NEAP_2006

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HSC Trial Examination 2006

Chemistry

This paper must be kept under strict security and may only be used on or after the afternoon of Friday 4 August, 2006 as specified in the Neap Examination Timetable.

General Instructions

Reading time 5 minutes.

Working time 3 hours.

Write using blue or black pen.

Draw diagrams using pencil.

Board-approved calculators may be used.

A data sheet and Periodic Table are provided at the back of this paper.

Total Marks 100

Section I Pages 218

Total marks 75

This section has two parts, Part A and Part B

Part A 15 marksAttempt Questions 115. Allow about 30 minutes for this part.

Part B 60 marksAttempt Questions 1628.Allow about 1 hour and 45 minutes for this part.

Section II Pages 1926

Total marks 25

Attempt ONE question from Questions 2933. Allow about 45 minutes for this section.

Students are advised that this is a trial examination only and cannot in any way guarantee the content or the format of the 2006 Chemistry HSC Trial Examination.

HSC Chemistry Trial Examination

2 TENCHEM_QA_06.FM Copyright 2006 Neap

Section ITotal marks 75

Part A

Total marks 15Attempt Questions 115.Allow about 30 minutes for this part.

Use the multiple-choice answer sheet.Select the alternative A, B, C, or D that best answers the question. Fill in the response oval completely.

Sample:2 + 4 =

If you think you have made a mistake, put a cross through the incorrect answer and fill in the new answer.

If you change your mind and have crossed out what you consider to be the correct answer, then indicate this by writing the word correct and draw an arrow as follows:

(A) 2(B) 6(C) 8(D) 9

A B C D

A B C D

A B C D

correct


Copyright 2006 Neap TENCHEM_QA_06.FM 3

1. What is the systematic name for the monomer from which polyvinyl chloride is built?(A) chloroethene(B) 1,1-dichloroethene(C) 1,2-dichloroethene(D) vinyl chloride

2. Consider the following standard reduction potentials:

Using the above table, which of the following metals is the strongest REDUCING AGENT?(A) Ca(B) Pb(C) Cu(D) Ag

3. In which of the following does the nitrogen have an oxidation state of +4?(A) HNO3(B) NO2(C) N2O(D) NH4Cl

Half-reaction E (V)Ca2+ + 2e Ca 2.87

Pb2+ + 2e Pb 0.13

Cu2+ + 2e Cu +0.34

Ag1+ + e Ag +1.80



4. Consider the following diagram.

Which of the following describes what happens to the concentrations of Ni2+, Cl2 and Cl and themasses of the Ni and Pt electrodes as this galvanic cell spontaneously generates an electric current at25C and 100 kPa?

5. Carbon-14 radioactively decays via the emission of a beta particle. Which of the following is theproduct nuclide of this decay?(A) boron-13(B) carbon-13(C) carbon-14(D) nitrogen-14

6. Which of the following substances would NOT be present in the reaction flask during the preparationof ethyl propanoate?(A) ethanoic acid(B) ethanol(C) propanoic acid(D) sulfuric acid

Concentrationof Ni2+

Concentrationof Cl2

Concentrationof Cl

Mass ofNi electrode

Mass ofPt electrode

(A) decreases increases increases increases decreases(B) increases decreases increases decreases increases(C) decreases no change no change increases no change(D) increases decreases increases decreases no change

V

salt bridge

Pt(s)Ni(s)

1.00 M Ni2+(aq) 1.00 M Cl(aq)

Cl2 (g)



7. An unknown solution is tested with four indicators to determine its pH. The table below shows theresults obtained.

Which of the following statements gives the best range for the pH of the solution?(A) The solution has a pH less than 8.3.(B) The solution has a pH between 6.0 and 8.0.(C) The solution has a pH between 6.4 and 7.6.(D) The solution is neutral (pH = 7).

8. Which of the following species could best be described as amphiprotic?(A) HNO3(B) NH2(C) H2PO4(D) CH3COO

9. Before carrying out a titration between acetic acid, CH3COOH, and potassium hydroxide, KOH, theequipment must be rinsed appropriately.If the acid is to be dispensed from the burette, which of the following indicates the best rinsing procedure?

10. During an experiment, a student measures the pH of a 0.01 mol L1 solution of citric acid to be 3.6, butthe pH of a 0.01 mol L1 solution of hydrochloric acid is 2.0.What is the most likely reason for this difference in pH?(A) Citric acid is a stronger acid.(B) Hydrochloric acid is a stronger acid.(C) Citric acid is triprotic.(D) Hydrochloric acid is more concentrated.

