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Chemistry 106 Expectations
As the title indicates, these are what I would expect of you, when you come into the classroom.
These should be common sense, but I am reiterating them for students. I also provide what you
can expect of me.
Buzz Piersol
Daily Classroom Expectations of Students
Regularly attend class
Arrive to class on time
Read and understand the syllabus and policies within
Be aware of campus policies and be familiar with the PC catalog
Cell phone is off or set on vibrate/silent
Bring all materials to every class meeting: pencil, notebook, calculator, textbook
Do not bring or eat food/drink to class (water OK)
Retain all handouts throughout the semester
Read the textbook
Perform homework/lab assignments on time
Prepare for quizzes/mid-term/final exam
Contact instructor outside of class, if making below-than-average progress
Be prepared to learn and participate
Daily Laboratory Expectations of Students
Arrive to lab on time
Turn cell phone off or set it to vibrate/silent
Bring/Borrow and wear safety goggles during experiments
Wear closed-toe shoes (i.e. not sandals)
Do not wear loose/dangling jewelry or loose clothing
Tie-back long hair.
Read the procedure and follow instructions for daily experiment
Notify instructor of any accident/spill/fire (including glass breakage)
Do not eat/drink in the laboratory
Be prepared to learn and participate
What Students Can Expect of the Instructor
Arrive to class/lab on time
Frequently invite questions, and answer all questions
Communicate with students respectfully
Be prepared for daily activity/lecture/laboratory with all supporting/necessary
materials.
Return laboratory assignments in a reasonable amount of time.
Return exams in a reasonable amount of time.
Regularly notify students of progress
Assign grades fairly, according to the syllabus, and high academic standards
Encourage student learning
CHEM 106 Summer 2016
Online Homework – Sapling Learning
Philosophy
Your online homework was selected and tailored with student learning in mind. Often, students
do their homework at home or away from the college, so they do not have access to the
professor. When they have trouble, they can either contact the professor by email or wait until
the next class meeting. Online homework allows immediate feedback and encourages online
contact with the instructor. Sapling Learning was selected for online homework for many
reasons. They specialize in chemistry homework. The assignments also provide hints and
assistance in a stepwise fashion—this makes learning with homework a better experience.
Purchase
You can purchase the online homework in one of two ways. You can purchase a physical package
in the bookstore or online when you register.
Registration
When you register with sapling, you can use your email address or a Facebook account (details
below). If you choose email, it is recommended that you use your Porterville College email
account. Be sure to enter your email address correctly when you register—this is a very
important step! The PC email typically has a pattern
“your.name####@email.portervillecollege.edu”. It is easy to mistype at least one character
incorrectly. See below for registration.
1. Go to https://www.saplinglearning.com/ibiscms
2. If you already have a Sapling Learning account, log in then skip to step 4, otherwise, click
CREATE AN ACCOUNT.
3, If you have Facebook account, you can use it to quickly create a Sapling Learning account,
otherwise, fill in the fields and register a new account.
4. Find your course in the list (you may need to expand the subject and term categories) and
click the link.
5. Use the bookstore package to register for the online homework or select a payment option
and follow the remaining instructions.
Once you have registered and enrolled, you can log in at any time with any computer on the
internet to review and complete or your homework assignments. During sign up - and
throughout the term - if you have any technical problems or grading issues, send an email to
[email protected] explaining the issue. The Sapling support team should be able
to help with support issues. If you have homework questions, email Buzz at
[email protected] or text at 559-791-8346.
