1. White board review - RULES
1. Work as teams. Score pts. as teams. If you score more than 15pts, the rest are bonus pts.
2. All team members MUST prepare a response for the class.
3. One team will present their response & reasons for their response.
4. ‘Audience teams will draw an affirmative (thumbs up) OR dissenting (thumbs down).

2. What are the three subatomic particles and their charges?
Question #1
What are the three subatomic particles and their charges?

3. A. Where are the protons & neutrons found in the atomic structure?
Question #2
A. Where are the protons & neutrons found in the atomic structure?
B. Where are the electrons found in the atomic structure?

4. write the Lewis dot structure Why does it have a specific # of dots?
Question #3
For silicon
write the Lewis dot structure
Why does it have a specific # of dots?

5. Question #4 Will Si gain or lose electrons? How many? Why?
What is the ion symbol for Si ? _______

6. A. What is the difference between Helium nuclei (52He) and (42He) ?
Question #5
A. What is the difference between
Helium nuclei (52He) and (42He) ?
B) Look at your periodic table. Circle the most common isotope above.

7. Where does all chemical bonding take place?
Question #6
Where does all chemical bonding take place?
(nucleus or electron cloud)
Explain--

8. Question #7 Draw the electron configuration for argon.
How many electrons does it gain or lose to become stable? (explain)

9. Question #8
1. List 3 properties of
Ionic compounds
Covalent compounds

10. Shifting to periodic table questions ---- Question #9
All elements on the periodic table are arranged by their ___________ number.
This number tells us how many _________
(the element has)

11. On the periodic table, the horizontal rows are called________?
Question # 10
On the periodic table, the horizontal rows are called________?
On the periodic table, the vertical columns are called________ or _________?

12. Question # 11
What family of elements is so stable that these elements do not gain or lose electrons?
Why?

13. Question #12
Look at your periodic table. Describe where the Metals and Non-metals located?
What separates the metal elements from the non- metal elements on the periodic table?

14. The av. atomic mass of silver is 107.87 amu’s.
Question #13
The av. atomic mass of silver is amu’s.
What is silver’s mass number?
Why is there a difference?

15. Use the atomic symbol to determine the number of P+ , No , e-
Question #14
Use the atomic symbol to determine the number of
P+ , No , e-
P=___ N=___ e=___ K 19

16. Use the atomic symbol to determine the number of P+ , No , e-
Question #15
Use the atomic symbol to determine the number of
P+ , No , e-
P=___ N=___ e=___ N 7

17. Question #16
Refer to your electronegativity (orange sheet). Show work to support your ans.
What type of bond forms between the elements H and F
Are the bonding electrons equally shared between the H atom and the F atom?

18. Question #17 Draw the Lewis dot structure for O2 .
(leave your dot structure on your board)
How do you know your structure is correct?

19. Question #18 Draw the “structural formula” for O2
What is the difference in the information that a Lewis dot structure shows and a structural formula?

20. How do you know how many electrons the metal will lose?
Question # 19
How do you know how many electrons the metal will lose?
How do you know how many electrons the non-metal will gain?

21. What charged ion will form from the following atoms:
Question #20
What charged ion will form from the following atoms:
atoms  ions
Rb  Be
N  S
He

22. What is the name for these type I ions? ion  (name) Ca2+ Al3+ F1- P3-
Question #21
What is the name for these type I ions? ion  (name)
Ca2+ Al3+
F P3-

23. What is the name for these type II ions? ion  (name) Fe2+ Co3+
Question #22
What is the name for these type II ions? ion  (name)
Fe2+ Co3+
Fe3+ Cu1+

24. Write the formulas for these ionic compounds: name (formula)
Question #23
Write the formulas for these ionic compounds: name (formula)
Copper (I) sulfide 
Lead (IV) oxide 

25. Write the formulas for these ionic compounds: name (formula)
Question #24
Write the formulas for these ionic compounds: name (formula)
Zinc phosphide 
Sodium oxide 

26. How many atoms are in these ion symbols? Fe2+ = Co3+ = S2- = CO31+ =
Question #25
How many atoms are in these ion symbols?
Fe2+ = Co3+ =
S2- = CO31+ =

27. Write the formulas for these ionic compounds: name (formula)
Question #26
Write the formulas for these ionic compounds: name (formula)
Strontium hydroxide 
Tin (II) sulfite 
Potassium phosphate 

28. What are the names of these polyatomic ions? Ion (name)
Question #27
What are the names of these polyatomic ions? Ion (name)
NO31-  NO21- 
CO32-  NH41+ 
SO42-  OH1- 

29. Name the following ionic compounds: formula  (name) CaCl2  Al2O3 
Question #28
Name the following ionic compounds: formula  (name)
CaCl2 
Al2O3 

30. Write the formulas for these ionic compounds: name (formula)
Question #29
Write the formulas for these ionic compounds: name (formula)
Copper (I) sulfate 
Lead (IV) nitrate 

31. Write the formulas for these ionic compounds: name (formula)
Question #30
Write the formulas for these ionic compounds: name (formula)
Iron (II) bromate 
Mercury (I) phosphate 

32. END OF THE REVIEW
I will up-load these questions to the website under (presentations) if you want to look at them again before the test.
Now discuss with the person next to you what you will put on your 3x5 card and if you need to add anything to your periodic table.

34. All non-metals’ names end with what 3 letters?
Question #27
All non-metals’ names end with what 3 letters?

35. Look at your reference list of polyatomic ions.
Question #29
Look at your reference list of polyatomic ions.
What last 3 letters do (most) their names end with? (give two common endings)

36. Name the following ionic compounds: formula  (name) CuF2  Hg2O 
Question #35
Name the following ionic compounds: formula  (name)
CuF2 
Hg2O 

37. Name the following ionic compounds: formula  (name) CsNO2 
Question #36
Name the following ionic compounds: formula  (name)
CsNO2 
Ca(NO3)2 

38. Name the following ionic compound: formula  (name)
Question #37
Name the following ionic compound: formula  (name)
(NH4)3PO4 

41. Fill out your personal assessment !
Hand in your assessment.
Start on (criss-cross) homework worksheet.

42. Most of the polyatomic ions are negatively charged.
Question #26
Most of the polyatomic ions are negatively charged.
What polyatomic ion is positively charged? (give symbol & name)

43. Silver’s av. atomic mass = 107.87 amu’s
Question #15
Silver’s av. atomic mass = amu’s
Silver’s mass number is 108 amu’s
Why is there a difference?

44. How many valence electrons does Calcium (Ca) have?
Question #18
How many valence electrons does Calcium (Ca) have?
What noble gas does it want to be like? (its equiv. noble gas)

45. All metals will lose valence _________ and become ________ charged.
Question #19
All metals will lose valence _________ and
become ________ charged.
All non-metals will gain valence _________ and