Straighterline Chemistry Final Exam | Verified with 100% Correct Answers

Straighterline Chemistry Final Exam | Verified with 100% Correct Answers What is the term used for findings that are summarized based on a pattern or trend? a. Law b. Hypothesis c. Theory d. Phenomena e. Prediction Which of the following is a tentative explanation for a set of observations? a. Law b. Hypothesis c. Theory d. Phenomena e. Prediction If a liquid contains 60% sugar and 40% water throughout its composition then what is it a. Solute b. Compound c. Homogeneous mixture d. Heterogeneous mixture e. Solvent Which of the following does not have a uniform composition throughout? a. Element b. Compound c. Homogeneous mixture d. Heterogeneous mixture e. Solvent Which one of these represents a physical change? a. Water, when heated, forms steam. b. Bleach turns hair yellow. c. Sugar, when heated, becomes brown. d. Milk turns sour. e. Apples, when exposed to air, turn brown. How many micrograms are in 65.3 kg? a. 0.653 μg b. 6.53 × 107 μg c. 6.53 × 104 μg d. 6.53 × 10-8 μg e. 6.53 × 1010 μg A smart phone has dimensions of 4.9 inches (height), 2.3 inches (width) and 8.0 millimeters (depth). What is the volume of the smart phone in cubic centimeters? (1 in = 2.54 cm) a. 58 cm3 b. 1.7 x 105 cm3 c. 90 cm3 d. 3.4 cm3 e. 34 cm3 Given that 1 inch = 2.54 cm, 1.00 cm3 is equal to a. 16.4 in3 b. 6.45 in3 c. 0.394 in3 d. 0.155 in3 e. 0.0610 in3 What terms defines a mass which is exactly equal to 1/12 the mass of one carbon-12 atom? a. Isotope number b. Mass number c. Mass-to-charge ratio d. Atomic number e. Atomic mass unit How many neutrons are there in an atom of lead whose mass number is 208? a. 82 b. 126 c. 208 d. 290 e. none of them Which of these elements is chemically similar to magnesium? a. Sulfur b. Calcium c. Iron d. Nickel e. Potassium C(graphite) and C(diamond) are examples of: a. isotopes of carbon. b. allotropes of carbon. c. the law of definite proportions. d. different carbon ions. The 80Br- ion has a. 45 protons, 35 neutrons, 45 electrons. b. 35 protons, 45 neutrons, 34 electrons. c. 35 protons, 45 neutrons, 36 electrons. d. 45 protons, 35 neutrons, 46 electrons. e. 35 protons, 45 neutrons, 46 electrons. The formula for sodium sulfide is a. NaS b. K2S c. NaS2 d. Na2S e. SeS Which one of the following formulas of ionic compounds is the least likely to be correct? a. NH4Cl b. Ba(OH)2 c. Na2SO4 d. Ca2NO3 e. Cu(CN)2 What is the name of ClO - ion? a. hypochlorite b. chlorate c. chlorite d. perchlorate e. perchlorite Which of the following is a molecular formula for a compound with an empirical formula of CH? a. C2H6 b. C3H9 c. C4H10 d. C6H6 e. None of the answers is correct. Which is the correct electron configuration for gold? a. [Xe]4f145d96s2 b. [Xe]4f145d106s2 c. [Xe]4f135d106s2 d. [Xe]4f145d106s1 e. None of the electron configurations is correct. A(n) _________ is a point at which a standing wave has zero amplitude. a. crevice b. node c. pit d. burrow e. orbital The Pauli exclusion principle states that no ____ electrons within an atom can have the same ____ quantum numbers. a. 4; 6 b. 2; 4 c. 3; 6 d. 6; 10 e. 3; 8 Emission spectra a. cannot be used to identify an unknown atom. b. can be used to identify unknown atoms. c. can be explained by the movement of protons colliding with electrons. d. none of the. Which one of the following equations correctly represents the process relating to the ionization energy of X? a. X(s) → X+(g) + e- b. X2(g) → X+(g) + X-(g) c. X(g) + e- → X-(g) d. X-(g) → X(g) + e- e. X(g) → X+(g) + e- Consider the element with the electron