Pickett CHEMISTRY – FINAL EXAM REVIEW – 2014-2015 Final Exam Date: D Period: 6/16: 9:50-11:50 C Period: 6/17: 7:30-9:30 PREPARING FOR THE EXAM: Working with others can help, however it is essential that you are able to complete this review on your own . Get help when needed, but solve problems independently. Begin by first reviewing your notes, homework, vocabulary and the textbook. Notes given in class have been posted on the course website as a reference, if needed. After your review, complete as much of this packet as possible on your own , without assistance. For questions that are difficult, review notes, homework and the textbook at least one more time, and then retry the questions. Get assistance from peers or the teacher if needed. Some class time will be available to work on reviewing for the exam, however you will be expected to work on this primarily outside of class. Help will be available at lunch and after school. EXAM REVIEW: Complete the entire review to prepare for the exam. Use the textbook for additional problems if necessary. Any questions that require calculations should be completed with all work. EXAM FORMAT: Keep in mind that these questions are only samples and may not include the specific examples of how vocabulary and other conceptual information might appear on the actual exam. Most questions will be multiple choice questions with four or five answer choices. Work will NOT be graded or checked on those questions. There may be some problems which will require a write-in answer or work for full credit. 1
Transcript
Pickett CHEMISTRY – FINAL EXAM REVIEW – 2014-2015
Final Exam Date: D Period: 6/16: 9:50-11:50
C Period: 6/17: 7:30-9:30
PREPARING FOR THE EXAM:
Working with others can help, however it is essential that you are able to complete this review on your own. Get help when needed, but solve problems independently.
Begin by first reviewing your notes, homework, vocabulary and the textbook. Notes given in class have been posted on the course website as a reference, if needed.
After your review, complete as much of this packet as possible on your own, without assistance. For questions that are difficult, review notes, homework and the textbook at least one more time, and then
retry the questions. Get assistance from peers or the teacher if needed. Some class time will be available to work on reviewing for the exam, however you will be expected to work
on this primarily outside of class. Help will be available at lunch and after school.
EXAM REVIEW:
Complete the entire review to prepare for the exam. Use the textbook for additional problems if necessary. Any questions that require calculations should be completed with all work.
EXAM FORMAT:
Keep in mind that these questions are only samples and may not include the specific examples of how vocabulary and other conceptual information might appear on the actual exam.
Most questions will be multiple choice questions with four or five answer choices. Work will NOT be graded or checked on those questions. There may be some problems which will require a write-in answer or work for full credit.
You will be provided with a periodic table and the attached reference sheet during the exam. You may have one 3x5 card with any notes you choose to have. The card may not
be altered in any way, must be hand-written, and will be turned in after you finish the exam.
Topics covered 7 unitsa. Gas lawsb. Thermochemistryc. Light & electrons, Periodic Trendsd. Chemical Bondinge. Solutions/Liquids & solidsf. Chemical Equilibrium
1
VOCABULARY:
States of MatterSolid ___________________________________________________________________Liquid __________________________________________________________________Gas ____________________________________________________________________
Label the phase change graph:
Be sure to include: Boiling point q=mcΔt Condensation point q=mHv
Freezing point q =mHf
Melting point Solid Liquid Gas Solid liquid Liquid gas
2
Define the following terms:exothermic __________________________________________________________________________________________________________________________________________________________endothermic __________________________________________________________________________________________________________________________________________________________
Gas LawsDefine the following gas laws and indicate whether they involve inverse or direct relationships. Boyle’s Law __________________________________________________________________________________________________________________________________________________________Dalton’s Law__________________________________________________________________________________________________________________________________________________________Charles’s Law__________________________________________________________________________________________________________________________________________________________Kinetic Molecular Theory__________________________________________________________________________________________________________________________________________________________
3
