Download THERMOCHEMISTRY EXAM

LEARNING TARGETS: STRUCTURE & PROPERTIES --- THERMOCHEMISTRY
INTERMOLECULAR ATTRACTIONS
I can describe: H-bonding, dipole-dipole, and dispersion forces.
I can draw a Lewis structure and predict the type of intermolecular attraction.
I can draw two Lewis structures to show a type of intermolecular attraction.
I can predict or rank boiling points based upon type of intermolecular attraction.
ORGANIC CHEMISTRY
I can draw and identify the following functional Groups: carboxylic acid, alcohol, ester, amine.
I can draw and recognize the structure of an amino acid.
I can write a reaction showing two amino acids reacting to form a protein.
I can define polymer, monomer and cross-linking.
SOLIDS/LIQUIDS/GASES
I can give a general description of the molecules in the solid phase.
I can recognize and describe the structure of ice.
I can describe and name three allotropes of carbon.
I can give a general description of the molecules in the liquid phase.
I can explain vapor pressure.
I can explain why equilibrium is reached in a closed container and not an open container.
I can explain/define surface tension.
I can give a general description of the gas phase.
I can explain pressure and do basic pressure conversion calculations
.
PHASE DIAGRAMS
I can sketch a phase diagram for water and for other substances.
I can explain what the negative slope between the solid and liquid phase indicates about solid water.
I can explain what equilibrium exists at any point on a division line.
I can tell where the triple point is on the graph and define triple point.
I can define equilibrium.
I can use a phase diagram to tell how one might make a change from one phase to another.
HEATING/COOLING CURVE
I can make a sketch of a heating/cooling curve for any pure substance.
I can tell where/when kinetic energy changes occur.
I can tell where/when potential energy changes occur.
I can label the phase changes and the temperature changes.
I can describe the change in movement of molecules during a temperature change.
I can describe the change in movement of molecules during a phase change.
I can tell when a change is endothermic and when it is exothermic.
I can write the q equation for each section of the graph.
I can label the melting/freezing point and the boiling/condensing point.
HEAT CALCULATIONS
I can calculate the heat energy related to a temperature change and to a phase change.
I can convert calories to Joules and Joules to calories [1 cal = 4.184 J].
I can determine when the q should be negative or positive.
I can define vapor pressure.
I can define boiling & boiling point.
I can define normal boiling point.
I know what a colligative property is and how they change the vapor pressure, freezing point and boiling points.
I can answer all of the homework questions & worksheet questions for this unit. I can answer all lab questions for
this unit. *I am able to apply all of the above to new situations (problems/questions/reactions)!*
LEARNING TARGETS
STRUCTURE & PROPERTIES --- THERMOCHEMISTRY
ASSIGNMENTS
STRUCTURE AND PROPERTIES
Review Reading: C20-2 p629-631 C21 p663-666, 674-679 and C21-4
C6-5 Read p189-193 #27-32
S#1-10
Lab: Polymers
IMF and Organic Chem Review Sheet
Read Ch 10-1 and 10-2 #1,11,13,17,18
Read Ch 12 (all) S#11-20
THERMOCHEMISTRY
Lab: Specific Heat of a Metal
Read 17-1 S#21-30
Heating/Cooling Curve Worksheet
Ch 12 #18-21,33,36
Lab: Heat of Fusion of Ice
* HONORS: Read 436-442 (Colligative Properties) #S31-35
Tentative EXAM DATE:
HONORS = Monday, March 2, 2015
REGULAR = Tuesday March 3, 2015
DUE DATE
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Supplemental Homework
1. Looking back over previous units . . . define the following bond types.
a. nonpolar covalent b. polar covalent
c. ionic
d. metallic
2. How must the electronegativites of two atoms compare if a covalent bond between them is to be polar?
3. The bonds between the following pairs of elements are covalent. Arrange them according to polarity, listing
the most polar bond first (It might be helpful to look back at an electronegativity table p151.).
a. H-Cl
b. H-C
c. H-F
d. H-O
e. H-H
f. S-Cl
4. What is a hydrogen bond?
5. Depict the hydrogen bond between two ammonia molecules and between one ammonia molecule and one
water molecule.
6. Why do compounds with strong intermolecular attractive forces have higher boiling points than compounds
with weak intermolecular attractive forces?
7. Draw a structure of each of the following functional groups.
a. alcohol
b. carboxylic acid
c. amine
d. ester
8. Describe how addition polymers form.
9. Describe how condensation polymers form. Give a biological example as discussed in class.
10. What is a polymer? A monomer?
11. Describe the liquid state according to the kinetic-molecular theory.
12. Compare vaporization and evaporation.
13. Describe the solid state according to the kinetic-molecular theory.
14. What is surface tension?
15. A liquid is in a closed container and has a constant vapor pressure. What is the relationship between the rate
of evaporation of the liquid and the rate of condensation of the vapor in the container?
16. State Le Chatelier’s Principle.
17. What condition must exist for a liquid to boil?
18. Use figure 12-12 to determine the boiling point of each liquid.
a. ethanol at 200 torr
b. diethyl ether at 600 torr
c. water at 101.3 kPa
19. Explain why the boiling point of a liquid varies with atmospheric pressure.
20. Describe the effect that increasing temperature has on the vapor pressure of a liquid.
21. In what direction does heat flow between two objects?
22. Review: how do endothermic processes differ from exothermic processes?
23. Two substances in a glass beaker chemically react and the beaker becomes too hot to touch. Is the reaction
exothermic or endothermic?
24. In what units do we measure heat flow (energy)?
25. Review: a. How do you convert between Joules and calories?
b. Convert 4.18J to calories
c. Convert 1.76 kcal (kilocalories) to Joules
26. Calculate how much heat (in joules) 32.0g of water absorbs when it is heated from 25.0˚C to 80.0 ˚C. You
will need to use the specific heat values in the table on p. 513. Watch your units!!!
27. Determine the specific heat of a material if a 35g sample absorbed 48J as it was heated from 293K to 313K.
28. If 980kJ of energy are added to 6200g of water at 291K, what will the final temperature of water be?
29. What is meant by enthalpy? What is its symbol?
30. What is the name given to a heat change at constant pressure?____________________________________
31. What are three colligative properties of solutions?
32. What factor determines how much vapor pressure, freezing point, and boiling point of a solution differ from
those properties of the pure solvent?
33. Would a dilute solution of sodium fluoride solution have a higher boiling point? Explain.
34. An equal number of moles of KI and MgI2 are dissolved in equal volumes of water. Which solution has the
higher
a) boiling point?
b) vapor pressure?
c) freezing point?
35. Explain why the vapor pressure, boiling point, and freezing point of an aqueous solution of a nonvolatile
solute are not the same as those of the pure solvent.