configuration [Kr]5s24d105p5. This element is a. a halogen. b. a transition metal. c. an alkali metal. d. an actinide element. e. a noble gas. Consider the element with the electron configuration [Kr]5s24d7. This element is a. a halogen. b. a transition metal. c. a nonmetal. d. an actinide element. e. a noble gas. How does atomic radius change as you move across the periodic table? a. Atomic radius decreases moving from left to right across a period and increases from top to bottom. b. Atomic radius increases moving left to right across a period and decreases from top to bottom. c. Smaller nuclear charge lowers energy; more electrons in an orbital lowers energy. d. Atomic radius increases diagonally across the periodic table. e. None of the answers is correct. Which of these choices is the electron configuration of the iron(III) ion? a. [Ar]3d5 b. [Ar]4s13d5 c. [Ar]4s23d3 d. [Ar]3d6 e. [Ar]4s23d9 An element with the general electron configuration for its outermost electrons of ns2np1 would be in which element group? a. 2A b. 3A c. 4A d. 5A e. 8A The effective nuclear charge for an atom is less than the actual nuclear charge due to a. shielding. b. penetration. c. paramagnetism. d. electron-pair repulsion. e. relativity. Which pair of ions exhibits the greatest attractive force between them? a. Na+ and Cl- b. Ca2+ and Cl- c. Na+ and S2- d. Al3+ and Mg2+ e. Mg2+ and O2- Which of the following is a basic oxide? a. P4O10 b. MgO c. Al2O3 d. SO2 e. Cl2O7 Which of these compounds is most likely to be covalent? a. Rb2S b. SrCl2 c. CS2 d. CaO e. MgI2 In the Lewis structure of the iodate ion, IO3-, that satisfies the octet rule, the formal charge on the central iodine atom is a. 2. b. 1. c. 0. d. -1. e. -2. Which molecule has the largest dipole moment? a. HF b. HI c. HBr d. HCl e. All of the molecules have the same dipole moment. In which of the following species does the central atom violate the octet rule? a. CH4 b. SF4 c. PCl4+ d. CCl3+ e. NH3 Which of these ionic solids would have the largest lattice energy? a. NaCl b. NaF c. CaBr2 d. CsI e. CaCl2 The total number of bonding electrons in a molecule of formaldehyde (H2CO) is a. 3. b. 4. c. 6. d. 8. e. 18. Which of the following molecules has a nonzero dipole moment? a. BeCl2 b. SF2 c. KrF2 d. CO2 e. CCl4 According to the VSEPR model, a molecule with the general formula AB5 with one lone pair on the central atom will have a ______ molecular geometry. a. tetrahedral b. trigonalbipyramidal c. square pyramidal d. octahedral e. seesaw Which is the most reasonable prediction for the three F-Br-F bond angles in BrF3? a. 90°, 90°, and 180° b. 86°, 94°, and 180° c. 86°, 86°, and 172° d. 94°, 94°, and 172° e. 120°, 120°, and 120° When PCl5 solidifies it forms PCl4+cations and PCl6- anions. According to valence bond theory, what hybrid orbitals are used by phosphorus in the PCl4+cation? a. sp b. sp2 c. sp3 d. sp3d e. sp3d2 What is the number of lone electron pairs on the central atom of a molecule having a trigonal pyramidal molecular geometry, such as NH3? a. 1 b. 2 c. 3 d. 0 e. 4 For which one of the following molecules is the indicated type of hybridization not appropriate for the central atom? a. BeCl2; sp2 b. SiH4; sp3 c. BF3; sp2 d. C2H2; sp e. H2O; sp3 According to the VSEPR model, the predicted molecular geometry of ammonia, NH3, is a. linear. b. trigonal planar. c. bent. d. tetrahedral. e. trigonal pyramidal. What is the mass of one copper atom? (NA = 6.022 × 1023 mol-1) a. 1.055 × 10-22 g b. 63.55 g c. 1 amu d. 1.66 × 10-24 g e. 9.476 × 1021 g What is the percent sulfur in iron(III) sulfate? a. 28% b. 