Naming and Reaction Types

Name: ________________________ Chemistry 11 1. 2. Block: _____ Final Exam Review Write the correct formula for the following compounds: a) ammonium chlorate ......................................................___________NH4ClO3_______ b) copper (II) sulphite ........................................................____________CuSO3________ c) zinc carbonate tetrahydrate ..........................................._______ZnCO3 ° 4H2O_______ d) nitric acid ......................................................................____________HNO3 (aq)______ e) phosphorus pentaiodide ................................................_______________PI5_________ f) iron (III) thiocyanate .....................................................____________Fe(SCN)3_______ g) sulphuric acid ................................................................_____________H2SO4_________ h) dinitrogen tetrafluoride .................................................____________N2F2____________ Write the correct names for the following compounds: a) Mn(SO4)2......................................_________________Manganese (IV) Sulphate _________ b) PbCrO4.6H2O ..............................._____________Lead (II) Chromate Hexahydrate________ c) As2O3............................................_______________Diarsenic Trioxide________________ d) CH3COOH ..................................._________________Acetic_acid____________________ e) Ni2(C2O4)3 ....................................____________Nickel (III) Oxalate___________________ f) NF3 ...............................................___________Nitrogen Trifluoride____________________ g) (NH4)2HPO4 .................................____________Ammonium Phosphate_______________ h) Ba(OH)2.10H2O............................__________Barium Hydroxide Decahydrate____________ Name: ________________________ Chemistry 11 (Final Exam Review) Block: _____ Balancing Equations and Reaction Types Review Using the different types of reactions (Synthesis, Decomposition, Single Replacement, Double Replacement, Neutralization, and Combustion) predict the products and balance the equation. 1) ___ H3PO4 + _3_ KOH → ___ K3PO4 + ___ H2O Type of Reaction: ____________ Neutralization____________ 2) _2_ C2H2 + _5_ O2 → _2_ H2O + _4_ CO2 Type of Reaction: _____________Combustion________________ Exothermic and Endothermic Reactions 1. Draw a diagram of an Exothermic and Endothermic Reaction. Label the Reactant, Products, Enthalpy Change (∆H), and Activation Energy (Ea) ENDOTHERMIC EXOTHERMIC 2. List the following Reactions as Exothermic or Endothermic: a. 2H2O2(l) → 2H2O(l) + O2(g) + 200kJ Answer: ____Exothermic___ b. Mn(s) + 2 HCl(aq) → MnCl2(aq) + H2(g) + 221 kJ Answer: ____Exothermic___ c. 2 N2O5 (g) + 110 kJ → 4NO2(g) + O2(g) Answer: ___Endothermic__ d. P4O10(g) + 6H2O(l) → 4 H3PO4(aq) + 424 kJ Answer: ____Exothermic__ Name: ________________________ 1. 2. Chemistry 11 (Final Exam Review) Block: _____ The Greek who developed the idea of atoms was _______Democritus__________ 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? ________Dalton_______ He called the ideas, the ___________Atomic__________ Theory. 