CHEM 106 Homework Assignments (mostly online)
Week Assignment
Available Date
Due Date
1
Practice Assignment
Wednesday, June 01
Wednesday, June 15
1
Math Review
Wednesday, June 01
Wednesday, June 15
1
HW1&2
Wednesday, June 01
Wednesday, June 15
1
HW2&3
Wednesday, June 01
Wednesday, June 15
2
HW4
Monday, June 06
Monday, June 20
2
HW11
Wednesday, June 08
Wednesday, June 22
3
Practice Drawing Molecules
Wednesday, June 08
--
3
HW12
Monday, June 13
Monday, June 27
3
HW5
Wednesday, June 15
Wednesday, June 29
4
HW6&7
Monday, June 20
Tuesday, July 5 *
4
HW8
Wednesday, June 22
Wednesday, July 6
5
HW9
Monday, June 27
Monday, July 11
5
HW13
Wednesday, June 29
Wednesday, July 13
6
HW14
Monday, July 4
Monday, July 18
6
HW15
Wednesday, July 6
Wednesday, July 20
* HW6&7 assignment due on July 5 as July 4 is a holiday (Independence Day)
6/6/2016 Conversion Factors
NOTE: All equalities are EXACT (i.e. ∞ number of SF), except those marked with an asterisk (*)
ENGLISH/US SYSTEM Be familiar with each unit, abbreviation and equality below.
Mass
Length
Volume
1 ton = 2000 lb (pounds)
1 lb = 16 oz (ounces)
1 mi (mile) = 5,280 ft (feet)
1 yd (yard) = 3 ft
1 ft = 12 in (inch)
1 gal (gallon) = 4 qt (quart)
1 qt = 2 pt (pint)
1 pint = 2 cups
1 qt = 32 fl oz (fluid ounces)
COMMON METRIC SYSTEM BASE UNITS
SI SYSTEM UNITS
Length:
Mass:
Volume:
Length:
Mass:
Time:
Temperature:
meter (m)
gram (g)
liter (L)
meter (m)
kilogram (kg)
second (s)
kelvin (K)
Any unit can be modified by by adding a prefix to a base unit. The value of the prefixed unit is the numerical
equivalent of the base unit (e.g. 1 µL = .000001 L)
PREFIX
mega
kilo
deci
centi
milli
micro
nano
ABBR
M
k
d
c
m
µ
n
NUMERICAL EQUIVALENT
106 or 1,000,000
103 or 1,000
100 or 1
10-1 or .1
10-2 or .01
10-3 or .001
10-6 or .000,001
10-9 or .000,000,001
TEMPERATURE CONVERSIONS:
TF = 1.8TC + 32
TC =
TF − 32
1.8
TK = TC + 273
TC = TK − 273
OTHER IMPORTANT METRIC EQUALITIES:
1 cubic centimeter (cm3) = 1 mL
1 angstrom (Ǻ) = 10-10m
ENGLISH - METRIC BRIDGE EXAMPLES
Mass
1 lb = 453.6 g *
1 kg = 2.205 lb *
Length
1 in = 2.54 cm
1 m = 1.094 yd *
1 mi = 1.609 km *
Volume
1 L = 1.0567 qt*
3
1 ft = 28.32 L *
Drawing Simple Lewis Structures
1. Count valence electrons contributed from all atoms.
a. For anions, add one electron for each negative charge.
b. For cations, subtract one electron for each charge. Use this number of
electrons exactly for bonding and non-bonding in the structure.
These electrons must be distributed to all atoms such that each has an octet
except hydrogen (“duet”).
2. Place atoms around a central atom (lone atom, or the atom with the lowest
Electronegativity).
3. Place one bond (2 electrons) between each outer atom and the central atom.
Subtract from the original electron count.
4. Place lone pairs (2 unshared electrons—non-bonding electron pairs) on the outer
atoms (except H), until each has satisfied the octet or until there are no more
remaining. Subtract from the count as you use them.
5. If there are remaining electrons, place them on the central atom, in pairs.
Subtract electrons used.
6. If the central atom does not meet the octet, then share previously assigned
nonbonding electrons from outer atoms to form double and triple bonds.
Valence Shell Electron Pair Repulsion Theory
Groups
0 Lone Pairs
1 Lone Pair
2 Lone Pairs
180°
2
Linear
120°
3
<120°
Trigonal
Planar
Bent
109.5°
4
<109.5°
Tetrahedral
Trigonal
Pyramid
Note: any structure with just two atoms bonded is linear
<109.5°
Bent
NOMENCLATURE CHART
OXYACIDS AND THEIR ANIONS
Acids (name of compound)
Anions (form latter part of name of ionic compound)
HNO3
NO3−
nitrate
−
nitrite
nitric acid
HNO2
nitrous acid
NO2
HClO4
perchloric acid
ClO4−
perchlorate
−
chlorate
HClO3
chloric acid
ClO3
HClO2
chlorous acid
ClO2−
chlorite
HClO
hypochlorous acid
ClO−
hypochlorite
HC2H3O2
acetic acid
acetate
H2CO3
carbonic acid
C2H3O2−
HCO3−
H2SO4
sulfuric acid
HSO4−
H2SO3
sulfurous acid
HSO3−
H3PO4 phosphoric acid
Each of these 4 ions and 4 acids
form similar structures and names
for Br, and I instead of Cl.
