Unit 6: Extra Topics

Unit 6: Extra Topics

Organic Chemistry, Heat, Gases, Rates, Acids and Bases, Nuclear Chemistry

Topic A: Organic Chemistry

1. How many carbon atoms are in each compound?

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Unit 6: Extra Topics

1. Methane ____
2. Ethane ____
3. Ethene ____
4. Pentane ____
5. Propene ____
6. Hexane ____
7. Ethyne ____
8. Propane ____
9. Heptane ____
10. Octane ____
11. Decane ____
12. Butyne ____
13. Butane ____
14. Propyne ____
15. Butene ____

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Unit 6: Extra Topics

1. For each compound fill in each blank:

Number of Carbon atoms Series Formula

1. Methane______
2. Butane______
3. Propyne______
4. Pentane______
5. Octane______
6. Heptene______
7. Propene______
8. Butyne______
9. Decane______
10. Nonane______
11. Heptane______
12. Ethyne______
13. Hexyne______
14. Ethane______

1. How many times does carbon bond and why?
2. For each of the following, draw the structural formula and then name the compound.

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Unit 6: Extra Topics

1. C2H6______
2. C5H10______
3. C6H12______
4. C7H12______
5. C9H20______
6. C2H2______
7. C8H16______
8. C4H8______
9. C10H18______
10. C5H8______
11. C6H14______
12. C9H16______

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Unit 6: Extra Topics

1. For each of the following use tables P and Q to determine the name.

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Unit 6: Extra Topics

1. CH4______
2. C10H20______
3. C3H4______
4. C8H18______
5. C5H12______
6. C9H18______
7. C2H6______
8. C4H6______
9. C7H16______
10. C6H12______

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Unit 6: Extra Topics

Functional Groups

For each of the following identify the functional group and then name the compound using table R.

Organic Reactions

Match the reaction to its name:

___ 1.Additiona. C13H28 C8H18 + C2H4 + C3H6

___ 2.Substitutionb. C3H8 + 5O2 3CO2 + 4H20

___ 3.Combustionc. (C17H35COO)3C3H5 + 3 NaOH C3H5(OH)3 + 3C17H35COONa

___ 4.Crackingd. C6H12O6 C2H5OH +CO2

___ 5.Polymerizatione. n(CH2CH2)  (CH2CH2)n

___ 6.Fermentationf. C2H6 + Cl2 C2H5Cl + HCl

___ 7.Esterificationg. C3H6COOH + C2H5OH  C3H6COOC2H5 + H2O

___ 8.Saponificationh. C3H6 + I2 C3H6I2

Name the reaction:

1. A saturated alkane reacts with fluorine
2. Small alkene chains connect to form larger alkane chains
3. Sugar is decomposed to form an alcohol
4. Large hydrocarbons are heated and break into smaller fragments
5. An unsaturated hydrocarbon reacts with bromine
6. An alcohol and an organic acid are reacted
7. A base is added to a fat molecule to form a soap
8. Hydrocarbons are burned in the presence of oxygen
9. Another name for hydrogenation*
10. Another name for halogenation*

1. Howmanyhydrogenatomsarepresentinonemoleculeofoctane?

2. WriteanIUPACnameofonesaturatedhydrocarbonthatleavesthefractionatingtoweratlessthan40°C.

3. Describetherelationshipbetweenthestrengthoftheintermolecularforcesandthenumberofcarbonatomsinthedifferenthydrocarbonmolecules.

