HONORS CHEMISTRY
MIDTERM EXAM REVIEW SHEET
The midterm exam will cover all material from day 1 of class. Below you will find information that
should help you review for the test. As usual, if you need assistance or guidance just let me know. You
will be provided with a periodic table. You may prepare a 4x6 notecard to use during the test, which you
will surrender at the end of your exam period. For your reference, a copy of the ion list is also available
on my teacher website.
CHEMISTRY BASICS (Chapters 3, 4)
1. Classify matter as: homogenous vs. heterogeneous, pure vs. impure, element vs. compound, metal
vs. nonmetal
2. Distinguish between compounds and mixtures and list characteristics of each
3. Differentiate among the three states of matter
4. Explain the difference between a physical and chemical properties and physical and chemical
changes
5. List four indicators of a chemical reaction
6. Apply the law of conservation of mass, law of definite proportions, and law of multiple
proportions
7. Trace the history of atomic models (Dalton, Rutherford, JJ Thomson) and associated experiments
8. Describe the structure of the atom in terms of the subatomic particles: protons, neutrons, &
electrons
9. Interpret and write symbols involving atomic number, mass number, average atomic mass, and
isotopes
10. Identify the following about elements by looking at the periodic table: atomic number, mass
number, # of protons, neutrons & electrons, anion, cation, most common isotope, etc.
11. Define isotope
12. Calculate the average atomic mass of an element from isotope data
ELECTRONS IN ATOMS/PERIODICITY (Chapters 5, 6)
1. Describe the Bohr model of the atom
2. Write electron configurations(shorthand and long version)
3. Apply the Aufbau principle, the Pauli exclusion principle, and Hund’s rule in writing the electron
configurations of elements
4. Explain how the wavelengths of light emitted by an atom provide information about electron
energy levels
5. List sublevels (s, p, d, f), number of orbitals per sublevel, and number of electrons per sublevel
6. Review the organization of the periodic table based on configurations (s-block, p-block, d-block,
f-block)
7. Calculate wavelength, frequency, or energy of light (c= λ v, E=hv, c = 3 x108 m/s, h=6.6262 x 1034 J x s)
8. Describe atomic emission spectrum
9. Distinguish between the Balmer series, Lyman series, and Paschen series
10. Explain the Heisenberg uncertainty principle
11. List the common properties of metals, nonmetals, and metalloids
12. Identify important groups on the periodic table (representative elements, alkali metals, alkaline
earth metals, noble gases, halogens, transition metals, etc)
13. Describe the historical development of the periodic table by Mendeleev and Mosley
14. Describe the arrangement of the modern periodic table according to periodic law
15. Explain why you can infer the properties of an element based on those of other elements in the
periodic table.
16. Use electron configurations to classify elements as noble gases, representative elements, transition
metals, or inner transition metals.
17. Define and interpret group trends and periodic trends in the periodic table (including ionization
energy, atomic radius, electronegativity, and ionic radius)
18. Distinguish between a quantum and a photon
19. Draw electron dot structures for atoms
20. State the octet rule
IONIC AND COVALENT BONDING (Chapters 7, 8)
1. Identify the seven diatomic molecules
2. Describe the type of atoms that form ionic vs. covalent bonds
3. Differentiate between single, double, and triple covalent bonds
4. List properties of ionic/covalent compounds(including boiling & melting points, conductivity,
solubility, etc)
5. Relate the electron configuration of an atom to its reactivity
6. Determine number of valence electrons, and use the octet rule to predict what stable ions the atom
is likely to form
7. Use electronegativity values to determine bond type
8. Use dot models to determine polarity
9. Explain the difference between polar and nonpolar covalent bonds(in terms of electron sharing)
10. Use the periodic table to determine the number of valence electrons in an atom and draw its
electron dot model
11. Draw electron dot models for molecules and polyatomic ions
12. Describe the formation of cations from metals and of anions from nonmetals
13. Identify and describe a dipole.
14. Use VSEPR to predict the shapes of simple covalently bonded molecules including bond angle
15. Use the periodic table to determine the charge of an ion
16. Explain the difference between a monatomic and polyatomic ion.
17. Apply the rules for naming and writing formulas for binary ionic and ternary ionic compounds
18. Apply the rules for naming and writing formulas for binary molecular formulas
CHEMICAL REACTIONS (Chapter 9)
1. Identify the 5 types of chemical reactions when provided a chemical reaction (composition,
decomposition, single replacement, double replacement, and combustion).
2. Balance chemical reactions when provided an unbalanced equation
3. Define chemical reaction, products and reactants
MAKE SURE TO REVIEW ALL OLD TESTS, QUIZZES, AND LABS!!