Chemistry Water B Reading Name_______________________________

Read pages 25-30.

1. Did preliminary water sample analysis show a likely cause for the fish kills?

2. What does DO stand for? How is this related to fish kills?

3. What are 2 factors EPA chemists will have to consider when examining the possibility that a dissolved substance may be responsible for the fish kill?

4. Was any illness reported from drinking water in Riverwood?

5. Define “physical properties”.

6. One ______________ of water at 25°C has a mass of one ________________.

7. One __________________ of volume = ____________________ (See figure 1.20)

8. What is the freezing point of water?

9. Why is water that seems pure never really entirely so?

10. What is an aqueous solution?

11. Pure water is clear, __________________________, __________________________, and ______________________________.

12. Please answer the questions B.2 on page 28 here:1.

2.

3.

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13. Which state of matter (solid, liquid, or gas) is usually the densest form of a substance? (Note! water is an exception to this!)

14. Define “mixture”.

15. A solution is a ____________________________ mixture in which the particles are so small they cannot be seen even with magnification.

16. Define “solute”.

17. Define “solvent”.

18. Describe a suspension:

19. Describe a colloid:

20. Why is milk a colloid?

21. What is the Tyndall effect?

22. If the Tyndall effect is apparent, the mixture is a ____________________________.

If you cannot see the Tyndall effect, the mixture is a ___________________________.Note: study the chart on page 30!!

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Water Part BWater Part BPhysical properties of water

______________molecules dissolve many substances Clear, colorless, odorless, tasteless Boiling point = ______________ Melting/freezing point = ___________ Density = ________________ Density of liquid water _____density of ice High _________________ _______________

Most solids sink in their liquids!Most solids sink in their liquids!

Defining matter according to makeupDefining matter according to makeup HomogeneousHomogeneous - ____________________properties throughout- ____________________properties throughout Heterogeneous- Heterogeneous- has parts with ___________________propertieshas parts with ___________________properties Appearance alone cannot always distinguish heterogeneous matter from homogeneous.Appearance alone cannot always distinguish heterogeneous matter from homogeneous.

Heterogeneous MatterHeterogeneous Matter Made of more than one type of substance.Made of more than one type of substance. Easily separated by Easily separated by ______________________________________________such as evaporation, magnetic separation, orsuch as evaporation, magnetic separation, or

picking pieces apart.picking pieces apart.

What is a mixture?What is a mixture? 2 or more substances, 2 or more substances, ______________________________________combinedcombined Mixtures may be __________________or _________________________Mixtures may be __________________or _________________________ Homogenous mixtures are called ___________________Homogenous mixtures are called ___________________

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Air is a _________________Air is a _________________ It is a homogenous mixture of nitrogen, oxygen, carbon dioxide and other gases.It is a homogenous mixture of nitrogen, oxygen, carbon dioxide and other gases.

Homogeneous matterHomogeneous matter Homogeneous matter may be ________________or________________.Homogeneous matter may be ________________or________________. Pure substances ____________________be separated by physical means. A Pure substances ____________________be separated by physical means. A ____________________ ____________________must occur to separate the parts.____________________ ____________________must occur to separate the parts. Pure substances are ________________if they are separable by chemical means. They Pure substances are ________________if they are separable by chemical means. They are _________________if they can not be further broken down.are _________________if they can not be further broken down.

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Salt water-Homogeneous mixture,Solution

How do we knowthis is a mixture?

It can be separatedby physical means:evaporation.

Other examples of solutionsOther examples of solutions

Rootbeer is a solution of water, sugar, carbon dioxide, and other flavorings

Brass is a solution of Copper and zinc

Water is a pure substanceWater is a pure substance Water (HWater (H22O) can be broken into ____________________and O) can be broken into ____________________and ________________________by electrolysis. It cannot be separated into hydrogen and oxygen ________________________by electrolysis. It cannot be separated into hydrogen and oxygen by any physical method.by any physical method.

