Criteria for Assessment 1– Applying Theory to a Case Study – A.docx

Criteria for Assessment 1– Applying Theory to a Case Study –
A Critique (1500 words)- 20%
Student ____________________________________ Student
Number _________________________________
Assessment Criteria
Content- (7
Points)
Exemplary Met Poor/Unmet Score
Understanding
of key principles
and concepts of
theory (ies)
Demonstrates understanding of all
the critical principles and concepts of
theory employed in case study (4)
Demonstrates understanding of some
of the key principles and concepts of
theory employed in case study (2 -3)
Insufficiently identifies the key
principles and concepts of theory
employed in case study (0-1pt)
Application of

theory to
explaining
problem,
behaviour
and/or
offending.
Identifies the salient arguments and
fully describes how the theoretical
concepts are used to explain the type
of offending or behaviour contained
in case study (3)
Identifies some of the salient
arguments and partially describes
how the theoretical concepts are used
to explain the type of offending or
behaviour contained in case study
(1.5-2)
Insufficiently describes the salient
arguments or describes how the
theoretical concepts are used to
explain the type of offending or
behaviour contained in case study (0-
1 pt)
Analysis (7 Ps)
Critical appraisal
of the strengths
and limitations
of theory and its
application

Well referenced from the case study,
analysis clearly sets out the strengths
and limitations of the theory, its
application and the empirical
evidence presented with respect to
the defined problem.
(4)
With some references to case study,
analysis addresses some strengths or
limitations of the application of the
theory, its application and the
empirical evidence presented with
respect to the defined problem . (2-3 )
Does not adequately analyse the
application strengths or limitations of
the theory and the empirical evidence
and/or fails to provide relevant
references from the case study. (0-
1pt)
Analyses ideas
and evidence
and implications
for public policy
and/or further
research
Integrates results of analysis to draw
conclusions about implications for
public policy and further research. (3-
3)
Conclusions are drawn with some

reference to critical analysis. This may
include public policy and/or further
research. (1.5-2)
Conclusions are drawn without
effective reference to critical analysis
and/or implications are not well
developed. (0-1pt)
Presentation: (6 Exemplary Met Poor/Unmet Score
Points)
Clear and
effective
structure which
responds to the
task
Responses to each criteria are
distinct, clearly delineated. Writing is
well structured with effective
transitions with introduction and
conclusion. (2)
Responses to criteria can be
identified, but may be incomplete or
are not clearly differentiated. Writing
has generally adequate structure. (1)
Responses to the essential criteria are
unclear or incomplete, Poor structure
leads to poor readability.

(.5-0 pts)
Complete and
appropriate
referencing
Complete referencing to APA
standard
(1.5)
Referencing generally complete with
some inconsistencies or errors (1)
Referencing incomplete and / or
incorrect. (.5-0 pts)
Clarity in writing
with due regard
to rules of
grammar and
spelling.
The writing is essentially error free
with respect to rules of grammar and
spelling. (1.5)
Writing follows normal rules with
some errors in spelling and/or
grammar. (1)
Writing contains numerous errors in
spelling and grammar that interfere
with readability. (.5-0 pts)

Student Reflection – 1 pt
Last Name: ID # # on the signature list:
First Name: (to be entered by the teacher)
Professor: Dr. G. DÉNÈS
Chem242-FE.W2011
CHEMISTRY 242/4 -51 Winter 2011
Final Examination Thursday April 21, 2011
Total number of pages: 24 19:00-22:00
*****************************************************
********************************
Enter your name and your Concordia ID number on the top of
this page, in the space
provided, and your Concordia ID number on the top of each
subsequent page, in the space
provided.
Answer all questions on this questionnaire. Balance all
equations.
Explain your answers, starting from the periodic table,

whenever possible.
Examination time: 6:00 - 7:00pm
No booklet
No book, note or periodical table allowed.
No scrap paper allowed. Use the back of the questionnaire
sheets for scrap.
Printed translation dictionaries are allowed.
No scientific, technical, definition, or electronic dictionary is
allowed
This final examination counts for 50 marks, out of a total of 100
marks.
If you do better in % in the final exam than in the midterm
exam, the midterm exam will not count and the
final exam will count for 75% instead of 50%.
When the question asks to compare values, such as distances,
radii, energies, etc..., you are expected to tell
whether numbers are larger, smaller, or about the same, and
explain why if an explanation is requested. No
numerical value is expected, unless requested.
This exam is made of two parts:
- Part I requires only short answers
- Part II requires full explanations
Answer all questions in the space provided on the questionnaire.
You can use the back of the
pages for scrap if you wish; it will not be graded.
1

