UNIVERSITY OF TORONTO

FACULTY OF APPLIED SCIENCE AND ENGINEERING

FINAL EXAMINATION, December 18, 2018

DURATION: 2 and 1/2 hrs

Second Year - MSE

MSE2441-11 F - Inorganic Material Chemistry & Processing

Calculator Type: 3

Exam Type: B

Examiner - Keryn Lian

Answer all the questions

Total Mark: 100

Student Name Student Number

Page 1 of 9 pages

No. I Comolete the followna Tables 1`16 nointsl

Name Chemical Formula

Donor atoms

Coordination Number

Lewis Acid

Type of hybridization

Tetra-ammine-dichioro-

platinum(IV) sulfate

(NH4)2[Zn(CN)3C1}

For all main group elements in the periodic table, iiioving from top to bottom, describe

the trend for the properties below:

Ionization energy

Charge density

electronegativity

For the P row of transition metals in the periodic table, moving from left to riht the

trend for the properties:

Number of oxidation states

jst ionization energy

Standard reduction potential (up to Cu)

No. 2 True or False [8 points]

L The covalent bonds in SiO2 are all single bonds

White phosphorous is less toxic than red phosphorous

A fully charged Pb-acid battery contain mainly PbSO4

Only transition metal ions can form Lewis acid in complex

Ca(HC0)2 is soluble in water

Enthalpy drives the formation of [Cu(en)2]2 over [Cu(NH3)4]2

True False

Page 2 of 9 pages

P is added to Si to provide excess electrons -

The oxidation numbers of 3d transition metals are always greater than 2

No. 3 Multiple Choices [10 points]

At certain temperature, pure water has a pH of 6.5, what is the pOI-I?

a. 7.5 b. 7 c. 6.5 d) > 7.5

Which molecule is the least polar?

a. HF b. HC1 c. HBr d. HI

Which one of the following has the highest electrical conductivity?

a. Au b. Ag c.Cu d. Fe

For reaction C032 +H20HCO3 +OH, C032 is a/an

a. base b. acid c. oxidation agent d. reducing agent

Which one is the most basic?

a. MnO b. Mn203 c. Mn02 d. Mn207

The most unstable one is:

a. NO b. N20 c. NO2 d. N203

Which solution has a pH that is independent of concentration?

a. NaOH b. Na3PO4 c. NH4C1 d. NH4CN

The coordination number of [Fe(EDTA)]2

a.1 b.2 c.4 d.6

Among the following, the weakest acid is

a. HC102 b. HBr02 c. H102 d. HC103

The electronic configuration [Ar]3d64s° corresponds to

a. Mn 21 b. Fe' C. CO3 d. Ni 2+

Page 3 of 9 pages

No. 4 Identify the X and Y elements [8 points] In alkaline battery, the anode and cathode are made of these X and Y.

In groups 1 and 2, these X and Y have similar charge density

Air bag inflation is due to decomposition of XY3 from groups 1 and 5.

This X is used as sacrificial anode to protect steel.

This X in group 7 has the fewest oxidation states.

No. 5 Short Questions [18 points] 1. Compare the following (and explain when required):

When performing anionic analyses, we used Na for all the salt solutions in lab 2. To

analyze cations such as A13 , Ag, Ni2 and Ti 41, which anion can we use to make

these salt solutions? Why?

Compare the following:

Sn(OH)2 and Pb(OH)2, which one is more basic?

Cl- vs. Br, which one is a stronger reducing agent?

Cr vs. Mn, which one has a higher electronegativity?

Rank the electron affinities of following element from high( I) to low (4)

Na Mg P Cl

Answer the following questions

a. 1) Complete reaction in blast furnace for steel;

What is the oxidation state of Fe in Fe304;

What is the difference of C in blast furnace vs Al process in terms of

functionality?

Page 40f9 pages

h The 3 main stens in conner hvdrometa11ury nrocess. their main reactants & nroducts?

Step Reactants Products

No. 6 Use balanced reactions to answer/explain the following [10 points]:

Sodium cyanide is lethal when ingested by human.

Potassium superoxide used in respiratory equipment.

Concentrate nitric acid decompose to gases under sunlight.

Can one use steel container to store 1) concentrated or 2) diluted H2SO4?