32% c. 24% d. 48% e. 42% Proteins found in humans are polymers that consist of different combinations of 20 amino acids. Proline, one of the 20 amino acids, has the molecular formula, C5H9NO2. If a human protein has 25 proline monomers, how many carbon atoms from proline are present in the protein? a. 4 C atoms b. 25 C atoms c. 40 C atoms d. 100 C atoms e. 125 C atoms Aluminum oxide, Al2O3, is used as a filler for paints and varnishes as well as in the manufacture of electrical insulators. Calculate the number of moles in 47.51 g of Al2O3. a. 2.377 mol b. 2.146 mol c. 1.105 mol d. 0.4660 mol e. 0.4207 mol Once the following equation is balanced with the smallest set of whole number coefficients, what is the sum of the coefficients? (Don't forget to include coefficients of one.) __ SF4 + __ H2O → __ H2SO3 + __ HF a. 4 b. 6 c. 7 d. 9 e. None of these answers is correct. What is the theoretical yield of chromium that can be produced by the reaction of 40.0 g of Cr2O3 with 8.00 g of aluminum according to the chemical equation below? 2Al + Cr2O3 → Al2O3 + 2Cr a. 7.7 g b. 15.4 g c. 27.4 g d. 30.8 g e. 49.9 g Which one of the following is a strong acid? a. CH3COOH b. H2SO3 c. NH3 d. H3PO4 e. HClO3 Which is a Lewis acid? a. CH3NH2 b. BCl3 c. F- d. BF4- e. CH4 Which is an amphoteric oxide? a. Na2O b. MgO c. Al2O3 d. SO2 e. Cl2O7 What is the value of the equilibrium constant for the autoionization of water at 25°C? a. 1.0 × 10-7 b. 1.0 × 10-14 c. 1.0 × 1014 d. 1.0 × 107 e. 14 Which is the strongest acid? a. SO42- b. H2SO3 c. H2SO4 d. HSO4- e. HSO3- In the van der Waals equation, the constant b is a constant that is part of a correction factor for _________. a. the volume of the gas b. the temperature of the gas c. the pressure of the gas d. the ideal gas constant A sample of nitrogen gas at 298 K and 745 torr has a volume of 37.42 L. What volume will it occupy if the pressure is increased to 894 torr at constant temperature? a. 22.3 L b. 31.2 L c. 44.9 L d. 112 L e. 380 L If the atmospheric pressure in Denver is 0.8800 atm, what is this pressure expressed in mmHg? (1 atm = 101,325 Pa = 760 torr, 1 torr = 1 mmHg)? a. 151.5 mmHg b. 1.16 × 10-3 mmHg c. 863.6 mmHg d. 8.92 × 104 mmHg e. 668.8 mmHg What are the conditions of STP? a. 0 K and 1 atm b. 273.15 K and 760 torr c. 0°C and 760 atm d. 273.15°C and 760 torr e. 0°C and 1 torr In the van der Waals equation, the constant a is a constant that is part of a correction factor for _________. a. the volume of the gas b. the temperature of the gas c. the pressure of the gas d. the ideal gas constant Which substance will exhibit hydrogen bonding between molecules? a. (CH3)3N b. CH3-O-CH3 c. CH3CH2-OH d. CH3CH2-F e. HI Which of the following statements is true? a. The higher the viscosity, the faster a liquid flows. b. The viscosity increases with increasing temperature. c. The stronger the intermolecular forces, the higher the viscosity. d. Hydrogen bonding in water gives rise to its unusually low viscosity. e. The viscosity of gases is larger than the viscosity of liquids. If liquid bromine is cooled to form a solid, which type of solid does it form? a. atomic b. metallic c. molecular d. ionic e. covalent In a sample of hydrogen iodide, __________________ are the most important intermolecular forces. a. dipole-dipole forces b. London dispersion forces c. hydrogen bonding d. covalent bonds e. polar covalent bonds Krypton has a higher melting point than argon because of its a. hydrogen bonding. b. stronger dispersion forces. c. permanent dipole moment. d. ionic bonds. e. greater ionization energy. Lead crystallizes in