hydrogen carbonate or
bicarbonate
CO32−
carbonate
hydrogen sulfate or
bisulfate
hydrogen sulfite or
bisulfite
SO42−
sulfate
SO32−
sulfite
H2PO4- dihydrogen phosphate
HPO42− hydrogen phosphate
PO43− phosphate
BINARY & OTHER NON-OXYACIDS AND THEIR ANIONS
HF(aq)
hydrofluoric acid
F−
fluoride
HCl(aq)
hydrochloric acid
Cl−
chloride
HBr(aq)
hydrobromic acid
Br−
bromide
HI(aq)
hydroiodic acid
I−
iodide
H2S(aq)
hydrosulfuric acid
S2−
sulfide
HCN(aq)
hydrocyanic acid
CN−
cyanide
MISCELLANEOUS IONS
H−
OH−
MnO4
−
CrO42−
Cr2O7
2−
O22−
AsO4
GREEK PREFIXES (BINARY MOLECULAR CPDS)
hydride
NH4
hydroxide
+
ammonium
1
mono-
6
hexa-
Ag+
silver
2
di-
7
hepta-
permanganate
Zn2+
zinc
3
tri-
8
octa-
chromate
Cd2+
cadmium
4
tetra-
9
nona-
dichromate
Al3+
aluminum
5
penta-
10
deca-
peroxide
3−
arsenate
it's the only non-metal cation we will see!
VARIABLE VALENCE (CHARGE) METAL IONS
Ion
stock name
traditional name (for information only)
Cu1+
copper(I)
cuprous
Cu2+
copper(II)
cupric
mercury(I)
mercurous
Hg2+
mercury(II)
mercuric
Au1+
gold(I)
aurous
Au3+
gold(III)
auric
Cr2+
chromium(II)
chromous
Cr3+
chromium(III)
chromic
Mn2+
manganese(II)
manganous
Mn3+
manganese(III)
manganic
Fe2+
iron(II)
ferrous
Fe3+
iron(III)
ferric
Co2+
cobalt(II)
cobaltous
Co3+
cobalt(III)
cobaltic
Ni2+
nickel(II)
nickelous
Ni3+
nickel(III)
nickelic
Sn2+
tin(II)
stannous
Sn4+
tin(IV)
stannic
Pb2+
lead(II)
plumbous
Pb4+
lead(IV)
plumbic
Hg2
2+
(Note: This is the only metal polyatomic ion!)
Anions end in -ide
Cation name is same as element
1A
COMMON IONS BASED ON PERIODICITY
3A 4A
2A
5A
6A
7A
H
+
Li
Na
+
N
2+
3+
Mg
Al
3B
K
+
Rb
+
+
Cs
Ca
Sr
2+
4B
5B
6B
7B
8B
1B
2B
Cr2+
Cr3+
Mn2+
Mn3+
Fe2+
Fe3+
Co2+
Co3+
Ni2+
Ni3+
Cu+
Cu2+
Zn2+ Ga3+
P
3-
O
2-
2-
S
-
F
-
Cl
Br
2+
Ag+ Cd2+ In3+
Sn2+
Sn4+
2+
Au+ Hg22+
Au3+ Hg2+
Pb2+
Pb4+
Ba
3-
-
I
-
-
8A
Inorganic Nomenclature Guidelines
First determine whether you compound is an ionic compound, an acid, or binary
molecular.
Ionic Compound – starts with a metal or ammonium (NH4+). Go to procedure 1.
Acid – Starts with H (except H2O and H2O2). Go to procedure 2.
