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Chemistry EOC Review Questions
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Goal 2.01
1) Describe the contribution of each of the following scientists:
Democritus:
Chadwick
Dalton:
Rutherford
Thomson & Millikan
Bohr
2)
3)
4)
5)
What atomic model is in use today? Describe it.
Why is the current atomic model referred to as a probability model?
What is the electron cloud? What are orbitals?
Describe the Gold Foil Experiment in detail, as well as what it proved.
6) Goal 2.02
Subatomic Particle
Charge
Location
Mass
7) Label the parts below:
8)
9) From where is the mass above derived?
10) Define amu:
11) What is an isotope?
12) List 3 isotopes of carbon using the 2 methods we learned.
13) How many P, N, and E’s are in an atom of Lithium-8?
14) An element has 5 electrons and 7 neutrons. What is its atomic number and mass number? What is the identity
of the element?
15) An element has a mass number of 14 and an atomic number of 8. How many P, N, and E’s does it contain?
16) An element has 8 protons and 7 neutrons. What is its atomic number?
17) What is the overall charge of an atom?
18) What is the overall charge of the nucleus?
19) Goal 2.03
20) Name and give the chemical formula for the 4 acids you are supposed to have memorized.
21) Write, with charges, the following polyatomic ions: (These are the ones most likely to show up on your EOC.
You should DEFINITELY recognize them easily!!!)
i)
Nitrate
iv) Acetate
ii) Sulfate
v) Ammonium
iii) Carbonate
22) List and identify the 4 state of matter symbols that can be used in chemical equations.
23) Write the chemical formula for the following:
24) Ammonium Chloride
i)
Barium Acetate
ii) Sodium Carbonate
iii) Aluminum Nitrate
xii) Ammonium Sulfate
xiii)Zinc Chloride
xiv) Silver Iodide
25) Name the following compounds:
iv) Disulfur Trioxide
i)
PbO
v) Iron (III) Oxide
ii) Pb2O3
vi) Iron (II) Oxide
iii) NH4Cl
vii) Tin (IV) Chloride
iv) BaSO4
viii) Copper (I) Sulfide
v) HCl
ix) Lead (II) Hydroxide
vi) N2O5
x) Sodium Hydride
vii) CO2
xi) Carbon Monoxide
viii) CO
26) Goal 2.04
27) Ethanol at 25C is in what state?
28) A substance is found to have a boiling point of 1413C, what is the substance?
29) A substance is found to have a melting point of 178K, what is the substance?
30) A 10.16g sample of an unknown substance has a volume of 8 cm3. What is the substance?
31) Describe the following solutions:
i) 110g NaNO3 at 30C in 100 g water
ii) 130g KNO3 at 70C in 100g water
iii) 90g NH3 at 20C in 100g water
iv) 45g NaCl at 80C in 100 g water
v) 50g KClO3 at 90C in 200g water
vi) 100g KClO3 at 90C in 200g water
32) An unknown substance has a solubility of 20g at 65C. What is the
substance?
33) What is the solubility of KCl at 40C in 100g water?
34) What is the solubility of KI at 10C in 100 g water?
35) What is the solubility of NH4Cl in 50g water at 70C?
36) Identify the following compounds as soluble or insoluble in water:
37) MgF2
iii) MgCl2
vi) HgSO4
Li2O
iv) BaCO3
vii) (NH4)3PO4
ii) NH4OH
v) NaNO3
viii) LiF
i)
38) Goal 2.05 -> Gas Laws
39) Match the variables used to describe gases to the correct unit.
40) kPa,
a. pressure
41) oC
b. temperature
42) mL
c. volume
43) K
44) mm Hg
45) atmospheres (atm)
46) L
47) oF
48) Complete the following statements by writing “decreases,” “increases,” or “remains the same” on the line
provided.
49) As a gas is compressed in a cylinder
a) its mass ______________________________.
b) the number of gas molecules ____________________________.
c) its pressure ___________________________
d) its volume __________________________.
e) the distance between gas molecules ________________________.
f) its density _________________________.
50) Boyle’s Law states that the pressure of a gas is inversely proportional to its volume. Explain that statement.