11. Which of the following substances would be least suitable for analysis by atomic absorption spectroscopy?(A) iron(B) sodium(C) nitrogen(D) potassium

Indicator Acidic colour pH range Basic colour Colour inunknown solution

methyl orange red 3.1 4.4 yellow yellowbromothymol blue yellow 6.0 7.6 blue greenphenol red yellow 6.4 8.0 red orangephenolphthalein colourless 8.3 10.0 bright pink colourless

Burette Pipette Conical flask(A) rinsed with CH3COOH rinsed with H2O rinsed with KOH(B) rinsed with H2O rinsed with KOH rinsed with H2O(C) rinsed with H2O rinsed with H2O rinsed with KOH(D) rinsed with CH3COOH rinsed with KOH rinsed with H2O



12. A student wished to analyse the sulfate content of a lawn fertiliser. Which of the following would bethe best reagent to add to a solution of the fertiliser to perform a gravimetric analysis?(A) iron sulfate(B) sodium sulfate(C) barium carbonate(D) barium chloride

13. The following table compares some properties of gaseous oxygen and the oxygen free radical.Which alternative best fits the correct descriptions?

14. Microscopic membrane filters may be used as an alternative to chemical treatment of water.Which of the following is the best reason to use these filters?(A) To remove harmful heavy metals.(B) To remove large particulate matter.(C) To remove fluoride and chloride.(D) To remove harmful microorganisms.

15. A sample of water was collected downstream from a factory producing batteries.The sample was analysed for zinc content using the following method. Standard solutions of zinc were used to prepare a calibration curve. One litre of river water was collected. A 100 mL sample of this water was diluted to 1 L using distilled deionised water. A 50 mL sample of the dilute solution was used to aspirate into an atomic absorption

spectrometer.The following graph was obtained using standard solutions of zinc nitrate.

The absorbance reading of the 50 mL sample of the diluted river water was 1. Which of the followingis closest to the concentration of zinc in the original river water sample?(A) 10 ppm(B) 40 ppm(C) 50 ppm(D) 100 ppm

Gaseous oxygen Oxygen free radical(A) less reactive monatomic more reactive molecular(B) less reactive molecular more reactive monatomic(C) more reactive monatomic less reactive molecular(D) more reactive molecular less reactive monatomic

5 10 15 20 25

1234567

30concentration of Zn (ppm)

absorbance

Calibration graph



Section I (continued)

Part B

Total marks 60Attempt Questions 1627.Allow about 1 hour and 45 minutes for this part.

Answer Part B questions in the spaces provided.Show all relevant working in questions that require calculations.

Marks Question 16 (6 marks)A student assembled the following equipment in order to determine the molar heat of combustionof ethanol.

Experimental results found that the temperature of 100 mL of water increased from 18C to 58Con burning 0.76 g of ethanol.

1(a) Define the term molar heat of combustion.. . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . .

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1(b) Write a balanced chemical equation to show the complete combustion of ethanol.

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2(c) Calculate the molar heat of combustion of ethanol based on the experimental results.

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2(d) Explain how this calculated value would compare to the theoretical value.

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aluminium calorimeter

water

alcohol burnerethanol

thermometerretort stand



MarksQuestion 17 (4 marks)The following flow diagram shows a series of reactions.

1(a) Draw a structural equation to illustrate the production of Q.

1(b) Ethylene can be readily converted into ethane. Give a reason for the presence of a catalystin this reaction.

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2(c) Polyethylene can be used as a cling film. Describe this use in terms of its properties.

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glucose

ethanol

ethylene

polyethylene ethaneQ

fermentation

dehydration

hydrogen and catalyst

liquid bromine

polymerisation



MarksQuestion 18 (3 marks)

On February 1, 2004, the synthesis of the transuranic elements ununpentium andununtrium was reported by Russian and American scientists.

3Describe how transuranic elements such as ununpentium and ununtrium may be synthesised andidentify ONE safe practice which must be adopted when working with radioactive elements suchas these.

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Z 115=( )Z 113=( )



MarksQuestion 19 (5 marks)A new vehicle is said to combine hybrid electric power with the capability of operating on amixture of 15 per cent petrol and 85 per cent ethanol.

