part 1, unit 2: chemical...

Part 1, Unit 2: Chemical Reactions

Unit 2 Performance ObjectivesUnit 2 Performance ObjectivesChemical Compounds

I I Define and distinguish between atoms, molecules and ions.I I List the properties of metals and incorporate them into the concept of metallic character.I Categorize an element as metallic or nonmetallic based on its properties.I Recognize metallic elements or non-metallic elements from their locations on the Periodic Table.I I Define and distinguish between alloys and compounds.I I Recognize an alloy from its constituents.I I Define and distinguish between ionic compounds and molecular compounds.I I Recognize an ionic compound from its name and list the ions that make it up.I I Contrast the properties of ionic compounds to those of molecular compounds.I I Categorize a compound as ionic or molecular based on the elements that make it up.I I Categorize a compound as ionic or molecular based on its properties.I Distinguish between organic compounds and inorganic compounds and categorize an organic

compound as molecular.

Chemical ReactionsI Define chemical reaction.I Define and distinguish between reactants and products.I List the reactants and products in a given word equation.I I Make and list multiple observations indicating that a chemical reaction has occurred in the

laboratory.I Apply the Law of Conservation of Mass to a chemical reaction.I I Make mass measurements precisely enough to verify the Law of Conservation of Mass.I I Categorize a reaction as exothermic or endothermic from observations in the laboratory.I Apply the Law of Conservation of Energy to a chemical reaction.I I Hypothesize the source of the energy released in an exothermic reaction witnessed in the lab.

Reaction TypesI I Define and give examples of the five reaction types: synthesis (formation), decomposition, single

replacement, double replacement, combustionI I Define and give examples of the six kinds of decomposition reactions.I I Define and give examples of the four kinds of single replacement reactions.I I Classify a given reaction into one of the five types from the word equation.I I Classify a given reaction into one of the five types from only the reactants.I I I Predict the products of a reaction when given the reactants.I Recognize and state the conditions under which a single replacement reaction will occur.I Recognize and state the organizing principle behind the activity series.I I Use the activity series to predict if a single replacement reaction will occur.I Recognize and state the conditions under which a double replacement reaction will occur.I I Use a solubility chart to predict if a double replacement reaction will occur.I I I Recognize spectator ions in single replacement or double replacement reactions.I I I Write word equations for single and double replacement reactions without spectator ions.

Part 1, Unit 2 Study Guide:


Unit 2 VocabularyUnit 2 VocabularyChemical Compounds

alloyatomcompound (From Unit 1 Vocabulary)ionionic compoundmetallic charactermoleculemolecular compoundorganic compoundinorganic compound

Chemical Reactionsactivity seriesendothermic process (From Unit 1 Vocabulary)exothermic process (From Unit 1 Vocabulary)Law of Conservation of Mass (From Unit 1 Vocabulary)Law of Conservation of Energy (From Unit 1 Vocabulary)precipitateproductsreactantsreaction (chemical reaction)species: (g), (l), (s), (aq)word equation(yields)

Reaction Typescombustion reactiondecomposition reactiondouble replacement reactionsingle replacement reactionsynthesis reaction



Activity Series for Various ElementsActivity Series for Various ElementsSingle Replacement Reactions only occur if a more active element replaces a less active one. The table

below, from Holt Chemistry: Visualizing Matter, gives the relative reactivities of various elements. The list on the left includes metals and elemental hydrogen; the list on the right includes halogens. Elements at the top of the list are the most active, and those at the bottom of the list are the least active. An element that is above another will replace it in a single replacement reaction, forcing the less active element out of the compound and taking its place. Note that metals can only replace other metals or hydrogen (same side of the stairstep line), and non-metals can only replace other non-metals.

Activity Series of Various ElementsMetals

lithiumrubidium

potassiumbarium

strontiumcalciumsodium

magnesiumaluminum

manganesezinc

chromiumiron

cadmium

cobalt nickel

tinlead

HYDROGENAntimonybismuthcopper

mercury

silverplatinum

gold


React with cold water and acids, replacing hydrogen. React with oxygen, forming oxides.

