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Chemistry
NYOS Secondary School
End of Year-Final Exam Learning Objectives
Dr. McPhee
Unit: Metric Conversions, Classification of Matter, Atomic Theory
1. understand metric units for measurement of length, mass, and volume, as well as, the meaning of prefixes
for scale (i.e., ‘kilo’ means thousand)
2. know the formula for determining density and the units of density
3. be able to convert from one metric unit to another (i.e., gram to milligram and vice versa)
4. convert a number into scientific notation to determine the number of significant figures
5. know the difference between intensive and extensive properties and give examples of each
6. know the difference between chemical and physical changes and give examples of each
7. Know the roles of these scientists in the development of historical and current models of the composition
of matter and models of the atom: Dalton, Rutherford, Thomson, Chadwick, Mendeleev, Einstein
Unit: Periodic Table Families; Element Properties; Electronic Configuration; Electromagnetic
Spectrum
8. know which materials are elements by name (eg, copper vs bronze) and know the location of these families
of the periodic table: alkali metal, alkaline earth, rare earth, coinage metal, halogen, noble gas
9. understand the difference between mixtures and pure substances; understand the differences between
homogeneous and heterogeneous mixtures
10. know the location, mass and charge of these subatomic particles (and the names of the scientists who
discovered them): electron, neutron, proton
11. understand how elements can be the same yet be different isotopes (what subatomic particle makes
them different?)
12. be able to determine the number of electrons associated with an ion given its shorthand notation
(e.g., Ni4+ )
13. be able to determine the number of protons, neutrons and electrons of a neutral atom given the name of
the element and its atomic mass (e.g., Cl37)
14. know the symbols associated with elements whose names don’t match their symbols, especially these:
Na, K, Fe, Cu, Ag, Au, Pb, Sn, As, W, Hg
15. understand the physical properties associated with metals (e.g., conductor of electricity)
16. understand the physical properties associated with non-metals (e.g., usually brittle)
17. given any element, be able to identify it is a metal, non-metal or metalloid
18. know the meaning of and the periodic trends for these: atomic radius, electron affinity, ionization energy,
electronegativity
19. when forming ions (i.e., cations or anions), know which ions metals usually form and which ions nonmetals usually form
20. understand which parts of the electromagnetic spectrum are high energy/high frequency/short
wavelength and which are considered low energy/low frequency/long wavelength
21. know how to use an Aufbau chart (along with Hund’s rule and the Pauli exclusion principle) and
suborbital notation (parentheses and arrows) to indicate the electron configuration (or noble gas shorthand notation) for a given atom
22. know the shapes and maximum number of electrons that can be placed into these orbitals: s, p, d, f
23. know which orbitals can be found on any given energy level
Unit: Ionic and Covalent Compounds: Names, Formulas, Properties/Reactions and Molecular Shapes
24. know the charges commonly found for ions in these families: alkali metal, alkaline earth, nitrogen family,
oxygen family, halogens; know the charges for silver, zinc and aluminum
25. given a metal and non-metal from one of the families listed above, be able to predict the formula of its
ionic compound
26. be able to list properties of ionic compounds
27. know that bonding between elements ultimately involves ELECTRONS
28. be able to use a polyatomic sheet to give the formula from a name of an ionic compound, and vice versa
29. understand the definition of valence electrons and how these form bonds between metals (i.e., metallic
bonding)
30. know which metals need Roman numerals in the names for their ionic compounds and be able to work
from a formula back to a name containing a Roman numeral
31. understand the nature of covalent bonding that holds together non-metal atoms
32. be able to name covalent compounds given a name and vice versa
33. given either a name or formula for a covalent compound, be able to calculate the number of valence
electrons
34. given a molecular formula, be able to determine the molecular shape for a molecule or ion [you will have
your molecular shape sheet]
35. given a Lewis structure, be able to compute the formal charge for an atom
36. know which elements are found in nature as diatomic molecules (e.g., H2)
37. given a chemical reaction, be able to state whether it is one of the following: synthesis, decomposition,
single replacement, double replacement, combustion or acid base reaction
38. given words or symbols for reactants and products, be able to balance a chemical reaction in order to
state the number of coefficients in front any species
39. know the products of these common reactions:
a. metal + acid
b. metal carbonate + acid
Unit: Stoichiometry; Properties of Solutions and Their Equations
40. be able to compute a Formula Weight from a named compound or a given chemical formula
41. be able to calculate the moles of an element or compound given its mass in grams either its atomic
weight [for elements] or formula weight [for compounds]