the face-centered cubic lattice. What is the coordination number for Pb? a. 4 b. 6 c. 8 d. 10 e. 12 What states that the solubility of a gas in a liquid is proportional to the pressure of the gas over the solution? a. Entropy b. Henry's law c. Dissolution d. Vapor pressure e. Enthalpy of salvation Which of the following pairs of liquids is least likely to be miscible? a. Hexane-heptane b. Hexane-benzene c. Hexane-acetic acid d. Hexane-diethyl ether e. Acetic acid-acetone What is the name given to a solution that contains less solute than it has the capacity to dissolve? a. Unsaturated b. Saturated c. Solvented d. Oversaturated e. Supersaturated An emulsion is a dispersion consisting of a a. solid in a liquid. b. liquid in a liquid. c. gas in a liquid. d. liquid in a solid. e. gas in a solid. Which is true regarding the solvation of a solute in a solvent? a. Separation of solute molecules from one another is an endothermic process, and separation of solvent molecules from one another is an exothermic process. b. Separation of solute molecules from one another is an exothermic process, and separation of solvent molecules from one another is an endothermic process. c. Separation of solute molecules from one another, and separation of solvent molecules from one another, are both endothermic processes. d. Separation of solute molecules from one another, and separation of solvent molecules from one another, are both exothermic processes. e. Separation of solute molecules from one another, and separation of solvent molecules from one another, both result in a decrease in entropy. What name is given to a minor component in a solution? a. Solvent b. Unsaturated c. Saturated d. Solute e. Supersaturated Which compound has the lowest solubility in pure water? a. Ag2C2O4, Ksp = 1.0 × 10-11 b. PbCl2, Ksp = 1.7 × 10-5 c. FePO4, Ksp = 1.3 × 10-22 d. Ca3(PO4)2, Ksp = 1.2 × 10-26 e. MgF2, Ksp = 6.9 × 10-9 What happens to the solution if sodium acetate is added to a solution of acetic acid? CH3COOH(aq) Picture H+(aq) + CH3COO-(aq) a. The equilibrium shifts to the right. b. There is an increase in percent ionization of acetic acid. c. Less of hydrogen ion is consumed. d. There is an increased concentration of acetate ions. e. Less of the acetate ion is consumed. Which is more soluble in an acidic solution than in pure water? a. CuI b. PbCl2 c. Ca3(PO4)2 d. NaNO3 e. NaBr What is the name of the principle of selective precipitation used to identify the types of ions present in a solution? a. Ionization b. Selective ion precipitation c. Selective ion typing d. Limited precipitation e. Qualitative analysis Methyl red is a common acid-base indicator. It has a Ka equal to 6.3 × 10-6. Its un-ionized form is red and its anionic form is yellow. What color would a methyl red solution have at pH = 7.8? a. green b. red c. blue d. yellow e. violet When a strong acid is titrated with a weak base, the pH at the equivalence point a. is greater than 7.0. b. is equal to 7.0. c. is less than 7.0. d. is equal to the pKa of the conjugate acid. e. is equal to the pKb of the base. Which is necessary for a process to be spontaneous? a. ΔHsys 0 b. ΔSsys 0 c. ΔSsurr 0 d. ΔSuniv 0 e. ΔGsys = 0 As the molar mass of a compound increases, the entropy ______. a. decreases b. is constant c. increases The most probable state is the one with the _______. a. highest energy b. largest number of possible arrangements c. lowest number of possible arrangements d. most symmetry e. highest enthalpy A spontaneous endothermic reaction always a. causes the surroundings to get colder. b. bursts into flame.