(Include the correct formula and examples)
51) Problems
a) A 7.0 liter balloon at room temperature (22oC) contains hydrogen gas. If the balloon is carried outside to
where the temperature is –3.0oC, what volume will the balloon occupy?
b) A 5.0 liter tank of oxygen gas is at a pressure of 3 atm. What volume of oxygen will be available if the
oxygen is used at standard pressure?
c) A 500 liter volume of helium gas is at a pressure of 750 mm Hg and has a temperature of 300K. What is
the volume of the same gas at STP?
d) Nitrogen (80 kPa), oxygen (21.0 kPa), carbon dioxide (0.03 kPa), and water vapor (2.0 kPa) are the usual
atmospheric components. What is the total atmospheric pressure in kPa?
e) Complete the following statements about the nature of gases as presented in the kinetic molecular theory
by filling in the appropriate word (s) from the list below.
f) kinetic energy
g) potential energy
no force
pressure
perfectly elastic
weak
random motion zero
h) Gas particles exert ________________________________ on one another.
i)
Gas molecules are said to be in ________________________.
j)
The volume of gas particles themselves is said to be ______________________.
k) The collisions between gas particles are __________________________.
l)
The temperature of a gas is a measure of the average _______________ of the gas particles.
52) Goal 2.06
53) What is the difference between a cation and an anion?
54) How is a cation formed?
55) Give the ionic charge for the following elements:
56) Na
iv) O
i) F
v) Mg
ii) Ne
vi) Ba
iii) S
vii) Al
viii) Zn
ix) Ag
x) I
xi) P
57) What is meant by the idea that ionic compounds are held together by electrostatic attraction?
58) What are the characteristics of an ionic compound?
59) What are the characteristics of a covalent compound?
60) What are the characteristics of a metallic compound?
61) Which type of bonding occurs between 2 nonmetals?
62) Which type of bond results in ions surrounded by a shared “sea” of mobile electrons?
63) What type of bond results between 2 atoms with a big difference in electronegativity? (>1.7)
64) What type of bond results between a metal and a nonmetal?
65) True or False: An ionic bond can occur only between a cation and an anion.
66) ** Understand that all bonds have some ionic and some covalent character, but can usually be characterized as
mostly ionic or covalent. **
67) Why do metallic compounds conduct electricity?
68) Chemistry EOC Review Goals 2.07-3.01
69) Goal 2.07
70) Atoms share electrons to become more like _________ _________
71) True or False: Atoms bond to become more stable.
72) Atoms form a mostly covalent bond if they have a _________ difference in electronegativity.
73) A _______________ compound is one that contains covalent bonds.
74) List the 7 diatomic molecules.
75) What type of bond exists in an N2 molecule? ______________ ______________
76) Name a diatomic that forms a double covalent bond.
77) Name a diatomic that forms a single covalent bond.
78) (Remember, to determine number of bonds, count VE’s, determine how many more are needed to make 8 [or 2 if
it it Hydrogen] and that is the number of covalent bonds needed.)
79) Covalent bonding occurs between a ___________ and a _____________.
80) Which compound has the longest bond, HF or HCl?
81) Which of the above compounds has the stronger bond?
82) Draw a Lewis Structure for Lithium, Neon, Sulfur, and Aluminum.
83) List and draw the 5 VSEPR shapes you are supposed to know.
84) Explain how bonds affect VSEPR shape versus how unshared pairs do.
85) Tell the shape of the following molecules:
i) H2O
iii)
ii) CH4
iv)
86) Which VSEPR shape as the largest bond angle?
87) The smallest?
88) Identify the following as polar or nonpolar:
i) H2O
iii)
ii) NaCl
iv)
NH3
CO2
v) CO
vi) BF3
F2
HCl
v) NO2
vi) CO2
89) Water is polar. Substance B will not dissolve in water. Is substance B polar or nonpolar?
90) What is the general rule for solubility as it relates to polarity?
91) Networks solids are a special type of molecular (covalent) compound, but possess some very different
properties.
92) Describe how a network solid differs from other molecular compounds.
93) Give an example of a network solid.
94) What is the strongest type of intermolecular force?
95) What is the weakest?
