Chemistry Semester Two Exam Review. The test will consist of 50 multiple choice questions over the following topics.
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1 Chemistry Semester Two Exam Review Name The test will consist of 50 multiple choice questions over the following topics. 1) Measuring (1): Triple beam balance, graduated cylinder, thermometer, ruler 2) Writing Rx & State Symbols (5): A) Solid aluminum hydroxide decomposes when it is heated. 2Al(OH) 3 Al 2 O 3 + 3H 2 O Decomposition Rxn B) A solution of iron (III) nitrate reacts with a solution of ammonium carbonate. 2Fe(NO 3 ) 3 + 3(NH 4 ) 2 (CO 3 ) 6(NH 4 )(NO 3 ) + Fe 2 (CO 3 ) 3 Precipitation Rxn C) Solid sodium carbonate decomposes when it is heated. Na 2 (CO 3 ) Na 2 O + CO 2 Decomposition Rxn D) A chunk of lithium reacts with a solution of sodium hydroxide. Li + Na(OH) Na + Li(OH) Single Replacement Rxn E) Gaseous C 4 H 10 burns. 2C 4 H O 2 8CO H 2 O Combustion Rxn F) Solid iron (III) reacts with fluorine. 2Fe + 3F 2 2FeF 3 Synthesis/Composition Rxn 3) Periodic Trends (6): A) Electron affinity across a period and down a family...why? Increase from left to right (fewer electrons needed to fill up orbital spaces) and decreases down (atomic radius is becoming larger). B) Electronegativity across a period and down a family why? Increase from left to right (fewer electrons needed to fill up orbital spaces wants to gain electrons) and decreases down (atomic radius is becoming larger). C) Ionization energy across a period and down a family why? Increase from left to right (atomic radius becoming smaller, more energy needed to remove an electron) and decreases down (atomic radius is becoming larger, less energy needed to remove electron). D) Atomic radius across a period and down a family why? Increase from right to left (fewer protons in nucleus not as strong of a pull to center) Increase down (more energy levels)
2 E) Chemical behavior & resulting oxidation number for each family Alkali metals very reactive metals (+1), Alkali earth metals not as reactive as alkali metals (+2), Halogens very reactive nonmetals (-1), Nobel Gases inert/nonreactive nonmetals (0), Transition and Inner transition metals not as reactive as alkali or alkali earth variable oxidation F) Most reactive metal & most reactive nonmetal why? Most reactive metal Francium (largest atomic radius easily loses valence electron), most reactive nonmetal Fluorine (smallest atomic radius easily gains valence electron due to large electronegativity) 5) Nuclear Reactions (2): A) Thorium-291 emits a beta particle what is the resulting atom? Protactinium-291 B) Lead-204 emits an alpha particle what is the resulting atom? Mecury-200 Alpha particle similar to a helium atom without electrons. Easily stopped by paper, clothing, skin, space. Contains two protons and two neutrons. Beta decay an electron emitted from nucleus at the same time a neutron is changed to a proton. 6) Law of Conservation of Mass/Balancing Equations (2) 7) Weighted Averages (3): A) g 25.0% B) g 33.00% g 70.0% g 52.00% g g 13.8 g Weighed average g Weighed average 8) LR/ER (7): Study Test 6-2 and/or Practice Problems for 6-2 9) Atoms and Molecule Drawings (3) 10) Protons, Neutrons, Electrons (3): A) How many protons, neutrons, electrons & valence electrons does a neutral atom of arsenic-73 have? P = 33, E= 33, N = 40, Valence e s = 5 B) Please write the isotopic notation for an atom of strontium Sr 38
