If you are planning to take a course in general chemistry for science majors at Skidmore, please fill out the following information and take the exam below. We will use the information that you provide and the score from your exam solely to help us advise you whether to enroll in CH 105, Chemical Principles I or CH 107H, Intensive General Chemistry Honors. It's important for you to take this exam so that we can get you into the course that's taught at the right level for you. CH 107H is intended for students who have already attained a strong foundation in the fundamentals of chemistry. This course moves rapidly through the material that we teach in our standard, two-semester sequence of general chemistry (CH 105 and CH 106).

Exam Directions

In order for us to advise you properly, we need an accurate assessment of your chemical knowledge. Therefore, please do not use textbooks or consult anyone while taking the diagnostic exam. You may use a calculator and the periodic table provided. You will need to complete the exam in one sitting. It is not possible to take a portion of the exam and save it for completion and submission at another time. Hence, you should take it at a time when you can devote at least 45 minutes to it. If there are questions that you are unable to answer, please leave them blank. Be sure to press the “submit exam” button once you have completed the exam. We will grade your exam and reply to you with our recommendation by e-mail or phone. Registration in CH 107H is by permission of the instructor only. If we advise you to take this course and you choose to do so, we will make the necessary accommodations so that you can register for it. If we advise you to take CH 105 and/or you choose to do so, you can register for this course through the normal process.

Please contact Steven Frey (e-mail: sfrey@skidmore.edu, phone: 518-580-5124) if you have any questions or concerns about the exam.

1. The formula for aluminum chloride is AlCl₃. The formula for potassium sulfate is K₂SO₄. what is the formula for aluminium sulfate?

a) AlSO₄
b) Al(SO₄)₃
c) Al₂(SO₄)₃
d) Al₂SO₄

2. The correct name for Na₂CO₃ is

a) disodium monocarbon trioxide
b) sodium carbonate
c) disodium carbonate
d) sodium (I) carbonate

3. How many moles of oxygen atoms are represented in 1 mole of Ca₃(PO₄)₂?

a) 4
b) 6
c) 8
d) 12

4. How many moles of NaOH are in 10.0 grams?

a) 0.250
b) 4.00
c) 1.51 x 10²³
d) 1.66 x 10^-23

5. Which of these substances exists as a solid at room temperature and atmospheric pressure?

a) Xe
b) KCl
c) CO
d) Br₂

6. A gaseous mixture containing 1.3 moles of CO₂ and 5.2 moles of H₂ has a total pressure of 1.5 atm. What is the partial pressure of CO₂ in the mixture?

a) 0.38 atm
b) 1.2 atm
c) 0.30 atm
d) 7.8 atm

7. What would happen to a closed sample of gas whose temperature decreased while its volume increased?

a) Its pressure would decrease.
b) Its pressure would increase.
c) Its pressure would remain constant.
d) Moles of gas would increase.

8. Consider the following unbalanced equation.

Al (s) + Br₂ (l) AlBr₃ (s)

When the equation is balanced, the smallest whole number coefficient for Br₂ is

a) 2
b) 3
c) 4
d) 5

9. Consider the following balanced equation.

Fe₂O₃ (s) + 3 CO (g) 2 Fe (s) + 3 CO₂ (g)

How many moles of Fe (s) can possibly be produced if 6.3 moles of CO are reacted with an excess of Fe₂O₃?

a) 4.2
b) 9.5
c) 2.0
d) 0.66

10. What type of reaction is represented by the following equation?

2 K (s) + Cl₂ (g) 2 KCl (s)

a) Precipication reaction
b) Oxidation - reduction reaction
c) Acid - base reaction
d) None of these

11. What are the expected products of a reaction between Mg(OH)₂ (s) and excess HBr (aq)?

a) MgH₂ (s) and HBrO₂ (aq)
b) Mg (s), Br₂ (l), and H₂O (l)
c) MgBr₂ (aq) and H₂O (l)
d) There will be no reaction.