3. Give the number of protons, neutrons and electrons in the following: Isotope 194 Protons 3+ Ir 202 Hg2+ 125 Te 2263 Sg 2 + H Neutrons 77 80 52 106 1 Electrons 117 202 – 80 = 122 125 – 52 = 73 263 – 106 = 157 2–1=1 74 78 54 106 0 194 – 77 = 4. Give the nuclear notation of the following: Isotope Protons Neutrons Electrons 262 105 157 103 51 72 48 33 42 36 54 79 54 94 150 91 Db2+ 123 Sb3+ 75 As3133 Xe 244 Pu3+ Name: ________________________ 5. Chemistry 11 (Final Exam Review) Block: _____ Element “X” is composed of the following naturally occurring isotopes: Isotope 79 X 81 X % Abundance 50.69 49.31 Calculate the average atomic mass of element “X” to 3 decimal places. [79 × (0.5069)] + [81 × (0.4931)] = 79.99𝑔/𝑚𝑜𝑙 Element “X” is actually the real element ____________Bromine_____________. 6. Regions in space occupied by electrons are called ___________Orbitals_______ 7. Write the ground state electron configurations (eg. 1s2 2s2 2p6) for the following atoms or ions. You may use the core notation. a) P 1s2 2s2 2p6 3s2 3p3 OR [Ne] 3s2 3p3 2 2 6 2 6 2 10 6 2 4 b) M 1s 2s 2p 3s 3p 4s 3d 4p 5s 4d OR [Kr] 5s2 4d4 c) Cl 1s2 2s2 2p6 3s2 3p6 OR [Ne] 3s2 3p6 d) Al3+ 1s2 2s2 2p6 OR [He] 2s2 2p6 22 2 6 2 6 e) S 1s 2s 2p 3s 3p OR [Ne] 3s2 3p6 8. Circle the metalloid: Be Rb Os Ge Pb Al 9. Circle the most reactive element in the following: Na Mg Si Al Ar 10. Circle the most reactive element in the following: Cl Br I At N 11. Circle the element with the largest atomic radius of these: Na Mg Si Al Ar 12. Circle the element with the largest ionization energy of these: K Ca Ga As Kr 13. What is meant by ionization energy? Energy required to remove the outermost electron 14. Circle the element with the largest density of these: C Si Ge Sn Pb 15. Circle the element with the highest electronegativity of these: Mg Sr Ba Ra 16. Circle the element with the highest electronegativity of these: F Cl Br I 17. What is meant by electronegativity? The attraction an atom has for the electrons of a neighboring atom 18. Circle the most metallic element of these: Be Mg Ca Sr Ba 19. Circle the most metallic element of these: Ga Ge Se Br Kr 20. Write a balanced equation for the reaction of potassium with water. 𝟐𝑲 + 𝟐𝑯𝟐 𝑶 → 𝑯𝟐 + 𝟐𝑲𝑶𝑯 21. Write a balanced equation for the reaction of aluminum with bromine. 𝟐𝑨𝒍 + 𝟑𝑩𝒓𝟐 → 𝟐𝑨𝒍𝑩𝒓𝟑 22. 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 ________ Name: ________________________ 23. 24. 25. 26. Chemistry 11 (Final Exam Review) Block: _____ 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 ________ 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 ________ 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 ________ Draw the Lewis Structures for: (a) CH3Cl Indicate if polar or non-polar. a. (c) PO4-3 (b) H2 (d) SF6 . b. Polar c Non-Polar d. Non-Polar Non-Polar Name: ________________________ Chemistry 11 (Final Exam Review) Block: _____ 27. Given the following graph of Temperature vs. Time for warming substance “X” which starts out as a solid, answer the questions below: Temperature oC 90oC 77oC 43oC 15oC 0.0 5.0 15.0 20.0 Time (minutes) 28.0 a) During time 0.0 – 5.0 minutes, the added heat energy is being used to _________Increase the temperature of the solid substance________ b) During time 5.0 – 15.0 minutes, the added heat energy is being used to __________________Melt the solid substance________________ c) During time 15.0 – 20.0 minutes, the added heat energy is being used to _______Increase the temperature of the liquid substance_________ d) During time 20.0 – 28.0 minutes, the added heat energy is being used to ______________________Boil the liquid____________________ e) The melting point of substance “X” is ________43 oC____________ f) The boiling point of substance “X” is _________77 oC____________ 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 