Chemistry Semester Exam Review

Chapter 1:

  1. Give examples of qualitative data(p.10).
  2. Give examples of quantitative data (p.11).

Chapter 2:

  1. Define “meter”.
  2. Calculate density (Practice Problems 1-3, p.29)
  3. Multiplying in scientific notation (Practice Problem 15, p.33)
  4. Convert 470 mg to grams --- SHOW ALL YOUR WORK!
  5. Define “accuracy”. Look at Table 2-4, p.37. Which student is most accurate?
  6. Determine the number of significant figures in a number (Practice Problems 31-32, p.39).
  7. Add numbers and round to the correct number of significant figures (Practice Problem 35, p.41).
  8. Using Graphs:
  9. Calculate slope (example on p.44)
  10. Interpret graphs (see p. 45)
  11. P.53 (8, 9)

Chapter 3:

  1. Define “substance” (p.55). Is seawater a pure substance?
  2. List physical properties of copper (Table 3-2, p.57).
  3. Distinguish between properties of solids, liquids, and gases, pp. 58-59. (You should have a Venn diagram of this.)
  4. Identify physical changes (pp.61-62).
  5. Define “chemical change”. (p.62)
  6. Identify chemical changes (pp.62-63).
  7. State the law of conservation of mass (p.63).
  8. Define “homogeneous mixture” and “heterogeneous mixture” (p.67).
  9. What is another name for homogeneous mixture?
  10. Is orange juice a heterogeneous or homogeneous mixture?
  11. Can you write a formula for a mixture?
  12. How can you very easily determine if something is an element?

Chapter 4:

  1. What did Democritus call the tiny particles that make up matter? (p.88)
  2. The neutral subatomic called a ______was discovered by James Chadwick.
  3. Negatively-charged subatomic particle:
  4. Positively-charged subatomic particle:
  5. Define “atomic number” (p.98).
  6. Identify atomic number and atomic mass in chemical symbols (Fig. 4-15, p.100).
  7. Define “isotope” (p.100).
  8. The number of electrons in an atom is equal to the number of ______.

Chapter 5:

  1. Define “electron configuration” (p.135).
  2. Write the noble gas form of the electron configuration for selenium and phosphorous.
  3. Write the electron dot structure of selenium and phosphorous.

Chapter 6:

  1. What are columns on the periodic table called?
  2. What are rows on the periodic table called?
  3. Identify whether an element is a metal, nonmetal, or metalloid.
  4. Define “metalloid” (p.158).
  5. What are group 1A elements called?
  6. What are group 2A elements called?
  7. What is the first transition metal?
  8. Identify the number of valence electrons on elements in each group:
  9. 1A
  10. 2A
  11. 3A
  12. 4A
  13. 5A
  14. 6A
  15. 7A
  16. 8A

Chapter 7:

  1. What is the charge of an ion formed by elements in each group?
  2. 1A
  3. 2A
  4. 3A
  5. 4A
  6. 5A
  7. 6A
  8. 7A
  9. 8A
  10. Which is more stable, a sodium atom or a sodium ion?
  11. What is another name for the charge on a monatomic ion? (p.222)
  12. Ionic bonds form between positively-charged ______(p.212) and negatively-charged ______(p.214).
  13. Ionic bonds are formed by electrostatic attraction between opposite charges.
  14. Write formulas for ionic compounds (Practice Problems 19-23, p.224).
  15. Define metallic bond” (p.228).
  16. Electron configuration of noble gases is called an octet.
  17. What is the difference between helium and the other noble gases?

Chapter 9:

  1. What makes up a:
  2. Single covalent bond (p.245)
  3. Double covalent bond (p.246)
  4. Triple covalent bond (p.246)
  5. Hydrogen forms a ______covalent bond with another hydrogen atom.
  6. Oxygen forms a ______covalent bond with another oxygen atom.
  7. Nitrogen forms a ______covalent bond with another nitrogen atom.
  8. Know prefixes used in naming covalent compounds (Table 9-1, p.248).
  9. Name binary acids (p.250).
  10. Oxyanion = -ate, acid = -ic. Oxyanion = -ite, acid = -ous.
  11. Difference in electronegativity = polar covalent bond (i.e., H is 2.20, and Cl is 3.55).