Learning Objectives:
Chemistry 121
Final Exam Review Fall
2003 P. Jackson
Chapter 1
- Explain how people observe
nature and attempt to recognize patterns through use of the scientific method.
- Recognize, use, and
interconvert common units from the SI system to describe characteristics
of the natural world; TI calculators are a useful professional tool.
- Explain the differences
between mass and weight.
- Identify the factors
that contribute to the uncertainty in every scientific measurement and use
them to explain how one designs experiments to minimize their contributions
to the results.
- Explain the differences
between accuracy and precision as well as the reporting of results with the
appropriate number of significant figures.
- Be able to classify matter from a
chemical point of view (see Fig. 1.13) and explain the differences between
elements, compounds, substances, and mixtures.
Chapter 2
- Describe how Dalton's
atomic theory relates to the three mass laws and what elements of his atomic
theory still hold true today.
- What contributions did
experiments by Thomson, Millikan, and Rutherford make to our conceptual picture
of atomic structure? Draw a cartoon that represents
a particular type of atom; make sure it includes the appropriate numbers
of subatomic particles.
- Explain what makes two
atoms isotopes of one another. What are their
differences and similarities?
- Recognize and use symbolic
representations for elements from periodic table. Explain
why elements are organized into rows and columns.
- Explain what the term
mole represents when
it is used to describe matter. What is a mole based on? What
is Avogadro's number?
Chapter 3
- Explain the differences
and similarities between covalent
and ionic bonding.
- Name inorganic compounds from chemical
formulas and vice versa.
- What is the difference
between Molecular mass and Molar mass?
- What does a chemical
formula represent? How can one determine empirical
and molecular formulas from mass data and vice versa?
- What does percent composition represent?
How do you determine the percentages of an element in a chemical compound?
Chapter 4
- Balance a chemical equation
and explain why it is important to do so.
- Use the mole-mass-number stoichiometric
relationships to solve chemical problems. (See
Fig. 4.8)
- Identify the type
of chemical reaction (i.e. displacement, combustion, decomposition, etc.)
from a chemical equation or write an appropriate chemical equation from the
description.
Chapter 5
- How are the terms concentration and molarity related to one another? How would you prepare a solution that is of lower concentration
from one of higher concentration?
- Describe the unique characteristics
of water as a solvent, specifically for solvating ionic compounds.
- Write, Balance and use Net Ionic Equations
to describe the reactions of chemicals in water.
- Employ solubility rules to predict
the properties of reactants and products in chemical reactions; use these
to assign the phase states of the specific chemicals.
- Recognized and describe the properties
of strong and weak electrolytes, including strong acids, weak acids, strong
bases and weak bases.
- Show how an acid-base reaction is
simply a proton transfer reaction; write a net ionic equation for the neutralization
reaction.
Chapter 10
- Give the definition of
and use a picture to illustrate the meaning of the term pressure.
- Be able to describe how the kinetic-molecular
theory predicts how gases behave.
- Use equations, words
and pictures to describe how the individual gas laws (Boyles, Charles, Avogadro)
are incorporated into the ideal gas law (PV=nRT).
- Use the ideal gas law,
stoichiometry, and Dalton's law of partial pressures to solve chemical problems.
TI calculators are good professional tools.
Chapter 14
- Explain what is meant
when a system attains "dynamic equilibrium".
- Explain how the magnitude
of K refers to the extent of a reaction.
- Explain how the reaction
quotient (Q) changes until equilibrium is reached, at which point Q=K.
- Show how the form of
Q (or K) is based exactly on the balanced chemical equation.
- Explain why pure solids
and pure liquids do not appear in equilibrium expressions.
- Show how the interconversion
between Kp and Kc is based on the ideal gas law and
(delta)ngas.
- Describe how the reaction
direction depends on the relative values of Q and K.
- Know how to use a reaction
table to set up and solve equilibrium problems.
- Provide a definition
for LeChatlier's Principle and give an example of how it works.
- Explain how temperature,
pressure (volume), and changes in concentration affect a system at equilibrium.
Chapter 16
- Compare and contrast
the Arrenhius and Bronsted-Lowry definitions for an acid or a base.
- Identify and describe
what constitutes a conjugate acid-base pair.
- Describe how the strength
of an acid or base relates to the extent of its ionization in water.
- Explain how relative
weak acid strength is expressed by the acid ionization constant, Ka.
- Explain how relative
weak base strength is expressed by the acid ionization constant, Kb.
- Identify and rank chemicals
according to their acid or base strength.
- Explain the difference
between a monoprotic acid and a polyprotic acid.
- Write the definition
of pH and pOH.
- Describe how the autoionization
of water gives pure water a pH = 7.00
- Calculate the pH of
strong acid and/or strong base solutions.
- Calculate the pH of
weak acid and/or weak base solutions.
- Explain how you would
find the value for Kb when only Ka and Kw
are given.
- Explain what an amphoteric
substance is and give an example of one.
- Describe how salts can be either neutral,
basic, or acidic when dissolved in water.
Chapter 17
- Describe what a buffer
solution is and how it works.
- Explain how you would
chose the components of a solution that would buffer a given system at a
specific pH.
- Describe the concentration
and pH ranges over which an acetic acid/sodium acetate buffer would work
most effectively.
- Explain why a titration
is a useful chemical experiment to design and implement.
- Sketch the shape of
titration curves, identify important points or regions in each, and be able
to calculate the pH at any point along the curve.
- Strong acid titrated
by strong base (or vice versa)
- Weak acid titrated
by a strong base
- Weak base titrated
by a strong acid
- Explain how you would
select an appropriate chemical indicator to help you determine the end point
of a titration.
- Explain the difference
between the Equivalence Point and the End Point of a titration.
- Describe how a slightly
soluble ionic compound reaches equilibrium in water, expressed by an equilibrium
(solubility product) constant, Ksp.
- Calculate the solubility
of a sparingly soluble salt by applying equilibrium principles.
- Explain how the addition
of a common ion to a solution decreases the solubility of a slightly soluble
salt.