React with steam (but not cold water) and acids, replacing hydrogen. React with oxygen forming oxides.

Do not react with water. React with acids, replacing hydrogen. React with oxygen forming oxides.

React with oxygen, forming oxides.

Fairly unreactive. Form oxides only indirectly.

More Active


Less Active

Non-Metals

fluorinechlorinebromineiodine



Solubilities of Various Ionic CompoundsSolubilities of Various Ionic Compounds

Double Replacement Reactions only occur if a solid, liquid, or gas is formed. The table below, from Holt Chemistry, gives the relative solubilities of a variety of ionic compounds. Cross-reference the cation (positive ion) on the left against the anion (negative ion) along the top. Compare the letter given with the key in the table. If the compound formed is soluble in water, then the ions forming it will not produce a solid. If, however, the compound formed is not soluble or partially soluble in water, then a precipitate will be formed.Key: S = Soluble in water. A = Insoluble in water, but soluble in acids. P = Partially soluble in water

solutions, and soluble in dilute acids. I = Insoluble in both water and dilute acids. a = insoluble in water, slightly soluble in acids. d = decomposes in water.

acetate

bromide

carbonate

chlorate

chloride

chromate

hydroxide

iodide

nitrate

oxide

phosphate

silicate

sulfate

sulfide

aluminum S S - S S - A S S a A I S dammonium S S S S S S - S S - S - S Sbarium S S P S S A S S S S A S a dcalcium S S P S S S P S S P P P P Pcopper (II) S S - S S - A - S A A A S Ahydrogen S S - S S - - S S - S I S Siron (II) S S P S S - A S S A A - S Airon (III) S S - S S A A S S A P - P dlead (II) S S A S S A P P S P A A P Amagnesium S S P S S S A S S A P A S dmanganese (II) S S P S S - A S S A P I S Amercury (I) P A A S a P - A S A A - P Imercury (II) S S - S S P A P S P A 0 d Ipotassium S S S S S S S S S S S S S Ssilver P a A S a P - I S P A - P Asodium S S S S S S S S S S S S S Sstrontium S S P S S P S S S S A A - Stin (II) d S - S S A A S d A A - S Atin (IV) S S - - S S P d - A - - S Azinc S S P S S P A S S P A A S A

Examples: Aluminum acetate is soluble in water (S); thus, it will not precipitate in water solution.Aluminum hydroxide is not soluble in water unless the solution is acidic (A). In non-acidic water solutions it will form a precipitate of solid aluminum hydroxide.



Determining Reaction Types IDetermining Reaction Types ICircle the reaction type for each of the following chemical reactions. In all of the problems on the following pages, S = synthesis; D = decomposition; SR = single replacement; DR = double replacement; C = combustion.1. iron + sulfur iron(II) sulfide

S D SR DR C

2. nitrogen + hydrogen ammonia

S D SR DR C

3. zinc + copper(II) sulfate zinc sulfate + copper

S D SR DR C

4. potassium nitrate + sodium bromide sodium nitrate + potassium bromide

S D SR DR C

5. potassium chlorate (heated) potassium chloride + oxygen

S D SR DR C

6. magnesium nitrate + calcium iodide calcium nitrate + magnesium iodide

S D SR DR C

7. water (electricity added) hydrogen + oxygen

S D SR DR C

8. potassium + lead (II) iodide lead + potassium iodide

S D SR DR C

9. aluminum + oxygen aluminum oxide

S D SR DR C

10. magnesium chloride + ammonium nitrate magnesium nitrate + ammonium chloride

S D SR DR C

If you got any of these wrong, do not go on until you figure out why.



