Unit 5 Test Review Nomenclature Practice PDF

Unit 5 Test Review (Optional) I. Nomenclature Practice 1. AgNO3 ________________________________ 29. tetraphosphorus decoxide ___________________ 2. Na2Cr2O7 ________________________________ 30. potassium peroxide ___________________ 3. Sr2Fe(CN)6 ___________________________...

Unit 5 Test Review (Optional) I. Nomenclature Practice 1. AgNO3 ________________________________ 29. tetraphosphorus decoxide ___________________ 2. Na2Cr2O7 ________________________________ 30. potassium peroxide ___________________ 3. Sr2Fe(CN)6 ________________________________ 31. ammonium silicate ___________________ 4. N2O5 ________________________________ 32. lithium phosphide ___________________ 5. Ca(MnO4)2 ________________________________ 33. mercury (I) nitrate ___________________ 6. Al(OH)3 ________________________________ 34. nitrogen dioxide ___________________ 7. Cs3N ________________________________ 35. copper (II) chloride ___________________ 8. Fe2(SO4)3 ________________________________ 36. potassium perchlorate ___________________ 9. MgSiO4 ________________________________ 37. aluminum acetate ___________________ 10. Zn3(PO3)2 ________________________________ 38. magnesium hydroxide ___________________ 11. MnSe2 ________________________________ 39. silver chloride ___________________ 12. SnCl2 ________________________________ 40. tin (IV) sulfide ___________________ 13. Ca(ClO)2 ________________________________ 41. magnesium nitride ___________________ 14. N2O3 ________________________________ 42. aluminum selenite ___________________ 15. K2S ________________________________ 43. sulfurous acid ___________________ 16. ZnSO4 ________________________________ 44. hydrobromic acid ___________________ 17. Al(NO3)3 ________________________________ 45. barium chlorite ___________________ 18. (NH4)2C2O4________________________________ 46. iodic acid ___________________ 19. HgO ________________________________ 47. ammonium carbonate ___________________ 20. Cu(NO3)2 ________________________________ 48. cobalt (II) tartrate ___________________ 21. Cr2Fe(CN)6 ________________________________ 49. sodium nitrite ___________________ 22. CaCO3 ________________________________ 50. chloric acid ___________________ 23. PbCl2 ________________________________ 51. dihydrogen monoxide ___________________ 24. Na2SnO2 ________________________________ 52. iron (II) oxalate ___________________ 25. Sb(NO2)3 ________________________________ 53. manganese (III) bromide ___________________ 26. H3PO4 ________________________________ 54. mercury (I) sulfide ___________________ 27. P4O9 ________________________________ 55. mercury (II) sulfide ___________________ 28. CH4 ________________________________ 56. octane ___________________ 1. Fe(NO2)2 ________________________________ 30. aluminum carbonate ___________________ 2. SnO ________________________________ 31. dinitrogen pentoxide ___________________ 3. Cs4Fe(CN)6 ________________________________ 32. iron (III) hydroxide ___________________ 4. MgH2 ________________________________ 33. scandium (II) nitride ___________________ 5. Ni(ClO4)2 ________________________________ 34. tungsten (II) ferrocyanide __________________ 6. CaCO3 ________________________________ 35. silver perchlorate ___________________ 7. PbO ________________________________ 36. manganese (III) sulfide ___________________ 8. SO3 ________________________________ 37. barium nitrite ___________________ 9. CuBr2 ________________________________ 38. calcium phosphite ___________________ 10. Zn(ClO)2 ________________________________ 39. dinitrogen monoxide ___________________ 11. AlN ________________________________ 40. sodium hypobromite ___________________ 12. Ag2SO4 ________________________________ 41. iron (III) oxide ___________________ 13. FeP ________________________________ 42. magnesium acetate ___________________ 14. Sb2S3 ________________________________ 43. mercury (I) oxalate ___________________ 15. NaCH3COO________________________________ 44. lead (IV) acetate ___________________ 16. B2Cl6 ________________________________ 45. nitrous acid ___________________ 17. HgC2O4 ________________________________ 46. potassium bromate ___________________ 18. Ba(OH)2 ________________________________ 47. chlorous acid ___________________ 19. Sn(NO3)3 ________________________________ 48. hydroiodic acid ___________________ 20. CuI2 ________________________________ 49. copper (II) iodide ___________________ 21. CoAsO4 ________________________________ 50. diphosphorus trisulfide ___________________ 22. MgF2 ________________________________ 51. sodium phosphide ___________________ 23. SCl2 ________________________________ 52. potassium chromate ___________________ 24. MnFe(CN)6 ________________________________ 53. sodium chlorite ___________________ 25. H2SO3 ________________________________ 54. hypochlorous acid ___________________ 26. HgI2 ________________________________ 55. mercury (I) fluoride ___________________ 27. Hg2I2 ________________________________ 56. mercury (II) fluoride ___________________ 28. P4O10 ________________________________ 57. nitrogen trioxide ___________________ 29. C6H14 ________________________________ 58. decane ___________________ II. Draw the skeletal formulas for the following molecules. 1. 3-octyne 4. 3-decene 2. butane 5. hexane 3. 1-propyne 6. 1-heptyne III. Name the following organic structures 1. _______________________ 4. _______________________ 2. _______________________ 5. _______________________ 3. _______________________ 6. _______________________ IV. Give the chemical formulas for the following molecules and draw their Lewis structures. 1. butane 2. 1-butene 3. 2-butyne V. Isomers 1. What is an isomer? 2. Draw all the possible isomers of propene. 3. What is the formula of these two structures? Are they isomers? ______________ ______________________________ ____________________________ VI. Review the Properties of Ionic vs. Covalent Compounds A. Properties of Ionic Compounds 1) Electrons are transferred, creating ions 2) Ions bound together by ionic bonding (columbic attraction between oppositely charged ions) 3) Ions form a crystal lattice with alternating ions (cation/anion/cation/anion) 4) The smallest part of the crystal lattice that has the correct ratio of ions is called a formula unit. (a) Examples: NaCl, MgCl2, Al2O3, (NH4)2S, AlPO4 5) Strong attraction between POSITIVE and NEGATIVE ions is the force that holds ionic compounds together 6) Ionic compounds generally have higher melting and boiling points since bonds (intramolecular forces) must be broken to melt or boil; more likely to be a solid at room temperature 7) Ionic compounds are hard and brittle (shifting one row causes repulsive forces to build forcing the layers to part) B. Properties of Molecular (Covalent) compounds 1) Electrons are shared 2) Molecules (atoms) held together by covalent bonds 3) Most covalent compounds melt at relatively low temperatures Bonds inside the molecule are not broken, but IMFs (intermolecular forces/attractions) are broken. a. Therefore, more likely to be a gas or liquid at room temperature 4) Generally have lower melting and boiling points 5) Not brittle; may be soft 6) in most cases, does not form a crystal lattice List as many ways you can think of to compare and contrast ionic and covalent bonding and the properties of ionic and covalent compounds below. Ionic Covalent