90oC? ____________Gas______________ i) Explain WHY the curve levels off between 5.0 min. and 15.0 min. All of the added heat energy is being used for the process of melting the solid (phase change) so none is available to warm the substance until after the melting is complete Name: ________________________ Chemistry 11 (Final Exam Review) Block: _____ 1. Which would be miscible with water: ethanol or butane? Why? Both ethanol and water are polar substances. Recall: “Like dissolves like” 2. Why are some solvents polar and some non-polar? Which would you use to dissolve salt? Polar molecules are molecules which are not symmetrical and have permanent dipoles because of an uneven sharing of electrons. NaCl is polar so you would use a polar solvent (“like dissolves like”) 4. Which of the following would you except to form conducting (“ionic”) solutions when added to water, and which would form non-conducting (“non-ionic”) solutions? (a) KI (b)HBr (c)CH4 (d)CsF = Conducting (e) H2CO3 (f)ICI (g)CaBr2 (h)CH3COOH 5. Which of the following conduct electricity? (a)HCl(aq) (b)Ag(s) (c)BaBr2(aq) (d)LiCl(s) (e)CO2(s) (f)LiOH(l) (g)C14H10(l) (h) CH3COOH(l) 6. Which should melt at a higher temperature? Why? (a)He or Xe (e)HI or HCI (b)F2 or Br2 (f)H2O or H2Te (c)CH4 or CH3F (d)HBr or Kr (g)CH3-CH3 or HO-CH2CH2-OH 7. What will be the [Cl-1] if 60.0 g of BaCl2(s) is dissolved in water to a final volume of 600.0mL? 8. If 35.0g of V(NO3)5 is dissolved in water to a final volume of 1.0L , what will the [NO3-1] be? 9. What mass of NaBr must be dissolved in 4.9L of water to make a 5.2 M NaBr solution? Name: ________________________ Chemistry 11 (Final Exam Review) Block: _____ 1. 0.0006 mm = ? m Answer ______0.6 m _______ 2. 0.054 mL = ? nL Answer ___5.4 × 104 𝑛𝐿_____ 3. 3.5 g/L = ? mg/mL 4. The density of iron is 7860 g/L. Calculate the mass of a 3.2 mL sample of iron. Answer __3.5 × 10−6 𝑚𝑔/𝑚𝐿__ 𝑔 𝑚𝑎𝑠𝑠 = 0.032𝐿 × 7860 𝐿 = 25.152 𝑔 = 25 𝑔 5. Manganese has a density of 7.20 g/mL. Calculate the volume occupied by a 4.0 kg piece of manganese. 4000𝑔 𝑣𝑜𝑙𝑢𝑚𝑒 = 7.20 𝑔/𝑚𝐿 = 555.56 𝑚𝐿 = 5.6 × 102 𝑚𝐿 6. 𝑚𝑎𝑠𝑠 8. Answer ____5.6 × 102 𝑚𝐿 _____ A 0.0460 L piece of copper has a mass of 410.32 g. Calculate the density of copper in g/mL. 𝑑𝑒𝑛𝑠𝑖𝑡𝑦 = 𝑣𝑜𝑙𝑢𝑚𝑒 = 7. Answer _________25 g______ 410.32𝑔 46.0 𝑚𝐿 = 8.92 𝑔/𝑚𝐿 Answer _____8.92 𝑔/𝑚𝐿 ____ Give the number of significant digits in each of the following. Assume they are all measurements. a) 0.0023 ..............................____2____ d) 3.2 x 10-4 .......................................____2___ b) 3953 000 ............................____4___ e) 50020.000 ......................................____8___ c) 1.0200 x 105 ......................____5___ f) 3450 ...............................................____3___ 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) 2.1500 x 0.31 ............____0.67_____ f) 8.90 x 103 ÷ 4.400 x 10-6 .__𝟐. 𝟎𝟐 × 𝟏𝟎𝟗 ___ b) 0.05 + 394.7322 ........__394.78____ g) 83.00 ÷ 1.2300 x 102 ..............____0.6748__ c) 4.905 x 106 ÷ 4 x 10-2____1x108____ h) 98.0076 - 2.195 ....................__95.813____ d) (3.33 x 9.52) + 13.983.___45.7_____ i) 0.00000200 x 245.912 ........._𝟒. 𝟗𝟐 × 𝟏𝟎−𝟒 _ e) 3.813 + 98.98 + 2.669 ......._105.46__ j) 5.802 ÷ 6.21 + 2.41 ÷ 9.2565 ... ___𝟏. 𝟏𝟗𝟓__ Name: ________________________ 9. 1. g) Chemistry 11 (Final Exam Review) Block: _____ Round the following numbers to 2 significant digits. (4 marks) a) 2 000 000 000_____𝟐. 𝟎 × 𝟏𝟎𝟗 _____ c) 3.88945 x 1028 ............ _____ 𝟑. 𝟗 × 𝟏𝟎𝟐𝟖 __ b) 106 000 ........... ___ 𝟏. 