4. Statethetrendbetweentheboilingpointofthehydrocarbonscontainedinthecrudeoilandthenumberof carbonatomsinthesemolecules.

Topic B: Heat

Heat Table I

1. Are the following endo or exothermic?

CH4 + 2O2CO2 + 2H2O_____ 2CH3OH + 3O22CO2 + 4H2O + 1452kJ _____

H2+ I22HI_____The dissolving of NaOH_____

25.69kJ + NH4NO3NH4+ + NO3-_____The dissolving of LiBr_____

2. Circle the more stable compound in each pair:

H2O(g) OR H2O(l)NH3 OR Al2O3

HI OR NOC2H6 OR C2H4

3. Circle the compound which is more likely to form in each pair:

CO2 from elements OR CO2 from CONO OR NO2

C2H6 OR C2H2NH3 OR HI

4. Will the following feel hot or cold?

Dissolving KNO3______Dissolving LiBr ______

Burning CH4 in O2______Forming Al2O3 ______

Specific Heat

Specific heat is defined as the amount of heat (in _____) needed to raise ____ gram of a substance ____˚C. Every substance has its own specific heat depending on the bonds and forces it has.

1. When you wake up in the morning and touch the floor, at first the carpet feels warm. The wood floor in the hallway is a bit chilly, but the tile floor in the bathroom is FREEZING! However, your whole house is probably 68˚F. What quality is different about each of these surfaces? Which has the highest specific heat?

1. At the park, why do you tend to steer clear of metal benches and prefer wooden picnic benches? Which has a lower specific heat?

1. Based on the specific heat values in the table below, why do Al, Cu, Au, Fe and Hg have very low values? (What do they have in common?)

1. Based on your answer to question 2 do you expect wood to have a higher or lower specific heat than these substances and why?

1. Glass is often called an insulator because it has a ______specific heat.

Heat Calculations

Define the following terms with units:

q: ______c: ______

m: ______ΔT: ______

Answer the following questions using the heat formula. Show work with units and significant figures.

1. How many Joules of energy are needed to change the temperature of 100.0 grams of water from 20.0C to 40.0C?

1. How many joules of energy are needed to change the temperature of 15.0 grams of water from 35.0C to 75.0C?

1. How many joules of heat must be released in order to change the temperature of 50.0 grams of air (specific heat 1.01 J/gC) from 35.0C to 25.0C?

______

Base answers to questions 4-5 on the diagram:

1. How much heat is added to change the

substance from the coldest to the warmest

pure liquid state?

1. How much heat will need to be added to the same sample in order to raise the temperature from 20.0C to 40.0C? (Notice this is not on the graph, you must calculate it based on your answers above.)

Heat of Vaporization and Fusion

Heat of Fusion of water: 334 J/g

Heat of Vaporization of water: 2260 J/g

Specific Heat Capacity of gaseous water: 1.84 J/gC

Specific Heat Capacity of liquid water: 4.18 J/gC

Specific Heat Capacity of solid water: 2.09 J/gC

Show all work and answers with three significant figures and proper units. Write the formula(s) you used first then show your work.

1. How many Joules of heat are required to change the temperature of 200.0 grams of solid water from -20.0C to 0.0C?

2. How many Joules of heat are needed to change 200.0 grams of water from solid to liquid?

3. How many Joules of heat are required to change the temperature of 200.0 grams of liquid water from 0.0C to 100.0C?

4. How many Joules of heat are needed to change 200.0 grams of water from liquid to gas?

5. How many Joules of heat are required to change the temperature of 200.0 grams of gaseous water from 100.0C to 120.0C?

6.How many Joules of heat are required to change the temperature of 200.0 grams of solid water from -20.0C to 0.0C and then melt it?

7. How is your answer to question 6 related to your answers to questions 1 and 2?

8. Using the rule you obtained in question 7 and your answers to questions 1-5, how much heat is required to heat 200.0 grams of water from -20.0 to 120.0C?

9. Draw a heating curve to show the phase changes that occurred during the processes described in questions 1-5. Label each segment with the phase(s) on the top of the line and the formula you used to determine the amount of heat added on the bottom of the line. Keep in mind the x axis should be the TOTAL heat used in the reaction and the y axis should be temperature in degrees Celsius.

