STUDY GUIDE FOR FINAL EXAM: HONORS CHEMISTRY
Material from Chapters 4, 5, 6, 7, 8; 9; 10; 11; 12; 13.2-13.3; 14.4-14.5; 16.1-16.2; 17.1-17.3; and
19.2-19.4
V. Chemical Formulas
A. Molecular v. Ionic
i. properties and identification
ii. formulas and element type
B. Diatomic v. binary molecules
i. diatomic elements (GENINE)
C. Atoms, molecules and formula units
i. know definitions.
D. Writing formulas–be able to write formulas from names for:
i. ionic compounds
ii. molecular compounds
iii. acids/bases
a. know properties of acids and bases
b. be able to identify each by properties and formulas
iv. organic compounds
a. saturated hydrocarbons; straight chain, 1-10 carbons
b. cyclic compounds, same as (a.)
c. primary alcohols same as (a) and (b)
E. Oxidation numbers
i. rules for assigning
ii. meaning
iii. periodic table relationship
F. Chemical Nomenclature-be able to write names from formulas for:
i. binary ionic
ii. ionic compounds containing polyatomic ions
iii. ionic compounds containing metals with more than one oxidation state
a. Stock system
b. “older” system using Latin roots and –ic and –ous endings
iv. binary molecular
v. organic – same classifications as in formula writing section
G. Calculations for:
i. molar mass
ii. mole-mass Conversions
a. grams to moles
b. grams to number of particles
c. number of particles to moles
d. the reverse of any of the above
iii. molar volume
a. to grams
b. to moles
c. to number of particles
d. the reverse of any of the above
iv. Percent composition
STUDY GUIDE FOR FINAL EXAM: HONORS CHEMISTRY
Material from Chapters 4, 5, 6, 7, 8; 9; 10; 11; 12; 13.2-13.3; 14.4-14.5; 16.1-16.2; 17.1-17.3; and
19.2-19.4
VI. Chemical Quantities and Chemical Reactions
A. Calculations for:
i. empirical and molecular formulas
a. from gram analysis data
b. from percent composition data
ii. molarity
a. determine molarity of a solution
b. determine the amount of solute required to prepare a solution of
specific concentration.
c. determine the amount of solution of specific concentration that can
be prepared from a specified amount of solute
d. determine the concentration of an ion in a solution containing an
ionic solute.
iii. dilutions
a. determine molarity of a solution through dilution
b. determine the amount of stock solution required to prepare a solution
of specific concentration or to prepare a specific amount of solution
of known concentration.
B. Writing Chemical Equations
i. general format
ii. physical states and conditions of reaction
C. Balancing Chemical Equations
i. by inspection
ii. redox by oxidation number method
D. Classifying Chemical Reactions
i. synthesis
ii. decomposition
iii. single replacement
iv. double replacement
a. neutralization
b. precipitation
c. insoluble gases
v. combustion-complete and incomplete
vi. oxidation-reduction
STUDY GUIDE FOR FINAL EXAM: HONORS CHEMISTRY
Material from Chapters 4, 5, 6, 7, 8; 9; 10; 11; 12; 13.2-13.3; 14.4-14.5; 16.1-16.2; 17.1-17.3; and
19.2-19.4
VII. Chemical Reactions
A. Predicting Products
i. single replacement and the use of activity series for metals and nonmetals
ii. double replacement
a. neutralization
b. precipitation and the use of solubility rules
c. insoluble gases
iii. combustion-complete and incomplete
B. Oxidation-Reduction Reactions
i. Should be able to determine:
a. substance oxidized
b. substance reduced
c. oxidizing agent
d. reducing agent
f. balance using oxidation number method
C. Stoichiometry
a. Mass-Mass/Mass-Volume/Volume-Volume Problems
b. Limiting Reactants
c. Energy of Chemical Reactions
i. reaction coordinate diagrams for exothermic and endothermic
reactions
ii. standard enthalpies of formation (ΔHof)
iii. enthalpy of reaction (ΔHorxn)
a. determine from (ΔHof)
iv. stoichiometry and (ΔHorxn)
D. Collision Theory-be able to discuss the conditions required for a reaction to occur.
E. Factors that affect reaction rate-be able to discuss the impact of varying these factors
on how fast a reaction occurs and relate to Collision Theory.
STUDY GUIDE FOR FINAL EXAM: HONORS CHEMISTRY
Material from Chapters 4, 5, 6, 7, 8; 9; 10; 11; 12; 13.2-13.3; 14.4-14.5; 16.1-16.2; 17.1-17.3; and
19.2-19.4
VIII. Chemical Bonding and Periodic Trends
A. Basic Periodic Trends for families and periods
i. atomic radius
ii. ionic radius
iii. ionization energy
1.exceptions for
2. successive/multiple ionization energies
iv. electron affinity
v. electronegativity
vi. exceptions for (iii) and (iv)
vii. definitions and meanings for (i) – (v)
viii. Explain why each trend occurs (i) – (iv)
ix.Use trends to determine the relationships between different atoms.
B. Ionic Bonding
i. definition and how to identify
ii. electron transfer diagrams/ charges and formulas
C. Covalent Bonding
i. molecular formula
ii. electron dot formula
a. rules for writing
iii.structural formula
a. bond types
I. single/double/triple
II. polar v. nonploar
D. Basic Molecular Structures and VSEPR Theory
i. linear
ii. trigonal planar
iii. tetrahedral
iv. trigonal bipyramidal
v. octahedral
vi. derivatives for (i) – (iii).
E. Bond angles for basic geometries
F. Hybridization
G. Polarity of bonds and molecules
STUDY GUIDE FOR FINAL EXAM: HONORS CHEMISTRY
Material from Chapters 4, 5, 6, 7, 8; 9; 10; 11; 12; 13.2-13.3; 14.4-14.5; 16.1-16.2; 17.1-17.3; and
19.2-19.4
H. Intermolecular Forces
i. dipole-dipole
a. hydrogen bonding
ii. dipole-induced dipole
iii. induced dipole-induced dipole; London dispersion forces
iv. affect of properties that involve change of state, i.e. melting point,
boiling point, rate of evaporation, solubility
I. Metallic bonding
J. Kinetic Molecular Theory and Gas Laws
i. Postulates of Kinetic Molecular Theory
ii. Pressure
a. units
b. causes
c. how it is measured
iii. Phase Diagrams
a. normal melting point and normal boiling point
b. triple point
c. critical point
iv. Phase changes, heating curves and calculations of the amount of energy
involved
v. LeChatelier’s Principle, vapor pressure and evaporation