Chem 242, Winter 2011, Final examination Your ID #
Part I starts here. Give only short answers in the space
provided. No explanation
required unless requested.
1: Give the name of the scientists who did the following:
- designed a method to determine the electron pair geometry and
molecular shape by evaluating
repulsion between electron :
- designed a rule to show the variation of health response of
nutrient with intake dose:
- determined the maximum number of electrons that can be
contained in an orbital :
- determined the electroneutrality rule that allows to evaluate
which of several non-equivalent Lewis
structures represent best a molecule or polyatomic ion:

- designed the most used scale of electronegativity, that has 4.0
for F and 0.7 for Fr:
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2: Draw the electron dot diagram of the cyanide CN- ion (no
explanation required):
and answer the following questions regarding it:
- Formal charge on C: - Formal charge on N:
- Oxidation number on C: - Oxidation number on N:
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2

3: Give the valence electronic structure of the element
located in group 16, period 5:
Give the symbol and name of the same element:
Give the expected oxidation number(s) of the same element:
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4: Give the type of all interatomic interactions that exist in
liquid NH3 (anhydrous) and what they are
responsible for.
I nteraction type Responsible for

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3
5: Compare qualitatively (using the sign < and the ions
symbol) the ionic radius of the ion obtained when
Se, Br, Rb and Sr achieve the nearest noble gas configuration.
Explain in 2 or 3 lines only.
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6: Circle the letter a, or b, or c, or... for the answer that

applies best to the properties of most ionic
compounds in the given conditions in each question below:
6.1 At ambient temperature, most ionic compounds are:
a. Hard and brittle
b. Hard but not brittle
c. Soft
d. Malleable
e. Ductile
a. Good electrical conductors
b. Semiconductors
c. Insulators
a. Gases
b. Liquids
c. Low melting point solids
d. High melting point solids
4

6.4 At ambient temperature:
a. Most ionic compounds dissolve in non-polar solvents and the
solution does not
conduct electricity.
b. Most ionic compounds dissolve in non-polar solvents and the
solution conducts
electricity.
c. All ionic compounds dissolve in high polarity solvents and
the solution does not
d. All ionic compounds dissolve in high polarity solvents and
the solution conducts
electricity.
e. Only some ionic compounds dissolve in high polarity
solvents and for those that
dissolve the solution does not conduct electricity.
f. Only some ionic compounds dissolve in high polarity solvents
and for those that
dissolve the solution conducts electricity.
6.5 When heated to the molten state in a non-reactive
atmosphere, most ionic compounds behave as
follows:

a. They decompose.
b. They do not decompose and they conduct electricity.
c. They do not decompose and they do not conduct electricity.
6.6 Find the incorrect statement.
a. Ionic compounds cannot be composed of only non-metals
b. Ionic compounds can be made of metals and non-metals.
c. Ionic compounds cannot be made of metals only.
d. An ionic bond is extreme case of a polar bond.
e. A small and highly charged cation can make covalent a bond
that would otherwise be
ionic
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5

7: The combustion reaction of hydrogen in oxygen to give
hydrogen peroxide has a negative Gibbs free
energy.
7.1 Write the balance equation for the above reaction.
7.2 However, the above reaction does not take place. Write
the balanced equation for the combustion
reaction of hydrogen in oxygen that actually takes place.
7.3 Compare qualitatively the Gibbs free energy of the
reaction that actually takes to that of the reaction
that gives hydrogen peroxide.
7.4 Using the position of oxygen in the periodic table,
justify why the compound obtained by combustion
of hydrogen in oxygen is the compound shown in your answer
to question 7.2, rather than hydrogen peroxide.
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********************************
8. Fill in the missing word in the following sentences:
8.1 A semiconductor not doped with impurity is called an
semiconductor.
8.2 The theory that explains bonding and the electrical
properties of metals based on the presence of a very
large number of molecular orbitals very close to one another to
form a continuum is called the
theory.
6
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9. Answer the following questions regarding the bcc structure
of a metal:
9.1 Tell what bcc stands for:
9.2 Tell what is the radius of a metal atom versus the bcc
unit-cell edge a:

9.3 Tell how many number of metal atoms there are in a bcc
unit-cell:
9.4 Tell what is the coordination number of each metal atom
in a bcc unit-cell:
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********************************
10: Answer the following questions about acids and bases.
10.1 An acid stronger than 100% sulfuric acid is called a
.
10.2 Magic acid is made of
.
10.3 Magic acid is used in the petroleum industry for
breaking bonds between
and .
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********************************

7
11. Complete and balance the following reactions of hydrogen:
11.1 CuO(s) + H2(g) 6
11.2 H2C = CH2(g) + H2(g) 6
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12. Answer the following questions about ionic hydrides:
12.1 They contain hydrogen in the following form (circle
your answer):
H H2 H+ H-

12.2 In addition to hydrogen, they contain one of the
following element:
a. An alkali metal or an alkaline earth metal
b. A transition metal
c. A metalloid
d. A non-metal
8
12.3 Their structure is:

a. Similar to the metal, with similar electrical and magnetic
properties
b. Molecular
c. Similar to a halide salt
d. Polymeric
12.4 Choose the correct statement about their structure:
a. At ambient temperature, they are gases, liquids or soft solids
b. They melt at high temperature to give stable electrically non-
conducting melts
c. They melt at high temperature to give stable electrically
conducting melts
d. They decompose at high temperature, on melting or before.
12.5 Choose the correct statement about their reactivity with
moisture:
a. They do not react with moisture

b. They react with moisture to give an acid and hydrogen gas
c. They react with moisture to give a base and hydrogen gas
d. They react with moisture to give hydrogen gas only
e. They react with moisture to give ammonia.
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9
13. Circle the following species that have an octahedral
molecular geometry:

[BrF6]- [AsF6]- [SnF6]- XeF6
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14. Answer the following questions about the electrolysis of
sodium chloride to produce sodium metal.
14.1 Tell what is the physical form of the sodium chloride
electrolyzed:
14.2 Tell what electrode produces sodium:
14.3 Tell what is produced at the other electrode:
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15. Circle in the following list the mixed-oxidation state
compounds:
PbO PbO2 Pb2O3 Pb3O4 In2O3 InO

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10
16. Comparing group 1 and group 11 elements:
16.1 Give the list of the elements of group 11 and their
electronic structure.
16 .2 Compare the reactivity of group 1 and group 11
elements with water, and use their electronic
structure to explain the similarities/differences.

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********************************
17. Beryllium oxide dissolves in both acids and bases.
17.1 This ability to dissolve in both acids or bases has two
names. Give the two names:
11
17.2 Write the two balanced reactions:

17.3 The name of the beryllium ion obtained in an acid is
.
The name of the beryllium ion obtained in a base is
.
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18. The shortest mercury-mercury distance in Hg2F2 is 2.51 Å.
Given that the ionic radius of the fluoride ion is 1.17 Å and that
of the chloride ion is 1.67 Å, estimate the
shortest mercury-mercury distance in Hg2Cl2. Justify your
answer.
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*********************************

19. The molecular formula of B(OH)3 is also written H3BO3.
19.1 Draw the molecule and show the polarity of the most
polar bonds only.
12
19.2 Give the name of the compound:
19.3 Choose the correct answer in the following list:
a. B(OH)3 is a weak base
b. B(OH)3 is a strong base
c. B(OH)3 is a weak acid

d. B(OH)3 is a strong acid
e. B(OH)3 is neither an acid nor a base
19.4 Give the molecular geometry of the B(OH)3 molecule:
19.5 Give the hybridization of boron in the B(OH)3
molecule:
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20. Positive oxidation states of group 14 elements:
20.1 Give the two positive oxidation states of group 14
elements and the trend within the group in terms of
their stability.
13