SolutionsDefine the following:miscible __________________________________________________________________________________________________________________________________________________________polar __________________________________________________________________________________________________________________________________________________________nonpolar __________________________________________________________________________________________________________________________________________________________solute__________________________________________________________________________________________________________________________________________________________solvent__________________________________________________________________________________________________________________________________________________________unsaturated__________________________________________________________________________________________________________________________________________________________saturated__________________________________________________________________________________________________________________________________________________________supersaturated__________________________________________________________________________________________________________________________________________________________solubility__________________________________________________________________________________________________________________________________________________________molarity__________________________________________________________________________________________________________________________________________________________
4
BondingDefine the following:covalent__________________________________________________________________________________________________________________________________________________ionic__________________________________________________________________________________________________________________________________________________polar covalent _________________________________________________________________________________________________________________________________________________________VSEPR Theory___________________________________________________________________________________________________________________________________________________Periodic TrendsDefine the following:electronegativity__________________________________________________________________________________________________________________________________________Ionization energy___________________________________________________________________________________________________________________________________________________Atomic Radius___________________________________________________________________________________________________________________________________________________
Light & EnergyDefine the following:wavelength_____________________________________________________________Frequency______________________________________________________________Electromagnetic spectrum_______________________________________________________________________________________________________________________________________________Relationships between the following variables: energy, wavelength, frequency__________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________
Chemistry College Prep Final :Review Problems
SOLUTIONS
1. What is the molarity of:
a. 10.0 Grams of NaCl in 300.0 mLof water?
b. 30.0. grams of MgO is 644mL of water?
c. .50 moles of RbI in 2 liters of water?
2. Define the following:
Saturated-
Unsaturated-
Supersaturated-6
Solute-
Solvent-
Dilute-
Aqueous-
Name the solute and solvent:
a. Apple juice-
b. Carbonated water
7
3. Use the solubility graph to answer the following:
1. What are the customary units of solubility on solubility curves? ___________
3. According to the graph, the solubility of any substance changes as _________ changes.
4. List the substances whose solubility decreases as temperature increases. ___________ ___________________________________________________ 4. Which substance is least affected by temperature changes? ____________________
5. How many grams of ammonium chloride (NH4Cl) at 50°C? ______________________
8
6. _____________ and ____________ have the same solubility at approximately 78oC.
7. Which compound is least soluble in water at 10°C? ___________
8. How many grams of KNO3 can be dissolved at 50oC? __________
9. Are the following solutions unsaturated, saturated, or supersaturated?
GAS LAWSGas Laws Review
Remember sig figs! Show all work.
PV=nRT PV/T = PV/T
1. List 5 characteristics of gases.
2. 1.00 Liter of a gas at standard temperature and pressure is compressed to 473 ml. What is the new pressure of the gas in atm units?
3. If a gas at 25.0 degrees Celsius occupies 3.60 liters at a pressure of 1.00 atm, what will be its volume at a pressure of 2.50 atm?
4. A 1.5 Liter flask is filled with nitrogen at a pressure of 12 atmospheres. What size flask would be required to hold this gas at a pressure of 2.0 atmospheres?
5. You are wearing scuba gear and swimming under water at a depth of 66.0 feet. You are breathing air at 3.00 atm and your lung volume is 10.0 L. Your scuba gauge indicates that your air supply is low, so to conserve air you make a fatal mistake: you hold your breath while you surface. What happens to your lungs? Why? Show work to support your answer.
6. A helium balloon has a volume of 50 L at 25 degrees Celsius and 1.08 atm. What volume will it have at .855 atm and 10 degrees Celsius?
7. At 120 degrees Celsius, the pressure of a sampleof nitrogen is 1.07 atm. What will be the pressure at 205 degrees Celsius, assuming constant volume?
9
Chapter 7 Light & The Quantum Model Review
Remember sig figs! Show all work.
Speed of Light (c): 3.00 x 108 m/sWavelength (λ): (in m, nm etc)Frequency (v): (in hertz)Energy (E): (in Joules)Planck’s Constant (h): 6.6262 x 10-34 J-s
1. A laser in an audio compact disc player uses a light with the wavelength of 7.80 x 102 nm. What is the frequency of the light?
