College Chemistry I PHS 1025 Fall 2012 Practice Exam 2B Name

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1 College Chemistry I PHS 1025 Fall 2012 Practice Exam 2B Name MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) Choose the compound below that contains at least one polar covalent bond, but is nonpolar. 1) SCl2 GeH2Br2 AsCl5 D) CF2Cl2 E) All of the above are nonpolar and contain a polar covalent bond. 2) Using periodic trends, place the following bonds in order of increasing ionic character. 2) Si-P Si-Cl Si-S Si-Cl < Si-P < Si-S Si-Cl < Si-S < Si-P Si-P < Si-S < Si-Cl D) Si-P < Si-Cl < Si-S E) Si-S < Si-Cl < Si-P 3) Which of the following contains BOTH ionic and covalent bonds? 3) CaI2 SF6 CaSO4 D) COS E) None of the above contain both ionic and covalent bonds. 4) Determine the electron geometry (eg) and molecular geometry (mg) of XeF2. 4) eg=tetrahedral, mg=bent eg=tetrahedral, mg=linear eg=trigonal bipyramidal, mg=bent D) eg=trigonal bipyramidal, mg=linear E) eg=linear, mg=linear 5) Determine the electron geometry (eg) and molecular geometry (mg) of PF5. 5) eg=trigonal planar, mg=octahedral eg=trigonal bipyramidal, mg=tetrahedral eg=trigonal bipyramidal, mg=trigonal bipyramidal D) eg=tetrahedral, mg=trigonal pyramidal E) eg=octahedral, mg=octahedral 6) Draw the Lewis structure for BrF4 -. What is the hybridization on the Br atom? 6) sp sp2 sp3 D) sp3d E) sp3d2 7) Determine the electron geometry (eg) and molecular geometry (mg) of the underlined carbon in CH3CN. eg=linear, mg=linear eg=trigonal planar, mg=bent eg=tetrahedral, mg=tetrahedral 7)

2 D) eg=trigonal planar, mg=trigonal planar E) eg=linear, mg=trigonal planar 8) Draw the Lewis structure for OF2. What is the hybridization on the O atom? 8) sp3d sp sp3 D) sp3d2 E) sp2 9) List the following compounds in decreasing electronegativity difference. 9) Cl2 HCl NaCl HCl > NaCl > Cl2 NaCl > HCl > Cl2 NaCl > Cl2 > HCl D) Cl2 > HCl > NaCl 10) Which of the following is a molecular compound? 10) SrI2 ZnS NaCN D) LiOH E) P4O10 11) Which molecule or compound below contains an ionic bond? 11) SiF4 OCl2 NH4NO3 D) C2Cl4 E) CO2 12) Choose the best Lewis structure for BF3. 12) D) E) 13) Place the following elements in order of increasing electronegativity. 13) K Cs P K < P < Cs Cs < K < P P < K < Cs

3 D) Cs < P < K E) P < Cs < K 14) Using periodic trends, place the following bonds in order of decreasing ionic character. 14) Sb-Cl P-Cl As-Cl Sb-Cl > P-Cl > As-Cl Sb-Cl > As-Cl > P-Cl As-Cl > Sb-Cl > P-Cl D) P-Cl > As-Cl > Sb-Cl E) Sb-Cl > P-Cl > As-Cl 15) Determine the electron geometry (eg) and molecular geometry(mg) of BCl3. 15) eg=tetrahedral, mg=trigonal pyramidal eg=trigonal planar, mg=trigonal planar eg=trigonal bipyramidal, mg= trigonal bipyramidal D) eg=tetrahedral, mg=trigonal planar E) eg=trigonal planar, mg=bent 16) Determine the electron geometry (eg), molecular geometry(mg) and polarity of XeO3. 16) eg=tetrahedral, mg=trigonal pyramidal, polar eg=octahedral, mg=tetrahedral, nonpolar eg=trigonal bipyramidal, mg=trigonal planar, nonpolar D) eg=trigonal planar, mg=trigonal pyramidal, polar E) eg=trigonal planar, mg=trigonal planar, nonpolar 17) Give the number of valence electrons for XeI2. 17) D) 18 18) Choose the best Lewis structure for NH4+. 18) D)

