Download Chemistry-Study-Guide-for-Spring-2014

Chem. Study Guide for Spring Benchmark
Name _______________________
Period _____
The chapters on the Benchmark include
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Gas Laws
Thermochemistry
Acids and Bases
Reaction Rates
Organic Chemistry
Nuclear Chemistry
chapter 14
chapter 17
chapter 19
chapter 18
chapters 22.1, 24
chapter 25
Tips to prepare:
 Study the vocabulary from each chapter
 As always you will receive a periodic table and polyatomic ion list.
 Answer the study guide questions below. They will be turned in for credit the day of the
exam.
Format of the Benchmark:
 The benchmark is 20% of your final grade.
 It is cumulative (everything that we have done second semester)
 There are 80 multiple choice questions
Gas Laws
1. Describe how gas particles diffuse.
2. Understand how the rate of diffusion relates to the temperature of a gasses environment.
As the temperature increases the rate of diffusion _____________. Why?
3. What is the temperature and pressure at Standard Temperature and Pressure (STP)?
a. Temperature = _______
b. Pressure = _______
4. Know that 1mole of ANY gas occupies 22.4L at STP. Why does the identity of the gas
(or the formula) not make a difference on the volume? HINT think of empty space!
5. Describe, using the Kinetic Molecular Theory, how a gas in a closed container creates
pressure on the container walls.
6. Define absolute zero, describe molecular motion at absolute zero and list this
temperature in Kelvin and Celsius.
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7. Be able to convert between the Celsius and Kelvin temperature scale.
Example 1: A chemist cools a solution to 250 K. What is its temperature in degrees Celsius?
Example 2: While making ice-cream you note that the temperature of the rock salt and ice is -3oC.
What is this temperature in Kelvin?
8. Be able to use Boyle’s Law to solve a problem.
Boyle’s Law Formula:
Example 1: A sample of nitrogen gas under 10 kPa of pressure has a volume of 100 L. The pressure
is changed to 20 kPa. What is the new volume of the sample?
Example 2: A 55L sample of oxygen gas at standard pressure (101 kPa) is allowed to expand to a new
volume of 100 L. What is the new pressure?
9. Be able to use Charles’ Law to solve a problem.
Charles’ Law Formula:
Example 1: A sample of hydrogen gas at a temperature of 50oC occupies a volume of 5L. At what
temperature would the gas occupy a volume of 15 L?
Example 2: A 75 L sample of oxygen gas at standard temperature (0oC) is heated to a new temperture
of 28 oC. What is the new expanded volume?
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10. List 3 variables that affect the pressure of a contained gas
a.
b.
c.
11. Be able to use the Combined Gas Law formula to solve a problem.
Combine Gas Law Formula:
Example 1: A research finds that a gas has a volume of 50L at 25oC and 100 kPa of pressure. What
will be the new volume if the gas is cooled to STP?
Example 2: A biologist finds that CO2 has a volume of 0.1L at 30oC and 200kPa inside of a pod on a
piece of Kelp. When dragged down to a new ocean depth the volume of the pod decreases to 0.05L
and the pressure increases to 300 kPa. What is the temperature of the new environment?
Thermo chemistry
12. Explain the relationship between kinetic energy, potential energy, temperature and
heat*. HINT (start by looking at the definition for each term and then see how they
relate).
13. What are Exothermic and Endothermic processes, describe with words or in a
diagram the heat exchange between the system and the surroundings.
14. Phase changes are physical changes because the substance obtains it’s physical
identity. On the physical changes below label the arrows exothermic or endothermic.
Also fill-in the terms freezing, melting, evaporation and condensation.
Sold  Liquid  Gas
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*Heat Transfer – know that heat transfers from warm to cool object until thermal equilibrium (the
same temperature throughout) is reached. Also understand that cool is the absence of heat
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15. What is the equation for Heat(Q)?
Q=
a. write the unit for each of the following variables
i. C
ii. Q
iii. m
iv. ∆T
16. The temperature of a piece of copper with a mass of 95.4g increases from 25oC to 48 oC
when the metal absorbs 849 J of heat. What is the specific heat of copper?
17. How much energy is required to heat a 250 g sample of water from 20oC to 80oC, given
that the specific heat of water is 4.18 J/goC?
18. The specific heat capacity of gold is 0.129 J/goC. A 100 gram sample of gold has an
initial temperature of 15oC. If 150 J of heat energy are added to the sample, what is the
final temperature?
