SMHS Chemistry I - Weebly



Name_________________________SMHS Chemistry I Practice North Carolina Final Exam Date…____________DIRECTIONS: For the following exercises, choose the best answer from the responses provided. Only North Carolina approved Chemistry Reference Table (2012) and a calculator may be used.Three isotopes of carbon are indicated below:126C 136C 146CHow are these isotopes alike?They have the same number of protons and the same atomic mass.They have the same number of neutrons and the same atomic mass.They have the same number of protons and the same atomic number.They have the same number of neutrons and the same atomic number.Which statement correctly compares an atom of boron-11 and an atom of carbon-14?An atom of boron-11 has one fewer proton and two fewer neutrons than an atom of carbon-14.An atom of boron-11 has one fewer neutron and two fewer protons than an atom of carbon-14.An atom of boron-11 has one fewer proton and three fewer neutrons than an atom of carbon-14.An atom of boron-11 has one fewer neutron and three fewer protons than an atom of carbon-14.Which best represent the electron configuration for an atom of iron?1s22s22p63s23p64s23d61s21p62s22p63s23p64s21s22s22p63s23p63d81s22s22p63s23p64s24d6How many electrons are in the outermost energy level of an electrically neutral atom of aluminum?13832Which transition occurs when light with a wavelength of 434 nm is emitted by a hydrogen atom?The electron jumps from n = 2 to n = 4.The electron jumps from n = 2 to n = 5.The electron falls from n = 4 to n = 2.The electron falls from n = 5 to n = 2.The nuclear equation below represent the alpha decay of QUOTE 22286Rn:22286Rn → 42He + XWhat is the mass number of the element represented by X?It is 88, because element X gains 2 protons.It is 218, because element X loses 2 protons and 2 neutrons.It is 220, because element X loses 2 neutrons.It is 226, because element X gains 2 protons and 2 neutrons.-2-What best compares the properties of ionic and metallic substances?The bonds of metallic substances are composed of delocalized electrons, and the bonds of ionic substances are composed of transferred electrons.The bonds of metallic substances are composed of isolated electrons, and the bonds of ionic substances are composed of shared electrons.A metallic substance insulates heat and electricity, and solid ionic substances conduct heat and electricity.A metallic substance has a low melting point, and an ionic substance has a low melting point.When aluminum and sulfur react, which compound is produced?Al2S3Al3S2AlS2AlSWhich combination of elements would most likely form and ionic compound?hydrogen and oxygencarbon and chlorinesodium and fluorinesilicon and sulfurWhich is an accurate comparison of bonds that occur between carbon atoms in terms of bond length and strength?Double bonds are shorter than single bonds, but single bonds are stronger than triple bonds.Triple bonds are shorter than double bonds, and double bonds are stronger than single bonds.Double bonds are both shorter and stronger than triple bonds.Triple bonds are the longest and the strongest.Which represents the formula for iron (III) chromate?Fe2(CrO4)3Fe2(CrO4)2Fe3(CrO4)2Fe3(CrO4)3What is the IUPAC name for the chemical formula PbO2?lead oxide B) lead (II) oxideC) lead (IV) oxide D) lead dioxideWhich is true about the melting points of ionic and molecular compounds?The melting points of ionic and molecular compounds are similar.The melting points of ionic compounds are lower than the melting points of molecular compounds.The melting points of ionic and molecular compounds increase with the number of atoms present in the compound.The melting points of ionic compounds are higher than the melting points of molecular compounds.Which pair of elements is both malleable and able to conduct heat?bromine and silveriodine and neoniron and brominesilver and ironWhich group includes elements with the most similar properties?N, O, and FO, S, and SeCr, Pb, and XeBr, Ga, and HgAn atom of which element has the strongest attraction for electrons?BaCsOF-3-What occurs when energy is removed from a liquid-vapor system in equilibrium?The amount of liquid increases.The amount of vapor increases.The amounts of liquid and vapor increase equally.The amounts of liquid and vapor decrease equally.Which best explains the relationship between heat energy and temperature?As heat energy increases and temperature increases, freezing occurs.As heat energy decreases and temperature remains constant, condensation occurs.As heat energy decreases and temperature remains constant, evaporation occurs.As heat energy increases and temperature decreases, melting occurs.Why does it require 5,511 J of heat energy to melt 16.5 g of ice?2,260 J/g of heat energy is absorbed by the ice as it is converted from a solid to a liquid.334 J/g of heat energy is