Name ___________KEY________________________ Date ______________________ Hour
_____
3rd Quarter Final Review
You should use your notes to do this review. If you do not have the notes go to
http://www.mpsaz.org/westwood/staff/latozzi/chemistry/notes/ to download the notes.
1. An anion and cation bonded together create _______Ionic___________ bonds.
2. Two non-metals that share a pair of electrons create Covalent bonds.
3. How does the atomic radius change as you go across a period from left to right? The radius
decresaes
Down a group? The radius increases
4. How does ionization energy change as you go across a period from left to right? IE increases
Down a group? IE decreass
5. How does electronegativity change as you go across a period from left to right? EN increases
Down a group?EN decreases
6. The modern periodic table is arranged in order by increasing atomic number
7. Which atom has the largest atomic radius Ca, Br, Se, Sr ? Sr
8. How do ions form? Atoms gain or lose electrons
9. Which element has the lowest electron negativity Cs, Ca, F, Cl? Cs
10. How is a cation formed? Metals lose electrons
What charge does it become? +
11. How is an anion formed? Nonmetals gain electrons
What charge does it become? –
12. Each period on the periodic table represents a(n) Energy level
13. List the properties of ionic compounds? Crystalline solids, high melting points, conduct
electricity, brittle solids
14. List the properties of molecular (covalent) compounds? Lower melting points then ionic
compounds, usually gases or liquids, do not conduct electricity
15. Which type of elements conduct electricity (metalloids, non-metals, metals) Metals
16. What type of elements make up ionic compounds?Metal and non metal, or metal and
polyatomic ions or 2 polyatomic ions
17. What type of elements make up molecular(covalent) compounds? 2 nonmetals only
18. What are valance electrons? Electrons in the outer most energy level
19. How do you determine the number of valence electrons an element has?the group number tell
the # of valence electrons
20. What is the octet rule? Elements need 8 electrons in their outer energy level to be stable, or
they want the ECN of a noble gas so atoms gain, lose or share electrons to become stable
21. How does barium obey the octet rule when it forms compounds? It loses 2 electrons
22. How does bromine obey the octet rule when forming a compound? It gains 1 electron
23. What is the charge on a Ca ion?Ca+2
24. What is the charge on a sulfur ion?S-2
25. Most elements on the periodic table are (metalloids, non-metals, metals)metals
26. Where are transition metals located on the periodic table?In the middle
27. Which pair of elements are in the same period?
(Mg, Ba)
( O, Te)
( Na, P)
(Cu, Ag)
28. What type of elements do not conduct electricity? (metalloids, non-metals, metals)
29. Write the formula for the following compounds and identify them as ionic or molecular
a) _____sodium carbonate _________Na2(CO3)_________
b) _____ dinitrogen trisulfide _____N2S3__________
c) _____ ammonium phosphate __(NH4)3(PO4)___________
d) _____ Copper(II) oxide _____CuO____________
e) _____ lead (IV) sulfide _____PbS2____________
f) _____ phosphorus hexafluoride ___PF6________
30. Name the following compounds
a) K2O Potassium oxide
b) FeO Iron(II) oxide
c) SF2 Sulfur difluoride
d) Fe2O3 Iron (III) oxide
e) N3O5 Trinitrogen pentaoxide
f) Na3(PO4) Soduim Phosphate
g) Al2(CO3)3 Aluminum Carbonate
h) (NH4)2CO3 Ammonium carbonate
31. Calculate the molar mass for 30 a –h
a. 94.2 g/mol
e. 122 g/mol
b. 72.0 g/mol
f. 164 g/mol
c. 70.0 g/mol
g. 234.0g/mol
d. 0.0 g/mol
h. 96 g/mol
32. 1 mole of atoms is equal to 6.02 x 1023
33. 1 mole of any gas at STP equals 22.4 liters
34. How many moles are in the following compounds. Show set up and units
a. 137 g NaCl
137.0 g NaCl x
1mole
1
58.5 g NaCl
= 2.34 mol
b) 275 g Ba(NO3)2
275.0 g Ba(CO3)2
1
x
1 mol
= 1.1 mol
261.3 g Ba(CO3)2
35. How many moles of carbon are in 2.9 x 1027 atoms of carbon?
2.9 x 1027 atoms C
1
x
1 mol
6.02 x 1023
=
4.8 x 103 moles
36. How many moles of water are in 8.7 x 1022 molecules of water?
8.7 x 1022 molecules
1
x
1 mol
6.02 x 1023
=
0.14 moles