19. Use the formula above to solve: A small pebble is heated and placed in a foam cup calorimeter
containing 25 ml of water at 25oC. The water reaches a maximum temp. of 26.4oC.
20. What is the heat of fusion of ice? (HINT see reference table)
21. Use the heat of fusion above to solve - How many grams of ice at 0C and 101.3 KPa could be
melted by the addition of 2.25 KJ of heat?
Acids/ Bases
22. List 3 properties of each of the following:
a. Acid ______________________ _________________ ___________________
b. Bases ______________________ __________________ ____________________
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23. What are the 3 rules for naming and writing formulas of Acids?
a. _______________________________________________________
b. _______________________________________________________
c. ______________________________________________________
24. Describe how bases are named.
a. __________________________________________________________________
25. Write the proper name for each of the following acid(s)/Base(s):
a. HClO____________________________________________
b. HCN ____________________________________________
c. H3PO4 __________________________________________________________________
d. KOH ____________________________________________
26. If the [H+] in a solution is 1.0 x 10-5 M…
a. What is the pH of this solution __________
Circle which term describes this solution: acidic, basic, or neutral?
b. What is the OH- of this solution?
27. What is the equation this describes the relationship between pH and pOH?
__________+____________= __________
28. Label the following pH scale with the terms: ACID, BASE and NEUTRAL
0…1…2…3…4…5…6…7…8…9…10…11…12…13…14
_______________
___________
__________________
Rates of Reaction/ Equilibrium
29. How does the collision theory explain rate of reaction? ________________________
_______________________________________________________________________
30. List 4 factors that affect reaction rates
a. _______________________________
b. _______________________________
c. _______________________________
d. _______________________________
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31. define - Reversible Reaction
_________________________________________________
a. What is the symbol that is used to represent a Rev. RXN? _____________________
32. What does it mean for a reversible RXN to be at Chemical Equilibrium?
__________________________________________________________________
Organic Chemistry
32. What are the four major classes of macromolecules that all living organisms are composed of? _____________
______________ ___________________________ ______________________________
33. The major component of all macromolecules is _______________.
34. How many electrons does carbon have in its outer energy level? ______
35. How is the number of valence electrons in carbon atoms related to the bonds that carbon atoms form?
________________________________________________________________________________________
36. What is the basic ratio of carbon, hydrogen, and oxygen in a carbohydrate? ____________________________
________________________________________________
37. Carbohydrates are well suited to energy storage because they contain many ______________-____________
bonds.
38. A lipid is not soluble in ___________, but is soluble in ___________.
39. Why is it that a fat can store more energy than a carbohydrate? ______________________________
_________________________________________________________________________________
40. Which has carbon to carbon double bonds, a saturated or an unsaturated fat? ___________________
41. What are the subunits that make up a protein? ___________________ _____________
42. True or False
The rate of chemical reactions is speeded up by enzymes.
43. True or False
There are 75 different kinds of amino acids that humans use.
44. What are the two major types of nucleic acids? _________ or ______________________ _________
and _________ or ______________________ _________
45. The subunits of DNA and RNA are called ________________________.
46. In the space at the left, identify the following statements as descriptions of DNA, RNA, or both.
_______ The macromolecule is a double helix.
_______ The subunits are nucleotides.
_______ The nucleotide subunits arranged in chromosomes.
_______ This is used in making copies of genes that are used in making proteins.
_______ This stores the information about how an organism will grow and develop.
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Nuclear Chemistry
47. List the three types of radiation. Use their name and symbol below.
a. __________________ ______________
b. __________________ ______________
c. __________________ ______________
48. What is needed to stop the types of radation listed above? fill-in-the-blanks below
a. ______Cardboard_____ ______________
b. ______ Paper ________ ______________
c. ______Lead/Concrete__ ______________
49. Define radiation: _______________________________________________________
________________________________________________________________________
50. Define half-life: ________________________________________________________
51. What is a common archeological process that uses half-life? ______________________
_____________________________________________________________________
52. Nitrogen 13 emits beta radiation and decays to carbon 13 with a half-life of 10 min;
assume a starting mass of 2g of nitrogen 13.
a. How long are three half-lives? __________________
b. How many g of the isotope will still be present at the end of 3 half lives?
_________
53. What is the difference between Fission and Fusion?___________________________
54. Name 3 applications of Nuclear Research/Power
a. ________________________
b. ________________________
c. ________________________
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