absorbed by the ice as it is converted from a solid to a liquid.4.18 J/g°C of heat energy is required as ice is converted from a solid to a liquid.2.05 J/g°C of heat energy is required as ice is converted from a solid to a liquid.The graph below shows a cooling curve for a sample of gas that is uniformly cooled from 250°C.Why does the freezing point of a substance occur at 50°C?The latent heat energy is absorbed by the substance as it is converted from a liquid to a solid.The latent heat energy is released into the air as the substance s converted from a liquid to a solid.The average kinetic energy is increasing for the substance as it is converted from a solid to a liquid.The average kinetic energy is decreasing for the substance as it is converted from a solid to a liquid.-4-The graph below represents a substance being heated from -30°C to 110°C.11090705030Temperature (°C)1010300 50 100 150 200 250 300 350 400 450Energy Absorbed (kJ)If 50 kJ of heat are removed from the substance when it is at 50°C, what will be the state at temperature of the substance?Gas at 70°CGas at 100°CLiquid at 0°CLiquid at 10°CHow many moles of nitrogen gas are in 135 L of nitrogen gas at standard temperature and pressure (STP)?4.82 moles of N25.53 moles of N26.02moles of N29.64 moles of N2A mixture of gases (NO2, CO2, SO2) is collected in a bottle. The partial pressure of NO2 is 1.25 atm, and the partial pressure of CO2 is 2.63 atm. If the total pressure of the gases is 11.20 atm, what is the partial pressure of SO2? 2.89 atm7.32 atm9.23 atm11.20 atm-5-The graph below represents a generalized potential energy diagram.What can be concluded from the potential energy diagram below?The reaction produced a covalent compound.The reaction produced an ionic compound.The reaction was exothermic.The reaction was endothermic.How does increasing temperature affect the collisions of reactant molecules in a chemical reaction?The reactant molecules collide more frequently with greater energy per collision.The reactant molecules collide more frequently with less energy per collision.The reactant molecules collide less frequently with less energy per collision.The reactant molecules collide less frequently with greater energy per collision.Which reaction produces gas that turns lime water milky?Zn + 2HCl ZnCl2 + H22KClO3 2KCl + 3O2CaCO3CaO + CO22NaCl 2Na + Cl2The chemical reaction below represents an unbalanced chemical reaction:Fe + O2 Fe2O3When the equation is balanced, what coefficient is needed for Fe2O3?1234When AgNO3 (aq) is mixed with NaCl (aq), which type of reaction will occur?Single replacementSynthesisDecompositionDouble replacementHow much mass is in a 3.25-mole sample of NH4OH?10.8 g34.0 g35.1 g114 g-6-The equation below represents a balanced chemical reaction:2Mg(s) + O2(g) 2MgO(s)How many moles of MgO are produced when 7.2 moles O2 react with excess Mg?3.6 moles14 moles22 moles29 molesWhy does the rate of a chemical reaction increase when the surface area of a reactant is increased?When the surface are increases, the reaction temperature increases.When the surface area increases, the number of particle collisions increases.When the surface area increases, the concentration of the substance increases.When the surface area increases, the density of the substance increases.Which best describes the role of enzymes in a chemical reaction?They lower the activation energy in the reaction.They prevent the reaction from occurring.They are produced by the reaction.They are consumed by the reaction.The equation below represents the reaction between nitrogen gas and hydrogen gas to form ammonia. The reaction occurs within a closed container and come to equilibrium:N2 + 3H2 2NH3What expression represents the equilibrium expression for this reaction?A)Keq = NH32N2H23B)Keq = N2H23NH32C)Keq = N2H2NH3D)Keq = N22H22NH33A sample of ammonia gas and hydrogen chloride gas is placed in a sealed container at 25°C and allowed to come to equilibrium according to this equation:NH3 (g) + HCl (g) NH4Cl (s)After equilibrium is established, the container is opened to allow the NH3 (g) and HCl (g) to escape. How would this affect the equilibrium?The reaction would produce less NH3 (g) and HCl (g).The reaction would shift to the right to produce more NH4Cl (s).The reaction would shift to the left to produce more NH3 (g) and HCl (g).The reaction would produce more NH3 (g), HCl (g), and NH4Cl (s) until the original equilibrium is reestablished.