Study Guide – CHEM 1015
These are examples of skills you should have in preparing for exams! This list is not
exclusive. Please note that exam questions may ask you to apply several of these skills
within one question J
Chapter 1
1. Describe the scientific method
2. Describe the subatomic particles that make up an atom
3. Sketch a picture of an atom, labeling the nucleus
4. Understand that opposite charges cancel one another
5. Identify an atom from its atomic number (using periodic table)
6. Determine the chemical symbol of an element given its name or atomic
number
7. Identify the groups of the periodic table that contain halogens, alkali metals,
alkaline earth metals, chalcogens, and noble gases
8. Recognize that elements in the same group have similar properties
9. Identify an element as a metal, nonmetal, or metalloid using a periodic table
10. Identify an element as a main-group or transition element
11. Define isotope
12. Determine whether two atoms are isotopes of one another, given the number
of protons and neutrons present in each
13. Determine the isotope (nuclear) symbol for a given isotope of an element
14. Determine the number of protons, neutrons, and electrons in a given species
15. Calculate the atomic mass of an element given the abundance and masses of
its isotopes
16. Identify the isotope of higher abundance given a periodic table and the
masses of the element’s isotopes.
Chapter 2
1. Sketch the Bohr model of the atom
2. Recognize the relationship between n levels and energy
3. Define “excited state” in terms of the Bohr model of the hydrogen atom
4. Understand that transitions in an atom give off light of specific wavelengths
5. Differentiate between absorption and emission of light by an atom
6. Define the term “atomic orbital”
7. Describe the shapes of the s, p, and d orbitals
8. Describe the number of orbitals present in each sublevel of an atom
9. Identify the maximum number of electrons that could be present in each
sublevel
10. Identify legitimate combinations of level and sublevel (2s, 1p, 2d?)
11. Write the electron configuration for a given element
12. Draw the orbital diagram for a given element
13. Write the electron configuration for a given element, using a noble gas core
14. Identify the valence electrons present in a given atom or ion
15. Describe the atomic size trend of main-group elements
16. Arrange elements in order of increasing/decreasing atomic size
17. Arrange elements in order of increasing/decreasing ionization energy (ease
of losing electron)
18. Describe the metallic character trend of elements
19. Arrange elements in order of increasing/decreasing metallic character
20. Write the electron configuration for a main-group ion
21. Predict the charge on the ion formed from a main-group element
22. Draw the Lewis dot structure for a main-group atom or ion
23. Define anion and cation
Chapter 3
1. Describe the three states of matter and their properties
2. Differentiate between heterogeneous and homogeneous mixtures
3. Differentiate between chemical and physical properties
4. Determine the chemical formula for a binary ionic compound formed from
two given elements
5. Deduce the charge on the metal ion given an ionic compound formula
6. Determine the name of an ionic compound given the chemical formula
7. Recognize the presence in an ionic compound of a metal that forms more
than one ion
8. Determine the name of a binary molecular compound from its chemical
formula
9. Determine the chemical formula of a binary molecular compound from its
name
10. Determine whether a compound is ionic or molecular
11. Differentiate between ionic bonding and covalent bonding
12. Determine an empirical formula from a molecular formula
13. Determine a chemical formula given a molecular model
14. Write the name and chemical formula, including charge, of common
polyatomic ions
15. Recognize simple acids
16. Determine the name for an acid
17. Determine the chemical formula of an acid given its name
Chapter 4
1. Define base units in the SI system
2. Define metric prefixes and their abbreviations
3. Write the metric conversion factor between base unit and any other metric
prefix
4. Convert between the three temperature scales
5. Write a very small or very large number in scientific notation
6. Determine the number of significant figures in a given value
7. Determine the number of significant figures to report in a measurement
8. Determine the number of significant figures in the answer to a calculation
9. Round a given value to a smaller number of digits
10. Recognize the 4 different ways of writing the same metric conversion factor
11. Convert between any base unit and metric prefix
12. Convert between two metric units, neither of which is a base unit
13. Convert between nonmetric base units given relationship
14. Recognize the physical relationship (sink/float/suspend) between two
substances with different densities
15. Determine density from mass and volume
16. Convert between density, mass, and volume
17. Convert derived units into another set of units
18. Convert squared or cubed units into another set of squared or cubed units
Chapter 5
1. Define the mole and Avogadro’s number
2. Convert between moles of element and number of atoms
3. Determine the molar mass of an element or compound
4. Convert between mass, moles, and atoms of an element
5. Convert between mass, moles, and molecules (or formula units) of a
compound
6. Determine the number of atoms, mass, or moles of a specific element present
in a given mass or number of moles of a compound
7. Determine conversion factors between moles of substances using a chemical
formula