Determining Reaction Types IIDetermining Reaction Types IICircle the reaction type for each of the following chemical reactions:1. iron(III) chloride + ammonium hydroxide iron(III) hydroxide + ammonium chloride

S D SR DR C

2. Hydrogen peroxide water + oxygen

S D SR DR C

3. magnesium oxide + iron iron (III) oxide + magnesium

S D SR DR C

4. iron + water hydrogen + iron(III) oxide

S D SR DR C

5. iron(III) chloride + potassium nitrate potassium chloride + iron(III) nitrate

S D SR DR C

6. copper + sulfuric acid copper (II) sulfate + hydrogen

S D SR DR C

7. Sodium carbonate + calcium hydroxide sodium hydroxide + calcium carbonate

S D SR DR C

8. carbon dioxide + water carbonic acid

S D SR DR C

9. phosphorus + oxygen diphosphorus pentoxide

S D SR DR C

10. Sodium + lithium hydroxide sodium hydroxide + lithium

S D SR DR C




Determining Reaction Types IIIDetermining Reaction Types III

Circle the reaction type for each of the following chemical reactions:1. potassium oxide + water potassium hydroxide

S D SR DR C

2. ammonium sulfide + lead(II) nitrate ammonium nitrate + lead(II) sulfide

S D SR DR C

3. sodium hydroxide + magnesium magnesium hydroxide + sodium

S D SR DR C

4. potassium hydroxide + phosphoric acid potassium phosphate + water

S D SR DR C

5. calcium chloride + nitric acid calcium nitrate + hydrochloric acid

S D SR DR C

6. mercury(II) oxide (heated strongly) mercury + oxygen

S D SR DR C

7. magnesium hydroxide + sulfuric acid magnesium sulfate + water

S D SR DR C

8. magnesium + nitric acid magnesium nitrate + hydrogen

S D SR DR C

9. aluminum + iron(III) oxide aluminum oxide + iron

S D SR DR C

10. potassium nitrate + calcium chloride calcium nitrate + potassium chloride

S D SR DR C




Determining Reaction Types IVDetermining Reaction Types IV

Circle the reaction type for each of the following chemical reactions:1. calcium bromide + chlorine calcium chloride + bromine

S D SR DR C

2. calcium carbonate (heated strongly) calcium oxide + carbon dioxide

S D SR DR C

3. Sodium chloride + sulfuric acid sodium sulfate + hydrochloric acid

S D SR DR C

4. aluminum sulfate + ammonium bromide aluminum bromide + ammonium sulfate

S D SR DR C

5. potassium fluoride + barium bromide barium fluoride + potassium bromide

S D SR DR C

6. copper(II) nitrate + ammonium hydroxide copper(II) hydroxide + ammonium nitrate

S D SR DR C

7. Sodium nitrate (heated strongly) sodium nitrite + oxygen

S D SR DR C

8. lead(II) hydroxide (heated strongly) lead(II) oxide + water

S D SR DR C

9. ammonia + sulfuric acid ammonium sulfate

S D SR DR C

10. hydrochloric acid + ammonia ammonium chloride

S D SR DR C



Determining Reaction Types VDetermining Reaction Types VCircle the reaction type for each of the following chemical reactions:1. copper + sulfuric acid copper (II) sulfate + hydrogen

S D SR DR C

2. aluminum sulfate + calcium hydroxide aluminum hydroxide + calcium sulfate

S D SR DR C

3. calcium oxide + water calcium hydroxide

S D SR DR C

4. iron + copper(I) nitrate iron(II) nitrate + copper

S D SR DR C

5. iron(II) nitrate + hydrochloric acid nitric acid + iron(II) chloride

S D SR DR C

6. iron (II) sulfate + copper copper (II) sulfate + iron

S D SR DR C

7. aluminum + hydrochloric acid aluminum chloride + hydrogen

S D SR DR C

8. carbon + oxygen carbon dioxide

S D SR DR C

9. potassium bicarbonate + sodium chloride sodium bicarbonate + potassium chloride

S D SR DR C

10. hydrogen choride + fluorine hydrogen fluoride + chlorine

S D SR DR C

If you got any of these wrong, you did not do the real job.By this time you should have learned how to determine reaction types PERFECTLY.

If you cannot do this, you should figure out how your thinking is incorrect.



Worksheet AnswersWorksheet AnswersDetermining Reaction Types I

1. S 6. N.R.2. S 7. D3. SR 8. SR4. N.R. 9. S, C5. D 10. N.R.

Determining Reaction Types II1. DR 6. N.R.2. D 7. DR3. N.R. 8. S4. SR 9. S,C5. N.R. 10. N.R.