3 C) Please give the name, atomic number, atomic mass, oxidation number, number of protons, number of neutrons & number of electrons for these atoms. Identify the type of ion & the type of isotope Fe Te Iron-54, AN = 26, AM = 54, ON = +4, P = 26, N = 28, E = 22, cation, light isotope Tellurium 124, AN = 52, AM = 124, ON = -2, P = 52, N = 72, E = 54, cation, light isotope D) Please give the isotopic notation, name, type of ion & type of isotope for each of these atoms. 76 protons, 130 neutrons, 71 electrons Osmium 206, cation, light isotope Os protons, 80 neutrons, 53 electrons Tellurium 132, anion, heavy isotope Te 52 11) Empirical/Molecular Formulas (3): A) A compound contains % phosphorus & % oxygen. Its molar mass is g. What is its empirical formula? What is its molecular formula? Empirical = P 2 O 5 Molecular = P 4 O 10 B) A compound contains g carbon, g hydrogen, g nitrogen & g oxygen. Its molar mass is g. What is its empirical formula? What is its molecular formula? Empirical = C 10 H 21 N 2 O 3 Molecular = C 20 H 42 N 4 O 6 C) What is the empirical formula of this copper compound? Before any reactions: Mass of crucible & lid Mass of crucible & lid + Cu After several reactions & drying: Mass of crucible & lid + CuxOy g g g If estimate 1.5 instead of the 1.4 Empirical formula would be Cu 2 O 3
4 12) % yield lab problems (2): Please calculate the % yield of oxygen based upon these lab results. 2 K(ClO 3 ) (s) 2 KCl (s) + 3 O 2 (g) Before heating: Mass of crucible & cover Mass of crucible & cover + K(ClO3) g g After heating: Mass of crucible & cover + contents g %Yield = Actual/Theoretical (have to do stoichiometry to get!!!) X 100 Actual amount = g, Theoretical = g % yield = 108% 13) Names & Formulas of Compounds (5): A) Cu 3 (PO 4 ) Copper (I) phosphate B) N 2 O 7 Dinitrogen heptoxide C) F 2 Fluorine gas D) Ca +2 Calcium ion E) Phosphide ion P -3 F) Trisulfur heptoxide S 3 O 7 G) Ammonium sulfate (NH 4 ) 2 (SO 4 ) H) Hydrogen H 2 I) Zinc (IV) bromide ZnBr 4 J) Aluminum sulfate Al 2 (SO 4 ) 3 14) Moles (2): A) How many molecules does 15.0 L of sulfur dioxide gas contain? 4.03 X molecules sulfur dioxide B) What is the density of 1 mole of Cl 2 O 7 at STP? D= M/V 8.17 g/l C) What volume will 3.25 X formula units of chlorine gas have at STP? 121 L D) What is identical in 1 mole of water and 1 mole of sugar? What is different? Number of molecules present 6.02 X Grams and volume are different
5 E) 1 mole of N 2 = g = 22.4 L = 6.02 X molecules. F) 1 mole of Au = g = 6.02 X atoms. 16) Acids and Bases (1): A) What is the ph range for a strong acid? 0-3 B) What is the ph range for a strong base? C) What is the ph range for a weak acid? 4-just below 7 D) What is the ph range for a weak base? 10-just above 7 17) Stoichiometry Problems (2): Use the equation below to answer A-C Al 4 C 3 (s) + 12 H 2 O (g) 4 Al(OH) 3 (s) + 3 CH 4 (g) A) Assuming excess amounts of water vapor present, how many atoms of methane gas would be produced from 26.9 g aluminum carbide? 3.37 X atoms methane gas B) If 45.7 g of aluminum hydroxide were produced, what mass of water was needed? 31.7 g water C) Assuming excess amounts of aluminum carbide, how many grams of methane gas would be produced from 35.7 L of water vapor? 6.39 g methane gas 18) Density, mass and volume (3): A) Please arrange these substances as they would appear in a graduated cylinder: Alcohol density = 0.62 g/ml Mercury density = 13 g/ml Water Air density = g/ml air, alcohol, water, mercury
6 B) What happens to the mass, volume and density of air that is compressed in a syringe? Why? Mass remains the same (not adding anything), volume decreases (added force), density increases (more mass in a smaller space) C) What happens to the density of a wooden block when it is cut in half? Why? Density stays the same the volume decreased the same proportion as the mass D) Please give an example of two objects with the same masses and different volumes. 1 kg bricks and 1 kg feathers E) Please give an example of two objects with the same volumes and different masses. 1 L ketchup and 1 L helium H) The density of air is 2.71 mg/l. How many kl will a sample of air occupy if it has a mass of dkg? (1000 mg = 1 g, 100 g = 1 dkg, 1000 L = 1kL) 27.9 kl J) A rock has a mass of 10.0 g and causes the water level in a graduated cylinder to rise from 15.0 ml to 21.0 ml. What is its density? 10g/6mL = 1.67 g/ml
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