Evaluate the likelihood of the success of ethanol as an alternative fuel.

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N102 GVE



MarksQuestion 20 (6 marks)Although the atmosphere naturally contains acidic oxides of carbon, nitrogen and sulfur, the levels of these oxides have been increasing since the industrial revolution.It has been observed that the pH of rainwater is lower near significant sources of these gases.

2(a) Account for the increasing concentration of oxides of nitrogen (NOx) in the atmosphere.. . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . .

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4(b) Explain the formation of acidic solutions from oxides of nitrogen and evaluate reasons forconcern about the effects of acid rain.

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Question 21 (3 marks)

3During the HSC Chemistry course you performed a first-hand investigation in which you identified the pH of a variety of salt solutions. If solutions of NH4Cl and Na2CO3 were used in this task, predict the acidic, basic or neutral nature that you would identify. Justify your prediction, including relevant equations in your answer.

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3(a) Using the graph above, explain the trend observed in the boiling points for molecules of thesame molar mass.

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2(b) Many products found in the supermarket contain acids or esters. Some of these areextracted from natural resources but an increasing number are being synthetically prepared.

Providing specific examples, outline the use of acids and esters in food products.

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50

100

150

200

250

0 20 40 60 80 100 120 140molar mass (g/mol)

boiling point (C)

Boiling points of straight-chained primary alkanols and alkanoic acids

alkanoic acids

alkanols



MarksQuestion 23 (4 marks)The following results were obtained during an investigation involving the decarbonation of twobottles of soda water. Each bottle was opened for a 24-hour period before re-sealing.

1(a) Calculate the volume of carbon dioxide (CO2) gas lost from bottle B at 25C and 100 kPa.

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Question 23 continues on page 14

bottle A bottle B

Initial massof sealed bottle (g) 125.5 125.5

Final massof sealed bottle (g) 125.1 124.8

Change in mass (g) 0.4 0.7Room conditions cold warmVolume of CO2

released at 25C and 100 kPa (mL)

225.3

sodabottle A

sodabottle B



MarksQuestion 23 (continued)(b) In each bottle the following equilibrium process exists:

CO2(g) + H2O(l) H2CO3(aq) + heat

3Explain the difference in the volume of carbon dioxide lost from the two bottles in terms ofLe Chateliers Principle.

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Question 24 (4 marks)

It is well known that safety glasses should always be worn during practicals involving acids since spills and splashes can occur. The corrosive nature of acids can damage workbenches or pose a risk to people working in the lab.A handbook for risk assessment states:To minimise risk, large acid spills should be neutralised with lime (CaCO3) before mopping up.

4Assess this recommended method. . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . .

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MarksQuestion 25 (5 marks)Good up high, bad down low is a statement which has often been made in reference to atmospheric ozone.

3(a) Explain this statement.

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2(b) Use Lewis electron dot structures to demonstrate the formation of the bonds in anozone molecule.




4A student was given a sample of an unknown soluble salt. She suspected the sample containedbarium ions. Describe the procedures she may have used to confirm her suspicion. Include at leastone precaution taken to minimise risk.

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MarksQuestion 27 (5 marks)Lake Upyajumpa is located in a highly-developed farming region and has a factory that utilisesthe lakes water in the production of steel.

A sample was taken from Lake Upyajumpa and tested for water quality. Two of the resultsobtained were:

The reading obtained for DO was very low and vertebrate life within the lake would be in danger.The BOD value was borderline to indicating the lake was polluted.

5Analyse the impact that the local community may have had which could have lead to the results ofDO and BOD obtained.

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Dissolved oxygen (DO): 3 mg L1Biological oxygen demand (BOD): 4.1 mg L1



MarksQuestion 28 (6 marks)In a modern ammonia-producing plant many factors need to be monitored carefully. The following diagram describes the main features of such a plant:

In this production plant, the pressure and temperature are closely monitored for the combination of the reactant gases (in the reactor) and for the removal of the product (in the condenser).

6Explain why the temperature and pressure must be carefully monitored in these chambers.Use appropriate equations to illustrate your answer.

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unreacted N2(g) and H2(g)

N2(g) + 3H2(g) compressorreactor

with a catalyst (400C, 200 atm)

condenser

NH3(l) is stored



Section II

Total marks 25Attempt ONE question from Questions 2933.Allow about 45 minutes for this section.Answer the question in a writing booklet. Extra writing booklets are available.

