1. Ionic Solids Characteristics
Formed from
a bond
between
a metal
and
nonmetal
Ionic Solids
Strong
Electrostatic
Attractions In
the molten
or aqueous
phase
Conductivity
the solid No
Yes
Rigid
crystalline
structure
Relatively High
Melting Point
Hard,
brittle
solids

2. The First Couple
# 1) Energy is released when bonds are formed. Energy is absorbed when bonds are broken.
#2) As a bond forms the PE decreases.
#3) Energy is released -> stability increases
#4) Two atoms combine to form a molecule, bond formed, energy is released

3. #5 Which electron-dot diagram represents H2?
Both hydrogen’s will equally share their valence electron H H H

4. #9) In which compound do the atoms have the greatest difference in electronegativity?
NaBr
|0.9 – 3.0| = 2.1 KF
|0.8 – 4.0| = 3.2
AlCl3
|1.6 – 3.2| = 1.6
LiI
|1.0 – 2.7| = 1.7

5. #13) Given the reaction: M + 2H2O -> M(OH)2 + H2 The metal represented by M is most likely a metal from Group
The subscript of 2 on the hydroxide came from the charge on the metal (M).
M(OH)2
M+2(OH)-1
So the Metal (M) must be from Group 2 because of its +2 oxidation state!

6. #16) Element X has an electron configuration of 2-8-3
#16) Element X has an electron configuration of This element will combine with the phosphate ion to form a compound with the formula
3 Valence e-’s means that is will have an oxidation state of +3
X+3(PO4)-3
From Table E: phosphate has a -3
Criss
Cross w/out
charges
X3(PO4)3 3 3
Reduce to
Lowest
Ratio
X (PO4)

7. #33 a. b. c. H
H2 is nonpolar and H2O is polar, like dissolves like, therefore H2 will not dissolve in H2O. H
1 Mg H2SO4  1 H2 + 1 MgSO4

8. #34 + H H N H
a b. H H N H H

9. #35 H Cl a. b.
c. H-Cl is polar, water is polar; like dissolves like H Cl +

10. #36 N N a. OR
b. N2 is very stable, unreactive because of triple bond (a lot of energy was released when this bond was formed). N N