Chemistry 11 Course Review

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1 Chemistry 11 Course Review Note: This review is meant for practice purposes. There are multiple outcomes that have not been covered in this booklet, which should be part of your personal review. Ch. 1: Skills and Processes of Chemistry (Intro. to Chemistry) 1.1 Demonstrate appropriate safety techniques / use of protective equipment 1.2 Demonstrate skills in measuring and in recording data 1.3 Communicate results and data in clear and understandable forms 1.4 Convert between metric units mm =? µm ml =? nl Answer Answer µg/l =? mg/ml Answer 4. The density of iron is 7860 g/l. Calculate the mass of a 3.2 ml sample of iron. Answer 5. Manganese has a density of 7.20 g/ml. Calculate the volume occupied by a 4.0 kg piece of manganese. Answer Page 1

2 6. A L piece of copper has a mass of g. Calculate the density of copper in g/ml. Answer 7. 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. (4 marks) a) c) x b) d) Page 2

3 Ch. 2: The Nature of Matter 2.1 Describe the characteristics of matter / Differentiate between physical and chemical changes 2.2 Relate the observable properties and characteristics of elements, compounds, and mixtures to the concept of atoms and molecules (Classifying) 2.3 Select an appropriate way of separating the components of a mixture 2.4 Write the names and formulae for ionic and covalent compounds, given appropriate charts or data tables 1. Define: Observation, Interpretation, Qualitative, Quantitative, Data, Experiment, Hypothesis, Theory, Laws, Matter, Chemistry, Physical and Chemical Properties, Malleability, Ductility, Lustre, Viscosity and Diffusion. Review the Phases of Matter. 2. Draw the diagram from your notes outlining the Classification of Matter. Make sure you can define each classification. Page 3

4 3. Concerning separation techniques 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) Explain how a centrifuge separates the components of a suspension. 4. Define a physical change Give some examples of physical changes. 5. Define a chemical change Give some examples of chemical changes. Page 4

5 6. Given the following graph of Temperature vs. Time for warming substance X which starts out as a solid, answer the questions below: 90 o C Temperature o C 77 o C 43 o C 15 o C 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 C? i) Explain WHY the curve levels off between 5.0 min. and 15.0 min. Page 5

6 2.4: Names and Formulas for Compounds 2.4 Write the names and formulae for ionic and covalent compounds, given appropriate charts or data tables 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... f) iron (III) thiocyanate... g) sulphuric acid... h) dinitrogen tetrafluoride Write the correct names for the following compounds: a) MnSO 4... b) PbCrO 4. 6H 2 O... c) As 2 O 3... d) CH 3 COOH... acid e) Ni 2 (C 2 O 4 ) 3... f) NF 3... g) (NH 4 ) 2 HPO 4... h) Ba(OH) 2. 10H 2 O... Page 6

7 Ch. 3: The Mole Concept 3.1/3.2 Explain the significance and use of the mole 3.2/3.3 Perform calculations involving the mole 3.4 Determine relationships between molar quantities of gases at STP 3.5 Perform calculations involving molecular and empirical formulas to identify a substance 3.6 Describe concentration in terms of molarity 1. Make the following conversions, clearly showing your steps. Include proper units in all of your work and in your answer. a) grams of PCl 5 =? moles b) moles of Li 2 Cr 2 O 7 =? grams Answer c) L of NO 2 at STP =? moles Answer d) g of PCl 3 gas =? L (STP) Answer e) ml of C 2 H 6 gas at STP =? g Answer Answer Page 7

8 f) 5.00 kg of nitrogen gas =? L (STP) Answer g) kg of CH 4(g) =? ml (STP) Answer 2. The density of liquid ethanol (C 2 H 5 OH) is g/ml. Calculate the number of molecules in a 35.0 ml sample of liquid ethanol. (NOTE: You CAN T use 22.4 L/mol since this is NOT a gas at STP!) Answer 3. A ml sample of liquid mercury contains 6.78 moles. Calculate the density of liquid mercury from this data. 4. Calculate the density of PCl 3(g) at STP. Answer Answer Page 8

9 5. a) The density of a gas at STP is g/l. Calculate the molar mass of this gas. b) The gas is an oxide of selenium. Determine the molecular formula. Answer 6. Find the percent composition (% by mass of each element) in the following compound: Sr 3 (PO 4 ) 2. Show your work. 7. 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. b) Determine the empirical formula for this compound. Answer %Sr, %P, %O Answer c) Determine the molecular formula for this compound. Answer: Empirical Formula: Answer: Molecular Formula: Page 9

