1. Unit 4 Review

2. Section 1: Forming Bonds 1) Why are noble gases unreactive?
2) Why do ions form?
3) What is the octet rule? How is it used?
4) Which is more likely to form a compound – Mg or Ne? Why?
5) Why are the halogens and the alkali metals most likely to form ions?
6) How would the following elements achieve stability?
Mg2+_________ O2-___________
C4+/-_________ Na+ __________
I1- __________ Xe _______
They have a full octet
To achieve a stable octet (8 valence electrons)
Atoms will gain/lose or share electrons to get 8 electrons. Used to predict ion formation.
Mg, because it does not have 8 valence electrons.
Because they only need one electron to be stable.
Lose 2 electrons
gain 2 electrons
Gain/ lose 4 electrons
Lose 1 electron
Gain 1 electron
none

3. 9) What is the charge on anions? __________Which
7) As potential energy (energy to react) goes down, stability goes _____________. When atoms complete their valence shell they gain stability and lost their potential energy. These reactions are ____________________________________, meaning they give off energy.
8) What is the charge on cations? ________Which is more likely to form a cation – a metal or a nonmetal? Do cations form by gaining or losing electrons? Would they be smaller or larger than their neutral atom? _____________________________
9) What is the charge on anions? __________Which
is more likely to form a anion – a metal or a
nonmetal? Do anions form by gaining or losing electrons? Would they be smaller or larger
than their neutral atom? ______________________________ up
exothermic
“+”
smaller
“-”
larger

4. 11) Describe how an ionic bond forms between sodium and chlorine.
10) What is an ionic bond?
11) Describe how an ionic bond forms between sodium and chlorine.
12) Why don’t we talk about ionic compounds as individual molecules?
13) What is another name for ionic compounds? ___________________
14) An ionic bond always forms between a __________________ & a _________________.
15) What are the properties of salts? Know what causes each property. 1. 2. 3. 4.
Attraction between a cation and anion
Sodium loses one electron to chlorine; Na+ + Cl- = NaCl
Because we never have individuals – they repeat 1000’s
of times in a crystal lattic
salts
Metal
Nonmetal
Hard and dense
brittle
High melting point
Only conduct when dissolved.

5. NaCN
Sodium cyanide _______________
Aluminum hydroxide ____________
Iron (III) oxide __________________
Titanium (I) sulfide ______________
Magnesium sulfide _____________
Strontium phosphide ____________
Lithium sulfide _________________
Rubidium phosphate ____________
Al (OH)3
Fe2O3
Ti2S
MgS
Sr3P2
Li2S
Rb3PO4

6. Rubidium selenide _____________
Barium iodide _________________
Copper (II) hydroxide____________
Manganese (IV) chloride _________
Strontium acetate ______________
Calcium sulfate _________________
Mercury (I) nitride _______________
Cesium nitride _________________
Rb2Se
BaI2
Cu(OH)2
MnCl4
Sr(C2H3O2)2
CaSO4
Hg3N
Cs3N

7. CaCl2 ____________________________ AgCl ____________________________
calcium chloride
CaCl2 ____________________________
AgCl ____________________________
K2S _____________________________
CuO ____________________________
Ba3N2 ____________________________
FeN _____________________________
MgBr2 ___________________________
Fe3N2 ____________________________
silver chloride
potassium sulfide
copper (II) oxide
barium nitride
iron (III) nitride
magnesium bromide
iron (II) nitride

8. ammonium chloride
NH4Cl ____________________________
AlPO4 ____________________________
LiNO2 ___________________________
Cs2SO3 __________________________
FeCl3 ____________________________
Cu2O____________________________
Ti2O _____________________________
Fe(NO2)2__________________________
aluminum phosphate
lithium nitrite
cesium sulfite
iron (III) chloride
copper (I) oxide
titanium (I) oxide
iron (II) nitrite

9. Metals are not ionic but DO share many properties with ionic compounds.
Name one similarity and one difference between ionic and metallic bonding.
Describe the electron sea model of metallic bonding & draw a picture.
What physical properties does the electron sea model give metallic bonds?
Similarity: attraction between positive and negative ions
Difference: metals are malleable and ionics are brittle
Positive metal cations have lost electrons to the “sea”
Malleable and ductile
Conductors
Lustrous

10. 19. What is an alloy? Give two examples.
20. What characteristic of metallic bonds enable them to conduct electricity?
Any Mixture of metals Ex: Steel- Mix of iron and carbon
Delocalized electrons are free to move which is how electricity is transferred
A mixture of metals
Example: steel = mix of iron and carbon