1. Chapter 5 Review Game Questions

2. Question #1
Name the following ionic compound: FeN
Iron (III) nitride

3. Question #2 All of the following have a filled valence shell except:
Li+
O-2
Sr+2
P-2 d

4. Question #3
What is the name given to the structure ionic compounds form?
Crystal lattice.

5. Question #4 Name two properties of ionic compounds.
-high melting and boiling points.
-conduct electricity in the liquid state
-hard
-brittle

6. Question #6
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.

7. Question #7
What is the formula for copper (II) fluoride?
CuF2

8. Question #8 What is the name of the ionic compound NH4OH?
ammonium hydroxide

9. Question #9 What is the rule for naming monatomic anions?
the –ide ending is added.

10. Question #10 Which of the following chemical formulas is correct?
a) Al2O3
b) Al3O2
c) AlO
d) Al2O a

11. Question #11
Which of the following compounds does NOT contain a polyatomic ion?
Na2CO3
BaCl2
NH4F
Mn(OH)2
b: Ba+2 Cl-

12. Question #12
What is the chemical formula for manganese (II) carbonate?
MnCO3

13. Question #13
Why can’t ionic compounds conduct electricity in the solid state?
Because the charges can’t move.

14. Question #14 What is the chemical formula for zinc (II) nitrate?
Zn(NO3)2

15. Question #15
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.

16. Question #16 What is the name for the compound AlPO4?
aluminum phosphate

17. Question #17
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.

18. Academic Final Question
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

19. Honors Final Question
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.