10 g of zinc nitrate, Zn(NO 3 ) 2 are dissolved in enough water to form ml of solution. Calculate the [Zn(NO 3 ) 2 ]) Include proper units in your work and in your answers. Answer 9. Calculate 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 10. What volume of 2.50 M Li 2 CO 3 would need to be evaporated in order to obtain g of solid Li 2 CO 3? Include proper units in your work and in your answers. Answer 11. Give directions on how to make 5.00 L of M Ca(ClO) 2 using solid Ca(ClO) 2 and water. Include proper units in your work and in your answers. Directions: Page 10

11 Ch. 4: Chemical Change / Reactions 4.1 Explain chemical reactions in terms of the rearrangement of the atoms as bonds are broken and new bonds are formed 4.1 Apply the law of conservation of mass to balance formula equations 4.2 Devise balanced equations for various chemical reactions 4.4 Describe reactions in terms of energy changes 4.5/4.6 Perform stoichiometric calculations involving chemical reactions 1. Balance the following equations NH 3 + O 2 NO + H 2 O (NH 4 ) 2 C 2 O 4 + AlCl 3 Al 2 (C 2 O 4 ) 3 + NH 4 Cl C 14 H 30 + O 2 CO 2 + H 2 O Fe + HNO 3 Fe(NO 3 ) 3 + H 2 P 4 + Cl 2 PCl 3 Na 2 Cr 2 O 7 + HCl NaCl + CrCl 3 + H 2 O + Cl 2 H 3 PO 4 + Ca(OH) 2 Ca 3 (PO 4 ) 2 + H 2 O Ba(ClO 4 ) 2 Ba + Cl 2 + O 2 C 7 H 15 OH + O 2 CO 2 + H 2 O MgSO 4. 5H 2 O MgSO 4 + H 2 O Page 11

12 2. 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 (C 3 H 7 OH) is burned in air c) ammonium nitrate is decomposed into it s elements d) a piece of zinc is placed in a test-tube containing a solution of silver nitrate e) bromine reacts with sodium iodide f) bromine reacts with aluminum g) rubidium reacts with chlorine gas h) hydrochloric acid reacts with strontium hydroxide 3. State whether each of the following are exothermic or endothermic. HCl kj H + Cl C 12 H 22 O O 2 12CO H 2 O H 2 O (s) H 2 O (l) Answer H = kj Answer Answer Energy (kj) A + B AB Reaction Proceeding Answer CD C + D H= 65.7 kj Answer E + F kj G + H Answer Page 12

13 4. Given the equation: C 12 H 22 O O 2 12CO H 2 O kj a. How much heat is released during the formation of g of CO 2? Answer b. How much heat is released during the formation of 5.6 moles of H 2 O? Answer c. If L of O 2 (STP) are consumed, how much heat is released? Answer 5. 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? Answer Page 13

14 6. Given the following balanced equation, answer the questions following it: 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 7. Given the following balanced chemical equation, answer the question below it. MgCO 3 (s) + 2HCl (aq) CO 2 (g) + H 2 O (l) + MgCl 2(aq) a) What mass of MgCO 3 will react completely with 15.0 ml of 1.5 M HCl? Answer b) Calculate the volume of 2.0 M HCl which would be needed to react completely with grams of magnesium carbonate. 8. Given the following balanced equation, answer the questions below it. 3 Cu (s) + 8HNO 3(l) 3 Cu(NO 3 ) 2(aq) + 2NO (g) + 4 H 2 O (l) a) If grams of Cu are placed into grams of HNO 3, determine which reactant is in excess. Answer Page 14

15 b) If the reaction in (a) is carried out, what mass of NO will be formed? Answer 9. 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) Calculate the theoretical yield of BF 3 in grams. b) Calculate the percentage yield of BF 3. Answer Answer 10. 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) Calculate the theoretical yield of NO in grams. b) Calculate the actual yield of NO in grams. Answer Answer Page 15

