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Coach Ryan’s Chemistry/Physical Science
Class Keep scrolling down for more helpful items
such as test reviews, extra credit, class rules, class syllabus calendar.,
etc. |
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CLASSROOM
INFO Per
BHS procedures, a $15.00 science lab fee must be paid. Please submit this to
me as soon as possible. |
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Rules |
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1)
Be
on time and have all materials necessary to begin working when the bell rings,
not after. 2)
Talk
only when given permission 3)
Respect
for others is demanded at all times 4)
Follow
dress code and no cell phones. 5)
Use
good common sense at all times. 6)
Follow
all |
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Consequences |
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1)
verbal
warning 2)
write
offs 3)
phone
call 4)
office
referral I
reserve the right to skip to whatever step I feel necessary and appropriate. |
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Biography: Master’s Degree- University of Bachelor’s Degree- University of
Memphis Member of the Highly qualified to teach Chemistry
and Physical Science |
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“ If you do what I ask you to do
then you will be more likely to succeed.” |
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Schedule |
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ODD |
EVEN |
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1st Block: Chemistry |
1st Block: Physical
Science7:32-9:12 |
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2nd Block: Chemistry 9:19-10:49 |
2nd Block: Physical
Science9:19-10:49 |
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3rd Block: Chemistry Lunch: 3rd block cont’d: Chemistry |
3rd Block: Chemistry Lunch: 3rd block cont’d: Chemistry |
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4th Block: Weightlifting |
4th Block: Weightlifting |
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IMPORTANT
LINKS |
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Please scroll down for additional
important information |
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Contact: |
Email |
Phone |
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Contact: (Michael Ryan) |
Email: |
Phone: 901-837-5800 |
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This
page last updated: 3-9-10 |
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Please
look below for additional information:
Class Rules:
M. Ryan
Class rules
1) Have all materials necessary for
class.
2) Talk only when given permission
3) Treat everyone with respect
4) No dress code or cell phone
violations
5) Use good common sense at all
times
6) Follow all
CHEMISTRY EVEN CALENDAR UPDATED 3-9-10
|
March Mon 1 o |
Tues 2 e |
Wed 3 o |
Thur 4 e All make-up and extra credit due for the
3rd nine weeks |
Fri 5 o |
|
Mon 8 o |
Tues 9 e Junior ACT day |
Wed 10 o Exam review day |
Thur 11 e 3rd nine weeks exam 1&2 e |
Fri 12 o End 3rd nine weeks 3rd nine weeks exam 1&2 o |
|
Mon 15 e Begin 4th nine weeks 3rd nine weeks exam 3&4 e |
Tues 16 o 3rd nine weeks exam 3&4 o |
Wed 17 e |
Thur 18 o |
Fri 19 e ACT WED |
|
Mon 22 o |
Tues 23 e 11.1 pack |
Wed 24 o Report Cards Sent Home |
Thur 25 e |
Fri 26 o |
|
Mon 29 e 11.1 pack due 11.2 pack |
Tues 30 o |
Wed 31 e 11.2 pack due 11.3 pack |
thur |
fri |
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April |
tues |
wed |
Thur 1 o Project +60 |
Fri 2 NO SCHOOL GOOD FRI. |
