Chemistry Final Study Guide-Pre-AP

Name:______

Chemistry Intro., Measurement; Scientific Method (Chpt, 1 and 2)

1. Convert 6.5 mm to cm

2.Convert 875mg to kg

3.Write 0.00125 g in scientific notation.

4.Write 598,000,000 light years in scientific notation.

What is the difference between accuracy and precision?

5.A student weighs a sample three times and gets the following results:

Trial 1: 3.50 g Trial 2: 3.51g Trial 3: 3.53g

The actual value was 4.5 g.

Was the student’s results accurate, precise, or both? Explain.

6.What is the density of a 125g sample with a volume of 35mL?

7.What is the volume of a 50g sample with a density of 2.8 g/mL?

8.Determine the number of significant figures in each measurement below.

  1. 5.600 g b. 5.09x10-4 g c. 0.00560g

9.Calculate and write the answer with the correct number of significant figures.

  1. 9.0g + 18.6g + 15g =
  2. 1.25m x 0.0450m x 2.04m =

Matter and Change (Chapter 3) (Study Matter flow chart)

10. Classify each as a physical change or a chemical change.

  1. cooking an egg d. evaporating water
  2. burning a match e. dissolving sugar in a glass of tea
  3. crushing a can f. animal decomposing

11.What is the difference between a substance and a mixture?

12.Classify each as a substance or a mixture.

  1. NaCl e. tap water
  2. NaCl solution f. deionized water
  3. Iron statue
  4. soil sample

13.Classify each as a heterogenous or homogenous mixture

  1. Salt water
  2. Oil and water
  3. Beef stew
  4. Kool-aid

14.Define shape and volume with each state of matter. (solid, liquid, gas)

15.What is the difference between intermolecular and intramolecular forces?

16.What happens to the intermolecular forces and kinetic energy during each phase process below:

  1. freezing
  2. evaporation
  3. condensation
  4. sublimation

17.A 77.5 g sample of an unknown solid is heated to 62.5˚C and placed into a calorimeter containing 93 g of water at 23.3˚C. If the final temperature of the solid sample and the water is 26.2˚C, what is the specific heat of the solid? (remember q=q or mΔTCp = mΔTCp)

18.What type of reaction does the graph show? How do you know?

19.What type of reaction does this graph represent? How do you know?

20.Define Specific Heat……What is the specific heat of water?

21.A silver bar with a mass of 250.0 g is heated from 22.0˚C to 68.5˚C. How much heat does the silver bar absorb? (Cp of silver is .235 J/g˚ C)

Atomic Structure: (Chapter 4)

22.What is Dalton’s Atomic Theory?

23.Complete the table on atomic subparticles.

Subparticle / Atom’s Location / Charge / Mass
proton
neutron
electron

24.Complete the table on atomic subparticles.

Element Symbol / Atomic # / Mass # / # of p+ / # of n0 / # of e-
Be / 9
107 / 47 / 46
Mg2+ / 25
15 / 16 / 15
N3- / 14

25.Classify the type of ion Mg2+ and N3-are ?

26.Iodine has three isotopes

I-127 has a natural abundance of 80%

I-126 has a natural abundance of 17%

I-128 has a natural abundance of 3%

  1. What is the atomic number for Iodine?
  2. Complete the table for each iodine isotope.

Iodine’s Isotopes / # of protons / # of electrons / # of neutrons
I-126
I-127
I-128
  1. What is a similarity and a difference between iodine’s isotopes?
  2. Calculate the atomic mass of Iodine.

27.What is the difference between mass number and atomic mass?

Periodic Table (Chapter 6)

28.How is the modern periodic table arranged?

29.Give me an example of a metal, non-metal, and a metalloid.

30.Classify each property below as a metal (M) or non-metal (NM)

  1. brittle b. conductors b. insulators d. malleable e. low melting point f. high melting point g. high density f. low density

31.Distinguish between representative elements and transitional elements. Give an example of each.

32.What element is in period 4, group 6?

33.What are valence electrons?

34.How many valence electrons does group 3 have? Group 17 have?

35.Which group of elements is consider to be the most stable and why?

36.a. What type of ion does a metal become to reach stability?

  1. What type of ion does a non-metal become to reach stability?

37.a. What is atomic radius?

b.Use the graph below to explain the periodic trend for atomic radius across a period and down a group.

38. a. What is ionization energy?

b.Use the graph below to explain the periodic trend for ionization energy across a period and down a group.

35. a. Rank the elements below from largest to smallest in size.

Li, Li1+, F, F1-

largest ______smallest

(size ) (size)

Electron Properties and Arrangement (Chapter 5)

36. Electrons have similar properties to light particles because they are both very tiny in size and travel extremely fast. An electromagnetic spectrum breaks light particles into different regions based on the following properties: frequency, wavelength, and energy. Use the table below to answer the following questions.

a.What happens to frequency when energy increases?

b.What happens to energy when wavelength increases?

c.What happens to wavelength when frequency decreases?

37. T or F Each period on the periodic table represents an energy level?

38. What is the maximum number of electrons on the 3rd energy level?

39. Draw the four type of orbitals that electrons can move around in.

40.What orbitals are present on the second energy level?

41.What is the electron configuration (arrangement) of oxygen, iron, and bromine?

42.How many unpaired electrons does iron have in its electron configuration?

Chemical Bonding and Naming (Chapter 7-9)

43. What is some similarities and differences between ionic and covalent compounds. (Drawing a Venn Diagram might be helpful).