16 Ch. 5 and 6: Atoms, Periodic Table and Bonding Describe the development of the model of the atom Describe the sub-atomic structures of atoms, ions, and isotopes, using calculation where appropriate 6.1 Describe the development of the modern periodic table 6.2 Draw conclusions about the similarities and trends in the properties of elements, with reference to the periodic table 6.3 Demonstrate knowledge of various types of chemical bonding 6.4 Apply understanding of bonding to create formulae and Lewis structures 1. Consider the following ideas: Compounds are made up of molecules which are combinations of atoms All atoms of an element are the same Atoms of different elements are different Atoms are indivisible particles Who came up with these ideas? He called the ideas, the Theory. 2. measured the charge/mass ratio of an electron and came up with the so-called plum pudding model of the atom. 3. devised the Scattering Experiment, which showed that all atoms had a small dense. 4. Bohr came up with an atomic model to explain the spectrum of. He said that the atom has certain levels which are allowed. These levels corresponded to in which electrons move. If an electron absorbs a certain photon of energy, it will jump to a level. It will release this energy (in the form of ) when it jumps back to a level. What were two limitations of Bohr s atomic model? 5. Give the number of protons, neutrons and electrons in the following: Isotope Protons Neutrons Electrons 194 Ir Hg Te Sg 2 H + Page 16

17 6. 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 Calculate the average atomic mass of element X to 3 decimal places. Element X is actually the real element. 8. Regions in space occupied by electrons are called 9. The principal quantum number is given the letter and refers to the level. 10. 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) Cl - f) Al 3+ g) K + h) S 2- Page 17

18 11. In order to become stable, an atom of Sr will electrons and become the ion an atom of As will electrons and become the ion an atom of Al will electrons and become the ion an atom of Se will electrons and become the ion an atom of N will electrons and become the ion an atom of I will electrons and become the ion an atom of Cs will electrons and become the ion an atom of Te will electrons and become the ion 12. Circle the metalloid: Be Rb Os Ge Pb Al 13. Circle the most reactive element in the following: Na Mg Si Al Ar 14. Circle the most reactive element in the following: Na K Rb Cs Li 15. Circle the most reactive element in the following: Cl Br I At Ne 16. Circle the element with the largest atomic radius of these: Na Mg Si Al Ar 17. Circle the element with the largest atomic radius of these: N P As Sb Bi 18. Circle the element with the largest ionization energy of these: K Ca Ga As Kr 19. Circle the element with the largest ionization energy of these: C Si Ge Sn Pb 20. What is meant by ionization energy? 21. Circle the element with the largest density of these: C Si Ge Sn Pb 22. Circle the element with the largest density of these: Na K Rb Cs Li 23. Circle the element with the highest electronegativity of these: Mg Sr Ba Ra 24. Circle the element with the highest electronegativity of these: Mg Si S Cl 25. Circle the element with the highest electronegativity of these: F Cl Br I 26. What is meant by electronegativity? Page 18

19 27. Circle the most metallic element of these: Be Mg Ca Sr Ba 28. Circle the most metallic element of these: B Al Ga In Tl 29. Circle the most metallic element of these: Ga Ge Se Br Kr 30. 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 31. In a covalent 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 32. In a polar covalent 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 33. In London forces, 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 34. What evidence do we have that ionic bonds are very strong? 35. Write electron-dot (LEWIS) diagrams for: MgCl 2 (ionic) PBr 3 (covalent) SeF 2 (covalent) CH 3 CH 2 I(covalent) Page 19

20 Ch. 7: Solutions 7.1 Distinguish between a solution and a pure substance 7.2 Predict the relative solubility of a solute in a solvent, based on its polarity 7.3 Relate ion formation to electrical conductivity in aqueous solutions 7.4 Calculate the concentration of ions in solution ml of water are added to ml of 0.45 M HNO 3. Calculate the final [HNO 3 ]. Include proper units in your work and in your answers. Answer 2. 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 3. 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 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 Page 20

Remember Organic Chemistry and Safety are also Fair game for the Final!! Study Hard! Answers: Ch. 1: Introduction to Chemistry 1. 0.6µm 2. 5.4 x 10 4 nl 10 3. 3.5 x 10-6 mg/ml 4. 25 g 5. 556 ml 6. 8.

