Review for Chemistry L3, L4 Final Exam: June 2013!
page 1
1. a. Write the dot diagram for CH3Cl, CO2 and NH3 !
(ans on back)
b. Use your VSEPR chart to identify the shape of each molecule. c. Is each molecule Polar or
Non-Polar? d. Use your “Forces Handout” (with the boxes) to identify the force of attraction
found in each. (Hint: for NH3 the force is the same as that found in H2O)
Molecule
CH3Cl
CO2
NH3
a. Dot Diagram
b. Shape of
Molecule
c. Polar or
Non-Polar
Molecule
d. Type of
Interparticle Force
P
NP
P
NP
P
NP
2. a. Identify the Type of Interparticle force in C10H10 ____________ In C6H12O6 _________
! In Ca(NO3)2 ______________
b. Match each compound to the appropriate picture of its particles.
c. Which would melt at the highest temperature? Use your type of forces of attraction to explain
why you think so.
d. Which would dissolve in water? Explain why you think so.
3. A student measured the Volume and Temperature of a gas in a flexible container. The Pressure
and amount of particles stay the same. Here is the data.
Volume(mL)! Temperature (K)!
a. Which Graph describes this data?! !
!
100 !
273 !
!
110!
300
!
117!
320
!
124.5!
340
b. Explain what about this data tells you this relationship.
c. Would V times T or V/T be constant in this relationship? Calculate the value for this constant.
3 (cont) d. Explain why this relationship happens, according to Kinetic Theory !
! (motion of particles).
Page 2
e. The Temp of this gas is changed until its volume is 146.5 mL. Calculate the final Temperature
of the gas in °C. !
f. The Pressure is 0.950 atm. How many moles of gas are in the flask? !
g. This container contains 8.5 x 10–3 g of gas. What is the Formula weight of the gas? This gas is
a diatomic element. What element is it?
4. Calculate the Molarity of 42.4 g Na2CO3 in 500 mL of solution. !
5. How many mL of 3.00 M HCl are needed to dilute to make 150 mL of 0.100 M HCl? ______
How many mL of water are needed? __________!
6. a. Calculate ∆H for this reaction using ∆Hf° values. Is it exothermic or endothermic?
!
CH4(g) + 2 O2(g) –––> CO2(g) + 2 H2O(l)!
b. Is ∆S + or – for this reaction? Explain why you think so.
c. Use your answers to ∆H and ∆S to decide when this reaction is spontaneous. (always, never,
high temp, low temp). Explain your reasoning.
(1b. tetr., lin, pyramid; c. P, NP, P; d. dipole, dispersion, H bonding; 2a. disp, dipole, ionic;
b. C10H10 , Ca(NO3)2, C6H12O6 ; c. Ca(NO3)2; d. Ca(NO3)2 & C6H12O6 (ionic and Polar diss. in water);
3. last graph, as V increases T incr; c. V/T = 0.366 mL/K; e. 400 K, 127°C; f. 4.24 x 10–3 mol ;
g. 2.0 g/mol, H2 ; 4. 0.800 M; 5. 5.00 mL stock, 145 mL H2O; 6a. ∆H = –890.24 kJ, exo ; b. ∆S = – ,
less mixed up; c. low temp, because -∆H & –∆S)
Review for Chemistry L3, L4 Final Exam: June 2013!
page 3
***1 and 2 are review for lab practical
*1. Here are some results of pH testing using the following indicators.
pH = !
1!
3!
5!
7!
9!
Bromo green!
yellow! yellow!
green!
blue!
blue!
Neutral red!
purple! purple! purple!
red!
yellow!
Indigo carmine!
blue!
blue!
blue!
blue!
blue!
11!
blue!
yellow!
gray!
13
blue
yellow
yellow
a.!Solution X turns Yellow in Bromo Green ! pH = ____________ ! Acidic, Basic, Neutral?
! Solution Y turns Yellow in Indigo Carmine ! pH = ____________!
Acidic, Basic, Neutral?
! Solution Z Turns Red in Neutral Red !
pH = ____________!
