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Spring Chemistry Resources

Use these to help you do problems, and on most tests and quizzes. You will have to add your own notes for certain resources.

Unit 5 Resources – Hydrocarbons and Organic Chemistry

Straight Chain Alkanes (Parent Groups) Name Formula Condensed Structural Formula

Methane CH4 CH4

Ethane C2H6 CH3CH3

Propane C3H8 CH3CH2CH3

Butane C4H10 CH3CH2CH2CH3 OR: CH3(CH2)2CH3

Pentane C5H12 CH3(CH2)3CH3

Hexane C6H14 CH3(CH2)4CH3

Heptane C7H16 CH3(CH2)5CH3

Octane C8H18 CH3(CH2)6CH3

Nonane C9H20 CH3(CH2)7CH3

Decane C10H22 CH3(CH2)8CH3

Side Chain Groups (Alkyl Substituents)

Name Methyl Ethyl Propyl Isopropyl Butyl

Condensed Structural Formula

-CH3 CH3CH2- CH3CH2CH2- CH3CHCH3 |

CH3(CH2)3-

Structural Formula

Line Structure:

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Putting the FUN in Functional Groups! Resource Note: “R” stands for any carbon chain or substituent.

Functional Groups with Halogens: Fluoro-, Chloro-, Bromo-, Iodo- Halogen Examples:

2-fluoropentane 2,3-dichloropentane 1-bromo-3-iodobenzene Functional Groups with Nitrogen: Amines Primary Secondary Tertiary

Amine Example:

2-butylamine

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Functional Groups with Oxygen:

Compound Type:

Alcohol Ether Aldehyde Ketone Carboxylic Acid

General Structural Formula

Functional Group

Hydroxyl Ether Carbonyl Carbonyl Carbonyl

Line Structure Appearance

Alcohol Ex: Ether Ex:

2-butanol Diethyl ether Aldehyde Ex: Ketone Ex: heptanal 3-hexanone

Carboxylic Acid Ex:

butanoic acid

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Unit 5 Test Review The following questions will be on the review, and many will be on your exam.

What is an isomer? Which elements are the halogens? What is a functional group? Name three. What is a saturated hydrocarbon?

Is this a saturated hydrocarbon? What is a polymer? Draw an example of a saturated hydrocarbon. Draw two isomers for the formula C4H8.

How many hydrogen atoms on: Draw: 1,2-dibromobenzene Draw: 3,4-diethyl-5-methyloctane. All Play: build an unsaturated hydrocarbon.

What functional group is shown? Which element was used in saturated oil research? What functional group is shown? Is Ca(HCO3)2 a hydrocarbon? Which functional group has nitrogen?

What functional group is shown? Draw: isopropyl btyl ether All Play! Build 3 – hexanol Build: 2,4-decanedione Draw: pentanal How many hydrogen atoms in 2-propanol? All Play! Build: hexanoic acid What is a parent chain? What is a "pie bond"? What type of bonds does 'alkyne' signify? What type of bonds does 'alkane' signify? What is a "pi bond"? What type of bonds does 'alkene' signify?

Name: Name: Name: Name:

Name: All Play! Name: Name:

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Which fat has a longer shelf life, saturated or unsaturated? Describe Frederich Kekule's dream. What is a 'parent ring’? What is a thermosetting polymer? What is a thermoplastic polymer? What is Ouroboros? Draw 2 - hexanol Draw: 1,2,3,4,5-pentafluorononane All Play! Build: ethyl methyl ether. All Play! Build: 2-chloro-1-butanoic acid What specifically does the term 'carbonyl' signify? Draw any polyaromatic compound. Unit 5 Notes: .

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Unit 6 Resources – Chemical Reactions

Table of Ions Resource Cations

1+ Ammonium, NH4

+ Cesium, Cs+ Copper (I), Cu+ Hydrogen, H+ Lithium, Li+

Potassium, K+ Silver, Ag+ Sodium, Na+

2+ Barium, Ba2+ Beryllium, Be2+ Cadmium, Cd2+ Calcium, Ca2+ Chromium (II), Cr2+ Cobalt (II), Co2+ Copper (II), Cu2+ Iron (II), Fe2+ Lead (II), Pb2+ Magnesium, Mg2+ Nickel, Ni2+ Strontium, Sr2+ Tin (II), Sn2+ Zinc, Zn2+