Show all relevant working in questions that require calculations.

Pages

Question 29 Industrial Chemistry......................................................................20

Question 30 Shipwrecks, Corrosion and Conservation ................................21

Question 31 The Biochemistry of Movement............................................2223

Question 32 The Chemistry of Art .....................................................................24

Question 33 Forensic Chemistry .................................................................2526



MarksQuestion 29 Industrial Chemistry (25 marks)

1(a) (i) Identify the products of the Solvay process.

3(ii) Explain the importance of ammonia in the Solvay process using appropriateequations.

7(b) The chlor-alkali industry is one of the largest in developed countries. It produces chlorine,hydrogen and sodium hydroxide on a commercial scale by an electrolytic process. Analysethe chlor-alkali industrys choice of concentrated salt water (brine) for electrolysis, ratherthan molten sodium chloride or dilute sodium chloride.

(c) Soaps and detergents are both cleaning agents.

2(i) Draw structural diagrams to distinguish between a soap and a cationic detergent.

2(ii) List two different uses of both the soap and the cationic detergent.

3(iii) Account for one of the uses of either the soap or the cationic detergent by specificreference to the soaps or detergents structure.

(d) Sulfuric acid is produced commercially using the contact process but it may be modelled inthe laboratory. One important step is the production of SO3 according to:

2SO2(g) + O2(g) 2SO3(g) H = 196 kJ mol-1

2(i) In one laboratory preparation of SO3 carried out in a 2 L reaction flask the number ofmole of SO2, O2 and SO3 were 0.224, 0.136 and 0.414 respectively at equilibrium.Calculate the value of the equilibrium constant for this reaction.

5(ii) Discuss the relationship between rate of reaction and equilibrium conditions withreference to the production of SO3.



MarksQuestion 30 Shipwrecks, Corrosion and Conservation (25 marks)(a) The ocean represents a massive electrolyte solution. It contains a large quantity of dissolved

minerals and notable levels of dissolved gases such as oxygen and carbon dioxide.

1(i) Identify the effect of increasing ocean depth on the solubility of oxygen andcarbon dioxide.

4(ii) Account for the fact that the relative solubility does not necessarily correspond to theactual concentrations of these gases at increasing depths. Include relevant equationsin your answer.

(b) During your study of this option you performed a first-hand investigation to compare thecorrosion of iron in different temperatures and salt concentrations.

3(i) Outline the procedure you used in this investigation.

3(ii) Justify the appropriateness of the experimental procedure in part (i) to generate validand reliable results and conclusions.

7(c) Describe the process of rusting and analyse and explain the conditions under which therusting of iron occurs.

(d) A student set up the following equipment to gather first-hand data about the factorsaffecting an electrolysis reaction:

1(i) Identify the cathode in this electrolytic cell.

2(ii) Calculate the voltage required for this cell and write the half-equations for thereactions occurring at the anode and cathode.

It is possible to vary the oxidation and reduction processes that take place in an electrolyticcell by altering components of the set up. This includes changing the electrodes used, theconcentration or nature of the electrolyte or changing the electrolyte species altogether.

A student wants to set up an electrolytic cell similar to the one shown in order todemonstrate the effect that some of these changes will have on the overall redox reaction.

3(iii) Describe two specific modifications that could be made to the experimental set upthat would alter the reactions occurring. Predict the changes that would occur.Include relevant half equations and electrode potentials in your answer.

1(iv) Identify one use of electrolysis in the conservation and restoration of artefactssalvaged from ocean wrecks.

power source+

1 M solution of sodium bromide

(NaBr)

platinum electrode (B)

silver electrode (A)



MarksQuestion 31 The Biochemistry of Movement (25 marks)

1(a) (i) ATP is an energy source for metabolic processes. Identify the original energy sourceof the energy secured in the bonds of ATP.

1(ii) Identify the site of the glycolysis in the cell.

4(b) Describe the formation of temporary bonds between actin and myosin fibres during musclecontraction and explain why ATP is consumed in the process.

(c) Use the chart of biochemical pathways shown below to:

4(i) compare the total energy output from glycolysis and the TCA cycle;2(ii) compare the formation of lactic acid with the process of fermentation.