2. An FM radio station broadcasts at 99.5 MHz. Calculate the wavelength of the corresponding waves.
3. What kind of relationship exists between wavelength and frequency? _______________________
4. What kind of relationship exists between energy and frequency? __________________________
5. Microwave radiation has a wavelength on the order of 1.0 cm. Calculate the frequency and the energy of a single photon of this radiation.
6. Which has the greater energy, a photon of yellow light or a photon of green light?
10
7. How would you show an atom of Litium in the excited state using an Aufbau diagram? Draw an example.
8. In each of the following sets of atoms which has the smallest ionization energy?a. Ca, Sr, Bab. K, Mn, Gac. N, O, F
9. In each of the following sets, which atom or ion has the smallest radius?a. Li, Na, Kb. O+, O, O-
c. S, Cl, Kr
Bonding Review
1H
2.13 4 5 6 7 8 9
11
Li1.0
Be1.5
B2.0
C2.5
N3.0
O3.5
F4.0
11Na1.0
12Mg1.2
13Al1.5
14Si1.8
15P
2.1
16S
2.5
17Cl3.0
19K
0.9
20Ca1.0
21Sc1.3
22Ti1.4
23V
1.5
24Cr1.6
25Mn1.6
26Fe1.7
27Co1.7
28Ni1.8
29Cu1.8
30Zn1.6
31Ga1.7
32Ge1.9
33As2.1
34Se2.4
35Br2.8
37Rb0.9
38Sr1.0
39Y
1.2
40Zr1.3
41Nb1.5
42Mo1.6
43Tc1.7
44Ru1.8
45Rh1.8
46Pd1.8
47Ag1.6
48Cd1.6
49In1.6
50Sn1.8
51Sb1.9
52Te2.1
53I
2.555Cs0.8
56Ba1.0
57La1.1
72Hf1.3
73Ta1.4
74W1.5
75Re1.7
76Os1.9
77Ir
1.9
78Pt1.8
79Au1.9
80Hg1.7
81Tl1.6
82Pb1.7
83Bi1.8
84Po1.9
85At2.1
87Fr0.8
88Ra1.0
89Ac1.1
Ionic X > 1.7 (symbolized as A+ and Z-)
Polar Covalent 1.7 > X .5 (symbolized as A+ and Z-)
Pure Covalent X < .5 (no charges)
10. Electronegativity
a. Determine which element in the compound is the most electronegative and label the direction of the bond. State if it is Ionic, Pure Covalent, or Polar Covalent. 1) C-F
2) B-O
3) Cs-F
4) S-O
5) MgH
6) Cu-O
12
b. First draw the VSEPR structure and identify shape.
1) CH4
2) H2O
3) SO3
Thermochemistry Q= mcΔt
11. How many joules of heat are needed to raise the temperature of 10.0 grams of aluminum from 22 degrees C to 55 degrees C if the specific heat of aluminum is .90 J/gC?
13
12. The specific heat of zinc is 0.386 J/g0C. How many joules would be released when 454 grams of zinc at 96.00C where cooled to 28.00C?
13. How many calories are needed to warm 15.0 grams of water at 12.00C to 86.00C?
Use the following diagram to answer questions below:
14
14. What phase or phases are present during segment (1) ______________________
b) What phase change, if any, is taking place? _____________________________________________
c) What equation do you use to calculate the energy required to raise temp to next phase?
15. a)What phase or phases are present during segment (2) _______________________________________
b) What phase change, if any, is taking place? _____________________________________________
c) What equation do you use to calculate the energy required to raise temp to next phase?
15
16. a)What phase or phases are present during segment (3) _______________________________________
b) What phase change, if any, is taking place? _____________________________________________
c) What equation do you use to calculate the energy required to raise temp to next phase?
17. a) What phase or phases are present during segment (4) _______________________________________
b) What phase change, if any, is taking place? _____________________________________________
c) What equation do you use to calculate the energy required to raise temp to next phase?
18. a)What phase or phases are present during segment (5) _______________________________________
b) What phase change, if any, is taking place? _____________________________________________
c.) What equation do you use to calculate the energy required to raise temp to next phase?