Use the respective reactions to explain.

No. 7 Lab Practices [10 points]

1. In a lab, you are provided the following: test tubes, water, and solutions of HC1, and

NaOH, NaHCO3, Na2CO3, NaCl, BaC12. Propose the simplest experimental steps to

perform the following tasks (use bullets to describe, no need to use all the chemicals):

a. There is an acid spill on the table and you need to neutralize it. Which one from the

above list is the most appropriate to use? Briefly explain your reason(s).

Answer:

Reason:

Page 5 of 9 pages

There are 4 unlabeled solutions: KC1, KOH, K2CO3, and K2SO4. Use pH paper and

only one chemical listed above to differentiate them:

Step 1:

Step 2:

Step 3:

Two unlabeled test tubes contain either 1M NaOH or 1 M HCl solution. You have run

out of pH paper. With some orange Cr 6+ solution in a beaker, please differentiate them.

Step:

Observation and conclusion:

No. 8 Calculations [10 points]:

1) A hypothetical battery using Cu as positive electrode and Fe as negative electrode.

Write anode and cathode reactions and the total reaction

Calculate the battery cell voltage

To run the battery for 500 hr at 10 mA, how much Cu and Fe (Ingram) are

needed respectively? Given mol = Q/nF and F = 96500 C/mol.

Page 60f9 pages

2) Determine the direction for [Cu(NH3)4]2 + Zn2 = [Zn(NH3)4]2 + Cu'. Given:

KSt[cU(NU3)4]2+ = 2.1 x 1013 and Kst[zfl(NH3)4}2+ = 2.9x 109. Show calculation.

No. 9 Your Element [10 points]:

Select one element from either group 4 (main) or 3d transition metals (3d), and answer

the following:

Name and electronic configuration:

Common oxidation state (s):

Any 3 general properties (e.g. electrical conductivity, acidity, color/colorless,

para- or dia-magnetism of the ion or oxides etc.) of the element or its ion of the

highest oxidation state:

Applications (2 examples):

What makes you interested in this element from materials science perspective?

Page 7 of 9 pages

Periodic Table of the Elements

1 J.&Q 2

3 4 2 Li Bc

9L9.012 ii 1 iz

3 Na Mg

19 20

4 L2Jo

37 38

51 R Sr La 5 .4 7J 7 .6 2

55 56

6 Cs 37. 3J

87 88 $

7 Fr I Ra!

7

ç Atomic number

13 14 15 16 17 Ile

Symbol F !sk7 6

7 1 8 9 10

Atomacweight 101 1 3.201 140Lj6QQ 1900 2018 13 1 14 15 16 17 18

\1 Si P S Cl Ar 3 4 5 6 7 8 9 10 11 12 16. 1.09 _3o,.971 39,95

21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36

S( Ti \ (r I NIiiI I:(.- Co Ni I CAI Zn (t G \s Se IBr Kr 7. si-qqlil~_ 55-BS 86 12 69.72 2261 292.

39 40 41 42 43 44 45 46 47 4S 49 50 51 52 53 54

'V Zr Ni) Mo l. Ru1Rh Pd \t (ci In Sn Si) Te I \&. 9J2 92.94 9!1jQLt 2 1J,9.L IV _L4,0 37. 136 13L

71 72 73 75 76 77 78 79 80 81 82 83 84 85 i 86

Lu III Lt \\ R' Ii Pt \u lhi Fl Pb Bi P0Al Rn 175.0 178.5 180,9, 183.8186,2190. 192.2 195.1 i97OjOth 204.4 207,2 209.O 209.04 210O 222,0

103 104 105 106 1 107 103 109 110 111 112 114 116 118

I r RI 1)b 'ti i Bh IIS Mt I '"111A,11111,111 I uq t uh I.ui 221. AL L, 26iL.LLi1 Z29 L212. L22?J 89j

_________ - r-----'""---- - -- -

57 58$59 60161 6263646 6667 686979

I t ( e Pr Nd Pm Sm I ii Gd lb I) lb I r Fm \ b

LL8.9 40,1 140, 469 150.4 152,0 3.57,3 158,9 162: 164,91167.3 3.68,9 173.0

\ 90 91 3 93 95 96 97 98 99 100 101 102

\.. I h P Ii ) Pu in ( in Rh ( t I ' 1:111 Md \o 9

22 21L QJ Q2i4J 23.iL4LL2ll .25 2Q 25LZL.22

Table 12.2: Standard Reduction Potentialsat 25°C

I1alf-reiction I.

