Name Hour January Semester Exam Practice B This exam will be given over 2 days. Part 1: Objectives 1-13 Part 2: Objectives 14-24 This practice exam will be graded in the exam portion of the grade book Objectives 1-13 Part 1: Due on Tuesday, January 18 th Objectives 14-24 Part 2: Due on Exam Day Solutions are available on Mrs. Hanson s Website http://www.reeths-puffer.org/profiles/linda Hanson_Profile/ 1
Objective 1 Identify the physical and chemical properties of common substances. 1. Define the term physical property: (2 pts) 2. Define the term chemical property: (2 pts) 3. Describe 3 physical properties and 1 chemical property for the substance: (8 pts) Copper Physical Physical Physical Chemical Score: /12 Objective 2: Use the atomic number and mass number of an element to find the number of protons, electrons, and neutrons. Directions: Complete the table for the following elements: Element Symbol Number of Protons Number of Electrons Number of Neutrons Atomic Number Mass Number Bismuth 210 46 106 Ni 31 13 26 Lithium 7 Score: /14 2
Objective 3: Identify the position of groups, periods, representative elements, transition elements, inner transition elements, metals, metalloids, and nonmetals on the periodic table. Directions: Complete the table for the following elements: Element Symbol Group Number Period Number Indium Antimony V 4A 4 1B 5 Representative or Transition? Metal, metalloid, nonmetal? Score: /13 Objective 4 Correctly classify a mixture as homogeneous or heterogeneous. Directions: For each sample of matter below, correctly classify it as a homogeneous mixture or a heterogeneous mixture. 1. Substance A = water based paint 1. 2. Substance B = iron filings and sulfur powder 2. 3. Substance C = Oil-based Paint 3. 4. Substance D = Air 4. 5. Substance E = Orange Juice, no pulp 5. Score: /10 3
Objective 5: Draw simple Bohr models of isotopes. Write the standard notation for any isotope. Calculate the average atomic mass of an element from isotope data. Sulfur has 4 natural isotopes. The first isotope has a mass of 31.972 amu and a relative abundance of 95.002. The second isotope has a mass of 32.971 amu and a relative abundance of 0.76. The third isotope has a mass of 33.967 amu and a relative abundance of 4.22. The fourth isotope has a mass of 35.967 amu and a relative abundance of 0.014. 1. Draw a simple Bohr model of all 4 isotopes of sulfur in the boxes below: First Isotope Second Isotope Third Isotope Fourth Isotope 2. Write the standard notation for all 4 isotopes below: First Isotope Second Isotope Third Isotope Fourth Isotope 3. Calculate the average atomic mass of an element from its isotope data. Show all work and circle final answer. Be sure to include units with your final answer! Score: /13 4
Objective 6: Distinguish between ionic and molecular compounds. Directions: Label the following compounds as either ionic or molecular. 1. Magnesium Fluoride 2. Dinitrogen trioxide 3. Aluminum Iodide 4. Se3Cl2 5. PI 2 Score: /5 Objective 7 Apply the rules for naming and writing formulas for binary ionic compounds. Directions: Hook together the following ions to write the correct formula AND place the name of the resulting compound within the box. Bromide Ion Barium Ion Copper (I) ion Phosphide Ion Score : /8 Objective 8 - Apply the rules for naming and writing formulas for ternary ionic compounds. Directions: Hook together the following ions to write the correct formula AND place the name of the resulting compound within the box. C 2 H 3 O 2-1 Cr +2 Al +3 CO 3-2 PO 4-3 Score: /12 5
Objective 9 Apply the rules for naming binary molecular compounds. Directions: Name the following binary molecular compounds: 1. Br 4 O 9 2. S 5 O 3. P 3 Cl 8 Score: /6 Objective 10 Apply the rules for writing formulas for binary molecular compounds. Directions: Write formulas for the following binary molecular compounds. 1. dicarbon tetrachloride 2. tetranitrogen monohydride 3. pentaphosphorus pentaoxide Score: /6 Objective 11 Apply the rules for naming and writing formulas for acids. Directions: Hook together the Hydrogen Ion to the following negative ions and write the correct formulas AND name the resulting acid. H +1 P -3 SO 4-2 PO 3-3 Score: /6 6
Objective 12 Write names of any compound when given its formula. Directions: Write the names of the following compounds in the blank provided. 1. HNO2 2. CuBr 3. C2Br4 4. Li3PO4 5. HI Score: /15 (3 points each) Objective 13 Write a formula for any compound when given its name. Directions: Write the correct formula for the following compounds. 1. potassium permanganate 2. hydrophosphoric acid 3. cobalt (II) phosphide 4. trichlorine pentafluoride 5. manganese (II) cyanide Score: /15 (3 points each) 7