4 E) 19) Determine the electron geometry (eg), molecular geometry (mg), and polarity of SO3. 19) eg=tetrahedral, mg=trigonal pyramidal, polar eg=trigonal planar, mg=trigonal planar, nonpolar eg=tetrahedral, mg=tetrahedral, nonpolar D) eg= trigonal bipyramidal, mg=trigonal planar, polar E) eg=trigonal pyramidal, mg=bent, nonpolar 20) Choose the bond below that is most polar. 20) C-C C-O C-N D) C-F E) F-F 21) Which of the following represent the Lewis structure for Ca2+? 21) D) E) 22) Which molecule or compound below contains a pure covalent bond? 22) Li2CO3 SCl6 Cl2 D) NaCl E) PF3 23) Determine the name for TiCO3. Remember that titanium forms several ions. 23) titanium (II) carbonite titanium carbide titanium carbonite D) titanium (I) carbonate E) titanium (II) carbonate 24) How many of the following elements can form compounds with an expanded octet? 24) I O Cl Xe D) 2 E) 0 25) Choose the compound below that contains at least one polar covalent bond, but is nonpolar. 25) SeBr4 HCN CF4 D) ICl3 E) Both B and C are nonpolar and contain a polar covalent bond. 26) Give the correct formula for aluminum sulfate. 26) Al(SO4)3 Al2(SO4)3 Al3(SO4)2 D) Al22SO4 27) Give the formula for sodium chlorate. 27)

5 NaClO3 NaClO2 NaClO D) NaClO4 28) How many of the following molecules are polar? 28) BrCl3 CS2 SiF4 SO D) 2 E) 4 29) Write the name for Ca3(PO4)2. 29) tricalcium phosphorustetraoxide calcium phosphate calcium (III) phosphite D) calcium phosphite E) calcium (II) phosphite 30) Use Lewis theory to determine the chemical formula for the compound formed between K and I. 30) KI KI2 K2I D) K2I2 31) Using periodic trends, place the following bonds in order of increasing ionic character. 31) S-F Se-F O-F Se-F < S-F < O-F O-F < S-F < Se-F Se-F < O-F < S-F D) O-F < Se-F < S-F E) S-F < Se-F < O-F 32) Determine the electron geometry (eg) and molecular geometry (mg) of SiF4. 32) eg=trigonal bipyramidal, mg=trigonal pyramidal eg=octahedral, mg=square planar eg=tetrahedral, mg=tetrahedral D) eg=tetrahedral, mg=bent E) eg=tetrahedral, mg=trigonal pyramidal 33) Which of the following represent the Lewis structure for S2? 33) D) E) 34) Choose the best Lewis structure for NO3. 34)

6 D) E) 35) Determine the name for aqueous HBr. 35) bromic acid bromous acid hydrobromic acid D) hydrobromous acid E) hydrogen bromate 36) Give the number of valence electrons for SF4. 36) D) 34 37) Write the name for Sn(SO4)2. Remember that Sn forms several ions. 37) tin (I) sulfate tin sulfide tin (II) sulfite D) tin (IV) sulfate E) tin (I) sulfite 38) A covalent bond is best described as: 38) the sharing of electrons between atoms. the transfer of electrons. a bond between two polyatomic ions. D) a bond between a metal and a polyatomic ion. E) a bond between a metal and a nonmetal. 39) An ionic bond is best described as: 39) the attraction between 2 metal atoms. the transfer of electrons from one atom to another. the attraction between 2 nonmetal atoms. D) the sharing of electrons. E) the attraction that holds the atoms together in a polyatomic ion. 40) Give the electron geometry, molecular geometry, and hybridization for CH ) eg = tetrahedral; mg = trigonal pyramidal; sp3 eg = tetrahedral; mg = tetrahedral; sp3 eg = trigonal planar; mg = trigonal planar; sp2 D) eg = trigonal pyramidal; mg = trigonal pyramidal; sp3 41) Choose the best Lewis structure for BeF2. 41)

