Chemistry 112 Name _______________________

Final Exam Form A Section _______________________

May 4, 2015 Signature _______________________

IMPORTANT: On the scantron (answer sheet), you MUST clearly fill your name, your student number, section number, and test form (white cover = test form A; yellow cover = test form B). Use a #2 pencil.

There are 40 questions on this exam. Check that you have done all of the problems and filled in the first 40 bubbles on the scantron. The maximum score on this exam is 40 points. Your score will be reported in percents (max 100%).

Exam policy This cover sheet must be signed and handed in with your answer sheet for your

exam to count. Calculators with text-programmable memory are not allowed. Relevant data and formulas, including the periodic table, are attached at the end of

this exam. Your grade will be based only on what is on the scantron form. The answer key will be posted on the web after the exam (under News).

Hints As you read the question, underline or circle key words to highlight them for

yourself. Avoid errors from "mis-reading" the question. Pay attention to units and magnitudes (decimal places) of numbers obtained from

calculations. There is no penalty for guessing.

CHEMISTRY 112 EXAM 4 May. 4, 2015

FORM A ---------------------------------------------------------------------------------------------------------------------

1. What is the bond order of the heteronuclear diatomic ion NO+

? Use the M.O. Energy diagram below.

A. 1

B. 1.5

C. 2

D. 2.5

E. 3 \--------------------------------------------------------------------------------------------------------------------- 2. Consider the following kinetic data for the reaction:

A + 2 B products

Experiment [A], M [B], M Initial Rate, M/s 1 0.10 0.10 7.00 10–5 2 0.20 0.10 2.80 10–4 3 0.20 0.20 2.80 10–4

The rate law for the reaction is:

A. k [A] [B]

B. k [A]2 [B]

C. k [A]1/2 [B]

D. k [A] [B]2

E. k [A]2 ---------------------------------------------------------------------------------------------------------------------

--------------------------------------------------------------------------------------------------------------------- 3. The most probable mode of decay of 40Cl is

A. emission

B. emission

C. positron emission

D. neutron emission

E. electron capture --------------------------------------------------------------------------------------------------------------------- 4. Which of the following combinations can make a buffer?

A. HNO3 + NaNO3

B. KCl + HCl

C. NaNO2 + NaBr

D. HF + KF

E. NaOH + NaCl --------------------------------------------------------------------------------------------------------------------- 5. Which element could be used to dope silicon to create a p-type semiconductor?

A. B

B. P

C. C

D. Ge

E. F --------------------------------------------------------------------------------------------------------------------- 6. Which one of the following statements is true regarding semiconductors?

A. Intrinsic semiconductors have an average of 5 electrons per atom.

B. An example of an intrinsic semiconductor is GaTe.

C. An example of an n-type semiconductor is Si doped with P.

D. Semiconductors have no band gap; electrons are free to move between the valence band and conduction band with little to no energy needed.

E. A p-type semiconductor consists of an intrinsic semiconductor that is intentionally doped with an impurity that contains more than 4 valence electrons.

---------------------------------------------------------------------------------------------------------------------

----------------------------------------------------------------------------------------------------------- 7. Band theory explains the conductive properties of materials. Match each MO band

theory pictured below to the proper material:

A. Conductor (metal) Semiconductor Insulator

B. Insulator Semiconductor Conductor (metal)

C. Conductor (metal) Insulator Semiconductor

D. Insulator Conductor (metal) Semiconductor

E. Semiconductor Insulator Conductor (metal)

--------------------------------------------------------------------------------------------------------------------- 8. Which of the following substances does not exist in the indicated solid type?

A. graphite – covalent network

B. SiO2 – molecular

C. Na – metallic

D. KI – ionic

E. diamond – covalent network --------------------------------------------------------------------------------------------------------------------- 9. What is ∆Go for the base hydrolysis of methylamine (CH3NH2) in an aqueous solution

at 25 oC? Kb (CH3NH2) = 4.4 × 10−4

A. 19.1 kJ/mol

B. 1.61 kJ/mol

C. 8.32 kJ/mol

D. −1.57 × 103 kJ/mol

E. −698. kJ/mol ---------------------------------------------------------------------------------------------------------------------

--------------------------------------------------------------------------------------------------------------------- 10. Which of the following statements regarding molecular solids is/are true?

i. All molecular solids have London dispersion forces between the molecules.

ii. The melting points of molecular solids depend only on molecular mass.

iii. Molecular solids are good conductors of heat and electricity.