8. Determine the number of ions present in a given mass or number of moles of
an ionic compound
9. Determine the mass or number of moles of an ionic compound present with a
given number of ions
10. Determine the mass percent composition of a given compound
11. Determine an empirical formula given the mass percent composition of a
compound
12. Determine a molecular formula, given an empirical formula and molar mass
Chapter 6
1. Draw the Lewis structure of a diatomic molecule
2. Draw the Lewis structure of a simple molecule with a central atom
3. Draw the Lewis structure of a polyatomic ion
4. Draw a Lewis structure of a molecule that contains double or triple bonds
5. Recognize exceptions to the octet rule
6. Draw resonance structures when necessary
7. Determine electron geometry and molecular shape of a given compound
8. Define electronegativity
9. Arrange several elements in order of increasing/decreasing electronegativity
10. Determine whether a bond is polar or nonpolar
11. Determine whether a compound is polar or nonpolar
12. Arrange compounds in order of increasing/decreasing polarity
13. Determine bond angles in a compound
14. Arrange compounds in order of increasing/decreasing bond angle
Chapters 6-7 (these topics are introduced in Chapter 6 and applied in Chapter 7)
15. Define dispersion, dipole-dipole, and hydrogen bonding forces
16. Sketch dispersion, dipole-dipole, and hydrogen bonding forces between two
species
17. Determine the intermolecular forces present in a given compound
18. Arrange several substances in order of increasing/decreasing strength of
intermolecular forces
Chapter 7
1. Describe the differences between ionic, molecular, and atomic solids
2. Identify a substance as an ionic, molecular, or atomic solid
3. Describe the relationship between vapor pressure and intermolecular force
strength
4. Describe the relationship between boiling point and intermolecular force
strength
5. Describe the relationship between melting point and intermolecular force
strength
6. Describe the relationship between viscosity and intermolecular force
strength
7. Describe the relationship between surface tension and intermolecular force
strength
8. Describe the relationship between substances with similar or different types
of intermolecular forces
9. Arrange several substances in order of increasing/decreasing boiling point
10. Arrange several substances in order of increasing/decreasing melting point
11. Arrange several substances in order of increasing/decreasing vapor pressure
12. Arrange several substances in order of increasing/decreasing surface tension
13. Arrange several substances in order of increasing/decreasing viscosity
14. Write the chemical equation to describe a physical change: melting/freezing,
vaporizing/condensing, and sublimation/deposition
15. Describe the states of matter present at the boiling point/freezing
point/sublimation point
16. Draw a sketch to represent the physical change of an element or compound
Chapter 8
1. Describe Kinetic Molecular Theory and its four assumptions
2. Describe the physical properties of the gaseous state
3. List the common elements that exist as gases at room temperature
4. Define pressure
5. Convert between pressure units of atmospheres, torr, mmHg, and psi
(pounds per square inch)
6. State the ideal gas equation, including the value/units of the constant
7. Recognize the relationship between two variables in the ideal gas law,
keeping the other two constant
8. Solve for a variable in the ideal gas equation, given the other three
9. State the combined gas equation
10. Solve for one variable in the combined gas equation, given the remainder
11. Recognize STP (standard temperature and pressure) and its definition
12. Solve for molar mass or gas density, using the ideal gas equation
13. State Dalton’s law of partial pressure
14. Determine the partial pressure of one gas in a mixture of gases given mole
fraction and total pressure
15. Determine the partial pressure of one gas in a mixture of gases given mole
fraction and the pressure(s) of other gases in the mixture
16. Determine the partial pressure of one gas in a mixture of gases given moles,
temperature and volume
17. Draw a sketch before and after a change in the conditions of a gas sample
Chapter 9
1. Define a solution, including solute and solvent
2. Describe solubility in an aqueous solution
3. Describe the differences between unsaturated, saturated, and supersaturated
solutions
4. Draw a sketch to represent a saturated or supersaturated solution
5. Use the solubility chart to determine the solubility of an ionic compound in
water
6. State the percent by mass concentration equation
7. Determine the concentration of a solution in percent by mass
8. Determine the mass of solute present, given a mass of solution and the
concentration in percent by mass
9. State the molarity equation
10. Determine the concentration of a solution in molarity
11. Use molarity to either determine the volume of solution or moles of solute
12. Sketch two solutions with the same molarity, but different volumes
13. Determine the concentration of a stock solution from its volume and the
volume and concentration of a diluted solution
14. Determine the volume of a stock solution from its concentration and the
volume and concentration of a diluted solution
15. Determine the concentration of a diluted solution from its volume and the
volume and concentration of a stock solution
16. Determine the volume of a diluted solution from its concentration and the
volume and concentration of a stock solution
17. State the molality equation
18. Determine the concentration of a solution in molality