|
Mon 5 e |
Tues 6 o |
Wed 7 e 11.3 pack due Chp 11 test review day |
Thur 8 o Project +50 |
Fri 9 e Chp 11 test open book 12.1 pack |
|
Mon12 No school Spring Break |
Tues 13 No school Spring Break |
Wed 14 No school Spring Break |
Thur 15 No school Spring Break |
Fri 16 No school Spring Break |
|
Mon 19 o |
Tues 20 e 12.1 pack due 12.2 pack |
Wed 21 o Progress reports |
Thur 22 e 12.2 pack due chp 12 test review day |
Fri 23 o project
+40 |
|
Mon 26 e Chp 12 test open book 13.1 pack |
Tues 27 o |
Wed 28 e |
Thur 29 o Project +30 |
Fri 30 e ACT DAY 13.1 pack due 13.2 pack |
|
MAY Mon 3 o |
Tues 4 e |
Wed 5 o |
Thur 6 e 13.2 pack due 13.3 pack |
Fri 7 o Project +20 |
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Mon 10 e ACT WED |
Tues 11o |
Wed 12 e 13.3 pack due Chp 13 test review |
Thur 13 o All extra credit and make-up due Project due |
Fri 14 e Chp 13 test 14.1 pack complete in class |
|
Mon 17 o Project -20 |
Tues 18 e 14.2 pack complete in class due today |
Wed 19 o Project – 40 Exam review day |
Thur 20 e Aft Teach Inservice BHS GRADUATION |
Fri 21o Project -60 last day to turn in project. Exam review day |
|
Mon 24 e Exams 1&2 e open book |
Tues 25 o Aft Teach Inservice Exams 1&2 o open book |
Wed 26 e Exams 3 & 4 e open book |
Thur 27 o Last Day for Students ˝ day Exams 3&4 o open book |
Fri 28 Teacher Admin Day |
|
Mon 31 |
tues |
wed |
thur |
fri |
CHEMISTRY ODD CALENDAR
UPDATED 3-9-10
|
March Mon 1 o |
Tues 2 e |
Wed 3 o |
Thur 4 e All make-up and extra credit due for the
3rd nine weeks |
Fri 5 o |
|
Mon 8 o |
Tues 9 e Junior ACT day |
Wed 10 o Exam review day |
Thur 11 e 3rd nine weeks exam 1&2 e |
Fri 12 o End 3rd nine weeks 3rd nine weeks exam 1&2 o |
|
Mon 15 e Begin 4th nine weeks 3rd nine weeks exam 3&4 e |
Tues 16 o 3rd nine weeks exam 3&4 o |
Wed 17 e |
Thur 18 o ACT WED |
Fri 19 e ACT WED |
|
Mon 22 o 11.1 pack |
Tues 23 e |
Wed 24 o Report Cards Sent Home |
Thur 25 e |
Fri 26 o 11.1 pack due 11.2 pack |
|
Mon 29 e |
Tues 30 o 11.2 pack due 11.3 pack |
Wed 31 e |
thur |
fri |
|
April |
tues |
wed |
Thur 1 o Project +60 |
Fri 2 NO SCHOOL GOOD FRI. |
|
Mon 5 e |
Tues 6 o 11.3 pack due Chp 11 test review day |
Wed 7 e |
Thur 8 o Project +50 Chp 11 test open book 12.1 pack |
Fri 9 e |
|
Mon12 No school Spring Break |
Tues 13 No school Spring Break |
Wed 14 No school Spring Break |
Thur 15 No school Spring Break |
Fri 16 No school Spring Break |
|
Mon 19 o 12.1 pack due 12.2 pack |
Tues 20 e |
Wed 21 o Progress reports 12.2 pack due chp 12 test review day |
Thur 22 e |
Fri 23 o project
+40 Chp
12 test open book 13.1 pack |
|
Mon 26 e |
Tues 27 o |
Wed 28 e |
Thur 29 o Project +30 ACT DAY 13.1 pack due 13.2 pack |
Fri 30 e ACT DAY |
|
MAY Mon 3 o |
Tues 4 e |
Wed 5 o 13.2 pack due 13.3 pack |
Thur 6 e |
Fri 7 o Project +20 ACT WED |
|
Mon 10 e |
Tues 11o |
Wed 12 e |
Thur 13 o All extra credit and make-up due Project due |
Fri 14 e |
|
Mon 17 o Project -20 |
Tues 18 e |
Wed 19 o Project – 40 Exam review day |
Thur 20 e Aft Teach Inservice BHS GRADUATION |
Fri 21o Project -60 last day to turn in project. Exam review day |
|
Mon 24 e Exams 1&2 e open book |
Tues 25 o Aft Teach Inservice Exams 1&2 o open book |
Wed 26 e Exams 3 & 4 e open book |
Thur 27 o Last Day for Students ˝ day Exams 3&4 o open book |
Fri 28 Teacher Admin Day |
|
Mon 31 |
tues |
wed |
thur |
fri |
===========================================================================================
Chem 3rd nine weeks exam chp 9 and 10 open book
Multiple Choice
Identify the choice that best completes the statement or
answers the question.