96) Goal 2.08
97) What phase is the substance at
point X?
i) a. solid
b. liquid
ii) c. gas
d. plasma
98) What is the normal melting point?
i) a. -78
b. 60
ii) c. 101
d. 0
99) At what pressure do all three states
exist?
i) a. 25
b. 1
ii) c. 200
d. 140
100)
What change in state would
occur as you moved from point Y to
point X?
i) a.melting
b. boiling
ii) c. sublimation d. freezing
101)
After what temperature is the
liquid phase indistinguishable from
the gas phase? (critical point)
102)
Upon what 2 things does a
substances state of matter depend?
103)
Define sublimation:
104)
105)
106)
Goal 3.01
What are the rows in the periodic table called?
What are the columns called?
107)
Give 2 other names for group 7A.
108)
What element is in group 3 period 4?
109)
Name an element with properties similar to Magnesium.
110)
Elements in the same group have the same number of _____________ ______________ and because of
this have similar _________________.
111) Elements in the same period have the same number of ______________ ___________ _____________
112)
What is the most reactive element in group 1A?
113)
What is the most reactive element in group 7A?
114)
Identify the group number for the following:
115)
Inert Gases/Noble Gases
116)
Alkali Metals
117)
Halogens
118)
Alkaline Earth Metals
119)
Transition Metals
120)
Are most of the elements metals or nonmetals?
121)
Name 3 metalloids.
122)
Where is the p block located?
123)
Where is the d block located?
124)
How could you identify an element based on it electron configuration?
125)
Could you still identify the element if you were given the e- config in noble gas shorthand? How?
126)
[Ar] 4s23d104p2. Identify this element.
127)
How many valence electrons does the above element have?
128)
[Ar] 4s23d4. How many valence electrons does this element have? What element is it?
129)
What is the oxidation number of Zinc?
130)
Of Silver?
Of Oxygen?
Of Calcium?
Of Lithium?
131)
Write the electron configuration for Oxygen and Silicon.
132)
Write the electron config using noble has shorthand for Iodine, Vandium, and Sulfur.
133)
Draw the orbital diagram for oxygen and silicon.
134)
135)
Define Ionization Energy:
Why does IE decrease as you move down a group?
136)
137)
138)
Which has a higher IE?
O or F?
Cl or Br?
Define Electronegativity:
Why does EN increase as you move across a period?
Ag or As?
Cs or Ca?
139)
Which has a higher EN?
O or F?
Cl or Br?
Ag or As?
Cs or Ca?
140)
Which has a bigger radius?
O or F?
Cl or Br?
Ag or As?
Cs or Ca?
2+
141)
Which has a bigger or radius? O or O
K or K
Mg or Mg2+
Br or Br-?
142)
Which has a smaller radius, a cation or the atom it forms from? Explain Why.
143)
A compound is polar if it contains Covalent bonds and the atoms involved have different
_________________ values.
144)
Goal 3.02
145)
146)
147)
148)
i) Mole Conversions
22.4
6.02E23
Molar Mass
Coefficients
i) Molarity & Dilutions
ii) Empirical and Molecular Formulas
iii) Percent Composition
149)
1a) How many atoms are in 5.5 mol of neon?
150)
1b) How many molecules are in 22 mol of water?
151)
1c) How many total atoms are in the problem above?
152)
1d) How many moles are in 2.4E25 molecules of methane (CH 4)?
153)
2a) What is the mass of 25 mol of LiBr?
154)
2b) What is the mass of 10 mol of Xenon?
155)
2c) What is the mass of 12 mol of BaSO4∙5H2O?
156)
2d) How many moles are in 212g of water molecules?
157)
3a) What is the mass of 2.5E21 molecules of NaCl?
158)
3b) What is the mass of 4.3E26 atoms of Helium?
159)
3c) How many molecules of water are in 345g?
160)
3d) How many atoms of Iron are in 600g of Iron?
161)
4a) What is the volume of 200 mol of chlorine gas at STP?
162)
4b) What is the volume of 10 mol of nitrogen gas at STP?
163)
4c) At STP, How many moles of oxygen gas occupy a volume of 600L?