𝟏 × 𝟏𝟎𝟏𝟎 ____ d) 0.000 000 7895 ....... ______ 𝟕. 𝟗 × 𝟏𝟎−𝟕___ Make the following conversions, clearly showing your steps. Include proper units in all of your work and in your answer. a) 133.44 grams of PCl5 = ? moles Answer _______0.64000 mol__________ b) 0.00256 moles of Li2Cr2O7 = ? grams Answer __________0.588 g___________ c) 170.24 L of NO2 at STP = ? moles Answer _______7.6000 mol________ d) 570.625 g of PCl3 gas = ? L (STP) Answer ________92.9600 mL_________ e) 1030.4 mL of C2H6 gas at STP = ? g Answer ________1.3853 g____________ f) 5.00 kg of nitrogen gas = ? L (STP) Answer _______𝟒. 𝟎𝟎 × 𝟏𝟎𝟑 𝑳_____ 0.5696 kg of CH4(g) = ? mL Answer _____𝟕. 𝟗𝟕𝟒 × 𝟏𝟎𝟓 𝒎𝑳 _______ 2. The density of liquid ethanol (C2H5OH) is 0.790 g/mL. Calculate the number of molecules in a 35.0 mL sample of liquid ethanol. (Note: You cannot use 22.4 L/mol since this is NOT a gas at STP!) Answer ____ 𝟑. 𝟔𝟐 × 𝟏𝟎𝟐𝟑 𝒎𝒐𝒍𝒆𝒄𝒖𝒍𝒆𝒔____ 3. A 100.0 mL sample of liquid mercury contains 6.78 moles. Calculate the density of liquid mercury from this data. Answer _________13.6 g/mL____________ Name: ________________________ 4. Chemistry 11 (Final Exam Review) Block: _____ a) The density of a gas at STP is 4.955 g/L. Calculate the molar mass of this gas. b) The gas is an oxide of selenium. Determine the molecular formula. Answer __________________________ 5. Find the percent composition (% by mass of each element) in the following compound: Sr3(PO4)2. Show your work. Answer ______%Sr, ______%P, ______% 6. A compound was analyzed and the following results were obtained: Molar mass: 270.4 g/mol Mass of sample: 162.24 g Mass of potassium: 46.92 g Mass of sulphur: 38.52 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. Answer: Empirical Formula: _____________________ b) Determine the molecular formula for this compound. Answer: Molecular Formula: _____________________ 7. 123.11 g of zinc nitrate, Zn(NO3)2 are dissolved in enough water to form 650.0 mL of solution. Calculate the [Zn(NO3)2] Include proper units in your work and in your answers. Answer _______________________ 8. Calculate the mass of potassium sulphite (K2SO3) needed to make 800.0 mL of a 0.200 M solution of K2SO3. Include proper units in your work and in your answers Answer ______________________ Name: ________________________ 9. Chemistry 11 (Final Exam Review) Block: _____ 150.0 mL of water are added to 400.0 mL of 0.45 M HNO3 . Calculate the final [HNO3]. Include proper units in your work and in your answers. Answer ______________________ 10. What volume of water needs to be added to 150.0 mL of 4.00 M H2SO4 in order to bring the concentration down to 2.50 M? Include proper units in your work and in your answers. Answer __________________ Unit 7— Stoichiometry Student Workbook 123 - 138 Extra Questions (Hebden) p.124, p.127, p.131, p.133, p.137 1. Given the following balanced equation, answer the questions following it: 2NF3(g) + 3H2(g) a) → N2(g) + 6HF(g) If 5.5 moles of H2 are reacted, how many moles of NF3 will be consumed? Answer ____________ b) In order to produce 0.47 moles of HF, how many moles of NF3 would be consumed? Answer ____________ c) If you needed to produce 180.6 g of N2, how many moles of H2 would you need to start with? Answer ____________ d) If you completely react 17.04 g of NF3 , what mass of HF will be produced? Answer ____________ Name: ________________________ 2. Chemistry 11 (Final Exam Review) Block: _____ Given the following balanced equation, answer the questions following it: HBrO3 + 5 HBr a) → 3 H2O(l) + 3 Br2(g) If 3.56 moles of HBr are reacted, how many litres of Br2 will be formed at STP? Answer ______________________ b) In order to produce 3.311 x 1024 molecules of Br2, what mass of HBr is needed? Answer ______________________ 3. Given the following balanced chemical equation, answer the question below it. MgCO3 (s) + 2HCl (aq) → CO2 (g) + H2O (l) + MgCl2(aq) a) What mass of MgCO3 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 37.935 grams of magnesium carbonate. 