12. The combustion of a hydrocarbon compound involves

a) decomposition of the compound to produce H₂ and C.
b) reaction of the compound with CO₂ to produce H₂O and O₂.
c) reaction of the compound with O₂ to produce CO₂ and H₂O.
d) reaction of the compound with itself to produce larger hydrocarbons.

13. Consider the following reaction.

2 AgNO₃ (aq) + BaCl₂ (aq) 2 AgCl (s) + Ba(NO₃)₂ (aq)

How many moles of AgCl(s) can you expect to produce by combining 3.6 moles of BaCl₂ (aq) with 8.9 moles of AgNO₃ (aq)?

a) 7.2 moles
b) 18 moles
c) 13 moles
d) 1.8 moles

14. Which of the following statements about the structure of an atom is true?

a) The nucleus takes up approximately 2/3 of the volume of an atom.
b) The mass of a proton is nearly identical to the mass of an electron.
c) The number of protons and neutrons is always the same for a neutral atom.
d) The majority of the mass of an atom is concentrated in its nucleus.

15. The isotope ⁴⁰Ca²⁺ contains

a) 22 protons, 20 neutrons, and 20 electrons
b) 20 protons, 20 neutrons, and 18 electrons
c) 22 protons, 18 neutrons, and 18 electrons
d) 40 protons, 40 neutrons, and 38 electrons

16. Which of the following molecules contains a double bond?

a) N₂
b) H₂S
c) NH₃
d) CS₂

17. The geometry of PCl₅ is

a) trigonal bipyramidal.
b) square pyramidal.
c) pentagonal planar.
d) octahedral.

18. Which of the following elements is most electronegative?

a) Ca
b) O
c) S
d) As

19. Which element has properties most similar to bromine?

a) Se
b) Cl
c) Kr
d) Ca

20. What is the most likely formula for a compound that forms between Li and N?

a) LiN
b) Li₂N
c) Li₃N
d) LiN₂

21. Which element is considered a metalloid?

a) Be
b) Fe
c) Ge
d) Xe

22. Which of the following elements has the highest, first ionization energy?

a) Cl
b) Br
c) Mg
d) Cs

23. The electronic configuration for Si is?

a) 1s²1p⁶1d⁶
b) 1s²2s²2p⁶3s²3p²
c) 1s²2s²2p⁶3s²3p⁶3d¹⁰
d) 1s²2s²2p⁶2d⁴

24. Which of the following is the strongest acid in aqueous solution?

a) CH₃OH
b) NH₃
c) CH₃COOH
d) HNO₃

25. Which of the following equations represents the reaction of the base methylamine (CH₃NH₂) with water?

a) CH₃NH₂(aq) + H₂O(l) CH₃NH^-(aq) + H₃O⁺(aq)
b) CH₃NH₂(aq) + H₂O(l) CH₃NH₃⁺(aq) + OH^-(aq)
c) 2 CH₃NH₂(aq) + 2 H₂O(l) 2 CH₃OH(aq) + N₂(g) + 2 H₂(g)
d) CH₃NH₂(aq) + 2 H₂O(l) CO₂(g) + NH₃(aq) + 3 H₂(g)

26. Which of the following compounds would you expect to be most soluble in water?

a) KCl
b) Fe(OH)₃
c) CuS
d) CO₂

27. The addition of sodium hydroxide to pure water will

a) raise the hydronium ion concentration and raise the pH.
b) lower the hydronium ion concentration and raise the pH.
c) raise the hydronium ion concentration and lower the pH.
d) lower the hydronium ion concentration and lower the pH.

28. How many grams of NaCl are contained in 7.5 x 10² mL of a 0.20 M sodium chloride solution?

a) 20 g
b) 150 g
c) 12 g
d) 8.8 g

29. What volume of 12.0 M HCl must be used to prepare 25.5 L of 0.125 M HCl?

a) 266 mL
b) 58.8 mL
c) 17.0 mL
d) 376 mL

30. Copper makes up 1.6 x 10^-4 percent by mass of the elements found in a normal, healthy body. How many grams of copper would be found in the body of a person weighing 165 lb? (Note that 2.2 lb = 1.0 kg)

a) 1200 g
b) 0.12 g
c) 12 g
d) 0.58 g