164)
4d) How many moles of nitrogen gas are needed to fill a 10L balloon at STP?
165)
5a) What is the molarity of a 10L solution containing 75g of NaCl?
166)
5b) What is the molarity of a 65L solution containing 220g of HCl?
167)
6a) What mass of nitric acid is needed to make 100L of 0.5M acid?
168)
6b) How many grams of NaCl are needed to make 20L of 2M solution?
169)
7a) What volume of stock 8M HCl is needed to prepare 200L of 1M acid?
170)
7b) What volume of 0.2M HCl could be prepared using 4L of stock 5M acid?
171)
8a) What is the empirical formula of the following compounds:
i)
36% Ca, 64% Cl
ii) 40%C, 6.71% H, 53.3% O
iii) 3.7% H, 44.4% C 51.9% N
iv) 25.9% N, 74.1% O **
172)
8b) What is the empirical formula of the compound C6H12O6?
173)
8c) Find the empirical formula for the oxide that contains 42.05 g of nitrogen and 95.95 g of oxygen.
174)
9a) What is the molecular formula of a compound with an empirical formula of CClN and a molar mass of
184.5?
175)
9b) What is the molecular formula of a compound whose molar mass is 60 g/mol and empirical formula is
CH4N.
176)
9c) What is the molecular formula of a compound whose molar mass is 34 and empirical formula is HO?
177)
10a) What is the percent composition of the compound formed when 2.64g of aluminum combine with 2.46g
of oxygen to form aluminum oxide?
178)
10b) When a 13.6g sample of a compound containing only magnesium and oxygen is decomposed, 5.4g of
oxygen is obtained. What is the percent composition of the compound?
179)
10c) A compound is formed when 9.03g Mg combines completely with 3.48g N. What is the percent magnesium
of the compound?
180)
10d) What is the percent nitrogen in NH3?
181)
11a) Imagine a compound is found to be 28% nitrogen by mass. How many grams of nitrogen would be found
in 340g of the compound?
182)
11b) A compound contains 63% Hydrogen by mass. What mass of Hydrogen would be found in 250g of the
compound?
183)
12a) What is the percent water of BaSO4∙5H2O?
184)
185)
Goal 3.03
Balance the following equations:
186)
___ N2 + ___ F2  ___ NF3
187)
___ C6H10 + ___ O2  ___ CO2 + ___ H2O
188)
___ HBr + ___ KHCO3  ___ H2O + ___ KBr + ___ CO2
189)
___ GaBr3 + ___ Na2SO3  ___ Ga2(SO3)3 + ___ NaBr
190)
___ SnO + ___ NF3  ___ SnF2 + ___ N2O3
191)
How many liters of nitrogen gas are needed to make 25 mol of nitrogen trifluoride?
192)
How many gram of the hydrocarbon Hexine would need to be combusted in order to form 500L of carbon
dioxide?
193)
How many molecules of dinitrogen trifluoride would form if 88 mol of tin(II) fluoride reacted with an
excess of nitrogen trifluoride?
194)
How many moles of bromic acid are needed to produce 15 mol of potassium bromide salt?
195)
How many molecules of sodium bromide salt would form if 84 mol of gallium bromide were reacted with an
excess of Sodium Sulfite?
196)
Using the following equation:
197)
i)
198)
2 NaOH + H2SO4  2 H2O + Na2SO4
How many grams of sodium sulfate will be formed if you start with 200 grams of sodium hydroxide and
you have an excess of sulfuric acid?
Using the following equation:
i)
199)
Pb(SO4)2 + 4 LiNO3  Pb(NO3)4 + 2 Li2SO4
How many grams of lithium nitrate will be needed to make 250 grams of lithium sulfate, assuming that
you have an adequate amount of lead (IV) sulfate to do the reaction?
200)
201)
Goal 4.01
Explain the difference between ground state and excited state for an atom.
202)
What is a photon?
203)
Write a possible electron configuration for Magnesium in an excited state.
204)
205)
206)
207)
According to the Bohr Model of the atom
Electrons circle the nucleus only in ________ energy ranges called orbits.
Electrons can neither gain nor lose energy inside this orbit but can move _____ or _____ to another orbit.