Binary Molecular – Two non-metal elements. Go to procedure 3.
1. Ionic Compound: Name is “cation anion”. Determine the names each of the
cation and anion. Divide the formula into the cation and anion. Use the
formulas to determine the names of each.
a. Name cation. Simple metal, variable valence or NH4+?
i. Simple metal: Cation is the name of the element.
ii. Variable valence: Determine the charge of the metal by looking
at the charge of the anion and the formula subscripts. Roman
numeral name of cation will be element (charge) where charge is
a roman numeral (without plus sign!). Classical name ends in “–
ous” if lower charged metal and “–ic” if higher charged.
iii. NH4+ cation name is ammonium.
b. Name anion. Is the anion a Non-metal or polyatomic anion?
i. Non-metal anion: Anion name is name of the element with “–ide”
ending.
ii. Polyatomic ion: Oxyanion or other?
1. Oxyanion: Name derived from the name of the non-metal
that oxygen is paired with. Larger subscript of oxygen in a
series name ends in “–ate.” Smaller subscript of oxygen in
a series name ends in “–ite.” See Oxyanion tips.
2. Other: Some other polyatomic anions include CNcyanide, OH- hydroxide, peroxide O222. Acid: Last word of acid name is always “acid.” Determine whether the acid
has oxygen or not:
a. Oxyacid: Name derived from non-metal that accompanies the oxyanion
i. “–ate” oxyanion becomes “-ic acid” (higher number of oxygens)
ii. “–ite” oxyanion becomes “-ous acid” (lower number of oxygens)
b. Non-Oxyacid: Name starts with “hydro-“ and the rest of the name is
derived from anion: “-ide” becomes “hydro[anion]-ic acid”
3. Binary Molecular: Two non-metals. Name is composed of two words:
a. First word is the first element in the formula. Second word is the second
element with the usual modified “-ide” ending.
b. Prefixes are added to each word based on the subscript of each
element. Refer to Greek prefix table (e.g. tri = 3 atoms)
c. Prefix exception: Mono is never used on the first word regardless if
there is one atom of that element. (e.g. carbon monoxide not
monocarbon monoxide)
d. Prefix vowel omitted if similar vowel sounds run together by addition of
the prefix. (e.g. carbon monoxide NOT carbon monooxide)
Notes:
Be aware of the following compounds, which use a common name. Common
names do not follow systematic (IUPAC) procedure:
H2O water
H2O2 hydrogen peroxide
NH3 ammonia
CH4 methane
Oxyanion Tips:
•
•
•
•
•
•
•
•
Oxyanion names will always end in –ate or –ite. Since oxyanions are
anions (negatively charged ions), they will always be found paired with a
cation and form the latter part of a name and formula.
Do not confuse the naming of oxyanions (end in –ate or –ite) with the
naming of binary molecular compounds because they have similar
formulas. Binary molecular compounds are named using the greek
prefixes.
Do not allow other instances of Greek or similar prefixes to confuse use in
naming some of the oxyanions. For example, Cr2O72- is named dichromate.
This has nothing to do with the naming of binary molecular compounds.
There are a few instances of oxyanions series for a non-metal with two
-
-
possible anions (e.g. NO3 , NO2 ). Remember the higher number of
oxygens name ends in –ate.
Most oxyanions with just one type in their series (e.g. only one type with
Carbon and Oxygen: CO32-) will end in “-ate.”
Cl, Br, and I each all form four oxyanions with the pattern (XO4-, XO3-, XO2-,
XO-) where X=halogen and names respectively (per____ate, ____ate,
____ite, and hypo____ite). Fill the halogen name (or shortened name in
each blank.
Recall oxyanions that are charged –2 and –3 form hydrogen-containing
polyatomic ions as well (e.g. HPO42- hydrogen phosphate).
Remember all common acids dissolve in water. The prefix “hydro” does not
necessarily indicate that it is an acid. Hydro means that the acid does not
contain the element oxygen. Oxoacids do not begin with the prefix “hydro.”
Chemical Equations and Balancing
Write and Balance
1. If the equation is not written out, first write the chemical equation using names
for each substance involved (reactants
products).
