Name Hour January Exam Practice A 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 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) Iron 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 Calcium 21 Atomic Number Mass Number 24 52 48 64 Nb 93 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 Chlorine Cu 6A 2 Representative or Transition? Metal, metalloid, nonmetal? W Score: /13 Objective 4 Correctly classify a sample of matter as an element, compound, homogeneous solution or heterogeneous solution. 1. Sample A = Table Salt 1. 2. Sample B = Air 2. 3. Sample C = Neon 3. 4. Sample D = Soil 4. 5. Sample E = Concrete 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. Oxygen has 3 natural isotopes. The first isotope has a mass of 15.995 amu and a relative abundance of 99.759. The second isotope has a mass of 16.995 amu and a relative abundance of 0.037. The third isotope has a mass of 17.999 amu and a relative abundance of 0.204. 1. Draw a simple Bohr model of all 3 isotopes of oxygen in the boxes below: Clearly label all subatomic particles! (2 points each) First Isotope Second Isotope Third Isotope 2. Write the standard notation for all 3 isotopes in the boxes below: (1 pt each) First Isotope Second Isotope Third Isotope (4 points) 3. Calculate the average atomic mass of an element from 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. Copper II Chloride 2. Carbon Dioxide 3. H 2 O 4. LiNO 3 5. CrF 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. Arsenide Ion Calcium Ion Manganese (II) ion Bromide 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. CN -1 Ni +2 NH 4 +1 CrO 4-2 PO 4-3 Score: /12 5
Objective 9 Apply the rules for naming binary molecular compounds. Directions: Name the following binary molecular compounds: 1. Cl 2 O 7 2. N 6 O 5 3. BCl 3 Score: /6 Objective 10 Apply the rules for writing formulas for binary molecular compounds. Directions: Write formulas for the following binary molecular compounds. 1. carbon disulfide 2. dinitrogen tetrahydride 3. pentaphosphorus trioxide 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 I -1 PO 3-3 CO 3-2 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. K 2 CO 3 2. HCN 3. C 2 O 4 4. Na 2 S 5. Cu 3 PO 4 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. sulfurous acid 2. lead (II) dichromate 3. hydrosulfurous acid 4. dinitrogen trichloride 5. magnesium fluoride Score: /15 (3 points each) 7
Part 2: Name: Hour: 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 molecules in 30.3 grams of HCl. 2. Calculate the volume, in Liters, of 3.40 x 10 23 molecules of Bromine (Br 2 ) gas at STP. 3. Calculate the mass of 53 Liters of Neon 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. Place your final answer on the line provided. Be sure to include the correct unit with your final answer. 1. When a 16.4 gram sample of Zirconium (II) oxide is decomposed into its elements by heating, 13.94 grams of Zirconium is obtained. What is the percent composition of this compound? 2. Calculate the percent composition of Silicone Dioxide, a major component of sand. 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. Determine the empirical formula for a compound that contains 93.3 % nitrogen and 6.7 % hydrogen. 2. Determine the empirical formula for a compound containing 40.4 % C, 7.8 % H, 35.9 % O, 15.7 % N. 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. 4KMnO 4 2K 2 O + 4MnO + 5O 2 2. Cu + 2AgNO 3 Cu(NO 3 ) 2 + 2Ag 3. C 12 H 22 O 11 + 12O 2 12CO 2 + 11H 2 O 4. Na 2 O + CO 2 Na 2 CO 3 5. 2CH 3 COCH 3 + 5O 2 6CO + 6H 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. sulfur dioxide reacts with water 2. chromium metal reacts with phosphorus producing a chromium (II) product 3. aluminum oxide reacts 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. Ammonium chlorate decomposes when heated 3. Carbonic 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 mercury (II) bromide 2. fluorine gas is bubbled through a solution of aluminum bromide 3. lead metal is placed into a solution of iron (III) acetate Score: (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 aluminum sulfate reacts with aqueous strontium nitrate Driving Force 2. Solutions of lithium carbonate reacts with silver nitrate Driving Force 3. Sulfuric is placed into a solution of cesium 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. C 7 H 6 O incompletely combusts. 2. Butane (C 4 H 10 ) 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