CHEMISTRY 1ST SEMESTER FINAL EXAM
STUDY Gliquid
UIDE
CHAPTER 1 & 2

 Scientific Method
 Open system
 Closed system
 Steps of the Scientific
method
 Theory
 Mass
 Hypothesis
 Weight
 Quantitative data
 Qualitative data
 System
 7 SI base units
 Metric prefixes
 Volume
 Density
 Accuracy
 Precision
 Percent Error
 Significant Figures
 Scientific Notation
 Derived SI units
 Conversion Factor
 6 branches of chemistry
 Chemistry
CHAPTER 3
 volume
 mass
 matter
 atom
 element
 compound
 molecule
 4 indicators of a
chemical reaction
 reactants
 products
 plasma
 conservation of energy
 pure substance
 group or family
 period
 intensive properties
 extensive properties
 physical properties
 physical change
 chemical properties
 chemical change
 homogenous mixture
 heterogeneous mixture
 solid

gas
 metals
 nonmetals
 metalloids
 noble gases
CHAPTER 4
 Law of Multiple
Proportions
 Law of Conservation of
Mass

Law of Definite
Composition
 JJ Thomson
 Ernst Rutherford
 John Dalton
 Robert Millikan
 Nucleus

Protons
 Neutrons
 Electrons
 Isotopes
 Atomic Number
 Mass Number
 Mole
CHAPTER 5
 Wave/Particle Nature of
Light
 Spectral Lines
 Wavelength
 Speed of Light
 Pauli Exclusion
Principle
 Hund’s Rule
 Aufbau Principle
 Frequency
 Photon
 Excited State
 Ground State
 4 Quantum Numbers
 Dmitri Mendeleev
 Henry Moseley
 Alkali Metals
 Alkaline Earth Metals
 Noble Gases
 Halogens
 Lanthanides
 Actinides
 Atomic Radii Trend
 Ionization Energy Trend
 Electronegativity Trend
 Valence Electrons
Cation
 Anion
 s, p, d, f block on
periodic table
CHAPTERS 6.1 AND 10.1 - 10.3
 Ionic bond
 Covalent bond
 Polar covalent bond
 Nonpolar covalent bond
 Octet rule
 VSEPR theory
 Molecular shapes
 Bond type using
electronegativity values
 Crystal Lattice
 Properties of ionic and
covalent compounds
CHAPTER 6
 Ionic Bonding
 Crystal Lattice
 Formula Unit
 Properties of Ionic
Compounds
 Properties of Covalent
Compounds
 Metallic Bonds
 Formula Writing and
Naming
 Ionic compounds
(binary and polyatomic)
 Molecular (covalent)
Compounds
 Acids
 Polyatomic ions
CHAPTER 7
 Mole
 Empirical formula
 Molecular formula
 Percent Composition
IMPORTANT !
Bring the following
items with you on
exam day:
◘ Calculator
◘ VSEPR Table
◘ Orbital Filling
Diagram
You will be provided
with the following:
◘ Periodic Table with
Polyatomic Ion List
◘ Chart of
Electronegativities