A. i only

B. ii only

C. iii only

D. i and iii only

E. ii and iii only --------------------------------------------------------------------------------------------------------------------- 11. The following is a titration curve for the titration of acetic acid and NaOH. Where is

the buffer region?

A. A

B. B

C. C

D. A and C

E. There is no buffer region. ---------------------------------------------------------------------------------------------------------------------

0

2

4

6

8

10

12

14

0 10 20 30 40 50

pH

mL NaOH added

A.

B

C.

--------------------------------------------------------------------------------------------------------------------- 12. A weak acid HA has a dissociation constant Ka = 1.0 x 10−7. For a 0.30 M solution of

HA in water, which of the following relationships is/are true?

i. [A−] << [HA]

ii. [H+] = (Ka[HA])1/2

iii. [OH−] >> [A−]

A. i only

B. ii only

C. i and ii only

D. ii and iii only

E. i, ii, and iii --------------------------------------------------------------------------------------------------------------------- 13. A 15.2 mg sample of 90Sr has an activity of 1.2 1012 dps. What will the activity of

the sample be after 60 years? (The half-life of 90Sr is 29 years.)

A. 1.8 1011 dps

B. 2.9 1011 dps

C. 4.5 1011 dps

D. 6.0 1011 dps

E. 8.0 1011 dps --------------------------------------------------------------------------------------------------------------------- 14. Magnesium hydroxide is the active ingredient in the liquid antacid called “milk of

magnesia.” The liquid appears milky because of the limited solubility of magnesium hydroxide in an aqueous solution. What is the pH of a saturated solution of Mg(OH)2(s) at 25 oC? Ksp of Mg(OH)2(s) = 5.6 × 10−12.

A. 3.95

B. 10.1

C. 3.65

D. 10.3

E. 7.00 ---------------------------------------------------------------------------------------------------------------------

--------------------------------------------------------------------------------------------------------------------- 15. Which one of the following is the strongest reducing agent under standard onditions?

A. H2(g)

B. Au(s)

C. F2(g)

D. Li+(aq)

E. Na(s) --------------------------------------------------------------------------------------------------------------------- 16. A voltaic cell is constructed:

What is Ecell at 25 oC when [Cu(NO3)2] = 0.0100 M and [Zn(NO3)2] = 1.90 M?

A. 1.03 V

B. 1.11 V

C. 1.17 V

D. 0.969 V

E. 1.24 V --------------------------------------------------------------------------------------------------------------------- 17. The addition of which one of the following will result in a decrease in the solubility of

CuCO3 (Ksp = 2.3 × 10−10)?

A. HNO3

B. Na2CO3

C. NH3

D. NaNO3

E. HCl ---------------------------------------------------------------------------------------------------------------------

----------------------------------------------------------------------------------------------------------- 18. Consider the hypothetical reaction:

A + 2B 2C + D

The mechanism for the reaction is:

2 Bk1

k1

X fast equilibrium

X A k2 2 C D slow

Which one of the reaction profiles shown below fits this mechanism? A. B.

C. D.

E. There is not enough information to choose. ---------------------------------------------------------------------------------------------------------------------

--------------------------------------------------------------------------------------------------------------------- 19. Benadryl is an over-the-counter drug that acts as an antihistamine. It is used to treat a

number of conditions that include allergies, insomnia, and motion sickness. At 25 oC, an aqueous solution of Benadryl, with a concentration of 0.025 M, has a pH of 10.7. Calculate Kb of Benadryl at 25 oC.

Structure of benadryl:

A. 6.2 10−6

B. 1.0 10−5

C. 5.0 10−4

D. 3.0 10−5

E. 2.5 10−7 --------------------------------------------------------------------------------------------------------------------- 20. Consider the following aqueous solution of Benadryl:

Which of the following would cause the equilibrium to shift to the RIGHT at 25 oC?

i. Dissolving more Benadryl

ii. Addition of HCl

iii. Addition of NaOH

iv. Diluting the solution by adding water

A. i only

B. ii only

C. iii only

D. i, ii and iv only

E. i, iii and iv only ---------------------------------------------------------------------------------------------------------------------

O N

+ H2O

O NH+

+ OH-

ON

--------------------------------------------------------------------------------------------------------------------- 21. Nittnium (Nt) cations readily form coordination compounds. Consider the compound: [Nt(en)Cl2]Br2. What is the charge on the central Nittnium cation and the coordination number of this complex? (en = NH2CH2CH2NH2) --------------------------------------------------------------------------------------------------------------------- 22. Which of the following structures represents the addition polymer that can be made

from the monomer indicated?

