Name ______Date:______

Chemistry Semester IFinal Exam Review Guide

Topics Covered

  • Unit 1:Metric system, Temperature Conversions, Unit Conversions, Significant Figures, Percent Error, Scientific Notation, Density, Dimensional Analysis with conversions, reading a graduated cylinder, recording significant figures in the lab
  • Unit 2: Elements, Compounds, Pure Substances, Mixtures, Physical and Chemical Changes and Properties, heat, specific heat
  • Unit 3: Groups on the Periodic table, Atomic Structure, Atoms, Ions, Isotopes, Atomic Mass, characteristics of metals, and nonmetals, balancing nuclear reactions, half-life problems, Identifying a pure substance, homogenous mixture, heterogenous mixture, element, and compound through molecular diagrams.
  • Unit 4: Naming and writing formulas for ionic compounds, molecules, and acids, cations, anions, polyatomic ions.
  • Unit 5: Percent composition, molar mass, mole conversions, empirical formulas, and molecular formulas

UNIT 1: Scientific Measurement (Chapter 2)

1. How many sig figs are in the following numbers?

2.04 ______0.002804 ______1,230 ______0.00989 ______

2. When adding and subtracting, the rule for sig figs is to look at the number of ______.

Calculate the following using correct sig figs: 18.345 + 4.12 = ______21.672 – 0.5 = ______

3. When multiplying and dividing, the rule for sig figs is to look at the number of ______.

Calculate the following using correct sig figs: 5.678 x 2.3 = ______18.1 x 3 = ______

4. Put the following numbers in scientific notation: 8,923,000,000 = ______

0.00000345 = ______0.00045 = ______

5. Do the following unit conversions: 6.7dm = ______mm325 cL = ______L

6. How many kilometers are in 7650milimeters? ______

7. How many centigrams are in 8.56 decigrams? ______

8. The formula for density is: ______Density is the ratio of ______to ______.

9. Calculate the density of an object if it has a mass of 13.2 grams and a volume of 3.4 liters.

Density = ______

10. Calculate the mass of a piece of plastic that has a density of 3.14 g/mL and a volume of 7.2 mL.

Mass = ______

11. Calculate the volume of an unknown substance that weighs 23.1 grams and has a density of 5.6 g/mL.

Volume = ______

12. Perform the following temperature conversions: 967ºC = ______K 435 K = ______ºC

13. Calculate the percent error: Experimental Length = 14.1 cmAccepted Length = 14.9 cm

14. Use dimensional analysis to solve the following density problem: How many liters are 45.7 kg of bromine? The density of bromine is 3.10g/mL.

UNIT 2: Matter and Change (Chapter 3)

15. What is a chemical change? ______

Which of the following is a chemical change: ripping a piece of paper, melting ice, burning wood?

16. Give 2 examples of physical changes: ______

17. What is the difference between physical and chemical properties? ______

______

Which of the following is NOT a physical property? color, boiling point, texture, density, reactivity

18. Name 2 chemical properties: ______

19. What is the difference between heterogeneous and homogeneous mixtures? ______

______

Which of the following is an example of a homogeneous mixture? copper, salsa, salt, Gatorade

20. Determine if each is a pure substance or a mixture:

sodium (Na)______Kool-Aid ______water ______

21. Name the 4 indicators of chemical change:

______, ______, ______, ______

22. Define heat:

23. Define specific heat:

24. Convert the following: 38.65 cal = J934 J = kcal

25. How much energy (in joules) is required to heat a piece of iron weighing 1.30g from 25.0oC to 46.0oC?

26. A 55.0g sample of a metal requires 675 J of energy to hear it from 25.0oC to 118.0oC. Calculate the specific heat of the metal.

