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Chemistry Review & Bonding Concepts Explained

Dive into the world of chemical bonding with detailed explanations on various types of bonds and chemical equations. Understand concepts like covalent, ionic, and metallic bonding, and learn how to balance chemical equations. Discover the properties of compounds formed by different elements and explore the phases of matter.

hedwig-buckley
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Chemistry Review & Bonding Concepts Explained

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  1. Chapter 21, 22, & 23 Review Day!

  2. What kind of bond would you expect between 2 Oxygen atoms? • nonpolar covalent • ionic • metallic • polar covalent

  3. What kind of bond would you expect between 2 Oxygen atoms? • nonpolar covalent • ionic • metallic • polar covalent

  4. Which set of coeffients balance the following chemical equations? Na + Cl2 NaCl • 2,1,1 • 1,2,1 • 2,3,1 • 2,1,2

  5. Which set of coeffients balance the following chemical equations? Na + Cl2 NaCl • 2,1,1 • 1,2,1 • 2,3,1 • 2,1,2

  6. How many electrons are shared in a double covalent bond? • 2 • 6 • 1 • 4

  7. How many electrons are shared in a double covalent bond? • 2 • 6 • 1 • 4

  8. What type of chemical bond would you expect between a calcium and chlorine atom? • Metallic • Ionic • Polar covalent • Nonpolar covalent

  9. What type of chemical bond would you expect between a calcium and chlorine atom? • Metallic • Ionic • Polar covalent • Nonpolar covalent

  10. The alkali metals tend to form 1+ while the alkali-earth metals tend to form 2+ because • The charges of these ions corresponds to the number of valence electrons that may be lost • The ion an atom forms is always equal to the group number • This is a random occurrence • Alkali metals are less massive

  11. The alkali metals tend to from 1+ while the alkali-earth metals tend to from 2+ because • The charges of these ions corresponds to the number of valence electrons that may be lost • The ion an atom forms is always equal to the group number • This is a random occurrence • Alkali metals are less massive

  12. If Aluminum ions have a 3+ charge and oxygen ions have a 2- charge, the compound aluminum oxide is • Al6O6 • Al4O3 • Al3O2 • Al2O3

  13. If gallium ions have a 3+ charge and sulfur ions have a 2- charge, the compound Aluminum oxide is • Al6O6 • Al4O3 • Al3O2 • Al2O3

  14. If calcium has a 2+ charge and oxygen has a 2- charge, what is the formula for calcium oxide? • Ca4O2 • CaO • Ca2O2 • Ca2O4

  15. If magnesium has a 2+ charge and oxygen has a 2- charge, what is the formula for calcium oxide? • Ca4O2 • CaO • Ca2O2 • Ca2O4

  16. The greater the difference in electro negativity between two covalently bonded atoms, • The closer together the atoms are located on the periodic table • The greater the polarity • The smaller the polarity • Two of the above are correct

  17. The greater the difference in electro negativity between two covalently bonded atoms, • The closer together the atoms are located on the periodic table • The greater the polarity • The smaller the polarity • Two of the above are correct

  18. Which set of coeffients balance the following chemical equation? C3H8 + O2 CO2 + H2O • 1,3,3,1 • 3,5,3,4 • 1,5,3,4 • 1,5,3,1

  19. Which set of coeffients balance the following chemical equation? C3H8 + O2 CO2 + H2O • 1,3,3,1 • 3,5,3,4 • 1,5,3,4 • 1,5,3,1

  20. The images below show particles in three phases. What are they from left to right? • Gas, liquid, solid • Solid, liquid, gas • Solid, gas, liquid • Liquid, gas, solid

  21. The images below show particles in three phases. What are they from left to right? • Gas, liquid, solid • Solid, liquid, gas • Solid, gas, liquid • Liquid, gas, solid

  22. Gases are so much easier to squeeze into smaller volumes than liquids or solids because • They are always warmer than liquids or solids • There is so much space in between the submicroscopic particles • They are so much lighter • Their atoms or molecules are already moving at high speeds

  23. Gases are so much easier to squeeze into smaller volumes than liquids or solids because • They are always warmer than liquids or solids • There is so much space in between the submicroscopic particles • They are so much lighter • Their atoms or molecules are already moving at high speeds

