Chemistry Final Review Packet – F10 Name:
Atom or Ion / Symbol / Name / Atomic Number / MassNumber / # of Protons / # of Neutrons / # of Electrons / Overall Charge
1. / Fe / 2. / 3. / 4. / 5. / 6. / 24 / 7.
For 8-16 put ALL letters that apply. P) protons N) neutrons e) electrons
8. Have a positive charge
9. Have a negative charge
10. Have a neutral charge.
11. These two types of particles are located in the nucleus of an atom.
12. Located in energy levels outside the nucleus of an atom.
13. Whether atom or ion, the number of these is always the same as the atomic number.
14. In an atom, the number of these is equal to the number of protons; In an ion, the number of these is different from the number of protons.
15. Add the total of these two types of particles to get the atom's mass (atomic mass).
16. Isotopes of an element, such as C-12 and C-14, have different numbers of this particle.
A substance has 6 protons, 8 neutrons, and 6 electrons. Decide if each statement is true or false. If false, explain.
17. This substance is nitrogen.
18. This substance is carbon.
19. This substance is an ion.
20. This substance is an isotope of carbon-12 (12C)
21. The Atomic Theory was first stated in the late 1700s. Which of the following is NOT part of this Atomic Theory?
A) All elements are composed of tiny indivisible particles called atoms.
B) Atoms are made of smaller particles of positive, neutral, and negative charges
C) All atoms of the same element are identical but different from those of every other element
D) In a chemical reaction atoms are rearranged but not created or destroyed
22. If you could somehow subtract a proton from a beryllium atom, it would become
A) lithium B) helium C) a + ion D) an isotope E) nitrogen
23. If you could somehow lose an electron from a beryllium atom, it would become
A) lithium B) helium C) a + ion D) an isotope E) nitrogen
24. If you could somehow add another neutron to a beryllium atom, it would become
A) lithium B) helium C) a + ion D) an isotope E) nitrogen
25. What is the difference between an ATOM and an ION?
26. Name the following:
a) SiF4 ______
b) N2S3 ______
c) CO ______
27. Write the formulas for the following:
d) diboron hexahydride ______
e) nitrogen tribromide ______
f) diphosphorus pentoxide ______
28. A positive ion is called a(n) ______. A negative ion is called a(n) ______.
Write the formula for:
29. Na and O ______
30. Ca and ClO3 ______
31. Write the formulas for the following binary compounds.
sodium fluoride ______
copper (II) chloride ______
iron (III) sulfide ______
32. Each of the following formulas or chemical names contains an error. Correct each example.
Al3O2 ______
(OH)3B ______
Ca2O2 ______
33. List three differences between ionic and covalent compounds:
For 34-39, decide whether the statement refers to ionic or covalent bonds.
34. This type of bond results from transfer of electrons.
35. This type of bond results from a sharing electrons.
36. This is a bond between two ions.
37. This type of bond would result from the bonding of an element from the far left of the periodic table bonding with an element from the far right.
38. A bond between a metal and a nonmetal would be this type.
39. A bond between two nonmetals in the same family would be this type.
40. What is the difference between polar and nonpolar bonds?
41. What are polyatomic ions?
42. The density of a metal bar is 5.8 g/cm3 and its volume is 14.7cm3. What is its mass?
43. Know the meaning of the following terms: matter, mass, weight, density, volume, mixture, molecule, diatomic molecule, homogeneous mixture, heterogeneous mixture, solution
44. Where do you find metals, metalloids, nonmetals, transition elements, periods, and groups on the periodic table?
45. What are the differences between a physical property and a chemical property? Between a physical change and a chemical change?
46. Define the following terms: precipitate, aqueous solution, reactant, product, coefficient, subscript
47. What is the difference between endothermic and exothermic? Which absorbs and which releases energy?
48. What is the Law of Conservation of Matter?
49. Compare and contrast the properties of solids, liquids, and gases.
50. Explain how kinetic energy is involved in changing states and know what we call each change (i.e. melting, sublimation, etc.)