Determining Reaction Types III1. S 6. D2. DR 7. DR3. N.R. 8. SR4. DR 9. SR5. N.R. 10. N.R.

Determining Reaction Types IV1. SR 6. DR2. D 7. D3. N.R. 8. D4. N.R. 9. S5. N.R. 10. S

Determining Reaction Types V1. N.R. 6. N.R.2. DR 7. SR3. S 8. S, C4. SR 9. N.R.5. N.R. 10. SR



Writing Word Equations IWriting Word Equations IEach of the problems below describes a chemical process. For the most part,

reactants and products are given in the description for the process, along with information about any species that might be unusual or important. For each process, do the following:

a. Circle the reaction type.b. Write a word equation for the reaction described. c. Indicate the species of each reactant and product with their names.

1. With a sufficient supply of oxygen, carbon burns completely to form carbon dioxide.

S D SR DR C

2. Where the oxygen supply is restricted, such as in an internal combustion engine, carbon burns in oxygen to form carbon monoxide.

S D SR DR C

3. Magnesium metal reacts with nitric acid to form hydrogen gas and a solution of magnesium nitrate.

S D SR DR C

4. Aluminum metal reacts with sulfuric acid to form hydrogen and a solution of aluminum sulfate.

S D SR DR C

5. Sodium peroxide reacts with water to form oxygen bubbles and a solution of sodium hydroxide.

S D SR DR C


Part 1, Unit 2: Chemical ReactionsWriting Word Equations I, Continued

6. When heated strongly, potassium chlorate decomposes to form oxygen and potassium chloride.

S D SR DR C

7. Although it happens too slowly to see, aluminum metal reacts with oxygen to form a very thin coating of aluminum oxide, which is so unreactive that aluminum cans decompose only with difficulty. Aluminum oxide, often called alumina, is the same material that makes up rubies and sapphires.

S D SR DR C

8. Salt dissolves to form a solution of sodium ions and chloride ions. Think about this one before answering it. What is the chemical change involved?

S D SR DR C

9. Ammonia reacts with oxygen to form nitrogen and water.

S D SR DR C

10. Like ALL hydrocarbons, methane (natural gas) burns completely to form carbon dioxide and water. Remember, oxygen is essential to the process of combustion.

S D SR DR C



Writing Word Equations IIWriting Word Equations IIEach of the problems below describes a chemical process. For the most part,

reactants and products are given in the description for the process, along with information about any species that might be unusual or important. For each process, do the following:

a. Circle the reaction type.b. Write a word equation for the reaction described. c. Indicate the species of each reactant and product with their names.

1. When rain falls through the atmosphere, it picks up carbon dioxide to form a carbonic acid solution.

S D SR DR C

2. When fluorine is bubbled through a solution of sodium chloride, chlorine is produced, along with a solution of sodium fluoride.

S D SR DR C

3. Phosphorus metal burns to form gaseous diphosphorus pentoxide. Remember what is required for burning to occur?

S D SR DR C

4. Diphosphorus pentoxide is bubbled through water to form phosphoric acid.

S D SR DR C

5. When heated strongly, sodium nitrate decomposes to form sodium nitrite and oxygen. No water is present.

S D SR DR C


Part 1, Unit 2: Chemical ReactionsWriting Word Equations II, Continued

6. Zinc lumps react with chlorine to form zinc chloride powder.

S D SR DR C

7. Steam and hot iron granules form hydrogen and grains of magnetite, a mixture of iron oxides that is found in nature as a mineral commonly called lodestone.

S D SR DR C

8. The red mineral cinnabar, mercury (II) oxide, can be heated to form metallic mercury and oxygen.

S D SR DR C

9. When heated, grains of sodium bicarbonate break down into sodium carbonate powder, carbon dioxide, and steam.

S D SR DR C

10. Under pressure, gaseous propane becomes a liquid, which is easy to store in tanks. When this liquid is burned in a BBQ grill, it is first reheated to form a gas, and then it burns completely in air. Propane is a hydrocarbon (an organic compound) and like all other hydrocarbons, it has only two combustion products: carbon dioxide and water.

