Chemistry 2015-2016
Name:
Ions, Ionic Compounds, and Bond Types Review
Date:
Per:
Directions: Answer the following to help you study for your Ionic test on Tuesday, October 20th.
Flame Test
1. Describe how you can predict the color of a chemical when it emits light if you know its chemical
formula.
Groups/Periods
1. What do all elements in a particular group have in common?
2. What do all elements in a particular period have in common?
Electron Shells/Ions
For Sodium – Draw in space to the righ .
1. Draw an electron shell diagram for a neutral Sodium atom.
2. How many valence electrons does it have?
3. How many core electrons?
4. What noble gas does it want to have the stability of?
5. Will it lose or gain electrons to get that stability?
6. Draw the new electron shell diagram for the ion of Sodium.
7. How many of each does it now have?
a. Protons
b. Electrons
8. What is its charge now? Why?
For Sulfur – Draw in space to the right.
1. Draw an electron shell diagram for a neutral Sulfur atom.
2. How many valence electrons does it have?
3. How many core electrons?
4. What noble gas does it want to have the stability of?
5. Will it lose or gain electrons to get that stability?
6. Draw the new electron shell diagram for the ion of Sulfur.
7. How many of each does it now have?
a. Protons
b. Electrons
8. What is its charge now? Why?
9. Define ion, cation, and anion.
Ion Questions
1. Explain why the charge of an atom is determined by the relationship between the number of
protons and the number of electrons.
2. What is a polyatomic ion?
Naming Ionic compounds
Write the name OR the formula for the following.
1. sodium carbonate _____________________
6. calcium sulfate_____________________
2. cobalt II phosphide_____________________
7. lead IV sulfite_____________________
3. zinc I nitrate_____________________
8. Fe2(SO4)3_____________________
4. calcium chloride_____________________
9. CaS_____________________
5. ammonium sulfide_____________________
10. K2CrO4_____________________
11. Ca(OH)2_____________________
14. KOH_____________________
12. (NH4)2S_____________________
15. Pb(SO4)2______________
13. ZnO_____________________
16. ZnCl2___________________
Interpreting Compounds
For the following compounds, list what atoms are present and how many of each atom:
5Cu(NO3)2 (s)
3HNO3 (aq)
2NaNO3 (aq)
Transition Metal Practice
Positive Ion or Negative Ion or Anion
Cation
Chemical Formula
Name
Ni F3
Zn3(AsO4)2
Mn(NO3)3
Iron(III) sulfide
Zirconium (II) bromide
Nickel (III) Chloride
Categorizing Chemicals by their physical properties
1. Define soluble and insoluble:
2. In order to conduct electricity a chemical either has to be
___________________________________________________ or ___________________________________________________
3. A chemical that does not conduct electricity is _______________________________ or a
_____________________________________.
4. Circle the substances that will conduct [note: (s) means solid, (l) means liquid, (g) means gas, and
(aq) means aqueous – dissolved in water]
MgCl2(s)
NH3 (l)
SrF2 (S)
C3H8 (g)
Ca (s)
C12H22O11(S)
Al(NO3)2(aq)
KBr (aq)
RbBr(S)
Pt (s)
S (s)
5. Explain your answers to number 4.
6. Circle the substances that will dissolve.
Pt (s)
KBr (s)
Ag(S)
W(S)
7. Explain your answers to number 6.
MgCl2 (s)
CsCl(S)
S (s)
3 types of bonding
Give the properties of and explain what the electrons are doing in each of the following.
1. Ionic Bonds
2. Molecular Covalent Bonds
3. Metallic Bonds
4. Network Covalent Bonds