Chemistry Semester One Exam Review

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1 Chemistry Semester One Exam Review Name: 1. Compare physical and chemical changes in matter. 2. State the law on conservation of mass. 3. On which type of mixture(s) does the Tyndall Effect scatter light? On which type of mixture does it pass thru? 4. Define the following terms and list one example of each. a. Heterogeneous mixture b. Solution c. Colloid d. Suspension e. Metal (properties) f. Nonmetal (properties) 4. Define the following terms a. Chemical property b. Chemical change c. Physical property d. Physical change 1

2 5. Distinguish the symbols of common elements, and match the names of common elements to their symbols a. Aluminum d. O b. Nitrogen e. C c. Copper f. S 6. Define a neutral atom. 7. What is the name of C 6 14? What is another isotope of carbon? What is the difference between the two? 8. Complete the following table. Element // Symbol Atomic # # of P + # of E - # of N 0 Mass # Hydrogen // H 1.0 Carbon // C 6 Neon // Ne Given the electron configurations for the following neutral atoms, predict the oxidation number each is most likely to have. Element Configuration Oxidation Number A 1s 2 2s 2 2p 6 3s 2 B 1s 2 2s 2 2p 6 3s 1 C 1s 2 2s 2 2p 6 D 1s 2 2s 2 2p 5 E 1s 2 2s 2 2p 1 2

3 10. Why do flame tests appear different colors (use the terms ground state and excited state in your response). 11. Write the electron configurations for the following elements. Lithium- Nitrogen- Zinc- Bromine- Barium- 12. What is the characteristic set of valence electrons for the following groups on the periodic table? Alkali metals (1); alkaline earth metals (2); halogens (17); noble gases (18) 13. Refer to a table of atomic and ionic radii, if necessary, to answer the following questions. a. Within a period, does the size of atoms generally increase or decrease with increasing atomic number? b. Within a family, does the size of atoms increase or decrease with increasing atomic number? c. Within a period, does ionization energy increase or decrease with increasing atomic number? d. In a group, does Ionization energy increase or decrease with increasing atomic number? 14. How is reactivity in metals a trend on the periodic table? 3

4 15. Circle the larger particle in each of the following pairs. Na Li Br I F F - Cs Ba K K What are the characteristics of each of the following reaction types? a) Synthesis b) Combustion c) Decomposition d) Double replacement e) Single replacement 17. Complete the word equation, write and balance the equation using symbols and indicate the type of the reaction on the left. a. Propane (C 3 H 8 ) burns in air b. Magnesium chloride + silver nitrate c. Zn reacts with hydrochloric acid d. Nitrogen gas + hydrogen gas e. Calcium oxide 18. Which of the above could use the solubility table to predict its insoluble product? What is the net ionic reaction for it?? 19. Write formulas for the following compounds. a. zinc chloride b. lead (IV) oxide c. silver bromide d. sodium phosphate e. magnesium sulfide f. cobalt (II) fluoride g. barium oxide 4

5 20. Name the following compounds. a. Pb 3 (PO 4 ) 2 b. Cu(IO 3 ) 2 c. Cr 2 O 3 d. Bi 2 (SO 4 ) 3 e. RbNO 3 f. C 4 H Name the following compounds. a. N 2 O 3 b. PCl 3 c. SiO 2 d. P 2 O 5 e. CS 2 f. Al 2 O Solve the following problems a. Find the mass of 0.89 mol of CaCl 2. b. How many molecules are present in mol of NaCl? c. Determine the number of moles of C 5 H 12 that are in g of the compound. d. How many moles would you have if you had 1.75 x molecules of HOH? 5

6 23. Find the percent composition of each element in the following: a. PbCl 2 b. Aspirin (C 9 H 8 O 4 ) 24. Define limiting reactant (reagent). 25. Using the following balanced equation to answer the following questions. 2Al Cl 2 4AlCl 3 + 3O 2 a. If 4.0 moles of Al 2 O 3 react completely, how many moles of AlCl 3 are formed? b. How many grams of Al 2 O 3 are needed to react with 12.0 mol of Cl 2? c. If 30.5 g of Cl 2 react completely, how many molecules of O 2 are produced? d. How many grams of AlCl 3 are produced if 24.2 g of Cl 2 react completely? 6

7 26. Use the following data to find the average atomic mass of the element given based on the data from its isotopes: Pb % Pb % Pb % Pb % 27. What are the parts of an atom according to the electron cloud model? 7

