Chemistry Final Exam 2013 Review

1. Why do atoms bond?

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Type of Bond / What happens with the electrons? / What type of elements
are involved in this bond? / Compounds / Examples

3. What are some properties of ionic compounds?

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4. What are some properties of covalent compounds?

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5. What is electronegativity?

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6. How do you use the periodic table of electronegativities to determine if a bond is nonpolar covalent, polar covalent, or ionic?

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7. What is atomic radius?

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8. What is the periodic trend for atomic radius as you go to the right on the PT and down the PT?

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9. How do you draw Lewis dot structures for atoms?

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10. How do you draw Lewis dot structures for ions?

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11. What is the VSEPR theory?

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12. What are the 5 shapes that we have discussed in class and provide one example of a compound for each shape. **Make sure that you properly draw each shape/compound.**

VSEPR Shape / Drawing of Example Compound

13. How do you write chemical formulas for monatomic ions? Provide some examples.

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14. How do you write chemical formulas for IONIC binary compounds?

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15. Write the formulas for the following ionic compounds:

A) copper (II) iodide ______

B) beryllium chloride ______

C) silver (I) oxide ______

D) potassium sulfide ______

16. How do you write chemical formulas for COVALENT binary compounds?

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17. Write the formulas for the following covalent compounds:

A)antimony tribromide ______

B)hexaboron silicide ______

C)chlorine dioxide ______

D)hydrogen iodide ______

E)iodine pentafluoride ______

18. How do you write chemical formulas for compounds with polyatomic ions?

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19. Write the formulas for the following compounds with polyatomic ions:

A) ammonium sulfate ______

B) calcium phosphate ______

C) hydrogen hydroxide ______

20. How do you name monatomic ions?

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21. Name these examples:

A) Be +2 ______B) F -1 ______

22. How do you name ionic compounds (transition metals vs. regular metals)?

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23. Name the following examples:

A) copper (II) iodide ______

B) beryllium chloride ______

C) ammonium sulfate ______

D) silver (I) oxide ______

E) potassium sulfide ______

24. How do you name covalent compounds?

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25. Name the following covalent compounds:

A)SeF6 ______

B)Si2Br6 ______

C)SCl4 ______

D)CH4 ______

26. How do you calculate molar mass (g/mol) of a compound?

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27. Calculate the molar mass for the following examples and show your work:

A)NaBrB) PbSO4C)Ca(OH)2

28. What are 5 signs of a chemical reaction?

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29. What are word equations?

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30. How are word equations different from equations with chemical formula?

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31. Change the following word equations to formula equations:

A) When fluorine gas is put into contact with calcium metal at high temperatures, calcium fluoride is created.

B) When sodium metal reacts with iron (II) chloride, iron metal and sodium chloride are formed.

32. What is the purpose of balancing equations?

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33. Balance the following example equations:

A)____ GaF3 + ____ Cs  ____ CsF + ____ Ga

B)____ BaS + ____ PtF2 ____ BaF2 + ____ PtS

C)____ N2 + ____ H2 ____ NH3

D)____ NaF + ____ Br2 ____ NaBr + ____ F2

34. How do you convert from grams to moles?

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35. How do you convert from moles to grams?

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36. What are the 5 types of reactions and their general formats?

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37. Classify the following examples of reactions as synthesis, decomposition, single replacement, double replacement or combustion:

______CO2  C + O2

______CH4 + O2  CO2 + 2H2O

______NaCl + AgNO3  AgCl + NaNO3

______S + Cl2  SCl2

______BaCl2 + 2NaOH  Ba(OH)2 + 2NaCl

38. What are 5 properties of gases?

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39. How do you convert a temperature given in Kelvins to degrees Celsius?

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40. How do you convert a temperature given in degrees Celsius to Kelvins?

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41. What is the equation for Boyle’s law?

42. What is the equation for Charles Law?

43. What scale must the temperature always be in before you can use Charles’s law?

44. What is the equation for the Ideal gas law?

45. What is the value with units of R, the universal gas constant?

46. What is the equation for calculating molarity?