7 D) E) 42) Identify the most electronegative element. 42) H Fr F D) At 43) Determine the name for CoCl2 6H2O. Remember that Co forms several ions. 43) cobalt (I) chloride cobalt (II) chloride heptahydrate cobalt chloride hydrate D) cobalt (I) chloride heptahydrate E) cobalt (II) chloride hexahydrate 44) Determine the electron geometry (eg) and molecular geometry (mg) of CO2. 44) eg=trigonal bipyramidal, mg=tetrahedral eg=linear, eg=linear eg=tetrahedral, mg=tetrahedral D) eg=tetrahedral, mg=bent E) eg=octahedral, mg=square planar 45) Draw the Lewis structure for BrCl3. What is the hybridization on the Br atom? 45) sp3d sp sp2 D) sp3d2 E) sp3 46) Use Lewis theory to determine the chemical formula for the compound formed between Ca and N. Ca3N2 CaN CaN2 D) Ca2N3 46) 47) Determine the electron geometry (eg) and molecular geometry (mg) of ICl2. 47) eg=tetrahedral, mg=bent eg=tetrahedral, mg=trigonal pyramidal eg=trigonal bipyramidal, mg=trigonal planar D) eg=trigonal bipyramidal, mg=linear E) eg=octahedral, mg=linear 48) Choose the best Lewis structure for PO )

8 D) E) 49) Give the name for SnO. 49) tin (III) oxide tin (I) oxide tin (IV) oxide D) tin (II) oxide 50) Draw the Lewis structure for NO2 including any valid resonance structures. Which of the following statements is TRUE? The nitrite ion contains one N-O single bond and one N=O double bond. The nitrite ion contains two N-O bonds that are equivalent to 1.5 bonds. The nitrite ion contains two N-O single bonds. D) The nitrite ion contains two N=O double bonds. E) None of the above are true. 50) 51) Determine the electron geometry, molecular geometry and polarity of HBrO2. 51) eg=trigonal bipyramidal, mg=trigonal planar, nonpolar eg=tetrahedral, mg=linear, nonpolar eg=linear, mg=linear, polar D) eg=tetrahedral, mg=trigonal pyramidal, polar E) eg=octahedral, mg=square planar, nonpolar 52) Determine the electron geometry (eg), molecular geometry (mg), and polarity of SO2. 52) eg=linear, mg=linear, nonpolar eg=tetrahedral, mg=bent, polar eg=tetrahedral, mg=tetrahedral, nonpolar D) eg=trigonal pyramidal, mg=trigonal pyramidal, polar E) eg=trigonal planar, mg=bent, polar 53) Choose the bond below that is most polar. 53) H-F C-H H-I D) H-Br E) H-Cl 54) Which of the following represent the Lewis structure for N? 54) D) E) 55) Give the name for NaNO3. 55) sodium nitrate sodium pernitrate

9 sodium nitrite D) sodium hyponitrate E) sodium hyponitrite 56) Choose the best Lewis structure for SeO ) D) E) 57) A molecule containing a central atom with sp3d2 hybridization has a(n) electron geometry. trigonal pyramidal trigonal planar octahedral D) tetrahedral E) trigonal bipyramidal 57) 58) Give the approximate bond angle for a molecule with a trigonal planar shape. 58) D) ) Determine the electron geometry (eg) and molecular geometry (mg) of BrF3. 59) eg=trigonal planar, mg=trigonal planar eg=trigonal bipyramidal, mg= T-shape eg=tetrahedral, mg=trigonal pyramidal D) eg=trigonal planar, mg=bent E) eg=trigonal bipyramidal, mg=see-saw

10 60) Use Lewis theory to determine the chemical formula for the compound formed between Rb and S. Rb3S2 Rb2S Rb2S3 D) RbS E) RbS2 60) 61) Choose the best Lewis structure for OCl2. 61) D) E) 62) Which of the following is an ionic compound? 62) PCl3 CF4 NO2 D) LiCl E) SeBr2 63) Give the formula for sulfurous acid. 63) H2SO3 HSO4 H2SO4 D) HSO3 64) Draw the Lewis structure for SF6. What is the hybridization on the S atom? 64) sp sp2 sp3 D) sp3d2 E) sp3d 65) How many of the following molecules are polar? 65) XeO2 SiCl2Br2 C2Br2 SeCl D) 4 E) 0 66) Which of the following elements can form compounds with an expanded octet? 66) Br Be N D) F E) None of the above can form compounds with an expanded octet. 67) Determine the electron geometry, molecular geometry and polarity of N2O (N central). 67) eg= linear, mg=linear, polar eg=tetrahedral, mg=linear, nonpolar eg=trigonal planar, mg=bent, polar D) eg=tetrahedral, mg=bent, polar E) eg=linear, mg=linear, nonpolar 68) Using Lewis structures and formal charge, which of the following ions is most stable? 68) OCN ONC NOC ONC OCN NOC D) None of these ions are stable according to Lewis theory. E) All of these compounds are equally stable according to Lewis theory.