Additional Questions:

10. How much heat is absorbed by 550.0g block of ice to raise the temperature from -15.0 to 0.0C?

11. How much heat is needed to vaporize 250.0 grams of water?

12. How much heat is released when 25.0 grams of water freezes?

13. Calculate the heat needed to change 50.0 grams of liquid water to gas at 100.0C.

14. Calculate the heat released when 125 grams of liquid water solidifies.

15.How much heat energy must be absorbed to raise the temperature of a 200.0 gram block of ice from -10.0 to 0.0C and then completely melt it to a liquid at the same temperature?

16. How much energy would be required to heat the same 200.0 grams of liquid water in #15 (at 0.0C) to the normal boiling point of water and then vaporize it?

17. If the temperature of the 200.0 grams of steam generated in #16 were heated to a new temperature of 120.0C, how much energy would be absorbed?

18. What is the total amount of energy needed to heat 200.0 grams of ice at -10C to gas at 120.0C?

19. What is the total amount of energy needed to heat 125g of ice at -25C to gas at 135.0C? (Use a heating curve to help you).

20. The heat of vaporization of substance X is 250.0J/g. How much heat is needed to change 10.0 grams of X from liquid to gas?

21. The heat of fusion of substance Y is 125 J/g. How much heat is needed to change 25.0 grams of Y from solid to liquid?

22. The heat of sublimation of substance XY2 is 780.0 J/g. calculate the heat required to sublime 200.0 grams of XY2.

23. Hypothesize a possible heat of sublimation for water and give your reasoning.

Topic C: Gases

KMT is the study of how ideal or ______gases behave. Real gases behave most like ideal gases under ______pressure and ______temperature.

1. Based on the demonstration performed by your teacher, describe how gas molecules behave:

Motion: ______

Collisions: ______

Volume: ______

Attractions: ______

1. How can you get a real gas to behave the LEAST like an ideal gas?
2. Of the following: H2, He, CO2, which would behave least like and ideal gas and why?
3. Which of the gases in question 3 behaves the most like ideal gases/ Why?
4. Compared to other gases, why doesn’t water vapor behave ideally?
5. Why do gases behave the least like ideal gases at low temperatures and high pressures?

Gas Laws

FILL IN THE BLANKS WITH INCREASE(S) OR DECREASE(S).

Boyle’s Law relates pressure and volume. When pressure is increased on a gas at constant temperature, the volume ______. This is an indirect relationship.

1. Pilots suffer from intestinal pain when they fly because at higher altitudes, the pressure is decreased so the air volume in their body ______.
2. Your lungs suck in air when the diaphragm is enlarged. When the diaphragm opens, the lung expands, the volume ______and the pressure ______which allows air in. When the diaphragm collapsed, there is less room so the volume ______and the pressure ______.
3. Scuba divers need to be careful when checking their air tanks. When they descend in the water the water pressure increases and pushes on the tank. The tank air pressure increases and the volume of the air ______. When they ascend to the surface, the pressure decreases and the volume of the gas in their tank and body ______.
4. Why do you ears pop on an airplane? (Hint: the air pressure decreases at high altitudes.) explain in terms of pressure and volume.

Charles’ Law relates volume and temperature. When temperature is increased on a gas at constant pressure, the volume ______. This is a direct relationship.

1. Hot air balloons work based on density changes affected by Charles law. To rise, the temperature is ______and the volume ______to make the density low. To come back down the fire is turned off so the temperature ______and volume ______so the density increases. The balloon is always inflated so the pressure is relatively constant.
2. To un-dent ping pong balls submerge them in hot water. Explain this phenomenon in terms of volume and temperature.
3. A balloon outside in the winter seems to deflate but inside it re-inflates. However the number of gas molecules stays constant. How does that happen? Explain in terms of volume and temperature.

Gay Lussac’s Law relates pressure and temperature. When temperature is increased on a gas at constant volume (in a rigid container), the pressure ______because the gas molecules move more. This is a direct relationship.

1. Drivers need to check the air pressure on their tires during change of seasons. In the winter the temperatures are decreased, the pressure inside the tires is ______and the tires are flat. In the summer temperatures are increased and pressures are______so the tires are swollen. But the volume the tires air can occupy stays the same.
2. Don’t put aerosol spray cans in direct heat or flames because they explode. Explain this phenomenon in terms of pressure and temperature.