20.2 In one of their oxidation states, there is a lone pair, that
can be stereoactive or non-stereoactive.
20.2.1 Explain in a few lines, using a drawing for each,
what is a stereoactive lone pair and what is a non
-stereoactive lone pair:
20.2.2 Give the difference between a stereoactive lone pair
and a non -stereoactive lone pair in terms of
the following:
a. Orbital hybridization:

b. Bonding:
c. Coordination number:
d. Regularity/distortions of the polyhedron of coordination:
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********************************
14
21. Dinitrogen monoxide, also called laughing gas, is a
dissymmetric molecule
21.1 Give its formula:
21.2 Draw all its Lewis structures and write the formal

charge of each atom above, in each Lewis structure:
21.3 Tell which of the Lewis structures is best representative
of bonding in dinitrogen monoxide, and give
the name and inventor of the law used to make this prediction:
21.4 Give the hybridization of the central atom:
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22. Compare oxygen to the rest of its group in terms of the
following:
22.1 Physical state:

15
22.2 Catenation (also define catenation):
22.3 Bond stability versus bond order, with a short
explanation:

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24. Group 17 elements:
24.1 Give the name of group 17:
24.2 Given the relative electronegativities of oxygen and
fluorine, answer the following with a short
explanation (no more than two lines each):
16
a. Tell which of oxygen or fluorine should bring out the
highest oxidation state of xenon, according
to their electronegativity:

b. The highest stable oxidation state compounds of xenon
obtained with oxygen and fluorine are
XeO4 and XeF6, respectively. Tell why.
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17
C hem 242, Winter 2011, Final examination Your ID #
Part II starts here. Give your answers in the space provided.
Detailed explanation required
25: Copper(I) chloride crystallizes in the fcc lattice, with
the following ionic positions: metal ions
in 0 0 0 and anions in 1/4 1/4 1/4 . The length of the edge of
the unit-cell of copper(I) chloride is
5.416 Å.
25.1. Give the chemical formula of copper(I) chloride:
25.2. Tell what fcc means:
25.3. Give the list of lattice translations present in a fcc
lattice:

25.4. Derive the list of all copper and chloride ions contained
in the unit-cell (show calculation):
18
25.5. Draw a three-dimensional picture of the unit-cell and
place all the ions inside;

25.6. Draw an appropriate projection of the unit-cell and
place all the ions inside and give their
height;

19
25.7. Determine the number of each kind of ions in the unit-
cell (explain);
25.8. Check that the stoichiometry of the unit-cell is in
agreement with that of the compound
formula;

25.9. Determine the number of unit formulas in the unit-cell;
show the formula used;
20
25.10. On the above projection, draw all the bonds for one
Cu, and the same for one Cl, showing
the three-dimensionality of the coordination of each ion.
Use the figure to give the coordination number and shape of the
polyhedron of coordination for

both ions.
25.11. Show on the figure one of each of the nearest Cu-Cu,
Cl-Cl, and Cu-Cl distances and
determine their numerical values. Show the detail of the
calculations.

21

22

24
Last Name: ID # # on the signature list:
First Name: (to be entered by the teacher)
Professor: Dr. G. DÉNÈS
Chem242-FE.W2012
CHEMISTRY 242/4 -51 Winter 2011
Final Examination Thursday April 16, 2012
Total number of pages: 26 14:00-17:00
*****************************************************
********************************
Enter your name and your Concordia ID number on the top of
this page, in the space
provided, and your Concordia ID number on the top of each

subsequent page, in the space
provided.
Answer all questions on this questionnaire. Balance all
equations.
Explain your answers, starting from the periodic table,
whenever possible.
No booklet
No book, note or periodical table allowed.
No scrap paper allowed. Use the back of the questionnaire
sheets for scrap.
Printed translation dictionaries are allowed.
No scientific, technical, definition, or electronic dictionary is
allowed
This final examination counts for 50 marks, out of a total of 100
marks.
If you do better in % in the final exam than in the midterm
exam, the midterm exam will not count and the
final exam will count for 75% instead of 50%.
When the question asks to compare values, such as distances,
radii, energies, etc..., you are expected to tell
whether numbers are larger, smaller, or about the same, and
explain why if an explanation is requested. No
numerical value is expected, unless requested.
This exam is made of two parts:
- Part I requires only short answers
- Part II requires full explanations
Answer all questions in the space provided on the questionnaire.
You can use the back of the
pages for scrap if you wish; it will not be graded.