The lowest energy orbit is __________ to the nucleus.
208) An atom releases light energy in the form of a ________ when it moves from the __________ state to
the _________ state.
209)
When an atom absorbs energy it moves to the _________ state.
210)
This model is still used for the __________ atom, but is not considered accurate for any other atom.
211)
Electrons in some ways act like _________ and in some ways act like ___________.
212)
A photon with a long wavelength has a _________ frequency.
213)
The energy of a wave is synonymous with its _____________.
214)
As an electron moves from n=4 to n=2, what color light is emitted?
215)
As an electron moves from n=3 to n=2, what color light is emitted?
216)
As an electron moves from n=5 to n=2, what color light is emitted?
217)
As an electron moves from n=6 to n=2, what color light is emitted?
218)
What type of electromagnetic radiation is released as an electron moves from n=4 to n=1?
219)
What wavelength of light is released as an electron moves from n=5 to n=3?
220)
What color light has the highest frequency?
221)
What color has the highest energy?
222)
Which type of EM radiation has the shortest wavelength?
223)
Which type of EM radiation has the most energy?
224)
225)
Review Qs:
Write the Chemical equation for zinc chloride.
226)
What is the oxidation number of the carbon in the compound MgCO3?
227)
What is the maximum number of electrons that can be contained in the fourth principle energy level?
228)
What is the maximum number of d orbitals in any given principle energy level?
229)
How many electrons can 1 orbital hold?
230)
What element is in period 5 group 4?
231)
What is the charge of an alpha particle?
232)
What is the mass of an alpha particle?
233)
Another word for average kinetic energy:
234)
Define entropy:
235)
Goal 5.01
236)
Identify the following reactions by type:
237)
238)
239)
240)
241)
242)
243)
244)
245)
Ni(s) + Cl2
2(s)
2Sc(s) + 3SnCl2
3(aq) + 3Sn(s)
NaNO3
3(aq)
Na2CO3
2O(s) + CO2(g)
3Zn(s) + 2Mn(NO3)3
3)2(aq)
HCl(aq) + NaOH(aq) → NaCl(aq) + H2O(l)
CH4 + 2O2 → CO2 + 2H2O
Cl2O3(g) + H2
2(aq)
2K3PO4(aq) + 3CaCl2
3(PO4)2(s) + 6KCl(aq)
246)
Predict Products: Attached Sheet
247)
What type or reaction is an acid-base neutralization?
248)
What 2 things are always produced during neutralization?
249)
Which of the 8 reactions above is an acid-base neutralization?
250)
What 2 things are always formed during combustion?
251)
Looking only at the reactants side, how can you recognize a combustion reaction?
252)
Goal 5.02
253) Balance the equations. Then, write the complete ionic and then the net ionic equation for each of the
following:
1.
_____ Zn (s) + _____ AgNO3 (aq) 
254)
Complete:
255)
Net:
256)
2. _____ Na (s) + _____ H2O (l) 
257)
Complete:
258)
Net:
259)
3. _____ NaCl (aq) + _____ AgC2H3O2 (aq) 
260)
Complete:
261)
Net:
262)
4. _____ Ca(OH)2 (aq) + _____ H3PO4 (aq) 
263)
Complete:
264)
Net:
265)
5. _____ HNO3 (aq) + _____ Ni (s) 
266)
Complete:
267)
Net:
268) Harder one. Aqueous solutions of barium chloride and sodium sulfate react to form a barium sulfate
precipitate. Write the complete and net ionic equation. (HINT: You guys messed this up on the CRT. Write
out the reactants and predict the products. The problem only tells you about the precipitate that forms, but
the others ions form something as well (that stays aqueous!)
269)
Chemical Equation:
270)
Complete:
271)
Net:
272) Explain how to use the activity series. (Both for halogens and for metals, based on order of metals and
using the arrows)
273)
Goal 5.03
274)
List the 4 indicators of a chemical change.
i) 1.
ii) 2.
iii) 3.
iv) 4.
275)
Explain how a burning splint can be used to test for hydrogen, oxygen, and carbon dioxide.
276) Lime water turns milky white and forms a precipitate when exposed to a gas. What is the identity of the
gas?