3+ Aluminum, Al3+ Chromium (III), Cr3+ Cobalt (III), Co3+ Iron (III), Fe3+

Manganese (III), Mn3+

4+ Chromium (IV), Cr 4+ Lead (IV), Pb4+ Tin (IV), Sn4+

Anions

1- Acetate, C2H3O2

-

Bromide, Br- Bromate, BrO3

- Chlorate, ClO3

- Chlorite, ClO2

- Chloride, Cl- Cyanide, CN- Dihydrogen Phosphate, H2PO4

-

Fluoride, F- Hydrogen Carbonate OR Bicarbonate, HCO3

-

Hydrogen Sulfate, HSO4

-

Hydroxide, OH- Hypochlorite, ClO- Iodide, I- Iodate, IO3

- Nitrate, NO3

-

Nitrite, NO2-

Permanganate, MnO4-

Perchlorate, ClO4-

Periodate, IO4-

2- Carbonate, CO3

2- Chromate, CrO4

2- Dichromate,Cr2O7

2- Hydrogen Phosphate, HPO4

2- Manganate, MnO4

2- Oxide, O2- Oxalate, C2O4

2- Peroxide, O2

2- Selenide, Se2- Sulfate, SO4

2- Sulfide, S2- Sulfite, SO3

2-

Tartrate, C4H4O62-

Thiosulfate, S2O32-

3- Arsenate, AsO4

3- Arsenide, As3- Borate, BO3

3- Nitride, N3- Phosphate, PO4

3- Phosphide, P3- Diatomic Elements

H2 N2 O2 F2 Cl2 Br2 I2

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Reactivity Series Resource – Only for Single Replacement Reactions! Metals Halogens F2 Cl2 Br2 I2

Table of Solubilities Resource s = insoluble aq = soluble – = reacts with water blank = no data

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Unit 6 Smartboard Review Problems Take 15 Minutes to answer these, then we’ll battle it out on the Smartboard!

List four signs that a chemical reaction has occurred. What happens for a metal atom to become a cation? Which are the seven diatomic elements? What is the formula for dinitrogen trioxide? What is the formula name of CaCl2? Define spectator ion. Write 2 H2SO4(aq) as it would appear in a complete ionic equation. What ar three signs that a double replacement reaction has occurred? Define skeleton equation. Is burning paper a chemical change? Why or why not? List three acids. What are the two products of an acid/base reaction? List three bases. What ion makes an acid an acid? What ion makes a base a base? Balance These ___CuCl2 + ___NaOH ___Cu(OH)2 + ___NaCl ____ NH4NO3 ___ N2O + ____ H2O ____CH4 + ____O2 ____CO2 + ___H2O ___ HCl + ___NaOH ____H2O + ___NaCl ___Li + ___H2O ___LiOH + ___H2 _____Na + ____Cl2 ____ NaCl What type of reaction is: AX + BY AY + BX What type of reaction is: AB A + B What type of reaction is: HA + BOH BA + H2O (HOH) What type of reaction is: A + B AB What type of reaction is:  A + BX AX + B What type of reaction is: CxHy + O2 CO2 + H2O List three monatomic ions List three polyatomic ions Which are the spectator ions in: AgNO3(aq) + HCl(aq) --> AgCl(s) + HNO3(aq) Balance this:

Is aluminum bromide soluble or insoluble? What is an endothermic reaction? How is a coefficient different from a subscript? Is calcium phosphate soluble or insoluble? What does insoluble mean? What is an exothermic reaction? What does soluble mean?

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Unit 6 Test Review- Balancing Reactions Practice 1) ____ Br2 + ____ LiF ____ LiBr + ____ F2

2) ____ H3PO4 + ____ Fe(OH)2 ____ H2O + ____ Fe3(PO4)2

3) ____ C3H7OH + ____ O2 ____ CO2 + ____ H2O

4) ____ Ni(OH)3 ____ Ni2O3 + ____ H2O

5) ____ K2SO3 + ____ Mn(OH)2 ____ KOH + ____ MnSO3

6) ____ NaOH + ____ H2SO4 ____ H2O + ____ Na2SO4

7) ____ Li + ____ Pb(OH)2 ____ Pb + ____ LiOH

8) ____ C4H8 + ____ O2 ____ CO2 + ____ H2O

9) ____ Ga(OH)3 + ____ KF ____ KOH + ____ GaF3

10) ____ V + ____ ZnBr2 ____ VBr3 + ____ Zn

11) ____ As2O5 + ____ H2O ____ H3AsO4

12) ____ NH3 + ____ O2 ____ NO + ____ H2O

13) ____ C3H8 + ____ O2 ____ CO2 + ____ H2O

14) ____ NaClO3 ____ NaCl + ____ O2

15) ____ Ca + ____ O2 ____ CaO

Unit 6 Notes:

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Unit 7 Resources – The Mole & Stoichiometry Mole Calculations Resource

Particles to Moles:

MolesParticles 23 E 6.02

Mole 1 Particles =×

Moles to Particles:

ParticlesMole 1

Particles 23 E 6.02 Moles =×

Particles can be atoms, formula units, molecules, ions, electrons, or anything countable. Molar Mass: 1. Assume that you have one mole of compound.

2. Write the formula of your compound. 3. List each element in the compound, as well as how many moles of each element in the

compound. 4. Multiply the moles of each element by that element’s molar mass (in grams). 5. Add all the masses together. (Units = g/mol)

Example: Find the molar mass of sulfuric acid.

1. I have one mole of sulfuric acid. 2. Formula = H2SO4

3. Hydrogen: H = 2 moles

Sulfur: S = 1 mole Oxygen: O = 4 moles

4. Hydrogen: H = 2 moles · 1.01 g/mol = 2.02 g

Sulfur: S = 1 mole · 32.07 g/mol = 32.07 g Oxygen: O = 4 moles · 16.00 g/mol = 64.00 g

5. Molar mass = 98.09 g/mol H2SO4

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Moles to Mass: (g) Mass Sample

mole 1(g) MassMolar Moles =×

Example: How many grams is in 3.0 moles of manganese? Mass to Moles:

Moles(g) MassMolar

Mole 1 (g) Mass =×

Example: How many moles of calcium are there in 70.5 g of calcium? Particles to Mass:

(g) Mass SampleMole 1

(g) MassMolar Particles 23 E 6.02

Mole 1 Particles =××

Example: How many atoms in 15.0 grams of sulfur?

Mass to Particles:

ParticlesMole 1

Particles 23 E 6.02 (g) MassMolar

Mole 1 (g) Mass =××

Example: How many grams in 2.12 E 24 atoms of gold?

Au grams 694 Au mole 1

Au grams 196.97Au atoms 23 E 6.02

Au mole 1Au atoms 24 E 2.12 =∗∗

S atoms E23 2.82 S mole 1

atoms 23 E 6.02S g 32.07S mole 1 S g 0.51 =∗∗

Ca mol 1.759 Ca g 40.078

Ca mole 1Ca g 70.5 =∗

Mng165Mnmol1

g54.93Mnmol3.0 =∗

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Stoichiometry Calculations Resource Mole Ratio: A ratio of any two chemicals from a balanced equation. Basic Stoichiometric Procedure: Mass Known Moles Known Mole Ratio Moles Seeking Mass Seeking

(Seeking) Mass (Seeking) Mole 1

(Seeking) Mass Mol.(Known) Moles(Seeking) Moles

(Known) Mass Mol.(Known) Mole 1 (Known) Mass =×××

Known chemical = what you’re given in the problem (or the limiting reactant). Seeking chemical = what you’re looking for. Limiting Reactant: Procedure:

1. Balance the reaction. 2. Calculate how many moles of reactants you have in your problem. 3. Make a ratio of moles of reactants from your problem, and then make a proportion so that the moles of the denominator’s reactant equals one mole.

Example:

2Reactant Of Mole 11Reactant Of Moles 1.6

2Reactant Of Moles 0.51Reactant Of Moles 0.8

Proportion Ratio

=

↓↓

4. Make a mole ratio of reactants from the balanced equation, so that the same reactant is on top as from your proportion. If necessary, make a proportion so that you have a 1 in the denominator. 5. Compare the two proportions If reactant 1 of your problem’s ratio is greater than reactant 1 of the balanced reaction’s ratio, then reactant 1 is in excess. If not, it is limiting.

Once you determine what the limiting reactant is, you can use stoichiometry to figure out: A. Amount of product formed. B. The amount of excess reactant left. Remember: Always start with your LIMITING REACTANT to calculate product formed and reactant left over.

