NATURAL SCIENCES DEPARTMENT-CHEMISTRY
CHM1025: Introduction to Chemistry
Study Guide for FINAL EXAM Fall 2018
Introduction
Every student registered for Introduction to Chemistry (CHM1025) in the Natural Sciences Department at Santa Fe
College will take a common CHM1025 Final Exam at the end of the semester. The CHM1025 Final Exam has 50
multiple choice questions that cover all topics in the latest CHM1025 course outline. Students have exactly 120
minutes to finish the test. Programmable (also known as graphing) calculators are not permitted on the exam.
Students with a disability OR scheduling conflicts must contact the Department Chairman’s office in person at X201 or by calling 352-395-5349 in advance, at least one week before Final Exam date or earlier.
What is provided for the student?
 A periodic table (no names of compounds) and a list of common physical constants.
 A scantron sheet to bubble in your chosen answers.
 Scratch paper.
Typical Final Exam Break Down by Topic:
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2.
3.
4.
5.
Measurements, Uncertainty, and Significant Figures (5 questions – 3 measurement and 2 others)
a) Reading scale with the correct nominal value and instrument reading error(uncertainty).
Examples: buret (inverted scale), graduated cylinder (concave meniscus), pipet, thermometer (convex
meniscus), speedometer, or beaker.
b) Using significant figures and scientific notation in mathematical operations and rounding off correctly.
c) Metric unit conversions.
Nomenclature. (5 questions)
a) Elements and simple cations and anions
b) Ionic compounds including polyatomic ions and certain multi-valent metal ions
c) Covalent compounds including acid and bases (but not organic compounds)
Balancing Equations (5 questions)
a) Including use of fractional coefficients in solving, and use of charge in solving
Stoichiometry (9 questions)
a) Conversions of:
i. Moles to particles/atoms/ions/formula units/molecules (vice versa)
ii. Grams to moles (vice versa)
iii. Moles to moles
iv. Stoichiometry using energy (endothermic/exothermic reactions)
b) Limiting reactant: Given a balanced equation predict how much product is formed or how much reactant is
needed.
c) Percent composition. Determining empirical and chemical formulas.
d) Calculations involving actual yield and % yield.
e) Visualization of reaction stoichiometry
f) Calculation of molarity
g) Titration calculation for a 1:1 mol ratio acid and base
Acid and Bases (5 questions)
a) Knowing the Bronstead-Lowry definitions and be able to identify acid, base, conjugated acid-base pairs in a
given reaction.
b) Be able to identify conjugate acid/ base pairs.
c) Identify a strong and a weak acids and their reaction with water.
d) Write molecular, ionic, and net ionic equations for acid/base reactions.
Rev. Fall 2018
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NATURAL SCIENCES DEPARTMENT-CHEMISTRY
e) Be able to make an inventory of electrolytes in solution. This means that based on the strength of the
electrolyte you should be able to identify which are the ions and/or molecules present in high concentration
in solution.
6.
7.
8.
Redox (Oxidation-Reduction Reactions) (5 questions)
a) Know the definitions and be able to identify the oxidation and the reduction reaction, as well as the oxidizing
and reducing agents in a given reaction.
b) Be able to calculate oxidations numbers in ionic an covalent compounds using both a set of rules and Lewis
diagrams.
c) Be able to identify conjugate redox pairs
d) Be able to identify oxidation-reduction reactions
e) Given a table be able to predict which side of the reaction is favored, also referred as the extent of the reaction.
Miscellaneous Questions (6 questions from these topics)
a) Visualization of atoms, diatomic elements, molecules, and compounds
b) Visualization of phase changes including name of phase change, endothermic or exothermic nature of change,
sign of the enthalpy change
c) Atomic structure: isotopes, mass number, atomic number, number of valence electrons
d) Know how to use the relative electronegativity of atoms to identify polar bonds
e) Know the difference between ionic dissolution, molecular ionization, and molecular dissolution.
Molecular Structure
a) Know how to identify correct Lewis Structures for: (5 multiple choice questions)
i. Molecules with one, two, or three central atoms with single, double, and triple bonds
ii. Structural isomers
iii. Ions and polyatomic ions (must have a bracket around ion with charge on outside)
iv. Know the difference between a chemical formula and the condensed structural formula.
v. Be able to calculate and show non-zero formal charges
vi. Be able to use formal charge arguments to choose the best (lowest energy) structure
b) Know the following for VSEPR (5 multiple choice questions)
i. VESPR Notation in the form of AXmEn up through the tetrahedral family of geometries.
ii. Know how to sketch the resulting (3D) molecular shape for molecule with one, two, or three central
atoms.
iii. Relate molecular geometry to molecular polarity. Be able to classify linear, trigonal planar,
tetrahedral, trigonal pyramidal and bent molecules as polar or nonpolar
iv. Polyatomic ions shape and polarity (polyatomic ions should be classified as ions, not as polar
molecules)
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