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Final

CHEM 1201 Study Guide - Final Guide: Scantron Corporation, Bicarbonate, Sulfur Trioxide


Department
Chemistry
Course Code
CHEM 1201
Professor
Mamdouh Shoukri
Study Guide
Final

Page:
of 5
CHEM 1201 GROUP FINAL EXAM
Time: 10:00 AM- noon
Date: Saturday December 13, 2014
Venue for Dr. Pathaks sections:
Section 001: 143 Coates
Section 020: 152 Coates
NOTE:
The following pages were given to me by Dr.
Patrick Kolniak. Dr. Kolniak has compiled them
together as a review for the final exam.
Please read everything very carefully.
Good luck and wish you success!
Dr. Priya Pathak
What follows is by Dr. Kolniak.
1. STUDY ALL Problems from your exams
especially, the problems missed & notes. Don’t
just read the solutions; work the problems out
touching your calculator. (First)
2. Work your blank exams until u make 104%
3. STUDY material emphasized in review.
4. Workout Old finals (Last) esp against the clock
5. Be on Time/Early.
6. Bring ID/drivers license, CALCULATOR, #2
pencils, large scantron.
Review Notes for CHEM 1201:
IT IS A FINAL IT IS COMPREHENSIVE -- YOU HAVE TO Prepare/STUDY
Reasons why some students may not study and bomb the final:
1. They are not here (for the review)
2. Only study the night before, stay up all night (result they panic for 24 hrs)
3. Go out the night before
4. Oversleep-miss the final or arrive late
5. They need to bring up their grade in another class and study less for chem (usually
those taking a biology, physics and/or calculus final)
6. Only need to make a D on the final to keep an A…”And I have never failed an exam”
7. Made A’s on all their exams, I don’t need to study much…”And I have never failed an
exam”
Q: What do I need to make on the final exam? A:100%
Preparation = Confidence, Not prepared = Not confident, F. Some of the questions on the final (~7/40)
are mine the rest are from everyone else, if you are not confident & prepared from studying then
when you come across someone else’s wording, you will get confused, then you 2nd guess yourself, then
you panic, then you blackout, then you bomb the final. So prepare!
There are usually 3-4 what the heck questions, but they are what the heck for everyone else and
become part of the curve, so expect that and prepare to look past that. But select best answer.
Chapter 1 Sig Figs’s – zeros in front don’t count (0.012 is two sig.fig’s)
Mult & Div: answer depends on the number of Sigs
Density = mass (g)/volume (ml or cm3) 100cm = 1 m, 1000g = 1 kg
Other Units of conversion:
1 kilo = 1 x 103
1 milli = 1 x 10-3
1 micro = 1 x 10-6
1 nm = 1 x 10-9m
1 pm = 1 x 10-12m
1 fm = 1 x 10-15m
Chapter 2
Isotope Problem-
Atomic # (Z) = number of protons
Mass # (A) = # protons + # neutrons
# neutrons = big little #
Molecular vs. Ionic compounds (recognize) all nonmetals vs metal + nonmetal
Naming compounds- molecular compounds get greek prefixes;
Know Common ions! Some common acids: acetic CH3COOH, Carbonic H2CO3
Transition metals with multiple oxidation states get roman numerals. Naming compounds wit
hydrogen HCO3
- = hydrogen carbonate ion etc.
Ionic compounds- know the most common ions.
1. per__ate (extra O) acids: per __ic acid
2. ___ate (point of reference) acids: __ic acid
3. ___ite (remove O) acids: __ous acid
4. hypo___ite (remove another O) acids: hypo __ous acid
SO4
-2 is sulfate, H2SO4 is sulfuric acid; ClO- hypochlorite, HClO is hypochlorous acid
Non oxy acids are hydro__ic
Chapter 3
Balance-Given the names of the reactants-complete the reaction and Balance Goes back to naming
above- need same number of elements on both sides of the equation; don’t forget to multiply
coefficients and subscript’s in a formula. Ex: 2NaNO3 means 2 Na’s and 2 N’s and 6 O’s.
Mass to moles or moles to mass Use MM
Mole/Avogadro: 1 mole of something = 6.02 x 1023 something and grams/MM= mol
The number of molecules = mol of substance*Avog. Number (molecules per mol).
The number of atoms = mol of substance*Avog. Number (molecules per mol) *Number of atoms per
molecule.
Avogadro from Molarity (need moles) = M*L = mol
The number of molecules = mol of substance*Avog. Number (molecules per mol).
The number of atoms = mol of substance*Avog. Number (molecules per mol) *Number of atoms per
molecule.
Hint: See 2nd example page 32 chap 3 notes- Atoms of Fe one…
Empirical Formula from %by Mass: Assume 100 g, get moles, ratio, adjust if fraction
Limiting Reagent Problem (more work) Determine moles of reactants; divide moles of reactant by
its coefficient the smallest number wins- it’s the limiting reagent. The moles of limiting reagent
times the coefficient of the product gives moles of product; then moles of product times the molar
mass of product gives you the grams of product.
Chapter 4
Electrolytes
STRONG: soluble salt or strong acid/strong base
SA: HCl, HBr, HI, HClO4, H2SO4, HNO3
SB: LiOH, NaOH, KOH, RbOH, CsOH
WEAK: weak acid or weak base
Weak acids can be organic in nature. Usually of the form HCxHyOz underscored
proton gets donated.
Weak bases can be organic in nature and usually include nitrogen (because of the
lone pairs) in the form of CxHyNz.
NonElectrolyte: molecular compound
Molarity is the moles of solute per liter of solution. (moles/Liter).- Det MM
Be able to calculate M from grams & volume or other combination.
Remember the rearrangement of units for molarity: M = mol/L
reactants
products
Given grams
?
MM
?
Calc Moles
LRxcoef
Coef from
reaction
Calc eqiv
Divide on the
way down to
determine the
limiting reagent
Multiply on the way up
to determine the grams
of product using
stoichiometry