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Percent Yield. This is determined by the following equation:

100% X Yield lTheoreticaYield alExperimentYieldPercent =

Where: Experimental Yield is the amount of product actually generated during a reaction. Theoretical Yield is the amount of product possible in ideal laboratory conditions. You must calculate this using stoichiometry, starting with the amount of a limiting reactant.

Hydrated Compound Prefixes Resource

Unit 7 Test Review Questions

Moles / Mole Ratios How many particles are there in 2.4 moles of gold? All Play You have 415 grams of silver chloride. How many formula units of silver chloride do you have? (Two step process). How many moles is 2.4 E 22 formula units of zinc chloride? When would a mole ratio be used? All Play: How many moles of carbon are there in one mole of Na2C7H22O2Cl? How many individual atoms are there in 2 moles of water? All Play: What mole ratio would you use to go from copper to silver in the following skeleton reaction? Write out any units you use: Cu + AgNO3 = Ag + Cu(NO3)2.

Mass & Stoichiometry All Play: What is the mass percent of sodium in sodium oxide? If you have 28.0 grams of boron, how many moles is that? All Play: How many grams of HCl would be needed to react with 15 grams of zinc, according to the reaction: 2 HCl + Zn = ZnCl2 + H2?

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What is the molar mass of calcium chloride? How much mass does two moles of sodium chloride have? All Play: What is the molar mass of lead (IV) nitrate?

Formulas & Limiting Reactants What is the percent by mass of chlorine in sodium chlorate, NaClO3? All Play: At the start of a reaction there is 8.5 mol X to 11.8 mol Y. Ideally, one would have a ratio of 3 mol X to 4 mol Y. Which is the limiting reactant, X or Y? Write the empirical formula for the following: Na2C8H16O4N4 All Play If the empirical formula of a compound is CH2O, and its molar mass is 180.18, what is the molecular formula? All Play What is the empirical formula of a compound that is 82.22% nitrogen and 17.78 % hydrogen?

Hydrated Compounds / Percent Yield Write the formula of barium hydroxide octahydrate. Name MgSO4

. 7 H2O. All Play: If a reaction has a % yield of 55%, how many grams of product would you get from 512 g of reactant? All Play If 0.0023 moles of copper (II) sulfate are connected to 0.0113 moles of water, what is the formula of the hydrate? Write the formula of sodium carbonate decahydrate. Describe a use for a desiccant. Unit 7 Notes:

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Unit 8 Resources – Solutions & Acids and Bases

Unit 8.A: Molal Boiling Point Elevation Constants (Kb) Solvent Boiling Point (°C) Kb (°C/m) Water 100.0 0.512

Benzene 80.1 2.53 Carbon Tetrachloride 76.7 5.03

Ethanol 78.5 1.22 Chloroform 61.7 3.63

Unit 8.A: Molal Freezing Point Depression Constants (Kf)

Solvent Freezing Point (°C) Kf (°C/m) Water 0.0 1.86

Benzene 5.5 5.12 Carbon Tetrachloride -23.0 29.8

Ethanol -114.1 1.99 Chloroform -63.5 4.68

Unit 8.B: Common Acids Resource

The three acids in boldface are the most common acids. Acetic acid (vinegar) CH3COOH Weak Carbonic acid H2CO3 Weak Chloric acid HClO3 Weak Chlorous acid HClO2 Weak Hydrobromic acid HBr Strong Hydrochloric acid HCl Strong Hydrocyanic acid HCN Weak Hydrofluoric acid HF Weak Hydroiotic acid HI Strong Hydrosulfuric acid H2S Weak Nitric acid HNO3 Strong Nitrous acid HNO2 Weak Phosphoric acid H3PO4 Weak Sulfuric acid H2SO4 Strong Sulfurous acid H2SO3 Weak

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Unit 8.B: Common Bases Resource Strong Bases

Barium Hydroxide Ba(OH)2 Beryllium Hydroxide Be(OH)2 Calcium Hydroxide Ca(OH)2 Lithium Hydroxide LiOH Magnesium Hydroxide Mg(OH)2 Potassium Hydroxide KOH Sodium Hydroxide NaOH Strontium Hydroxide Sr(OH)2

Weak Bases All others, including: Aluminum Hydroxide Al(OH)3 Ammonium Hydroxide NH4OH Copper (I) Hydroxide CuOH Copper (II) Hydroxide Cu(OH)2 Iron (II) Hydroxide Fe(OH)2 Iron (III) Hydroxide Fe(OH)3 Zinc Hydroxide Zn(OH)2