11 69) Which of the following represent the Lewis structure for Cl? 69) D) E) 70) Determine the electron geometry (eg) and molecular geometry (mg) of CO ) eg=tetrahedral, mg=trigonal planar eg=trigonal planar, mg=bent eg=tetrahedral, mg=tetrahedral D) eg=tetrahedral, mg=trigonal pyramidal E) eg=trigonal planar, mg=trigonal planar 71) Which molecule or compound below contains a polar covalent bond? 71) NCl3 AgCl ZnS D) LiI E) C2H4 72) Which of the following elements can form compounds with an expanded octet? 72) Li F Se D) C E) All of the above elements can form compounds with an expanded octet. 73) Which of the following represent the Lewis structure for Mg? 73) D) E) 74) Identify the shape that goes with sp3d. 74) octahedral tetrahedral trigonal bipyramidal D) trigonal planar 75) Place the following elements in order of increasing electronegativity. 75) Sr N Na N < Sr < Na Sr < Na < N N < Na < Sr D) Sr < N < Na E) Na < N < Sr 76) How many of the following molecules have sp3d2 hybridization on the central atom? 76) SeCl6 XeF4 IF5 AsCl D) 1 E) 4 77) Which of the following is an ionic compound? 77) PF5 CH2O Cl2O D) SCl2 E) Mg3(PO4)2

12 78) A molecule containing a central atom with sp3 hybridization has a(n) electron geometry. trigonal bipyramidal tetrahedral linear D) bent E) octahedral 78) 79) Write the formula for strontium nitride. 79) Sr(NO2)2 Sr(NO3)2 SrN D) Sr2N3 E) Sr3N2 80) Determine the name for P4O10. 80) diphosphorus pentoxide phosphorus (II) oxide phosphorus oxide D) phosphorus (IV) oxide E) tetraphosphorus decoxide 81) Choose the best Lewis structure for XeI2. 81) D) E) 82) Draw the Lewis structure for BrO4. What is the hybridization on the Br atom? 82) sp sp3d sp3d2 D) sp3 E) sp2 83) Determine the electron geometry, molecular geometry and polarity around the O of CH3OH. 83) eg=linear, mg=linear, polar eg=tetrahedral, mg=linear, nonpolar eg=octahedral, mg=square planar, nonpolar D) eg=trigonal bipyramidal, mg=trigonal planar, nonpolar E) eg=tetrahedral, mg=bent, polar 84) Determine the electron geometry (eg) and molecular geometry (mg) of CH ) eg=tetrahedral, mg=trigonal planar eg=tetrahedral, mg=tetrahedral eg=trigonal planar, mg=bent D) eg=tetrahedral, mg=trigonal pyramidal E) eg=trigonal planar, mg=trigonal planar 85) Write the formula for copper (II) sulfate pentahydrate. 85) CuS 5H2O CuSO4 5H2O Cu2S H2O D) (CuSO4)5 E) Cu2SO3 H5

13 86) Draw the Lewis structure for SO3. What is the hybridization on the S atom? 86) sp3d2 sp3 sp2 D) sp3d E) sp 87) Choose the best Lewis structure for CH2Cl2. 87) D) E) 88) How many of the following molecules are polar? 88) XeCl2 COF2 PCl4F SF D) 3 E) 0 89) Write the formula for barium nitrite. 89) B(NO2)3 Ba3N2 Ba(NO2)2 D) BaNO3 E) BN 90) Choose the best Lewis structure for SF4. 90) D)

14 E) 91) Choose the best Lewis structure for SO ) D) E) 92) How many of the following molecules are polar? 92) PCl5 COS XeO3 SeBr D) 1 E) 4 93) Use Lewis theory to determine the chemical formula for the compound formed between Ca and N. Ca2N3 Ca3N2 CaN2 D) Ca2N E) CaN 93) 94) Choose the bond below that is least polar. 94)

