Honors Chemistry Midterm Exam Review

Topics: UNIT 1 – UNIT 5

Formula writing Nomenclature Molar mass and gram/mole conversions Gram/mole/liter/molecule conversions Balancing equations Reaction types Stoichiometry Radioactivity Nuclear chemistry equations Scientists for atomic theory Periodic Table (everything) and Trends Quantum numbers, orbitals, electron configurations Solutions and Solubility Concentraion and Molarity calculations Colligative prop calculations

Example Questions:

1. What is the symbol for the sulfate ion?

2. Write the formula for magnesium acetate.

3. What is the name of Na2CO3?

4. What is the formula for nitric acid?

5. Name C2H6

6. What is the formula for iron(III) chloride?

7. Calculate the molar mass of iron(III) chloride.

8. How many grams of hydrogen gas at STP are in 3.50L? 9. Know how to balance equations.

10. How many moles are in 25.0g sodium chloride?

11. How many grams are in 0.959 moles of water?

12. List the 5 different types of reactions and write an example of each.

13. Define limiting reactant and % yield.

14. Sodium reacts with water and forms sodium hydroxide and hydrogen gas. If 24.8g of sodium is added, then how many molecules of hydrogen are formed?

15. Define half-life.

16. How many protons are in C-14?

17. How many neutrons are in U-235? 18. Define isotope.

19. Define radioactivity.

20. List and define the 3 types of radioactivity.

21. Who discovered the uncertainty principle?

22. Who said the atom was like a solar system and the electrons transition between energy levels?

23. Who discovered the nucleus using a Gold Foil experiment?

24. Define fission and fusion.

25. What family name applies to iodine and other Group 17 non-metals?

26. What family name applies to magnesium and other Group 2 metals?

27. Define ionization energy and electronegativity.

28. Define and compare/contrast energy levels, sublevels and orbitals: 29. How many p-orbitals are there in a p-sublevel?

30. What types of orbitals are found in the 4th energy level?

31. Know how to write and analyze electron configurations.

32. How many valence electrons do the alkali metals have?

33. Define wavelength and frequency.

34. Who created the first Periodic Table of the Elements?

35. What happens to the size of the atom when it becomes a positive ion?

36. Define allotrope.

37. Know the property differences between metals and nonmetals.

38. Calculate the molarity of 5.00g of potassium nitrate in a 250.0 mL flask.

39. Compare and contrast the properties of solids and liquids.

40. Define colligative property.

41. List the various types of intermolecular forces and compare them in terms of definitions and relative strengths:

42. What is the molality of a non-electrolyte solution of C2H4(OH)2 in water if the new freezing point is -5.50 ºC? Kf is -1.86 ºC/m.

43. How do you prepare a 0.500M solution of sodium chloride in a 100.0 mL flask?

44. Know the difference between a beaker, grad. cylinder, volumetric flask and Erlenmeyer flask. There will be two, 10 point open-ended questions for you to answer on the midterm exam. The following are examples and practice to prepare for the midterm questions. The essay topics are: 1. Reactions and Stoichiometry 2. Periodic Table Trends 3. Solutions and Solubility 4. Atomic Theory

1. Reactions and Stoichiometry

Ex. “A lab scientist combines 55.0 grams of magnesium metal with an excess quantity of nitrogen gas” Write the balanced chemical equation:

What type of chemical reaction is this?

Show stoichiometry work to calculate the theoretical mass (grams) of product that will form for this reaction:

Show work to calculate percent yield if this lab scientist experimentally collects 61.5 grams of product: 2. Periodic Table Trends

Ex. “The location of Barium on the periodic table reminds us that atoms of Barium have very distinct properties compared to atoms of other elements”

Do atoms of Barium have larger or smaller atomic radii than most other metals? Explain the scientific factors behind your choice:

Do atoms of Barium have large or small electronegativity values compared to atoms of other elements? Explain the scientific factors behind your choice:

Define ionization energy and explain why the 1st and 2nd ionization energy values for Barium atoms would be small in comparison to the 3rd ionization energy value for Barium: 3. Solutions and Solubility

Ex. “Describe, on a molecular level, the dissolving process of sodium chloride in a water solvent. Discuss the difference between unsaturated and saturated solutions and describe the saturation point and define solubility.”

4. Atomic Theory

Ex. “Our view and understanding of the atom has changed drastically throughout recent history. Many scientists have contributed to the understanding that we have about the atom.” Describe the role each of the following scientist hade in the development of atomic theory: Thomson, Rutherford and Bohr. Include a diagram to show the model of the atom that was commonly accepted at the time each scientist did their work.