(aql + e - IA(. I

K (d(j ) e K( .0 -

Ba ( aq } 4 2e --' 13M ,0

S ((Iq) + 2c Sr( I -

Ca1 (we> + 2e -• (.':tt )

Na ' ( flit ) -v e - Na)

Mg2 (aq) 2e - Mg) I 2.37

13e (ij) 4 2e 11e(.)

I\I (aq) - 3e -. ,\I).$)

M11 2 ' (aq) i- 2V . Mn(

N(g) + 411,01) 1 4e -- N.Il(,) 4011 (q1 1.1(

211,0(1) + 2e --' 11,(g) -+. 2031 (uq)

Fe (aq) -f 2e --• Ed 0,44

1'l (aq) ± e iI(.) I, 33

I11S0( 0 + ' 3)( W. (aq) 0. 11

Sn2 '(flit) + 2. - Sn) s ) 0, [ I

PW'(wi) -i 2' • Ph) I 11. 1-1

211(cuj) + 2e '

S40; (aj) + 2' — 2S0 (( It/) .• 1,08

- Sn 4 (th/) + 2e Sn2 '(iq) II. 11

5(s) s 211 ' (iuj) f 2e [1Ng) UI-)

S0, (aq) + 411 (ail ) 1- 2e -' SOAg 2 11 .031) ()21)

(u2 (fill) 2 - ('u(s) D.34

S0, (aq) 4 81I • )1(f) -1 Oe -. 5(c) 't 411 0(/) UP

211,01) -- 4t ---' 4011 (aq) 0.431

(.0(g) + 231 '(aft) - 2e — ('(sI 4 Il)(/)

i(s) 2e --- 21 (tuj) (I_s,)

MnO, (aq) 211 0(1) -f 3e --• Mn0(s) -1011 (aq)

211 ' (aj)

l

Ag (aq) -f e -. Ag(s)

NO (uq) 1 211 (aq) •4 e N O,(g) [1,0(/) UU

OCI (it(/) i [1,0(1) i 2' CI (nq)* 2011 (nq) — c)) NO, I aq I + 431 (aq ) - 3e -. No(g) - 211. (')( I 03)6

r3 - .(1) ± 2e —• 213r (aq) 1.117

(Hg) + 411 (iq) ---1e --• 211 MM .23

Mn0,(s) + 411 (aj) 2e -. Mn 2 (a(/) + 211.(1I) 3.23

Cr,O (aq) - I311 (1q) 1- (' ---p 2Cr (aq) - 71L0(/) -- I 33

(l(g ) + 2e 20 (flit)

PhO,(s) - 41-1(aq) + 2e -. Ph 2 (aq) + 2110(fl 1.40

MnO3T (aq) + II (aq) + -. Mir (uql 4- 4lI0(/) ... I.:Sl

CC, (aq) + e -+ ( (aft) I -

21 [OCRaq) + 211 (aq) + 2+ -. ('l .(g) 2110(1) -'- 1153

PbO2( s) + 431 (aq) -+. SO (aft) f 2 e

PhSO4(s) + 231,(.)(1) + 1.70

Br04 (aq) + 211-(aq) - 2s' . 13r()- (aq) [10(/) 3,74

11,0(aq) + 211' (fill) + 2e -+ 211.0(1) .- 3.77

NO(g) + 2H(aq) + 2. -. N.(g) 4- iIO(I) -- 377

((aq) 1- t' —p (n2(tiq) ~

S2O (uq) + 2e '-. 2SO. Wit)

O(g) + 2I1(aq) + 2e ---* 04,$) + 11.,0(/) 71.07

XeO 4(aq) + 61-1 (aq) + (u —. XeI.g ) ± 311.0(/) -2.1(I

XeF-(aq) + 231 (aq) -t 2e ---p Xc(g ) -+ 2111-'(aq) 4. 2.04

+ 2t''-'-' 2F(aq) 2.57

Page 9of9 pages