1
Part I starts here. Give only short answers in the space
provided. No explanation
required unless requested.
1: Give the name of the scientists who did the following:
- designed a method to determine the electron pair geometry and
molecular shape by evaluating
repulsion between electron :
- designed a rule to show the variation of health response of
nutrient with intake dose:
- determined the electron distribution and the electron spin
within a set of degenerate orbitals :

- established the most commonly used electronegativity scale
that assigns a 4.0 electronegativity to the
most electronegative element :
- established rules to explain the polarization of some ions:
2:
2.1. Draw the electron dot diagram of the [IF4]- ion (no
explanation required):
2
2.2. Answer the following questions regarding the [IF4]- ion :

- Formal charge on I: - Formal charge on F:
- Oxidation number on I: - Oxidation number on F:
2.3. The formal charges found above violate a rule. Give the
following about the rule that is violated:
- name of the inventor of the rule:
- name of the rule:
- tell in 2 or 3 lines what the rule says regarding the above
violation:

- Tell what is the other statement of the same rule:
3
2.4. Give the following structural information about the [IF4]-
ion :
- Electron pair geometry :
- Molecular geometry :
- Polarity: is the ion polar or nonpolar?
- Hybridization of iodine :

3: Give the valence electronic structure of the element
located in group 15, period 5:
Give the symbol and name of the same element:
Give the expected oxidation number(s) of the same element:
4: Give the most important interatomic interaction
responsible for the following :
- Boiling point of anhydrous HF :
- Boiling point of anhydrous HCl :
- Hydration of the barium ion :
- Hydration of the beryllium ion :
- Bonding in CaH2 :
4

5: Compare qualitatively (using the sign < and the ions
symbol) the ionic radius of the ion obtained when
Te, I, Cs and Ba achieve the nearest noble gas configuration.
Explain in 2 or 3 lines only.
6: Circle the letter a, or b, and/or c, or... for the answer that
applies best to the properties of most
molecular compounds in the given conditions in each question
below (MORE than one answer may apply):
6.1 At ambient temperature, most molecular compounds are:
a. Hard and brittle
b. Hard but not brittle
c. Soft
d. Malleable
e. Ductile

a. Good electrical conductors
b. Semiconductors
c. Insulators
a. Gases
b. Liquids
c. Low melting point solids
d. High melting point solids
5
6.4 At ambient temperature:
a. Most molecular compounds dissolve in non-polar solvents
and the solution does not
b. Most molecular compounds dissolve in non-polar solvents

and the solution conducts
electricity.
c. All molecular compounds dissolve in high polarity solvents
and the solution does not
d. All molecular compounds dissolve in high polarity solvents
and the solution conducts
electricity.
6.5 When heated to the molten state in a non-reactive
atmosphere, most molecular compounds behave as
follows:
a. They decompose.
b. They do not decompose and they conduct electricity.
c. They do not decompose and they do not conduct electricity.
6.6 Find the incorrect statement(s).
a. Molecular compounds cannot be composed of only non-
metals
b. Molecular compounds can be made of metals and non-metals.
c. Molecular compounds cannot be made of metals only.
d. An ionic bond is extreme case of a polar bond.
e. A small and highly charged cation can make covalent a bond
that would otherwise be

ionic
6
7: The combustion reaction of hydrogen in oxygen to give
hydrogen peroxide has a negative Gibbs free
energy.
7.1 Write the balance equation for the above reaction.
7.2 However, the above reaction does not take place. Write
the balanced equation for the combustion
reaction of hydrogen in oxygen that actually takes place.

7.3 Compare qualitatively the Gibbs free energy of the
reaction that actually takes to that of the reaction
that gives hydrogen peroxide.
7.4 Using the position of oxygen in the periodic table,
justify why the compound obtained by combustion
of hydrogen in oxygen is the compound shown in your answer
to question 7.2, rather than hydrogen peroxide.
7

8. Fill in the missing word in the following sentences:
8.1 A semiconductor doped with impurity is called an
semiconductor or an
semiconductor.
8.2 The theory that explains bonding and the electrical
properties of metals based on the presence of a very
large number of molecular orbitals very close to one another to
form a continuum is called the
theory.
9. Answer the following questions regarding the fcc structure
of a metal:
9.1 Tell what fcc stands for:

9.2 Tell what is the radius of a metal atom versus the fcc
unit-cell edge a:
9.3 Tell how many number of metal atoms there are in a fcc
unit-cell:
9.4 Tell what is the coordination number of each metal atom
in a fcc unit-cell:
8
10: Answer the following questions about acids and bases.
10.1 An acid stronger than 100% sulfuric acid is called a
.