Hydrogen gas is a pure substanceHydrogen gas is a pure substance Hydrogen may be a ________________(HHydrogen may be a ________________(H22) or an _____________________(H). ) or an _____________________(H). Hydrogen gas as it normally exists is the compound HHydrogen gas as it normally exists is the compound H22 . .

Classifying matter according to make-upClassifying matter according to make-upPure Substances Pure Substances Mixtures Mixtures Compounds Compounds Homogeneous Homogeneous HeterogeneousHeterogeneous

Elements Elements SolutionsSolutions Suspension Suspension or Colloids or Colloids

What type of matter?What type of matter?

Classifying mixtures by particle sizeClassifying mixtures by particle size _________________: particles too small to see or separate out. No Tyndall effect._________________: particles too small to see or separate out. No Tyndall effect.

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_________________: Tiny particles produce a cloudy appearance. Shows Tyndall effect_________________: Tiny particles produce a cloudy appearance. Shows Tyndall effect _________________: Big particles you can see and that will settle out. _________________: Big particles you can see and that will settle out.

SolutionsSolutions ________________________mixtures________________________mixtures Have different parts which are uniformly distributed and are too small to distinguish with Have different parts which are uniformly distributed and are too small to distinguish with the eye.the eye. Examples:____________________________________Examples:____________________________________ Solid solutions are called________________; they are a mixture of metalsSolid solutions are called________________; they are a mixture of metals Examples: ________________________________________Examples: ________________________________________

Made of 2 parts- solute and solventMade of 2 parts- solute and solvent ____________________dissolve in things____________________dissolve in things _____________________do the dissolving_____________________do the dissolving

ColloidsColloids Can’t see the particlesCan’t see the particles Foggy or _________________appearanceFoggy or _________________appearance Show Tyndall effectShow Tyndall effect

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Particles too small to see, evenly distributed,cloudy appearance

SuspensionsSuspensions Particles _____________enough to see and settle outParticles _____________enough to see and settle out

Many medicines are suspensionsMany medicines are suspensions

Particles big enough to seethat maysettle out

Rivers have particles suspended in their water

Colloid, suspension, or solution?Colloid, suspension, or solution?

7

8

CLASSIFYING MATTER FLOWCHART

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Water B-2Water B-2Atoms and molecules, Polar molecules, Ions and ChemicalAtoms and molecules, Polar molecules, Ions and Chemical

formulasformulasLet’s review the molecule!Let’s review the molecule!

2 or more atoms ______________ __________together make a molecule.2 or more atoms ______________ __________together make a molecule.

Let’s review the molecule!Let’s review the molecule!The water molecule consists of ________ hydrogen atoms, and __________oxygen atom.Its formula is _________________

The ethane molecule consists of ________carbon atoms and __________ hydrogenatoms. Its formula is ______________________

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Let’s review molecular formulas:Let’s review molecular formulas: How many atoms of each element are in the following molecules?How many atoms of each element are in the following molecules?

1. H1. H22SOSO4 4 ____________________________________________________________________2. Ca(OH)2. Ca(OH)2 2 ____________________________________________________________________3. NaCl __________________________________3. NaCl __________________________________4. (NH4. (NH33))33P0P04 4 ____________________________________________________________________5. 3 H5. 3 H22O (this means 3 water molecules) O (this means 3 water molecules)

____________________________________________________________________6. 4 Al6. 4 Al22(CO(CO33))3 3 (4 aluminum carbonate molecules) (4 aluminum carbonate molecules)

____________________________________________________________________

Do an atom inventory for this equation:Do an atom inventory for this equation: NaOH + HCl NaOH + HCl NaCl + H NaCl + H22OO

Interpret this equation in terms of moleculesInterpret this equation in terms of molecules (Tell in words what is happening in this reaction)(Tell in words what is happening in this reaction) 2H2H22 + O + O22 2H 2H22OO

______________________________________________________________________________________________________________________________