21 Remember Organic Chemistry and Safety are also Fair game for the Final!! Study Hard! Answers: Ch. 1: Introduction to Chemistry µm x 10 4 nl x 10-6 mg/ml g ml g/ml 7. a. 2 b. 4 c.5 d. 2 e. 8 f a b c. 1 x 10 8 d e f x 10 9 g h i x 10-4 j a. 2.0 x 10 9 b. 1.1 x 10 5 c. 3.9 x d. 7.9 x a. 1.9 g/ml b. 0.0 g c. Mass = 1.9 g/ml volume d. 285 g e. 126 ml f. D = slope= 1.9 g/ml Ch. 2: Properties of Matter 1. See textbook or notes. 2. See textbook or notes. 3. a. Components have different melting points. Increase in temperature until only one boils. Vapour condensed to liquid. Other substances stay in the flask. b. Small amounts of ink, pigments, etc. c. Spins quickly. Dense materials forced outward to the bottom of the test tube. 4. New chemical substances formed. Eg: Burning, photosynthesis, neutralization, etc. 5. a. Increase in temperature of the solid. b. Melting the solid. c. Warm up the liquid of substance X. d. Boil the liquid. e. 43 C f. 77 C g. 3 h. gaseous i. All the energy is being used for melting the solid. No energy is available to warm the substance until melting is complete. Section2.4: Names and Formulas for Compounds 1. a. NH 4 ClO 3 b. CuSO 3 c. ZnCO 3 4H 2 O d. HNO 3 e. PI 5 f. Fe(SCN) 3 g. H 2 SO 4 h. N 2 F 4 2. a. Manganese (II) sulphate b. Lead (II) chromate hexahydrate c. Diarsenic trioxide d. Acetic acid e. Nickel (III) oxalate f. Nitrogen trifluoride g. Ammonium monohydrogen phosphate h. Barium hydroxide decahydrate Ch. 3: The Mole Concept 1. a mol b g c. 7.6 mol d L e g f x 10 3 L g x 10 5 ml x molecules g/ml g/l 5. a. 111 g/mol b. SeO % Sr, Page 21

22 13.69% P, 28.27% 0 6. a g b. KSO 4 c. K 2 S 2 O 8 7. [Zn(NO 3 ) 2 ] =1.000 M g L 10. Add g of Ca(ClO) to less than 5.00 L of water and dissolve. Add more water to a final volume of 5.00 L. Ch. 4: Chemical Reactions 1. a. 4, 5, 4, 6 b. 3, 2, 1, 6 c. 2, 43, 28, 30 d. 2, 6, 2, 3 e. 1, 6, 4 f. 14, 2, 2, 7, 3 g. 2, 3, 16 h. 1, 1, 1, 4 i. 2, 21, 14, 16 j. 1, 1, 5 2. a. 3 K 2 SO Co(NO 3 ) 3 Co(SO 4 ) KNO 3 (D.R.) b. 2 C 3 H 7 OH + 9 O 2 6 CO H 2 O (Comb.) c. 2 NH 4 NO 3 2 N H 2 +3 O 2 (Dec.) d. Zn + 2 AgNO 3 2 Ag + Zn(NO 3 ) 2 (S.R.) e. Br NaI I NaBr (S.R.) f. 3 Br Al 2 AlBr 3 (Syn.) g. 2 Rb + Cl 2 2 RbCl (Syn.) h. 2 HCl + Sr(OH) 2 2 H 2 O + SrCl 2 (Neut.) 3. a. endo b. exo c. endo d. exo e. endo f. endo 4. a kj b kj c kj 5. a mol b mol c mol d g HF 6. a L Br 2 b g HBr 7. a g b L 8. a. Cu in excess. b g 9. a g BF 3 b. 74.0% 10. a g NO b g Ch. 5 and 6: Atoms, Periodic Table and Bonding 1. John Dalton; Atomic 2. J.J. Thompson 3. Ernest Rutherford; nucleus 4. a. Hydrogen; energy; orbitals (shells); higher; light (photons); lower b. Only worked for hydrogen; no evidence that e- travel in orbits. 5. Isotope Protons Neutrons Electrons 194 Ir Hg Te Sg H a. 105Pb b. 51Sb c. 33As d Xe e. 94Pu g/mol; Bromine 8. orbitals 9. n; energy 10. a. [Ne] 3s 2 3p 3 b. [Kr] 5s 2 4d 4 c. [Ar] 4s 2 3d 10 4p 4 d. [Kr] 5s 1 e. [Ne] 3s 2 3p 6 f. [He] 2s 2 2p 6 g. [Ne] 3s 2 3p 6 h. [Ne] 3s 2 3p lose, 2, Sr 2+ ; gain, 3, As 3- ; lose, 3, Al 3+ ; gain, 2, Se 2- ; gain, 3, N 3- ; gain, 1, I - ; lose, 1, Cs + ; gain, 2, Te Ge 13. Na 14. Cs 15. Cl 16. Na 17. Bi 18. Kr 19. C 20. Energy required to remove outermost e Pb 22. Cs 23. Mg 24. Cl 25. F 26. The ability of an atom to attract the shared pair of electrons to itself. 27. Ba 28. Tl 29. Ga 30. c 31. a 32. b 33. e 34. High melting points 35. ask your teacher Ch. 7: Solutions 1. [HNO 3 ] = 0.33 M ml 3. a. [HNO 3 ] = M b L Page 22

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