10.2 Magic acid is made of
.
10.3 Magic acid is used in the petroleum industry for
breaking bonds between and
.
11. Write two balanced equations for reactions used for the
production of hydrogen in the two following
cases. For each, give the physical states of reactants and
products, and the reaction conditions.
11.1 Preparation in the laboratory:
11.2 Preparation in the industry:

9
12. Answer the following questions about metallic hydrides:
12.1 They contain hydrogen in the following form(s) (circle
your answer(s)):
H H2 H+ H- Not well defined
12.2 In addition to hydrogen, they contain one of the
following element:
a. An alkali metal or an alkaline earth metal
b. A transition metal
c. A metalloid

d. A non-metal
12.3 Their structure is:
a. Similar to the metal, with similar electrical and magnetic
properties
b. Molecular
c. Similar to a halide salt
d. Polymeric
10

12.4 Choose the correct statement about their physical state
and properties:
a. At ambient temperature, they are gases, liquids or soft solids
b. They melt at high temperature to give stable electrically non-
conducting melts.
c. They melt at high temperature to give stable electrically
conducting melts.
d. They decompose at high temperature, releasing hydrogen gas
and the metal.
12.5 Choose the correct statement about their stoichiometry:
a. All are stoichiometric compounds with an expected oxidation
state of the metal.
b. All are stoichiometric compounds with unexpected oxidation
states of the metal
c. Most are non-stoichiometric

12.6 Choose the method used for their preparation:
a. Reaction of an ionic hydride with a metal-containing
compound.
b. Reaction of an ionic hydride with a non-metal or a metalloid.
c. Decomposition of another hydride at high temperature.
d. Heating a metal under flow oh hydrogen.
e. Heating a metal under high pressure hydrogen.
11
13. Circle the following species that do NOT have an
octahedral molecular geometry in the gas phase:

[IF6]- [PF6]- SF6 XeF6
14. Tell what is obtained when each alkali metal is burned in an
excess of oxygen. Justify any difference
of behavior of each in no more than 3 or 4 lines.
12
15. Circle in the following list the mixed-oxidation state
compounds:
PbO PbO2 Pb2O3 Pb3O4 In2O3 InO
16. Comparing group 1 and group 11 elements:

16.1 Give the list of the elements of group 11 and their
electronic structure.
16 .2 Compare the reactivity of group 1 and group 11
elements with water, and use their electronic
structure to explain the similarities/differences.
13

17. Zinc oxide dissolves in both acids and bases.
17.1 This ability to dissolve in both acids or bases has two
names. Give the two names:
17.2 The formula and name of the zinc ion obtained in an acid
are:
17.3 The formula and name of the zinc ion obtained in a base
are:
18. Answer the following questions regarding spinels.
18.1 Give the formula of the spinel mineral:
18.2 Give the name of spinels that contain sulfide ions:

18.3 Give the formula of the three kinds of spinels, including
metal ion site occupation:
14
18.4 For the spinel containg zinc and iron(III), with a ratio
Fe/Zn = 2/1, give the formula and the magnetic
property for each kind of spinel, such as defined in above
question 18.3. Do NOT justify your answers.

19. Give the formula of each borate anion. Draw each anion,
including three variations for one of them,
and for each, give the ratio of bridging oxygen over terminal
oxygen

15

16
20. Answer the following question regarding graphite:
20.1 Most reliable method of preparation from amorphous
carbon at a large scale. Give the name of the
method and a brief description
20.2 Give the bonding type observed in graphite:
20.3 Tell whether graphite is molecular, ionic, metallic or a
covalent polymeric network

20.4 Give the hybridization of carbon in graphite
20.5 Tell whether graphite is hard or soft, and give a practical
application of its harness or softness.
20.6 Give its electrical property, and whether that property is
isotropic or anisotropic.
17
21. Answer the following regarding nitrogen dioxide :
21.1 Give its formula:

21.2 Draw all its Lewis structure(s) and tell whether there is
resonance in that molecule.
21.3 Give the hybridization of nitrogen:
21.4 Give the approximate bond angle, with a short explanation:
21.5 Give the bond order in the real nitrogen dioxide molecule:

21.6 Give the magnetic property of the molecule with a short
explanation:
18
22.
22.1 Explain briefly, using balanced equations, what happens
to the sulfur contained in coals and natural
gas when these are burned, and the resulting damage to the
environment:

22.2 Describe briefly, using a balanced equation, what is the
method used in industry to reduce the
emission of the sulfur compound formed in power plants that
burn coal or natural gas. Explain briefly why
such a reaction to neutralize the sulfur compound formed works.
19

23. Group 17 elements:
23.1 Give the name of group 17:
23.2 Given the expected oxidation states for group 17 elements,
and explain briefly why the first element
of the group behaves differently from the rest of the group with
respect to oxidation states:
23.3 Give the main natural source of fluorine :
See Part II of this exam on the next page

20
Part II starts here. Give your answers in the space provided.
Detailed explanation required
2x: Explain, using balanced equations, how caved are formed
underground and how columns of material
grow up from the floor of the caves and down from their
ceiling. Give the names of these columns of
material.

21
25: The structure of rubidium calcium fluoride, RbCaF3 has the
following characteristics:

- simple (primitive) cubic unit-cell, with a unit-cell edge a =
3.905 Å
- atomic positions: Ca in 0 0 0 Rb in 2 2 2 F in 2 0 0
25.1. Give the list of lattice translations present in a
primitive lattice (No redundant ones):
25.2. Derive the list of all ions contained in the unit-cell
(show calculation, do NOT give
redundant ones):
25.3. Draw a three-dimensional picture of the unit-cell and
place all the ions inside.
Draw all the bonds on the same picture.
Also draw one example of the shortest distance for the
following: Rb-Rb, Rb-Ca, Rb-F,
Ca-Ca, Ca-F and F-F.
22

25.4. Determine the number of each kind of ions in the unit-cell
(explain)
25.5. Check that the stoichiometry of the unit-cell is in
agreement with that of the compound
formula.
25.6. Determine the number of unit formulas in the unit-cell;
show the formula used.
23

25.7. Just using the position of the three elements in the
periodic table, i.e. without using the
figure, tell which elements form bonds to one another in
RbCaF3, and give, with
justifications, the mode of bonding.
25.8. Give the coordination number (for Rb, Ca and F) and
shape (for Ca and F only) of the
polyhedron of coordination of the ions, as shown on the figure.

25.9. Determine the values of the nearest Rb-Rb, Ca-Ca, F-F,
Rb-Ca, Rb-F and Ca-F
distances and. Show the detail of the calculations, and give the
coordinates of the pair of ions
used to calculate each interionic distance.
24
25.10. On the above figure, draw all the bonds for one Cu,
and the same for one Cl, showing the
three-dimensionality of the coordination of each ion.
Use the figure to give the coordination number and shape of the
polyhedron of coordination for
both ions.

25.11. Show on the figure one of each of the nearest Cu-Cu,
Cl-Cl, and Cu-Cl distances and
determine their numerical values. Show the detail of the
calculations.

25

26
qustion
Agnew, R. (2001) Building on the Foundation of General Strain
Theory: Specifying the Type of Strain Most
Likely to Lead to Crime and Deviance, Journal of Research in
Crime and Delinquency, 38(4):319-
361.
Writing a Critique
Please find below some tips for preparing your critique.
1. First look at the criteria sheet which you will find in the
[email protected] website under Assessment tab. Navigate to
Assessment 1 and then scroll down to folder saying Assessment
1. Open this and find the criteria sheet for marking – this will
tell you what you need to include.
2. The critique should set out:
· What article are you reviewing
· A brief summary of the article including what it’s aim was,
what was studied, and the theory it is testing.
· A summary of the key principles and concepts of the theory
and how these are applied to the problem
· Analysis of the strengths and limitations of the theory with
respect to its application
· Discuss the implications for public policy and/or future
research.
3. Structuring and Referencing

· The critique should have a clear structure which is readily
identifiable
· While this is not a research exercise, and therefore is not
asking for lots of references, where you are using references
(including the article being reviewed) ensure references use the
APA system.
· Spell and grammar check!!
4. Please ensure that the critique is 1.5 or double spaced in size
12 font.

Criteria for Assessment 1– Applying Theory to a Case Study – A.docx

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