2. Rewrite the equation by translating each word into the correct symbol or
formula, indicating the state or condition after each (s), (l), (g), or (aq).
3. Balance the equation:
a. Count up the total number of each atom in all formulas on each side of
the equation.
b. Balance any unbalanced atom by placing the necessary whole-number
coefficient in front of the appropriate symbol or formula. The coefficient
applies to the entire formula. Never change the subscript of a
formula!
c. Often, step b will unbalance another atom. Repeat steps a & b until all
atoms are balanced.
d. The equation is balanced when there is the same number of atoms of a
given type on each side of the equation.
Equation Formulation Tips
a. The “formula” of any uncombined element is its symbol (e.g. Copper is Cu),
except for the diatomic elements (H2, N2, O2, F2, Cl2, Br2, I2).
b. The state of any element is solid, except:
a. Hg, Br2 are liquids
b. H2, N2, O2, F2, Cl2 are gases (as well as with the noble gases)
c. Ionic compounds are in the solid state, except that they are usually dissolved
in water, thus are aqueous (aq).
Balancing Tips
a. A rule of thumb for the order of balancing atoms is: Balance metals first, then
non-metals, then hydrogen, then oxygen.
b. Use the principle of Least Common Multiple to balance atoms.
c. An uncombined element in the equation is good to balance last.
d. Polyatomic ions that are present on both sides of the equation can be counted
as a whole unit for ease. This is especially useful for double replacement
reactions.
e. Remember to multiply coefficients & subscripts, when counting atoms, for
example:
3Ca3(PO4)2
has a total of ___ calcium ___ phosphorus ___ oxygen atoms
cpiersol –2015.10.13
Piersol 10-17-2012
All Reactions
Double Replacement
Oxidation-Reduction
Precipitation
Combination (Synthesis)
Acid-Base
Decomposition
Reactions may have more than one classification,
but the following are mutually exclusive:
Double Replacement and Oxidation-Reduction
Single Replacement
Combustion
Synthesis and Decomposition
Other
2H2(g) + O2(g) 2H2O(g)
HNO3(aq) + KOH(aq) KNO3(aq) + H2O(l)
Pb(NO3)2(aq) + KI(aq) PbI2(s) + KNO3(aq)
KClO3(s) KCl(s) + O2(g)
C6H12O6(s) + 6O2(g) 6CO2(g) + 6H2O(g)
2H2O(g) 2H2(g) + O2(g)
Zn(s) + 2HCl(aq) ZnCl2(aq) + H2(g)
2Zn(s) + O2(g) 2ZnO(s)
2H2(g) + O2(g) 2H2O(g)
combination (synthesis)
combustion
oxidation-reduction
HNO3(aq) + KOH(aq) KNO3(aq) + H2O(l) acid-base
double-replacement
Pb(NO3)2(aq) + KI(aq) PbI2(s) + KNO3(aq) precipitation
double-replacement
KClO3(s) KCl(s) + O2(g)
decomposition
oxidation-reduction
C6H12O6(s) + 6O2(g) 6CO2(g) + 6H2O(g)
oxidation-reduction
combustion
2H2O(g) 2H2(g) + O2(g)
decomposition
oxidation-reduction
Zn(s) + 2HCl(aq) ZnCl2(aq) + H2(g)
single-replacement
oxidation-reduction
2Zn(s) + O2(g) 2ZnO(s)
oxidation-reduction
combination (synthesis)
combustion
Empirical Formula Determination (in 4 or 5 easy steps)
1. If given percent composition, take each percentage in grams (as if using a 100-gram
sample).
2. Convert each element from grams à moles
3. Divide each element by the smallest number.
4. If the numbers are reasonably whole numbers, round each and use as subscripts.
Otherwise, go to then next step.
5. Determine which decimal ending is close to that in the table below and multiply
each by the common denominator.
Principle of Common Denominator
decimal
(approximate)
Multiply each by
denominator:
ending
fraction
0.25
1/4
4
0.33
1/3
3
0.50
1/2
2
0.67
2/3
3
0.75
3/4
4
Stoichiometry Chart
molar
mass
mole
ratio
Moles A
Grams A
A
molar
mass
Grams B
Moles B
(equation)
B
PV=nRT
n = PV
RT
Gas A
Gas B
• “A” represents the known quantity of substance A, which
can be a reactant or product.