Do an atom inventory:Do an atom inventory: 2H2H22 + O + O22 2H 2H22OO

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Interpret this equation in terms of moleculesInterpret this equation in terms of molecules3N3N2 2 + H+ H22 2 NH 2 NH33

____________________________________________________________________________________________________________________________________________________________

Interpret this equation in terms of molecules: Interpret this equation in terms of molecules:

Do an atom inventoryDo an atom inventory

Please read pages 34-36 in your text and do the exercises B.7 #1-3 on pages 36-37 here, then also answer questions 4 - 6 on the next page:

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4. What are diatomic molecules?

5. List the elements that exist as diatomic molecules.

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6. Look up these elements on your periodic table. Trace the positions of all except hydrogen. What shape do they make ( if you don’t include hydrogen)?

It will be easy to remember them, because there are 7 elements and they make the number 7 on the periodic table (plus you have to remember hydrogen!)

Or, you can just remember the magic word…

HNOFClBrI

Ions and chemical formulasIons and chemical formulasLet’s review the atom:Let’s review the atom:

The atom has 3 subatomic particlesThe atom has 3 subatomic particles _________-in the nucleus, + charge _________-in the nucleus, + charge _________- in the nucleus, neutral _________- in the nucleus, neutral __________- outside the nucleus, - charge (moving!)__________- outside the nucleus, - charge (moving!)

IONSIONS Elements that have gained or lost an electronElements that have gained or lost an electron Cations are positiveCations are positive They have lost an electronThey have lost an electron Anions are negativeAnions are negative They have gained an electronThey have gained an electron

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When the two combine, you get sodium chloride-When the two combine, you get sodium chloride-everybody’s happy!everybody’s happy!

Ionic bondsIonic bonds NaNa++ ClCl-- Makes the ionic compound ________________Makes the ionic compound ________________

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Is this sodium ion a cation or an anion?

Chlorine gains an electron when it ionizes. Is it a cation or an anion?

Question:Question: Calcium prefers to lose 2 electrons. What kind of ion Calcium prefers to lose 2 electrons. What kind of ion would calcium be?would calcium be? ____________, a ________________________________, a ____________________

Question:Question: Fluorine would like an extra electron. What kind of ion Fluorine would like an extra electron. What kind of ion will it become?will it become? ____________, a fluoride _______________________________, a fluoride ___________________

Question:Question: What compound is made from calcium and fluoride What compound is made from calcium and fluoride ions?ions? Calcium fluoride, _______________Calcium fluoride, _______________ Question: Why are 2 F’s needed for one Ca?Question: Why are 2 F’s needed for one Ca? FF-- CaCa2+2+ FF- - The charges need to______________________!The charges need to______________________!

Atoms prefer a full outer shell of electrons!Atoms prefer a full outer shell of electrons!

Draw some atoms and ions!Draw some atoms and ions! Draw some atoms as Neils Bohr represented them. Then you Draw some atoms as Neils Bohr represented them. Then you will draw some ions as you see if atoms prefer to gain or lose will draw some ions as you see if atoms prefer to gain or lose electrons to fill their outer shell.electrons to fill their outer shell.

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Names and formulas of ionic compounds

Molecular- ______________bonds, electrons are Molecular- ______________bonds, electrons are __________________________ Ionic- ionic bonds, electrons are _________________Ionic- ionic bonds, electrons are _________________

Covalent or ionic?Covalent or ionic? Ionic bonds form between a _________and a ________________Ionic bonds form between a _________and a ________________

Covalent bonds form between 2 ______________or a nonmetal Covalent bonds form between 2 ______________or a nonmetal and ____________and ____________

Covalent or ionic?Covalent or ionic? Na and ClNa and Cl ________________________________ C and HC and H

_______________________________

C and SC and S_____________________________________

N and NN and N________________________________________

Ca and SCa and S___________________________________________

Fe and ClFe and Cl____________________________________________

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Naming ionic compoundsNaming ionic compounds The first name is the name of the _______________The first name is the name of the _______________

–– Example: CaClExample: CaCl22 has first name ______________ has first name ______________

The last name has the name of the____________. Anion names The last name has the name of the____________. Anion names always end in “__________” unless they are from your polyatomic ion always end in “__________” unless they are from your polyatomic ion chart.chart.

–– Example: CaClExample: CaCl22 has last name chloride, has last name chloride, so is CaClso is CaCl22 __________________ ____________ __________________ ____________

Name these ionic compoundsName these ionic compounds 1. BaF1. BaF22__________________________________________________________________ 2. K2. K22Se_________________________________Se_________________________________ 3. CaS__________________________________3. CaS__________________________________ 4. AlF4. AlF33__________________________________________________________________ 5. LiH5. LiH____________________________________________________________________

1) MgS ___________________________ 2) KBr ____________________________ 3) Ba3N2 ___________________________ 4) Al2O3 ___________________________ 5) NaI ____________________________ 6) SrF2 _____________________________

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Naming ionic compounds-moreNaming ionic compounds-more Some compounds need __________ _______________________to Some compounds need __________ _______________________to distinguish between possible first names.distinguish between possible first names. For example, a compound of iron and chloride may be iron (II) For example, a compound of iron and chloride may be iron (II) chloride or iron (III) chloride.chloride or iron (III) chloride. The roman numeral is equal to the ___________on the ionThe roman numeral is equal to the ___________on the ion

Name these ionic compounds using roman numerals:Name these ionic compounds using roman numerals: 1. A compound of Mn1. A compound of Mn3+3+ and Cl and Cl--

________________________________________________________________ 2. NiN2. NiN__________________________________________________________________

3. SnO3. SnO____________________________________________ 4. SnO4. SnO22

______________________________________________________________

5. PbO5. PbO__________________________________________________________________

CrCl3

______________________________________CoO______________________________________Mn2O3

______________________________________Co2S3

______________________________________AuF______________________________________CrBr2 ___________________________________________________

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Which elements need roman numerals in theirWhich elements need roman numerals in their names?names?

Any elements listed as _________________metalsAny elements listed as _________________metals All ________________________metals except zinc, cadmium, and All ________________________metals except zinc, cadmium, and silver.silver.–– Zinc and cadmium always form _________ions, silver always forms a Zinc and cadmium always form _________ions, silver always forms a ___________ion.___________ion.

Naming ionic compounds that contain more than 2Naming ionic compounds that contain more than 2 elementselements

Compounds containing polyatomic ions are named by Compounds containing polyatomic ions are named by using your _____________ __________chart.using your _____________ __________chart.

Name these ionic compounds that contain polyatomicName these ionic compounds that contain polyatomic ions:ions:

1. NH1. NH44ClCl

____________________________________________________________________

2. NH2. NH44OHOH

–– ____________________________________________________________________

3. (NH3. (NH44 ) )33POPO33_____________________________________________________________

4. AlPO4. AlPO44

–– ________________________________________________________________

5. Fe(NO5. Fe(NO22) ) 22__________________________________________________________________

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Mixed practice naming ionic compounds!Mixed practice naming ionic compounds! 1. NaCl1. NaCl________________________________________________________

2. Fe2. Fe22OO33

_________________________________________________________

3. CuCl3. CuCl22__________________________________________________________

4. CuCl4. CuCl__________________________________________________________

5. (NH5. (NH44))22COCO33

___________________________________________________________

6. Ca6. Ca33(PO(PO44) ) 22

____________________________________________________________

Rule for writing ionic formulas:Rule for writing ionic formulas:________________________________________________________________________

Practice writing ionic formulasPractice writing ionic formulas 1. Ca1. Ca2+2+ combined with F combined with F--__________________________________________

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2. Co2. Co3+3+ combined with PO combined with PO443-3-______________________________________________

