NAME 1. When compared to H 2 S, H 2 O has a higher 8. Given the Lewis electron-dot diagram: boiling point because H 2 O contains stronger metallic bonds covalent bonds ionic bonds hydrogen bonds 2. Which kinds of bonds are found in a sample of liquid H 2 O? covalent bonds, only hydrogen bonds, only both covalent and hydrogen bonds both ionic and hydrogen bonds 3. Hydrogen bonds are formed between molecules in which hydrogen is covalently bonded to an element having low high low ionization energy high atomic mass 4. Which compound is the most polar? H 2 S H 2 Te H 2 Se 5. Argon has a higher boiling point than neon because argon has fewer electrons in its 2nd principal energy level more electrons in its outermost principal energy level weaker intermolecular forces of attraction stronger intermolecular forces of attraction 6. At 25ºC, F 2 is a gas but I 2 is a solid. This is most likely due to the fact that F 2 is a dipole but I 2 is not I 2 is a dipole but F 2 is not F 2 molecules have stronger intermolecular attractions I 2 molecules have stronger intermolecular attractions 7. Which bond is least polar? As Cl Bi Cl P Cl N Cl Which electrons are represented by all of the dots? the carbon, only the hydrogen, only the carbon and hydrogen all of the carbon and hydrogen electrons 9. When a sodium atom reacts with a chlorine atom to form a compound, the electron configurations of the ions forming the compound are the same as those in which noble gas atoms? krypton and neon krypton and argon neon and helium neon and argon 10. Which is the correct electron-dot formula for a molecule of chlorine, Cl 2? 11. Which electron-dot diagram represents H 2? 12. Which bond has the least ionic character? KBr HF MgO BrCl
13. Based on values, which type of elements tends to have the greatest attraction for electrons in a metals metalloids nonmetals noble gases 14. Based on the values in your table of electronegativities, the atoms of which of these elements have the strongest attraction for electrons in a chemical N Na P Pt 15. Given the electron dot diagram: 18. Electronegativity is a measure of an atom's ability to attract the electrons in the bond between the atom and another atom repel the electrons in the bond between the atom and another atom attract the protons of another atom repel the protons of another atom 19. Which type of bonding is usually exhibited when the difference between two atoms is 1.1? ionic covalent metallic network The electrons in the bond between hydrogen and fluorine are more strongly attracted to the atom of hydrogen, which has the higher fluorine, which has the higher hydrogen, which has the lower fluorine, which has the lower 16. Which of the following elements has the greatest ability to attract electrons? Li Be Na Mg 17. An element with an of 0.9 bonds with an element with an of 3.1. Which phrase best describes the bond between these elements? mostly ionic in character and formed between two nonmetals mostly ionic in character and formed between a metal and a nonmetal mostly covalent in character and formed between two nonmetal mostly covalent in character and formed between a metal and a nonmetal 20. Which compound has the least ionic character (Cl = chlorine)? KCl CaCl 2 AlCl 3 CCl 4 21. Which pair of elements below will form a compound with the greatest ionic character? Pb and F Ca and O Na and Cl Cs and N 22. Given the electron dot formula: Which atom represented as X would have the least attraction for the electrons that form the F Cl I Br 23. In which compound do the atoms have the greatest difference in? NaBr AlCl 3 KF LiI 24. Which substance contains metallic bonds? Hg( ) H 2 O( ) NaCl(s) C 6 H 12 O 6 (s)