-7-Why is KOH considered to be an Arrhenius base?It produces OH+ ions in solution.It produces H+ ions in solution.It produced H- ions in solution.It produces OH- ions in solution.The chart below shows the characteristics of several common acid-base indicators.IndicatorpH RangeColor RangeBromocresol Green3.8 – 5.4Yellow to BlueCongo Red3.0 – 5.0Blue to RedPhenol Red6.8 – 8.2Yellow to RedIndigo Carmine11.6 – 13.0Blue to YellowWhich indicator would appear to be yellow in solution with a hydrogen ion concentration of 1.0 x 10-7?Bromocresol GreenCongo RedPhenol RedIndigo CarmineWhich best describes electrolytic and nonelectrolyte solutions?A) Electrolytic solutions produce ions in solution, while nonelectrolytes do not produce ions in solution.B) Electrolytic solutions include alcohols and sugars, while nonelectrolytes include acids and bases.C) Electrolytic solutions are not able to conduct electricity, while nonelectrolytes are able to conduct electricity.D) Electrolytic solutions are composed of polar covalent substances, while nonelectrolytes are composed of ionic compounds.38. The graph below shows the solubility of various compounds.At what temperature will 50 g of NH4Br produce a saturated solution when dissolved in 100 g of water?A) 45°CB) 56°CC) 60°C D) 66°C-8-The graph below shows the solubility of various compounds.Which salt solution could contain approximately 50 g of solute per 100 g of water at 80°C?A saturated solution of KClA saturated solution of KNO3An unsaturated solution of NaClA supersaturated solution of NH4ClWhen table salt (NaCl) is dissolving in water (H2O), what happens to the attraction between the salt ions and the oxygen atoms of the water?The chlorine ion is attracted to the partial negative charge of the oxygen atoms.The chlorine ion is attracted to the partial positive charge of the oxygen atoms.The sodium ion is attracted to the partial negative charge of the oxygen atoms.The sodium ion is attracted to the partial positive charge of the oxygen atoms.41. What is the chemical formula for magnesium bromate?MgBr B) MgBr2 C) MgBrO3D) Mg(BrO3)242. How are compounds with metallic bonds similar to ionic compounds?Both tend to have double and triple bonds.Both tend to have low boiling points.Both tend to have poor conductivity.Both tend to have high melting points.-9-43. Which of these elements has the greatest atomic radius?A) H B) NC) ClD) Cs44. How does the amount of heat energy change as a 250-g sample of water is heated from 5.0°C to 30.0°C?The amount of heat energy increases, causing the water to sublime.The amount of heat energy increases, causing the water to evaporate.As the temperature increases, the amount of heat energy decreases.As the temperature increases, the amount of heat energy increases.45. This graph represents data collected when a sample of a gas is uniformly cooled from 155°C. Why does the temperature of the sample remain constant between point X and point Y?because the sample is transitioning from a gaseous state to a solid statebecause the sample is transitioning from a gaseous state to a liquid statebecause the sample is transitioning from a solid state to a gaseous statebecause the sample is transitioning from a liquid state to a solid state46. When a gamma ray is emitted by an element, what happens to the atomic mass and the atomic number?The atomic mass stays the same, and the atomic number stays the same.The atomic mass changes, and the atomic number stays the same.The atomic mass stays the same, and the atomic number changes.The atomic mass changes, and the atomic number changes.47. How does a single covalent bond between two carbon atoms compare to a double covalent bond between two carbon atoms?A single covalent bond is stronger and has a longer bond length than a double covalent bond.A single covalent bond is stronger and has a shorter bond length than a double covalent bond.A single covalent bond is weaker and has a shorter bond length than a double covalent bond.A single covalent bond is weaker and has a longer bond length than a double covalent bond.-10-48. The phases of a substance under various pressure and temperature combinations are shown on this phase diagram.What occurs if the pressure of the substance at point F remains constant, and the temperature increases to point G?It will transition from a solid state to a liquid state.It will transition from a liquid state to a solid state.It will transition from a solid state to a gaseous state.It will transition from a gaseous state to a solid state.49. The potential energy diagram of a chemical reaction is shown below. Which best describes the energy in the chemical reaction?Heat energy was released.Energy was lowered by a catalyst.8 J of energy were required to start the reaction.10 J of energy were required to start the reaction.