8 Student Review BCRs were put on the exam review sheets to encourage appropriate student collaboration and review of concepts in preparation for the entire exam (not just the BCRs). Teachers should not address these BCRs during the course of their instruction and review with students other than highlighting their availability to support STUDENT review and to teach, model and encourage collaboration around the concepts. Students should be prepared to answer any of the following BCRs. Teachers will select two from the list below: BCR: Separating a Precipitate A chemistry student must separate solid barium sulfate, a precipitate, from an aqueous solution. Equipment and glassware normally found in the chemistry classroom are available to the student. Describe how the student could separate the solid barium sulfate from the aqueous solution. Be sure to list the lab equipment needed to do the procedure explain how each item is used in the procedure list any safety equipment needed and how it is used in the procedure describe how this procedure might be used in a situation outside the chemistry classroom BCR: Comparing Substances Two solids, A and B, are located in the same family on the periodic table. A sample of each is placed in a beaker of HCl. Substance A produces a few bubbles that rise to the top of the liquid. Substance B bubbles vigorously. Based on this information, compare substances A and B. Be sure to describe the following: what the bubbles indicate where the substances are located in relation to one another on the periodic table and the activity series the name of a family the substances could belong to which substance will have a larger atomic radius which substance will have a larger first ionization energy Chemistry Semester A Exam 5 Montgomery County Public Schools

9 Student Review BCR: Types of Reactions Students observations of three chemical reactions are shown in the table below. Use their data and the solubility table to classify each of the types of reactions. Be sure to include the name of each type of reaction evidence that supports how each type is classified the reactants and products for each reaction Reaction Initial Observations / Notes Final Observations / Notes Clear, colorless KI solution is added to clear, colorless Pb(NO 3 ) 2 solution in a beaker. Magnesium (Mg), a solid silver-colored ribbon, is ignited in the flame of a Bunsen burner. The Mg burns with a bright white light. Mercury (II) oxide, a red, powdery solid, is heated in a test tube. A yellow solid appears in a clear liquid. The yellow solid is lead (II) iodide. White ashes remain after the Mg burns. Magnesium oxide is produced. Mercury metal condenses on the walls of the test tube. A glowing splint inserted into the mouth of the test tube burns brightly. Chemistry Semester A Exam 6 Montgomery County Public Schools

10 Student Review BCR: Stoichiometry Propane is used as a fuel in most gas grills to cook food on during the warm summer months. When the propane is burned, the following reaction takes place: C 3 H 8 (l) + 5O 2 (g) 3CO 2 (g) + 4H 2 O(g) A standard propane tank contains 6804 g of propane. Determine how many molecules of carbon dioxide gas are released into the atmosphere when an entire tank of propane is burned. In your answer be sure to: Describe the type of chemical reaction the propane undergoes Calculate the number of moles of propane used in the reaction Explain the mole ratio between propane and carbon dioxide in this reaction Calculate the number of moles of carbon dioxide produced Calculate the number of molecules of carbon dioxide produced Chemistry Semester A Exam 7 Montgomery County Public Schools

11 Student Review BCR: The Flame Test A student burns a small amount of six solutions in the flame of a Bunsen burner and records the color for each. Her data are shown in the table below. Solution Lithium chloride Sodium chloride Potassium chloride Calcium chloride Strontium chloride Barium chloride Color Red Yellow Violet Red-orange Red-orange Green Analyze the results of the flame test colors. Be sure to include An explanation of the flame test results in terms of energy and electron movement An explanation of how the flame test can be used to identify ions The limitations of the flame test in identifying ions Chemistry Semester A Exam 8 Montgomery County Public Schools

12 Student Review BCR: Unknown Compound Bob s chemistry teacher gives him a solid compound to use in a chemical reaction. The teacher tells him the compound is either sodium carbonate, Na 2 CO 3, or sodium bicarbonate, NaHCO 3. Bob must determine the identity of the compound. He reacts the compound with excess HCl and measures the mass of the product. His data are shown in the table below. MASS OF PRODUCT IN REACTION Substance Mass (g) Mass of beaker Mass of beaker + solid compound Mass of beaker + dried product (NaCl) The balanced chemical equations below show each possible reaction. #1 Na 2 CO 3 (s) + 2HCl(aq) H 2 O(l) + CO 2 (g) + 2NaCl(s) #2 NaHCO 3 (s) + HCl(aq) H 2 O(l) + CO 2 (g) + NaCl(s) Describe how you would use the information from the data table to determine the identity of the compound. In your response, be sure to identify the compound support your choice by o explaining how you would use data from the table o showing calculations, including moles of reactants and moles of products o describing reasons for not choosing the other compound describe how using stoichiometry is necessary to select the correct compound Chemistry Semester A Exam 9 Montgomery County Public Schools

Semester 1 Exam Review

Semester 1 Exam Review 1. Compare physical and chemical changes in matter. Physical changes involve changing a substance s shape, texture, or size, not its chemical composition. Chemical changes result