Supplemental Instruction
Iowa State University / Leader: / Matt H
Course: / Chem 177
Instructor: / DrHolmeDrAwino
Date: / 9-10-17
What is likely to be on the Exam?
-Temperature Conversions
-Unit Conversions
-Sig Figs
-Ionic and Covalent Bonding, isotopes
-Parts of an Atom: proton, neutron, electron
-Nomenclature: compounds, polyatomic ions, acids
-Average atomic masses
-Balanced chemical equations
-Combustion
-Basic Stoichiometry and the Mole
Strategies for Success
-do lots of practice tests. You will notice trends between tests
-Relax. Sometimes the first question on the test is purposely intimidating.
-As always, skip questions and come back if you are stuck
Ways to Practice
-Practice Tests: Available on SI website
-old SI worksheets
-google worksheets online over certain subject
-confused on a topic? Khan Academy is great!
Provided
-Periodic Table
Memorize
-Polyatomic Ions
-Diatomic Ions
-Metric prefixes
-Equations for Temperature, Density…
-Avogodro’s Number
Chem 177 Equation Sheet
Exam 1
Exam 2
M = mols / L
Exam 3
Formal Charge = Val e - nonbonding e - bonds
BO = Total Bonds / Bonding Locations
ΔH = Bonds Broken - Bonds Formed
Post Exam 3
Electron Domains = lone pairs + bonding locations
STP = 1 atm 0ºC 1 atm = 760 torr = 760 mmHg = 1.013 x 105 Pa
1. In the following list, only ______is not an example of a chemical reaction.
a. dissoulution of penny in nitric acid
b. condensation of water vapor
c. burning a candle
d. formation of polyethylene from ethylene
2. Which famous chemist in 1803 wrote the Atomic Theory describing the nature of matter?
a. Rutherford
b. Dalton
c. Avogadro
d. Mendeleev
3. One mole of which contains the most atoms?
a. hydrogenb. calciumc. silverd. one mole of anything contains the same #
4. Which of these is the highest temperature?
a. 94 ° F b. 39 ° Cc. 300 K
5. The following measurements of a pencil were taken by 3 students. The pencil is actually 5 cm long. Which set of measurements represents accuracy, which represents precision, and which represents neither.
[ 3.9, 3.8, 4.0 ][ 5.2, 6.8, 5.7 ][ 5.1, 4.8, 5.2 ]
6. Which of the following is a metalloid?
a. Aluminum b. Silicon c. Sulfur d. Selenium
7. What is the charge on the phosphate ion?
a. -1b. -2c. -3d. neutral
8. What is the formula for Chromium (II) Bromide?
a. CrBr b. CrBr2c. Cr2Brd. Cr2Br2
9. Fill the table
Charge / Mass (amu) / Location in Atom / When happens to atom when you change amountProton
Neutron
Electron
10. Count the number of Sig Figs
0.002700.005170.0560
7000.6.022 x 10233.00 x 1089.11
11. ______boning is the transfer of electrons, where ______bonding is the
sharing of elections.
12. Which atom has the largest number of Neutrons?
a. 40Ar
b. 39 K
c. 40 Ca
d. 35Cl
13. List the seven diatomic molecules
14. Name the following Polyatomic Ions and Acids they form
CO4 2-
CO3 2-
CO2 2-
CO2–
15. Write name or chemical formula for the following. Are they ionic or molecular?
a. N2O5
b. Barium Sulfite
c. NBr3
d. Hydroiodic Acid
e. NaClO
f. Fe2(CO3)3
g. LiOH
h. MgSO3
i. HClO4
j. Hypochlorous acid
k. P2O5
l. Lithium Fluoride
m. Chromium (III) Acetate
16. What is the percent composition by mass of O in dinitrogen pentoxide?
17. Convert 65 mph to m/s. (1 mi = 5280 ft) (3.3 ft = 1 m)
18. What are the products and reactants in…
Complete Combustion:
Incomplete Combustion:
19. Write a Balanced Chemical Equation for the Complete Combustion of ethane( C2H6 )
20. Chlorine has an average atomic mass of 35.450amu, which is calculated from the two isotopes of Cl. Isotope A: 34.969 amu Isotope B: 36.966amu
What are the percent compositions in nature of isotope A and B?
21. Count the total number of atoms in .111 mol Fe(CO)3(PH3)2
22. How many hydrogen atoms are in 17 g of CH3COOH (acetic acid)?
23. How much mass is 125 billion atoms of copper?
24. A solution of ammonia and water contains:
34.8moles of water
8.10 x 1024ammonia molecules
How many total hydrogen atoms are in the solution?
25. A certain box contains 6.0 kg of water. The box width and height are 18 cm and 15 cm respectively. What is the height of the box?
Advanced Stoichiometry: Probably not on Exam 1
26. The following is a step in the commercial process of converting ammonia into nitric acid.
4NH3 (g) + 5 O2 (g) 4NO (g) + 6H2O (g)
In this experiment, 2.00 g of NH3 reacts with excessO2
a. How many grams of NO and H2O are produced?