____ 1. What
is the correct name for the N
ion?
|
a. |
nitrate
ion |
c. |
nitride
ion |
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b. |
nitrogen
ion |
d. |
nitrite
ion |
____ 2. The
nonmetals in Groups 6A and 7A ____.
|
a. |
lose
electrons when they form ions |
|
b. |
have a numerical
charge that is found by subtracting 8 from the group number |
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c. |
all have
ions with a –1 charge |
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d. |
end in -ate |
____ 3. Which
of the following is NOT a cation?
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a. |
iron(III)
ion |
c. |
Ca |
|
b. |
sulfate |
d. |
mercurous
ion |
____ 4. Why
are systematic names preferred over common names?
|
a. |
Common
names do not provide information about the chemical composition of the
compound. |
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b. |
Common names
are derived from the method used to obtain the compound. |
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c. |
Common
names were assigned by the scientist who discovered the compound. |
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d. |
Common
names are not very descriptive. |
____ 5. Which
of the following is true about the composition of ionic compounds?
|
a. |
They are
composed of anions and cations. |
|
b. |
They are
composed of anions only. |
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c. |
They are
composed of cations only. |
|
d. |
They are
formed from two or more nonmetallic elements. |
____ 6. Which
of the following formulas represents an ionic compound?
|
a. |
CS |
c. |
N |
|
b. |
BaI |
d. |
PCl |
____ 7. Which
of the following shows correctly an ion pair and the ionic compound the two
ions form?
|
a. |
Sn |
c. |
Cr |
|
b. |
Cu |
d. |
Fe |
____ 8. In
which of the following are the formula of the ionic compound and the charge on
the metal ion shown correctly?
|
a. |
UCl |
c. |
IrS |
|
b. |
ThO |
d. |
NiO, Ni |
____ 9. Which
of the following compounds contains the lead(II) ion?
|
a. |
PbO |
c. |
Pb2O |
|
b. |
PbCl4 |
d. |
Pb2S |
____ 10. Which
set of chemical name and chemical formula for the same compound is correct?
|
a. |
iron(II)
oxide, Fe |
c. |
tin(IV)
bromide, SnBr |
|
b. |
aluminum
fluorate, AlF |
d. |
potassium
chloride, K |
____ 11. What
is the correct formula for potassium sulfite?
|
a. |
KHSO |
c. |
K |
|
b. |
KHSO |
d. |
K |
____ 12. Which
set of chemical name and chemical formula for the same compound is correct?
|
a. |
ammonium
sulfite, (NH |
c. |
lithium
carbonate, LiCO |
|
b. |
iron(III)
phosphate, FePO |
d. |
magnesium
dichromate, MgCrO |
____ 13. What
type of compound is CuSO
?
|
a. |
monotomic
ionic |
c. |
polyatomic
ionic |
|
b. |
polyatomic
covalent |
d. |
binary
molecular |
____ 14. Which
polyatomic ion forms a neutral compound when combined with a group 1A monatomic
ion in a 1:1 ratio?
|
a. |
ammonium |
c. |
nitrate |
|
b. |
carbonate |
d. |
phosphate |
____ 15. Which
of the following is a binary molecular compound?
|
a. |
BeHCO |
c. |
AgI |
|
b. |
PCl |
d. |
MgS |
____ 16. Consider
a mystery compound having the formula M
T
.
If the compound is not an acid, if it contains only two elements, and if M is
not a metal, which of the following is true about the compound?
|
a. |
It
contains a polyatomic ion. |
c. |
Its name
ends in -ic. |
|
b. |
Its name
ends in -ite or -ate. |
d. |
It is a
binary molecular compound. |
____ 17. What
is the name of H
SO
?
|
a. |
hyposulfuric
acid |
c. |
sulfuric
acid |
|
b. |
hydrosulfuric
acid |
d. |
sulfurous
acid |
____ 18. What
is the formula for phosphoric acid?
|
a. |
H |
c. |
HPO |
|
b. |
H |
d. |
HPO |
____ 19. What
is the formula for hydrosulfuric acid?
|
a. |
H |
c. |
HSO |
|
b. |
H |
d. |
H |
____ 20. What
is the correct name for the compound CoCl
?
|
a. |
cobalt(I)
chlorate |
c. |
cobalt(II)
chlorate |
|
b. |
cobalt(I)
chloride |
d. |
cobalt(II)
chloride |
____ 21. What
is the correct formula for calcium dihydrogen phosphate?
|
a. |
CaH |
c. |
Ca(H |
|
b. |
Ca |
d. |
Ca(H |
____ 22. What
does an -ite or -ate ending in a polyatomic ion mean?
|
a. |
Oxygen
is in the formula. |
c. |
Nitrogen
is in the formula. |
|
b. |
Sulfur
is in the formula. |
d. |
Bromine
is in the formula. |
____ 23. Which
of the following is the correct name for N
O
?
|
a. |
nitrous
oxide |
c. |
nitrogen
dioxide |
|
b. |
dinitrogen
pentoxide |
d. |
nitrate
oxide |
____ 24. What
is the correct name for Sn
(PO
)
?
|
a. |
tritin
diphosphate |
c. |
tin(III)
phosphate |
|
b. |
tin(II)
phosphate |
d. |
tin(IV)
phosphate |
____ 25. How
many hydrogen atoms are in 5 molecules of isopropyl alcohol, C
H
O?
|
a. |
5 |
c. |
35 |
|
b. |
5 |
d. |
35 |
____ 26. Which
of the following is NOT a representative particle?
|
a. |
atom |
c. |
anion |
|
b. |
cation |
d. |
all of the above |
____ 27. Which
of the following elements exists as a diatomic molecule?
|
a. |
neon |
c. |
nitrogen |
|
b. |
lithium |
d. |
sulfur |
____ 28. How
many moles of tungsten atoms are in 4.8
10
atoms of tungsten?
|
a. |
8.0 |
c. |
1.3 |
|
b. |
8.0 |
d. |
1.3 |
____ 29. How
many moles of silver atoms are in 1.8
10
atoms of silver?
|
a. |
3.0 |
c. |
3.0 |
|
b. |
3.3 |
d. |
1.1 |
____ 30. How
many atoms are in 3.5 moles of arsenic atoms?
|
a. |
5.8 |
c. |
2.1 |
|
b. |
7.5 |
d. |
1.7 |
____ 31. The
mass of a mole of NaCl is the ____.
|
a. |
molar mass |
c. |
molecular mass |
|
b. |
atomic mass |
d. |
gram atomic mass |
____ 32. What
is the molar mass of (NH
)
CO
?
|
a. |
144 g |
c. |
96 g |
|
b. |
138 g |
d. |
78 g |
____ 33. What
is the mass in grams of 5.90 mol C
H
?
|
a. |
0.0512 g |
c. |
389 g |
|
b. |
19.4 g |
d. |
673 g |
____ 34. What
is the number of moles in 432 g Ba(NO
)
?
|
a. |
0.237
mol |
c. |
1.65 mol |
|
b. |
0.605
mol |
d. |
3.66 mol |
____ 35. What
is the number of moles of beryllium atoms in 36 g of Be?
|
a. |
0.25 mol |
c. |
45.0 mol |
|
b. |
4.0 mol |
d. |
320 mol |
____ 36. What
is the volume, in liters, of 0.500 mol of C
H
gas at STP?
|
a. |
0.0335 L |
c. |
16.8 L |
|
b. |
11.2 L |
d. |
22.4 L |
____ 37. What
is the number of moles in 9.63 L of H
S
gas at STP?
|
a. |
0.104
mol |
c. |
3.54 mol |
|
b. |
0.430
mol |
d. |
14.7 mol |
____ 38. What
is the density at STP of the gas sulfur hexafluoride, SF
?
|
a. |
0.153
g/L |
c. |
3270 g/L |
|
b. |
6.52 g/L |
d. |
3.93 |
____ 39. The
molar mass of a certain gas is 49 g. What is the density of the gas in g/L at
STP?
|
a. |
3.6 |
c. |
2.2 g/L |
|
b. |
0.46 g/L |
d. |
71 g/L |
____ 40. Which
of the following gas samples would have the largest number of representative
particles at STP?
