Chemistry 11 Course Review

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1 Unit 1. Nature of Matter lass Assignments Hand-In #1 Unit onversions Hand-In #2 Significant Digits Hand-In #3 Separation Methods and Phase hange 1. Give the number of significant digits in each of the following. Assume they are all measurements. a) d) 3.2 x b) e) c) x f) Perform the following calculations and round the answers off to the correct number of significant digits as justified by the data. Assume all numbers are measurements. a) x f) 8.90 x x b) g) x c) x x h) d) (3.33 x 9.52) i) x e) j) Round the following numbers to 2 significant digits. a) c) x b) d) mm =? µm µg/l =? mg/ml Answer Answer Page 1

2 6. The density of iron is 7860 g/l. alculate the mass of a 3.2 ml sample of iron. Answer 7. Manganese has a density of 7.20 g/ml. alculate the volume occupied by a 4.0 kg piece of manganese. Answer ml 8. Review separation methods. Answer the following: a) Explain how distillation can be used to separate the substances in a solution. b) What types of mixtures does paper chromatography work best for? c) Solvent extraction involves using two different solvents which are (miscible/immiscible). A device called a funnel is used. 9. Define a physical change Give some examples of physical changes. 10. Define a chemical change Give some examples of chemical changes. Page 2

3 11. Given the following graph of Temperature vs. Time for warming substance X which starts out as a solid, answer the questions below: 90 o Temperature o 77 o 43 o 15 o Time (minutes) a) During time minutes, the added heat energy is being used to b) During time minutes, the added heat energy is being used to c) During time minutes, the added heat energy is being used to d) During time minutes, the added heat energy is being used to e) The melting point of substance X is f) The boiling point of substance X is g) If a greater amount of substance X was used, the melting point would be 1. a lower temperature 2. a higher temperature 3. the same temperature Answer h) What phase is substance X at 90 o? i) Explain WHY the curve levels off between 5.0 min. and 15.0 min. Page 3

4 Unit 2. Atoms, Periodic Table and Bonding lass Assignments Hand-In Assignment # 12 Electronic Structure of the Atom Hand-In Assignment #13 Lewis Diagram 1. Give the number of protons, neutrons and electrons in the following: Isotope Protons Neutrons Electrons 194 Ir Hg Te Sg 2 H + 2. Give the nuclear notation of the following: Isotope Protons Neutrons Electrons Element X is composed of the following naturally occurring isotopes: Isotope % Abundance 79 X X alculate the average atomic mass of element X to 3 decimal places. Element X is actually the real element. Page 4

5 4. Write the ground state electron configurations (eg. 1s 2 2s 2 2p 6 ) for the following atoms or ions. You may use the core notation. a) P b) Mo c) Se d) Rb e) l - f) Al 3+ g) K + h) S 2-5. ircle the element with the largest atomic radius of these: Na Mg Si Al Ar 6. ircle the element with the largest atomic radius of these: N P As Sb Bi 7. ircle the element with the largest ionization energy of these: K a Ga As Kr 8. ircle the element with the largest ionization energy of these: Si Ge Sn Pb 9. What is meant by ionization energy? 10. ircle the element with the highest electronegativity of these: Mg Sr Ba Ra 11. ircle the element with the highest electronegativity of these: Mg Si S l 12. ircle the element with the highest electronegativity of these: F l Br I 13. What is meant by electronegativity? 14. ircle the most metallic element of these: Be Mg a Sr Ba 15. ircle the most metallic element of these: B Al Ga In Tl 16. ircle the most metallic element of these: Ga Ge Se Br Kr 17. ircle the substance that is isoelectronic to argon: l - Mg 2+ Mn 2+ Li + Page 5

6 18. In an ionic bond, electrons are a. shared equally by two atoms b. shared unequally by two atoms c. transferred from a metal to a non-metal d. transferred from a non-metal to a metal e. closer to one end of a molecule, forming a temporary dipole Answer (In an ionic bond, the ΔEN must be ) 19. In a covalent bond, electrons are f. shared equally by two atoms g. shared unequally by two atoms h. transferred from a metal to a non-metal i. transferred from a non-metal to a metal j. closer to one end of a molecule, forming a temporary dipole Answer (In a covalent bond, the ΔEN must be ) 20. In a polar covalent bond, electrons are k. shared equally by two atoms l. shared unequally by two atoms m. transferred from a metal to a non-metal n. transferred from a non-metal to a metal o. closer to one end of a molecule, forming a temporary dipole Answer (In a polar covalent bond, the ΔEN must be ) 21. In London forces, electrons are p. shared equally by two atoms q. shared unequally by two atoms r. transferred from a metal to a non-metal s. transferred from a non-metal to a metal t. closer to one end of a molecule, forming a temporary dipole Answer 22. Write Levis diagrams for: Mgl 2 (ionic use[ ] ) BH 3 (covalent) H 3 OOH(covalent) Page 6