---------------------------------------------------------------------------------------------------------------------

Answer Charge on Nt Coordination Number

A 2+ 3

B 4+ 3

C 2+ 4

D 4+ 4

E 2+ 6

--------------------------------------------------------------------------------------------------------------------- 23. Which of the following structures represents the monomer that can be used to make the polypeptide polymer indicated?

--------------------------------------------------------------------------------------------------------------------- 24. Rick T. Cat needs golden claws for his next great adventure across the deserts of

Caldeum and he needs them fast! He decides to use a 60 ampere current to reduce his solution of Au(NO3)3 into solid gold. How long will it take him to plate 10 grams of gold for his next amazing adventure?

A. 148 sec

B. 245 sec

C. 14,700 sec

D. 48,250 sec

E. 882,000 sec ---------------------------------------------------------------------------------------------------------------------

--------------------------------------------------------------------------------------------------------------------- 25. Consider the following complexes with their respective colors:

Complex Observed Color

[CoBr6]3− Green

[Co(CO)6]3+ Orange

[Co(NH3)6]3+ Blue

[Co(CN)6]3− Yellow

Based on this information, place the following ligands in order of increasing crystal field splitting strength:

Br−, CO, NH3, CN−

A. Br− < CO < NH3 < CN−

B. Br− < NH3 < CO < CN−

C. CO < CN− < Br− < NH3

D. CO < CN− < NH3 < Br−

E. Br− < NH3 < CN− < CO --------------------------------------------------------------------------------------------------------------------- 26. Given the following table of thermodynamic data, complete the following sentence.

Substance Hf (kJ/mol)

S (J/mol • K)

TiCl4 (g) 763.2 354.9

TiCl4 (l) 804.2 221.9

The vaporization of TiCl4 is _____.

A. spontaneous at all temperatures

B. spontaneous at low temperature and nonspontaneous at high temperature

C. non-spontaneous at low temperature and spontaneous at high temperature

D. non-spontaneous at all temperatures

E. not enough information given to draw a conclusion ---------------------------------------------------------------------------------------------------------------------

--------------------------------------------------------------------------------------------------------------------- 27. Which of the following statements are true?

i. A chelating ligand will form a more stable complex than a comparable monodentate ligand (assuming the same metal ion is involved) because the entropy associated with chelate formation is more positive.

ii. If a solution containing a metal complex is blue, yellow light is being absorbed.

iii. A low spin complex will have a smaller crystal field splitting (∆) than a high spin complex if the metal ion and geometry are the same.

A. i only

B. ii only

C. iii only

D. i and ii

E. i and iii --------------------------------------------------------------------------------------------------------------------- 28. Which one of the following will have the greatest number of unpaired electrons?

A. [Mn(H2O)6]2+ (weak field)

B. [Fe(en)3]3+ (strong field)

C. [Ru(NH3)6]2+ (strong field)

D. [Cr(Cl)6]4− (weak field)

E. [Fe(en)3]2+ (strong field)

--------------------------------------------------------------------------------------------------------------------- 29. What would be the observed color of a complex with a crystal field splitting energy

of 300 kJ/mole?

A. Red

B. Orange

C. Yellow

D. Blue

E. Violet ---------------------------------------------------------------------------------------------------------------------

--------------------------------------------------------------------------------------------------------------------- 30. Which of the following when dissolved in water will form an acidic solution?

1. FeCl3 2. NH4Cl 3. Na2CO3

4. P4O10

A. 1 and 2

B. 1 and 3

C. 2 only

D. 2 and 4

E. 1, 2, and 4 --------------------------------------------------------------------------------------------------------------------- 31. Which one of the following reactions is BEST described by the graph below:

A. 2 C8H18(l) + 25 O2(g) → 16 CO2(g) + 18 H2O(g)

B. Heat + CaCO3(s) → CaO(s) + CO2(g)

C. 2 H2(g) + O2(g) → 2 H2O(g)

D. Heat + 3 O2(g) → 2 O3(g)

E. C6H12O6(s) + 6 O2(g) → 6 CO2(g) + 6 H2O(g) ---------------------------------------------------------------------------------------------------------------------

T

--------------------------------------------------------------------------------------------------------------------- 32. Chlorine bleach is a water solution of sodium hypochlorite. Regular strength laundry Bleach is typically a 0.70 M NaClO (aq) solution. Given that Ka for HClO = 3.0 × 10−8 at 25 oC, what is the pH of bleach?

