HONORS CHEMISTRY

FALL EXAM REVIEW

 

 

TEST ELEMENTS

 

Below is a listing of the types of questions to be expected on the fall semester examination.  Also listed is the value given to each question.

 

                       

QUESTION CATEGORY	POINT VALUE
60 multiple choice	1/2 point each
40 matching	1/2 point each
5 essay questions / problems	10 points each

 

 

 

EXAM CONDITIONS

 

1.   Exam content shall include a comprehensive evaluation of the student.

2.   The exam shall take the full 1 hour and 10 minutes.

3.   Students will not be allowed to bring into the exam any study material for any exam, other than the exam they are currently taking. This means there will be no backpacks allowed in the classroom.

4.   The student will need a pencil, eraser, and calculator to complete the exam. No other materials are necessary, nor allowed.

5.   Any student completing the exam before the end of the exam period shall review their exam answers for correctness and accuracy. No exam may be turned in before the end of the exam period.

 

 

TESTED MATERIAL

 

The problems listed below may be used to guide your review of the material covered on the semester examination. The number in parenthesis at the end of each question is the chapter from which the question was taken.

 

1. What are the differences between a mixture and a compound?  (2)

2. What must occur for a process to be a chemical reaction?  (2)

3. Which group of measurements is the most precise?  (Each group of measurements is for a different object.)  (3)

(A) 2 g, 3 g, 4 g              (B) 2 g, 2.5 g, 3 g                        (C) 2.0 g, 3.0 g, 4.0 g

(D) 1 g, 3 g, 5 g              (E) 2.0 g, 3.0 g, 4.0 g, 5.0 g

4.  When multiplying and dividing measured quantities, the number of significant figures in the result should be equal to the number of significant figures in _____. (3)

5. What a correct conversion factor for changing kilometers to meters? grams to micrograms? liters to centiliters?  (3)

6 . The density of osmium, which is the densest metal, is 22.57 g/cm³.  What is the mass of a block of

    osmium that measures  1.00 cm x 4.00 cm x 2.50 cm? (3)

7.  What are the components of Dalton's atomic theory? (5)

8.  How do the isotopes hydrogen-1 and hydrogen-2 differ? (5)

9.  Why do chemists use relative comparisons of masses of atoms? (5)

10.  Isotopes of the same element have different _____. (5)

11. If E is the symbol for an element, which two of the following symbols represent isotopes of the same element? (5)

12.  Consider an element Z that has two naturally occurring isotopes with the following percent abundances: the isotope with a mass number of 20 is 25% abundant; the isotope with a mass number of 22 is 75% abundant. What is the average atomic mass for element Z? (5)

13.  Which subatomic particle plays the greatest part in determining the physical and chemical properties of an element? (5)

14.  The modern periodic table is arranged in order of increasing atomic _____.  (5)

15.  In any chemical compound, the elements are always combined in the same proportion by _____.  (6)

16. Which of the following formulas represents: (6)

(a)    an ionic compound? (A) BaI₂     (B) N₂O₄     (C) Kr (D) CS₂     (E) PCl₃

(b)    a molecular compound? (A) Xe    (B) SO₂     (C) BeF₂ (D) ZnO     (E) Mg₃N₂

(c)    binary molecular compound? (A) BeHCO₃   (B) PCl₅    (C) AgI  (D) MgS    (E) Cr₂O₃

(d)    When naming acids, the prefix hydro- is used when the name of the acid anion ends in _____.

17. (a) When Group 2 elements form ions, they gain / lose two electrons.  (6)

      (b) The nonmetals in Group 17 gain / lose one electron, when they form ions.

18. (a) An -ite or -ate ending on the name of a compound indicates that the compound _____.  (6)

      (b) Ternary ionic compounds contain three different _____.

19. Which of the following compounds contains the lead(IV) ion? (6)

 (A) PbO₂   (B) PbCl₂   (C) Pb₄O₃ (D) PbO   (E) Pb₂O

20. Consider a mystery compound having the formula M_xT_y.  If the compound is not an acid, if it contains only two

       elements and if M is not a metal; which of the following is true about the compound? (6)

(A) It contains a polyatomic ion.   (B) It is a binary molecular compound.

(C) Its name ends in -ic.     (D) Its name ends in -ite or -ate.

(E) It is a binary ionic compound.

21.  The lowest whole-number ratio of the elements in a compound is called the _____.  (6)

22. (a) The molar volume of a gas at STP occupies _____.  (7)

      (b) What combination of temperature and pressure correctly describes standard temperature and pressure, STP?

23. Which of the following compounds has the lowest percent gold content by weight? (7)

(A) AuCl₃ (B)  AuBr₃ (C)  AuI₃ (D)  Au(OH)₃ (E)  AuOH

24. Which of the following compounds have the same empirical formula? (7)

(A) CO₂ and SO₂                       (B) NO and NO₂                     (C) C₇H₁₄ and C₁₀H₂₀

(D) C₄H₁₀ and C₁₀H₄              (E) C₆H₁₂ and C₆H₁₄

25. What is the percent composition of NiO, if a sample of NiO with a mass of 10.3 g contains 8.1 g Ni and 2.2 g O? (7)

26.  The percentage composition of a polymer used for the non- stick surfaces of cooking utensils, is 24.0% C and 76.0%

       F by mass. What is the empirical formula of the polymer? (7)

27.  The ratio of carbon to hydrogen to nitrogen atoms in nicotine is 5 to 7 to 1.  What is the molecular formula of

nicotine if its gram molecular mass is 162 g? The empirical formula is C₅H₇N. (7)

28. If 4.0 g of H₂ are made to react with excess CO, how many grams of CH₃OH can theoretically be produced according to the following equation? (9)         CO(g) + 2H₂ (g) à CH₃OH(l)

 

29. How many grams of butane (C₄ H₁₀) must be burned in an excess of O₂ to produce 15.0 g of CO₂? (9)

2C₄ H₁₀ (g) + 13O₂ (g) à 8CO₂ (g) + 10H₂O(g)

30. What is the importance of the coefficients in a balanced chemical reaction? (9)

31. In which kind of stoichiometric calculation can the steps involving conversion to and from moles be omitted?  Explain why it is possible to do so. (9)

32. Explain why it takes more energy to remove a 4s electron from zinc than from calcium. (13)

33. Give the electron configuration for a neutral atom of chlorine. (13)

34. Describe the different principles that govern the building of an electron configuration. (13)

35. Explain why the 4s sublevel fills before the 3d sublevel begins to fill as electrons are added. (13)

36. What is the quantum mechanical model? (13)