LA City College
Dr. Han
Chem 60 Study Guide (EXAM #2)
In order to do well on this exam, the student MUST master the following material:
Chapter 5:
Understand Dalton’s Atomic Theory.
Know and understand the Law of Multiple Proportions.
Know the subatomic particles and their properties (mass, charge, etc.).
Understand Rutherford’s experiment and its conclusion for the nuclear model of the atom.
Know what is an isotope and be able to write an elements contents (atomic number and mass number) in
isotope notation.
Calculate the atomic mass of an element by its respective abundance (by %) and its mass of at least two
known isotopes of the element.
Know the periodic table (periods, groups, etc.)
Know the nicknames of specific main groups (IA, IIA, VIIA, VIIIA).
Write the name of an element by its chemical symbol (or vice versa).
Chapter 6:
Know what nomenclature is.
Know the seven elements whose chemical formula is a diatomic molecule (i.e. hydrogen-H2).
Be able to either write the chemical name or formula for the following categories:
1. Acids (Binary and Oxyacids)
2. B inary Compounds (Type I and Type II (metals with 2 stable charges)
*Including polyatomic ions
3. Molecular Compounds
4. Hydrates
Chapter 7:
Know the relationship between the element to a compound in a substance.
Know and perform calculating molar mass.
Know and perform calculations involving Avogadro’s number (for molecules and/or atoms).
Know and perform converting a substance from grams to moles to atoms or molecules.
Perform percent composition for any element in a substance’s formula.
Understand and perform solving for an empirical formula and/or molecular formula using given
mass percentage’s of all elements in a substance.
Chapter 11:
Understand the electromagnetic spectrum with respects to its corresponding radiations (units
of wavelength, frequency, or energy).
Understand why any form of light travels at a velocity= 3.00 x 108 m/s.
Know why each form of radiation contains a packet of energy known as photons.
Understand the Bohr model of a hydrogen atom.
Understand excitation and emission with regards to the movement of an electron in the Bohr’s
model.
Understand the term quantized with regards to energy.
Understand the Quantum-Mechanical model with regards to many electron atom.
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Dr. Han
Know the terms n (principle quantum number), l (electron orbitals [s, p, d, f]), and ranking the
orbitals in units of energy (i.e. 2s < 2p; 3s < 3p < 3d [lowest < ==== highest])
Understand the Pauli exclusion principle.
Perform writing electron configuration for any atom (both complete or noble gas configuration)
from atomic number #1-#56.
Determine the number of valence electrons for any element.
Know trends for the following characteristics with the aid of the periodic table:
a) Atomic Radius
b) Ionization Energy
c) Metallic Character
Know properties for both metals and nonmetals.
Know what isoelectronic means in regards to electronic configurations.
Draw the Lewis dot structure for any element (main group elements only).
NOTE: Students MUST know all of the prefix conversions (i.e. 1000g = 1kg, 10 mm = 1 cm, etc.)
and I will assist US-metric and US equalities as needed), Review WORKSHEETS and/or labs
relevant to chapters 5-7 & 11.
Also, look at the assigned problems at OWL and in your textbook. Make sure you understand
the concepts relative to the question in each section. Good luck!!!
LA City College
Dr. Han
PRACTICE Problems
This is just to see how you would handle the short answer, fill-in, and problem solving portion
of the exam. Expect no key to be provided. If you’re struggling with any of these questions,
please refer back to your textbook and reread the section which best explain the concept(s) of
the question.
1. Write the chemical name or chemical formula for each substance.
Zn3(PO4)2 _____________________________
mercury(I) nitrate __________________________
CuO ___________________________________
diphosphorus tetrachloride ________________
BI3 _____________________________________
bromous acid________________________________
HCN __________________________________
hydrosulfuric acid __________________________
Mg(MnO4)2 ___________________________
silver peroxide ______________________________
Zn(NO3)2 · 9H2O ______________________
iron (II) sulfide _____________________________
2. An aluminum cylinder has a volume of 54.11 cm3. If the density of aluminum is 2.70
g/cm3, how many aluminum atoms occupy this cylinder?
3. An organic molecule comprises of 49.48% C, 5.19% H, 28.85% N, and 16.48% O. If the
molecular weight of this compound is 194.19g/mol, what is the molecular formula of this
substance?
4. How many grams of aluminum are in 344.6g of aluminum oxide?
LA City College
Dr. Han
5. Write the electron configurations (complete and noble gas) for the following elements?
Ag
Mn
Zn
In
Sr
6. In the jewelry business, 200. mg of carbon = 1 carat. A customer purchases a 24-carat
diamond ring (most in carbon). How many carbon atoms are present in this ring?
7. How many molecules of butane are present in 25.0 mL of butane? The density of butane
is 0.6011g/mL and the molecular formula of butane is C4H10.
8. In a laboratory experiment, a student burned a 2.465-g sample of copper, which reacted
with oxygen from the air to form an oxide of copper. This metal oxide weighed 2.775g.
Determine the empirical formula of this compound and name this compound.
HINT: You will need to use the law of conservation of mass to find the mass of oxygen.
HINTS:
Useful Conversions:
1 in. = 2.54 cm
1 yd. = 3 ft.
12 in = 1 ft.
16 oz. = 1 lb.
453.59g = 1 lb.
2000 lbs. = 1 ton
956 mL = 1 quart
1 qt =32 fl oz.
1 gallon = 3.785L
5280 ft. = 1 mile