42. Be able to use stoichiometry to calculate the mass in grams of a product given a balanced equation.
43. Be able to calculate a percent yield (% yield) given an actual yield and a theoretical yield.
44. Be able to calculate mass percent for an element given a formula [eg % C by mass in CH4]
45. Know how to distinguish between an molecular formula and an empirical formula
46. Be able to calculate average atomic mass given isotopic masses and abundances
47. Be able to calculate the density of a gas at STP given a molecular formula; (what ratio is important here?)
48. Know the definitions of the concentration terms molarity and molality
49. Know how to use the dilution formula to calculate final volume or final molarity
50. Understand which component is the solute and which is the solvent in a word problem; together these
make a solution
51. Understand how to distinguish between an electrolyte and non-electrolyte [via conduct of electricity]
52. Have a working definition for each of these: unsaturated, saturated, super-saturated
Unit: Thermodynamics
53. Know the names of ALL phase transitions (example: gas to solid is called deposition)
54. Be able to describe the terms endothermic and exothermic in terms of heat transfer
55. Know that heat flow at constant pressure, qp, is equal to mC∆T where m = mass in grams and C is the
specific heat
56. Know the definitions of these symbols: G, H, S and the definitions of the 1st and 2nd Laws of
Thermodynamics
57. Know that spontaneity has nothing to do the speed of a reaction
58. Understand what the sign (negative or positive) means for ∆H, ∆S or ∆G
59. Know which type of calorimeter (coffee cup or bomb) is used when pressure or volume are held constant
60. Be able to calculate ∆G using the Gibbs Free Energy Equation (what unit does T have to be in?)
61. Know that bond formation is exothermic and bond breaking is endothermic—be able to decide which is
which given a balanced equation and/or chemical structures
62. Know that heat flow at constant pressure, qp, is equal to mC∆T where m = mass in grams and C is the
specific heat
63. Know the properties of water that make it unique: density, high specific heat, polar molecule, high
melting and boiling point due to H bonding, high surface tension, low vapor pressure
64. be able to state the van’t Hoff factor (i), given a molecular formula
65. Be able to calculate ∆T (temperature change) given kb or kf and the molality and molecular formula of a
solute
Unit: Acids and Bases; Redox Reactions; Gas Laws
66. Know the definitions of Arrhenius and Bronsted-Lowry acids and bases and be able to classify a substance
as one or more of these based on its dissociation reaction
67. Know what pH means and where acids and bases appear on the pH scale
68. Be able to use the pH equation to calculate pH from hydrogen ion concentration [H+]
69. Know that protons actually exist as hydronium ions in solution
70. Know the products of these reactions:
 an acid and an Arrhenius base
 an acid and a metal above Hydrogen in the activity series
 an acid and a metal carbonate
71. Be able to assign oxidation numbers to any atom in a compound, element or ion
72. Be able tell if the atom has undergone an oxidation, reduction or neither
73. Be able to identify the oxidizing or reducing agent
74. Know the common name of a galvanic cell and what electrical potential is called
75. Understand the relationship between and sign of E (cell voltage) and ∆G
76. Know which gas law name goes with which variable (example: P and V goes with Boyle)
77. Be able to solve word problems using the various gas laws, including the combined gas law and PV=nRT
[recall that T must always be in Kelvin and TK = TC + 273 and that R = 0.0821]
78. Know what STP stands for and what is the value of T and P in degrees Celsius or Kelvin (for T) and in torr
or atm (for P)
Unit: Kinetics; Nuclear Chemistry; Chemical Equilibria
79. Know that the speed of a reaction depends does NOT depend on the change in enthalpy (∆H;
endothermic or exothermic) or change in Gibbs Free Energy (∆G; spontaneous or non-spontaneous)—it
ONLY depends on the height of the activation barrier (Ea)
80. Know at least three ways to increase the rate of a reaction (temperature, surface area and concentration)
81. Given a diagram of enthalpy (H) versus time, be able to calculate ∆H and Ea
82. Given a multistep process containing a fast step and a slow step, know which step is the rate determining
step (rds)
83. Know the symbols of the following types of radiation: alpha, beta, positron, and gamma
84. Understand that matter can be converted to Energy by either fission or fusion processes and this energy
is given by the equation E=mc2 [note: m must be in kilograms; E will come out in Joules]
85. Given a nuclear reaction, be able to determine the missing particle (alpha, beta or positron) that balances
the equation
86. Know how severe each type of radiation is to living cells (which is the most dangerous?)
87. Be able to determine the amount of material remaining in a radioactive sample after a specified number
of half-lives
88. Possess a working definition of the idea of a dynamic equilibrium
89. Know which factor affects the size of Keq (temperature) and which do not (concentration, catalysts)
90. Given a balanced equation, be able to construct an expression for Keq (what 3 things should you
remember in order to do this?)
91. Be able to apply Le Chatelier’s principle to predict the direction of a reaction (forward or backward) upon
application of any of these three stresses: pressure, temperature or a change in concentration
92. Given values of Q and K, be able to predict if a reaction will go in the forward or backward direction to reestablish equilibrium