5. Answer _______________________ Given the following balanced equation, answer the questions below it. 3 Cu(s) + 8HNO3(l) → 3 Cu(NO3)2(aq) + 2NO(g) + 4 H2O(l) a) If 317.5 grams of Cu are placed into 756.0 grams of HNO3, determine which reactant is in excess. Answer _______________________ b) If the reaction in (a) is carried out, what mass of NO will be formed? Answer _______________________ 12 Name: ________________________ 6. Chemistry 11 (Final Exam Review) Given the balanced equation: 2BN + Block: _____ 3F2 → 2BF3 + N2 , When 161.2 grams of BN are added to an excess of F2, a reaction occurs in which 326.118 grams of BF3 are formed. a) Calculate the theoretical yield of BF3 in grams. Answer _______________________ b) Calculate the percentage yield of BF3. Answer _______________________ 7. When reacting NH3 with O2 according to the reaction: 4 NH3 + 5 O2 → 4 NO + 6 H2O Using 163.2 grams of NH3 with an excess of O2 produces a 67% yield of NO. a) Calculate the theoretical yield of NO in grams. Answer ____________________ b) Calculate the actual yield of NO in grams. Answer ______________________ Name: ________________________ Chemistry 11 (Final Exam Review) Block: _____ 2,3,4-trimethylhexane 3,4-dimethylhexane 3,4-dimethylheptane 2,2,3-trimethylpentane 2,2-dimethylbutane 3,4,5-trimethylheptane 2-methylpetane 2-methylbutane 2,4-dimethylpetane 3-methylhexane Heptane 2,4-dimethylpetane 2,2,3-trimethylpropane 3-methylpetane 2,2-dimethylpetane Name: ________________________ Chemistry 11 (Final Exam Review) Block: _____ IONIC COMPOUND NAMES Cation = Positive (+) Ion Ionic Compounds = Metal + Non-metal Anion = Negative (-) Ion Metal Name + Non-Metal Name (change ending to “-ide”) PREFIX Mono = 1 E.g: Calcium Chloride Copper (II) Iodide (CaCl2) (CuI2) Di = 2 COVALENT COMPOUND NAMES Tri = 3 Covalent Compounds = Non-Metal + Non-Metal Tetra = 4 Prefix+Non-Metal Prefix+Non-Metal(“-ide”) Penta = 5 E.g: Trinitrogen Decabromide (N3Br10) Hexa = 6 Hepta = 7 HYDRATES Octa = 8 Ionic Compound + Prefixhydrate Nona = 9 E.g: Copper (II) Sulfate Pentahydrate (Ionic Name) (Prefix Hydrate) Deca = 10 ACID NAMES No Oxygen: “Hydro_________ic Acid” (Ex. Hydrobromic Acid – HBr) With Oxygen: Identify the polyatomic oxyanion, and o Metals (Rows 1 & 2) (Do not need to add number when naming Ionic Compounds) “ite” → “ous” “ate” → “ic” Name the oxoanion and add the word “acid”. (Example: Chlorous Acid – HClO2) Change the endings: BASE NAMES 1. Name the metal first 2. The polyatomic ion "hydroxide" (-OH) after Example: NaOH - Sodium Hydroxide Metals – add number (I, II, III, IV...) when naming Ionic Compounds Name: ________________________ Chemistry 11 (Final Exam Review) Block: _____ Organic Naming Rules Number of Carbon Atoms Root Alkane (Parent) Branch 1 2 3 4 5 6 7 8 9 10 Meth- Eth- Prop- But- Pent- Hex- Hept- Oct- Non- Dec- Methane Ethane Propane Butane Pentane Hexane Hept Octane Nonane Decane Methyl Ethyl Propyl Butyl Pentyl Hexyl Heptyl Octyl Nonyl Decyl Reaction Types Sig Fig Rules Stoichiometric Conversions ATOMIC RADIUS