7 Unit 3. The Mole oncept lass Assignments Hand-In Assignment # 4 Mass-Mole-Molecules onversions Hand-In Assignment #5 Summary of Mole Hand-In Assignment #6 Percent omposition, Empirical and Molecular Formulas Hand-In Assignment #7 Molarity and Dilution 1. Make the following conversions, clearly showing your steps. Include proper units in all of your work and in your answer. a) grams of Pl 5 =? moles b) moles of Li 2 r 2 O 7 =? grams Answer c) L of NO 2 at STP =? moles Answer d) g of Pl 3 gas =? L (STP) Answer Answer e) ml of 2 H 6 gas at STP =? g Answer f) 5.00 kg of nitrogen gas =? L (STP) Answer Page 7

8 2. The density of liquid ethanol ( 2 H 5 OH) is g/ml. alculate the number of molecules in a 35.0 ml sample of liquid ethanol. (NOTE: You AN T use 22.4 L/mol since this is NOT a gas at STP!) 3. alculate the density of Pl 3(g) at STP. Answer Answer 4. Find the percent composition (% by mass of each element) in the following compound: Sr 3 (PO 4 ) 2. Show your work. Answer %Sr, %P, %O 5. A compound was analyzed and the following results were obtained: Molar mass: g/mol Mass of sample: g Mass of potassium: g Mass of sulphur: g Mass of oxygen: the remainder of the sample is oxygen a) Determine the mass of oxygen in the sample. Answer b) Determine the empirical formula for this compound. c) Determine the molecular formula for this compound. Answer: Empirical Formula: Answer: Molecular Formula: Page 8

9 g of zinc nitrate, Zn(NO 3 ) 2 are dissolved in enough water to form ml of solution. alculate the [Zn(NO 3 ) 2 ]) Include proper units in your work and in your answers. Answer 7. alculate the mass of potassium sulphite (K 2 SO 3 ) needed to make ml of a M solution of K 2 SO 3. Include proper units in your work and in your answers. Answer 8. What volume of 2.50 M Li 2 O 3 would need to be evaporated in order to obtain g of solid Li 2 O 3? Include proper units in your work and in your answers. Answer 9. What volume of water needs to be added to ml of 4.00 M H 2 SO 4 in order to bring the concentration down to 2.50 M? Include proper units in your work and in your answers. Answer Page 9

10 10. Given the following balanced equation, answer the questions following it: 2NF 3(g) + 3H 2(g)! N 2(g) + 6HF (g) a) If 5.5 moles of H 2 are reacted, how many moles of NF 3 will be consumed? Answer b) In order to produce 0.47 moles of HF, how many moles of NF 3 would be consumed? Answer c) If you needed to produce g of N 2, how many moles of H 2 would you need to start with? Answer d) If you completely react g of NF 3, what mass of HF will be produced? 11. Given the following balanced equation, answer the questions following it: Answer HBrO HBr! 3 H 2 O (l) + 3 Br 2(g) a) If 3.56 moles of HBr are reacted, how many Litres of Br 2 will be formed at STP? Answer b) In order to produce x molecules of Br 2, what mass of HBr is needed? Answer Page 10

11 Unit 4. hemical Reactions lass Assignments Hand-In Assignment #8 hemical Equations Hand-In Assignment #9 Predicting, Balancing and lassifying hemical Equations Hand-In Assignment #10 Energy in hemical Reactions Hand-In Assignment #11 Titration Hand-In Assignment #12 Excess and Percent Yield Problems 1. Write the correct formula for the following compounds: a) ammonium chlorate... b) copper (II) sulphite... c) zinc carbonate tetrahydrate... d) nitric acid... e) phosphorus pentaiodide Write the correct names for the following compounds: a) Mn(SO 4 ) 2... b) PbrO. 4 6H 2 O... c) As 2 O 3... d) H 3 OOH... acid e) Ni 2 ( 2 O 4 ) 3... f) NF Balance the following equations NH 3 + O 2! NO + H 2 O (NH 4 ) 2 2 O 4 + All 3! Al 2 ( 2 O 4 ) 3 + NH 4 l 14 H 30 + O 2! O 2 + H 2 O Fe + HNO 3! Fe(NO 3 ) 3 + H 2 P 4 + l 2! Pl 3 Na 2 r 2 O 7 + Hl! Nal + rl 3 + H 2 O + l 2 Page 11