Acidic, Basic, Neutral?
b. Which solution is most acidic? ________ Which has the highest [H+]? _______
! Which has most OH– ions in solution? __________ Which is most likely KCl? ________
c. Could Solution X be a weak acid? Could it be 0.1 M HCl? Explain why you think so.
d. A student says solution Y is probably NH4Cl. Explain why he is wrong.
*2. a. Complete and Balance this neutralization reaction: KOH + H3PO4 –––>
b. Name the salt produced in part a. _______________________
c. What color would this Salt turn in the Neutral Red indicator? Explain why you think so.
d. How many mL of 0.15 M KOH would neutralize 30.0 mL of 0.10 M H3PO4?
e. How many mL of 0.250 M H3PO4 will neutralize 8.40 grams of KOH? !
3. a. Calculate the pH of a solution with [H+] = 6.5 x 10–4 M ________________!
!
b. Calculate the pH of a solution with [OH–] = 5.0 x 10–6 M _______________!
!
c. Calculate the [H+] of a solution with a pH of 2.60 ____________________!
4. a. Write in the oxidation numbers in this redox Reaction.
b. What is oxidized _______ reduced _________ (Include oxidation numbers for part b and c)
c. What is the oxidizing agent ________ What is the reducing agent _______
d. Balance the reaction using the oxidation number change method.
!
Sn !
+
KIO2 !
+
HCl
–––>
I2 !
+
SnCl4 ! +
H2O
+
KCl
! !
Page 4
5. You mix together the following. Fill in the blank with the other product. Why do you think so?
What is the final color of the solution in the beaker? Is there any solid made?
FYI: !
!
Fe(s) is a solid!
Fe+2 is colorless!
Fe+3 is yellow
Cr2O7–2 + Fe+2 + H+ ---> Cr+3 + ________ + H2O
6. For this voltaic cell : Zn|Zn+2 and Ag|Ag+ Write the half reaction for the oxidation,
reduction and Calculate the standard cell potential, E°cell.!
7. For this redox reaction: Fe + Ni+2 –––> Fe+2 + Ni
spontaneous in this direction or in reverse?!
Calculate E°cell for the reaction. Is it
(1a. X pH 1-3, A, Y pH 13, B, Z pH 7, N; b. X, X, Y, Z (salt of SB, SA = Neutral); c. either, pH 1(HCl)
to 3 (WA) ; d. salt of WB, SA = slightly acidic; 2a. 3 KOH + H3PO4 ––> 3 H2O + K3PO4;
b. potassium phosphate; c. yellow-orange, salt of SB, WA = slightly basic; d. 60 mL, e. 200 mL ; 3a.
3.19, b. 8.70, c. 2.5 x 10-3 M ; 4b. Sn, I+3 in KIO2, c. I+3 in KIO2, Sn, d. 3, 4, 16, 2, 3, 8, 4; 5. Fe+3
yelllow, no; 6. Zn ox, Ag+ red, +1.56 V ; 7. +0.19 V, forward )
Anagram Puzzle
Write down the letters for each answer, depending on if the statement is true(yes) or false (no)
Yes No
M!
T!
If Cu+2 is a better oxidizing agent than Mg+2
I!
S!
If Mg and Zn would make a higher voltage than Mg and Ag
I!
P!
If the temperature of a liquid stays the same while boiling
E!
O!
If an H2CO3 solution is more acidic than an HCl solution
H!
U!
If a reaction with –∆H and –∆S is always spontaneous
!D!
L!
If the electron configuration of O–2 is 1s2 2s2 2p6
-------------------D!
C!
If the conjugate acid of HCO3– is H2CO3
O!
B!
If the pressure of a gas increases as the temperature increases
C!
X!
If the motion of particles (kinetic energy) decreases as the temp. increases
R!
H!
If a crystal added to a saturated solution all crystallizes at once
A!
R!
If gases are usually heavy, very polar molecules
I!
E!
If polar solutes usually dissolve in water
O!
Y!
If a solid has a higher entropy than a liquid
E!
N!
If substances with metallic bonds are flexible and conduct electricity
D!
