+JMJ+
Chemistry Honors Semester Exam Study Guide
Fall 2013
The semester exam for Chemistry Honors is scheduled for Wednesday, December 18th at 11am
in the Theater. This exam for will be a comprehensive exam encompassing all material we have covered
this semester. This study guide is intended to be an outline of the major topics presented in this class. It
is not worth any points and will not be collected. It is also not an extensive list of material, but a guide to
prompt your studying. You are responsible for all of the material we have covered in chapters 1-5 in
addition to any special topics presented and/or discussed. If you have questions about a particular topic,
don’t be afraid to ask in class or see me for help. Teaching and quizzing one another will serve very
useful in demonstrating your mastery of the material, so study together, ask questions, and continue to
learn!
I. Part I: Lab Practical Exam (50pts, 40 min.)
A) In a series of five (5) Lab stations, you will demonstrate your proficiency in lab techniques you
have learned this semester. This is to be treated as a test. You may not converse with anyone
and must turn in your completed answer sheet without help from classmates. Stations will
include:
1) Lab Safety: Safely lighting a Bunsen burner and describing the flame.
2) Using a spectroscope to classify an unknown.
3) Making accurate and precise measurements.
4) Identifying Lab Equipment
5) Hypothesis generation (asking an answerable question)
II. Part II: Written Exam (150pts, 2 hrs.)
A) Chapter 1: The Science of Chemistry
Vocabulary:
Chemical
Chemical reactions: reactants/reagents and products
States of matter
Matter
Volume
Weight vs. Mass
Meniscus
Chemical vs. physical property
Density
Atom vs. molecule
Element
Compound
Pure substance
Mixtures: homogeneous vs. heterogeneous
Key Concepts: 1) Kinetic molecular theory 2) SI units for measurements in chemistry
3) Properties of matter 4) Classification of matter
B) Chapter 2: Matter and Energy
Vocabulary:
Heat and Energy and Temperature
Physical vs. chemical change
Evaporation
Endothermic vs. exothermic (draw and/or interpret a graph)
+JMJ+
Specific heat (remember the formula? units? meaning?)
Heating curve for H2O
The Scientific Method
Hypothesis
Theory vs. law
Law of conservation of mass
Law of conservation of energy
Accuracy vs. precision
Significant figures
Key concepts: 1) Energy and mass conservation 2) The Scientific Method 3) Making
measurements in chemistry 4) distinguishing between chemical and
physical changes.
C) Chapter 3: Atoms and Moles
Vocabulary:
Law of definite proportions
Law of multiple proportions
Electron
Nucleus
Proton
Neutron
Atomic number
Atomic mass
Mass number
Molar mass
Isotope
Orbitals: s, p, d, f and their max. # of eElectromagnetic spectrum: ROYGBIV (Light and e- properties)
Ground vs. excited state for ePrincipal quantum number: what does it mean?
Pauli exclusion principle
Aufbau principle
Hund’s rule
Mole and Avogadro’s # (based off of which element?)
Key concepts: 1) The structure of an atom 2) Formation of an isotope 3) Particles
common charges and masses (for p+, e-, and n0) 4) Finding # of n0
5) nuclear symbol notation 6) Determining # of particles in isotopes
7) Principal quantum number: How does it relate to element position on
the periodic table? 8) Electron configuarions (all three methods)
9) Dual wave-particle nature of electrons 10) the mole 11) Conversions
using amount in moles to grams and/or atoms 12) Ununpentium and
creating synthetic elements
D) Chapter 4: The Periodic Table
Vocabulary:
Periodicity and the Periodic law
Valence eGroup
Period
Main group elements: which ones are they?
+JMJ+
All group names, for example: alkali metals, halogens, noble gases, etc.
Ionization energy
Electron shielding
Atomic radius
Electronegativity
Nuclear reactions- nuclear fusion vs. nuclear fission
The Big Bang Theory (not the TV show)
Key Concepts: 1) Names of the different blocks of the periodic table 2) group properties
3) Forming ions 4) Synthetic elements
E) Chapter 5: Ions and Ionic Compounds
Vocabulary:
Octet rule
Ion: cation or anion
Salt
Crystal lattice
Polyatomic ion
Key Concepts: 1) Electron configurations change in making an ion, why? TO BE STABLE
LIKE THE NOBLE GASES 2) Ion charges and valence electron numbers of
the main group elements 3) Metals are weird-can be cations of various
charges 4) Properties of ionic compounds 5) Naming ionic compounds
6) Ionic compounds MUST be neutral in charge 7) Proper use of
parentheses and subscripts and superscripts for compound formulas
and ions, respectively.