Chemistry I Honors – Final Exam Study Guide 2014-2015
Chapter 1 – Matter and Change:
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Physical vs chemical properties
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Physical vs chemical changes
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Particle model of gas/liquid/solid states of matter
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Law of Conservation of Energy
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Mixture vs pure substance
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Distinguish elements, compounds, mixtures
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Element names and symbols
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Arrangement of periodic table
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Methods for separating mixtures (filter, distill)
Chapter 2 – Measurements and Calculations
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Scientific method – steps
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Qualitative vs quantitative observations
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Metric units for length, mass, time, volume, and
density – also Metric unit conversions
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Density calculations
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Accuracy vs precision
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Significant figures – rules for math operations
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Scientific notation – be able to use it
Chapter 3 – Atoms – Building Blocks of Matter
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Dalton’s Atomic theory
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Laws of Conservation of Mass, Definite Proportions,
Multiple Proportions
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Rutherford’s experiment
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Properties of protons, neutrons, electrons
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Isotopes-use isotope masses and percent
abundances to calculate average atomic mass

Atomic number and mass number – how they are
related

Determine the number of protons, neutrons, and
electrons in a nuclide given its symbol
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Define ‘mole’ , Avogadro’s number, molar mass
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Convert between mass, moles, and
number of particles (atoms or molecules)
Chapter 4 – Arrangement of Electrons in Atoms
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Bohr model of the hydrogen atoms – basic ideas
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What causes atomic line (absorption and emission)
spectra
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Electromagnetic spectrum – relationships between
energy, frequency, and wavelength

Quantum model of the atom
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Orbitals and quantum numbers
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Write electron configurations for atoms and ions

Identify elements from their electron configuration
(either electron configuration notation or orbital notation)
Chapter 5 – The Periodic Law

Describe how elements of a group are related
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Relationship between electron configuration and
the structure of the Periodic table.

Name 4 blocks of the periodic table
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Periodic trends in atomic radius, ionization energy,
electron affinity, and electronegativity

Define valence electrons and state the number
present in atoms of each main group element

Know the common group/family names and typical
properties for elements of Groups 1, 2, 17, and 18.
Chapter 6 – Chemical Bonding

Distinguish between ionic and covalent bonding

Classify bond type by electronegativity differences
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Write Lewis electron dot structures
Describe the differences in bond length and bond
energy in single, double, and triple bonds
Describe the electron-sea model of metallic bonding
and relate to properties of metals
Predict shapes and polarities of molecules and ions
using VSEPR theory
Discuss the types of intermolecular forces and relate
them to physical properties
Chapter 7 – Chemical Formulas and Chemical Compounds

Write formulas for ionic compounds and name them
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Name binary molecular compounds using prefixes
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Write the formula of binary molecular compounds
given the name

Give oxidation numbers for each element in a
compound or ion.

Calculate molar mass for a given compound.

Calculate mass percent of an element in a given
compound

Convert between mass, moles, and number of
particles

Define empirical formula and explain the relationship
between the empirical formula and the molecular
formula of a compound

Calculate empirical formula from percent composition

Calculate molecular formula from percent
composition and molar mass
Chapter 8 – Chemical Equations and Reactions

List observations that indicate a chemical reaction is
occurring

Balance formula equations by inspection

List the five types of chemical reactions and classify a
given reaction according to type

Use an activity series and/or a solubility table to
predict whether a given reaction will occur and predict
the probably products formed.
Chapter 9 – Stoichiometry

Define stoichiometry

Write a mole ratio relating two substances in a
chemical equation

Determine the amount (grams or moles) of product
formed from a given amount (grams or moles) of
reactant

Calculate percentage yield, given theoretical yield and
actual yield.
Chapter 10 – States of Matter

State the kinetic-molecular theory of matter and
describe how it explains macroscopic properties of a
gas.

Describe the motion of particles in liquids and solids,
and the properties of liquids and solids according to
the kinetic-molecular theory.

Discuss changes of state as equilibrium processes

Interpret phase diagrams

Define vapor pressure and explain its relationship to
state changes

Describe the structure of a water molecule and its
relationship to the physical properties of water
Chapter 11 - Gases

Define ‘pressure’, know units of pressure, use
Dalton’s Law of partial pressures to calculate partial
pressure, total pressure, and mole fraction of gases in
a mixture.