Unit 8 – Solutions & Acids and Bases Test Review Questions Give an example of a homogeneous mixture. What is a colloid? What happens to a thixotropic mixture when it is agitated? Give an example of a suspension. List two miscible liquids. Give an example of a heterogeneous mixture. What is the molar concentration if 0.5 moles KCl are dissolved and made into 2.0 L? How many liters of 2.0 M solution could you make with 12 moles of solute? What is the volume percent of 30 mL alcohol in 140 mL total? What is the molar concentration if 2.5 moles NaCl are dissolved and made into 15 L? What is the percent by mass of a mixture of 15 grams sodium chloride in 140 grams of water? How many grams NaCl would have to be dissolved to make 1.0 L of 0.5 M concentration? Which is more concentrated, a 5.0 M solution of NaCl or a 6.0 M solution of LiCl? List two immiscible liquids. Is salt a solute or solvent in water? What is a stock solution? Which is a polar compound, water or methane? List three ways of speeding solvation. What is the solubility of a gas at 15.8 atm, if its initial solubility at 4 atm is 2.8 g/L? How many mL of a 6.0 M stock solution are needed to make 150 mL of 0.6 M dilute solution? If the freezing point depression of an aqueous salt solution is 3.4 oC, what's the actual freezing point? What is the concentration of 100 mL of a dilute solution made from 13 mL of a 4.0 M solution?

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Which water solution has a lower freezing point: 1 L with 1 mole of NaCl, or 1 L with 1 mole of CaCl2 in it? Which water solution has a lower freezing point: 1 L with 1 mole of NaCl, or 1 L with 1 mole of sugar in it? What is boiling point elevation? What polyatomic ion do all bases contain? What is a supersaturated solution? Are acids tart or bitter? What do Arrhenius acids contain? What is freezing point depression? What is the pH of a 0.023 M H2SO4 solution? What is the pH range of acids? How many ionizable hydrogen are there on phosphoric acid? How many ionizable hydrogen are there on sulfuric acid? What is the pH and pOH of a 0.053 M HCl solution? How many ionizable hydrogen are there on vinegar? Name two monoprotic acids. Why is ammonia, NH3 not an Arrhenius base? What makes an acid strong? What is hydrolyzation? What is the pOH of a neutral solution? Name two diprotic acids. Will K2SO4 be an acidic, basic, or neutral salt? What is the pOH of a solution with pH of 9.2? How many hydronium ions could carbonic acid produce? What is the pH of a solution with pOH of 2.2? What is the concentration of a HCl solution with pH of 3.2? Will Na2CO3 be an acidic, basic, or neutral salt? What tool is used to conduct titrations? What can be used to tell when the end point of a titration is reached? What do you neutralize an acid spill with? What are two products of a neutralization reaction? What kind of salt will a strong base and weak acid make? What is titration? Write and balance the reaction of HCl and Ba(OH)2. 25 mL of 0.25 M H2SO4 neutralizes 50 mL of NaOH. What is the concentration of NaOH? What are the names and formulas of the parent acid and base of lithium chloride? Write and balance the reaction of H2SO4 and Ba(OH)2. 15 mL of 1.2 M HCl neutralizes 50 mL of NaOH. What is the concentration of NaOH? Unit 8 Notes:

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Unit 9 Resources – Redox Reactions and Electrochemistry

Assigning Oxidation Numbers Resource: 1. Pure elements (even diatomic ones) have a charge of 0. 2. Oxide = -2 when an oxide, but in peroxide (O2

2-) = -1. 3. Fluoride is always -1. 4. A. First group metals including hydrogen has a charge of +1.

B. Second group metals have a charge of +2. 5. The hydride ion has a charge of -1. (Ex: NaH) 6. The sum of oxidation numbers in neutral compounds is 0. 7. The sum of oxidation numbers in a polyatomic ion is equal to its charge.

