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Use the units of the metric system and convert them.
Use significant figures.
Use scientific notation doing calculations.
Use dimensional analysis in solving problems.
Define, use, and measure mass, volume, density, temperature, and heat
Describe the characteristics of elements, compounds, and mixtures.
Use molecular concepts to explain the three states of matter and their
transitions
8. Apply the Law of Constant Composition.
9. Describe a model of the atom in terms of its subatomic parts.
10. Identify main group, transition elements, metals, nonmetals, and metalloids
11. Correlate the arrangement of the periodic table with the electron
configurations of the valence shells of the elements.
12. Describe the relation between the octet rule and the formation of ions.
13. Predict the formulae of binary ionic compounds.
14. Correctly name ionic compounds.
15. Correctly name covalent compounds.
16. Write a chemical reaction as an equation.
17. Balance a chemical equation.
18. Apply the Law of Conservation of Mass.
19. Explain molecular characteristics necessary for solution formation.
20. Calculate the percent composition of a compound.
21. Define and use atomic mass in calculation
22. Calculate the formula mass of a compound.
23. Use the mole as a conversion factor to convert mass to mole and mole to
mass.
24. Apply Avogadro’s number to estimate the number and magnitude of atoms
and molecules.
25. Calculate the empirical and molecular formulae of a compound.
26. Calculate the percent composition of a compound.
27. Define and use atomic mass in calculation
28. Use a balanced chemical equation to predict the amount of compounds
produced and use in a chemical process.
29. Use gas pressure units them in calculations.
30. Summarize the gas laws, including the Ideal Gas Law.
31. Apply the appropriate gas laws to particular experimental conditions.
32. Describe the properties of mixtures of gases using Dalton’s Law.
33. Use the gas laws to determine molecular mass.
34. Determine the amount of gas dissolved in a liquid using Henry's Law
35. Apply the mole and molar mass concepts to gases, liquids, and solids
36. Describe the octet rule. Describe shape of orbitals.
37. Use Lewis symbols to represent elements and chemical reactions.
38. Describe the difference between ionic and covalent bonds.
39. Create and apply Lewis structures for compounds.
40. Describe the difference between polar and non-polar covalent bonds.
41. Use VSEPR theory to predict molecular shape.
42. Use Lewis symbols to represent elements and chemical reactions.
43. Describe the relation between the octet rule and the formation of ions.
44. Apply the mole and molar mass concepts to gases, liquids, and solids
45. Describe secondary forces and correlate chemical structure with types of
forces.
46. Correlate physical properties such as VP, BP, MP, and surface tension with
secondary forces.
47. Explain molecular processes associated with Vapor Pressure.
48. Explain the molecular characteristics of solids.
49. Describe how molecular properties effect the formation of a solution (solute
vs. solvent)
50. Give the quantitative definitions of concentration and use them as conversion
factors in calculations (molarity and %v/v, w/w, and w/v)
51. Specify reasons and methods for preparing dilute solutions from
concentrated solutions.
52. Explain molecular characteristics necessary for solution formation.
53. Describe how the concentrations of acids and bases may be determined by
titration. (Molarity)
54. Describe diffusion and the characteristics of semi-permeable membranes in a
solution.
55. Describe the origin of osmotic pressure.
56. Describe the properties of macromolecules.
57. Describe the central role of water in acid-base chemistry.
58. Explain the difference between strong and weak acids and strong and weak
bases.
59. Use the ion product of water to calculate the hydronium ion and hydroxide
ion concentrations.
60. Define pH and describe its use as a measure of acidity.
61. Describe the behavior of strong acid solution from its measured pH.
62. Use the Bronsted-Lowry theory to explain the properties of salts of weak
acids, bases and buffers.
63. Apply dynamic equilibrium concepts to problems
64. Describe how the rates of reactions are affected by the concentrations of
reactants, the temperature and presence of a catalyst.
65. Describe how complex chemical reactions are result of collisions that lead to
the formation and decay of an activated complex.
66. Explain how a chemical system reaches a state of dynamic equilibrium.
67. Describe how chemical systems respond to stresses (LeChatelier’s principle).
68. Describe how equilibrium constant provides a quantitative description of
chemical equilibrium.
69. These chapters are NOT part of the UF Grade:
70. Describe and understand metal-nonmetal oxidation-reduction reactions
71. Explain how to apply oxidation states and apply them.
72. Identify oxidizing and reducing agents
73. Balance oxidation-reduction reactions
74. Describe the types of bonds formed by the carbon atom
75. Explain the bonding and characteristics of alkanes, alkenes, and alkynes
76. Describe and draw structural isomers.
77. Name and draw hydrocarbons and structural hydrocarbons
78. Describe reactions of alkanes (substitution, addition)
79. Explain structure, names, bonding, uses and characteristics of aromatic
hydrocarbons, alcohols, aldehydes, ketones, carboxylic acids and polymers