Know Avogadro’s Law and use it to compare
properties of different samples of gases.

Know the standard conditions of temperature and
pressure used in gas law problems.

Use kinetic-molecular theory to explain relationships
between gas volume, temperature, and pressure.

Use the ideal gas law to calculate pressure, volume,
temperature, or moles of gas when the other three
quantities are known.

Define ‘standard molar volume’ and use it to calculate
gas masses and volumes.
Chapter 12 - Solutions

Distinguish between electrolytes and nonelectrolytes

Explain solution equilibrium and distinguish between
saturated, unsaturated, and supersaturated solutions

Explain the meaning of ‘like dissolves like” in terms of
polar and nonpolar substances

Perform calculations related to solution concentration
(e.g. molarity, molality, and dilutions)
Chapter 13 – Ions in Aqueous Solutions and Colligative
Properties

Write equations for the dissolution of soluble ionic
compounds in water
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Distinguish between strong and weak electrolytes
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Predict whether a precipitate will form when solutions
of soluble ionic compounds are combined, and write
net ionic equations for precipitation reactions.

Calculate freezing point depression, boiling point
elevation, and solution molality of nonelectrolyte and
electrolyte solutions.
Chapter 14 – Acids and Bases

List properties of aqueous acids and bases, and
identify Arrhenius and Bronsed-Lowry acids/bases.

Name common binary acids and oxoacids

Explain the difference between strong and weak acids
and bases.

Define a conjugate acid, a conjugate base, and an
amphoteric compound

Give the products of an acid-base neutralization
reaction
Chapter 15 – Acid-Base Titration and pH

Write the equilibrium equation for the self-ionization of
water

Define pH and explain the pH scale.

Identify the most acidic or most basic solution from a
list, given pH or [OH-] or [ H3O+].
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Perform calculations relating pH and pOH to [H3O]+
and [OH] –

Explain how to perform an acid-base titration and how
an indicator works

Calculate solution molarity from titration data
Chapter 16 – Reaction Energy
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Distinguish ‘heat’ and its units from ‘temperature’ and
its units.
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Perform specific heat calculations (choose the best
material for heat storage based on Specific.Heat values)
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Explain enthalpy change, enthalpy of reaction,
enthalpy of formation, and enthalpy of combustion
Calculate the heat released or absorbed for a given
reaction, given the ΔH and amounts of reactants
Distinguish exothermic from endothermic chemical
reactions and changes of state
Explain enthalpy, entropy, and free energy, and their
relationship to the driving force for reactions to occur
Chapter 17 – Reaction Kinetics
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Explain the concept of a reaction mechanism

Define activated complex
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Relate activation energy to enthalpy of reaction

Discuss the factors that affect reaction rate.

Define ‘chemical kinetics’ and explain the two
conditions necessary for a reaction to occur.

Define ‘catalyst’, explain how a catalyst works to
speed up the reaction. Give examples of catalyzed
reactions
Chapter 18 – Chemical Equilibrium

Define equilibrium and state the conditions necessary
for a system to be at equilibrium

Write chemical equilibrium expressions and perform
calculations involving them

List factors that disturb equilibrium and predict shifts
in equilibrium using LeChatelier’s Principle

Explain acid ionization constants and write the Ka
expressions

Explain and calculate values for Ksp (solubility product
constants) and molarity of ions in solubility equilibria.
Chapter 19 – Oxidation – Reduction Reactions

Define oxidation and reduction

Assign oxidation numbers to reactant and product
species

Identify redox reactions, and write oxidation and
reduction half-reactions for a given redox reaction.

Relate chemical activity to oxidizing and reducing
strength
Chapter 20 – Electrochemistry

Identify the parts of an electrochemical cell and their
functions.

Distinguish a voltaic cell from an electrolytic cell

Calculate cell potentials from a table of standard
electrode potentials.

Identify cathode and anode and write the halfreactions occurring at each electrode in a given
electrochemical cell
Chapter 21 – Nuclear Chemistry

Explain why nuclear reactions occur and know how to
balance a nuclear equation

Define half-life and explain how it relates to the
stability of the nucleus; work simple half-life problems

Define and relate the terms ‘radioactive decay’ and
‘nuclear radiation.’
Chapter 22 – Organic Chemistry

Identify functional groups in a molecule

Give names of simple organic compounds, given their
structural formulas