Gases Review Questions

1.Whichtermisdefinedasameasureoftheaveragekineticenergyoftheparticlesinasample?

A)temperatureB)pressureC)thermalenergyD)chemicalenergy

2.AtwhichtemperaturewouldatomsofaHe(g)samplehavethegreatestaveragekineticenergy?

A)25°C B)37°CC)273 K D)298K

3.Theaveragekineticenergyofwatermoleculesisgreatestinwhichofthesesamples?

A)10gofwaterat35°CC) 10gofwaterat55°C

B)100gofwaterat25°CD) 100gofwaterat45°C

4.Whichchangeinthetemperatureofa1-gramsampleof waterwouldcausethegreatestincreaseintheaveragekineticenergyofitsmolecules?

A) 1°Cto10°C B)10°Cto1°CC)50°Cto60°C D)0°Cto50°C

5.Whatistheequivalentof0KelvinontheCelsiusscale?

A)–100º B)100ºC)–273º D)273º

6.Thetemperatureofasampleofasubstancechangesfrom10.°Cto20.°C.HowmanyKelvindoesthetemperaturechange?

A)10.B)20.C)283D)293

7.Thetemperature30.KexpressedindegreesCelsiusis
A)243ºCB)–243ºCC)303ºCD)–303ºC

8.Whichtemperatureisequalto+20K?

A)–253ºCB)–293ºCC)253°CD)293°C

9.WhichKelvintemperatureisequalto–73ºC?

A)100 K B) 173K C)200 K D)346 K

10.Asampleofagasiscontainedinaclosedrigidcylinder.Accordingtokineticmoleculartheory,whatoccurswhenthegasinsidethecylinderisheated?

A)Thenumberofgasmoleculesincreases.

B)Thenumberofcollisionsbetweengasmoleculesperunittimedecreases.

C)Theaveragevelocityofthegasmoleculesincreases.

D)Thevolumeofthegasdecreases.

11.UnderwhichconditionsoftemperatureandpressurewouldHebehavemostlikeanidealgas?

A)50Kand 20kPa C)50Kand600kPa

B)750Kand600kPa D)750Kand20 kPa

12.Thekineticmoleculartheoryassumesthattheparticlesofanidealgas

A)areinrandom,constant,straight-linemotion

B)arearrangedinaregulargeometricpattern

C)havestrongattractiveforcesbetweenthem

D)havecollisionsthatresultinthesystemlosingenergy

13.Theconceptofanidealgasisusedtoexplain

A)themassofagassampleC) whysomegasesarediatomic

B)thebehaviorofagassampleD) whysomegasesaremonatomic

14.Underwhichconditionsdoesarealgasbehavemost likeanidealgas?

A)atlowtemperaturesandhighpressures C)atlowtemperaturesandlowpressures

B)athightemperatureshighpressures D) athightemperaturesandlowpressures

15.Twobasicpropertiesofthegasphaseare

A)adefiniteshapeandadefinitevolume

B)definiteshapebutnodefinitevolume

C)nodefiniteshapebutadefinitevolume

D)nodefiniteshapeandnodefinitevolume

16.Anassumptionofthekinetictheoryofgasesisthattheparticlesofagashave

A)littleattractionforeachotherandasignificantvolume

B)littleattractionforeachotherandaninsignificantvolume

C)strongattractionforeachotherandasignificantvolume

D)strongattractionforeachotherandaninsignificantvolume

17.Accordingtothekinetictheoryofgases,whichassumptioniscorrect?

A)Gasparticlesstronglyattracteachother.

B)Gasparticlestravelincurvedpaths.

C)Thevolumeofgasparticlespreventsrandommotion.

D)Energymaybetransferredbetweencollidingparticles.

