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Multiple Choice Questions (1 Mark Each, Total Marks = 50) Your multiple choice answers MUST be transferred to the scantron DURING the time allotted for the test. ONLY THE ANSWERS ON THE SCANTRON SHEET WILL BE SCORED 1) Choose the best Lewis structure for BeF 2 . A) B) C) D) E) 2) Determine the identity of the daughter nuclide from the positron emission of O. A) F B) C C) N D) C E) N 3) Determine the molecular geometry for the molecule PCl 5 . A) Linear B) Square planar C) Trigonal bipyramidal D) Square pyramidal E) Seesaw 4) Calculate the amount of heat (in kJ) required to raise the temperature of a 79.0 g sample of ethanol from 298.0 K to 385.0 K. The specific heat capacity of ethanol is 2.42 J g -1 °C -1 . A) 16.6 kJ B) 73.6 kJ C) 28.4 kJ D) 12.9 kJ E) 57.0 kJ 5) Give the approximate bond angle for a molecule with an octahedral shape. A) 109.5° B) 180° C) 120° D) 105° E) 90° 6) What element is being oxidized in the following (unbalanced) redox reaction? Zn 2 + ( aq ) + NH 4 + ( aq ) → Zn( s ) + NO 3 ⁻( aq ) A) N B) O C) Zn D) H This study source was downloaded by 100000875719904 from CourseHero.com on 11-30-2023 14:39:16 GMT -06:00 https://www.coursehero.com/file/55715040/CHMA10-Final-Exam-Practice-Version-1pdf/

7) Choose the best Lewis structure for SO 4 2 ⁻. A) B) C) D) E) 8) Which molecule or compound below contains a polar covalent bond? A) NCl 3 B) AgCl C) ZnS D) C 2 H 4 E) LiI 9) Choose the statement that is TRUE. A) Valence electrons are the most difficult of all electrons to remove. B) Core electrons are the easiest of all electrons to remove. C) Core electrons effectively shield outer electrons from nuclear charge. D) Outer electrons efficiently shield one another from nuclear charge. 10) Define sublimation. A) the phase transition from gas to solid B) the phase transition from solid to gas C) the phase transition from liquid to solid D) the phase transition from liquid to gas E) the phase transition from gas to liquid This study source was downloaded by 100000875719904 from CourseHero.com on 11-30-2023 14:39:16 GMT -06:00 https://www.coursehero.com/file/55715040/CHMA10-Final-Exam-Practice-Version-1pdf/

11) Give the number of valence electrons for SF 4 . A) 32 B) 30 C) 34 D) 28 12) Use the information provided to determine H ° for the following reaction: H ° (kJ ) 3Fe 2 O 3 ( s ) + CO( g ) → 2Fe 3 O 4 ( s ) + CO 2 ( g ) H ° = ? Fe 2 O 3 ( s ) -824 Fe 3 O 4 ( s ) -1118 CO( g ) -111 CO 2 ( g ) -394 A) -111 kJ mol -1 B) +144 kJ mol -1 C) +277 kJ mol -1 D) -47 kJ mol -1 E) -577 kJ mol -1 13) Choose the compound that exhibits hydrogen bonding as its strongest intermolecular force. A) CH 2 F 2 B) SCl 2 C) CH 3 OH D) C 2 H 6 E) None of the above compounds exhibit hydrogen bonding. 14) The following reaction represents what nuclear process? Pb → e + Bi A) electron capture B) alpha emission C) neutron bombardment D) beta emission E) gamma emission 15) Describe a pi bond. A) side by side overlap of p orbitals B) overlap of two s orbitals C) end to end overlap of p orbitals D) p orbital overlapping with a d orbital E) s orbital overlapping with the end of a p orbital 16) What mass of ethane (CH 3 CH 3 ) is contained in 50.0 mL of a 13.9% by mass solution of ethane in hexane? The density of the solution is 0.611 g mL -1 . A) 2.35 g B) 8.49 g C) 4.25 g D) 11.8 g E) 6.95 g This study source was downloaded by 100000875719904 from CourseHero.com on 11-30-2023 14:39:16 GMT -06:00 https://www.coursehero.com/file/55715040/CHMA10-Final-Exam-Practice-Version-1pdf/