A. 5.6

B. 7.9

C. 10.7

D. 12.5

E. 13.1

--------------------------------------------------------------------------------------------------------------------- 33. 50.0 mL of 0.50 M NaOH is added to a 250 mL solution containing 0.30 M NH3 and

0.36 M NH4Cl. What is the pH of the resulting solution?

Kb of NH3 = 1.8 10−5

A. 8.56

B. 9.26

C. 9.08

D. 9.44

E. 12.12 --------------------------------------------------------------------------------------------------------------------- 34. One of the ways to determine the concentration of ethanol in the blood is via

titration. Ethanol reacts with a solution of dichromate ions under acidic conditions in the following unbalanced reaction:

Cr2O7

2−(aq) + CH3CH2OH (aq) → Cr3+ (aq) + CO2 (g)

When balanced in acid, what is the coefficient in front of H+ (aq)?

A. 4

B. 8

C. 12

D. 16

E. 28 ---------------------------------------------------------------------------------------------------------------------

--------------------------------------------------------------------------------------------------------------------- 35. Equal volumes of 0.05 M solutions of several different acids are titrated with 0.1 M NaOH. The acid for which the pH at the equivalence point will be the highest is:

A. HClO4

B. HBrO

C. HClO

D. HClO3

E. HIO --------------------------------------------------------------------------------------------------------------------- 36. What is the activation energy for a reaction whose rate constant increases by a

factor of 10 upon increasing the reaction temperature from 303 K to 333 K?

A. 30 kJ/mol

B. 33 kJ/mol

C. 46 kJ/mol

D. 64 kJ/mol

E. 89 kJ/mol --------------------------------------------------------------------------------------------------------------------- 37. The plot of the experimental data for the following reaction is shown below.

2 A B + C

If the slope of the plot is 1.00 M−1s−1, and the y-intercept is 1.00 M−1 how long does it take for [A] to drop from [A]0 to 0.50 M?

A. 0.50 s

B. 1.00 s

C. 0.693 s

D. 2.00 s

E. 100 s ---------------------------------------------------------------------------------------------------------------------

1

[A]

t (s)

--------------------------------------------------------------------------------------------------------------------- 38. What is the nuclear binding energy of iron-56 in kJ/mol?

The mass of the iron-56 nucleus is 55.92068 amu.

A. 7.90 10–11 kJ/mol

B. 2.78 109 kJ/mol

C. 4.76 1010 kJ/mol

D. 8.78 10–28 kJ/mol

E. 5.38 1012 kJ/mol --------------------------------------------------------------------------------------------------------------------- 39. Which one of the following statements concerning electrochemistry is FALSE?

A. If a voltaic cell has a positive cell potential, it is spontaneous as written and will have a negative ∆G.

B. In a voltaic cell when Ecell = 0 and ∆G = 0, the system is at equilibrium.

C. In order to maintain electrical neutrality in a voltaic cell, anions in a salt bridge flow towards the cathode and cations in a salt bridge flow towards the anode.

D. Electrons in a voltaic cell always travel from the anode to the cathode.

E. During electrolysis, electrical work pulls electrons from the anode and forces electrons into the cathode to force a non-spontaneous reaction in the forward direction.

---------------------------------------------------------------------------------------------------------------------

--------------------------------------------------------------------------------------------------------------------- 40. Using reaction progress kinetic analysis, the following data were collected for a reaction producing nitrous and nitric acid:

Using these data, the following mechanism was proposed:

NO (g) + NO (g) N2O2 (g) N2O2 (g) + O2 (g) N2O4 (g)

N2O4 (g) + H2O (g) HNO2 (g) + HNO3 (g) What is the observed rate law consistent with this graph and mechanism?

