Chemistry Review Sheet for Final Exam, Semester 2, 2012-2013
You should be able to...
Chapters 1-3: Introduction, Data Analysis and Problem-solving, Matter
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Read a chemical formula for type of elements and number present
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Use metric prefixes to convert metric units using dimensional analysis
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Convert temperatures from Kelvin to Celsius and vice-versa
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Use significant figures in measurements and calculations
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Calculate density and manipulate it find unknown parts of calculations
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Interpret data
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Distinguish among observation, law, hypothesis and theory
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Compare and contrast the three states of matter
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Describe the energy changes involved in changes of state
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Identify and classify physical/chemical changes and properties of matter, with examples
Chapter 11: Moles
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Define Avogadro’s number
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Perform conversions among moles, # particles, molar mass, gas volumes, kJ and the # atoms of an element in a compound
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Determine molar masses of elements and compounds
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Determine percent composition of elements in a compound
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Determine empirical formula of a compound from the masses or percent composition of elements in a compound
Chapters 4 & 5: Atomic Structure
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Describe and interpret the key experiments that contributed to the evolution of the modern theory of the atom, including those of
Thomson, Rutherford, and Bohr
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Define and discuss the structure of an atom including the locations, relative masses, and charges of electrons, neutrons and protons
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Use the atomic number and mass number to find the number of protons, electrons, and neutrons in an atom
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Describe how the isotopes of an atom differ, and apply specific notation to distinguish among these isotopes
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Write simple nuclear equations representing radioactive decay and formation of new elements
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Describe the quantum mechanical model of the atom
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Distinguish among principal energy level, energy sublevel, and atomic orbital
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Use the Aufbau Principle, the Pauli Exclusion Principle and Hund’s Rule to write the electron configurations and orbital diagrams of
the elements
Chapters 6 and 7: Periodic Table
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Classify and describe the elements the following ways
o according to the configuration of their outermost electrons (s, p, d, f; representative, transition and inner transition
(rare earth) elements, noble gases)
o according to their properties (metals, nonmetals, metalloids, noble gases; alkali metals, alkaline earth metals,
halogens)
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Write and compare electron configurations for atoms and ions
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Draw electron dot diagrams (Lewis Structures) of the elements
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Describe and predict the following group and period trends in the periodic table: ionization energies, atomic and ionic radius
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Use the periodic table to find the number of valence electrons in an atom and the charge on an ion
Chapters 8 and 9: Bonding and Naming
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Compare/contrast ionic, metallic and covalent bonding (including covalent networks)
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Compare and contrast ionic, metallic and covalent compounds
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Write the chemical formulas of ionic and molecular compounds when given the name of the compound, vice versa
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Write the chemical formulas of ionic compounds given the ions, or by using the position of the elements on the periodic table
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Use dot diagrams (Lewis structures) to represent covalent bonding in molecules and polyatomic ions
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Predict the formation of single, double, and triple bonds
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Use VSEPR theory to describe the shapes of simple covalently bonded molecules
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Compare the structure and properties of polar and nonpolar molecules
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Compare the nature and effects of London (dispersion) forces, dipole forces and hydrogen bonding
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Define polymer and describe examples of polymers (e.g. DNA, proteins, long-chain carbohydrates)
Chapter 10: Chemical Reactions
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State the four types of evidence that demonstrate that a chemical reaction has probably occurred
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Identify the reactants and products in a chemical equation
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Use appropriate symbols when writing an equation to accurately describe the chemical reaction, including reaction conditions and
states of matter
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Write a balanced chemical equation when given the names or formulas of all the reactants and products in a
chemical reaction
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Classify a reaction as synthesis (combination), decomposition, single replacement, double replacement or combustion
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Predict the products of simple synthesis (combination) and decomposition reactions
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Use the generalizations based on the activity series to predict whether or not a single replacement reaction will occur and what the
products will be
Write the double-replacement reaction between two ionic compounds in aqueous solution, including the use of net and total ionic
equations
Identify the three common types of products produced in double replacement reactions
Classify a reaction as exothermic or endothermic
Describe the general properties of acids and bases
Distinguish between strong and weak vs. concentrated and dilute acids and bases
Define pH, identify whether a solution is acidic, neutral or basic based on its pH
Identify hydrogen ion donors and acceptors in acid-base reactions
Define and calculate molarity, calculate pH from molarity and molarity from pH for simple pH problems
Chapter 12: Stoichiometry
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Interpret balanced equations in terms of interacting moles, particles, masses, and volumes of gases (at STP)
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Construct mole ratios from balanced chemical equations for use as conversion factors in stoichiometric problems
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Perform stoichiometric calculations with balanced equations using mass, moles, representative particles, volumes of gases (at STP)
and/or kJ
Chapter 13 & 14: Gases, Liquids and Solids
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Describe the kinetic theory of matter and explain how it accounts for observed gas (and liquid and solid) behavior
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Convert among kPa, atm, Torr and mm Hg
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qualitatively compare rates of effusion or diffusion of gases with their relative molar masses
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Use Dalton’s Law of Partial Pressures to calculate partial and total pressures of gases and vapors
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Compare the properties of solids, liquids and gases in terms of intra- and intermolecular forces
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Describe the phase and energy changes that occur when substances change state
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Interpret a phase diagram, including phase changes, triple point, critical point (critical T)
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Relate attractive forces to boiling point, volatility, and surface tension
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Identify and describe several physical properties of gases
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Use the combined gas law to account for changes in P,V, T
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Determine density of gases in g/L (application of Avogadro’s Principle) and use gas density to determine molar mass at STP and
under non-standard conditions
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Use the ideal gas law to calculate an unknown with three known quantities (P, V, T, # particles)
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Apply stoichiometry to gases problems
Chapter 16: Thermodynamics
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Define and explain the difference between heat and temperature
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Define specific heat and incorporate it into calculations of heat absorbed or released
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Perform calculations that require the q equation, including calorimetry
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Interpret heating curves in terms of temperature and phase changes (heating vs. change of state)
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Interpret an energy diagram of a reaction pathway for an endothermic or an exothermic reaction, including calculations for heat of
reaction and activation energy
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Explain what activation energy is and how it affects chemical changes
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Explain what a catalyst is and how it affects activation energy and reaction progress
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Identify whether a chemical or physical change is exothermic or endothermic by the sign of H
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Apply Hess’s Law (versions 1 and 2) to solve problems involving physical and chemical changes
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Explain the relationship between a change in entropy and stability
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Use standard entropy values in calculations of changes in entropy
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Summarize the five conditions that increase entropy of a chemical or physical change
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Predict the sign for change in entropy in a system
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Summarize the conditions that favor a spontaneous chemical reaction (and those that don’t), including the effects of temperature
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Calculate the free energy to predict whether a reaction will occur spontaneously
Equilibrium and Reaction Rates (handouts)
 Define chemical equilibrium
 Predict the effects of changing concentration of reactants or products, temperature and pressure on the direction of reactions
 Define reaction rate (change in concentration or pressure or similar units relative to time)
 Predict the effects of temperature , catalysts, reactant and product concentrations on reaction rate
Chapter 15: Solutions (handout)
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Define solute and solvent in terms of solutions
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Identify examples of different types of solutions
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Define and apply the terms soluble and insoluble and miscible and immiscible to solutions
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Describe how temperature, agitation and particle size affect the rate of solvation
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Define and apply the term solubility; calculate solubility and interpret solubility curves
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Compare unsaturated, saturated and supersaturated solutions
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Compare concentrated with dilute solutions
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Calculate solution concentrations in terms of mass percent and molarity (Moles Unit)