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17) Which of the following represent the Lewis structure for Ca 2 ⁺? A) B) C) D) E) 18) Consider the molecule below. Determine the molecular geometry at each of the three labelled atoms. A) 1 = trigonal planar, 2 = tetrahedral, 3 = trigonal pyramidal B) 1 = trigonal planar, 2 = trigonal pyramidal, 3 = trigonal pyramidal C) 1 = trigonal planar, 2 = tetrahedral, 3 = tetrahedral D) 1 = tetrahedral, 2 = tetrahedral, 3 = trigonal planar E) 1 = tetrahedral, 2 = tetrahedral, 3 = tetrahedral 19) Place the following elements in order of increasing electronegativity. K Cs P A) Cs < P < K B) K < P < Cs C) Cs < K < P D) P < K < Cs E) P < Cs < K 20) Use the bond energies provided to estimate Δ r H ° for the reaction below. PCl 3 ( g ) + Cl 2 ( g ) → PCl 5 ( l ) Δ r H ° = ? Bond Bond Energy (kJ mol -1 ) Cl-Cl 243 P-Cl 331 A) -905 kJ mol -1 B) -419 kJ mol -1 C) -67 kJ mol -1 D) -243 kJ mol -1 E) -662 kJ mol -1 21) Identify the strongest bond. A) single covalent bond B) double covalent bond C) triple covalent bond D) All of the above bonds are the same strength. This study source was downloaded by 100000875719904 from CourseHero.com on 11-30-2023 14:39:16 GMT -06:00 https://www.coursehero.com/file/55715040/CHMA10-Final-Exam-Practice-Version-1pdf/

22) The volume of a gas is inversely proportional to the pressure of a gas. What is this known as? A) Avogadro's law B) Ideal gas law C) Charles's law D) Boyle's law E) Dalton's law 23) List the number of sigma bonds and pi bonds in a triple bond. A) 2 sigma, 1 pi B) 3 sigma, 0 pi C) 1 sigma, 2 pi D) 1 sigma, 1 pi 24) Identify the number of electron groups around a molecule with sp 2 hybridization. A) 1 B) 2 C) 3 D) 4 E) 5 25) Write a nuclear equation for the alpha decay of Am. A) Am → He + Np B) Am → e + Pu C) Am → n + Am D) Am → e + Cm E) Am → He + Bk 26) Place the following elements in order of decreasing atomic radius. Xe Rb Ar A) Ar > Xe > Rb B) Rb > Xe > Ar C) Ar > Rb > Xe D) Rb > Ar > Xe E) Xe > Rb > Ar 27) Identify the ground-state electron configuration for Se. A) [Ar]4 s 2 3 d 10 4 p 4 B) [Ar]4 s 2 3 d 10 4p 6 C) [Ar]4 s 2 3 d 10 D) [Ar]4 s 2 4 d 10 4 p 4 E) [Ar]3 d 10 4 p 4 28) Identify what a bomb calorimeter measures. A) measures Δ H for reduction reactions B) measures Δ H for oxidation solutions C) measures Δ H for aqueous solutions D) measures Δ U for combustion reactions E) measures Δ T for hydrolysis solutions This study source was downloaded by 100000875719904 from CourseHero.com on 11-30-2023 14:39:16 GMT -06:00 https://www.coursehero.com/file/55715040/CHMA10-Final-Exam-Practice-Version-1pdf/

29) Give the approximate bond angle between two equatorial positions for a molecule with a trigonal bipyramidal geometry. A) 109.5° B) 180° C) 120° D) 105° E) 90° 30) Consider the molecule below. Determine the hybridization at each of the two labelled carbons. A) C1 = sp 2 , C2 = sp 3 B) C1 = sp 3 , C2 = sp 3 d C) C1 = sp 2 , C2 = sp 3 d D) C1 = sp , C2 = sp 2 E) C1 = sp 3 d , C2 = sp 3 d 2 31) Choose the valence orbital diagram that represents the ground state of Zn. A) B) C) D) E) This study source was downloaded by 100000875719904 from CourseHero.com on 11-30-2023 14:39:16 GMT -06:00 https://www.coursehero.com/file/55715040/CHMA10-Final-Exam-Practice-Version-1pdf/

