Chemistry 2015-2016Name:
Ions, Ionic Compounds, and Bond Types ReviewDate: Per:
Directions: Answer the following to help you study for your Ionic test on Tuesday, October 20th.
Flame Test
- 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 .
- Draw an electron shell diagram for a neutral Sodium atom.
- How many valence electrons does it have?
- How many core electrons?
- What noble gas does it want to have the stability of?
- Will it lose or gain electrons to get that stability?
- Draw the new electron shell diagram for theion of Sodium.
- How many of each does it now have?
- Protons
- Electrons
- What is its charge now? Why?
For Sulfur – Draw in space to the right.
- Draw an electron shell diagramfor a neutral Sulfur atom.
- How many valence electrons does it have?
- How many core electrons?
- What noble gas does it want to have the stability of?
- Will it lose or gain electrons to get that stability?
- Draw the new electron shell diagram for the ion of Sulfur.
- How many of each does it now have?
- Protons
- Electrons
- What is its charge now? Why?
- Define ion, cation, and anion.
Ion Questions
- Explain why the charge of an atom is determined by the relationship between the number of protons and the number of electrons.
- What is a polyatomic ion?
Naming Ionic compounds
Write the name OR the formula for the following.
1. sodium carbonate ______
2. cobalt II phosphide______
3. zinc I nitrate______
4. calcium chloride______
5. ammonium sulfide______
6. calcium sulfate______
7. lead IV sulfite______
8. Fe2(SO4)3______
9. CaS______
10. K2CrO4______
11. Ca(OH)2______
12. (NH4)2S______
13. ZnO______
14. KOH______
15. Pb(SO4)2______
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 orCation / Negative Ion or Anion / 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
- Define soluble and insoluble:
- In order to conduct electricity a chemical either has to be
______or ______
- A chemical that does not conduct electricity is ______or a
______.
- 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)
C3H8 (g)
Al(NO3)2(aq)
Pt (s)
NH3 (l)
Ca (s)
KBr (aq)
S (s)
SrF2(S)
C12H22O11(S)
RbBr(S)
- Explain your answers to number 4.
- Circle the substances that will dissolve.
Pt (s)KBr (s)MgCl2 (s)S (s)
Ag(S)W(S)CsCl(S)
- Explain your answers to number 6.
3 types of bonding
Give the properties of and explain what the electrons are doing in each of the following.
- Ionic Bonds
- Molecular Covalent Bonds
- Metallic Bonds
- Network Covalent Bonds