|
a. |
12.0 L
He |
c. |
0.10 L
Xe |
|
b. |
7.0 L O |
d. |
0.007 L
SO |
____ 41. Given
1.00 mole of each of the following gases at STP, which gas would have the greatest
volume?
|
a. |
He |
c. |
SO |
|
b. |
O |
d. |
All would have the same volume. |
____ 42. What
is the percent composition of chromium in BaCrO
?
|
a. |
4.87% |
c. |
20.5% |
|
b. |
9.47% |
d. |
25.2% |
____ 43. Which
of the following compounds has the lowest percent gold content by weight?
|
a. |
AuOH |
c. |
AuCl |
|
b. |
Au(OH) |
d. |
AuI |
____ 44. Which
of the following compounds has the highest oxygen content, by weight?
|
a. |
Na |
c. |
BaO |
|
b. |
CO |
d. |
H |
____ 45. The
ratio of carbon atoms to hydrogen atoms to oxygen atoms in a molecule of
dicyclohexyl maleate is 4 to 6 to 1. What is its molecular formula if its molar
mass is 280 g?
|
a. |
C |
c. |
C |
|
b. |
C |
d. |
C |
____ 46. Which
field of science studies the composition and structure of matter?
|
a. |
physics |
c. |
chemistry |
|
b. |
biology |
d. |
geology |
____ 47. A
golf ball has more mass than a tennis ball because it ____.
|
a. |
takes up more space |
c. |
contains different kinds of matter |
|
b. |
contains more matter |
d. |
has a definite composition |
____ 48. The
expression of 5008 km in scientific notation is ____.
|
a. |
5.008 |
c. |
5.008 |
|
b. |
50.08 |
d. |
5.008 |
____ 49. The
smallest particle of an element that retains the properties of that element is
a(n) ____.
|
a. |
atom |
c. |
proton |
|
b. |
electron |
d. |
neutron |
____ 50. In the
Bohr model of the atom, an electron in an orbit has a fixed ____.
|
a. |
position |
c. |
energy |
|
b. |
color |
d. |
size |
====================================================================================
Chemistry Final Exam review 2010
Multiple Choice
Identify the choice that best completes the statement or answers the
question.
____ 1. The study of substances
containing carbon is
|
a. |
organic chemistry. |
c. |
nuclear chemistry. |
|
b. |
inorganic chemistry. |
d. |
analytical chemistry. |
____ 2. The branch of chemistry
concerned with the properties, changes, and relationships between energy and
matter is
|
a. |
inorganic chemistry. |
c. |
physical chemistry. |
|
b. |
analytical chemistry. |
d. |
theoretical chemistry. |
____ 3. A theory is an accepted
explanation of an observed phenomenon until
|
a. |
one study conflicts with the theory. |
|
b. |
repeated data and observation conflict with the theory. |
|
c. |
scientists disagree about the methods used to gather the
data. |
|
d. |
an eminent scientist declares that it is inadequate. |
____ 4. All of the following
describe measurement standards EXCEPT
|
a. |
measurement standards avoid ambiguity. |
|
b. |
measurement standards must be unchanging. |
|
c. |
a standard need not agree with a previously defined size. |
|
d. |
confusion is eliminated when the correct measurement is
applied. |
____ 5. All but one of these units
are SI base units. The exception is the
|
a. |
kilogram. |
c. |
liter. |
|
b. |
second. |
d. |
Kelvin. |
____ 6. The symbol mm
represents
|
a. |
micrometer. |
c. |
milliliter. |
|
b. |
millimeter. |
d. |
meter. |
____ 7. The mass of a 5.00 cm3
sample of gold is 96.5 g. The density of gold is
|
a. |
0.0518 g/cm3. |
c. |
101.5 g/cm3. |
|
b. |
19.3 g/cm3. |
d. |
483 g/cm3. |
____ 8. 100 milliliters is
equivalent to
|
a. |
1 hectoliter. |
c. |
1 centiliter. |
|
b. |
1 microliter. |
d. |
1 deciliter. |
____ 9. If 1 inch equals 2.54
cm, how many centimeters equal 1 yard?