Name: Part 2 Practice Exam B Objective 14 Use the mole to convert among measurements of mass, volume, and number of particles. Directions: Solve the following problems. Show work using *dimensional analysis. *(show how the units cancel throughout the entire problem.) Place your final answer on the line provided. Be sure to include the correct unit with your final answer. 1. Calculate the number of liters in 49.3 grams of SO2. 2. Calculate the mass of 4.98 x 10 24 molecules of Bromine (Br 2 ) gas at STP. 3. Calculate the number of atoms of 38 Liters of Helium at STP. Score: /12 (4 points each) Objective 15 Calculate the percent composition of a substance from its chemical formula or experimental data. Directions: Solve the following problems. Show work using *dimensional analysis. *(show how the units cancel throughout the entire problem.) Place your final answer on the line provided. Be sure to include the correct unit with your final answer. 1. Calculate the percent composition of potassium dichromate: 2. Calculate the percent composition of aluminum phosphide: Score: /10 (5 points each) 8
Objective 16 Derive the empirical formula of a compound from experimental data. Directions: Solve the following problems. Show work using *dimensional analysis. Place your final answer on the line provided. Be sure to include the correct unit with your final answer. 1. What is the empirical formula of a compound that is 35.63% Phosphorus and 64.37% Oxygen? 2. Determine the empirical formula for a compound that contains 22.86% C, 2.86% H, 13.33 % N, and 60.95% O. Score: /10 (5 points each) Objective 17: Identify a reaction as combination, decomposition, single-replacement, double-replacement, complete combustion, or incomplete combustion. Directions: Identify the following reactions as a combination, decomposition, single-replacement, doublereplacement, complete combustion, or an incomplete combustion. 1. 2C 8 H 18 + 25O 2 16CO 2 + 18H 2 O 2. H 2 C 2 O 4 + 2KOH 2H 2 O + K 2 C 2 O 4 3. Mg + H 2 SO 4 H 2 + MgSO 4 4. 4Na + O 2 2Na 2 O 5. (NH 4 )NO 3 N 2 O + 2H 2 O Score : /10 (2 points each) Objective 18: Predict the product of a combination reaction by writing a complete balanced equation. Directions: Write a complete balanced equation for the following combination reactions, predicting the correct product. 1. beryllium reacts with phosphorus when heated strongly 2. sulfur trioxide combines with water 3. magnesium oxide combines with water Score: /15 (5 points each) 9
Objective 19: Predict the products of a decomposition reaction by writing a complete balanced equation. Directions: Write a complete balanced equation for the following decomposition reactions, predicting the correct products. 1. barium carbonate will decompose when heated 2. aluminum chlorate decomposes when heated 3. Sulfurous acid decomposes Score: /15 (5 points each) Objective 20: Using the activity series, predict the products of a single-replacement reaction by writing a complete balanced equation. Directions: Write a complete balanced equation for the following single-replacement reactions, predicting the correct products. Be sure to check the activity series to make sure the reaction occurs. 1. Calcium metal is placed into a solution of iron (III) chloride 2. fluorine gas is bubbled through a solution of lithium iodide 3. silver metal is placed into a solution of sodium acetate Score: /15 (5 points each) 10
Objective 21: Predict the products of a double-replacement reaction by writing a complete balanced equation and indicating the driving force of the reaction. Use the solubility chart to help predict precipitates. Directions: Write a complete balanced equation for the following double-replacement reactions, predicting the correct products. 1. Aqueous silver nitrate reacts with aqueous aluminum chloride Driving Force 2. A solution of sodium hydroxide reacts with magnesium sulfate Driving Force 3. Hydrochloric acid is placed into a solution of sodium hydrogen carbonate, creating carbon dioxide gas, as well as two other products. Driving Force Score : /21 (7 points each) Objective 22: Predict the products of either a complete or an incomplete combustion reaction by writing a complete balanced equation. Directions: Write a complete balanced equation for the following combustion reactions, predicting the correct products. The term complete or incomplete will be provided in the sentence to guide you in your predictions. 1. Butene (C 4 H 8 ) completely combusts. 2. Acetone (C 3 H 6 O) completely combusts. Score : /10 (5 points each) 11
Objective 23: Patterns of Chemical Change Write a balanced equation for the following reactions. Also, indicate what category of reaction it is; (combination, decomposition, single-replacement, doublereplacement, or combustion.) 1. Solutions of copper (I) phosphate and chromium (III) sulfite Category are mixed. 2. Zinc oxide is heated strongly. Category 3. Aluminum oxide is formed. Category 4. Barium metal is placed into nitric acid. Category 5. Propanol, CH 3 CH 2 CH 2 OH, is incompletely burned. Category Score: /35 (7 points each) 12
Objective 24: Chemical and Physical Changes: Directions: a. Indicate if the following is a physical or a chemical change. b. Explain the reason(s) for your choice. c. For each chemical change, write a complete balanced equation. 1. Lithium is dropped into water: 2. Aluminum is dropped into water: 3. A solution of sodium hydroxide is placed into a solution of calcium chloride: 4. A solution of potassium chloride is placed into a solution of ammonium nitrate. 5. Tin and sulfur are placed in a test tube together. Score: /25 (5 points each) 13