j0215086

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.

j0301076

Brighton High School ~ 8045 Highway 51 South – Brighton, TN  38011

 

 

 

CLASSROOM INFO

Per BHS procedures, a $15.00 science lab fee must be paid. Please submit this to me as soon as possible.

 

 

Rules

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 Tipton County and Brighton High rules of conduct.

Consequences

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.

Biography:

Master’s Degree- University of Memphis

Bachelor’s Degree- University of Memphis

Member of the Tennessee Army National Guard

Highly qualified to teach Chemistry and Physical Science

 

“ If you do what I ask you to do then you will be more likely to succeed.”

 

 

 

Schedule

ODD

EVEN

1st Block:                 Chemistry 7:32-9:12

1st Block: Physical Science7:32-9:12

2nd Block:               Chemistry  9:19-10:49

2nd Block: Physical Science9:19-10:49

3rd Block:                Chemistry 10:56-11:16

Lunch:       11:16-11:46

3rd block cont’d:      Chemistry 11:46-12:56

3rd Block:                Chemistry 10:56-11:16

Lunch:       11:16-11:46

3rd block cont’d:     Chemistry 11:46-12:56

4th Block: Weightlifting

4th Block: Weightlifting

sportlne

 

IMPORTANT LINKS

Please scroll down for additional important information

 

 

 

 

 

 

 

 

Contact:

Email  
 @tipton-county.com

Phone
901-837-5800

Contact:   (Michael Ryan)

Email:
mryan@tipton-county.com

Phone:  901-837-5800

This page last updated:  3-9-10

 

 

 

 

 

 

 

 

 

 

 

 

 

 


                                                        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 Tipton County and Brighton High School general rules of conduct.

 

 

 

 

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

 

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

 

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 3:15-6:15

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 3:15-6:15

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 3:15-6:15

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 3:15-6:15

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

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

c.

all have ions with a –1 charge

d.

end in -ate

 

 

____    3.   Which of the following is NOT a cation?

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.

b.

Common names are derived from the method used to obtain the compound.

c.

Common names were assigned by the scientist who discovered the compound.

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.

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.

NO

b.

BaI

d.

PCl

 

 

____    7.   Which of the following shows correctly an ion pair and the ionic compound the two ions form?

a.

Sn, N; SnN

c.

Cr, I; CrI

b.

Cu, O; CuO

d.

Fe, O; FeO

 

 

____    8.   In which of the following are the formula of the ionic compound and the charge on the metal ion shown correctly?

a.

UCl, U

c.

IrS, Ir

b.

ThO, Th

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, FeO

c.

tin(IV) bromide, SnBr

b.

aluminum fluorate, AlF

d.

potassium chloride, KCl

 

 

____  11.   What is the correct formula for potassium sulfite?

a.

KHSO

c.

KSO

b.

KHSO

d.

KSO

 

 

____  12.   Which set of chemical name and chemical formula for the same compound is correct?

a.

ammonium sulfite, (NH)S

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 MT. 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 HSO?

a.

hyposulfuric acid

c.

sulfuric acid

b.

hydrosulfuric acid

d.

sulfurous acid

 

 

____  18.   What is the formula for phosphoric acid?

a.

HPO

c.

HPO

b.

HPO

d.

HPO

 

 

____  19.   What is the formula for hydrosulfuric acid?

a.

HS

c.

HSO

b.

HSO

d.

HS

 

 

____  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.

CaHPO

c.

Ca(HPO)

b.

CaHPO

d.

Ca(HHPO)

 

 

____  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 NO?

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, CHO?

a.

5  (6.02  10)

c.

35

b.

5

d.

35  (6.02  10)

 

 

____  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  10 moles

c.

1.3  10 moles

b.

8.0  10 moles

d.

1.3  10 moles

 

 

____  29.   How many moles of silver atoms are in 1.8  10 atoms of silver?

a.

3.0  10

c.

3.0  10

b.

3.3  10

d.

1.1  10

 

 

____  30.   How many atoms are in 3.5 moles of arsenic atoms?

a.

5.8  10 atoms

c.

2.1  10 atoms

b.

7.5  10 atoms

d.

1.7  10 atoms

 

 

____  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 CH?

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 CH 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 HS 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  10 g/L

 

 

____  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  10 g/L

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.

NaO

c.

BaO

b.

CO

d.

HO

 

 

____  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.

CHO

c.

CHO

b.

CHO

d.

CHO

 

 

____  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  10 km

c.

5.008  10 km

b.

50.08 10 km

d.

5.008  10 km

 

 

____  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?