2013 Chemistry Semester
FINAL Review
Sr. Julia Marie, O.P.
This review might give you an idea of some areas you may need to study. It is not a complete list. If you discover
sections that you’ve struggled with during the school year you should return to your notes, the book, and the numerous
worksheets you have completed. Refer to your class notes, worksheets, and the textbook to complete this review sheet.
Study early so that you will have time to ask questions about what you don’t understand. Do not forget to use your
study guide from the first quarter exam to also help you review for your semester final.
Final Exam:
Date: 5/27/13
Time: 8:30am in Theater
Preparations: Bring two #2 pencils and a scientific calculator. NO sharing of calculators will be permitted.
Provided with test: periodic table with names, atomic number, atomic mass (g/mole), geometry chart for 3D
molecules, activity series, solubility rules
Semester I General Outline
Chemical Foundations
A. Laboratory
-Scientific Method
-Differentiate qualitative and quantitative measurements
-Lab Equipment identification (see handout on webpage)
-Explain proper lab procedures such as lighting a Bunsen burner
-Laboratory safety (review rules in lab)
B. Measurements
-measuring to the correct number of sig figs.
-International System of units (SI units, base and derived units)
-scientific notation
-conversion of units (know your prefixes!!)
C. Significant figures
-amount of significant figures of a given number
-rounding numbers to the correct number of significant figures
-calculations with significant figures
D. Density
-mass, volume and density and temperature
-calculations of density, mass and volume (D = M/V)
E. Matter
-identify states of matter and transitions of states
-correctly classify matter (mixture, pure substance, etc.)
-identify a physical and chemical change; provide evidence for chemical changes
Atoms and Elements
A. History of atom (development of atomic theory- see history review packet)
-history of atomic models through time including Democritus, Dalton, J.J. Thomson, Ernest
Rutherford, Neils Bohr, DeBroglie and Schrodinger, Heisenberg
- what each scientist contributed to chemistry (know the packet well!)
- what experimental evidence was involved in development of each atomic model
Atomic Structure (know history, quantum number/electron configuration packets)
B. Bohr model of atom
-emission-line spectrum of hydrogen and how it comes about by explaining transition of
electrons between energy levels in atoms
-ground and excited states of electrons
-identification of elements by line spectrA
C. Quantum mechanical model of atom
-principle, angular, magnetic and spin quantum numbers (know symbols, define, identify)
-atomic orbitals (s,p,d,f), their electron density (=shape), energy and electron capacity
-know number of shapes, orientations, electrons, etc. are within each energy level
D. Electron configurations of elements
-Write out electron configurations of atoms and ions (take into account charges)
try using periodic table versus memorizing electron configuration pattern
-abbreviated configuration method (using noble gas symbols)
-Pauli exclusion principle, Aufbau principle, Hund’s rule
-exceptions to the rules in electron configurations (transition metals have funny pattern when
you get to the d and f orbitals)
-valence electrons, define/identify
Atomic Structure
 Identify the groups/families of the periodic table
 Define parts of an atom
 Determine number of each type of particle in atom from information given on periodic table
 Define ion and polyatomic ion
 Define isotope
 Define and calculate average atomic mass
 History of the Atom
 Quantum Mechanical Model of the Atom
 Emission Spectrum (Atomic Spectrum)
 Electron Configurations and Valance Electrons
Mole Concept
 Explain the mole
 Convert between moles and grams, grams and moles (mole road)
 Memorize Avogadro’s number
 Convert between moles and # particles, # particles to moles (mole road)
Molecules
 Calculate molar mass
 Calculate percent composition of a compound (including hydrates)
 Electron configurations of atoms
 Valance electrons (determine from electron configurations and/or periodic table)
 Covalent and Ionic Bonds
 Lewis Structures
 Electronegativity
 Polarity of bonds and molecules
 3D Molecular structure (VSEPR Theory)
 Drawing Lewis structures of molecules and polyatomic ions
Nomenclature
 Identify and distinguish between an ionic and covalent compound
 Name ionic compounds without transitional metals
 Name ionic compounds with transitional metals (that need Roman Numerals)
 Name ionic compounds that contain polyatomic ions
 Name covalent compounds (memorize the prefixes for these)
 Name both types of acids (containing and not containing polyatomic ions)
 Write the chemical formula of any compound when given the name
o Know how to pair charged ions to balance the charge within ionic compounds!
Chemical Equations
 List all of the parts of a chemical equation including symbols
 List and identify the six types of chemical reactions
 Properly write out chemical equations when given each compound’s name
 Define diatomic and list the seven diatomic elements. Watch for them when balancing equations or when
doing word problems
 Balance chemical equations
Stoichiometry and Limiting Reagents
 Define stoichiometry and calculate stoichiometry problems
 Calculate the moles of compounds in a balanced equation when given grams or moles of one compound using
coefficient ratios
 Define and identify limiting reagent when given quantities of two reactants in a chemical reaction
 Calculate products formed after finding a limiting reagent
 Calculate excess reactant that is not used after a reaction is complete
 Calculate percent yield when given actual yield