CHEMISTRY I HONORS

SPRING SEMESTER 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

1. Name the five major divisions of chemistry and give examples of the types of subjects studied within each division.

2. Identify five examples of matter and five examples of nonmatter.

3. Explain the difference between a qualitative and a quantitative measurement. Provide examples to illustrate this difference.

4. Explain what is meant by dimensional analysis. Use an example in your explanation.

5. Explain how the atoms of one element differ from those of another element.

6. Explain the terms molecular formula and formula unit. Give an example of each.

7. What is the advantage of using the specific term, gram molecular mass, instead of the general term, gram formula mass?

8. What determines whether one metal will replace another metal from a compound in a single-replacement reaction?

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

10. Name the three basic assumptions of the kinetic theory.

11. Explain the difference between temperature and heat. Also, state what determines the direction of heat transfer.

12. What are some of the differences between a real gas and an ideal gas?

13. Describe the shapes and relative energies of the s, p, d, and f atomic orbitals.

14. Describe the periodic trends in atomic radii that can be observed in the periodic table. Provide examples.

15. Explain the octet rule and give an example of how it is used.

16. Explain what an unshared pair of electrons is. Give an example.

17. Describe the structure of the water molecule and indicate how this structure is responsible for many of the unique properties of this vital compound.

18. Explain what a saturated solution is. Give a specific example.

19. Explain the effects of reactant concentration and particle size on the rate of a reaction.

20. Compare and contrast the properties of acids and bases.

21. What happens in a neutralization reaction? Use an example.

22. What are the steps of the oxidation number change method of balancing REDOX reactions?

23. What are the steps of the half-reaction method of balancing REDOX reactions?

24. Explain what occurs in an electrochemical cell.

25. Explain why carbon is able to form such a wide variety of compounds.

26. Given the name of an alkane, indicate how you can reconstruct its structural formula according to IUPAC rules.

27. Explain how geometric isomers differ from each other. Describe the difference between the trans and cis configurations of geometric isomers. Provide an example of each configuration for molecules that exhibit geometric isomerism.

28. Explain the concept of resonance. Give an example of a compound that displays resonance.

29. Describe the process of making sucrose. Give an example.

30. Give an example of a substitution reaction and describe what happens in the reaction.

31. Distinguish between alpha particles, beta particles, and gamma rays. Indicate how the atomic number and atomic mass number change when each type of radiation is emitted.