Exam will have 100 points.
You will be allowed the entire class period to complete the exam.
The exam will be a mix of multiple-choice and show your work problems, following the format of the quizzes.
Review your quiz zes, homework problems, class notes, instructor’s homepage,
Chang’s web site and textbook.
Do not forget to bring a functioning calculator !!!
 Know the basic steps in the “scientific method”

Distinguish between a hypothesis, a theory, and a law

Know the 3 states of matter and their general properties

Distinguish between homogeneous mixtures (solutions) and heterogeneous mixtures

Distinguish between physical and chemical means of separation and physical and chemical changes

Distinguish between atoms and molecules and elements and compounds

Know the difference between macroscopic and microscopic properties, and intensive and extensive properties
 Be able to express measurements in “scientific notation”

Know the basic metric units of mass, volume and length and be able to convert them into other units

Know the prefixes used with SI Units (Table 1.3 in text)

Be able to convert between Fahrenheit, Celsius and Kelvin temperature scales

Know the difference between accuracy and precision

Be able to express all answers with the correct number of significant figures

Be able to find density and use density to find volume and mass
 Be familiar with Dalton’s Atomic Theory, the Law of Conservation of Mass, the
Law of Definite Proportions, and, the Law of Multiple Proportions

Know the subatomic particles, their approximate mass, charge, and location within the atom

Know the basic findings of the experiments of JJ Thompson (electron charge –
1.76 x 10 8 C/g), Millikan (charge of single electron
–1.6022 x 10 -19 C), and
Rutherford (small, dense nucleus) and Thompson’s ‘Plum-Pudding” Model of the
Atom
 Use “atomic notation” to find the number of electrons, protons and neutrons of an atom or ion number: protons + number of neutrons X or mass number X or Z X
number of protons atomic number A

Be able to define isotopes (same element, but different mass/number of neutrons)

 Know “family” names and general sections of the periodic chart (alkali metals, alkaline earth metals, transition metals, halogens, noble gases)

Know which elements are metals, metalloids and nonmetals

Know names and symbols of all elements in Figure 2.11 of text

Know the definition of a molecule, and which elements occur as diatomic molecules

Know the definition of ions, cations, and anions and be able to predict ion charge of an element from its location in the periodic chart (Table 2.2)

Be able to identify if a compound is an ionic compound

Know the definition of isoelectric and be able to recognize atoms and ions that are isoelectric

Be able to give the atomic composition of a compound from its formula

Know the definition of empirical formula and be able to recognize them

Be able to name binary and ternary compounds

Know the names of the common acids and ions (Table 2.3)

Know how to name oxoacids, oxoanions and bases

Be able to name compounds with waters of hydration
 Know the definition of Mole, Avogadro’s Number and Molar Mass

Be able to calculate average atomic mass from an atom’s isotopic distribution and vice versa

Determine the number and types of atoms in a formula

Be able to find the Molar Mass of elements on the periodic chart and calculate the Molar Mass of compounds

Do conversions: mass moles
 Find % composition from a compound’s formula
individual particles
 Find a compound’s empirical formula from its % composition
 Find a compound’s (true) molecular formula from its empirical formula and molar mass

Write and balance chemical reactions

Use balanced equations to do stoichiometry problems (and calculate Theoretical yield)

Know how to identify and calculate limiting reagents and excess reagents

Be able to calculate % Yield (given actual yield) and vice versa

Know the definitions of solution, solvent and solute

Be able to identify electrolytes and nonelectrolytes and which are strong electrolytes

Be able to describe the hydration of ions in aqueous solutions

Know the solubility rules (Table 4.2)

Be able to write molecular equations, ionic equations and net ionic equations for precipitation reactions


Know the Arrhenius and Brønsted theories of acids and bases

Know the definition of monoprotic, diprotic and triprotic acids

Know the difference between strong and weak acids an bases

Know whi ch acids are strong (“Big Six”) and which are weak

Know which bases are strong and which are weak

Define a neutralization reaction according to the
Brønsted theory (proton transfer)

Know how to identify Oxidation-Reduction Reactions (Redox reactions)

Be able to calculate oxidation numbers

Be able to identify which elements are oxidized, and reduced, and which reagents are oxidizing agents and which are reducing agents

Be able to write half reactions showing the transfer of electrons for an oxidation or reduction

Identify types of reactions: Combination, Decomposition, Metal Displacement,
Halogen Displacement, Hydrogen Displacement and Disproportionation
Reactions

Be able to find the concentration of a solution in units of Molarity (mol/L)

Be able to use Molarity as a conversion factor between moles and volume of a solution

Be able to calculate dilutions of solutions

Be able to stoichiometry problems that involve solutions of known Molarity

Know what an acid-base titration is, the definitions of equivalence point, titrant, standard solution and analyte

Be able to do stoichiometry problems that involve acid/base neutralizations
(titrations)

Be able to do stoichiometry problems that involve precipitation reactions
(gravimetric analysis).

Know the properties of gases

Know which substances exists as gases and why
 For gases, be able to change pressure units from “atm” to “torr” and “mm of Hg”

Know what a barometer, closed end manometer and open-end manometer are and how to calculate the pressure of a gas
 Know how to use the gas laws (Boyles’, Charles’, Gay-Lussac’, Avogadro’s, and
Combined) to do calculations.
Potentially Useful Information:
1 atm = 760. mm Hg = 760. torr = 101.325 kPa = 29.92 in Hg
N
A
= 6.022 x 10 23 R = 0.082057 L atm / K mole
°C = (°F – 32°F)*(5°C/9°F) °F = (9°F/5°C)*°C + 32°F K = °C + 273.15