Download PAP Chemistry - Fall Final Review

PAP Chemistry - Fall Final Review
Chapter 1 (Matter) & 2 (Measurements)
1. Be able to determine the number of significant figures present in a given number
a. 0.00203
b. 123
c. 100
d. 100.
e. 100.050
2. 7.65 * 2 = (with correct s.f.)
3. 2.30 + 3.225 = (with correct s.f.)
Chapter 3 (Atoms)
4. Define atom, nucleus, electron, neutron, proton
5. What did Rutherford discover from the Gold Foil Experiment
6. When is a bright-line spectrum produced by an atom? IE – How does an atom give off
color (especially when burned)?
7. Use the mass number and atomic number to determine the element and its number of
protons, electrons, and neutrons
8. Be able to determine the atomic number and mass number of an element when the
number of protons, neutrons, and electrons is specified
9. Determine the number of protons, electrons, and neutrons in the following isotopes:
a. sodium-23
b. calcium-40
c. Cu
d. Ag
10. How does mass number relate to number of protons when talking about isotopes?
Chapters 4 (Electrons in Atoms) & 5 (Periodic Law)
11. How many electrons are held is each quantum sublevel (s, p, d, f)
12. Understand groups vs. periods
13. Write electron configurations and orbital filling diagrams (including energy level,
sublevels, and orbitals for any element)
14. Be able to locate the alkaline earth, alkali metals, noble gases, and halogens
15. Periodic Trends – know atomic radius, electronegatitivity, ionization energy, ionic radius
and how they compare
16. What is the octet rule? What orbitals (s,p,d,f) must be filled for it to be satisified?
17. What is the general electron configuration for a noble gas? (s, p, d, f)
18. Write the electron configuration for the following
a. carbon
b. neon
c. sulfur
d. potassium
e. vanadium
Chapter 6 (Chemical Bonding)
19. What is VSEPR? Define. What is it used for?
20. Draw the structure for H2O and determine the number of electrons that are shown.
21. Draw the structure for OH22. Draw the Lewis Structure for NH4+
23.
24.
25.
26.
27.
Draw the Lewis Structure for PO43What is the shape of H2O?
Know what tetrahedral, linear, and bent shapes look like
Understand covalent vs. ionic bonds; know the difference
Understand polar vs. nonpolar and be able to determine the polarity of various
compounds
Chapter 7 (Formulas and Compounds)
28. Be able to name compounds
a. Pb3(PO4)2
b. NaF
c. C2O
d. H2SO4
e. HF
f. FeP
29. Write formulas for the following:
a. magnesium hydroxide
b. calcium sulfide
c. iron (III) oxide
30. Be able to convert between gramsmolesatoms.
a. How many grams of Al2S3 are in 2.00 moles of Al2S3?
b. How many atoms are found in 1.00 moles of Na?
c. How many atoms are found in 1.00 moles of NaF?
31. What is Avogadro’s Number?
32. How many atoms are in 1 mole of each element? Does this number change?
33. Be able to do mol-mass conversions
34. Determine the mass in grams of the following:
a. 2.00 mol N
b. 3.01 x 1023 atoms Cl
35. Determine the amount of moles of the following:
a. 12.15 g Mg
b. 1.50 x 1023 atoms F
36. Determine the number of atoms present in a 251.2 g sample of manganese.
37. What is the oxidation number of C in CO2?
38. What is % composition?
39. Determine the % composition of NaCl.
40. Determine the % composition of magnesium chloride.
41. What is empirical and molecular formula?
42. Be able to determine the empirical formula.
a. What is the empirical formula for a compound that is found to contain 63.52% iron
and 36.48% sulfur?
43. Given the empirical formula and a molar mass, be able to determine the molecular
formula.
a. The empirical formula is CH5. Its formula mass is 85.0 g/mol. What is the molecular
formula?
Chapter 8 (Rxns)
44. What is a precipitate?
45. Understand and apply the Law of Conservation of Mass.
46. When is a chemical equation balanced?
47. What is a subscript? What is a coefficient? Where are the products and reactants located
in a chemical reaction?
48. Be able to balance chemical equations.
a. Al4C3 + H2O  CH4 + Al(OH)3
b. How many moles of hydrogen ions are present in Al(OH)3
c. How many moles of oxygen atoms are present in Ca3(PO4)2
49. Be able to recognize a synthesis reaction, a single replacement reaction, a double
replacement reaction, and a decomposition reaction.
50. When a double replacement reaction produces a precipitate, what happened?
51. What products are formed when Lithium metal reacts with water?
52. Given solubility rules, be able to determine what products will form precipitates
Ch.14 – Net Ionic Equations
63. Write 1 net ionic reaction
a. solutions of potassium sulfate and barium nitrate are combined.
b. solutions of zinc nitrate and ammonium sulfide are combined.