CHEMISTRY - Suffolk Teaching Activities & Resourcesstar.spsk12.net/science/chem/ChemistryCRN.pdf · Chemistry Content Review Notes are designed by the High School Science Steering

Designed by Ann-Rene Challenger, Amanda Griffin, Dr. Donna Keene, Marianne Lawrence, Deborah Oliver,

and Ashanta Ruffin

STANDARDS OF LEARNING

CONTENT REVIEW NOTES

CHEMISTRY


and Ashanta Ruffin

OVERVIEW

Chemistry Content Review Notes are designed by the High School Science Steering Committee as a

resource for students and parents. Each nine weeks’ Standards of Learning (SOLs) have been

identified and a detailed explanation of the specific SOL is provided. Specific notes have also been

included in this document to assist students in understanding the concepts. A “ ” section has

also been developed to provide students with the opportunity to check their understanding of the

content.

The document is a compilation of information found in the Virginia Department of Education

(VDOE) Curriculum Framework, Enhanced Scope and Sequence, and Released Test items. In

addition to VDOE information, Glencoe Textbook Series and resources have been used. Finally,

information from various websites is included. The websites are listed with the information as it

appears in the document.

The Chemistry Blueprint Summary Table is listed below as a snapshot of the reporting categories,

the number of questions per reporting category, and the corresponding SOLs.

It is the Chemistry Instructors’ desire that students and parents will use this document as a tool

toward the students’ success on the end-of-year assessment.


and Ashanta Ruffin

Standards of Learning

Notes

&

Activities


and Ashanta Ruffin

First Nine Weeks

LAB SAFETY EQUIPMENT

SOL 1C

SCIENTIFIC METHOD

SOL- 1D, E

REPORTING SCIENTIFIC

DATA

SOL- 1E, G

SOL 1G

SOL- 1A,E,F

SOL- 1F

MATTER AND ENERGY

SOL 2H

ATOMIC STRUCTURE

SOL 2I

SOL 2A

SOL 2C

SOL 2B

PERIODIC TABLE

SOL 3 A

SOL- 2D,E

SOL 2A

SOL 2F

SOL 2C

ELECTRON CONFIGURATION

SOL 2I

SOL-2 A, B,C, E,G

SOL-2 A, B, C, D, G


and Ashanta Ruffin

TOPIC: LAB SAFETY EQUIPMENT

1. What is the correct procedure to neutralize an acid?

2. When diluting an acid solution, one should always do what and why?

3. Describe the sequence of actions you would take if you spill a strong acid on your

clothing in the lab.

4. Describe what you would do if your lab partner’s shirt-sleeve caught on fire.

5. When is it most important to wash your hands while in the laboratory?

6. Describe the procedure to smell a substance?

CHEMISTRY

STANDARD CH. 1C

The student will investigate and understand that experiments in which

variables are measured, analyzed, and evaluated produce observations and

verifiable data. Key concepts include: c) proper response to emergency

situations


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TOPIC: SCIENTIFIC METHOD

Student measurement of Temperature in ° C

Reading 1 Reading 2 Reading 3

Student A 88.6 88.5 88.7

Student B 92.6 90.1 91.6

Student C 90.0 88.9 92.5

Student D 80.1 89.8 90.0

1. Use the above chart to answer the following question. Four students each took

temperature readings of a sample of water. The actual temperature of the sample was

90.0 ° C. Which student’s measurements were both accurate and precise?

2. A student was asked to determine the density of a mineral. Outline the steps in which to

accurately determine the density using the displacement method.

3. What is the first step that should be taken when a caustic chemical gets into a person’s

eye?

4. What is the mass of a substance whose density is 0.2396 g/mL and a volume of 20.0 ml?

5. What is the minimum number of trials needed for a measurement to be reliable?

CHEMISTRY

STANDARD CH. 1D, E


variables are measured, analyzed, and evaluated produce observations

and verifiable data. Key concepts include:

d) manipulation of multiple variables, using repeated trials; and

e) accurate recording, organization, and analysis of data through

repeated trials.


and Ashanta Ruffin

TOPIC: REPORTING SCIENTIFIC METHOD

1. Determine the number of significant figures in the following:

a. 5006 b. 1200

c. 0.001200 d. 5

2. Compute the following. Record your answer to the correct number of significant figures.

a. (4.33 x 103)(1.6 x 10

-2)

b. 2.36 x 102 x 4.2655 x 10

4

c. 9.65 x 105/7.2 x 10

-3

d. 2.33 x 10-3

x 1.05 x 102/1.234

3. The SI base unit for mass is the ______________________.

4. The SI base unit for the volume of a liquid is the ________________.

5. Use the factor label method or dimensional analysis to solve the following problems.

a. Convert 950 m to km

b. Convert 2.56 kg to g

c. Convert 0.7526 mg to kg

d. Convert 4.85 L to mL

6. Convert the following temperatures.

a. 543K to Celsius

b. 23K to Celsius

CHEMISTRY

STANDARD CH. 1E,G

The student will investigate and understand that experiments in which variables are

measured, analyzed, and evaluated produce observations and verifiable data. Key

concepts include:

e) accurate recording, organization, and analysis of data through repeated trials.

g) mathematical manipulations (SI units, scientific notation, linear equations,

graphing, ratio and proportion, significant digits, dimensional analysis).


and Ashanta Ruffin

1. What piece of equipment would serve the purpose for each of the following?

a. Adding 5 ml of 5% HCl to 5 different solutions. ______________

b. To measure 97.0 ml of water. _______________

c. To mass a solid substance. ________________

d. To dry out a precipitate for measuring. _______________

2. Which of the following items should be used if you need approximately 100 ml of a

liquid? (Choose one)

a. Beaker

b. Erlenmeyer flask

c. Graduated cylinder

3. A student measures the mass of a piece of copper three times and records the results in

the following table:

Trial Mass (grams)

1 15.5

2 15.6

3 15.7

The actual mass of the metal is 17.2 grams. Are the trial measurements accurate and/or precise?

Explain your answer.

4. A student measured the temperature of a solution and found it to be 46.0◦C at standard

pressure. The theoretical temperature of that boiling solution is 45.0◦C. What is the

percent error according to the student’s measurement?

CHEMISTRY

STANDARD CH. 1 A, E, F The student will investigate and understand that experiments in which variables are

measured, analyzed, and evaluated produce observations and verifiable data. Key

concepts include: a) designated laboratory techniques

e) accurate recording, organization, and analysis of data through repeated trials.

f) mathematical and procedural error analysis


and Ashanta Ruffin

DIRECTIONS: Show all work using dimensional analysis

1. Convert 3.5 x 10-3

L to mL.

2. How many kilograms are there in 4223 g?

3. Using the rules for significant figures, what is the correct answer for 2.5 m times 44.8 m?

4. (3.5 x 106)(5.3 x 10

-5) =

CHEMISTRY

STANDARD CH. 1G


variables are measured, analyzed, and evaluated produce observations and

verifiable data. Key concepts include:

g) mathematical manipulations including SI units, scientific notation, linear

equations, graphing, ratio and proportions, significant digits and dimensional

analysis.


and Ashanta Ruffin

DIRECTIONS: Determine the percent error in the following problems.

1. Experimental Value = 1.44 g Accepted Value = 1.54 g

2. Experimental Value = 22.2 L Accepted Value = 22.4 L

3. Experimental Value = 128.6 mg Accepted Value =128.3 mg

4. Experimental Value = 9.98 x 10-3

g Accepted Value =1.03 x 10-2

g

CHEMISTRY

STANDARD CH. 1 F The student will investigate and understand that experiments in which

variables are measured, analyzed, and evaluated produce observations

and verifiable data. Key concepts include

f) mathematical and procedural error analysis


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TOPIC: MATTER AND ENERGY

Chemical and Physical Properties

The student will be given an object or substance and must identify the physical and chemical

properties of that object. (This assignment is to be given after lecture on chemical and physical

properties and how to correctly identify each.)

1. Describe the chemical properties of this object below, citing any evidence you have

collected:

2. Describe the physical properties of this object below, citing any evidence you have

collected:

CHEMISTRY

STANDARD CH. 2H

The student will investigate and understand that the placement of elements on the

periodic table is a function of their atomic structure. The periodic table is a tool

used for the investigations of:

h) chemical and physical properties.


and Ashanta Ruffin

TOPIC: ATOMIC STRUCTURE

CHEMISTRY

STANDARD CH. 2I The student will investigate and understand that the placement of elements on the periodic

table is a function of their atomic structure. The periodic table is a tool used for the

investigations of:

i) historical and quantum models.

Students will create a two page foldable for the models of an atom. Each outside flap will be the

names of the scientists (Democritus, Dalton, Rutherford, Bohr), and the inside picture will be

each scientist’s contribution to the historical model. A one page foldable will be created for the

quantum models with Heisenberg and Planck. Students will be creative using mnemonics and/or

graphics.


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Element Average Atomic mass Mass number Atomic number

Ne

Al

Ge

P

Br

Ca

K

I

Sr

Sn

CHEMISTRY

STANDARD CH. 2A The student will investigate and understand that the placement of elements on the

periodic table is a function of their atomic structure. The periodic table is a tool used

for the investigations of

a) average atomic mass, mass number, and atomic number


and Ashanta Ruffin

.

Warm-up: Complete the following chart:

Subatomic Particle Symbol Charge Relative mass Location in atom

protons

neutrons

electrons

Atomic Structure Element/Ion Atomic

Number

Atomic

Mass

Mass

Number

Protons Neutrons Electrons

3H

1H

+

12C

7Li

+

35Cl

-

39K

24Mg

2+

77As

3-

108Ag

30S

-2

238U

CHEMISTRY

STANDARD CH. 2C The student will investigate and understand that the placement of

elements on the periodic table is a function of their atomic structure.

The periodic table is a tool used for the investigations of:

c) mass and charge characteristics of subatomic particles


and Ashanta Ruffin

DIRECTIONS: Answer the following questions

Average Atomic Mass

1. Rubidium has two common isotopes, Rb-85 and Rb-87. If the abundance of Rb-85 is

72.2% and the abundance of Rb-87 is 27.8%, what is the average atomic mass of

rubidium?

2. Uranium has 3 common isotopes. If the abundance of U-234 is 0.01%, the

abundance of U-235 is 0.71% and the abundance of U-238 is 99.28%, what is the

average atomic mass?

3. Titanium has five common isotopes: Ti-46 (8.0%), Ti-47 (7.8%), Ti-48 (73.4%), Ti-49

(5.5%), and Ti-50 (5.3%). What is the average atomic mass of titanium?

4. Explain why atoms have different isotopes. In other words, how is it that helium can

have three different sized atoms and they all are still the element Helium.

5. Draw and label 3 possible isotopes of hydrogen. Which isotope can you predict to be

the most abundant? Why? Correctly name the 3 isotopes using the symbol “H”?

6. Select an element on the Period Table. Create 4 isotopes for your element and form

an average atomic mass calculation to support the given atomic mass.

CHEMISTRY

STANDARD CH. 2B The student will investigate and understand that the placement of elements

on the periodic table is a function of their atomic structure. The periodic

table is a tool used for the investigations of:

b) isotopes, half lives, and radioactive decay

http://images.google.com/imgres?imgurl=http://www.napavalley.edu/Academics/SME/Chemistry/PublishingImages/chemistry_molecules.gif&imgrefurl=http://www.napavalley.edu/Academics/SME/Chemistry/&usg=__fDSWwyxism1d7SeVcIazPWUvH3s=&h=326&w=350&sz=27&hl=en&start=2&itbs=1&tbnid=ZY7xJER4mDpJ6M:&tbnh=112&tbnw=120&prev=/images?q=chemistry+images&hl=en&sa=G&gbv=2&tbs=isch:1


and Ashanta Ruffin

TOPIC: PERIODIC TABLE

Writing Binary Formulas

Cation Anion Formula Cation Anion Formula

Na+ Cl

- Fe

+2 O

-2

Ba+2

F- Fe+2

O-2

K+ S

-2 Cr

+2 S

-2

Li+ Br

- Cr

+3 S

-2

Al+3

I- Cu

+ Cl

-

Zn+2

S-2

Cu+2

Cl-

Ag+ O

-2 Pb

+2 O

-2

Mg+2

P-3

Pb+4

O-2

Ni+2

O-2

Mn+2

Br-

Ni+3

O-2

Mn+4

Br-

CHEMISTRY

STANDARD CH. 3A The student will investigate and understand how conservation of energy and

matter is expressed in chemical formulas and balanced equations. Key

concepts include

a) nomenclature


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and Ashanta Ruffin

Counting Valence Electrons

Element Group Number Number of Valence

Electrons

Ne

Al

Ge

P

Br

Ca

K

I

Sr

Sn

CHEMISTRY

STANDARD CH. 2 D, E The student will investigate and understand that the placement of elements on

the periodic table is a function of their atomic structure. The periodic table is a

tool used for the investigations of:

d) families or groups;

e) periods


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DIRECTIONS: State the periodic trend and explain.

PERIODIC TRENDS LEFT TO

RIGHT EXPLAINATION TOP TO

BOTTOM EXPLAINATION

ATOMIC RADII

ELECTRONEGATIVITY

SHIELDING EFFECT

IONIZATION ENERGY

CHEMISTRY

STANDARD CH. 2 F The student will investigate and understand that the placement of

elements on the periodic table is a function of their atomic structure.

The periodic table is a tool used for the investigations of:

f) trends including atomic radii, electronegativity, shielding

effect, and ionization energy.


and Ashanta Ruffin

DIRECTIONS: Complete the chart below.

Ions and Subatomic Particles

Ion Symbol Protons Electrons Charge

S2-

K1+

Ba2+

Fe3+

Fe2+

F1-

O2-

P3-

Sn4+

Sn2+

N3-

Br1-

Mg2+

Cu1+

Cu2+

U6+

Mn5+

Cl1-

Se2-

CHEMISTRY

STANDARD CH. 2 C The student will investigate and understand that the placement of

elements on the periodic table is a function of their atomic structure. The

periodic table is a tool used for the investigations of:

c) mass and charge characteristics of subatomic particles.

http://images.google.com/imgres?imgurl=http://upload.wikimedia.org/wikipedia/commons/f/f4/Salicylic_acid_methyl_ester_chemical_structure.png&imgrefurl=http://ilovechemistryweee.blogspot.com/&usg=__1_Ksn05zhXnbrBY3SZ79CH5gPyg=&h=695&w=813&sz=4&hl=en&start=35&itbs=1&tbnid=-ySfhEoCPQgSqM:&tbnh=123&tbnw=144&prev=/images?q=chemistry+formula&start=20&hl=en&sa=N&gbv=2&ndsp=20&tbs=isch:1


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Second Nine Weeks

IONIC AND COVALENT BONDING AND COMPOUNDS SOL- 3 A, C, D

MOLE/EMPIRICAL AND MOLECULAR FORMULA SOL- 4A, B


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TOPIC: IONIC COMPPOUNDS

Multiple Choice

1. What is the ionic charge on the copper ion in the ionic compound that has the

formula CuSO4 ?

a. +1

b. -2

c. +3

d. +2

2. Which element when combined with Bromine would most likely form an ionic

compound?

a. potassium

b. carbon

c. phosphorus

d. iodine

3. An –ite or –ate ending on the name of a compound indicates that the compound

_________________.

a. is a binary ionic compound b. is a binary molecular compound

c. contains a polyatomic ion

d. contains a polyatomic cation

4. In general, ionic compounds _____________.

a. are amorphous solids at room temperature

b. conduct electricity when in the solid state

c. conduct electricity when they are dissolved in water

d. all of these

CHEMISTRY

STANDARD CH. 3A,C, D The student will investigate and understand how conservation of energy

and matter is expressed in chemical formulas and balanced equations.

Key concepts include

a) nomenclature

c) writing chemical formulas

d) bonding types


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5. Which of the following is the correct name for the compound MnF3?

a. Manganese fluoride (III)

b. Manganese (III) fluoride

c. Manganese (I) fluoride (III)

d. Manganese (III) fluoride (III)

6. According to the periodic table, Mg will most likely react with elements in which of

these groups?

a. 1

b. 3

c. 17

d. 18

7. Which of these compounds is most likely to contain an ionic bond?

a. H2

b. SO2

c. CH4

d. CaCl2

8. What is the name of NH4OH?

a. Ammonium hydroxide

b. Nitrogen oxygen hydride

c. Nitrogen hydroxide

d. Ammonium oxygen hydride

9. All of the following formulas are correct except:

a. NaOH

b. CaF2

c. H3PO4

d. AlSO4

10. In forming NaCl, energy is required to

a. change chlorine to a gas

b. add an electron to a chlorine atom

c, remove an electron from a sodium atom

d. bring together the sodium ions and chloride ions


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Critical Thinking:

1. Why are there no rules for naming Group 18 ions?

2. Determine the ratios of cations to anions that are most likely in the formulas for ionic

substances of the following elements:

a. An alkali metal and a halogen

b. An alkaline earth metal and a halogen

c. An alkali metal and member of Group 16

d. An alkaline earth metal and a member of Group 16

3. Compound B has lower melting and boiling points than compound A does. At the same

temperature, compound B vaporizes faster and to a greater extent than compound A. If

only one of these compounds is ionic, which one would you expect it to be? Why?

TOPIC: COVALENT COMPOUNDS AND BONDING

Multiple Choice

1. Which of the following is the name of the molecule PCl3?

a. Phosphorus trichloride

b. Phosphorus chloride

c. Potassium trichloride

d. Potassium chloride

2. The type of formula that shows the arrangements of atoms and bonds is called-

a. Empirical

b. Chemical

c. Molecular

d. Structural

CHEMISTRY

STANDARD CH. 3 A, C, D

The student will investigate and understand how conservation of energy and matter is

expressed in chemical formulas and balanced equations. Key concepts include

a) nomenclature

c) writing chemical formulas

d) bonding types


and Ashanta Ruffin

3. What shape does the molecule BF3 have?

a. Bent

b. Linear

c. Tetrahedral

d. Trigonal planar

4. H H

: Z – Z :

H H

The figure above shows a compound containing hydrogen (H) and an unknown

element Z. To which group on the periodic table does element Z belong?

5. Bonding between two elements of equal electronegativity would be-

a. 100% covalent

b. Primarily ionic

c. 50% ionic

d. Metallic in character

6. The small attractive force between molecules of nitrogen gas, N2, is due to-

a. Hydrogen bonds

b. Van der Waals forces

c. Dipole-dipole attraction

d. Magnetism

7. Which of the following is a polar covalent bond?

a. NaCl

b. O2

c. Al

d. SO2

8. In chemical compounds, covalent bonds form when-

a. The electronegativity difference between two atoms is very large

b. Electrons are completely transferred between two metals

c. Pairs of electrons are shared between two nonmetal atoms

d. Two nonmetal ions are attracted to each other by opposite charges


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9. The Lewis electron dot system represents electrons in the-

a. Outer energy level

b. Inner level

c. Middle level

d. Core level

10. An alien landed on Earth and created the periodic table shown. The astronaut was

trying to determine what type of bond would be present in several compounds. The

type of bond in a compound containing D and B would be-

a. A metallic bond

b. A nonmetallic bond

c. A covalent bond

d. An ionic bond

SOL Release Chemistry Test 2005

Critical Thinking

1. Ionic compounds tend to have higher boiling points than covalent substances do. Both

ammonia, NH3, and methane, CH4, are covalent compounds, yet the boiling point of

ammonia is 130 C higher than that of methane. What might account for the large

difference?

2. Create a concept map using the following terms: valence electrons, non-polar, covalent

compounds, polar, dipoles, and Lewis structures.

3. Create a Venn Diagram to compare and contrast ionic and covalent bonding. Make sure

you have 5 similarities and 5 differences.


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TOPIC: MOLE/EMPIRICAL AND MOLECULAR FORMULA

Multiple Choice:

1. The molar mass (gram formula mass) for the compound sodium thiosulfate,

Na2S2O3 is

a. 71 grams

b. 153 grams

c. 158 grams

d. 254 grams

2. The empirical formula for C6H12 is ----

a. C3H6

b. C2H4

c. CH3

d. CH2

3. How many moles of copper are equivalent to 3.44 x 1023

atoms of copper?

a. 0.571 moles

b. 1.75 moles

c. 5.41 x 1021

moles

d. 5.71 x 1022

moles

4. What is the mass of one mole of CO2?

a. 24 g

b. 28 g

c. 44 g

d. 56 g

CHEMISTRY

STANDARD CH. 4 A, B

The student will investigate and understand that quantities in a

chemical reaction are based on molar relationships. Key concepts

include

a) Avogadro’s principle and molar volume

b) Stoichiometric relationships


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5. Which of the following shows the correct number of atoms of each element in the

formula Mg(NO3)2?

a. 1 magnesium atom, 2 nitrogen atoms, and 6 oxygen atoms

b. 1 magnesium atom, 2 nitrogen atoms, and 5 oxygen atoms

c. 1 magnesium atom, 1 nitrogen atom, and 6 oxygen atoms

d. 1 magnesium atom, 1 nitrogen atom, and 5 oxygen atoms

Practice:

1. Formula Mass: Determine the molar mass of the following. Show all work and units.

a. CuSO4

b. CaCO3

c. H3PO4

d. Al2(SO4)3

2. Determine the empirical formula for the following:

a. 80.0 g of carbon and 20.0 g of oxygen

b. 71.5% Ca and 28.5% O

3. Percent Composition. Determine the percent composition of the following

compounds. Show all work.

a. NO2

b. Al2(SO4)3


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THIRD Nine Weeks

CHEMICAL REACTIONS

SOL 3E

STOICHIOMETRY

SOL- 1G, 3B, 4B

THERMOCHEMISTRY

SOL- 3E, 4B, 5D, 5E, 5F

CHEMICAL KINETICS

SOL- 3F

GAS LAWS

SOL- 4A, 5A, 5B, 5C

TOPIC: CHEMICAL REACTIONS


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Directions: Determine the reaction type of each of the following reactions.

1. Fe2O3 + CO FeO + CO2

2. Cr + S8 Cr2S3

3. Eu + HF EuF3 + H2

4. NH4Cl HCl + NH3

5. C12H22O11 + O2 CO2 + H2O

6. Zn + HCl ZnCl2 + H2

7. SiO2 + C Si + CO

8. Pb(NO3)2 + H3AsO4 PbHAsO4 + HNO3

9. KClO3 KCl + O2

10. C6H6 + O2 CO2 + H2O

Directions: Complete the following table:

Reaction

Energy

Description

Sign of ΔH,

Positive or

Negative?

Temperature,

Increase or

Decrease?

Energy,

Product or

Reactant?

Exothermic

Endothermic

TOPIC: STOICHIOMETRY

CHEMISTRY

STANDARD CH. 3e


expressed in chemical formulas and balanced equations. Key concepts include:

e) reaction types


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a. 602 c. 0.00345 e. 34.08 g. 0.970

b. 1200 d. 0.1040 f. 3

2. Record your answer to the correct number of sig. figs.

a. (7.502 x 102 )(5.43 x 10

4)

b. 9.01 x 106

/ 1.22 x 105

3. Write the following numbers in scientific notation, or translate the numbers to

expanded notation.

a. 556,000,000,000 c. 9.32 x 10-5

b. 0.00000751 d. 7.68 x 107

4. Use conversion factors to solve the following: SHOW ALL WORK!!

a. Convert 250 m to km. c. Convert 3.54 L to kL.

b. Convert 18.50 kg to g. d. Convert 0.5420 kg to mg

5. Convert the following temperatures to Kelvin or to degree’s Celsius.

a. 100˚C b. 45˚C c. 273 K d. 400 K

CHEMISTRY

STANDARD CH. 1g


variables are measured, analyzed and evaluated produce observations and

verifiable data. Key concepts include:

g) mathematic manipulations (SI units, scientific notation, linear

equations, graphing, ratio and proportion, significant digits,

dimensional analysis)


and Ashanta Ruffin

DIRECTIONS: Balance the following equations:

1. Fe2O3 + CO FeO + CO2

2. Cr + S8 Cr2S3

3. Eu + HF EuF3 + H2

4. C12H22O11 + O2 CO2 + H2O

5. Zn + HCl ZnCl2 + H2

6. SiO2 + C Si + CO

7. Pb(NO3)2 + H3AsO4 PbHAsO4 + HNO3

8. NaCl + H2O Cl2 + H2 + NaOH

9. KClO3 KCl + O2

10. C6H6 + O2 CO2 + H2O

TOPIC: STOICHIOMETRY

CHEMISTRY STANDARD

CH. 3B

The student will investigate and understand how conservation of

energy and matter is expressed in chemical formulas and balanced

equations. Key concepts include b) balancing chemical equations.


and Ashanta Ruffin

1. Fill in the blanks.

a. The amount of a substance equal to 6.02 x 1023

particles is called a

________________________.

b. 6.02 x 1023

is also known as __________________________________.

c. If you have 1 mole of copper, you have 6.02 x 1023

________________________.

2. Molar (Formula) Mass. Determine the molar mass of the following and show all work

and units.

a. CuSO4 b. CaCO3 c. H3PO4 d. Al2(SO4)3

3. Mole Conversions. Solve the following problems. Show all work

a. How many grams are there in 1.55 x 1023

molecules of CO2?

b. How many atoms are there in 2.18 moles of nitrogen gas?

c. What is the volume, at STP, occupied by 4.30 moles of oxygen gas?

d. How many grams are there in 56.32 liters of carbon monoxide, at STP?

e. How many moles are in 8.67 x 1025

atoms of sulfur?

4. Percent Composition. Determine the percent composition of the following compounds.

Show all work.

a. NO2 b. Al2(SO4)3 c. What is the percent of Mg in MgCl2?

Solve the following problems and show all work.

5. Determine the empirical formula for 71.5% Ca and 28.5% O.

6. Determine the molecular formula for the empirical formula of C3H5O2, with a molar mass

of 146 g/mol.

7. 4Al + 3O2 → 2Al2O3 , How many moles of oxygen are required to react completely

with 0.84 mol of Al? How many moles of aluminum are needed to form 2.3 mol of

Al2O3?

8. The combustion of acetylene gas is represented by this equation: 2C2H2(g) + 5O2(g) →

4CO2(g) + 2H2O(g)

CHEMISTRY

STANDARD CH. 4B

The student will investigate and understand that quantities in a chemical reaction

are based on molar relationships. Key concepts include: b) stoichiometric

relationships.


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a. How many grams of oxygen are required to burn 13.0g of C2H2 ?

b. How many moles of C2H2 are needed to react completely with 98.0 g of water?

9. Calcium carbonate can be decomposed by heating. CaCO3(s) → CaO) (s) + CO2(g)

What is the percent yield of this reaction if 24.8 g of CaCO3 is heated to give 13.1 g of

CaO?

10. Copper reacts with sulfur to form copper (I) sulfide. 2Cu(s) + S(s) → Cu2S(s)

What is the limiting reactant when 80.0 g of Cu reacts with 25.0 g of S?

11. How many moles of CS2 form when 2.7 mol of C reacts? 5C + 2SO2 → CS2 +4CO

TOPIC: THERMOCHEMISTRY


and Ashanta Ruffin

See Previous “Try It” in Chemical Reactions for CH.3E

See previous “Try It” in Stoichiometry for CH.4b

CHEMISTRY STANDARD CH. 3E



e) reaction types

CHEMISTRY

STANDARD CH. 4B

The student will investigate and understand that quantities in a chemical

reaction are based on molar relationships. Key concepts include:

b) stoichiometric relationships


and Ashanta Ruffin

Solve the following problems. Show all work.

1. How much heat is released as a 75.0 g sample of ethanol gas at the boiling point condenses to

a liquid? Heat of vaporization is 879 J/g.

2. The heat of vaporization of water is 540. cal/g. How many calories would be needed to

convert 3 moles of water to vapor?

CHEMISTRY

STANDARD CH. 5E

The student will investigate and understand that the phases of matter

are explained by kinetic theory and forces of attraction between

particles. Key concepts include:

e) molar heats of fusion and vaporization


and Ashanta Ruffin


1. How much heat is lost as a 500. g cube of aluminum is cooled from 200°C to 25.0°C?

The specific heat for aluminum is 0.897 J/g°C

2. How much heat is required to melt 550.0 g of Cu that has already been heated to its

melting point? Heat of fusion is 205 J/g.

3. How many joules of heat are required to raise the temperature of 1.00 kg of water from

10.2˚C to 26.8˚C?

4. How much heat is released when 274 g of water cools from 85.2˚C to 38.4˚C?

TOPIC: CHEMICAL KINETICS

CHEMISTRY

STANDARD CH. 5F

The student will investigate and understand that the phases of

matter are explained by kinetic theory and forces of attraction

between particles. Key concepts include:

f) specific heat capacity


and Ashanta Ruffin

1. Define the following terms: catalyst, activated complex, activation energy, heating

curve, phase diagram, and heat capacity.

2. Draw labeled (reactants, products, activation energy, Δ H) reaction progress diagrams for

endothermic and exothermic reactions.

TOPIC: GAS LAWS

CHEMISTRY

STANDARD CH. 3F



f) reaction rates, kinetics and equilibrium


and Ashanta Ruffin


1. What volume of oxygen gas at STP can be produced when 17.5 grams of potassium

chlorate is decomposed? 2KClO3 → 2KCl + 3O2

2. Chlorine gas will react with 3.45 L of hydrogen gas to yield what mass of hydrogen

chloride gas at STP? H2 + Cl2 → HCl

CHEMISTRY

STANDARD CH. 4A



include:

a) Avogadro’s principle and molar volume.


and Ashanta Ruffin


1. A mixture of He, Ne, Ar and Xe has a total pressure of 2.5 atmospheres. Calculate

the partial pressure of the He if the pressure due to Ne, Ar and Xe, respectively, is

0.3, 0.8 and 1.0 atmospheres.

2. A sample of carbon dioxide gas was collected over water at 24 °C. If the pressure of

the sample was 758 mm Hg and the vapor pressure of water is 20. mm Hg, what is the

pressure due to the carbon dioxide.

CHEMISTRY

STANDARD CH. 5B



b) partial pressure and gas laws.


and Ashanta Ruffin

1. If 4.50 g of methane gas (CH4) is introduced into an evacuated 2.00 L container at 35°C,

what is the pressure in the container, in atmospheres?

2. How many grams of iron would be produced from 52.5g of iron (III) oxide reacting with

aluminum? Al + Fe2O3 → Al2O3 + Fe

3. In the reaction between calcium hydride and water, the theoretical yield of hydrogen gas

from 75.0 g of calcium hydride is 7.18 g. In running this reaction the actual amount of

hydrogen produced was 6.94 g. What is the percent yield of this reaction? CaH2 + H2O

→ Ca(OH)2 + H2

4. Hydrogen gas can be produced in the laboratory by the reaction of magnesium metal with

hydrochloric acid. Mg + HCl → MgCl2 + H2 What is the limiting reactant, when 6.00 g

of HCl is added to 5.00 g of Mg to product hydrogen gas?

CHEMISTRY

STANDARD CH. 5B


chemical reaction are based on molar relationships. Key

concepts include:

b) partial pressure and gas laws.


and Ashanta Ruffin

1. A gas with a volume of 300 mL at 150°C is heated until its volume is 600 mL. What is

the new temperature of the gas if the pressure is constant?

2. Calculate the volume of a gas in liters at 1 atm if its volume at 900 mmHg is 1500 mL.

3. A 3.50 L gas sample at 20°C and a pressure of 650 mmHg is allowed to expand to a

volume of 8.00 L. What is the final temperature in degrees Celsius if the final pressure of

the gas is 425 mm Hg?

4. A gas cylinder contains nitrogen gas at 10 atm and temperature of 20°C. The cylinder is

left in the sun and the temperature of the gas increases to 50°C. What is the pressure in

the cylinder?

CHEMISTRY

STANDARD CH. 5B

The student will investigate and understand that the phases of matter are

explained by kinetic theory and forces of attraction between particles. Key

concepts include:

b) partial pressure and gas laws


and Ashanta Ruffin

1. How is the normal boiling point of a substance related to its vapor pressure?

2. The atmospheric pressure of a mountain in South America is 400 mm Hg. Using the

vapor pressure curve of water from your textbook (page 401), determine the boiling

point of water at this altitude.

3. Sketch a graph of the vapor pressure of a liquid. Show the dependency of pressure

on temperature.

CHEMISTRY

STANDARD CH. 5C



concepts include:

c) vapor pressure.


and Ashanta Ruffin

Directions: Fill in the blanks with the correct response.

The particles in a ______________ phase are very close together in an orderly, fixed and usually

crystalline arrangement. _______________ is an endothermic change of state in which a solid

becomes a liquid. The temperature and pressure at which a solid becomes a liquid is its

____________________.

Because particles in the ____________ phase have enough kinetic energy to be able to move

past each other easily, they take the shape of their container. While many liquids flow readily,

many are resistant to flow, or are ________.

Because they are held close together, liquid particles are more affected by forces between

particles. They have attraction for each other, or ____________, as well as attraction for

particles of solid surfaces, called _______________. Liquids tend to form spherical drops

because of ____________, or the tendency to decrease their surface area to the smallest possible

size. Particles in a liquid can gain enough kinetic energy to leave the surface and become a gas

in a process called ______________.

Attractive forces between ____________ particles do not have a great effect, which makes the

particles independent of each other. The temperature and pressure at which the number of liquid

particles become gas particles is the same as the number of gas particles returning to the liquid

phase is called a substance’s _______________. Gas particles lose energy and become liquid

during ________________.

The process during which a liquid loses energy and becomes a sold is called ____________.

The temperature at which this change occurs is the _______________ of the substance.

When particles of solid become gas particles without first melting, the substance undergoes a

process called _____________. The reverse of this process, when a gas becomes a solid directly,

is called ________________.

CHEMISTRY

STANDARD CH. 5D



concepts include:

d) phase changes.


and Ashanta Ruffin

TOPIC: ORGANIC CHEMISTRY AND BIOCHEMISTRY

DIRECTIONS: Answer the questions below.

1. List the 3 factors that make the bonding of carbon atoms unique.

2. Draw Lewis structures, identify shape, and describe polarities of the following

molecules: CH4, C2H6, CH3CH2OH, C6H6

3. List 6 natural, biological polymers.

4. List 6 common pharmaceuticals that are organic compounds.

5. List 6 man-made, synthetic polymers.

CHEMISTRY

STANDARD CH. 6A, B

The student will investigate and understand how basic chemical properties relate to

organic chemistry and biochemistry. Key concepts include:

a) Unique properties of carbon that allow multi-carbon compounds

b) Uses in pharmaceuticals and genetics, petrochemicals, plastics and food


and Ashanta Ruffin

FOURTH Nine Weeks

SOLUTIONS

SOL- 3F, 4D, 5G

ACIDS AND BASES SOL- 4D


and Ashanta Ruffin

TOPIC: SOLUTIONS

DIRECTIONS: Solve the following problems. Show all work.

1. What is the molality of a solution in which 3.0 moles of NaCl is dissolved in 1.5 kg of

water?

2. How many grams of I2 should be added to 750 g of CCl4 to prepare a 0.020 m solution?

3. Calculate the molarity of 5.85 g of NaCl in 2.00 L of solution.

4. How many moles are needed to make 2.0 L of 0.30M solution of Na2SO4?

5. How would you correctly prepare 125 mL of a 0.30M solution of copper(II) sulfate

(CuSO4) from a 2.00M solution of CuSO4?

6. What is the boiling point of a solution that contains 1.25 mol of CaCl2 in 1400 g of

water? Kb for water = 0.512 °C/m

7. What is the freezing point of Na2SO4 in 1750 g of water? Kf of water = 1.86 °C/m

CHEMISTRY

STANDARD CH. 4C



c) solution concentrations.


and Ashanta Ruffin


1. What is a reversible chemical reaction? How does the format of the arrow differ from

a reaction that goes to completion?

2. What is Le Châtelier’s principle? How would the equilibrium in the following

reaction be impacted by:

CO (g) + O2 (g) ↔ CO2 (g)

a. increasing [CO2]?

b. decreasing pressure?

c. decreasing [CO]?

CHEMISTRY

STANDARD CH. 3F



include:

f) reaction rates, kinetics and equilibrium


and Ashanta Ruffin

TOPIC: ACIDS, BASES, and SOLUTIONS


1. Define the following terms: conjugate acid, acid, base, conjugate base, Bronsted-Lowry

acid, Bronsted-Lowry base, indicator, neutralization and pH scale.

2. Solve the following problems.

a. Calculate the pH and pOH for each solution: [H+] = 5.0 x 10

-6 and [OH

-] = 4.5 x 10

-11

b. Calculate the [H+] for each solution: pH = 5.0 and pH = 12.20

3. List the properties of an acid and a base.

4. Identify the conjugate acid and conjugate base in the following equation.

NH3 + H2O ↔ NH4+ + OH

-

CHEMISTRY

STANDARD CH. 4D

The student will investigate and understand that quantities in a chemical reaction are

based on molar relationships. Key concepts include:

d) acid/base theory: strong electrolytes, weak electrolytes, and nonelectrolytes;

dissociation and ionization, pH and pOH; and the titration process.


and Ashanta Ruffin


1. What is the freezing point of a solution of 200 grams of ethylene glycol (HOCH2CH2OH)

mixed with 400 grams of water?

2. What is the boiling point elevation of a solution of 26.8 grams of NaCl dissolved in 500

grams of water?

3. Calculate the boiling point and freezing point of a solution of 220 g of sucrose

(C12H22O11) dissolved in 1.0 kg of water. How does this compare to the boiling point and

freezing point of pure water?

CHEMISTRY

STANDARD CH. 5G

The student will investigate and understand that the phases of

matter are explained by kinetic theory and forces of attraction

between particles. Key concepts include:

g) colligative properties.


and Ashanta Ruffin

ANSWERS

FIRST NINE WEEKS STANDARD CH. 1 F

1. Experimental Value = 1.44 g Accepted Value = 1.54 g

6.5%

2. Experimental Value = 22.2 L Accepted Value = 22.4 L

0.89%

3. Experimental Value = 128.6 mg Accepted Value =128.3 mg

0.23%

4. Experimental Value = 9.98 x 10-3

g Accepted Value =1.03 x 10-2

g

3.11%

STANDARD CH. 2H

Chemical and Physical Properties

The student will be given an object or substance and must identify the physical and chemical properties of that

object. (This assignment is to be given after lecture on chemical and physical properties and how to correctly

identify each.)

1. Describe the chemical properties of this object below, citing any evidence you have collected:

Answers will vary.

2. Describe the physical properties of this object below, citing any evidence you have collected:

Answers will vary.

STANDARD CH. 2I

.Students will create a two page foldable for the models of an atom. Each outside flap will be the names of the

scientists (Democritus, Dalton, Rutherford, Bohr), and the inside picture will be each scientist’s contribution to the

historical model. A one page foldable will be created for the quantum models with Heisenberg and Planck. Students

will be creative using mnemonics and/or graphics.

Answers will vary.


and Ashanta Ruffin

STANDARD CH. 2A

Element Average Atomic mass Mass number Atomic number

Ne 20.179 20 10

Al 26.9812 27 13

Ge 72.59 72 32

P 30.97376 31 15

Br 79.904 80 35

Ca 40.08 40 20

K 39.0983 39 19

I 126.904 127 53

Sr 87.62 88 38

Sn 118.69 119 50

Atomic mass answers may slightly vary depending on the Periodic Table used.

STANDARD CH. 2C

Warm-up: Complete the following chart:

Subatomic Particle Symbol Charge Relative mass Location in atom

protons P + 1 In nucleus

neutrons N 0 1 In nucleus

electrons E - 0 Outside nucleus or electron

cloud

Atomic Structure

Element/Ion Atomic

Number

Atomic

Mass

Mass

Number

Protons Neutrons Electrons

3H 1 1.00797 3 1 2 1

1H

+ 1 1.00797 1 1 0 0

12C 6 12.0115 12 6 6 6

7Li

+ 3 6.941 7 3 4 2

35Cl

- 17 35.453 35 17 18 18

39K 19 39.0983 39 19 20 19

24Mg

2+ 12 24.305 24 12 12 10

77As

3- 33 74.922 77 33 44 36

108Ag 47 107.868 108 47 61 47


and Ashanta Ruffin

30S

-2 16 32.064 30 16 14 18

238U

92 238.03 238 92 146 92

STANDARD CH. 2B

DIRECTIONS: Answer the following questions

Average Atomic Mass

1. Rubidium has two common isotopes, Rb-85 and Rb-87. If the abundance of Rb-85 is 72.2%

and the abundance of Rb-87 is 27.8%, what is the average atomic mass of rubidium? 85.556

2. Uranium has 3 common isotopes. If the abundance of

U-234 is 0.01%, the abundance of U-235 is 0.71% and the abundance of U-238 is 99.28%, what is

the average atomic mass? 237.9783

3. Titanium has five common isotopes: Ti-46 (8.0%), Ti-47 (7.8%), Ti-48 (73.4%), Ti-49 (5.5%),

and Ti-50 (5.3%). What is the average atomic mass of titanium? 47.923

4. Explain why atoms have different isotopes. In other words, how is it that helium can have

three different sized atoms and they all are still the element Helium. Atoms of the same element will have the

same number of protons but different numbers of neutrons.

5. Draw and label 3 possible isotopes of hydrogen. Which isotope can you predict to be the

most abundant? Why? Correctly name the 3 isotopes using the symbol “H”?

Answers will vary.

6. Select an element on the PTOE. Create 4 isotopes for your element and form an

average atomic mass calculation to support the given atomic mass.

Answers will vary.

STANDARD CH. 3A

Writing Binary Formulas

Cation Anion Formula Cation Anion Formula

Na+ Cl

- NaCl Fe

+2 O

-2 FeO

Ba+2

F- BaF2 Fe+3

O-2

Fe2O3

K+ S

-2 K2S Cr

+2 S

-2 CrS

Li+ Br

- LiBr Cr

+3 S

-2 Cr2S3

Al+3

I- AlI3 Cu

+ Cl

- CuCl

Zn+2

S-2

ZnS Cu+2

Cl- CuCl2

Ag+ O

-2 Ag2O Pb

+2 O

-2 PbO


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Mg+2

P-3

Mg3P2 Pb+4

O-2

PbO2

Ni+2

O-2

NiO Mn+2

Br- MnBr2

Ni+3

O-2

Ni2O3 Mn+4

Br- MnBr4

STANDARD CH. 2 D, E

Counting Valence Electrons

Element Group Number Number of Valence Electrons

Ne 18 8

Al 13 3

Ge 14 4

P 15 5

Br 17 7

Ca 2 2

K 1 1

I 17 7

Sr 2 2

Sn 14 4

STANDARD CH. 2 F

DIRECTIONS: State the periodic trend and explain.

PERIODIC TRENDS

LEFT TO RIGHT

EXPLAINATION TOP TO BOTTOM

EXPLAINATION

ATOMIC RADII DECREASE STRONGER

NUCLEAR

ATTRACTION

INCREASE MORE ENERGY

LEVELS

ELECTRONEGATIVITY INCREASE MORE VALNCE

ELECTRONS

DECREASE LARGER RADIUS

SHIELDING EFFECT SAME SAME ENERGY

LEVEL

INCREASE MORE ENERGY

LEVELS

IONIZATION ENERGY INCREASE MORE VALENCE

ELECTRONS

DECREASE MORE SHIELDING

STANDARD CH. 2 C

Ions and Subatomic Particles

Ion Symbol Protons Electrons Charge

S2-

16 18 -2

K1+

19 18 +1

Ba2+

56 54 +2

Fe3+

26 23 +3

Fe2+

26 24 +2


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F1-

9 10 -1

O2-

8 10 -2

P3-

15 18 -3

Sn4+

50 46 +4

Sn2+

50 48 +2

N3-

7 10 -3

Br1-

35 36 -1

Mg2+

12 10 +2

Cu1+

29 28 +1

Cu2+

29 27 +2

U6+

92 86 +6

Mn5+

25 20 +5

Cl1-

17 18 -1

Se2-

34 36 -2

SECOND NINE WEEKS SOL 3C

1. D 2.A 3.C 4. C 5. B 6. C 7. D 8. A 9. D 10. D

SOL 3 A,C,D

1. A 2. D 3. B 4. Group 15 5. A 6. B 7. D 8. C 9. A

SOL 4A

1. C 2. C 3. A 4. C 5. A

THIRD NINE WEEKS CHEMISTRY

STANDARD CH. 3e

11. Fe2O3 + CO FeO + CO2 double replacement

12. Cr + S8 Cr2S3 synthesis

13. Eu + HF EuF3 + H2 single replacement

14. NH4Cl HCl + NH3 decomposition

15. C12H22O11 + O2 CO2 + H2O combustion

16. Zn + HCl ZnCl2 + H2 single replacement

17. SiO2 + C Si + CO single replacement


and Ashanta Ruffin

18. Pb(NO3)2 + H3AsO4 PbHAsO4 + HNO3 double replacement

19. KClO3 KCl + O2 decomposition

20. C6H6 + O2 CO2 + H2O combustion

Directions: Complete the following table:

Reaction Energy

Description

Sign of ΔH, Positive

or Negative?

Temperature,

Increase or

Decrease?

Energy,

Product or Reactant?

Exothermic - increase product

Endothermic + decrease reactant

STANDARD CH. 1g


c. 602 3 c. 0.00345 3 e. 34.08 4 g. 0.970 3

d. 1200 2 d. 0.1040 4 f. 3 1

7. Record your answer to the correct number of sig. figs.

c. (7.502 x 102 )(5.43 x 10

4) 4.07 x 10

7

d. 9.01 x 106 / 1.22 x 10

5 7.39 x 10

1

8. Write the following numbers in scientific notation, or translate the numbers to regular notation.

c. 556,000,000,000 5.56 x 1011

c. 9.32 x 10-5

0.0000932

d. 0.00000751 7.51 x 10-6

d. 7.68 x 107

76,800,000

9. Use conversion factors to solve the following: SHOW ALL WORK!!

c. Convert 250 m to km. 0.25 km c. Convert 3.54 L to kL. 3.54 x 10-3

d. Convert 18.50 kg to g. 1.85 x 104 d. Convert 0.5420 kg to mg 5.42 x 10

5

10. Convert the following temperatures to Kelvin or to degree’s Celsius.

b. 100˚C 373K b. 45˚C 318K c. 273 K 0°C d. 400 K 127°C

CH. 3B

21. Fe2O3 + CO 2FeO + CO2

22. 16Cr + 3S8 8Cr2S3

23. 2Eu + 6HF 2EuF3 + 3H2


and Ashanta Ruffin

24. C12H22O11 + 12 O2 12 CO2 + 11H2O

25. Zn + 2 HCl ZnCl2 + H2

26. SiO2 + 2C Si + 2CO

27. Pb(NO3)2 + H3AsO4 PbHAsO4 + 2 HNO3

28. 2NaCl + 2 H2O Cl2 + H2 + 2NaOH

29. 2 KClO3 2KCl + 3O2

30. 2C6H6 + 15O2 12CO2 + 6 H2O

STANDARD CH. 4B

12. Fill in the blanks.

d. The amount of a substance equal to 6.02 x 1023

particles is called a _mole_______________________.

e. 6.02 x 1023

is also known as ____Avogadro’s number_____________.

f. If you have 1 mole of copper, you have 6.02 x 1023

__atoms__________.

13. Molar (Formula) Mass. Determine the molar mass of the following and show all work and units.

b. CuSO4 159.58g/mol b. CaCO3 100.06g/mol c. H3PO4 97.96g/mol d. Al2(SO4)3 342.05g/mol

14. Mole Conversions. Solve the following problems. Show all work

f. How many grams are there in 1.55 x 1023

molecules of CO2? 11.3g

g. How many atoms are there in 2.18 moles of nitrogen gas? 1.31 x 1024

atoms

h. What is the volume, at STP, occupied by 4.30 moles of oxygen gas?96.3L i. How many grams are there in 56.32 liters of carbon monoxide, at STP?70.40g

j. How many moles are in 8.67 x 1025

atoms of sulfur?144 moles

15. Percent Composition. Determine the percent composition of the following compounds. Show all work.

b. NO2 30.5%N, 69.5%O b. Al2(SO4)3 15.8%Al, 28.1%S, 56.1%O c. What is the percent of Mg in

MgCl2?25.5%Mg

Solve the following problems and show all work.

16. Determine the empirical formula for 71.5% Ca and 28.5% O. CaO

17. Determine the molecular formula for the empirical formula of C3H5O2, with a molar mass of 146 g/mol.

C6H10O4

18. 4Al + 3O2 → 2Al2O3 , How many moles of oxygen are required to react completely with 0.84 mol of

Al? .63 mol O2 How many moles of aluminum are needed to form 2.3 mol of Al2O3?4.6 mol Al

19. The combustion of acetylene gas is represented by this equation: 2C2H2(g) + 5O2(g) → 4CO2(g) + 2H2O(g)

a. How many grams of oxygen are required to burn 13.0g of C2H2 ? 39.9 g O2 b. How many moles of C2H2

are needed to react completely with 98.0 g of water? 5.44 mol C2H2

20. Calcium carbonate can be decomposed by heating. CaCO3(s) → CaO(s) + CO2(g)

What is the percent yield of this reaction if 24.8 g of CaCO3 is heated to give 13.1 g of CaO?94.2%

21. Copper reacts with sulfur to form copper (I) sulfide. 2Cu(s) + S(s) → Cu2S(s)


and Ashanta Ruffin

What is the limiting reactant when 80.0 g of Cu reacts with 25.0 g of S?LR=Cu

22. How many moles of CS2 form when 2.7 mol of C reacts? 5C + 2SO2 → CS2 +4CO

0.54 mol CS2

CHEMISTRY STANDARD CH. 3E

See Previous “Try It” in Chemical Reactions for CH.3E

STANDARD CH. 4B

See previous “Try It” in Stoichiometry for CH.4b

STANDARD CH. 5D


3. How much heat is released as a 75.0 g sample of ethanol gas at the boiling point condenses to a liquid? Heat of

vaporization is 879 J/g.6.59 x 104J

4. The heat of vaporization of water is 540. cal/g. How many calories would be needed to convert 3 moles of

water to vapor?3 x 104 cal

STANDARD CH. 5E


5. How much heat is lost as a 500. g cube of aluminum is cooled from 200°C to 25.0°C? The specific heat for

aluminum is 0.897 J/g°C 8 x 104 J

6. How much heat is required to melt 550.0 g of Cu that has already been heated to its melting point? Heat of

fusion is 205 J/g. 1.128 x 105 J

7. How many joules of heat are required to raise the temperature of 1.00 kg of water from 10.2˚C to 26.8˚C?

6.95 x 104 J

8. How much heat is released when 274 g of water cools from 85.2˚C to 38.4˚C?

-5.37 x 104 J

STANDARD CH. 3F

1. Define the following terms: catalyst, activated complex, activation energy, heating curve, phase diagram,

and heat capacity.

a. Catalyst – a substance that changes the rate of a chemical reaction without being consumed.


and Ashanta Ruffin

b. Activated complex – molecule in an unstable state intermolecular to the reactant and products in

the chemical reaction.

c. Activation energy – the minimum amount of energy required to start a chemical reaction.

d. Heating curve – shows the change in temperature of a substance as heat is added and the substance

undergoes phase changes.

e. Phase diagram – graph of the relationship between the physical state of a substance, temperature,

and pressure of the substance.

f. Heat capacity – energy needed to increase the temperature of 1 mole (1 gram) of the substance by

1°C.

2. Draw labeled (reactants, products, activation energy, Δ H) reaction progress diagrams for endothermic and

exothermic reactions.

STANDARD CH. 4A


1. What volume of oxygen gas at STP can be produced when 17.5 grams of potassium chlorate is

decomposed? 2KClO3 → 2KCl + 3O2 4.80L O2

2. Chlorine gas will react with 3.45 L of hydrogen gas to yield what mass of hydrogen chloride gas

at STP? H2 + Cl2 → HCl 11.2g HCl

STANDARD CH. 4C


1. A mixture of He, Ne, Ar and Xe has a total pressure of 2.5 atmospheres. Calculate the partial pressure

of the He if the pressure due to Ne, Ar and Xe, respectively, is 0.3, 0.8 and 1.0 atmospheres. 0.4 atm

2. A sample of carbon dioxide gas was collected over water at 24 °C. If the pressure of the sample was

758 mm Hg and the vapor pressure of water is 20. mm Hg, what is the pressure due to the carbon

dioxide. 738 mmHg


and Ashanta Ruffin

STANDARD CH. 4D

1. If 4.50 g of methane gas (CH4) is introduced into an evacuated 2.00 L container at 35°C,

what is the pressure in the container, in atmospheres? 3.5 atm

2. How many grams of iron would be produced from 52.5g of iron (III) oxide reacting with aluminum? Al +

Fe2O3 → Al2O3 + Fe 36.7 g

3. In the reaction between calcium hydride and water, the theoretical yield of hydrogen gas from 75.0 g of

calcium hydride is 7.18 g. In running this reaction the actual amount of hydrogen produced was 6.94 g.

What is the percent yield of this reaction? CaH2 + H2O → Ca(OH)2 + H2 96.4%

4. Hydrogen gas can be produced in the laboratory by the reaction of magnesium metal with hydrochloric

acid. Mg + HCl → MgCl2 + H2 What is the limiting reactant, when 6.00 g of HCl is added to 5.00 g of Mg

to product hydrogen gas? LR=HCl

STANDARD CH. 5A

1. A gas with a volume of 300 mL at 150°C is heated until its volume is 600 mL. What is

the new temperature of the gas if the pressure is constant? 800K

2. Calculate the volume of a gas in liters at 1 atm if its volume at 900 mmHg is 1500 mL.

2 L

3. A 3.50 L gas sample at 20°C and a pressure of 650 mmHg is allowed to expand to a volume of 8.00 L.

What is the final temperature in degrees Celsius if the final pressure of the gas is 425 mm Hg? 200°C

4. A gas cylinder contains nitrogen gas at 10 atm and temperature of 20°C. The cylinder is left in the sun and

the temperature of the gas increases to 50°C. What is the pressure in the cylinder? 10 atm

STANDARD CH. 5B

1. How is the normal boiling point of a substance related to its vapor pressure?

When you increase the temperature of a system to the point at which the vapor pressure of a substance

is equal to the standard atmospheric pressure, you have reached the substance’s normal boiling point.

2. The atmospheric pressure of a mountain in South America is 400 mm Hg. Using the vapor pressure

cure of water from your textbook (page 401), determine the boiling point of water at this altitude.

84°C

3. Sketch a graph of the vapor pressure of a liquid. Show the dependency of pressure on temperature.


and Ashanta Ruffin

STANDARD CH. 5C

Directions: Fill in the blanks with the correct response.

The particles in a __solid________ phase are very close together in an orderly, fixed and usually crystalline

arrangement. __Melting_______ is an endothermic change of state in which a solid becomes a liquid. The

temperature and pressure at which a solid becomes a liquid is its _heat of fusion___.