Question 31 and biochemical pathways chart continue on page 23

glucose

NADH + H+

NADH + H+

NAD+ADP + PATP

pyruvic acid

NADH + H+NAD+CO2

acetyl coenzyme A

citric acid C6C6

C6C5C4

C4

C4

C4

C4

C6

NADH + H+

NADH + H+

NAD+

NAD+

NAD+

FAD

FADH2

GDP + PGTPATP

CO2CO2

Carbohydrates

NADH + H+

NAD+ FAD

FADH2

O2 H2O

(ADP + P) ATP

}}

}

Glycolysis

Oxidative decarboxylation

Oxidative phosphorylation

TCA cycle

Enzymes in the cytochrome chain catalyses reactions that release energy to convert ADP + P to ATP.



MarksQuestion 31 (Continued)

7(d) Assess the importance of the compounds NADH and FADH2 in providing energy formuscle contraction.

1(e) (i) Draw a glycerol molecule.

2(ii) Compare the structure of glycerol with the structure of fatty acids.

3(iii) Predict the viscosity and solubility of glycerol compared to fatty acids and explainthe reasons for your predictions.

End of Question 31

glucose

NADH + H+NAD+

NADH + H+

NAD+NADH + H+

NAD+

ADP + PATP

pyruvic acid

lactic acidethanol

+ carbon dioxide

CH3CHOHCOOHC2H5OH

CO2

CH3COCOOH

Fermentation

Anaerobic glycolysis

The anaerobic release of energy

} }



MarksQuestion 32 The Chemistry of Art (25 marks)

1(a) (i) Identify the element which gives a violet (pale purple) flame colour.

3(ii) In your practical work you observed the characteristic flame colours of a range ofmetals. Explain why characteristic flame colours are produced.

2(b) (i) Identify TWO properties of minerals which made them important as pigments toancient cultures.

4(ii) Discuss the potential health risks associated with the use of pigments as cosmeticsby ancient cultures.

7(c) When green CuCl2(s) and white CuSO4(s) are dissolved in water, both produce a pale bluesolution. Explain why this is the case and describe the bonding in the resulting complexion. Include the structural formula of the complex in your answer.

1(d) (i) State the electron configuration of the Zn2+ ion using s, p, d notation.

2(ii) In your practical work you investigated the colours of a transition metal as it changedoxidation state. Name the metal you studied. Identify two oxidation states youinvestigated and their associated colours.

5(iii) Give a detailed account of the method that you used to carry out the investigationreferred to in d(ii) above. Include a risk assessment in your answer.



MarksQuestion 33 Forensic Chemistry (25 marks)

3(a) An HSC Chemistry student had pure samples of cyclohexene, ethanoic acid and ethanolbut did not know which was which. Describe tests that would allow him to distinguishbetween the chemicals.

(b) During your study of this option you performed a first-hand investigation in which youcarried out a chemical test to distinguish between reducing and non-reducing sugars.

2(i) Describe the chemical difference between a reducing and non-reducing sugar.

(ii) The following structure is that of the carbohydrate sucrose:

1Classify sucrose as a reducing or a non-reducing sugar.

2(iii) Outline the procedure you used in this investigation and describe the results thatwere observed.

(c) The table below gives the abbreviations, formulae and isoelectric points of three amino acids.

1(i) Identify the major functional groups in an amino acid.1(ii) Draw the structural formula of a dipeptide that can be made from the amino acids

aspartic acid and valine.

Question 33 continues on page 26

O

OH

HOH

H

H

CH2OH

HOCH2

O

O H

CH2OH

H

OHH

OHHO

HH

Name Abbreviation Structural formula Isoelectric point (pI)

aspartic acid asp 2.95

lysine lys 9.90

valine val 6.00

HOOC C

H

H

C COOH

H

NH2

C(CH2)3 COOHCH2H

NH2NH2

C C CH3H2N

H CH3

COO

H

H



MarksQuestion 33 (Continued)

Gel electrophoresis was carried out on a mixture of the three amino acids shown in the tableon page 25. The electrophoresis was run for 5 hours and the developed gel isillustrated below.

3(c) (iii) Explain the characteristics that allow for the mixture of the three amino acids tobe separated.

1(iv) Identify the amino acid from the table that corresponds to each of the three letters onthe above diagram.

(d) Progress in analytical chemistry and changes in technology have altered forensicinvestigations over time. In particular, advances in DNA analysis have enabled crime sceneinvestigators to draw more accurate conclusions about the identity of individualsimplicated in crimes.

2(i) Describe the structure and composition of DNA.