277)
Explain how color change could be a chemical or physical change.
278)
279)
280)
281)
282)
283)
284)
Identify the following as a chemical or physical change:
Melting Ice
Burning Paper
Rusting
Decomposing
Smashing a rock
Dissolving sugar in water
285)
286)
287)
288)
289)
290)
291)
Identify the following as exothermic or endothermic:
During a reaction, the beaker gets hot
burning a candle
Chemical cold pack gets cold
During a reaction, the beaker gets cold
Freezing rainwater
∆H is positive
292)
Goal 5.04
293)
According to Bronsted-Lowery:
i) Acids are proton ___________
ii) Bases are proton ___________
294)
According to Arrhenius:
i) Acids dissociate in water to form ____________ ions
ii) Bases dissociate in water to form ____________ ions
295)
Identify the following properties as belonging to an acid or a base:
i) Sour
ii) Slippery
iii) pH<7
iv) pH>7
v) electrolytes in water
vi) bitter
vii) pH=7
296)
Know how to solve acid Molarity and Dilution problems!
297)
How many liters of stock 2M HNO3 are needed in order to prepare 50L of 0.1M solution?
298)
What is the molarity of 80g of HCl dissolved in 20L of solution?
299)
What is the molarity of 5 mol of HC2H3O2 dissolved in 10L of water?
300) Molarity is used to measure ___________________. Remember Acid Strength is not the same as its
concentration. Watering down an acid reduces its _______________. Its _______________ (weak vs.
strong acid or base) is purely based on how well that acid dissociates in water.
301)
A graph of pH vs. concentration would appear _______________ in shape.
302)
Indicator
304)
Acid
305)
Base
306)
Pentamethoxy
red
307)
1.22.3
308)
redviolet
310)
Methyl yellow
311)
2.94.0
312)
red
314)
Bromcresol
green
315)
4.05.6
316)
yellow
317)
blue
318)
Chlorphenol
red
319)
5.46.8
320)
yellow
321)
red
322)
Rosolic acid
323)
6.88.0
324)
yellow
325)
red
colorless
329)
red
blue
333)
red
326)
Phenolphthalein 327)
330)
334)
338)
303) pH
Range
8.0- 328)
10.0
Nile blue
331)
10.111.1
Tropeolin O
335)
11.013.0
332)
336)
yellow
309)
colorless
313)
337)
yellow
orangebrown
Using the chart above:
i) What indicator would you use in order to titrate a basic solution to a pH of 4?
ii) What would be the best indicator to use to neutralize a solution?
340)
339)
If [H+] = 1E-6, what is [OH-]?
341)
If [H+] = 1E-3, what is the pH?
342)
If [OH-]= 1E-10, what is the pOH? Is the substance an acid or a base?
343)
If [OH-] = 1E-5, what is the pH?
Is it an acid or a base?
344)
If [H+]= 0.0001, what is the pOH?
Is it an acid or a base?
345)
If the hydrogen ion concentration is 1E-2, what is the pOH?
346)
Identify the acid, base, conjugate acid, and conjugate base below:
i)
HBr + H2O  H3O+ + Br–
ii)
NH3 + H2O  NH4+ + OH–
1.
Is it an acid or a base?
Is it an acid or a base?
How many milliliters of 0.100 M HCl are required to neutralize 25.0 mL of 0.100 M
Ba(OH)2?
2. What is the molarity of a hydrochloric acid solution, 30.0 mL of which is just
neutralized by 48.0 mL of 0.100 M NaOH?
347)
Goal 4.02
348) In a closed system, energy is neither ________ nor _____________, but can be _____________ from
one form to another.
349)
The total useful energy of an open system is always ________________ due to ________________.
350)
351)
Define:
Enthalpy-
352)
Entropy-
353)
Specific heat capacity-
354)
Temperature-
355)
Joule-
356)
Endothermic reaction (w/ examples)-
357)
Exothermic reaction (w/ examples)-
358)
Catalyst (and tell how it does what it does)-
359) Be sure you understand this diagram.
360) (Effect of catalyst, activation energy, reactant side,
product side)
363)
361)
Be sure you could label EXACTLY activation energy.