25. Which substance contains bonds that involved the transfer of electrons from one atom to another? CO 2 NH 3 KBr Cl 2 26. Which type of bond is found in sodium bromide? covalent hydrogen ionic metallic 32. What is the total number of pairs of electrons shared in a molecule of N 2? one pair two pairs three pairs four pairs 33. What is the total number of electrons shared in the bonds between the two carbon atoms in a the molecule shown below? 6 2 3 8 27. Compared to a calcium atom, the calcium ion Ca 2+ has more protons fewer protons more electrons fewer electrons 28. Which elements combine by forming an ionic sodium and potassium sodium and oxygen carbon and oxygen carbon and sulfur 29. An ionic compound consists of positive and negative ions each with 10 electrons. Half of these ions have a charge of 1 + and the other half have a charge of 1. What is the formula of this compound? KF KCl NaF NaCl 30. Element X is in Group 2 and element Y is in Group 17. What happens when a compound is formed between these two atoms? X loses electrons to Y to form an ionic bond. X loses electrons to Y to form a covalent bond. X gains electrons from Y to form an ionic bond. X gains electrons from Y to form a covalent bond. 31. When a potassium atom reacts with bromine, the potassium atom will lose only 1 electron lose 2 electrons gain only 1 electron gain 2 electrons 34. Which compound contains only covalent bonds? NaOH Ba(OH) 2 Ca(OH) 2 CH 3 OH 35. The bond between Br atoms in a Br 2 molecule is ionic and is formed by the sharing of two ionic and is formed by the transfer of two covalent and is formed by the sharing of two covalent and is formed by the transfer of two 36. Which element has atoms that can form single, double, and triple covalent bonds with other atoms of the same element? hydrogen oxygen fluorine carbon 37. Which molecule contains a triple covalent H 2 N 2 O 2 Cl 2 38. Which pair of atoms is held together by a covalent HCl LiCl NaCl KCl
39. In which compound do atoms form bonds by sharing electrons? Na 2 O CaO MgO 40. Which molecule will have a double covalent F 2 O 2 Cl 2 N 2 46. Which type of bonding involves positive ions immersed in a sea of mobile electrons? ionic nonpolar covalent polar covalent metallic 47. Which type of bond is present in copper wire? covalent ionic electrovalent metallic 48. A diamond is an example of a supercooled liquid an ionic compound a metallic substance a network solid 41. Which type of bond is found in one molecule of methane, CH 4? a covalent bond a hydrogen bond an ionic bond a metallic bond 42. Conductivity in a metal results from the metal atoms having high high ionization energy highly mobile protons in the nucleus highly mobile electrons in the valence shell 43. The high electrical conductivity of metals is primarily due to high ionization energies filled energy levels mobile electrons high electronegativities 44. Which element consists of positive ions immersed in a "sea" of mobile electrons? sulfur nitrogen calcium chlorine 45. Which factor distinguishes a metallic bond from an ionic bond or a covalent the mobility of electrons the mobility of protons the equal sharing of electrons the unequal sharing of electrons 49. Which formula represents a nonpolar molecule containing polar covalent bonds? CCl 4 NH 3 H 2 50. Which type of bond is formed between the carbon atom and the oxygen atom in CH 3 OH? ionic electrovalent polar covalent nonpolar covalent 51. Which electron-dot formula represents a substance that contains a nonpolar covalent
52. Which molecule is nonpolar? NH 3 CO CO 2 54. The diagram below represents a water molecule. 53. Which structural formula represents a nonpolar molecule? This molecule is best described as polar with polar covalent bonds polar with nonpolar covalent bonds nonpolar with polar covalent bonds nonpolar with nonpolar covalent bonds 55. Which sequence of Group 18 elements demonstrates a gradual decrease in the strength of the London dispersion forces? Ar( ), Kr( ), Ne( ), Xe( ) Kr( ), Xe( ), Ar( ), Ne( ) Ne( ), Ar( ), Kr( ), Xe( ) Xe( ), Kr( ), Ar( ), Ne( ) 56. Nitrogen gas, N 2, will become a liquid at low temperatures primarily because of London dispersion forces hydrogen bonding covalent bonding dipole-dipole interactions
Answer Key 1. D 2. C 3. B 4. A 5. D 6. D 7. D 8. C 9. D 10. D 11. B 12. D 13. C 14. A 15. B 16. B 17. B 18. A 19. B 20. D 21. B 22. C 23. C 24. A 25. C 26. C 27. D 28. B 29. C 30. A 31. A 32. C 33. A 34. D 35. C 36. D 37. B 38. A 39. A 40. B 41. A 42. D 43. C 44. C 45. A 46. D 47. D 48. D 49. B 50. C 51. B 52. D 53. C 54. A 55. D 56. A
Name Class Date 1. 2. 3. 4. 5. 6. 7. 8. 9. 10. 11. 12. 13. 14. 15. 16. 17. 18. 19. 20. 21. 22. 23. 24. 25. 26. 27. 28. 29. 30. 31. 32. 33. 34. 35. 36. 37. 38. 39. 40. 41. 42. 43. 44. 45. 46. 47. 48. 49. 50. 51. 52. 53. 54. 55. 56.