Cr2O7
Write formulas for the following compounds:
1. sodium bromide
11. vanadium (III) oxide
2. strontium chloride
12. iron (III) iodide
3. aluminum nitrate
13. nitrogen dioxide
4. sulfur trioxide
14. ammonium nitrate
5. cobalt (II) oxide
15. magnesium fluoride
6. lead (IV) iodide
16. gallium (III) chloride
7. hydrogen sulfide
17. cadmium chloride
8. calcium chlorate
18. silicon tetrachloride
9. lithium acetate
19. sodium hydride
10. krypton difluoride
20. manganese (VII) oxide
Section V: Nomenclature Practice II
Name the following compounds:
1. Na2S
11. Mg(NO3)2
2. Ba(OH)2
12. (NH4)2SO4
3. P2O3
13. AuCl
4. Rb2SO4
14. S2O4
5. Ca3(PO4)2
15. NiCl3
6. Cd(NO3)2
16. K3PO4
7. FeCl2
17. Co(NO3)2
8. AlF3
18. N4H6
9. Sn(OH)4
19. MgCl2
10. PBr3
20. XeF4
Write formulas for the following compounds:
1. chromium (III) nitrate
11. copper (I) sulfite
2. cesium oxide
12. phosphorus pentachloride
3. sodium bicarbonate
13. arsenic trichloride
4. thallium (I) sulfate
14. mercury (II) oxide
5. carbon tetrachloride
15. potassium oxalate
6. ammonium chloride
16. tin (II) nitrate
7. iron (III) carbonate
17. zinc oxide
8. barium chloride
18. lead (II) sulfate
9. silver chromate
19. sodium acetate
10. hydrogen iodide
20. iron (III) hydroxide
Section VI: Nomenclature Practice III
Name the following compounds:
1. KI
11. Ca3P2
2. ZnCl2
12. Na2C2O4
3. Li2Cr2O7
13. MnI2
4. TiO2
14. SH6
5. N2O
15. Fe(ClO2)2
6. CuSO4
16. Al(OH)3
7. BrCl3
17. Cr2O3
8. Mn2O5
18. SO2
9. BeCl2
19. KH2PO4
10. N2O5
20. PbCl4
Write formulas for the following compounds:
1. calcium chloride
11. potassium dichromate
2. magnesium carbonate
12. boron trifluoride
3. disulfur pentoxide
13. carbon monoxide
4. iron (II) sulfate
14. platinum (I) chloride
5. nickel (III) nitrate
15. silver nitrate
6. ammonium carbonate
16. cobalt (II) acetate
7. sodium cyanide
17. tin (IV) sulfate
8. lead (II) oxide
18. sodium hypochlorite
9. lithium iodide
19. potassium hydrogen phosphate
10. copper (I) sulfide
20. tungsten (IV) phosphate