362)
Is this an exothermic or endothermic reaction?
Contrast heat and temperature:
364)
Label the relevant parts.
365) Where is Potential Energy
changing?
366) Where is kinetic energy
changing?
367) What is the freezing
point?
368)
What is the melting point?
369) At what point would some
of the material be liquid and
some gas?
370)
The above diagram is called a heating curve. Draw and label a cooling curve.
371)
This is called a
____________________
_
372) Label the relevant
parts.
373) What substance is this
for?
374) If you move from 50 to
-50 at standard pressure
what change has occurred?
375) Moving from 0.5 to
100kPa at 50C what change
occurs?
376) Describe the conditions
at point Y.
377)
Describe the conditions
at point X?
378)
This is a phase diagram for carbon dioxide.
379) What is interesting about the change in state it
undergoes at standard pressure according to the
diagram?
380) At what sort of conditions could you have liquid
carbon dioxide? (You may answer qualitatively.)
381)
Goal 4.03
382)
Entropy is a measure of disorder.
383)
Increasing Entropy: solid  liquid  gas
1. Ionic Compounds  Ions in solution
384)
The entropy of the universe is always _____________.
385)
Systems tend to move towards the lowest energy level and in the direction of greatest entropy.
386)
Goal 4.04
387)
388)
Describe the penetrating power of the 3 types of radiation:
1.
389)
390)
2.
3.
391)
Write the symbol for an alpha particle:
392)
Write the symbol for a beta particle:
393)
Write the symbol for gamma radiation:
394)
What type of radiation results in a change in mass # and atomic number?
395)
U-238 undergoes beta decay, what atom results?
396)
True or False: There is no way to control the rate of nuclear decay.
397)
Contrast Fission and Fusion:
398)
399)
Which equation above represents beta decay?
400)
Which represents alpha decay?
401)
Which represents fusion?
402)
403)
What does the above equation represent?
404)
What is the mass of an alpha particle?
405)
What is the charge of an alpha particle?
406)
List 3 uses of nuclear chemistry:
1.
An isotope of cesium (cesium-137) has a half-life of 30 years. If 1.0 mg of cesium-137
disintegrates over a period of 90 years, how many mg of cesium-137 would remain?
2. A 2.5 gram sample of an isotope of strontium-90 was formed in a 1960 explosion of an
atomic bomb at Johnson Island in the Pacific Test Site. The half-life of strontium-90
is 28 years. In what year will only 0.625 grams of this strontium-90 remain?
3. Actinium-226 has a half-life of 29 hours. If 100 mg of actinium-226 disintegrates over
a period of 58 hours, how many mg of actinium-226 will remain?
4. The half-life of isotope X is 2.0 years. How many years would it take for a 4.0 mg
sample of X to decay and have only 0.50 mg of it remain?
5. After 3 half-lives have passed, 0.375 grams of Bismuth-218remain. How big was the
original sample?
407) The half-life of a radioactive element is 30 seconds. In what period of time would the activity of the sample
be reduced to one-sixteenth of the original activity?
408) The half-life of francium is 3 minutes. After 18 minutes, what fraction of the original sample remains?
409) Thermochemistry Problems
1. How much energy must be absorbed by 20.0 g of water to increase its temperature
from 283.0 °C to 303.0 °C?
2. When 15.0 g of steam drops in temperature from 275.0 °C to 250.0 °C, how much heat
energy is released?
3. How much energy is needed to melt 150g of ice?
4. How much energy is required to heat 120.0 g of water from 2.0 °C to 24.0 °C?
5. If 720.0 g of steam at 400.0 °C absorbs 800.0 kJ of heat energy, what will be its
increase in temperature?
6. How much energy is needed to boil 75g of water?
7. How much heat (in kJ) is given out when 85.0 g of lead cools from 200.0 °C to 10.0 °C?
8. If it takes 41.72 joules to heat a piece of gold weighing 18.69 g from 10.0 °C to 27.0 °C,
what is the specific heat of the gold?
9. It takes 333.51 joules to melt exactly 1 gram of a substance. What is the molar heat of
fusion for water, from this data?
10. What mass of water can be melted using 800J of heat?