19. Use molality to determine mass of solution or moles of solute
20. Describe the difference between an electrolyte and nonelectrolyte
21. Sketch a solution composed of an ionic compound dissolved in water
22. Sketch a solution composed of a molecular compound (as a nonelectrolyte)
dissolved in water
23. Determine the molarity of a particular ion in solution, given the mass or
moles of ionic compound present
24. Determine the new molarity of a solution following dilution with water
25. Describe the impact on water’s freezing point, boiling point, or osmotic
pressure after addition of a solute
Chapter 10
1. Recognize when a chemical reaction has taken place
2. Select a sketch that represents a chemical reaction vs. a physical change
3. Write a chemical equation to represent a chemical reaction described in
words
4. Balance a chemical equation
5. Understand the symbols used in a chemical equation and identify reactants
and products
6. Use a solubility table to predict whether an ionic compound is aqueous or
solid
7. Classify a reaction as a precipitation, acid-base, gas-evolution, or oxidationreduction (redox) reaction
8. Recognize combustion reactions
9. Predict the products of a precipitation, acid-base, or gas-evolution
(producing) reaction
10. Predict whether or not a reaction will occur
11. Define neutralization reaction
12. Write a molecular, complete ionic, and net ionic equation for a precipitation
reaction
13. Write a molecular, complete ionic, and net ionic equation for an acid-base
reaction
14. Determine the oxidation number (state) of an element, alone, in a polyatomic
ion, or in a compound
15. Determine the substance undergoing oxidation in a given redox reaction
16. Determine the substance undergoing reduction in a given redox reaction
17. Recognize a gas-evolution (gas-producing) reaction involves the quick
decomposition of products H2SO3, NH4OH, H2CO3
18. Recognize that heat is a reactant or product in most reactions
Chapter 11
1. Write mole to mole conversion factors from a balanced chemical equation
2. Use a balanced chemical equation to determine moles of a reactant needed,
or product formed, from moles of one reactant or product
3. Use a balanced chemical equation to determine mass of a reactant needed, or
product formed, from moles or mass of a reactant or product
4. Define limiting reactant
5. Determine the limiting reactant when given moles, mass,
volume/concentration (solution), or pressure/volume/temperature (gas) of
two reactants
6. Define theoretical and actual yield
7. Determine the amount of remaining excess reactant, given moles, mass,
volume/concentration (solution), or pressure/volume/temperature (gas) of
two reactants
8. Determine percent yield given actual yield
9. Determine a volume of acid (or base) needed to neutralize a given quantity of
a base (or acid)
10. Determine the volume of a gas formed (or needed), given a chemical
equation and the conditions of the gas
11. Use a balanced thermochemical equation that includes heat of reaction to
determine the amount of heat energy needed (or given off) during a reaction
12. Use a balanced thermochemical equation to determine the moles or mass of a
reactant or product when a given amount of heat is released (or absorbed)
Chapter 12
1. Recognize Arrhenius acids and bases
2. Define Arrhenius acid, base and Bronsted acid, base
3. Define hydronium ion
4. Define conjugate acid-base pair
5. Identify a conjugate acid-base pair
6. Define the term amphoteric
7. Write a chemical equation to represent the autoionization of water
8. State the product of hydronium ion concentration and hydroxide ion
concentration in water at 25°C
9. Given either hydronium or hydroxide ion concentration, determine the other
10. Identify the strong acids
11. Identify the strong bases
12. Describe the properties of a strong acid using a chemical equation
13. Calculate [OH–] or [H3O+] given the concentration of either a strong acid or
strong base
14. State the pH equation – the relationship between pH and [H3O+]
15. Calculate pH given the concentration of either a strong acid or strong base
16. Determine [H3O+] from pH
17. Describe the difference between a strong acid and weak acid
18. Describe the difference between a strong base and weak base
19. Illustrate the behavior of a strong acid in water
20. Illustrate the behavior of a weak acid in water
21. Illustrate the behavior of a strong base in water
22. Illustrate the behavior of a weak base in water
23. Estimate the pH value of a weak acid or weak base solution
24. Define the terms titration and equivalence point
25. Calculate the concentration of an unknown acid or base, given titration data
26. Describe a buffer and how it works
27. Recognize solutions that exhibit buffer properties
Chapter 16
1. Describe alpha, beta, and gamma radioactivity
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Differentiate between chemical and nuclear reactions
Write nuclide symbols for atoms and subatomic particles
Balance nuclear equations
Write a balanced nuclear equation for a given radioactive process
Describe the relationship between radioactive decay and ionizing power
Describe the relationship between radioactive decay and penetrating power
Arrange radioactive decay in order of increasing/decreasing ionizing power
Arrange radioactive decay in order of increasing/decreasing penetrating
power
10. Describe the process defined by half-life
11. Calculate the amount of product present after a given number of half-lives
12. Calculate the amount of starting material present after a given number of
half-lives
13. Describe nuclear fission
14. Describe nuclear fusion