18.Whenasampleofagasisheatedatconstantpressure,theaveragekineticenergyofitsmolecules

A)decreases,andthevolumeofthegasincreases

B)decreases,andthevolumeofthegasdecreases

C)increases,andthevolumeofthegasincreases

D)increases,andthevolumeofthegasdecreases

19.UnderwhichconditionsoftemperatureandpressurewouldasampleofH2(g)behavemostlikeanidealgas?

A)0°Cand100kPa B)0°Cand300kPa C)150°Cand100kPaD)150°Cand300kPa

20.Arealgasbehavesmorelikeanidealgaswhenthegasmoleculesare

A)closeandhavestrongattractiveforcesbetweenthem

B)closeandhaveweakattractiveforcesbetweenthem

C)farapartandhavestrongattractiveforcesbetweenthem

D)farapartandhaveweakattractiveforcesbetweenthem

21.Arealgasdiffersfromanidealgasbecausethemoleculesofrealgashave

A)somevolumeandnoattractionforeachother

B)somevolumeandsomeattractionforeachother

C)novolumeandnoattractionforeachother

D)novolumeandsomeattractionforeachother

Topic D: Rates

1. In order for a reaction to occur the particles must ______with proper ______and ______. Therefore, the more collisions the reactant particle have, the faster the rate.
2. Recall 5 ways to increase the rate of reaction. Be specific.

1. ______
2. ______
3. ______
4. ______
5. ______

1. Matches have the potential to burn on fire. But they will not without sufficient activation energy. Explain what activation energy means and what type of activation energy the matches need.

Regents Questions

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Unit 6: Extra Topics

1.Whicheventmustalwaysoccurforachemicalreactiontotakeplace?

A)formationofaprecipitate

B)formationofagas

C)effectivecollisionsbetweenreactingparticles

D)additionofacatalysttothereactionsystem

2.Increasingthetemperatureincreasestherateofareactionby

A)loweringtheactivationenergy

B)increasingtheactivationenergy

C)loweringthefrequencyofeffectivecollisionsbetweenreactingmolecules

D)increasingthefrequencyofeffectivecollisionsbetweenreactingmolecules

3.AfterbeingignitedinaBunsenburnerflame,apieceofmagnesiumribbonburnsbrightly,givingoffheatandlight.Inthissituation,theBunsenburnerflameprovides

A)ionizationenergy

B)activationenergy

C)heatofreaction

D)heatofvaporization

4.Asthenumberofeffectivecollisionsbetweenreactingparticlesincreases,therateofreaction

A)Decreases

B)increases

C)remainsthesame

5.Inmostaqueousreactionsastemperatureincreases,theeffectivenessofcollisionsbetweenreactingparticles

A)Decreases

B)increases

C)remainsthesame

6.Giventhereaction: Mg+2H2O Mg(OH)2+H2

Atwhichtemperaturewillthereactionoccuratthegreatestrate?

A)25ºCB)50ºC

C)75ºCD)100ºC

7.A5.0-gramsampleofzincanda50.-millilitersampleofhydrochloricacidareusedinachemicalreaction.Whichcombinationofthesesampleshasthefastestreactionrate?

A)azincstripand1.0MHCl(aq)

B)azincstripand3.0MHCl(aq)

C)zincpowderand1.0MHCl(aq)

D)zincpowderand3.0MHCl(aq)

8.A1.0-grampieceofzincreactswith5millilitersofHCl(aq).Whichoftheseconditionsofconcentrationandtemperaturewouldproducethegreatestrateofreaction?

A)1.0MHCl(aq)at20.°C

B)1.0MHCl(aq)at40.°C

C)2.0MHCl(aq)at20.°

D)2.0MHCl(aq)at40.°C

9.AtSTP,which4.0-gramzincsamplewillreactfastestwithdilutehydrochloricacid?

A)lumpC)bar

B)powderedD)sheetmetal

10.Giventhereaction:

Fe(s)+2HCl(aq) FeCl2(aq) +H2(g)

Inthisreaction,5gramsofpowderedironwillreactfasterthana1-grampieceofsolidironbecausethepowderediron

A)haslesssurfacearea

B)hasmoresurfacearea

C)islessdense

D)D)ismoredense

11.Whichstatementbestexplainstheroleofacatalystinachemicalreaction?