A. kobs[NO]2[O2]

B. kobs[NO]2

C. kobs[N2O2][O2]

D. kobs[N2O4][H2O]

E. kobs[N2O2][O2][H2O] --------------------------------------------------------------------------------------------------------------------- --------------------------------------------------------------------------------------------------------------------- ---------------------------------------------------------------------------------------------------------------------

End of Exam

CH

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CHEM 112 Spring 2015

Final Exam - Form A Scrap Paper

Chem 112 Equations Constants, Conversions And Equations For Use During Exams And Quizzes

 

Conversions     Constants  1J = kg ⋅m2 ⋅s−2 = C ⋅V     c = 2.99792458 ×108 m ⋅s−1     R = 0.08206 L ⋅atm ⋅mol−1 ⋅K−1  

1A = C ⋅s−1     h = 6.63 ×10−34 J ⋅s     R = 8.314 J ⋅mol−1 ⋅K−1  

1g = 6.02×1023 amu     F = 96,485 C ⋅mol−1     01 n = 1.0086649 amu  

    NA = 6.022×1023 mol−1     11 p = 1.0072765 amu  

    KW = 1×10−14 at 25 oC      Equations  

k = Ae−EaRT

⎛

⎝⎜⎞

⎠⎟

  Rate = kN   ΔG = ΔH −TΔS = −nFE  

ln k =

−Ea

RT+ ln A  

ln

Nt

N0

= −0.693tt1 2

= −kt   ΔGo = −2.303 RT log K = −RT ln K  

ln A⎡⎣ ⎤⎦ = ln A⎡⎣ ⎤⎦0

− kt   E=hν = hcλ   ΔG = ΔGo +RT ln Q  

ln

k1

k2

=Ea

R1

T2

− 1T1

⎛

⎝⎜⎞

⎠⎟   E = mc2   ΔG = ΔGo + 2.303 RT log Q  

t1 2 = ln2

k= 0.693

k  

Ka ×Kb = KW = H+⎡⎣ ⎤⎦ OH−⎡⎣ ⎤⎦  

Eo = 0.0592

nlog K at 25 oC( )  

1A⎡⎣ ⎤⎦

= 1A⎡⎣ ⎤⎦0

+ kt   pH = pKa + log

X−⎡⎣ ⎤⎦HX⎡⎣ ⎤⎦

  E = Eo − 0.0592

nlog Q at 25 oC( )  

Kp = Kc RT( )Δn

  pKW = pH+pOH = pKa +pKb

   

Molecular  Orbital  Theory  Diagrams   Crystal  Field  Theory  Diagram                                                 Color  Wheel  with  Wavelength  Ranges                                                                      

   

Chem 112 Equations Constants, Conversions And Equations For Use During Exams And Quizzes

Standard  Reduction  Potentials  in  Water  at  25°C    Half  Reaction   E°1/2(V)  F2 g( ) + 2 e− → 2F− aq( ) + 2.87

H2O2 aq( ) + 2H+ aq( ) + 2 e− → 2H2O ℓ( ) + 1.776  Au+ aq( ) + e− → Au s( ) + 1.69  PbO2 s( ) + 4 H+ aq( ) + SO4

2− aq( ) + 2 e− → PbSO4 s( ) + 2H2O ℓ( ) + 1.685  Cl2 g( ) + 2 e− → 2 Cl− aq( ) + 1.359  O2 g( ) + 4 H+ aq( ) + 4 e− → 2H2O ℓ( ) + 1.23  ClO4

− aq( ) + 2H+ aq( ) + 2 e− → ClO3− aq( ) + H2O ℓ( ) + 1.23  

Pt2+ aq( ) + 2 e− → Pt s( ) + 1.20  

2 IO3

− aq( ) +12 H+ aq( ) +10 e− → I2 s( ) + 6 H2O ℓ( ) +1.195  Br2 ℓ( ) + 2 e− → 2Br − aq( ) + 1.065  NO3

− aq( ) + 4 H+ aq( ) + 3 e− →NO g( ) + 2H2O ℓ( ) + 0.96  Ag+ aq( ) + e− → Ag s( ) + 0.799  Fe3+ aq( ) + e− → Fe2+ aq( ) + 0.771  O2 g( ) + 2H+ aq( ) + 2 e− →H2O2 aq( ) + 0.68  I2 s( ) + 2 e− → 2 I− aq( ) + 0.536  I3− aq( ) + 2 e− → 3 I− aq( ) + 0.53  Cu+ aq( ) + e− → Cu s( ) + 0.521  Cu2+ aq( ) + 2 e− → Cu s( ) + 0.337  Sn4+ aq( ) + 2 e− → Sn2+ aq( ) + 0.154  Cu2+ aq( ) + e− → Cu+ aq( ) + 0.153  2H+ aq( ) + 2 e− →H2 g( ) + 0.00  Pb2+ aq( ) + 2 e− → Pb s( ) − 0.126  Sn2+ aq( ) + 2 e− → Sn s( ) − 0.136  Co2+ aq( ) + 2 e− → Co s( ) − 0.277  Ni2+ aq( ) + 2 e− →Ni s( ) − 0.28  Cd2+ aq( ) + 2 e− → Cd s( ) − 0.403  Fe2+ aq( ) + 2 e− → Fe s( ) − 0.440  Cr3+ aq( ) + 3 e− → Cr s( ) − 0.74  Zn2+ aq( ) + 2 e− → Zn s( ) − 0.763  2H2O ℓ( ) + 2 e− →H2 g( ) + 2 OH− aq( ) − 0.83  SO4

