ADVANCED CHEMISTRY – Test#1, chapter 7, sections 7.1 & 7.2
Topic: Ionic Bonding
Answer in the space provided.
1. Complete the following table: (20)
Element: # valence e # core e - potassium
Ionic charge: # e lost or gained by atom to form the ion.
State “lost” or “gained” in each case phosphorus barium selenium
2. Name the element in period 4 that has 3 valence electrons. ________________ (1)
3. Draw the electron dot structure of: (6) a. an atom of carbon, b. an atom aluminum, c. an ion of iodine,
4. When the following ions form they follow either the octet rule or the duet rule. Complete the following: (9)
Ion:
Sulfide ion d. an ion of nitrogen.
Written configuration in FULL (1s 2 ….etc) Duet or Octet rule?
...
circle one
Duet or Octet
Sodium ion Duet or Octet
Nitride ion Duet or Octet

5. Based on the information given to you via the periodic table, why would a thallium atom (Z = 81) when changing to its common ion, not follow the duet or octet rule?
Explain in full using written configurations for both the atom and the ion. (6)
Answer:
6. (a). What is meant by the coordination number of an ion in a crystal structure of an ionic compound?
Answer: ________________________________________________________________
_____________________________________________________________________(2)
(b). What is the coordination number for each ion in the following: (6)
(i) Na + in NaCl: ________ (ii) Cl in CsCl: ________ (iii) Ti 4+ in rutile? ________
(iv) Zn in the structure (v) Zn in the structure (vi) Ni in the structure shown below: shown below: shown below:

7. (a) Draw a fully labeled diagram to show the electrolysis of molten sodium chloride.
(b). Below the diagram express what happens chemically at both the anode and
cathode using half equations. State which half reaction is oxidation and which one is reduction.
(a) Diagram: (10)
(Include in your diagram: the electrodes and their charge, all wiring, direction of electron flow, power source, a current meter, container of molten salt, chloride ions and sodium ions and the direction of flow…and labels pointing out all of these details.)
(b) Equations: (6)

8. Consider the combination reaction between strontium and nitrogen.
Write the two REDOX half reactions (label which one is oxidation and which one is
reduction) and then write the overall balanced chemical equation for this chemical reaction. (6)
9. Complete the table of formula units that form between elements shown: (12) fluorine nitrogen carbon iodine sodium indium copper (II)
10. Write the equation (using symbols/formulas) to represent the change from… a. …an atom to ion for cesium: ___________________________ (3) b. …an atom to ion for selenium: ___________________________ (3) c. …an atom to ion for aluminum: d. …an atom to ion for tin (IV):
___________________________ (3)
___________________________ (3)
11. Complete abbreviated noble gas core electron configurations for atoms of: a. germanium (Z = 32), __________________________________________ (4) b. Curium (Z = 96), ______________________________________________ (3)

12. Write the equation (using Lewis dot structures) to represent the change from… a. …an atom to ion for oxygen: _____________________________ (3) b. …an atom to ion for calcium: _____________________________ (3)
13. Use orbital diagrams to show how an atom of potassium may change into its common ion: (3)
14. Draw a BOHR model for:
(a), An ATOM of chlorine,
(4)
(b) An ION of magnesium
(4)

ADV CHEM TEST #2 (SEMESTER #2) re-take opportunity –
Consider each of the 16 compounds/ions and be prepared to provide the information as previously requested on the original test for each based on the “best” possible structure using formal charge
1.
hydrogen sulfide, H
2
S
2.
Iodine trifluoride, IF
3
3.
sulfur trioxide, SO
3
4.
formaldehyde, H
2
CO
5.
hydronium ion, H
3
O +
6.
Xenon difluoride, XeF
2
7.
Nitrogen dioxide, NO
2
8.
Nitrite ion, NO
2
-
9.
Nitrate ion, NO
3
-
10.
Nitronium ion, NO
2
+
11.
Acetylene, C
2
H
2
12.
Cyanide ion, CN -
13.
Phosphate ion, PO
4
3http://www.youtube.com/watch?v=gl4d80g6cow
14.
Sulfur dioxide, SO
2 http://www.youtube.com/watch?v=REugD0mJxPk
15.
Chlorine dioxide, ClO
2 http://www.youtube.com/watch?v=1hrjh7ndHrg
16.
Sulfate ion, SO
4
2http://www.youtube.com/watch?v=lEjQKATnI2A
17.
Sulfur trioxide, SO
3 http://www.youtube.com/watch?v=a-ppp5_qhZY
18.
Cyanate ion, OCN http://www.youtube.com/watch?v=v--mTzZpcWA
The above YouTube references are all useful and hopefully very helpful presentations for your review. In each of these six cases, the final answer is based on the “best” possible answer with respect to formal charge. The previous 12 examples in this list are based on the answers discussed in class (test review, test and practice problems). Please rest assured that I am willing and eager to further explain ALL 18 examples as needed.
You are strongly encouraged to meet with me for extra help either individually or in small groups as you prefer.