A)Acatalystisaddedasanadditionalreactantandisconsumedbutnotregenerated.

B)Acatalystlimitstheamountofreactantsused.

C)Acatalystchangesthekindsofproductsproduced.

D)Acatalystprovidesanalternatereactionpathwaythatrequireslessactivationenergy.

12.Whichchangewouldmostlikelyincreasetherateofachemicalreaction?

A)decreasingareactant'sconcentration

B)decreasingareactant'ssurfacearea

C)coolingthereactionmixture

D)addingacatalysttothereactionmixture

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Unit 6: Extra Topics

Topic E: Acids and Bases

1.Use Table K and Table L to help you identify the rules for determining whether a substance is an acid, a base, or a salt based on the formula. Underline all the acids, circle bases, and box in salts. Leave the covalent substances alone.

NH3NaClCH3OHH2SO4Ca(OH)2CH4

NH4BrHClNa2SO4HNO3CH3COOHNaOH

H3PO4LiOHCH2(OH)2NH4OHCa(NO3)2HC2H3O2

• All acids have the ______ion in common.
• All bases have the ______ion in common.
• All salts have formulas: ______
• All other compounds have formulas: ______
• Organic acids have the general formula: ______

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Unit 6: Extra Topics

2.Which formula represents a hydronium ion?

(1) H3O+(2) OH– (3) NH4+ (4) HCO3–

3.Which compound is an Arrhenius acid?

(1) H2SO4 (2) NaOH (3) KCl (4) NH3

4.Which substance is an Arrhenius acid?

(1) Ba(OH)2 (2) H3PO4 (3) CH3COOCH3(4) NaCl

5.Which compound releases hydroxide ions in an aqueous solution?

(1) CH3COOH (2) HCl (3) CH3OH (4) KOH

6.The Arrhenius theory explains the behavior of

(1) acids and bases

(2) alcohols and amines

(3) isomers and isotopes

(4) metals and nonmetals

7.Which two compounds are electrolytes?

(1) C6H12O6 and CH3CH2OH

(2) C6H12O6 and HCl

(3) NaOH and HCl

(4) NaOH and CH3CHOH

8. Given the equation:

HCl(g) + H2O(l)→X(aq) + Cl−(aq)

Which ion is represented by X?

(1) hydroxide (3) hypochlorite

(2) hydronium (4) perchlorate

9.When one compound dissolves in water, the only positive ion produced in the solution is H3O+(aq). This compound is classified as

(1) a salt (2) a hydrocarbon

(3) an Arrhenius acid(4) an Arrhenius base

10.An aqueous solution of lithium hydroxide contains hydroxide ions as the only negative ion in solution. Lithium hydroxide is classified as an

(1) aldehyde(3) Arrhenius acid

(2) alcohol (4) Arrhenius base

11.Which compound is an Arrhenius acid?

(1) H2SO4 (3) NaOH

(2) KCl (4) NH3

12.An Arrhenius base yields which ion as the only negative ion in an aqueous solution?

(1) hydride ion (3) hydronium ion

(2) hydrogen ion (4) hydroxide ion

13.Which two formulas represent Arrhenius acids?

(1) CH3COOH and CH3CH2OH

(2) HC2H3O2 and H3PO4

(3) KHCO3 and KHSO4

(4) NaSCN and Na2S2O3

14.According to the Arrhenius theory, an acid is a substance that

(1) changes litmus from red to blue

(2) changes phenolphthalein to pink

(3) produces hydronium ions as the only

positive ions in an aqueous solution

(4) produces hydroxide ions as the only

negative ions in an aqueous solution

15.Which formula represents a hydronium ion?

(1) H3O+ (2) OH–(3) NH4+ (4) HCO3–

16.Which substance is an Arrhenius acid?

(1) Mg(OH)2 (2) H2SO4 (3) CH3COOCH3 (4) LiCl

17.Which compound releases hydroxide ions in an aqueous solution?

