Final Exam Study Guide
Chapter 1

• What affects all aspects of life?
• 5 traditional areas of study in chemistry and difference between each
• Difference between pure and applied chemistry
• Scientific method steps and detail about each

Chapter 2

• Matter properties can be classified as?
• Every sample of a given substance has?
• 3 states of matter
• Physical changes are classified as?
• Homogenous mixtures are also called?
• Differences in _____ can be used to separate ______.
• 2 separation techniques
• Identify reactants and products
• Law of conservation of mass

Chapter 3

• Difference between precision and accuracy
• Calculating error and percent error
• 5 commonly used SI units
• SI units on Table 3.1 page 73
• Conversion factors on Table 3.2 page 74
• Metric units of volume on Table 3.4 page 75
• Converting from °C to K
• Converting between metric units
• Density equation and using it
• How temperature affects density

Chapter 4

• What did Democritus believe about atoms?
• Dalton’s atomic theory
• 3 subparticles
• Determining the number of protons, neutrons, and electrons
• Calculating average atomic mass

Chapter 5

• Three rules of finding electron configurations
• Electron configurations of elements and ions

Chapter 6

• How Mendeleev arrange the elements versus the modern periodic table arrangement
• 3 classes of elements
• Periodic atomic size trend
• First ionization energy trend
• Ionic size trends
• Electronegatively trends

Chapter 7

• Valence electrons in each group
• Electron dot structure
• Identify ionic compounds
• Ionic compound characterists
• Sterling silver and bronze components
• Why alloys are important?

Chapter 8

• Identify molecular compounds
• Molecular compounds characterists
• Difference between single, double, and triple covalent bonds
• Exceptions to the octet rule
• Difference between sigma and pi bonds
• Geometric shapes page 233
• Table 8.3 electronegativity and bond types
• Which molecules are polar or nonpolar?
• Difference between the intermolecular forces and example of a compound with each

Chapter 9

• The difference between a monatomic and polyatomic ion
• How to name transition metal, polyatomic, and Group 1A-3A cations
• How to name polyatomic and Group 5A-7A anions
• The difference between stock and classical naming methods of transition metal ions
• The difference between –ite, –ate, and hypo- in reference to polyatomic ions
• Be able to match polyatomic ions with their correct names
• The difference between a binary ionic compound and binary molecular compound
• How to name or determine the chemical formula of binary ionic compounds, binary molecular compounds, and compound with polyatomic ions
• The difference between an acid and a base
• How to name acids and bases

Chapter 10

• Know 3 common forms of measurement
• Know the 7 diatomic molecules
• Know how to use Avogadro’s number to convert to or from moles or molecules/atoms
• Be able to calculate the molar mass of a compound
• Know how to use the molar mass of a compound to convert to or from a number of moles or grams
• Know how to use Avogadro’s gas constant to convert to or from moles or volume
• Know how to calculate to or from density or molar mass
• Know how to determine the percent composition of each element in a compound

Chapter 11

• Be able to write skeleton equations from word equations
• Be able to identify the 5 types of chemical reactions and determine the products
• For single replacement reactions, know what determines if an element will displace another in a compound
• Be able to predict what chemical compound is a precipitate and write the ionic, net ionic, and identify spectator ions

Chapter 12

• Know how to use a mole ratio to convert from moles of one compound to moles of another
• Know how to convert mass (g) of one compound to mass (g) of the other compound
• Know how to convert to or from molecules/atoms between two compounds
• Know how to convert to or from volume between two compounds
• Be able to identify a limiting reagent in a multiple choice question
• Know how to calculate the theoretical yield
• Know how to calculate percent yield

Chapter 13

• What are the 3 points of the kinetic theory?
• How do you convert between atm, kPa, and mmHg?
• What is the relationship between temperature and average kinetic energy?
• What are the 2 factors that affect boiling points?
• What are the phase changes between the 3 states of matter?
• Is a certain phase change exothermic or endothermic?
• What is the difference between a phase diagram of water versus other molecules?

Chapter 14

• What are the 3 factors that effect gas pressure?
• What is the equation of Boyle’s Law and how do you use the equation to solve for an unknown quantity?
• What is the equation of Charles’s Law and how do you use the equation to solve for an unknown quantity?
• What is the equation of Gay-Lussac’s Law and how do you use the equation to solve for an unknown quantity?
• What is the equation of the combined gas law and how do you use the equation to solve for an unknown quantity?
• What is the equation of the ideal gas law and how do you use the equation to solve for an unknown quantity?
• What are the conditions when real gases deviate the most from being ideal?
• What is the equation of Dalton’s law of partial pressures and how do you use the equation to solve for an unknown quantity?
• What is the equation of Graham’s law of effusion and how/why do you use the equation?

Chapter 15

• What are water’s unique properties and how are they formed?
• What happens if bonding is interfered?
• What is the crystal structure of ice like?
• In a solution, be able to identify the solute and solvent.
• What depicts electrolyte strength and what are examples of each type of electrolyte.
• Know uniformity and filtration on pg 462 Table 15.4

Chapter 16

• What determines how fast substances will dissolve and how does each factor effect the dissolving process?
• What factor affects solids, liquids, and gases versus what only affects gases?
• For most solids, what is the effect of solubility and temperature?
• Using Henry’s Law equation to solve for solubility, pressure, or mass.
• How to calculate molarity or use molarity to calculate moles or volume.
• How to use the dilution equation.
• How to use the percent volume and mass equations.
• What are and a description of each of the three colligative properties?
• How to calculate molality or use molality to calculate moles or kg.
• How to calculate mole fractions of substances.
• How to calculate freezing point depression and boiling point elevation of a solution.

 

Final Exam Vocabulary Study Guide
Chapter 1
Matter
Chemistry
Macroscopic
Microscopic
Manipulated variable
Responding variable
Theory
Scientific law

Chapter 2
Mass
Volume
Extensive property
Intensive property
Substance
Physical property
Solid
Liquid
Gas
Physical change
Mixture
Heterogeneous mixture
Homogeneous mixture
Phase
Chemical change
Chemical symbol
Precipitate

Chapter 3
Accepted value
Experimental value
Error
Absolute zero
Conversion factor
Dimensional analysis

Chapter 4
Atom
Nucleus
Mass number
Atomic number
Isotope
Period
Group
Chapter 5
Aufbau principle
Pauli exclusion principle
Hund’s rule

Chapter 6
Alkali metals
Alkaline earth metals
Halogens
Noble gases
Representative elements
Transition metals
Inner transition metals
Ionization energy
Electronegativity

Chapter 7
Valence electron
Octet rule
Ionic bonds
Formula unit
Alloys

Chapter 8
Covalent bond
Nonpolar covalent bond
Unshared pair
Bond dissociation energy
VSPER theory

Chapter 10
Mole
Avogadro’s number
Molar mass
Molar volume
STP
Avogadro’s gas constant

Chapter 11
Chemical reaction
Chemical equation
Chemical word equation
Skeleton equation
Catalyst

 

Chapter 12
Stoichiometry
Mole ratio
Limiting reagent
Excess reagent
Theoretical yield
Actual yield
Percent yield

Chapter 13
Allotrope
Barometer
Crystal
Gas pressure
Kinetic energy
Triple point
Vacuum
Vapor pressure

Chapter 14
Compressibility
Diffusion
Effusion
Ideal gas constant
Partial pressure

Chapter 15
Surface tension
Surfactant
Aqueous solution
Suspension
Colloid
Coagulation
Emulsion

Chapter 16
Solubility
Concentration
Dilute solution
Concentrated solution