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Exam 2 Review

by: Becca LeBoeuf

Exam 2 Review Chemistry 101

Becca LeBoeuf

GPA 3.0

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About this Document

This is the exam 2 review. This covers the material we learned in class on electronic configurations, naming of compounds, making formulas, Lewis structure, etc.
General, Organic, Biological Chemistry
George Vater Olsen
Study Guide
#Chemistry #Chem101 #Exam2 #LewisStructure #ElectronicConfigurations #NamingCompounds #MakingFormulas
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This 5 page Study Guide was uploaded by Becca LeBoeuf on Wednesday March 2, 2016. The Study Guide belongs to Chemistry 101 at University of Wisconsin - Oshkosh taught by George Vater Olsen in Spring 2016. Since its upload, it has received 42 views. For similar materials see General, Organic, Biological Chemistry in Chemistry at University of Wisconsin - Oshkosh.


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Date Created: 03/02/16
Exam 2 Review:    1. A formula unit of ammonium phosphate ​​3PO​ contains the following number of  atoms of each element:  a. 1 Phosphorus, 12 Hydrogen, 4 Oxygen, 3 Nitrogen.  b. 1 Phosphorus, 4 Hydrogen, 4 Oxygen, 1 Nitrogen.  c. 1 Phosphorus, 12 Hydrogen, 4 Oxygen, 1 Nitrogen.  d. 1 Phosphorus, 4 Hydrogen, 4 Oxygen, 3 Nitrogen.  e. None of the above.    2. The total number of electrons in a Se^2­ ion would be:  a. 6  b. 16  c. 34  d. 36  e. None of the above.    3. The total number of valence electrons you have to use in a Lewis structure of the  phosphate ion is:  a. 26  b. 32  c. 24  d. 30  e. None of the above.    4. The most polar bond of the following is:  a. H­H  b. H­O  c. H­N  d. H­Cl  e. H­Fr    5. The electrons in a carbon oxygen bond:  a. are more likely found by the oxygen atom, making it partially positive.  b. are more likely found by the oxygen atom, making it partially negative.  c. are more likely found by the carbon atom, making it partially positive.  d. are more likely found by the carbon atom, making it partially negative.    6. Which of the following is most likely to be soluble in water:  a. C ​H7OH  b. C​6H​3OH  c. C​6H​3NH  d. C​8H​7NH  e. None of the above.    7. Which of the following is most likely to be soluble in water:  a. C​H​1OH  b. C​H​3OH  c. C​H​3NH  d. C H​1​^1+C​1­  e. None of the above.    8. The number of electrons an orbital can hold is:  a. Dependent on the type of orbital.  b. Independent on the type of orbital.  c. Always one electron.  d. Able to vary.  e. None of the above.    9. What is the shape of nitrate ion according to VESPER theory?  a. Linear.  b. Trigonal Planar.  c. Pyramidal.  d. Tetrahedral.  e. None of the above.    10. There are how many sites of electron density around phosphorus in the phosphite ion:  a. 2  b. 3  c. 4  d. 5  e. None of the above.    11. Metals prefer to form:  a. Cations.  b. Anions.  c. Covalent bonds.  d. Coordinate covalent bonds.  e. None of the above.    12. Each of the following compounds is a salt with the exception of:  a. K​​O​4  b. H ​ O4  c. KNO​3  d. NH ​I  e. None of the above.  13. Nitric acid has the formula of:  a. HNO​ 2  b. HNO​ 3  c. HNO​ 4  d. H ​​O​3  e. None of the above.    14. The formula H3PO​4would be named:  a. Trihydrogen phosphate.  b. Phosphorus acid.  c. Phosphoric acid.  d. Trihydrogen phosphite.  e. None of the above.    15. The name for NH​​ r is:  a. Nitrogen tetrahydride monobromide.  b. Ammonium bromide.  c. Ammonia bromide.  d. Nitrogen hydrobromic acid.  e. None of the above.    16. The name for L2​ is:  a. Dilithium monosulfide.  b. Lithium monosulfide.  c. Lithium sulfide.  d. Lithium (I) sulfide.  e. None of the above.    17. The name for Fe​(SO )​ is:  a. Iron sulfate.  b. Iron(III) sulfate.  c. Iron(II) sulfate.  d. Diiron trisulfate.  e. None of the above.    18. The name for Sn3N4 is:  a. Tin Nitride.  b. Tritin Tetranitride.  c. Tin(IV) nitride.  d. Tin(VI) nitride.  e. Tin(III) nitride.      19. The name for 4N​4 is:  a. Sulfur nitride.  b. Tetrasulfur tetranitride.  c. Pentasulfur pentanitride.  d. Hexasulfide hexanitride.  e. None of the above.    20. The formula for Lead (IV) sulfate is:  a. Pb​​ O4  b. Pb​​ O3  c. Pb(SO ​)​  d. Pb(SO ​)​  e. None of the above.    21. The formula Cu(NO​​​would be named:  a. Copper (I) nitrite.  b. Copper (II) nitrite.  c. Copper (II) nitrate.  d. Copper (I) nitrate.  e. None of the above.    22. The subatomic particle with a negative charge is:  a. The nucleus.  b. The proton.  c. The neutron.  d. The electron.  e. None of the above.    23. The charge on gold in 2​3 is:  a. 2+  b. 3+  c. 4+  d. 6+  e. None of the above.    24. The trend in the electronegativity of the elements in the periodic table is:  a. That it increases from left to right across the table, and decreases down the  table.  b. That it decreases from left to right across the table, and decreases down the  table.  c. That it increases from left to right across the table, and increases down the table.  d. Thar it decreases from left to right across the table, and increases down the  table.  e. None of the above.  25. Which of the following would have a coordinate covalent bond:  a. NH​ 3  b. NH​ 4​^1+  c. NO​ 2  d. SO​ 3​^2­  e. None of the above.    26. If the dosage of a medication is 11.00 mg/5.00 kg; how much do you need to give to a  180.0 lb patient?  a. 180 mg.  b. 396 mg.  c. 871 mg.  d. 37 mg.  e. None of the above.    27. The electronic configuration of a copper atom is:  a. [Ar]4S^2 3D^9  b. [Ar]4S^1 3D^9  c. [Ar]4S^2 3D^10  d. [Ar]4S^1 3D^10  e. None of the above.    28. The electronic configuration of 1S^2 2S^2 2P^6 3S^2 3P^6 could be that of:  a. Ar, Cl ^1­, or K ^1+.  b. S ^2­, Ca ^1+, or Cl ^1­.  c. Ar, Ca ^2+, or N ^3­.  d. All of the above.  e. None of the above.    29. The difference between electronic configuration of a calcium atom and a calcium ion is:  a. There is no difference.  b. The ion has two fewer electrons than the atom.  c. The ion has two more electrons than the atom.  d. None of the above. 


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