44. Classify the following as either ionic or covalent (molecular).

a. CaCl2 b. CO2 c. K3(PO4) d. SO3 e. O2 f. Pb3N g. (NH4)2(SO3)

b.Write the chemical names of the compounds listed in question 43.

45. Write the chemical formula for each of the following compounds.

  • sulfur hexafluoride
  • lithium nitride
  • chromium (III) carbonate
  • tin(II) chloride
  • ammonium acetate
  • bromine

46. Molecular Compounds: H2 H2O 3 CO2 (You will need electronegativity table)

a. Draw the molecular structure for each molecule above.

b. Classify their covalent bonds as either sigma or pi.

c. Classify the bonds as either polar or non-polar.

d. Classify the molecules as either polar or non-polar.

e. Identify what type of intermolecular force holds a collection of the molecules together in a sample of matter: hydrogen bonding, London’s dipole-dipole forces, Vander Waal forces.

Chemical Reactions (Chapter 10) and Nuclear Reaction (Chpt. 25)

47.Classify and balance the following chemical reactions.

a. H2O -----> H2 + O2

b. CH4 + O2 ----> CO2 + H2O

c. O2 + KCl -----> KClO3

d. Na(OH) + FeBr3 ----> NaBr + Fe(OH)3

48.What are some similarities and differences between chemical and nuclear reactions?

(Venn Diagram)

49. What is the symbol and charge for alpha, beta, and gamma radiation?

50. If beta was placed in an electrical field would its pathway change? If so, would it bend near the positive magnet or the negative magnet? Explain.

51.Complete the nuclear equations:

a. Beta decay of Potassium-40

b. Alpha decay of Plutonium-242

c. Alpha decay of Uranium-239

52. What is a radioisotope?

53. Using the band of stability graph, determine which of the following isotopes are classified as radioisotopes?

a. N-14 b. Ba-112 c. Th-240 d. Sn-110

54. a. What is the half-life for a radioisotope?

b. If we start with a 175 gram sample of Thorium-134, how much will be left after three half-lives. The half-life of T-134 is 24.1 days.

55. Use the radioactive decay graph to answer the following questions.

a. Label the line that represents the parent and daughter isotope.

b. How much of the parent isotope is left over when 0.85 of the sample has decayed into the

daughter isotope?

c. At what half-life is the daughter isotope fraction equal to 0.65.

Chapter 10: Chemical Quantities

56. What is the mole conversion used to convert to representative particles of a substance?

57. What is the mole conversion used to convert to mass of a substance.

58. Identify what type of representative particle (atom, ionic compound, molecule) represents each substance below.

a. H2O B. MgCl2 c. Br2 d. Fe

59. Convert 6.32x1020 atoms of Fe to moles of Fe.

60. Convert 8.6 grams of Ba3(PO3)2 to moles of Ba3(PO3)2.

61. How many atoms of copper are in 30.2 grams of copper wire?

62. How many grams are equivalent to 4.32x1022 compounds of NaCl?

63. What is a hydrate?

64. Calculate the percent composition of water in the following hydrate: Fe(SO4) 7H2O .

65. T or F: When an anhydrous salt is produced from a hydrate this is an example of a chemical reaction.

Chapter 12: Stoichiometry

66. What is stoichiometry?

67. Use your balanced equation from 47b. to answer the following questions.

a. Calculate how many moles of water will be produced if 0.35 moles of methane, CH4 reacts with oxygen.

b. Calculate how many moles of carbon dioxide will be produced if 0.35 moles of methane, CH4 reacts with oxygen.

c. Calculate how many grams of O2 is needed to react with 2.8 grams of CH4.

d. Calculate how many grams of CH4 is needed to produce 9.75 grams of CO2.

68. a. What is the difference between limiting and excess reactants?

69. 2Cu + S ------> Cu2S.

a. What is the limiting reactant when 80.0 grams of Cu reacts with 25.0 grams of S ?

b. Using the limiting reactant, calculate how many grams of Cu2S you should theoretically produce from this reaction?

c. If you actually produced 95 grams of Cu2S in the lab, calculate what your percent yield would be?

% yield= (actual yield divided by theoretical yield)x100

Chapter 14: Gas Laws

68. Determine the volume of 12.3 grams of formaldehyde gas (CH2O) at STP.

69. A sample of ammonia gas occupies a volume of 1.58L at 22.0˚C and a pressure of 0.983 atm. What volume will the sample occupy at 1.00 atm and 0˚C?

70. A balloon is inflated with 2.42 L of Helium at a temp of 27˚C. Later, the volume of the balloon has changed to 2.37 L at a temp of 19˚C and a pressure of 99.7 kPa. What was the pressure when the balloon was inflated?

71. Find the total pressure of ammonia in a mixture of three gases with a total pressure of 75.6 kPa if the sum of the partial pressures of the other two gases is 34.9 kPa.

72. A container with two gases, helium and argon, is 30.0% by volume helium. Calculate the

partial pressure of helium and argon if the total pressure inside the container is 4.00 atm.

73. What is the final volume of a 400.0 mL gas sample that is subjected to a temperature

change from 22.0 °C to 30.0 °C and a pressure change from 760.0 mmHg to 360.0 mmHg?

74. What is the volume at STP of 720.0 mL of a gas collected at 20.0 °C and 3.00 atm pressure?

75. How many moles of gas would be present in a gas trapped within a 100.0 mL vessel at 25.0

°C at a pressure of 2.50 atmospheres?