T!
If an acid with Ka = 1 x 10–4 is weaker than an acid with Ka = 1 x 10–3
Now rearrange the letters into two words to spell a common chemical.
__________________________!
________________________
Chemistry Level 3, 4
Final Exam Review Puzzle
ACROSS
1.
5.
6.
8.
pH of a solution with [OH–] = 10–8 M
The coldest possible Temperature is ___ Kelvin
A(n) ____ cell needs to have energy added.
CaCO3(s) + 176 kJ ––> CO2(g) + CaO(s): This
reaction absorbs energy and is ____
11. A(n) ___ compound is a brittle non-conductor
12. Oxidation number of V in Na4V2O7 is + ___
17. The weakest force, holds non-polar molecules
together
18. For gas law problems, the temperature is in
_____
20. Particles move rapidly and at random in a ____
21. A(n) __ makes a solution with lots of H+ ions
22. The ____ the mass of a non-polar molecule, the
weaker the force.
23. Number of electrons Mg wants to lose
24. F– ion has the same electron config. as ____
26. In Co + AgNO3 ---> Ag + Co(NO3)2 the
element oxidized
27. In 26A, Co is the _________ agent
DOWN
1. The positive part of a base and negative part
of an acid
2. The reaction in 8A has a ______ ∆S
3. As the temp. increases, ___ energy increases.
4. A molecule with + and — ends
7. The salt made from NaOH and citric acid.
9. The salt of a strong acid and a strong base is
_____
10. H2CO3 and Na2CO3 together make a ______
solution
13. The unique properties of water are due to __
bonding
14. A ____ acid only slightly ionizes in water
15. Number of dots (or electrons) in a happy
atom
16. Electron sharing is _______ bonding
19. Na2CO3 would make a ____ solution
23. The pH of a weak base can be about ___
25. Standard pressure is ____ atm.
Chemistry Level 3, 4 Final Exam 2013: Pre Exam directions
!
The Chemistry Level 3 and 4 final exams test your mastery of the Chemistry
competencies: 1. Lab Skills, 2. Problem Solving and 3. Matter and Energy. A Lab Practical will
check your Lab skills. All questions and problems on the exam will check your mastery of
Matter, Energy and the Changes they undergo. Problem Solving includes conducting research
by looking up data on various charts and tables, then interpreting and using this information
in questions and problems. It is also essential that you communicate your answers clearly and
completely. Show your work for problems, and write complete answers for questions.
!
You must be sure you find each of the following BEFORE you come in to take the exam!
If you cannot find one of them, go to the new web site and follow the links to Level 3
Chemistry, then Second semester downloads: (Downloads2nd)
http://centralhighchem.com
or directly to :
http://centralhighchem.com/ChemLevel3/Downloads2nd.html
DO NOT walk in on exam day and expect to be given the charts you need that day. This is
your responsibility to assemble the following prior to the exam. If the links aren’t working
email your teacher and we can email you a pdf file.
!
If you do not have a study guide for a specific chapter you may make a new one of your
own. You may not photocopy or borrow another student’s work.
Your self prepared study guides from each chapter from second semester :
!
Bonding!
Thermochemistry! Neutralization and titrations!
!
Phases of matter!
Solutions !
Oxidation and Reduction
!
Gas Laws!
Acids and Bases! Electrochemistry
Make sure the following information is on your study guide(s):
!
Gas law Equations
!
∆H, ∆S spontaneity chart
!
List of strong and weak acids and bases
The charts and Handouts from the year!
!
Periodic Table of the Elements!
Polyatomic ion chart !
Metric conversion Table
!
VSEPR chart
!
Types of Materials and Forces Table (you filled in)!
!
Vocabulary from Phases of matter
!
Water heating cooling curve, ∆Hf° chart
!
Solubility chart and !
Vocabulary List from Solutions
!
Reduction potential Table (E°red)
Bring your Book! Cost of replacement is $56.
Also be sure you have a scientific calculator (with logs) and a pencil.
!
The best way to study for this exam is to complete the review worksheets. You may
use these exam review worksheets on the exam.