-11-50. This balanced chemical equation represents a chemical reaction:6NO + 4NH3 → 5N2 + 6H2OWhat volume of NH3 gas, at Standard Temperature and Pressure (STP), is required to react with 15.0 g of NO?A) 5.68 L B) 7.47 L C) 10.0 L D) 11.2 L51. The equation represents a chemical reaction at equilibrium.HCl (aq) + Mg (s) → MgCl2 (aq) + H2 (g) + heat What happens to the system when the temperature is decreased?The reaction shifts toward the right, and the amount of hydrogen gas increases.The reaction shifts toward the right, and the amount of hydrogen gas decreases.The reaction shifts toward the left, and the amount of hydrogen gas increases.The reaction shifts toward the left, and the amount of hydrogen gas decreases.52. This equation represents a chemical reaction at equilibrium:2SO2 (g) + O2 (g) → 2SO3 (g) What will happen when the concentration of SO3 is increased?The reaction shifts to the right, and concentrations of SO2 (g) and O2 (g) decrease.The reaction shifts to the right, and concentrations of SO2 (g) and O2 (g) increase.The reaction shifts to the left, and concentrations of SO2 (g) and O2 (g) decrease.The reaction shifts to the left, and concentrations of SO2 (g) and O2 (g) increase.53. A student conducts an experiment to identify the pH of some common household substances. The data is recorded in this table.Which substance would be classified as containing the highest concentration of hydroxide ions?A) ammonia B) drain cleanerC) lemon juice D) vinegar-12-54. A newly synthesized ionic compound is placed in water to make an aqueous solution. Which best describes the new ionic solution?The ionic solution conducts electricity.The ionic solution dissolves nonpolar solutions.The ionic solution cannot conduct electricity.The ionic solution is a neutral solution.55. Why is potassium chloride able to dissolve in water?because potassium ions are attracted to the partial negative charge of hydrogenbecause potassium ions are attracted to the partial positive charge of hydrogenbecause potassium ions are attracted to the partial negative charge of oxygenbecause potassium ions are attracted to the partial positive charge of oxygen56. Which occurs if an electron transitions from n = 5 to n = 2 in a hydrogen atom?Energy is absorbed, and visible light is emitted.Energy is released, and visible light is emitted.Energy is released, and visible light is not emitted.Energy is absorbed, and visible light is not emitted.57. Which of the following is not considered to be an electrolyte?Sodium chloride (NaCl)Glucose (C6H12O6)Sodium phosphate (Na3PO4)Hydrogen sulfide (H2S)58. Adding sodium chloride to water will cause theA) boiling point to drop and the freezing point to rise. B) both the boiling point and the freezing point to drop.C) both the boiling point and the freezing point to rise. D) boiling point to rise and the freezing point to drop.59. Which of the following substances would be predicted to have the greatest solubility in benzene, C6H6, which is a nonpolar solvent?A) NaCl; B) C8H18; C) H2O; D) K3PO4; E) solid aluminum metal60. Which of the following shows the most metallic character?A) As; B) Sb; C) Ba; D) Te; E) Cd.#Ans.#Ans.#Ans.#Ans.1C16D31B46A2A17A32A47D3A18B33A48C4C19B34C49C5D20B35D50B6B21D36C51A7A22C37A52D8A23B38A53B9C24C39A54A10B25A40C55C11A26C41D56B12C27B42D57B13D28D43D58D14D29D44D59B15B30B45B60CChemistry I-HNorth Carolina Final Exam Analysis WorksheetDIRECTIONS: Use the item analysis chart below and the answer key to determine at least two priority topics for you to study. These priority topics should focus on the areas in which you missed the most questions.Priority Topic #1: ________________________________________Priority Topic #2: ________________________________________Priority Topic #3: ________________________________________Reflection Questions1. Of the topics you chose as priority, do you notice any trends in the types of questions you missed? An example might be that most of your missed questions may come from the Nomenclature unit and upon further analysis you find that you missed naming all of the ionic compounds.2. What types of questions were you the most successful on? Do you think you should spend much time reviewing these topics?======= Item Analysis =============================================================1Atomic Theory2Atomic Theory3Quantum Theory4Periodic Properties5Quantum Theory6Nuclear Chemistry7Nomenclature8Nomenclature9Nomenclature10Chemical Bonding11Nomenclature12Nomenclature13Nomenclature14Nomenclature15Periodic Properties16Periodic Properties17States of Matter18States of Matter19States of Matter20States of Matter21States of Matter22Gas Laws23Gas Laws24Chemical Reactions25Chemical Reactions26Chemical Reactions27Chemical Reactions28Chemical Reactions29Mole Concept30Stoichiometry31Chemical Reactions32Chemical Reactions33Equilibrium34Equilibrium35Acid-Base Chemistry36Acid-Base Chemistry37Solutions38Solutions39Solutions40Solutions41Nomenclature42Nomenclature43Periodic Properties44States of Matter45States of Matter46Nuclear Chemistry47Chemical Bonding48States of Matter49Chemical Reactions50Stoichiometry51Equilibrium52Equilibrium53Acid-Base Chemistry54Nomenclature55Solutions56Quantum Theory57Solutions58Solutions59Solutions60Periodic Properties ................
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