Reduction Potentials Resource

Unit 9 Notes:

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Spring Semester Review Problems Chemistry Final Exam Review – These are conceptual problems only. You will also be accountable for mathematical ones – during your review, make sure to practice this type of problem as well. Answers are at the end of the questions. Unit 5 Hydrocarbons and Organic Chemistry 1. What is a hydrocarbon? 2. What is an organic compound? 3. What is distillation? 4. What is an alkane? . 5. How many carbon atoms does hexane have? 6. What is a substituent group? 7. What is a parent chain? 8. What are alkenes? 9. What are alkynes? 10. What is a saturated fat? 11. What is a structural isomer? 12. What is a polymer? 13. What does the prefix “cyclo” mean in organic chemistry? 14. How many carbon atoms are in 1-methyl cyclooctene? 15. How is benzene a special cyclic hydrocarbon? 16. Draw the structure of benzene. 17. What elements could make for a halogenated functional group? 18. Draw an example of a ketone. 19. Draw an example of an alcohol. 20. Draw an example of an ether. Unit 6 – Chemical Reactions 21. What are three of the five signs that a chemical change may have occurred? 22. What does aqueous mean? 23. What is a skeleton equation? 24. What is a synthesis reaction? 25. What are the products of a combustion reaction? 26. What is a single replacement reaction? 27. List two ions that will always be soluble. 28. What is a precipitate? 29. What is a spectator ion? Unit 7– The Mole and Stoichiometry 30. How many particles are in a mole? 31. List two types of particles. 32. What is molar mass? 33. How many atoms are in one formula unit of CaCO3? 34. How many moles of oxygen are there in one mole of H2SO4? 35. What is percent composition? 36. What is empirical formula?

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37. What is molecular formula? 38. What is a hydrate? 39. How many water units are there in a “tetrahydrate”? 40. What is stoichiomentry? 41. What is a mole ratio? 42. What is a limiting reactant? 43. What is an excess reactant? 44. Why would a chemist use an excess reactant? 45. What is a theoretical yield? 46. What is the actual yield of a reaction? Unit 8 – Solutions & Acids and Bases 47. What is a heterogeneous mixture? 48. What is a suspension? 49. What is a colloid? 50. What is a solvent? 51. What is a solute? 52. In chemistry, what is concentration? 53. What type of concentration would you use when both solute and solvent are liquids? 54. What is the definition of molarity? 55. What is a stock solution? 56. What is the dilution equation? 57. What are two ways you could increase the rate of solvation of a solid in water? 58. What is a supersaturated solution? 59. What is a saturated solution? 60. What is an electrolyte? 61. What is boiling point elevation? 62. What is freezing point depression? 63. What does an Arrhenius acid contain? 64. What is a polyprotic acid? 65. What is a strong acid? 66. List three strong acids. 67. List two weak acids. 68. List three strong bases. 69. Will an acid have a high or low pH? 70. What is pOH? 71. What do you neutralize an acid spill with? 72. What is titration? 73. What is a way of determining the end point of a titration? Unit 9 – Redox Reactions & Electrochemistry 74. What is oxidation? 75. What is reduction? 76. What is a redox reaction? 77. What is an oxidizer? 78. What is a reducer?

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79. What is the oxidation number of a pure element? 80. What is the oxidation number of the elements in CO2? 81. Can you have an oxidation without a corresponding reduction? 82. What is electrochemistry? 83. How is a voltaic cell made? 84. What does red-cat-positive mean in an electrochemical cell? 85. What does the following notation tell: Zn│Zn2+║Cu2+│Cu? 86. What is a primary battery? 87. What is a secondary battery? 88. What is the electrolyte in a dry cell battery? 89. Name an example of a secondary battery. 90. What are the reactants of a fuel cell? 91. What is corrosion? 92. What is galvanization? 93. What is electrolysis? 94. What are the products of the electrolysis of water? 95. What are the products of a Down’s Cell? 96. What are the products of the electrolysis of brine? 97. In electroplating, will the cathode or anode grow in size?

Spring Semester Review Answers 1. A compound containing only carbon and hydrogen. 2. They contain C and H, as well as (usually) non-metallic elements such as oxygen, nitrogen,

sulfur, phosphorus, halogens, etc. 3. A separation technique relying on specific sizes of molecules. Smaller molecules boil at lower

temperatures, larger ones at higher. 4. Hydrocarbons that contain only single bonds 5. Six. 6. A hydrocarbon chain that replaces a hydrogen in a parent chain. 7. The longest continuous sequence of carbon in a molecule. 8. Hydrocarbons that contains at least one double bond. 9. Hydrocarbons that contains at least one triple bond. 10. A hydrocarbon with only single bonds. 11. Two or more compounds with the same formula but different structures. 12. A compound with a repeating structure. 13. A carbon ring structure. 14. Nine. 15. It has an alternating series of single and double bonds.

