Ionic Solids Characteristics
Formed from
a bond
between
a metal
and
nonmetal
Ionic Solids
Strong
Electrostatic
Attractions
Rigid
crystalline
structure
Conductivity
Relatively High
Melting Point
Yes
No
In
the solid
phase
Hard,
brittle
solids
In
the molten
or aqueous
phase
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
#5 Which electron-dot diagram
represents H2?
Both hydrogen’s
will equally
share their
valence
electron
H H
H H
#9) In which compound do the atoms have
the greatest difference in electronegativity?
(1) NaBr
|0.9 – 3.0| = 2.1
(2) AlCl3
|1.6 – 3.2| = 1.6
(3) KF
|0.8 – 4.0| = 3.2
(4) LiI
|1.0 – 2.7| = 1.7
#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
+2
-1
M (OH)
So the Metal (M) must be from Group 2 because of its +2 oxidation state!
#16) Element X has an electron configuration of
2-8-3. 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
+3
X (PO4)
-3
Criss
Cross w/out
charges
X3(PO4)3
3
Reduce
to
Lowest
Ratio
X (PO4)
3
From Table
E:
phosphate
has a -3
#33
a.
H H
b.
H H
c. 1 Mg +
H2 is nonpolar and H2O is polar, like
dissolves like, therefore H2 will not
dissolve in H2O.
1 H2SO4  1 H2 + 1 MgSO4
#34
a.
HNH
H
b.
H
HNH
H
+
#35
a.
b.
H Cl
+
H Cl
c. H-Cl is polar, water is polar; like dissolves
like
#36
a.
N N
OR
N N
b. N2 is very stable, unreactive because of triple
bond (a lot of energy was released when this
bond was formed).
#6) Group 1 metals are highly reactive and form stable
compounds.
#7) Na 1s22s22p63s1
Will become
[Na]+1
Na
Cl 1s22s22p63s23p5
Cl
1s22s22p6 Ne
Will become
1s22s22p63s23p6 Ar
Cl
-1
#8. Radon is a group 2 (metal), it wants to lose its 2
valence electrons to a nonmetal.
1) Iodine – nonmetal, wants to gain 1 e2) Fluorine – nonmetal, wants to gain 1 e3) sodium – metal, wants to lose 1 e4) calcium – metal, wants to lose 2 eOf the 2 choices that want electrons choice 2 is
more reactive, larger electronegativity, than
choice 1. Fluorine is the answer (choice 2).
#10) Which compound would most likely
have the greatest ionic character?
(1) CO
|2.6 – 3.5| = 0.9
(2) KF
|0.8 – 4.0| = 3.2
(3) CaO
|1.0 – 3.5| = 2.5
(4) LiH
|1.0 – 2.1| = 1.1
#11) Given the reaction
H2 + Cl2 → 2HCl
• Bond Breaking requires/absorbs energy.
• Bond Formation releases/emits energy.
The H2 and Cl2 bonds are broken – requires energy!
The HCl bond is formed- releases energy!
 The answer is choice (4) the forming of the HCl
bond releases energy
#12) Noble gases have the most stable
electron configuration, choice 1 (Ne).
#14) In order for the electrons to have been
transferred to Oxygen, the oxygen will
have to be the most electronegative
element and the ionic character of the
compound would be 1.7 or greater.
(1) CO2
(2) N2O
|2.6 – 3.5| = 0.9
|3.0 – 3.5| = 0.5
(2) NO2
|3.0 – 3.5| = 0.5
(4) Na2O
|0.9 – 3.5| = 2.6
15) Compounds including polyatomic ions have
covalent bonding within and ionic bonding to the
metal outside the parenthesis (brackets).
2-
Ca
2+
O
O SO
O