• “B” represents an unknown quantity of substance B, which
can be a reactant or product.
Chemistry P106 Final Fact Sheet
Important Stuff:








Bring a pencil.
Bring a scientific calculator.
Bring a card no larger than 3”x5” filled with any desired information
Bring a green scantron sheet with your name written on it.
Use the restroom before you begin taking the final exam.
Turn your cell phone off before you begin taking the final exam.
Review 8 – 9:40 a.m. Thursday, July 21
Final Exam 10 a.m. – 12:15 p.m. Thursday, July 21
Majority of Topics Covered on the Final Exam:
Chapter 1




– Introduction to Chemistry
Terminology
Scientific Method
Physical and chemical change
Physical and chemical properties
Chapter 2





- Measurement
Metric System
Conversions
Significant Digits (Figures)
Temperature Conversions
Density
Just the
facts, ma’am!
Chapter 3 – Matter
 Classify matter: Elements, compounds, substances, homogeneous or heterogeneous
mixtures
 Physical vs Chemical Change/Properties
Chapter 4




– Elements, Atoms, Ions
The 3 subatomic particles and their properties (mass, charge)
Atomic number (= number of protons)
Isotopes (same atomic number, different numbers of neutrons)
Periodic Table classification (alkali metal, alkaline earth metals, etc)
Chapter 5 – Nomenclature
 Responsible for naming compounds that contain the following anions: sulfate, sulfite,
nitrate, nitrite, chlorate, chlorite, and halides (e.g. bromide)
 Name binary molecular (2 non-metals; uses Greek prefixes)
Chapter 6



& 7 – Chemical Equations
Principles, descriptors, coefficients
Balancing equations
Determine reaction type: combustion, double replacement (precipitation or acid/base),
combination (synthesis), decomposition, redox
Chapter 8





– Chemical Composition
Avogadro’s number : 6.022 X 1023 = 1 mole
Convert between any of the following: grams, moles, atoms, molecules
Molar mass
Percent composition
Empirical formula calc
Chapter 9





– Chemical Reaction Quantities (Stoichiometry)
Convert moles A  Moles B
Convert grams A Moles B
Convert grams A grams B
Theoretical yield vs. actual yield
Limiting Reactant
Chapter 11 – Modern Atomic Theory
 Orbitals defined
 Electronic configuration of the elements
 Valence electrons
 Periodic Table – Classification by electron config / valence electrons
 Trends: atomic radius, ionization energy
Chapter 12 – Chemical Bonding
 Covalent vs. ionic bonding (electronegativity trend)
 Draw Lewis structures: polyatomic ions, molecules
 Single, double, triple bonds
 Unpaired (non-bonding) electrons
 3D Structures (VSEPR theory—geometries, bond angles, sketch structure)
 Bond and molecular polarity
Chapter 13 – Gases
 Gas Laws:
Boyle’s Law (P1V1 = P2V2)
Charles’ Law (V1/T1 = V2/T2)
Avogadro’s Law (V1/n1 = V2/n2)
Ideal Gas Law: PV = nRT
Dalton’s Law of Partial Pressures: Ptot = P1 + P2 + P3 + …
 Gas Stoichiometry
Chapter 14 – Solids, Liquids
Heating/Cooling curve (sketch & label)
Intramolecular vs intermolecular forces
Intermolecular forces: (DD, HB, LD), and predict properties trends
Vapor Pressure
Types of solids (Ionic, Molecular, Atomic)
Chapter 15 – Solutions
 Solution = solute + solvent (definitions)
 Calculate mass percent solution
 Calculate molarity from (grams or moles) solute, and volume solution
 Calculate moles from molarity and volume, and convert to grams if needed.
Also, know what each of these scientists contributed to chemistry: Dalton,
J.J. Thomson, Mendeleev, Rutherford, Bohr, Schrödinger
The Final Exam is worth 20% of
your grade. Don’t forget to study!