  24. The phase in which atoms and molecules no longer move is • Gas • Liquid • Solid • none

  25. The phase in which atoms and molecules no longer move is • Gas • Liquid • Solid • none

  26. When two different elements combine to form a compound, the resulting properties of the compound are • Predictable based upon the nature of the combining elements • Not necessarily anything like those of the elements • Most like the element given in the greatest amount • About the average of the properties of the two elements

  27. When two different elements combine to form a compound, the resulting properties of the compound are • Predictable based upon the nature of the combining elements • Not necessarily anything like those of the elements • Most like the element given in the greatest amount • About the average of the properties of the two elements

  28. What type of chemical bond would you expect between 2 neon atoms? • Covalent • Ionic • Metallic • None of the above

  29. What type of chemical bond would you expect between 2 neon atoms? • Covalent • Ionic • Metallic • None of the above

  30. Which of the set of coefficients balance the following equation? BaCl2+ NaOH  NaCl + Ba(OH)2 • 1,2,1,1 • 1,2,2,2 • 1,2,2,1 • 2,1,2,1

  31. Which of the set of coefficients balance the following equation? BaCl2+ NaOH  NaCl + Ba(OH)2 • 1,2,1,1 • 1,2,2,2 • 1,2,2,1 • 2,1,2,1

  32. Which of the below shows a mixture? A B C D • A • B • C • D

  33. Which of the below shows a mixture? A B C D • A • B • C • D

  34. Which set of coefficients balance the following chemical equation? CaBr2 + Na3P Ca3P2 + NaBr • 3,2,1,6 • 3,2,2,6 • 3,1,2,6 • 3,3,1,6

  35. Which set of coefficients balance the following chemical equation? CaBr2 + Na3P Ca3P2 + NaBr • 3,2,1,6 • 3,2,2,6 • 3,1,2,6 • 3,3,1,6

  36. Which set of coefficients balance the following chemical equation? NaF  Na + F2 • 2,1,2 • 2,2,1 • 1,2,2 • 1,2,1

  37. Which set of coefficients balance the following chemical equation? NaF  Na + F2 • 2,1,2 • 2,2,1 • 1,2,2 • 1,2,1

  38. If Na is +1 and CrO4 is -2, the compound’s formula is • NaCrO4 • Na2CrO4 • Na(CrO4)2 • Na2(CrO4)2

  39. If Na is +1 and CrO4 is -2, the compound’s formula is • NaCrO4 • Na2CrO4 • Na(CrO4)2 • Na2(CrO4)2

  40. How does a solid phase differ from a liquid phase on the molecular level? • The molecules of a solid are always more compact • The molecules of a solid are fixed, while the molecules of a liquid are mobile • There are molecular attractions in the solid phase but not to the liquid phase • Solids have crystalline structure while liquids are amorphous

  41. How does a solid phase differ from a liquid phase on the molecular level? • The molecules of a solid are always more compact • The molecules of a solid are fixed, while the molecules of a liquid are mobile • The are molecular attractions in the solid phase but not to the liquid phase • Solids have crystalline structure while liquids are amorphous

  42. What elements tend to form ionic bonds? • Those found in the upper right hand side of the periodic table • Metallic elements • Elements found on opposite sides of the periodic table • Any two elements of the same phase can form an ionic compound

  43. What elements tend to form ionic bonds? • Those found in the upper right hand side of the periodic table • Metallic elements • Elements found on opposite sides of the periodic table • Any two elements of the same phase can form an ionic compound

  44. Which set of coefficients balance the following chemical equation? Li3PO4 Li + P + O2 • 1,3,2,1 • 1,3,2,2 • 1,2,4,4 • 1,3,1,2

  45. Which set of coefficients balance the following chemical equation? Li3PO4 Li + P + O2 • 1,3,2,1 • 1,3,2,2 • 1,2,4,4 • 1,3,1,2

  46. During a chemical reaction • Old atoms disappear to be replaced by new ones • Old atoms transform into new ones • Old atoms stick around merely switching partners • None of the above

  47. During a chemical reaction • Old atoms disappear to be replaced by new ones • Old atoms transform into new ones • Old atoms stick around merely switching partners • None of the above

  48. What type of chemical bond would you expect between a Carbon and an Oxygen? • Polar covalent • Nonpolar covalent • Metallic • Ionic

  49. What type of chemical bond would you expect between a Carbon and an Oxygen? • Polar covalent • Nonpolar covalent • Metallic • Ionic

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