12 4. Write a balanced chemical equation for each of the following, and classify each as synthesis, decomposition, single replacement, double replacement, neutralization or combustion. a) potassium sulphate is mixed with cobalt (III) nitrate b) liquid propanol ( 3 H 7 OH) is burned in air c) ammonium nitrate is decomposed into it s elements 5. State whether each of the following are exothermic or endothermic. Hl kj! H + l 12 H 22 O O 2! 12O H 2 O H 2 O (s)! H 2 O (l) Answer ΔH = kj Answer Answer Energy (kj) A + B AB Reaction Proceeding! Answer D! + D ΔH= 65.7 kj Answer E + F kj! G + H Answer 6. Given the following balanced equation, answer the questions below it. Ba(OH) 2(aq) + 2 HNO 3(aq)! 2 H 2 O (l) + Ba(NO 3 ) 2 a) In a titration, ml of M Ba(OH) 2 is required to react completely with a 25.0 ml sample of a solution of HNO 3. Find the [HNO 3 ]. Answer Page 12

13 b) In a titration, ml of M HNO 3 is required to react completely with a sample of 0.250M Ba(OH) 2. Find the volume of the Ba(OH) 2 sample. Answer 7. Given the following balanced equation, answer the questions below it. 3 u (s) + 8HNO 3(l)! 3 u(no 3 ) 2(aq) + 2NO (g) + 4 H 2 O (l) a) If grams of u are placed into grams of HNO 3, determine which reactant is in excess. Answer b) If the reaction in (a) is carried out, what mass of NO will be formed? Answer Page 13

14 8. Given the balanced equation: 2BN + 3F 2! 2BF 3 + N 2, When grams of BN are added to an excess of F 2, a reaction occurs in which grams of BF 3 are formed. a) alculate the theoretical yield of BF 3 in grams. b) alculate the percentage yield of BF 3. Answer Answer 9. When reacting NH 3 with O 2 according to the reaction: 4 NH O 2! 4 NO + 6 H 2 O Using grams of NH 3 with an excess of O 2 produces a 67% yield of NO. a) alculate the theoretical yield of NO in grams. b) alculate the actual yield of NO in grams. Answer Answer Page 14

15 Unit 5. Solution hemistry lass Assignments Hand-In Assignment # 15 Electrolyte and Ion oncentration Hand-In Assignment # 16 Polarity Hand-In Assignment # 17 Like Dissolves Like and Intermolecular Force Sugar 1. Determine whether the following is electrolyte or not. Provide explanation for each. ompound Electrolyte or Non- electrolyte Reason Table Salt Acetic acid (Vinegar) 2. onsider M of a 3 (PO 4 ) 2 solution. a. Write a balanced dissociation equation for a 3 (PO 4 ) 2 b. alculate the concentration of each ion. [a 2+ ]= M [PO 4 3- ]= M c. 20.0mL of 1.50M a 3 (PO 4 ) 2 solution is mixed with 80.0mL of 1.00M abr 2. alculate the final concentration of each ion. (Show all steps and appropriate dissociation equations.) Page 15

16 [a 2+ ]= M [PO 4 3- ]= M [Br - ]= M 3. lassify whether the following molecules are polar or not by drawing Lewis diagram based on VSEPR theory. a. H 2 O b. H 3 H 2 ONH 2 c. F 4 (amide) 4. Draw H 2 O and H 3 H 2 ONH 2 molecules and label hydrogen bond in between. 5. What is the strongest intermolecular attraction found between the following? a) Two molecules of BH 3 (Boron is electron deficient) Lewis Diagram Type of ompound Possible Intermolecular Attractions Strongest Intermolecular Attraction b) Two molecules of H 3 OOH Lewis Diagram Type of ompound Possible Intermolecular Attractions Strongest Intermolecular Attraction Page 16

17 Unit 6. Organic hemistry lass Assignments Hand-In Assignment # 18 Electrolyte and Ion oncentration Hand-In Assignment # 19 Polarity Hand-In Assignment # 20 Like Dissolves Like and Intermolecular Force 1. Fill in the table to summarize characteristics of all families. Family Name Ending What it looks like (Use 3 carbons) alkane cycloalkane alkene alkyne benzene aldehyde keton amine amide alcohol carboxylic acid ether ester Page 17

18 2. Draw the following organic molecules using condensed structure. a. 2- fluorohexanal b. 3,4- dimethylcyclooctyne c. cis- 2- heptene d. diethyl ether e. 3- methyl- 4- chlorobutanoic acid f. 1,3,5- triethylbenzene g. methyl ethanoate h. cyclopentanamine i. butyl propyl ether j. 2,2- dimethylpropanamide Page 18

19 3. Name the following organic molecules. a. H H 3 H H 3 H 2 H H H 3 H 3 b. H 3 H 2 OH H H 2 O c. H 3 H H 3 H 2 H 2 H 3 d. H Br H 3 H 2 H H H OH Br H H 2 H 2 e. H3OOH2H2H3 Page 19

Chemistry 11 Course Review

Introduction to Chemistry 1. 0.0006 mm =? µm Chemistry 11 Course Review 6. A 0.0460 L piece of copper has a mass of 410.32 g. Calculate the density of copper in g/ml. 2. 0.054 ml =? nl 3. 3.5 µg/l =? mg/ml