Transcript Chapter 3 Review Questions

Name the following ionic compound: FeN

Iron (III) nitride

All of the following have a filled valence
shell except:
Li+
b. O-2
c. Sr+2
d. P-2
a.
d

What is the name given to the structure
ionic compounds form?
Crystal lattice.

Name two properties of ionic
compounds.
-high melting and boiling points.
-conduct electricity in the liquid state
-hard
-brittle

When ions are formed, are the identities
of the atoms changed? Why or why not?
No because the number of protons
(atomic number) is staying the same,
which dictates the identity of the atom.
Only the electrons are changing.

What is the formula for copper (II)
fluoride?
CuF2

What is the name of the ionic compound
NH4OH?
ammonium hydroxide

What is the rule for naming monatomic
anions?
the –ide ending is added.

Which of the following chemical formulas
is correct?
a) Al2O3
b) Al3O2
c) AlO
d) Al2O
a

a)
b)
c)
d)
Which of the following compounds does
NOT contain a polyatomic ion?
Na2CO3
BaCl2
NH4F
Mn(OH)2
b: Ba+2 Cl-

What is the chemical formula for
manganese (II) carbonate?
MnCO3

Why can’t ionic compounds conduct
electricity in the solid state?
Because the charges can’t move.

What is the chemical formula for zinc (II)
nitrate?
Zn(NO3)2

Does the electron configuration shown
below represent a stable atom/ion?
1s22s22p63s23p4
No because there are only 6 valence
electrons and it needs 8 to be stable.

What is the name for the compound
AlPO4?
aluminum phosphate

Compound A has a melting point of
425°C and Compound B has a melting
point of 649°C. Which would you
expect to have a larger lattice energy?
Compound B because a higher melting
point indicates ions are held more tightly
together, and are more stable.

Use the following elements to develop a
feasible ionic compound AND give the
charges for each ion: Fe and O.
Fe+2 or Fe+3 and O-2
 FeO or Fe2O3

Trends can be seen in the periodic table
for lattice energy. In general, this trend is
opposite to the trend seen for atomic
radius. Lattice energies tend to increase
across a period and decrease down a
group. Explain why this trend occurs.