16. 17. F, Cl, Br, I.

18.

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19.

20. 21. Temperature change, Color change, Generation of gas (odor), Generation of light. Formation of solid 22. Dissolved in water. 23. A reaction that shows only reactants and products – it may not be balanced. 24. Two or more reactants form one product. 25. Carbon dioxide and water. 26. One element exchanges places with another one. 27. Ammonium, group 1 element ions, nitrate. 28. Solids that come out of solutions during some double replacement reactions. 29. Ions that don’t react in a reaction. 30. 6.02 E 23 31. Atoms, electrons, molecules, ions, formula units, or whatever you want to count. 32. The mass of one mole of a compound. 33. 5. 34. 4 moles. 35. A list of the percents of elements in a compound. 36. A chemical formula with the smallest whole number ratio of the elements. 37. The actual formula of a chemical. 38. A chemical compound that has water in its formula. 39. Four. 40. Study of quantitative relationships between amounts of reactants used and products formed in chemistry. 41. Ratio between the numbers of moles of any two of the substances in a balanced chemical equation. 42. The reactant that runs out first in a chemical reaction. 43. The reactant that is left over at the end of a reaction. 44. Not all reactions go to completion – if there is an excess reactant, the limiting reactant might be

all used up. And reactions might go faster with an excess reactant. 45. Maximum amount of product possible from a limiting reactant. 46. Measured amount of product from a reaction. 47. A combination of two or more pure substances that don’t blend smoothly. 48. A mixture that contains particles that settle out if left undisturbed. 49. A mixture in which the particles don’t settle out over time. 50. A substance that dissolves something. 51. A substance that is dissolved. 52. A measure of how much solute is dissolved in a specific amount of solvent. 53. Percent by volume. 54. Moles of solute/Liter of solution. 55. A concentrated solution of a chemical. 56. M1V1 = M2V2 57. Agitation – stirring or shaking; Larger surface area – pulverize solute; Heating – solids dissolve faster in warm solvent 58. An unstable situation – more solute is dissolved than ‘should’ be possible. 59. Solvent holds the maximum amount of solute. 60. A compound that breaks into ions in solution. It will conduct electricity. 61. The increase in boiling point of a solvent when a solute is added.

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62. The decrease in freezing temperature of a solvent when a solute is added. 63. Ionizable hydrogen ions. 64. An acid with more than one ionizable hydrogen ion. 65. One that ionizes completely in water. 66. Hydrochloric – HCl; Hydrobromic – HBr; Hydroiotic – HI; Nitric – HNO3, Perchloric – HClO4, Sulfuric – H2SO4 67. Hydrofluoric – HF, Acetic – CH3COOH, Carbonic – H2CO3, Hypochlorous – ClO, Phosphoric – H3PO4 68. NaOH, KOH, RbOH, CsOH, Ca(OH)2, Ba(OH) 2 69. Low pH. 70. The negative log of the hydroxide ion concentration. A scale of how basic something is. 71. Baking soda. 72. A method for determining the concentration of a solution, by reacting a known volume of an

unknown concentration with an amount of a known solution (called a titrant). 73. pH meter, color changing indicator. 74. Loss of electrons from a compound. 75. Gaining of electrons in a compound. 76. A reaction that involves electron transfer. 77. The chemical in a redox reaction that oxidizes another (it gains electrons and is reduced) 78. The chemical in a redox reaction that reduces another (it loses electrons and is oxidized) 79. Zero. 80. Carbon = + 4. Oxygen = -2. 81. No – they are inseparable. 82. The study of the redox processes that convert chemical energy into electrical energy. 83. Two half-cells are connected with a salt bridge, and their electrodes connected with a wire. 84. Mnemonic – reduction occurs at the cathode and is positive. 85. Zinc is oxidized and copper is reduced in this cell. 86. A single use (non-rechargeable) battery 87. A rechargeable one. 88. A moist paste containing chemicals. 89. Lead-Acid, lithium, Ni-Cad. 90. Hydrogen and oxygen. 91. Loss of metal due to redox reactions. 92. Coating a metal in zinc for protection. 93. The use of electrical energy to bring about a chemical reaction. 94. Hydrogen and oxygen. 95. Sodium and Chlorine. 96. Chlorine, hydrogen, and sodium hydroxide. 97. The cathode.

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