Download General Chemistry - Review for final exam: (Make sure you bring

CP Chemistry - Review for final exam: (Make sure you bring your 3 x 5 cards!!!!!)
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What is matter?
What is a physical property of matter?
What is a chemical property of matter
List the properties of the 3 states (phases) of matter.
a. Solid
b. Liquid
c. Gas
5. What is the difference between a compound and a mixture?
6. What is a homogeneous mixture?
7. What is the name of a solid homogeneous mixture of metals?
8. What is a heterogeneous mixture?
9. What are the 2 pure substances?
10. How are elements represented on the periodic table?
11. What does a chemical formula tell you about a compound?
12. Where do you find the reactants and products in a chemical equation?
13. How does the law of Conservation of Mass relate to chemical equations?
14. 0.00004950 (place in scientific notation)
15. How many significant digits do the following have?
a. 0.000204
b. 10050
c. 10000
d. 5078.00
e. 587 x 100 (solve)
f. 456 +12.0 (solve)
g. multiply the following: 3.1 x 103, 2.0 x 10-2, 1.5x10-5
16. In a measurement what is the estimated digit?
17. List the metric measurements mega – micro, include their magnitude.
18. What are the SI units for mass, length, quantity, time.
19. What is weight?
20. How is Celsius converted to Kelvin?
a. What is the boiling point of water in K?
21. What is the formula for density?
22. Where are the subatomic particles (protons, neutrons, electrons) found in an atom?
23. What did Rutherford tell us about the composition of the atom?
24. What is an isotope?
25. Write out Na ion in chemical notation and list the numbers of the subatomic particles.
26. What is the unit for atomic mass?
27. How is atomic mass derived?
28. How is the mass on the periodic table calculated?
29. What are the shapes of the s & p orbitals?
30. How many orbitals & electrons are in the following systems?
a. s
b. p
c. d
d. f
31. What is the max # of electrons that can fit into an orbital?
32. What did the following say about orbital systems:
a. Hund
b. Aufbau
c. Pauli
33. List parts of the visible electromagnetic spectrum & label in terms of frequency,
wavelength, & energy.
34. What is the formula for the speed of light?
35. How is a photon created as an atom is heated?
36. According to Schrodinger, where are you most likely to find the electron in an s orbital?
37. Where are periods and groups on the periodic table?
38. Where are the following found on the periodic table>
a. Metals
b. Non-metals
c. Transitional metals
d. Representative elements
e. Semi-metals
39. Write the electron configuration for the following:
a. O
b. N3c. Sr
d. Mg2+
40. Define the following trends:
a. Atomic radius
b. Ion radius
c. Electronegativity
d. Ionization energy
e. 2nd ionization energy
41. What are cations and anions? Which type of elements form each?
42. Write the ions formed by the following: State how many electrons were gained or lost.
a. F
b. Ca
c. H
d. S
e. Al
43. What is the octet rule?
44. What are some basic properties of ionic compounds?
45. What is the overall charge on any ionic compound?
46. What is a valence electron?
47. Use the criss-cross formula to correct the following ionic compounds: Name them after
solving.
a. AlO
b. HSO4
c. Fe(III)Cl
d. CaOH
48. Where are the diatomic molecules found? What kind of substance are they?
49. What are unshared electron pairs?
50. What are the charges on the ions that make up the following compounds (reverse crisscross)
a. Fe3O2
b. GaCl3
c. Pb2O4
51. Draw the Lewis for the following: Name, list its shape & hybrid orbital pattern
a. CH4
b. NH3
c. N2
d. H2O
e. PCl5
52. What are sigma bonds?
53. What are pi bonds?
54. What is VSEPR?
55. How is bond polarity determined?
56. List & define the intramolecular forces. Which is the strongest & weakest?
57. What substances have the following:
a. Suffix –ide
b. Suffix –ite & -ate
c. Siffix –ic & -ous
d. Prefix hydroe. Roman numerals
58. What is a binary compound?
59. What is a polyatomic ion compound?
60. Name the following acids:
a. HBr
b. H2SO4
61. What is an empirical formula?
62. What is a molecular formula?
63. What is a structural formula?
64. Solve the following:
a. Aluminum + Chlorine yield aluminum chloride + bromine
b. KClO3  KCl + O2
65. What are coefficients and what do the multiply?
66. What are subscripts and what do they multiply?
67. How does the activity series of metal determine the product of a single replacement
reaction?
68. Define the following reactions: Give an example of each
a. Direct combination
b. Decomposition
c. Single replacement
d. Double replacement
e. Combustion
69. Balance the following reactions:
a. N2 + H2  NH3
b. NaCl + F2  NaF + Cl2
c. AgNO3 + MgCl2  AgCl + Mg(NO3) 2
d. Ag2O  Ag + O2
e. C3H8 + O2  CO2 + H2O
70. Write a skeleton equation for the following reactions:
a. S8 + O2  (Combination)
b. Na + H2O  (Single Replacement)
c. FeCl3 + NaOH  (Double Replacement)
d. KClO3  (Decomposition)
e. CH4 + O2  (Combustion)
71. In the above reaction, NaCl + F2  NaF + Cl2, F is more or less reactive than Cl?
72. In the activity series of metals are the more reactive metals found on the top or the
bottom of the chart?
73. What conditions in the reactants must be present in order for a double-replacement to
take place?
74. What types of products are you likely to find in a double-replacement reaction?
75. How can you identify a Combustion reaction by the reactants and products?
76. What values in a chemical equation are used to calculate molar ratios between different
compounds?
77. What values are used to calculate molar ratios within a compound?
78. What is the name of the force that holds the nucleus together?
a. Which two atomic sub-particles are held together by this force?
79. Define the following nuclear reactions.
a. Fusion –
b. Fission 80. What does the law of conservation of mass say about nucleons involved in nuclear
reactions?
81. Compare the amount of energy released in nuclear reactions compared to the amount of
energy released in an average sized chemical reaction (combustion).
82. Define the following:
a. Parent isotope –
b. Daughter isotope c. Half-life –
83. Describe the following three types of radioactive decay.
a. Alpha –
b. Beta –
c. Gamma –
84. Describe the health consequences associated with each of the previous types of radiation.
a. Alpha –
b. Beta –
c. Gamma –