(1) CH3COOH (2) HF (3) CH3OH (4) LiOH

18.Which substance is an Arrhenius base?

(1) CH3OH (2) LiOH (3) CH3Cl (4) LiCl

19.The only positive ion found in H2SO4(aq) is the

(1) ammonium ion (3) hydronium ion

(2) hydroxide ion (4) sulfate ion

20.Which substance, when dissolved in water, forms a solution that conducts an electric current?

(1) C2H5OH (3) C12H22O11

(2) C6H12O6(4) CH3COOH

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Unit 6: Extra Topics

Strong or Weak, Concentrated or Dilute?

Directions: For each case, decide if the picture shows a weak or strong, and concentrated or dilute solution.

Acid: H+ ion: Anion A-:

5. What does concentrated mean in terms of amount of particles? ______

6. What does dilute mean in terms of amount of particles?______

7. What does strong mean in terms of ions? ______

8. What does weak mean in terms of ions? ______

The pH Scale

The pH scale is a measure of the H+ or H3O+ concentration in a solution. “pH” stands for “potential to ATTRACT Hydrogen ions”“potential to ATTRACT Hydrogen ions

Acids have a LOW pH (a LOW potential to attract H+ ions (release/DONATE H+)

Bases have a HIGH pH (a HIGH potential to attract H+ ions (bases are H+ acceptors)

The pH scale is logarithmic, which means that a change of one pH unit will change the concentration of H+ by a factor of 10.

4. Complete the table below using the grid above:

5. Using the table you created, complete the rules for pH of acids and bases:

1. Acids have pH values in the range of ___ to ___ and hydronium ion concentrations between ______and ______.
2. Bases have pH values in the range of ___ to ___ and hydronium ion concentrations between ______and ______.
3. To obtain the pH of an acid or base, find the ______of the hydronium concentration. Therefore, pH can also be known as the “power” of the hydronium concentration.

6. Find the pH of the following solutions and determine if its acidic or basic:

7. Circle one to complete the table:

Indicators

Table M

Ex: If you add bromthymol blue… to a solution with a pH of 8, it will be blue

to a solution with a pH of 6, it will be green

to a solution with a pH of 4, it will be yellow

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Unit 6: Extra Topics

1. Which indicator, when added to a solution, changes color from yellow to blue as the pH of the solution is changed from 5.5 to 8.0?

(1) bromcresol green

(2) bromthymol blue

(3) litmus

(4) methyl orange

2. Which indicator would best distinguish between a solution with a pH of 3.5 and another with a pH of 5.5?

(1) bromthymol blue (3) litmus

(2) bromcresol green (4) thymol blue

3. In which solution will bromcresol green appear blue?

(1) 1 M NaCl(3) 1 M NH3

(2) 1 M H2CO3(4) 1 M CH3COOH

4. In which solution will thymol blue indicator appear blue?

(1) 0.1 M CH3COOH(3) 0.1 M KOH

(2) 0.1 M HCl(4) 0.1 M H2SO4

5. What is the color of the indicator methyl orange in a solution that has a pH of 2?

(1) blue(3) yellow

(2) orange(4) red

6. In a solution with a pH of 3, what color is bromcresol green?

(1) yellow(3) green

(2) blue(4) red

7. At what pH will bromothymol blue be yellow and bromocrescolgree be blue?

(1) 10.5(2) 5.7 (3) 7.0

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Unit 6: Extra Topics

Topic G: Nuclear Chemistry

Use Table O to fill in the chart:

Writing Nuclear Equations – Use Table N! When elements undergo radioactive decay, they change from one element to another. This happens by losing high energy alpha or beta particles, or by emitting positrons. The process of an atom becoming a different atom is called transmutation. Nuclear equations are written to track the changes that occur during transmutation. When writing nuclear equations, it is important to make sure that mass and charge are conserved. Write the complete nuclear equation for the spontaneous decay of the following nuclides: