Table of ContentsPhysical and Chemical Changes

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Physical and Chemical Changes in Matter Reading……………….……...………………5Physical and Chemical Changes in Matter Questions…………………..…………...……7Changes in State of Water Reading…………………………......…………..…………….8Changes in State of Water Questions……………………………………………………...9Chemical Changes Reading and Questions………………………………………………10Reaction of Matter Worksheet……………………………………..…………………….11Properties of Matter Worksheet………………………………………………………….12Physical vs. Chemical Properties Worksheet………………………….…………………13Physical vs. Chemical Changes Worksheet……………………...………………….…...14

Chemical Bonding

Naming Compounds………………………….…………………………….……………15Writing Binary Formulas………………………………………………………………...26Naming Binary Compounds (Ionic)………….………………………………………….27Naming Binary Compounds (Covalent)……………………………………………...….28Formulas with Polyatomic Ions………………………………………………………….29Naming Compounds (Mixed)………………….……………………………...…………30Writing Formulas from Names………………………………………………….………31

Balancing Equations

Counting Atoms Worksheet……….……………………………………………………32Law of Conservation of Mass Reading & Questions……….…………….…………….34Balancing Chemical Equations Reading and Questions……..………………………....35Balancing Equations Challenge………………………………..……………………….37Balancing Equations – Mr. Murray Page……………………..……….………….…….38Balancing Equations Practice Worksheets Multiple Choice………..……….……….....39Balancing Equations Worksheet……………………………………..……….………....43The Laws and Principles of Chemical Reactions – Mr. Murray Page……..…………....44Conservation of Mass Worksheet…………………………………………………..…...45Exothermic vs Endothermic Reactions Wksht ……………………….……..…………46Exothermic and Endothermic Lab…………………………………….……..…………47

Polarity of Water

Structure of Water Reading…………………………………..…….….………………..51Water as a Universal Solvent Reading……………………...……………………..……52Structure of Water Questions……………………….………..…….….………………..53Water as a Universal Solvent Questions……………..……...……………………..……54Solutions – Mr. Murray Page ….………………….……………………………………56Willy the Water Strider Lab.. ….………………….……………………………………57Polarity of Molecules Worksheet……………………………………………………….61Solubility (Polar vs. Non-polar) Worksheet ……….……………..……………….……62Polar vs. Non-Polar Lab…………………………………………………………….…..63

Solutions and Solubility

What is Your Favorite Flavor? Reading and Questions.………………..……….…….65

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Chromatography Lab…………………………………..……………….…………..….67Concentrations on Solutions Reading & Questions…………………..……………….71A Tasty Solution Lab…………………………………………….…….………………73Colloids Reading…………………………………………………..…….……………..75Solutions, Colloids, and Suspensions Worksheet……………...………………………76Colloid Lab…………………………………………………………….……………….77Solubility and Factors that Affect it Reading and Questions.………….………...…….79Temperature Questions…………….………………………………….……………….81Solubility Curves Worksheets…………………………………..………………..…….83Detergents Helpful or Harmful?……………………………..……………………..….85Rate at which dissolving occurs Reading and Questions…………………....…..…….87Electrolytic Behavior Reading and Questions……………….………………..………88

Acids and Bases

Acid and Base Reading……………………..……...……………………….…………91Acid and Base Questions………………………………………..……………….……93Acid, Base, or Salt Worksheet……………….……………………..……………..…..94The pH Scale Reading………….……………………..……………..………….…….95The pH Scale Questions………………………………………...…………………….96A Balance in the Body Worksheet……………………….…………..………….……97pH Worksheet……….……………………………………….………………….……99Indicators and Solutions Lab………………………………………..……………….101Acids and Bases – Mr. Murray Page……………………………….………………..105What does an Antacid do? Lab ……………………………………………………...107Acids and Bases Worksheet…………………………………………………………109Strength of Acids and Bases Worksheet………………………….…………………110

Nuclear Chemistry

The Three Types of Radiation Reading……………………….…….……………….111Radiation Hazards and Uses…………………………………………………………112Nuclear Power- Mr. Murray Page…………………………………...………………113Radiation and Medicine Worksheet………………………………….…..………….114Nuclear Fission and Fusion Reading……………………………………..…………115Fission versus Fusion - Mr. Murray Page………………………………..………….116The Life Cycle of a Star Reading and Questions…………………..…….………….117

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Physical and Chemical Changes in Matter Questions

Read the preceding pages and answer the questions in complete sentences

1. What products are produced when burning a candle?

2. What happens when a chemical changes takes place?

3. Compare a chemical change and a physical change.

4. Where do chemical changes occur?

5. What is dissolving?

6. What does physical changes involve?

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Changes in State of WaterRead the preceding page and answer the following questions in complete sentences

1. What do we call water in each of its states?

2. At what temperature does water change from one state to another?

3. How does ice change to steam?

4. What role does energy lay in water changing its state?

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1. What is a chemical change?

2. What happens in a chemical change?

3. What are some indicators that a chemical change is taking place?

4. What role does energy play in a chemical change?

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Reactions of Matter

Decide whether the changes listed below are chemical or physical. Write your answer in the blank provided.

_______________________________ Dissolving sugar in coffee

_______________________________ Burning coal

_______________________________ Mining coal

_______________________________ Boiling an egg

_______________________________ Boiling water

_______________________________ Heating an iron nail

_______________________________ Adding food coloring to water

_______________________________ Dipping blue litmus paper in lemon juice

_______________________________ Dissolving carbon dioxide in water

_______________________________ Adding vinegar to baking soda to form CO2

_______________________________ Mixing salt and pepper

_______________________________ Mixing lye and hydrochloric acid

_______________________________ Melting a nail

_______________________________ Letting a nail rust

Study the two drawings and label them either physical or chemical change

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Naming CompoundsIONIC COMPOUNDS versus MOLECULAR COMPOUNDS

Ionic compound: consist of cations (positive ions) and anions (negative ions) held together by electrostatic attractions--Usually metal + nonmetal(s)--Made of monatomic ions, polyatomic ions, and/or both

--Monatomic ions; consist of a single atom--Polyatomic ions; consist of more than one atom

Molecular compound: consist of nonmetals atoms bonded together by shared electrons (covalent bonding)--acid: a molecular compound that releases hydrogen ion (H+)

when dissolved in water

NAMING MONATOMIC CATIONS:

Metal atoms lose valence electrons to form positively charged ions, called cations. An ion formed from an individual atom is a monatomic (or monoatomic) cation.

I. Groups IA, IIA, IIIA, elements silver (Ag) and zinc (Zn) form only one type of ion; Group IA elements form +1 ions: H+, Li+, Na+, K+

Group IIA elements form +2 ions; Be+2, Mg +2, Ca+2, Sr+2, Ba+2

Group IIIA elements form +3 ions; Al+3

Silver ion = Ag+; zinc ion = Zn+2

When a Group IA, IIA, IIIA element, silver, or zinc forms an ion, it is named:

Element name + ion

e.g. Na+ = sodium ion Sr+2 = strontium ion Zn+2 = zinc ion

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II. The Stock system is used to name transition metals and other metals that form more than one ion:

--iron (Fe) forms two ions: Fe+2 and Fe+3

--lead (Pb) forms two ions: Pb+2 and Pb+4

When a metal can form more than one ion, each ion is named:

Element name (charge in Roman numberals) + ion

e.g. Fe+2 = iron (II) ion Pb+2 = lead (II) ion Cu+ = copper (I) ionFe+3 = iron (III) ion Pb+4 = lead (IV) ion Cu+2 = copper (II) ion

Name each of the following monatomic cations:

Li+ = _________________________ Ba+2 = ___________________________

Ag+ = _________________________ Cu+2 = ____________________________

Al+3 = _________________________ Mg+2 = ____________________________

Mn+2 = ________________________ Sn+4 = _____________________________

H+ = __________________________ Co+3 = ____________________________

Fe+3 = ________________________ Na+ = _____________________________

K+ = __________________________ Ti+4 = _____________________________

Ca+2 = ________________________ Ni+2 = _____________________________

NAMING MONATOMIC ANIONS:

Nonmetal atoms gain valence electrons to form negatively charged ions called anions.

When a nonmetal forms an ion, it is named:

Element stem name + “ide” + ion

e.g. O = oxygen atom → O-2 = oxide ion N = nitrogen atom → N-3 = nitride ion

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Name each of the following monatomic anions:

F- = _________________________________ Cl- = ____________________________

Br- = ________________________________ S-2 = ____________________________

I- = _________________________________ P-3 = ____________________________

NAMING POLYATOMIC IONS:

Ions made up of more than one atom are polyatomic ions:

--only one polyatomic cation: NH4+ = ammonium ion

__many polyatomic anions: see table

NH4+ Polyatomic Ions

OH- = hydroxide ion NO2- = nitrite ion C2H3O2

- = acetate ion

CN- = cyanide ion NO3- = nitrate ion PO4

-3 = phosphate ion

CrO4-2= chromate ion SO4

-2 sulfate ion MnO4-= permanganate ion

Cr2O7-2= dichromate ion SO3

-2 = sulfate ion CO3-2 = carbonate ion

HCO3- = hydrogen carbonate ion or bicarbonate ion

Name each of the following polyatomic ions:

CN- = ____________________________ CrO4-2 = ____________________________

SO4-2 = ___________________________ NO3

- = _____________________________

OH- = ____________________________ PO4-3 = ____________________________

NH4+= ____________________________ C2H3O2

- = ___________________________

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WRITING CHEMICAL FORMULAS GIVEN INDIVIDUAL IONS

Compounds must be neutral → total + ve charge = total –ve charge

If the two ions have exactly opposite charges (+1 and -1, +2 and -2, +3 and -3)

→ formula of the compound contains one of each ion

e.g. Na+ + Cl- → NaCl K+ +NO3- → KNO3

Ca+2 + S-2 → CaS Ba+2 + SO4-2 → BaSO4

Al+3 + N-3 → AlN Fe+3 + PO4-3 → FePO4

Combine each pair of ions to get the formula of the compound they form:

NH4+ + F-→_________________________ Li+ + CN- →_________________________

Sr+2 + CO3-2 →______________________ Al+3 + PO4

-3→________________________

Na+ + C2H3O2- → ___________________ K+ + OH- → _________________________

Ni+2 + CrO4-2 → _____________________ Fe+3 + N-3 → ________________________

Cu+2 + SO4-2 → _____________________ Co+3 + P-3 → _________________________

If two monatomic ions have different charges

→ use crossover rule to get formula of the compound

superscript for cation becomes subscript for anion superscript for anion becomes subscript for cation simplify subscripts to get lowest ratio of atoms (NOTE: Only the numbers cross

down, NOT the signs!)

Na+ S2- Ba2+ N3- Ti4+ O2-

Na2S Ba3N2 Ti2O4

TiO2 (simplified)

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If two ions have different charges and at least one polyatomic ion is involved:

→ use crossover rule to get formula of the compound

--if more than one of polyatomic ion in formula, use parentheses--simplify subscripts to get lowest ration of atoms (NOTE: Again only the

numbers cross down , NOT the signs!)

NH4+ O2- Ca2+ NO3

-PB4+ CO32-

(NH4)2O Ca(NO3)2Pb2(CO3)4

Pb(CO3)2 simplified!

Combine each pair of ions to get the formula of the compound they form:

Cu+ O-2 Sn+4 SO4-2 K+ P-3

Li+ CO3-2 Fe+3 S-2 Ni+2 PO4

-3

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CHEMICAL FORMULAS AND NAMES FROM INDIVIDUAL IONS

Compounds are named from the individual ions they come from.

Name the cation and the anion, then remove “ion from each name:

e.g. Na+ = sodium ion

Cl- = chloride ion → NaCl = sodium chloride

K+ = potassium ion

CO3-2 = carbonate ion → K2CO3 = potassium carbonate

Fe+3 = iron (III) ion

NO3- = nitrate ion → Fe(NO3)3 = iron (III) nitrate

Ag+ = silver ion

S-2 = sulfide ion → Ag2S = silver sulfide

Combine each pair of ions to get the chemical formula, then name the compound:

Individual ions Compound Formula Compound Name

Mg+2 F- ________MgF2________ __magnesium fluoride

Ni+2 S-2 _____________________ __________________

Ca+2 Br- _____________________ ___________________

Al+3 P-3 _____________________ ___________________

Co+2 NO2- _____________________ ___________________

K+ CrO4-2 _____________________ ___________________

Fe+3 O-2 _____________________ ____________________

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GIVEN THE CHEMICAL FORMULA, NAME THE COMPOUND

If the metal is in Groups IA – IIIA, silver, cadmium, or zinc, then just name the metal cation and the anion:

e.g. NaCl → Na = sodium and Cl = chloride → sodium chloride

BaI2 → Ba = barium and I = iodide → barium iodide

Al(OH)3 → Al = aluminum and OH = hydroxide → aluminum hydroxide

ZnSO4 → Zn = zinc and SO4 = sulfate → zinc sulfate

If the metal can form more than one ion

a. Determine the charge on the cation using the charge on the anion.

b. Name the cation and the anion, then remove “ion” from both.

e.g. NiBr2 → since the ion formed is Br-, then 2 Br’s have an overall negative charge of -2. to get an overall charge of zero for the compound, the overall positive charge must be +2. Thus, Ni must have a charge of +2, so the ion nickel forms is Ni+2.

→ Ni+2 = nickel (II) ion Br- = bromide ion

→ NiBr2 = nickel (II) bromide

c. If a polyatomic ion is involved, remember that more than one polyatomic is shown in parentheses—i.e. DO NOT multiply the charge of the polyatomic ion with the subscript of the atoms in a polyatomic ion.

CuSO4 → There is only ONE Cu and ONE SO4, so get the charge for the Cu based on the SO4. The formula is SO4

-2, and there is only ONE SO4-2, so Cu’s

charge here must be +2 for the compound to have an overall charge of zero.

→ Cu+2 = copper (II) ion SO4-2 = sulfate ion

Then → CuSO4 = copper (II) sulfate

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Give the name for each compound given its chemical formula:

Formula Individual Ions Name of Compound

MgCl2 Mg+2 Cl-

LiOH

ZnCO3

K2S

FePO4

SnO2

CuBr2

Ag3N

Mn(CN)2

AgC2H3O2

WRITING CHEMICAL FORMULAS GIVEN THE COMPOUND NAME

Get the individual ions from the name, then combine them using the crossover rule:

e.g. barium chloride → barium = Ba+2 chloride = Cl-

Ba+2 Cl- → BaCl2

Aluminum sulfate → aluminum = Al+3 sulfate = SO4-2

Al+3 SO4-2 → Al2(SO4)3

Give the chemical formula for each compound given its name:

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Name of Compound Individual Ions Formula

Lithium cyanide Li+ CN- LiCN

Iron (III) sulfate

Calcium iodide

Tin (IV) dichromate

Silver nitrite

Copper (II) acetate

Zinc carbonate

Lead (II) phosphide

Potassium sulfite

Cobalt (II) nitride

Nickel (II) permanganate

NAMING MOLECULAR COMPOUNDS

Indicate number of atoms of each element with Greek prefix before element name:

# of atoms Greek Prefix # of atoms Greek Prefix

1 mono (usually omitted) 6 hexa

2 di 7 hepta

3 tri 8 octa

4 tetra 9 nona

5 penta 10 deca

For the first element: Greek prefix + element name

For the second element: Greek prefix + element name stem + “—ide”

Note: Mono is generally omitted, except in common names like

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CO = carbon monoxide

P2O5 SF6

diphosphorus pentaoxide sulfur hexafluoride

Name the following molecular compounds:

SO3 = ______________________________ SiBr4 = ____________________________

XeF6 = _____________________________ ClF3 = _____________________________

N2O4 = _____________________________ Cl2O7 = ___________________________

PCl5 = ______________________________ P4O10 = ___________________________

DETERMINING FORMULAS OF MOLECULAR COMPOUNDS

Use Greek prefix(es) to determine number of atoms of each element in formula

Get elements and number of atoms of each from the name:

tetraphosphorus hexasulfide

P4S6

Give the formula for each of the following molecular compounds

nitrogen trichloride dibromine heptaoxide dinitrogen pentasulfide

PUTTING IT ALL TOGETHER:

Name each of the following compounds:

BaCl2 ____________________________ NiBr2 ________________________

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HNO3 (aq) ________________________ SO2 _________________________

AgF _____________________________ PbS2 ________________________

CuSO3 ___________________________ PF5 _________________________

K2SO4 ___________________________ Cr(C2H3O2)3 _________________

FeP ______________________________ Al2(CO3)3 ___________________

NiSO4 ___________________________ ZN(OH)2 _____________________

KMnO4 __________________________ Sn(CN)2 ______________________

WRITING BINARY FORMULASWrite the formulas for he compounds formed from the following ions.

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1. Na+, Cl- ____________________

2. Ba+2, F- ____________________

3. K+, S-2 ____________________

4. Li+, Br- ____________________

5. Al+3, I- ____________________

6. Zn+2, S-2 __________________

7. Ag+, O-2 __________________

8. Mg+2, P-3___________________

9. Ni+2, O-2___________________

10. Ni+3, O-2___________________

11. Fe+2, O-2 ___________________

12. Fe+3, O-2 __________________

13. Cr+2, S-2 ___________________

14. Cr+3, S-2 ___________________

15. Cu+, Cl- ___________________

16. Cu+2, Cl- ___________________

17. Pb+2, O-2 __________________

18. Pb+4, O-2 __________________

19. Mn+2, Br- __________________

20. Mn+4, Br- __________________

NAMING BINARY COMPOUNDS (IONIC)1. BaCl2 __________________________________________________

2. NaF ___________________________________________________

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3. Ag2O __________________________________________________

4. CuB ___________________________________________________

5. CuBr2__________________________________________________

6. FeO ___________________________________________________

7. Fe2O3 __________________________________________________

8. MgS ___________________________________________________

9. Al2O3___________________________________________________

10. CaI2 ____________________________________________________

11. K2S _____________________________________________________

12. CrCl2____________________________________________________

13. CrCl3 ____________________________________________________

14. CaO _____________________________________________________

15. Ba3P2 ____________________________________________________

16. Hg2I2 ____________________________________________________

17. Na2O ____________________________________________________

18. BeS _____________________________________________________

19. MnO ____________________________________________________

20. Mn2O3 ___________________________________________________

NAMING BINARY COMPOUNDS (COVALENT)Name the following compound using the prefix method.

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1. CO ____________________________________________________________

2. CO2 __________________________________________________________________________________________

3. SO2 __________________________________________________________________________________________

4. NO2 __________________________________________________________________________________________

5. N2O ____________________________________________________________

6. SO3 __________________________________________________________________________________________

7. CCl4 __________________________________________________________________________________________

8. NO ____________________________________________________________

9. N2O5 __________________________________________________________________________________________

10. P2O5 __________________________________________________________________________________________

11. N2O4 __________________________________________________________________________________________

12. CS2 __________________________________________________________________________________________

13. OF2 __________________________________________________________________________________________

14. PCl3 __________________________________________________________________________________________

15. PBr5 __________________________________________________________________________________________

FORMULAS WITH POLYATOMIC IONS

Matching the horizontal and vertical axes, write the formulas of the compounds with the following combination of ions. The first one is done for you.

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OH- NO3- CO3

-2 SO4-2 PO4

-3

H+ HOH(H2O)

HNO3 H3CO3 H2SO4 H3PO4

Na+

Mg+2

NH4+

Ca+2

K+

Al+3

Pb+4

NAMING COMPOUNDS (MIXED)Name the following compounds.

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1. NaCl ___________________________________________________________

2. MnS ___________________________________________________________

3. K2O ___________________________________________________________

4. CuBr2 ________________________________________________________________________________________

5. CuBr ___________________________________________________________

6. CO2 ________________________________________________________________________________________

7. PbSO4 ________________________________________________________________________________________

8. Li2CO3 ________________________________________________________________________________________

9. Na2CO3 __________________________________________________________

10. NO2 ________________________________________________________________________________________

11. N2O4 ________________________________________________________________________________________

12. Ca(OH)2 ______________________________________________________________________________________

13. NH4Cl ___________________________________________________________

14. SO3 ________________________________________________________________________________________

15. AlPO4 ________________________________________________________________________________________

16. CCl4 ________________________________________________________________________________________

17. CaS ___________________________________________________________

18. NH3 ________________________________________________________________________________________

19. MgI2 ________________________________________________________________________________________

20. K3PO4 ________________________________________________________________________________________

WRITING FORMULAS FROM NAMES

Write the formulas for the following compounds.

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1. carbon monoxide ________________________________________________

2. sodium chloride ________________________________________________

3. carbon tetrachloride ________________________________________________

4. magnesium bromide ________________________________________________

5. aluminum iodide ________________________________________________

6. hydrogen hydroxide ________________________________________________

7. iron (II) fluoride ________________________________________________

8. carbon dioxide ________________________________________________

9. sodium carbonate ________________________________________________

10. ammonium sulfide ________________________________________________

11. iron (II) oxide ________________________________________________

12. iron (III) oxide

________________________________________________

13. magnesium sulfate ________________________________________________

14. sodium phosphate ________________________________________________

15. dinitrogen pentoxide ________________________________________________

16. phosphorus trichloride _______________________________________________

17. aluminum sulfite ________________________________________________

18. copper (I) carbonate ________________________________________________

19. potassium hydrogen carbonate _________________________________________

20. sulfur trioxide ________________________________________________

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Counting AtomsCalculate how many atoms of each element are present in the following compounds.

1. NaHCO3

2. C2H4O2

3. Mg(OH)2

4. 3H3PO4

5. 2H2SO4

6. (NH4)3PO4

7. C6H12O6

8. 4CaCO3

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Law of Conservation of MassRead the preceding page and answer the following questions in complete sentences.

1. State the Law of Conservation of Mass.

2. How does the Law of Conservation of Mass apply to chemical reactions?

3. How does the Law of Conservation of Mass apply to writing chemical formula?

4. How are mass and energy related?

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Balancing Chemical Equations

Read the preceding page and answer the following questions in complete sentences.

1. What is a chemical equation?

2. Name the parts of a chemical equation and explain each.

3. Compare the atoms in a reactant to the atoms in the product.

4. Why are there words or symbols above the arrow in some chemical equations?

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Name ___________________________Balancing Equations Practice

Part A: Identify the following parts of each chemical formula by circling the subscripts and drawing a square around the coefficients.

H2 2HCl 4O2 CH4

3CO3 2NaOH

Part B: List the symbols for the atoms in each formula and give the number of each.C2H6 2MgO 4P4O10

NH3 3Al(OH)3 2H2O2

Part C: Count the atoms on each side of the equation.

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P + O2 → P4O10 Mg + O2 → MgO

P = P = Mg = Mg =

O = O = O = O =

BaCl2 + H2SO4 → BaSO4 + HCl Ba = Ba =

Cl = Cl =

H = H =

S = S =

O = O =

Part D: Choose which coefficients balance the equations

_Cl2 + _NaBr → _NaCl + _Br2 __H2 + _N2 → _NH3

a. 2,2,2,1 a. 3,2,1b. 3,2,1,1 b. 3,1,2c. 1,2,2,1 c. 1,2,3d. 1,1,2,3 d. 1,1,2

_Na + _Br2 → _NaBr _CuCl2 + _H2S → _CuS + _HCl

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a. 2,1,1 a. 2,1,2,1b. 1,2,2 b. 1,1,1,2c. 1,1,2 c. 2,2,1,1d. 2,1,2 d. 1,2,1,2

_HgO + _Cl2 → __HgCl + _O2 __C + _H2 → _CH4

a. 1,2,1,2 a. 1,2,1b. 2,2,1,1 b. 2,1,2c. 2,1,2,1 c. 1,1,2d. 1,1,1,2 d. 2,2,1

Name _____________________________________ Date ___________________

Balancing Equations

Multiple Choice. Choose the correct numbers to balance out the equation. Once it is balanced count the atoms to check your answer.

1. _____Na + _____O2 → _____Na2Oa. 2, 1, 2b. 4, 1, 2c. 2, 1, 1

2. _____H2 + _____O2 → _____H2Oa. 1, 2, 1b. 2, 2, 2c. 2, 1, 2

3. _____Na2SO4 + _____CaCl2 → _____CaSO4 + _____NaCl

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a. 1, 1, 1, 2b. 2, 1, 1, 4c. 1, 2, 1, 2

4. _____Al2O3 → _____Al + _____O2

a. 1, 2, 2b. 2, 3, 4c. 2, 4, 3

5. _____N2 + _____ H2 → _____NH3

a. 1, 2, 3b. 2, 3, 1c. 1, 3, 2

6. _____Fe + _____H2O → _____Fe3O4 + _____H2

a. 3, 4, 1, 4b. 3, 4, 2, 1c. 3, 3, 1, 4

7. _____P4 + _____O2 → _____P4O10

a. 2, 3, 2b. 1, 5, 2c. 1, 5, 1

8. _____SiCl4 → _____Si + _____Cl2

a. 1, 1, 4b. 1, 1, 2c. 1, 2, 2

Balancing equations

1. 2.

_HgO + _Cl2 → __HgCl + _O2 __C + _H2 → _CH4

a. 1,2,1,2 a. 1,2,1b. 2,2,1,1 b. 2,1,2c. 2,1,2,1 c. 1,1,2d. 1,1,1,2 d. 2,2,1

3. 4.

_Na + _Br2 → _NaBr _CuCl2 + _H2S → _CuS + _HCl

a. 2,1,1 a. 2,1,2,1

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b. 1,2,2 b. 1,1,1,2c. 1,1,2 c. 2,2,1,1d. 2,1,2 d. 1,2,1,2

5. 6.

_Cl2 + _NaBr → _NaCl + _Br2 __H2 + _N2 → _NH3

a. 2,2,2,1 a. 3,2,1b. 3,2,1,1 b. 3,1,2c. 1,2,2,1 c. 1,2,3d. 1,1,2,3 d. 1,1,2

7. __Na2SO4 + __CaCl2 → __CaSO4 + __NaCl

a. 1, 1, 1, 2b. 2, 1, 1, 4c. 1, 2, 1, 2d. 2, 2, 1, 3

Balancing Equations

Balance the following chemical equations

1) ___CH4 + ____O2 → ____CO2 + ____H2O

2) ____Na + ____I → ____ NaI

3) ____N2 + ____O2 → ____N2O

4) ____ N2 + ____H2 → ____NH3

5) ____KI + ____Cl2 → ____KCl + ____I2

6) ____HCl + ____Ca(OH)2 → ____CaCl2 + ____H2O

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7) ____KClO3 → ____ KCl + ____O2

8) ____K3PO4 + ____HCl → ____KCl + ____H3PO4

9) ____S + ____O2 → ____SO3

10) ____KI + ____Pb(NO3)2 → ____KNO3 + ____PbI2

11) ____CaSO4 + ____AlBr3 → ____CaBr2 + ____Al2(SO4)3

12) _____H2O2 → ____H2O + ____O2

13) _____Na + ____H2O → ____NaOH + ____H2

14) ____C2H6 + ____O2 → ____CO2 + ____ H2O

15) _____ Mg(NO3)2 + ____K3PO4 → ____Mg3(PO4)2 + ____KNO3

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Endothermic Reactions vs. Exothermic Reactions Worksheet

Classify each of the following changes as either exothermic or endothermic. Also, determine whether each change is a chemical reaction or a physical change. Explain your reasoning for each.

1. An ice cube melts after being left out on the table over an extended period of time.

2. Cracking a raw egg into a hot frying pan and cooking it.

3. A match burns/ignites after being struck against a rough surface.

4. The human body uses the energy provided from the digestion of food.

5. Morning dew forming on grass and plants.

6. Dynamite explodes in the destruction of a building

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Name ______________________________________________

Endothermic Vs Exothermic LabBackground Information:A reaction occurs in a system with surroundings (see diagram below).

reaction occurs here

surroundings system surroundings

surroundings

Chemical and physical reactions that produce heat are exothermic processes. When an exothermic reaction occurs, heat flows from the system into the surroundings, and an increase in the temperature of the surroundings is detected. You can feel it get hot.

Chemical and physical reactions that absorb heat are called endothermic processes. When an endothermic reaction occurs, heat flows from the surroundings into the system, and a decrease in temperature of the surroundings is detected. It feels cool to the touch. In this lab, you will explore endothermic and exothermic reactions.

Hypothesis:Predict whether the following reactions will be endothermic or exothermic:

Calcium Chloride and water:

Ammonium nitrate and water:

Borax in water:

Baking Soda in vinegar:

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Safety Concerns:

Goggles must be worn at all times. Follow all lab safety procedures. Discard the solutions by filling the bags with water first to dilute the solution and then pouring them down the drain. Throw empty ziplock bags in the trash

Materials:4 Ziplock bags Calcium ChlorideBorax Baking SodaVinegar water Graduated cylinder Ammonium Nitrate

Procedure

1. Place ½ teaspoon of calcium chloride in one corner of a plastic bag. Then twist the bag at the corner where the calcium chloride is to seal it off.

2. Measure 10 mL of water in the graduated cylinder and pour it into the opposite side of the plastic bag. Be careful not to let the water come in contact with the substance.

3. Seal the plastic bag.4. Once the plastic bag is sealed untwist the corner of the bag and allow the water to

come in contact with the substance. 5. Begin mixing the water and the substance.6. Record your observations and any temperature changes.7. Repeat steps 1-6 for the ammonium nitrate and borax.8. Repeat steps 1-6 for the baking soda and vinegar but instead of water measure

10mL of vinegar.

Observations

Calcium Chloride and water:

Ammonium nitrate and water:

Borax in water:

Baking Soda in vinegar:

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Questions

1. Which reactions were endothermic? Explain how you know.

2. Which reactions were exothermic? Explain how you know.

3. Determine whether the following everyday occurrences are examples of endothermic or exothermic reactions and explain your reasoning.

a. a car engine

b. ice cream maker

c. an oven

d. ice in a glass of cold soda

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The Structure of Water

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Water as a Universal Solvent

1. What is the formula of water?

2. Draw a water molecule. Include the angle of the bonds.

3. Why is water a polar molecule?

4. Why is water an effective solvent?

5. How does table salt dissolve in water?

6. Why will a solid dissolve in one substance but not another?

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Water as a Universal Solvent Questions

1. What are some of the special properties of water?

2. What happens to density as water becomes ice?

3. What is specific heat?

4. Why is water an important solvent?

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Polarity of MoleculesDetermine whether the following molecules are polar or non-polar

1. N2

2. H2O

3. CO2

4. NH3

5. CH4

6. SO3

7. HF

8. CH3OH

9. H2S

10. I2

11. CHCl3

12. O2

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Solubility (Polar vs. Nonpolar)

Generally, “like dissolves like”. Polar molecules dissolve other polar molecules and ionic compounds. Nonpolar molecules dissolve other nonpolar molecules. Alcohols, which have characteristics of both, tend to dissolve in both types of solvents, but will not dissolve ionic solids.

Check the appropriate columns as to whether the solute is soluble in a polar or nonpolar solvent.

SolutesSolvents

Water CCl4 Alcohol

1. NaCl

2. I2

3. ethanol

4. benzene

5. Br2

6. KNO3

7. toluene

8. Ca(OH)2

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Name ____________________________

Polar vs. Non-Polar

Purpose: To determine the relationship between polar and non-polar solutes and their

ability to dissolve in polar and non-polar solvents.

Safety Equipment: These chemicals are dangerous and you need to be careful. You

MUST wear goggles at all times. You also need an apron and gloves.

Procedure:

1. Add about 20 mL of water to each of the 2 beakers.

2. Add a small amount of sodium chloride (salt) to only 1 beaker with water. Attempt to

dissolve this mixture using a popsicle stick. Record your observations as part of your

data table.

3. Add a small amount of paradichlorobenzene (C6H4Cl2– non-polar) to the other

beaker with water. Attempt to dissolve this mixture using a popsicle stick. Record

your observations as part of your data table.

4. When finished, pour both solutions down the drain. Wash all glassware..

5. In the 2 beakers, add about 20 mL of acetone (C3H6O – non-polar) to each beaker).

6. Add a small amount of sodium chloride to only 1 beaker with acetone. Attempt to

dissolve this mixture using a popsicle stick. Record your observations as part of your

data table.

7. Add a small amount of paradichlorobenzene (C6H4Cl2– non-polar) to the other

beaker with acetone. Attempt to dissolve this mixture using a glass stirring rod.

Record your observations as part of your data table.

8. When finished, pour both solutions down the drain. Wash all glassware.

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Observations/Data Tables: (Label all parts!)

1. Observation of sodium chloride and water mixture:

2. Observation of paradichlorobenzene and water mixture:

3. Observation of sodium chloride and acetone mixture:

4. Observation of paradichlorobenzene and acetone mixture:

Processing The Data:

1. Are water molecules polar or non-polar? Explain.

2. In terms of polarity (polar vs. non-polar), explain why some of the mixtures in Part A

dissolved and some mixtures did not dissolve (all 4 observations need to be

explained!).

3. What is the “common name” or the “common product” that usually contains acetone?

4. What is the “common name” or the “common product” for paradichlorobenzene ?

Conclusion: Write a conclusion statement based on the lab and its results.

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Chromatography LabIntroduction:

The inventor of modern chromatography was a Russian botanist, Mikail Tsvet, who wanted to analyze leaf pigments. In 1903, he devised a column for separation the component compounds. His discovery was ignored for the next 30 years. Eventually Tsvet’s invention made possible the identification of chlorophylls, vitamins, and many other substances, and led to advances in the understanding of biochemical processes.

Background:

Chemists often need to separate the components of a solution to identify them. One of the most powerful techniques available for this purpose is chromatography. It is based on the fact that substances differ in their affinities for solvents and other media.

Paper chromatography is relatively easy procedure to perform in the laboratory. It can be used to separate a mixture of colored substances. A small drop of the sample mixture is placed near the bottom edge of a piece of filter paper and is allowed to dry. The filter paper is placed in a shallow container so that the bottom edge just touches the chosen solvent. Capillary action causes the solvent to travel up the filter paper. Substances with little affinity for the paper migrate up the strip almost as fast as the solvent. Components with greater affinity for the paper migrate at slower rates. The further the solvent migrates, the more the component substance of the sample mixture becomes separated. By changing the solvent, the degree of migration and separation can be varied.

Several other types of chromatography are also available. In some of these systems the liquid solvent, also called the mobile phase, is replaced by a gas solvent. The filter paper, the stationary phase, can be substituted by a liquid, a colloid, or more appropriate type of solid. The type of chromatographic system used depends on the substance that must be separated.

Commercial laboratories and research facilities make great use of chromatography. For example, the food industry uses a gas chromatograph to isolate and identify compounds responsible for food aromas. This is the first step in the process of producing flavorings that imitate natural flavors. Chromatography is used in many areas of chemical, medical, and biological research.

Problem: How can chromatography be use to determine solvent and solutes?

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Pre Lab Questions

1. Who is the father of modern chromatograph?

2. What is chromatography?

3. Explain what type of change is involved with chromatography.

Materials: Black colored ink RulerFilter paper Graduated cylinderBeaker Water3 straws OilClip or tape Isopropyl

Procedure:

1. Cut 3 strips of filter paper 9.5 cm in length

2. Place 7 mL of water in the 1st beaker

3. Place 7 mL of isopropyl alcohol into the 2nd beaker

4. Place 7 mL of oil into the 3rd beaker

5. Tape the strips of filter paper to the center of the straws

6. Place a black dot near the bottom of the strip

7. Place one strip in each beaker and rest the straw across the top. Roll the strip so that just the bottom edge is in the liquid

8. Observe the strip. Measure the length of solvent absorption on the filter paper every minute for 5 minutes. Record in a data table.

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Data: Data table to record results

Time Length of Absorption(solvent)

Colors Color Length

Post lab Questions

1. How far did the ink spread in each solvent?

2. Does the blue dye have a structure more like the paper or the solvent? Explain

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3. How would the results differ if the inks were made from a lighter single dye instead of black dye?

4. Which solvents separated the inks the most?

5. Did any of the solvents not separate the inks? Why not? Explain

6. What factors of the solvent affected the separation of inks?

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1. What is the concentration of a solution?

2. What is a saturated solution?

3. What is a supersaturated solution?

4. Explain how a substance is diluted?

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Colloid LabBackground:

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Any substance—solid, liquid, or gas—that is evenly dispersed or distribute throughout another substance—solid, liquid, or gas—is a solution. Solutions are often called homogeneous mixtures because they are not pure substances, yet the substances that comprise them are evenly dispersed throughout the mixture. The brass faucet is a solid solution made of copper and zinc atoms that are dissolved in various proportions.

Within a solution the substance that is the dissolving medium is known as the solvent. The solute is the substance dissolved in the solvent. Some liquids are so soluble in each other, like alcohol and water, that as you add more and more water to alcohol, the concentration of the water exceeds the concentration of the alcohol. The water is then said to be the solvent, and the alcohol becomes the solute. Because the same substance can be referred to as a solute in one instance and a solvent in another, the terms solute and solvent should not be thought of as absolutes.

Colloids are homogeneous solutions. The particles are evenly mixed and do not settle out.

Problem: How does temperature affect particle separation?

Pre Lab Questions

1. What is a solution?

2. What is the relationship between a solute and solvent?

3. Describe a colloid.

II. Procedure

1) Dissolve 2 tablespoons of sugar in 1/2 cup of milk, then add 3-5 drops of vanilla or other extract for flavor.2) Pour milk mixture in a zip-close sandwich bag and close securely.

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Half fill a 1 gallon zip-close freezer bag with ice cubes, then add about 2 tablespoons of rock salt. Place the sandwich bag into the freezer bag and securely close the freezer bag. Gently massage the bags together to keep the inner bag mixing without heating it with your hands (you do NOT want the inner bag to open).

After 25 minutes or so, the ice cream should be ready to scoop into a cup and enjoy.

Post Lab

1. What was the solute and solvent in this experiment?

2. What factors allowed the mixture to form ice cream?

3. Explain what a colloid is using the ice cream as an example.

4. Evaluate your ice cream making by writing a paragraph about the process.

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1. What is solubility?

2. Why must you state the temperature when you talk about solubility?

3. What is the solubility of sodium chloride at 60 C? Potassium bromide at 40 C? Sodium nitrate at 0 C?

4. What happens to solubility as temperature increases?

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Temperature Questions

1. How does temperature affect solubility?

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2. On the solubility graphs, what does the x-axis represent? The y-axis?

3. What happens to the solubility of a gas as the temperature of the solvent raises?

4. What does it mean when the gas solubility graph shows a negative slope?

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Name: ______________________ Solubility Graphs

Solubility measures the amount of a material (solute) that will dissolve in a solvent at a given temperature. Often the solvent will be water. As you would expect, different materials dissolve at different rates. Use the solubility graph provided to answer the following questions.

1) Is solubility a physical or chemical property?

2) According to the graph. as the temperature increases, what happens to the amount of solute being dissolved in water?

3) The slope of a graph indicates how rapidly the solute dissolves as the temperature increases - the steeper the slope the more rapidly it dissolves. According to the graph, what substance dissolves the fastest between 0°C and 50°C based on the slope of the curve?

4) What substance changes the least in solubility across the entire temperature range?

5) How many grams of potassium iodide will dissolve at 30°C? ________

6) At what temperature will 20 grams of potassium chlorate dissolve in water? ________

7) How many grams of sodium nitrate will dissolve at 90°C? ________

8) At approximately what temperature will 85 grams of potassium nitrate dissolve in water? ________

9) What substance dissolves best at the freezing point of water (0°C ) ? _________________________

10) Based on your knowledge of how heat energy affects particle spacing and movement, why would more material (solute) dissolve in water (solvent) at higher temperatures?

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1. How can the rate of dissolving be increased?

2. What is diffusion?

3. How does increasing temperature affect solubility of a substance?

4. Explain why the dissolving rate and solubility is unrelated.

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1. What is a conductivity device?

2. What is electrolyte?

3. How do electrolytes affect acids and bases?

4. Why can tap water easily carry an electric current and pure water cannot?

5. How do solutes change properties of solvents?

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Acid and Base Questions

1. What are acids?

2. Give two characteristics of acids.

3. What is an indicator?

4. Compare a strong acid to a weak acid.

5. What is a base?

6. What type of ions do bases form?

7. Give two characteristics of bases.

8. Compare a strong base to a weak base.

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ACID, BASE, OR SALTClassify each of the following compounds as an acid, base or salt. Then, indicate whether each acid and base is strong or weak.

1. HNO3 _______________________ ______________________

2. NaOH _______________________ ______________________

3. NaNO3 ___________________________________ _________________________________

4. HCl _______________________ ______________________

5. KCl _______________________ ______________________

6. Ba(OH)2 __________________________________ _________________________________

7. KOH _______________________ ______________________

8. H2S _______________________ ______________________

9. Al(NO3)3 __________________________________ _________________________________

10. H2SO4 ___________________________________ _________________________________

11. CaCl2 ___________________________________ _________________________________

12. H3PO4 ___________________________________ _________________________________

13. Na2SO4 ___________________________________ _________________________________

14. Mg(OH)2 ___________________________________ _________________________________

15. H2CO3 ___________________________________ _________________________________

16. NH4OH _______________________ ______________________

17. NH4Cl _______________________ ______________________

18. HBR _______________________ ______________________

19. FeBr3 __________________________________ _________________________________

20. HF _______________________ ______________________

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The pH Scale

1. What is litmus paper used for?

2. What is a pH scale used for?

3. What scale is used for the pH scale?

4. What is the range of acids? Bases? Neutral?

5. What is a neutralization reaction?

6. Compare the substances at either end of the scale to those in the center of the scale.

7. What is the very IMPORTANT laboratory rule about acids? Why do labs have this rule?

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pH

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Indicators and SolutionsBackground:

Indicators can be used to identify an acid from a base by a color change. The color change is due to the changing proportion of the indicator molecules in the acid or base. This changing of proportions occurs over various pH values.

A scale of acidity has been set up to rank substances. A measure of the acidity of a substance is known as ph. The ph scale is form 0 to 14. Substance with a pH value of 7 is neither acidic nor basic. It can be called neutral. Substances with pH values less than 7 are acidic. Substance with pH values greater than 7 is basic. The lower the pH value, the more acidic the substance is. The higher the pH value, the more basic the substance is.

Problem: Which household substances are acids, which are bases, and which are neither?

Pre Lab Questions:

1. What is an indicator used for?

2. What causes the color change in an indicator?

3. Draw a pH scale.

Materials: Various household substances pH chartTray pH paperPipettes Red LitmusBlue litmus

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Procedure:

1. Place 4 drops of sample 1 in cup 1 of tray.

2. Place 4 drops of sample 2 in cup 2 of tray.

3. Place 4 drops of sample 3 in cup 3 of tray.

4. Place 4 drops of sample 4 in cup 4 of tray.

5. Place 4 drops of sample 5 in cup 5 of tray.

6. Place 4 drops of sample 6 in cup 6 of tray.

7. Place 4 drops of sample 7 in cup 7 of tray.

8. Place 4 drops of sample 8 in cup 8 of tray.

9. Place 4 drops of sample 9 in cup 9 of tray.

10. Determine which substances are acids by dripping a small piece of blue litmus in each cup. Record the results.

11. Determine which substances are bases by dipping a small piece of red litmus in each cup. Record the results.

12. Determine the pH of each substance by dipping a small piece of pH paper in each cup. Compare the color change to pH chart and record results.

13. After all testing has been completed, trash pH and litmus papers. Clean tray by wiping out substances..

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Data:

Sample

Name of Substance Blue Litmus

Red Litmus

pH paper

1

2

3

4

5

6

7

8

9

Post Lab

1. Which samples are acids? Which samples are bases? Which samples are neither?

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2. How did you determine which substances were acids?

3. How did you determine which substances were bases?

4. Identify the acids, bases, and neutrals?

5. Why is it important to know the ph of a household substance?

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What does an Antacid do?

Materials: Vinegar 2 BeakersAntacid Tablets StirrerWater Litmus, blue:

Procedure:

1. Pour 100 mL of water into beaker.

2. Add vinegar one drop at a time while stirring with the stirrer.

3. Test the solution with litmus paper after each drop is added. Record the number of drops it takes for the solution to turn blue litmus paper bright red.

4. Crush an antacid tablet.

5. Pour 100 mL of water into the second beaker and add crushed antacid tablet. Stir solution until powder dissolves completely.

6. Use litmus paper to find out whether the solution is acidic, basic, or neutral. Record your results.

7. Now add vinegar one drop at a time to the antacid solution. Record the number of drops it takes the blue litmus paper to turn bright red.

8. Compare this solution with the solution that has only vinegar and water. Record observations.

Data Table

Create a data table to record the number of drops and color change

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Analysis

1. How does an antacid work to relieve the pain caused by excess stomach acid?

2. How many drops of vinegar were needed to turn the litmus red?

3. How did the antacid solution compare with the vinegar solution?

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Acids and BasesIdentify each item listed below as to whether it refers to an acid, a base, or both an acid and a base. Use the letters in the key.

KEY: A = acid B = base AB = acid and base

_____ 1. sour taste _____ 12. is used in pickling

_____ 2. bitter taste _____ 13. forms through ionization

_____ 3. produces hydrogen ions in _____ 14. forms through dissociation solution

_____ 4. is an electrolyte _____ 15. Compounds that produce this in solution are made up of polar molecules.

_____ 5. is slippery _____ 16. produces hydronium ions

_____ 6. is often corrosive _____ 17. most compounds that produce this in solution are made up of polar molecules

______ 7 exists as a crystalline solid in _____ 18. exists in aqueous solution an undissolved state

______ 8. produces hydroxide ions in _____ 19. HCl is an example solution

______ 9. can be detected with an indicator ______ 20. ammonia is a common example

______10. soaps are an example ______ 21. conducts electricity

______11 may be used to make fertilizer

Complete the following. Write you answers on the lines provided.

21. Use the information above to identify four properties that acids and bases have in common

22. Identify three characteristics of acids that are NOT true of bases.

24. Identify three characteristics of bases that acids do not have.

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