4(ii) Discuss the issues associated with the uses of DNA analysis in terms of themaintenance of DNA data banks.

5(e) Explain how the emission spectra of elements may assist with the identification of theorigin of a mixture.

End of paper

+

anodecathodestart

DC power supply

A CB

Buffered electrolyte solution of pH 6.


Copyright 2006 Neap TENCHEM_DS_06.FM 27

Data SheetAvogadros constant, NA . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 6.022 1023 mol1

Volume of 1 mole of ideal gas at 100 kPa andat 0C (273.15 K) . . . . . . . . . . . . . . . . . . . . 22.71 Lat 25C (298.15 K. . . . . . . . . . . . . . . . . . . . 24.79 L

Ionisation constant for water at 25C (298.15 K), Kw. . . . . . . . 1.0 1014Specific heat capacity of water . . . . . . . . . . . . . . . . . . . . . . . . . 4.18 103 J kg1 K1

Some useful formulae

pH = log10[H+]

Some standard potentialsK+ + e K(s) 2.94 VBa2+ + 2e Ba(s) 2.91 VCa2+ + 2e Ca(s) 2.87 VNa+ + e Na(s) 2.71 VMg2+ + 2e Mg(s) 2.36 VAl3+ + 3e Al(s) 1.68 VMn2+ + 2e Mn(s) 1.18 VH2O(l) + e H2(g) + OH 0.83 VZn2+ + 2e Zn(s) 0.76 VFe2+ + 2e Fe(s) 0.44 VNi2+ + 2e Ni(s) 0.24 VSn2+ + 2e Sn(s) 0.14 VPb2+ + 2e Pb(s) 0.13 VH+ + e H2(g) 0.00 VSO42 + 4H+ + 2e SO2(aq) + 2H2O 0.16 VCu2+ + 2e Cu(s) 0.34 V

O2(g) + H2O(l) + 2e 2OH 0.40 VCu+ + e Cu(s) 0.52 V

I2(s) + e I 0.54 VI2(aq) + e I 0.62 V

Fe3+ + e Fe2+ 0.77 VAg+ + e Ag(s) 0.80 V

Br2(l) + e Br 1.08 VBr2(aq) + e Br 1.10 VO2(g) + 2H+ + 2e H2O(l) 1.23 VCl2(g) + e Cl 1.36 VCr2O72 + 7H+ + 36e Cr3+ + H2O(l) 1.36 VCl2(aq) + e Cl 1.40 V

MnO4 + 8H+ + 5e Mn2+ + 4H2O(l) 1.51 VF2(g) + e F 2.89 V

H mC T=

12---

12---

12---

12--- 12---

12--- 12--- 12--- 12--- 12--- 72---12---

12---

Per

iod

ic T

able

of

the

Ele

men

ts

Whe

re th

e at

omic

wei

ght i

s no

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the

rela

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ass

of th

e m

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omm

on ra

dioa

ctiv

e is

otop

e is

sho

wn

in b

rack

ets.

Th

e at

omic

mas

ses

of N

p an

d Tc

are

giv

en fo

r the

isot

opes

237 N

p an

d 99

Tc.

1 H1.

008

Hydr

ogen

KEY

2 He

4.00

3He

lium

3 Li6.

941

Lith

ium

4 Be

9.01

2Be

rylli

um

Ato

mic

num

ber

Ato

mic

mas

s

79

Au

197.

