Name: Polly A. Tomic
Chemistry Review Sheet – Types of Bonds & Ionic Formulas
PART 1: Definitions
1. Ion – an atom that has a positive or negative charge
2. Compound – 2 or more elements that are chemically combined
3. Ionic bond – a bond between a metal and a nonmetal where electrons are transferred from the
metal to the nonmetal
4. Covalent bond – a bond between two nonmetals where electrons are shared
5. Chemical formula – shows the elements that a compound contains and the number of atoms of
each element
6. Polyatomic ion – a charged group of covalently bonded atoms
7. Oxidation number – the charge that an ion has after gaining or losing electrons
PART 2: Periodic Table Information
Element
Symbol
Metal or
Number of
Gain or Lose
Oxidation
Nonmetal
Valence e-
Electrons
Number
Beryllium
Be
Metal
2
Lose
+2
Sulfur
S
Nonmetal
6
Gain
-2
Sodium
Na
Metal
1
Lose
+1
PART 3: Short Answer
8. Why do the Noble Gases not form compounds? Noble gases have a full outer shell, so they have
no unpaired valence electrons with which to bond.
9. Why are elements from the same periodic table group chemically similar? Elements in the same
group (or family) are chemically similar because they have the same number of valence
electrons and bond in similar ways.
10. A binary compound is made of a metal & a nonmetal (in other words, there are no polyatomic
ions).
11. The sum of the oxidation numbers in an ionic compound equals zero (it’s electrically neutral).
12. Why are metals ductile and malleable? Metals are ductile and malleable because they are
composed of metallic cations in a “sea of valence electrons”. These free-floating electrons allow
cations to slide past one another when subjected to pressure or heat.
13. Identify the properties of ionic, covalent and metallic bonds.
ionic bonds – formed between a metal and a nonmetal, electrons are transferred; ionic compounds
have crystalline structures and only conduct electricity in the molten state or in solution.
covalent bonds – formed between two or more nonmetals, electrons are shared; covalent
compounds are brittle and do not conduct electricity in solution.
metallic bonds – bonds using the metal’s “sea of electrons”; metallic compounds are ductile and
malleable; they are good conductors of heat and electricity, regardless of whether they are in
solution.
PART 4: Types of Bond
14. MgSO4
Ionic
15. Cl2O
Covalent
16. FeCl2
Ionic
17. H2O
Covalent
18. AlPO4
Ionic
19. SO3
Covalent
Identify the following as either an ionic or covalent compound.
PART 5: Ionic Formulas
Write the formula for each of the following:
Calcium sulfate
Ammonium chloride
Aluminum sulfate
CaSO4
NH4Cl
Al2(SO4)3
Copper II oxide
Ammonium nitride
Aluminum sulfide
CuO
(NH4)3N
Al2S3
Sodium carbonate
Magnesium Hydroxide
Iron II nitrate
Na2CO3
Mg(OH)2
Fe(NO3)2
PART 6: Naming Ionic Compounds
Name the following ionic compounds.
20. MgCO3
Magnesium Carbonate
21. NH4NO3
Ammonium Nitrate
22. FeCl2
Iron (II) Chloride
23. MgS
Magnesium Sulfide
24. Cu3P
Copper (I) Phosphide
25. Cr(OH)2
Chromium (II) Hydroxide
26. Co(NO3)2
Cobalt (II) Nitrate