2− aq( ) + H2O ℓ( ) + 2 e− → SO32− aq( ) + 2 OH− aq( ) − 0.93  

Mn2+ aq( ) + 2 e− →Mn s( ) −1.18  Al3+ aq( ) + 3 e− → Al s( ) −1.66  Mg2+ aq( ) + 2 e− →Mg s( ) − 2.37  Na+ aq( ) + e− →Na s( ) − 2.71  Ca2+ aq( ) + 2 e− → Ca s( ) − 2.87  Li+ aq( ) + e− → Li s( ) − 3.05  

PERIODIC TABLE of the ELEMENTS MAIN GROUPS MAIN GROUPS

1A 1

8A 18

1 H

1.008

2A 2

3A 13

4A 14

5A 15

6A 16

7A 17

2 He

4.003

3 Li

6.941

4 Be

9.012

TRANSITION METALS

5 B

10.811

6 C

12.011

7 N

14.007

8 O

15.999

9 F

18.998

10 Ne

20.180

11 Na

22.990

12 Mg

24.305

3B 3

4B 4

5B 5

6B 6

7B 7

8B 8

8B 9

8B 10

1B 11

2B 12

13 Al

26.982

14 Si

28.086

15 P

30.974

16 S

32.066

17 Cl

35.453

18 Ar

39.948

19 K

39.098

20 Ca

40.078

21 Sc

44.956

22 Ti

47.867

23 V

50.942

24 Cr

51.996

25 Mn

54.938

26 Fe

55.845

27 Co

58.933

28 Ni

58.693

29 Cu

63.546

30 Zn

65.39

31 Ga

69.723

32 Ge 72.61

33 As

74.992

34 Se

78.96

35 Br

79.904

36 Kr

83.80

37 Rb

85.468

38 Sr

87.62

39 Y

88.906

40 Zr

91.224

41 Nb

92.906

42 Mo 95.94

43 Tc [98]

44 Ru

101.07

45 Rh

102.90

46 Pd

106.42

47 Ag

107.87

48 Cd

112.41

49 In

114.82

50 Sn

118.71

51 Sb

121.76

52 Te

127.60

53 I

126.90

54 Xe

131.29

55 Cs

132.91

56 Ba

137.33

57 La*

138.91

72 Hf

178.49

73 Ta

180.95

74 W

183.84

75 Re

186.21

76 Os

190.23

77 Ir

192.22

78 Pt

195.08

79 Au

196.97

80 Hg

200.59

81 Tl

204.38

82 Pb

207.2

83 Bi

208.98

84 Po [209]

85 At

[210]

86 Rn [222]

87 Fr

[223]

88 Ra [226]

89 Ac** [227]

104 Rf

[261]

105 Db [262]

106 Sg [266]

107 Bh [264]

108 Hs [265]

109 Mt [268]

110

[269]

111

[272]

112

[277]

114

[285]

116

[289]

118

[293]

* LANTHANOIDS

58 Ce

140.12

59 Pr

140.91

60 Nd

144.24

61 Pm [145]

62 Sm

150.36

63 Eu

151.96

64 Gd

157.25

65 Tb

158.92

66 Dy

162.50

67 Ho

164.93

68 Er

167.26

69 Tm

168.93

70 Yb

173.04

71 Lu

174.97

** ACTINOIDS

90 Th

232.04

91 Pa

231.04

92 U

238.03

93 Np [237]

94 Pu [244]

95 Am [243]

96 Cm [247]

97 Bk [247]

98 Cf

[251]

99 Es [252]

100 Fm [257]

101 Md [258]

102 No [259]

103 Lr

[262]

Periodic TableC

HEM

112 – SPRIN

G 2015

71