Because particles in the __liquid______ phase have enough kinetic energy to be able to move past each other easily,

they take the shape of their container. While many liquids flow readily, many are resistant to flow, or are

viscous_____.

Because they are held close together, liquid particles are more affected by forces between particles. They have

attraction for each other, or cohesion__, as well as attraction for particles of solid surfaces, called adhesion_.

Liquids tend to form spherical drops because of surface tension_, or the tendency to decrease their surface area to

the smallest possible size. Particles in a liquid can gain enough kinetic energy to leave the surface and become a gas

in a process called _vaporization______.

Attractive forces between __gas____ particles do not have a great effect, which makes the particles independent of

each other. The temperature and pressure at which the number of liquid particles become gas particles is the same

as the number of gas particles returning to the liquid phase is called a substance’s __heat of vaporization___.

Gas particles lose energy and become liquid during _condensation____.

The process during which a liquid loses energy and becomes a sold is called freezing. The temperature at which this

change occurs is the _freezing point______ of the substance.

When particles of solid become gas particles without first melting, the substance undergoes a process called

sublimation___. The reverse of this process, when a gas becomes a solid directly, is called deposition____.

STANDARD CH.6A, B

1. List the 3 factors that make the bonding of carbon atoms unique. Strong single bond, not extremely reactive, different bonding arrangements


and Ashanta Ruffin

2. Draw Lewis structures, identify shape, and describe polarities of the following molecules: CH4, C2H6,

CH3CH2OH, C6H6 CH4 –tetrahedron, non-polar C2H6,- tetrahedron at each carbon, non-polar

CH3CH2OH – tetrahedron at each carbon, polar due to the oxygen

C6H6 – hexagonal, planar, non-polar

3. List 6 natural, biological polymers.

DNA, RNA, starch, cellulose, protein, poly-lipids, etc.

4. List 6 common pharmaceuticals that are organic compounds.

aspirin, vitamins, insulin, Tylenol, ibuprofen, Ritalin, etc.

5. List 6 man-made, synthetic polymers. Nylon, polyethylene, polypropylene, PVC, polystyrene, Kevlar, etc.

FOURTH NINE WEEKS

STANDARD CH. 4E

1. What is the molality of a solution in which 3.0 moles of NaCl is dissolved in 1.5 kg of water? 2.0 m

2. How many grams of I2 should be added to 750 g of CCl4 to prepare a 0.020 m solution?

3.8 g

3. Calculate the molarity of 5.85 g of NaCl in 2.00 L of solution. 0.0500 M

4. How many moles are needed to make 2.0 L of 0.30M solution of Na2SO4? 0.60 mol

5. How would you correctly prepare 125 mL of a 0.30M solution of copper(II) sulfate (CuSO4) from a 2.00M

solution of CuSO4? 19 mL

6. What is the boiling point of a solution that contains 1.25 mol of CaCl2 in 1400 g of water? Kb for water =

0.512 °C/m 101.37°C = 101°C

7. What is the freezing point of Na2SO4 in 1750 g of water? Kf of water = 1.86 °C/m

-3.19°C

STANDARD CH. 4F


3. What is a reversible chemical reaction? A chemical reaction in which the products reform the original

reactants. How does the format of the arrow differ from a reaction that goes to completion? Arrows

that point in opposite directions.

4. What is Le Châtelier’s principle? States that a system in equilibrium will oppose a change in a way that

helps eliminate the change. How would the equilibrium in the following reaction be impacted by:

CO (g) + O2 (g) ↔ CO2 (g)

d. increasing [CO2]? Shift to the left

e. decreasing pressure? Shift to the right

f. decreasing [CO]? Shift to the left


and Ashanta Ruffin

STANDARD CH. 4G


1. Define the following terms: conjugate acid, acid, base, conjugate base, Bronsted-Lowry

acid, Bronsted-Lowry base, indicator, neutralization and pH scale.

Conjugate acid- compound with a hydrogen ion

Acid – donates a proton Base – accepts a proton

Conjugate base – same compound of the acid but without the hydrogen ion

Bronsted-Lowery acid – substance that is capable of donating a proton

Bronsted-Lowery base – substance that is capable of accepting a proton

Indicator – dyes that can be added that will change color in the presence of an acid or base

Neutralization – adding an acid to a base to produce a salt and water

pH scale – a way of expressing the strength of acids and bases

2. Solve the following problems. a. Calculate the pH for each solution: [H

+] = 5.0 x 10

-6 pH = 5.3and [OH

-] = 4.5 x 10

-11 pH = 3.7

b. Calculate the [H+] for each solution: pH = 5.0 [H] = 1x10

-5 pH = 12.20 [H] = 6.3 x 10

-13

1. List the properties of an acid and a base.

Acid: produces hydrogen ions, taste sour, corrodes metal, electrolyte, pH<7, reacts with a base, litmus

paper turns red

Base: produces hydroxide ions, taste bitter, electrolytes, reacts with acids, pH>7, litmus paper turns

blue

4. Identify the conjugate acid and conjugate base in the following equation.

NH3 + H2O ↔ NH4+ + OH

-

Conjugate acid: NH4+

conjugate base: NH3

Conjugate acid: H2O, conjugate base: OH-

STANDARD CH. 5F


1. What is the freezing point of a solution of 200 grams of ethylene glycol (HOCH2CH2OH) mixed with 400

grams of water? -14.9°C

2. What is the boiling point elevation of a solution of 26.8 grams of NaCl dissolved in 500 grams of water?

100.9°C

3. Calculate the boiling point and freezing point of a solution of 220 g of sucrose (C12H22O11) dissolved in 1.0

kg of water. Tb = 100.3°C Tf = -1.2°C How does this compare to the boiling point and freezing point of

pure water? Both are close to pure water.

CHEMISTRY STANDARD CH. 4G

See previous “Try It” in Solutions for CH.4G


and Ashanta Ruffin

REFERENCES

www.222.nano.gov

www.chemmybear.com

www.chemistry.merlot.org

Holt Chemistry Textbook http://my.hrw.com/

www.nsta.org

Prentice Hall Textbook http://www.phschool.com/home.html

Virginia Department of Education Blueprint

http://www.doe.virginia.gov/testing/sol/blueprints/science_blueprints/blueprint_ch

emistry.pdf

Virginia Department of Education Framework

http://www.doe.virginia.gov/testing/sol/frameworks/science_framewks/framework

_science-chem.pdf

Virginia Department of Education Scope and Sequence

http://www.doe.virginia.gov/testing/sol/scope_sequence/science_scope_sequence/s

copeseq_science_chemistry.pdf

Virginia Department of Education Standards of Learning

http://www.doe.virginia.gov/testing/sol/standards_docs/science/courses/stds_chemi

stry.pdf

www.scitoys.com

www.stevespanglescience.com

http://www.222.nano.gov/

http://www.chemmybear.com/

http://www.chemistry.merlot.org/

http://my.hrw.com/

http://www.nsta.org/

http://www.phschool.com/home.html

http://www.doe.virginia.gov/testing/sol/blueprints/science_blueprints/blueprint_chemistry.pdf

http://www.doe.virginia.gov/testing/sol/blueprints/science_blueprints/blueprint_chemistry.pdf

http://www.doe.virginia.gov/testing/sol/frameworks/science_framewks/framework_science-chem.pdf

http://www.doe.virginia.gov/testing/sol/frameworks/science_framewks/framework_science-chem.pdf

http://www.doe.virginia.gov/testing/sol/scope_sequence/science_scope_sequence/scopeseq_science_chemistry.pdf

http://www.doe.virginia.gov/testing/sol/scope_sequence/science_scope_sequence/scopeseq_science_chemistry.pdf

http://www.doe.virginia.gov/testing/sol/standards_docs/science/courses/stds_chemistry.pdf

http://www.doe.virginia.gov/testing/sol/standards_docs/science/courses/stds_chemistry.pdf

http://www.scitoys.com/

http://www.stevespanglescience.com/

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