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ld

Sym

bo

l of e

lem

ent

Nam

e of

ele

men

t

5 B10

.81

Boro

n

6 C12

.01

Carb

on

7 N14

.01

Nitr

ogen

8 O16

.00

Oxyg

en

9 F19

.00

Fluo

rine

10

Ne

20.1

8N

eon

11

Na

22.9

9So

dium

12

Mg

24.3

1M

agne

sium

13 Al

26.9

8Al

umin

ium

14 Si

28.0

9Si

licon

15 P

30.9

7Ph

osph

orou

s

16 S

32.0

7Su

lfur

17 Cl

35.4

5Ch

lorin

e

18 Ar

39.9

5Ar

gon

19 K

39.1

0Po

tass

ium

20

Ca

40.0

8Ca

lciu

m

21 Sc

44.9

6Sc

andi

um

22 Ti

47.8

7Ti

tani

um

23 V

50.9

4Va

nadi

um

24 Cr

52.0

0Ch

rom

ium

25

Mn

54.9

4M

anga

nese

26 Fe

55.8

5Iro

n

27

Co

58.9

3Co

balt

28 Ni

58.6

9N

icke

l

29

Cu

63.5

5Co

pper

30 Zn

65.4

1Zi

nc

31

Ga

69.7

2Ga

llium

32

Ge

72.6

4Ge

rman

ium

33 As

74.9

2Ar

seni

c

34 Se

78.9

6Se

leni

um

35 Br

79.9

0Br

omin

e

36 Kr

83.8

0Kr

ypto

n

37 Rb

85.4

7Ru

bidi

um

38 Sr

87.6

2St

ront

ium

39 Y

88.9

1Yt

trium

40 Zr

91.2

2Zi

rcon

ium

41

Nb

92.9

1N

iobi

um

42

Mo

95.9

4M

olyb

denu

m

43 Tc

[98.

91]

Tech

netiu

m

44 Ru

101.

1Ru

then

ium

45 Rh

102.

9Rh

odiu

m

46 Pd

106.

4Pa

lladi

um

47

Ag

107.

9Si

lver

48

Cd

112.

4Ca

dmiu

m

49 In

114.

8In

dium

50 Sn

118.

7Ti

n

51 Sb

121.

8An

timon

y

52 Te

127.

6Te

lluriu

m

53 I

126.

9Io

dine

54

Xe

131.

3Xe

non

55 Cs

132.

9Ca

esiu

m

56 Ba

137.

3Ba

rium

5771

Lant

hani

des

72 Hf

178.

5Ha

fniu

m

73 Ta

180.

9Ta

ntal

um

74 W

183.

8Tu

ngst

en

75 Re

186.

2Rh

eniu

m

76

Os

190.

2Os

miu

m

77 Ir

192.

2Iri

dium

78 Pt

195.

1Pl

atin

um

79

Au

197.

0Go

ld

80

Hg

200.

6M

ercu

ry

81 Tl

204.

4Th

alliu

m

82 Pb 207.

2Le

ad

83 Bi

209.

0Bi

smut

h

84 Po

[209

.0]

Polo

nium

85 At

[210

.0]

Asta

tine

86 Rn

[222

.0]

Rado

n

87 Fr

[223

.0]

Fran

cium

88 Ra

[226

.0]

Radi

um

89103

Actin

ides

104

Rf

[261

.1]

Ruth

erfo

rdium

105

Db

[262

.1]

Dubn

ium

106

Sg

[266

.1]

Seab

orgi

um

107

Bh

[264

.1]

Bohr

ium

108

Hs

[277

]Ha

ssiu

m

109

Mt

[268

]M

eitn

eriu

m

110

Ds

[271

]Da

rmst

adtiu

m

111

Rg

[272

]Ro

entg

eniu

m

Lant

hani

des

57 La

138.

9La

ntha

num

58 Ce

140.

1Ce

rium

59 Pr

140.

9Pr

aseo

dymi

um

60

Nd

144.

9N

eody

miu

m

61

Pm[1

46.9

]Pr

omet

hium

62

Sm

150.

4Sa

mar

ium

63 Eu

152.

0Eu

ropi

um

64

Gd

157.

3Ga

dolin

ium

65 Tb

158.

9Te

rbiu

m

66

Dy

162.

5Dy

spro

sium

67

Ho

164.

9Ho

lmiu

m

68 Er

167.

3Er

bium

69

Tm

168.

9Th

uliu

m

70

Yb

173.

0Yt

terb

ium

71 Lu

175.

0Lu

tetiu

m

Act

inid

es89

Ac

[227

.0]

Actin

ium

90 Th

232.

0Th

oriu

m

91 Pa

231.

0Pr

otac

tiniu

m

92 U

238.

0Ur

aniu

m

93

Np

[237

.0]

Nep

tuni

um

94 Pu

[244

.1]

Plut

oniu

m

95

Am

[243

.1]

Amer

iciu

m

96

Cm

[247

.1]

Curiu

m

97 Bk

[247

.1]

Berk

eliu

m

98 Cf

[251

.1]

Calif

orni

um

99 Es

[252

.1]

Eins

tein

ium

100

Fm[2

57.1

]Fe

rmiu

m

101

Md

[258

.1]

Men

dele

vium

102

No

[259

.1]

Nob

eliu

m

103

Lr[2

62.1

]La

wre

nciu

m

NEAP_2006

Documents

Transcript of NEAP_2006