3. Ni3. Ni2+2+ combined with OH combined with OH--____________________________________________More practiceMore practice

1. calcium combined with oxygen1. calcium combined with oxygen

________________________________________________________

2. potassium combined with oxalate2. potassium combined with oxalate

__________________________________________________________

3. chromium (II) hydrogen sulfate3. chromium (II) hydrogen sulfate

__________________________________________________

Write formulas for these! Tin (II) oxide ____________________ Tin (IV) oxide ____________________ Tin (II) hydroxide ____________________ Tin (II) dichromate ____________________ Tin (II) phosphate ____________________ Ammonium phosphite ____________________

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NAMING COVALENT (MOLECULAR) COMPOUNDS

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LAB B8 Water Testing Read pages 42- 45

1. Define:a. Qualitative tests: b. Quantitative tests:

c. Precipitate:

2. Cations:a. definition: (from previous notes)

b. the cations we will be testing for in this lab are:

c. Why must we call the iron ion we will be testing for “iron III”?

3. Anions:a. definition: (from previous notes)

b. the anions we will be testing for in this lab are:

4. Why are you using distilled water as one of the solutions that you will test?

5. What is a reference solution?

6. List the 4 reference solutions you will use. The reference solutions are named the same as the ions for which you will be testing.

7. Since the reference solutions contain the ions we are testing for, should you always see some sort of reaction when you test the reference solutions?

8. What will you use as your unknown solutions?

9. How will you tell if the ion you are testing for is present in the tap water?

10. Will any ions be present in the distilled water? If not, then why are you testing for them?

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Read suggestions on page 43!!!

GOGGLES ARE REQUIRED!!!!!!

All solutions except distilled, tap water and natural water are in pipettes.

Thoroughly wash, rinse, and dry 3 small beakers. Put distilled water in one, tap water in another, and natural (pond) water in the third.

Follow procedures in book.

CLEAN UP: Rinse excess chemicals in pipettes down drain with tap H20 running. Rinse insides of pipettes thoroughly with tap water twice and then with distilled water. DO NOT DISCARD PIPETTES!!

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26

Naming Ionic Compounds

Name These:

1. MgCl2 _________________ 2. K2O____________________

3. Be3S2 __________________ 4. NH4Cl __________________

5. NH4OH_________________ 6. Ba(CN) 2 _________________

7. Na2SO3 _________________ 8. (NH4) 3PO4 _______________

9. (NH4) 3PO3 ______________ 10. NaBr ___________________

11. NH4Br _______________ 12. H2O ___________________

13. Ar ____________________ 14. CuSO4 __________________

15. CuOH _________________ 16. Cu(OH) 2 _________________

17. Pb(OH) 2 _______________ 18. Pb(OH) 4 _________________

19. MnSO4 ________________20. MnPO4 __________________

21. SnO___________________ 22. SnO2____________________

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Write formulas for these ionic compounds:

1. Calcium hydroxide: _____________

2. Calcium bromide: ______________

3. Copper (I) sulfate: ______________

4. Copper (II) sulfate: ______________

5. Ammonium nitrate: ______________

6. Tin (II) oxide: __________________

7. Tin (IV) oxide: _________________

8. Chromium (II) dichromate: ______________

9. Barium Phosphate ______________

10. Ammonium Carbonate: ______________

11. Strontium bromide________________

12. Cadmium sulfide ____________________

13. Cadmium phosphate___________________

14. Iridium (III) oxide ___________________

15. Iridium (II) phosphate_________________

16. Vanadium(IV) phosphide_______________

18. Mercury(I) selenide___________________

19. Mercury(I) selenate____________________

20. Mercury(II) selenate___________________

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Chem worksheet: names Your name is:________________________________

Write the correct chemical name for:

1) MgS

2) KBr

3) Ba3N2

4) Al2O3

5) NaI

6) SrF2

7) Li2S

8) RaCl2

9) CaO

10) AlP

11) K2S

12) LiBr

13) Sr3P2

14) BaCl2

15) NaBr

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Write the correct name for: (these need roman numerals)

