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Chemistry Final Exam Study Guide
First Semester :
1. What is density? How is density calculated?
2. What are the steps of the scientific method?
3. What is a quantum of energy?
4. What is matter?
5. What is the difference between heterogeneous
and homogeneous mixtures?
6. What are the contributions of Bohr, Heisenberg,
Dalton, Thompson, & Rutherford to atomic
theory?
7. Calculate the number of protons, neutrons &
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electrons of a given element: 20 Ca+2
What does a chemical formula tell you about a
molecule?
What is the difference between physical &
chemical changes?
What are the properties of the four states of
matter: solid, liquid, gas and plasma?
What are the properties of the alkali metals
group?
What causes a substance to move from one
state of matter to another?
What are the laws of Conservation of Mass and
Conservation of Energy?
What are the parts of the atom? Where are they
located? What are their charges?
What keeps the nucleus of an atom together?
Define ground state and excited state.
How is the energy of an electron calculated?
What are the different categories of matter?
What are isotopes & how are they written?
How did Rutherford find the nucleus of the
atom?
What is mass number? Atomic number?
Average atomic mass?
What is the difference between physical &
chemical properties?
What is wavelength & frequency?
What is a quantum of energy?
What are the signs of a chemical change?
What do each of the following measure: mass,
volume, density, length, temperature?
Convert nm to meters.
How did JJ Thompson discover the electron?
Know the names of each group on the periodic
table.
What is the strong nuclear force?
What are the properties of the alkaline-earth
metal group?
What are the properties of the halogen group?
Why was Democritus’ Atomic theory discarded
for 2000 years?
What is the Planetary Model of the Atom? Who
invented it?
What is an independent variable? Dependent
variable? Control?
What is an orbital?
37. What are the characteristic properties of metals?
Nonmetals? Metalloids?
38. What are the main points of Dalton’s atomic
theory?
39. What are the properties noble gasses?
40. What are the vertical columns on the periodic
table called?
41. What are the horizontal rows on the periodic
table called?
42. What is quantitative data? What is qualitative
data?
43. What is in the nucleus of an atom?
44. Write the orbital diagram & electron
configurations for the following elements: K, Ar,
H, He, Br
45. Define precision and accuracy.
46. What determines an element’s order on the
periodic table?
47. What happens to the temperature of a
substance as it is changing states?
48. What is kinetic energy?
49. Why is an atom electrically neutral even though
it contains charged particles?
50. How are a Na atom and a Na+1 ion different?
51. What is the difference between a pure
substance and a mixture?
52. What is the chemical formula of water?
53. How many orbitals are in each energy level?
54. Convert mL to cm3.
55. When does an electron emit light?
Chapter 6
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Identify the different parts of Periodic Table
Define and know the trend for ionization energy
Define and know the trends in atomic/ionic radius
Define and know the trends in electronegativity
Chapter 7
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Understand Bond polarity (intramolecular forces) vs.
molecular polarity (intermolecular forces)
Bond types vs. electron transfer/share, based on
elements involved
Understand the octet rule
Bond types vs. properties of compounds
IMFs in samples of different types of compounds
Second Semester:
Students should be able to:
Chapter 9
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Write formulas for compounds given the name.
Name a compound from a given formula.
Given formula, determine placement of unknown element on P.T.
Determine oxidation number of elements in a cpd; in polyatomic ion
Chapter 11
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Balance equations
Identify types of chemical reactions
Describe chemical reactions in terms of reactant products and all symbols
Use Activity Series to predict outcome of single replacement reactions
Chapter 10 & 12
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Meaning of mole ratios
Mole  mole stoichiometry
Mole  mass stoichiometry
Mass  mole stoichiometry
Mass  mass stoichiometry
Calculations of limiting and excess reactant
% yield calculation
Chapter 13
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Assumptions of the Kinetic-Molecular Theory
Properties of liquids and solids as it relates to Kinetic Molecular Theory
Relationship of temperature and average kinetic energy
Phase diagram – identify important points & know definitions (critical point, triple point, normal boiling & melting point, etc.)
Phase diagram – determine state(s) of matter at certain temperature and pressure
Heating curve vs. state of matter
Chapter 14
 Conditions when gases behave most/least ideally
 Combined gas law problem
 Ideal gas equation problem
 Volume  volume stoichiometry