The re-take test (total points = 60) will feature 15 multiple-choice questions and FIVE of the above examples (9 points each). The latter 5 questions will have the same format as used in the initial test – see below. The maximum time given to complete this assignment is 50 minutes.
Molecule or ion:
H
2
S a. Lewis Structure: (3) b. The number of bonded pairs of electrons: _________ (1) c. The number of lone pairs of electrons*. _________ (1)
*
Indicate if there are any extra ‘single’ electrons beyond
the loan pair count d. The geometric shape of the species.
Name: _________________________ (1)
Drawing: (1) e. The bond angle(s) of the central atom(s) with adjacent atoms – label on the diagram in answer to d.
(1+)  f. Number of resonance forms: _________ (1)
If no resonance forms, state “NONE”
Scoring of the re-take test:
Since the re-take test is out of 60 points, student scores for the re-take will be multiplied by 96/60 (= 1.6) and the highest of the two scores out of 96 will be entered as the test
#2 score and the lower score will be discarded. Neither test will be curved.

ADV CHEM Test#2 Review Name ___________________________ Section ___
Topics 7.3 and Ch.8 (all)
Answer the following:
1. For each of the following molecules/ions, provide: a.
The Lewis structure following the 4-step process of analysis. b.
The number of bonded pairs of electrons. c.
The number of loan pairs of electrons*. d.
The geometric shape of the species – name and drawing. e.
The bond angles of the central atom(s) with adjacent atoms – label on the diagram in answer to d. f.
Number of resonance forms.
* Indicate if there are any extra ‘single’ electrons beyond the loan pair count.
(i) hydrogen sulfide, H
2
S
(ii) Iodine trifluoride, IF
3
(iii) sulfur trioxide, SO
3
(iv) formaldehyde, H
2
CO
(v) hydronium ion, H
3
O +
2. Indicate how and why the SIX exceptions to the octet rule are different from the norm. The six are: NO, NO
2
, BF
3
, SF
6
, PCl
5
, ClO
2
.
3. Name and sketch the 9 different geometric molecular shapes and provide one example for each shape. ALSO in each case give the bond angles present in each case – all possible angles in each case.
4. Using the tables on pages 177 and 238 state the most probable type of bond found in each and whether or not the molecule is polar:
(i) CBr
4
, (ii) PH
3
, (iii) HCl, (iv) CO (v) CO
2
.
5. Refer to Table 8.4, page 244, and list the characteristics of ionic and covalent compounds then answer the following:
(i). Why are ionic compounds in aqueous solution good conductors of electricity?
(ii). Why do ionic compounds usually have melting points higher than 300˚C
(iii). What is the difference between a molecule and a formula unit?
(iv). What type of bonding would you expect to be found in the following compounds and why?
(a) cobalt (II) chloride? (b) Xenon trioxide, (c) barium iodide.
6. Show how a coordinate covalent bond forms in
(i) an ammonium ion, NH
4
+
.
(ii) a molecule of carbon monoxide.
(iii) the chemical bonding between a boron trifluoride molecule and an ammonia molecule.

ADVANCED CHEMISTRY Test#3, Semester 2: Ch. 9 & 10 5/9/14
Rubric guidelines -- points in brackets:
1. Each entry (the “given” and both the numerator and denominator of each conversion factor) MUST include a #, unit, I.D. (1, 1 /
2
, 1 /
2
)
2. A final answer that is expressed to the correct number of significant figures, includes units, and the I.D. of the substance. (1, 1 /
2
, 1 /
2
)
Question # 1.
1. Calculate the number of hydrogen atoms present in a 82.6 liter sample of ammonia at STP.
Answer: (16 points)
_______________ _______________ _______________ _______________
2. Calculate the mass in grams of a sample of cobaltous chlorite that contains 7.18 x 10 23 formula units of the compound.
Answer: (12 points)
_______________ _______________ _______________

Question # 2.
Name:
Formula:
2
3
2
3
5
2
2
4
2
4
2