15 P-F C-F C-I D) C-Br E) C-Cl 95) Determine the electron geometry (eg) and molecular geometry (mg) of ICl ) eg=tetrahedral, mg=bent eg=octahedral, mg=square planar eg=linear, eg=linear D) eg=trigonal bipyramidal, mg=tetrahedral E) eg=tetrahedral, mg=tetrahedral 96) Determine the electron geometry, molecular geometry and polarity of SF6. 96) eg=tetrahedral, mg=tetrahedral, polar eg=trigonal bipyramidal, mg=trigonal bipyramidal, nonpolar eg=octahedral, mg=trigonal bipyramidal, nonpolar D) eg=trigonal bipyramidal, mg=see-saw, polar E) eg=octahedral, mg=octahedral, nonpolar 97) Determine the name for Cl2O. 97) chlorate chlorine oxide dichlorine monoxide D) chlorine (I) oxide E) chlorine (II) oxide 98) How many of the following molecules have sp3d hybridization on the central atom? 98) SiCl4 BrF5 AsF5 BrF D) 4 E) 3 99) Choose the best Lewis structure for ICl5. 99) D) E)

16 100) Determine the name for H2CO3. 100) hydrocarbonic acid hydrocarbide acid dihydrogen carbonate D) carbonous acid E) carbonic acid 101) Identify the formula for nitric acid. 101) HNO4 HNO3 HNO2 D) HNO 102) Determine the name for HClO3. 102) hydrochlorus acid chloric acid hydrochloric acid D) perchloric acid E) chlorate acid 103) Write the formula for the compound formed between potassium and sulfur. 103) KS K2SO3 K3S2 D) K2S E) KS2 104) Determine the electron geometry, molecular geometry and polarity of TeCl6. 104) eg=trigonal bipyramidal, mg=trigonal bipyramidal, nonpolar eg=octahedral, mg=octahedral, nonpolar eg=trigonal bipyramidal, mg=see-saw, polar D) eg=octahedral, mg=square planar, polar E) eg=tetrahedral, mg=trigonal pyramidal, polar 105) Determine the name for N2O5. 105) nitrogen oxide dinitrogen pentoxide nitrogen (IV) oxide D) nitrogen tetroxide E) nitrogen (II) oxide 106) Draw the Lewis structure for CO3 2- including any valid resonance structures. Which of the following statements is TRUE? The CO3 2- ion contains one C-O single bond and two C=O double bonds. 106) The CO3 2- ion contains three double bonds. The CO3 2- ion contains two C-O single bonds and one C=O double bonds D) The CO3 2- ion contains two C-O single bonds and one C O triple bond. E) None of the above are true. 107) Determine the electron geometry (eg) and molecular geometry (mg) of XeF4. 107) eg=linear, eg=linear

17 eg=trigonal bipyramidal, mg=tetrahedral eg=tetrahedral, mg=bent D) eg=octahedral, mg=square planar E) eg=tetrahedral, mg=tetrahedral 108) Give the approximate bond angle for a molecule with a tetrahedral shape. 108) D) ) Which of the following statements is TRUE? 109) A pair of electrons involved in a covalent bond are sometimes referred to as "lone pairs." A covalent bond is formed through the transfer of electrons from one atom to another. A covalent bond has a lower potential energy than the two separate atoms. D) Single bonds are shorter than double bonds. E) It is not possible for two atoms to share more than two electrons. 110) Which of the following represent the Lewis structure for Br? 110) D) E)

18 1) C 2) C 3) C 4) D 5) C 6) E 7) A 8) C 9) B 10) E 11) C 12) B 13) B 14) B 15) B 16) A 17) B 18) A 19) B 20) D 21) A 22) C 23) E 24) B 25) C 26) B 27) A 28) C 29) B 30) A 31) B 32) C 33) D 34) A 35) C 36) D 37) D 38) A 39) B 40) A 41) B 42) C 43) E 44) B 45) A 46) A 47) D 48) B 49) D 50) B 51) D

19 52) E 53) A 54) B 55) A 56) E 57) C 58) D 59) B 60) B 61) C 62) D 63) A 64) D 65) C 66) A 67) A 68) B 69) D 70) E 71) A 72) C 73) D 74) C 75) B 76) C 77) E 78) B 79) E 80) E 81) A 82) D 83) E 84) E 85) B 86) C 87) E 88) D 89) C 90) E 91) D 92) C 93) B 94) C 95) B 96) E 97) C 98) A 99) A 100) E 101) B 102) B 103) D

20 104) B 105) B 106) C 107) D 108) B 109) C 110) D