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32) Using the graph below, determine the gas that has the lowest density at STP. A) A B) B C) C D) D E) All of the gases have the same density at STP. 33) Place the following elements in order of decreasing electronegativity. S Cl Se A) S > Cl > Se B) Se > Cl > S C) Cl > S > Se D) Se > S > Cl E) Cl > Se > S 34) Determine the identity of the daughter nuclide from the positron emission of C. A) C B) B C) B D) N E) N 35) Place the following ions in order of increasing radius. Ca 2 ⁺ S 2 ⁻ Cl⁻ A) Ca 2 ⁺ < S 2 ⁻ < Cl⁻ B) Ca 2 ⁺ < Cl⁻< S 2 ⁻ C) Cl⁻ < Ca 2 ⁺ < S 2 ⁻ D) Cl⁻ < S 2 ⁻ < Ca 2 ⁺ E) S 2 ⁻ < Cl⁻ < Ca 2 ⁺ This study source was downloaded by 100000875719904 from CourseHero.com on 11-30-2023 14:39:16 GMT -06:00 https://www.coursehero.com/file/55715040/CHMA10-Final-Exam-Practice-Version-1pdf/

36) Which of the following statements is TRUE? A) Beta radiation has the highest ionizing power of any radioactivity. B) Gamma radiation has the lowest penetrating power. C) Gamma rays have the lowest ionizing power of any radioactivity. D) Beta emitters will do more damage than alpha emitters within the body. E) Alpha radiation has the highest penetrating power of any radioactivity. 37) Which of the following represent the Lewis structure for Cl? A) B) C) D) E) 38) Use the standard reaction enthalpies given below to determine H ° for the following reaction: 2S( s ) + 3O 2 ( g ) → 2SO 3 ( g ) H ° = ? Given: SO 2 ( g ) → S( s ) + O 2 ( g ) H ° = +296.8 kJ 2SO 2 ( g ) + O 2 ( g ) → 2SO 3 ( g ) H ° = -197.8 kJ A) -293.0 kJ mol -1 B) -791.4 kJ mol -1 C) 1583 kJ mol -1 D) -692.4 kJ mol -1 E) -494.6 kJ mol -1 39) How many of the following elements have one unpaired electron in the ground state? B Al S Cl A) 1 B) 2 C) 3 D) 4 40) In molecular orbital theory the acronym HOMO stands for A) homogenous orbital-molecular orientation. B) highly ordered molecular orbital. C) highest orbital-molecular orientation. D) highest occupied molecular orbital. E) It has no meaning. 41) Which molecule or compound below contains a pure covalent bond? A) PF 3 B) Cl 2 C) Li 2 CO 3 D) SCl 6 E) NaCl 42) Which particle has the lowest penetrating power? A) positron emission B) electron capture C) alpha particle D) beta particle E) gamma rays 43) Place the following in order of decreasing metallic character. P As K A) K > P > As B) As > K > P C) K > As > P D) P > As > K E) As > P > K This study source was downloaded by 100000875719904 from CourseHero.com on 11-30-2023 14:39:16 GMT -06:00 https://www.coursehero.com/file/55715040/CHMA10-Final-Exam-Practice-Version-1pdf/

44) Determine the electron geometry (eg) and molecular geometry (mg) of SiF 4 . A) eg = octahedral, mg = square planar B) eg = tetrahedral, mg = tetrahedral C) eg = trigonal bipyramidal, mg = trigonal pyramidal D) eg = tetrahedral, mg = trigonal pyramidal E) eg = tetrahedral, mg = bent 45) Choose the bond below that is most polar. A) C-O B) C-C C) C-N D) F-F E) C-F 46) A solution containing less solute than the equilibrium amount is called A) a saturated solution. B) an unsaturated solution. C) a concentrated solution. D) a supersaturated solution. E) a dilute solution. 47) A molecule containing a central atom with sp hybridization has a ________ electron geometry. A) tetrahedral B) trigonal bipyramidal C) trigonal planar D) linear E) bent 48) Identify triple point. A) the temperature, pressure, and density for a gas B) the temperature at which the solid and liquid coexist C) the temperature that is unique for a substance D) the temperature and pressure where liquid, solid, and gas are equally stable and are in equilibrium E) the temperature at which the boiling point equals the melting point 49) Which of the following quantum numbers describes the size and energy of an orbital? A) angular momentum quantum number B) Schrödinger quantum number C) magnetic quantum number D) spin quantum number E) principal quantum number 50) Determine the molecular geometry for the molecule BrF 3 . A) Square planar B) Square pyramidal C) Seesaw D) T-shaped E) Trigonal planar This study source was downloaded by 100000875719904 from CourseHero.com on 11-30-2023 14:39:16 GMT -06:00 https://www.coursehero.com/file/55715040/CHMA10-Final-Exam-Practice-Version-1pdf/ Powered by TCPDF (www.tcpdf.org)

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