UNIT 3: Atomic Structure (Chapter 4)

27. Calculate the atomic mass of iron based on the following information:

Fe-56 (94.5 %) Fe-57 (2.3 %) Fe-59 (3.2 %)

28. The mass number is found by adding ______plus ______.

29. What is the difference between a cation and an anion? (Which is positive/negative? Gained or lost e-?)

Cation: ______

Anion: ______

30. Nickel: Protons = ______Neutrons = ______Electrons = ______

Chlorine: Protons = ______Neutrons = ______Electrons = ______

31. How many neutrons are in the following isotopes?

Co-60 ______U-235 ______W-185 ______

32. Name 2 noble gases: ______, ______Name 2 halogens: ______, ______

33. Give 3 examples of transition metals: ______, ______, ______

34. What do the numbers represent in the following symbol? 190Os

76

190 = ______76 = ______

35. The rows on the periodic table are called ______.

The columns on the periodic table are called ______.

36. Write the correct charge and name for the following ions.

Example:Calcium = Ca2+ Calcium ionSulfur = S2- Sulfide

Lithium = ______Fluorine = ______

Magnesium = ______Nitrogen = ______

37. As Potassium becomes as ion, it likes to ______(gain/lose) electrons. How many? ______

As Oxygen becomes an ion, it likes to ______(gain/lose) electrons. How many? ______

38. Sn-120: Protons = ______Neutrons = ______Electrons = ______

39. Atoms of the same element alwayshave the same number of ______(protons, neutrons, electrons)

40. An isotope has 12 protons, 12 electrons, and 14 neutrons. Name the isotope using hyphen notation: ______

41. Metals are located on the side of the periodic table, and tend to electrons to

form . List two characteristics of metals:

42. Nonmetals are located on the side of the periodic table, and tend to

electrons to form . List two characteristics of nonmetals:

43. List the metalloids:

44. What are the four nuclear particles?

______

45. Balance the following nuclear reactions:

46. Write a balanced reaction for each nuclear reaction.

Decay of polonium-218 by alpha emission.Decay of chlorine-32 by positron emission.

Decay of promethium-142 by electron capture.Decay of oxygen 18 by emission of two neutrons

47. What is half-life?

48. The half-life of phosphorous-30 is 2.5 min. If you start with 35 g of phosphorus-30, how many grams would remain after 20.0 min?

49. The half-life of polonium-210 is 138.4 days. How many milligrams of polonium-210 remain after 415.2 days if you start with 2.0 mg of the isotope?

50. 20.0 g of a radioactive isotope are present at 1:00 p.m., and 5.0 g remain at 2:00 p.m.

  1. How many half-lives have gone by?______
  2. How long is the half-life of the isotope? ______
  3. Predict how many grams will be left at 2:30 p.m.______

51. Know the safety rules

52. Be able to identify the various lab equipment and know their uses and know what units each measures.

Unit 4: Naming (Chapter 5)

53. What do all ionic compounds begin with?

54. Why do you have to use a roman numeral to identify some cations?

55. What do all acids begin with?

56. What do all molecules begin with?

57. Name the following compounds/molecules.

Zn3(PO3)2______

Co3N2 ______

S4Br7______

H2CO3______

58. Write the formula for the following compounds/molecules.

Hydrofluoric acid______

Nickel (II) chlorate ______

Dicarbon pentaiodide______

Aluminum nitrate ______

Unit 6 The Mole (Chapter 8)

59. What is Avogadro’s number?

60. How many things are in one mole?

61. What is the molar mass of MgCl2?

62. How many moles of SO3 are in 2.4 x 1024 molecules of SO3?

63. How many atoms of aluminum are present in a 0.275 mole sample of Al2(CO3)3?

64. How many grams of Ba(IO3)2 are there in a 1.25 x 1022 formula unit sample of Ba(IO3)2?

65. Determine the percentage composition of sulfur in SCl2

66. Given the following percent composition data. Determine the empirical formula of the following compound.

56.8 % C

6.50 % H

28.4 % O

8.30 % N

67. The empirical formula was found to be C2H4O. What is the molecular formula if the molar mass of this molecule is 132.16?