51. Know the basics of the major contributions of the following individuals to the development of the atomic theory: John Dalton, J.J. Thompson, Ernest Rutherford, and Neils Bohr.
52. Name the ion formed by each. Indicate whether an anion or cation: S Na
53. What are valance electrons and oxidation numbers? Know how to identify them from the periodic table.
54. When you put an element in a flame, you see different colors of light given off. How/why?
55. Write the long and short electron configuration for:
Al
Pt
56. How do the mass of reactants and products compare?
57. Define limiting and excess reagent
58. In the chemical reaction that follows, if you have 19.4 grams of CO2, how much glucose (C6H12O6) could be made? Balance the equation first. CO2 + H2O à C6H12O6 + O2
59. Suppose you buy some inflated party balloons that are at room temperature. What will happen to those balloons if you take them outside on a very cold day? Explain.
60. If four moles of a gas at a pressure of 5.4 atmospheres have a volume of 120 liters, what is the temperature?
61. What unit for temperature is used for all gas law problems?
62. If I initially have a gas at a pressure of 12 atm, a volume of 23 liters, and a temperature of 200 K, and then I raise the pressure to 14 atm and increase the temperature to 300 K, what is the new volume of the gas?
63. Define “mole”.
64. Roundup™, an herbicide manufactured by Monsanto has the formula C3H8NO5P. What is the molar mass?
65. How many grams of chlorine gas should be produced if 84.2 grams of aluminum chloride and 68.4 grams bromine are combined? 2AlCl3 + 3Br2 à 2AlBr3 + 3Cl2
66. How many moles of Cu are needed to react with 5.8 moles of AgNO3?
Cu + 2 AgNO3 à Cu(NO3)2 + 2 Ag
67. A sample of sulfur has a mass of 223 g. How many moles of sulfur are in the sample?
68. Calculate the mass of 3.89 moles of ethanol (C2H5OH).
69. Determine the mass of 0.187 mol of tin (II) sulfate (SnSO4)
70. Calculate the number of atoms in 27.2 g of plutonium.
71. If a student has 9.22 x 1023 atoms of cobalt, how many grams do they have?
72. What is the percent composition of C4H8O?
73. How many liters of O2 do you have if you have 5.8 mols of O2?
74. Vinegar has a percent composition of 40.0% Carbon, 53.3% Oxygen and the remainder is Hydrogen. The atomic mass of vinegar is 60 g/mol. What is the molecular formula of vinegar?
75. Find the empirical formula for the following percent composition: 25.9% Nitrogen and 74.1% Oxygen
76. Convert the following into scientific notation.
0.00000078 = ______21000 = ______
77. Convert the following into standard notation.
3.8 x 10-3 =______3.8 x 106 =______
78. Identify the number of sig figs in the following.
0.00203 ______120,000 ______
79. Write a balanced chemical equation that illustrates each type of reaction.
Synthesis
Decomposition
Single-Replacement
Double-Replacement
Combustion
80. Balance: C2H6 + O2 à CO2 + H2O
81. Compare/contrast acids and bases
82. What is pH and how is it measured?
83. What factors affect solubility?
84. What is molarity?
85. If I have 2.5 mol of calcium carbonate in .3 L of solution, what is the molarity?
86. If I have 700 mL of a 5 M NaOH solution, how many grams of NaOH were used to make the solution?
87. What are colligative properties?
88. What are intermolecular forces and intramolecular forces?
89. What is the specific heat of a substance that absorbs 2.5 x 103 joules of heat when a sample of1000 g of the substance increases in temperature from 10.0 0C to 70.0 0C?
90. How many grams of water would require 2.20 x 104 joules of heat to raise its temperature from 34.0°C to 100.0°C? The specific heat of water is 4.18 J/g∙°C