1) CuS

2) PbBr4

3) Pb3N2

4) Fe2O3

5) FeI2

6) Sn3P4

7) Cu2S

8) SnCl2

9) HgO

10) Hg2F2

11) CuCl2

12) CuBr

13) PbO

14) Fe2S3

15) PbCl2

16) SnO

17) Cu2O

18) PbO2

19) FeO

20) SnO2

21) Hg2O

22) Hg2I2

23) AuCl3

24) MnO

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POLYATOMIC IONS: Write the correct name for:

1) AlPO4

2) KNO2

3) NaHCO3

4) CaCO3

5) Mg(OH)2

6) Na2CrO4

7) Ba(CN)2

8) K2SO4

9) NaH2PO4

10) NH4NO3

These formulas involve the use of a polyatomic ion. The cations are all of variable oxidation state, so Roman numerals are needed.

Write the correct name for:

11) Sn(NO3)2

12) FePO4

13) Cu2SO4

14) Ni(C2H3O2)2

15) HgCO3

16) Pb(OH)4

17) Cu2Cr2O7

18) Cu(ClO3)2

19) FeSO4

20) Hg2(ClO4)2

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Chemical Formula Writing Worksheet

Write chemical formulas for the compounds in each box. The names are found by finding the intersection between the cations and anions. Example: The first box is the intersection between the “zinc” cation and the “chloride” anion, so you should write “ZnCl2”, as shown.

zinc iron (II) iron (III) gallium silver lead (IV)chloride ZnCl2acetatenitrateoxidenitridesulfate

Write the formulas for the following compounds:

1) copper (II) chloride ____________________________________

2) lithium acetate ____________________________________

3) vanadium (III) selenide ____________________________________

4) manganese (IV) nitride ____________________________________

5) beryllium oxide ____________________________________

6) sodium sulfate ____________________________________

7) aluminum arsenide ____________________________________

8) potassium permanganate ____________________________________

9) chromium (VI) cyanide ____________________________________

10) tin (II) sulfite ____________________________________

11) vanadium (V) fluoride ____________________________________

12) ammonium nitrate ____________________________________

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Polyatomic Ions

Note: The charge on the ions below is the net charge. For example, PO4 has a -3 charge because the oxidation number of the oxygen (O4) is -2 x 4 = -8 and the oxidation number of the phosphorus (P) is +5. -8 + 5 = -3. Therefore, when writing formulas with polyatomic ions, simply use the charge given in the column above the ion.

+1 ion -1 ions

Formula Name Formula Name

NH4 Ammonium H2PO4 Dihydrogen phosphateC2H3O2AcetateHSO3 Hydrogen sulfite (or bisulfite)HSO4 Hydrogen sulfate (or bisulfate)HCO3 Hydrogen carbonate (or bicarbonate)NO2 NitriteNO3 NitrateCN CyanideOH HydroxideMnO4 PermanganateClO HypochloriteClO2 ChloriteClO3 ChlorateClO4 PerchlorateSCN Thiocyanate

-2 ions

Formula Name HPO4 Hydrogen phosphateC2O4 Oxalate -3 ions SO3 Sulfite Formula Name SO4 SulfateCO3 Carbonate PO4 PhosphateCrO4 Chromate PO3 PhosphiteCr2O7 Dichromate Fe(CN)6 FerricyanideSiO3 SilicateSeO4 Selenate

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Activity series of metalsLi LithiumK PotassiumBa BariumCa CalciumNa SodiumMg MagnesiumAl AluminumZn ZincFe IronNi NickelSn TinPb Lead(H) HydrogenCu CopperHg MercuryAg SilverAu Gold

(metals from Li to Na will replace H from acids and water, from Mg to Pb they will replace H from acids only)

Acid namesanion acid nameending

-ide hydro----ic acid-ite -------ous acid-ate -------ic acid

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