S D SR DR C



Worksheet AnswersWorksheet AnswersWriting Word Equations I

1. S,C carbon (s) + oxygen (g) carbon dioxide (g)

2. S,C carbon (s) + oxygen (g) carbon monoxide (g)

3. SR magnesium (s) + nitric acid (aq) hydrogen (g) + magnesium nitrate solution (aq)

4. SR aluminum (s) + sulfuric acid (aq) hydrogen (g) + aluminum sulfate solution (aq)

5. DR sodium peroxide (s) + water (l) oxygen (g) + sodium hydroxide solution (aq)

6. D potassium chlorate (s) potassium chloride (s) + oxygen (g)

7. S,C aluminum (s) + oxygen (g) aluminum oxide (s)

8. N/A physical process, not chemical: sodium chloride (s) sodium ions (aq) + chloride ions (aq)

9. SR ammonia (g) + oxygen (g) nitrogen (g) + water (l)

10. C methane (g) + oxygen (g) carbon dioxide (g) + water (l)

Writing Word Equations II1. S water (l) + carbon dioxide (g) carbonic acid (aq)

2. SR fluorine (g) + sodium chloride solution (aq) chlorine (g) + sodium fluoride solution (aq)

3. S.C phosphorus (s) + oxygen (g) diphosphorus pentoxide (g)

4. S diphosphorus pentoxide (g) + water (l) phosphoric acid (aq)

5. D sodium nitrate (s) sodium nitirite (s) + oxygen (g)

6. S zinc (s) + chlorine (g) zinc chloride (s)

7. SR water (g) + iron (s) hydrogen (g) + magnetite (s)

8. D mercury (II) oxide (s) mercury (l) + oxygen (g)

9. D sodium bicarbonate (s) sodium carbonate (s) + carbon dioxide (g) + water (l)

10. C propane (g) + oxygen (g) carbon dioxide (g) + water (l)



Predicting Reaction ProductsPredicting Reaction ProductsTo predict the products of a reaction when you only know the reactants, first examine the reactants and try to determine the type of reaction that is expected. Generally this is fairly straightforward. Use the guidelines below as a first guess. There may be exceptions where this prediction is not correct, but these will be rare.

Characteristics of Reactants Probable Reaction TypeTwo elements SynthesisMetal plus oxygen Synthesis AND combustionOnly one reactant DecompositionElement plus a compound Single replacementMetal plus acid Single replacementReactive metal plus water Single replacementTwo ionic compounds Double replacementIonic compound plus an acid Double replacementHydrocarbon plus oxygen CombustionMolecular compound plus oxygen Combustion

After you have decided on the probable reaction type, predict the products using these guidelines:

Reaction Type Probable ProductsSynthesis One compoundDecomposition Two products simpler than the reactant. If the reactant is an ionic

compound, look for a simple molecule “hidden” in the negative ion, such as carbon dioxide in the carbonate ion.

Single replacement An element plus a compound. The element in the reactants will be part of the compound, and part of the compound in the reactants will be the element.

Double replacement Two ionic compounds or an ionic compound plus water.Combustion Oxides

Finally check to see your answer is reasonable.

Reaction Type CheckSynthesis Check to see that ONLY one product is formed. Check to see if it

is the reverse of one of the six types of decomposition.Decomposition Products simpler than the reactant. Check against the six types of

decomposition.Replacement Replacement reactions frequently, but not always, occur in

aqueous solution. It is unlikely that two solids will react.Single replacement Use the activity series to make sure the element in the reactants is

more reactive than the element in the products. If not, no reaction will occur.


Double replacement Check to see if a gas or water is produced. If not, use the solubility chart to see that one of the ionic compounds formed is insoluble. If all products are soluble, no reaction occurs.

Combustion Check to see that ALL products are oxides. If the reactant is a hydrocarbon, make sure the products include water (the oxide of the hydrogen atoms) and carbon dioxide (the oxide of the carbon atoms).



Predicting SpeciesPredicting SpeciesWhen attempting to determine the species of reactants and products, use the following guidelines. Realize that your prediction may not be accurate, but your skill will improve as you come to know more about the materials involved.

Material Probable SpeciesMetallic element SolidNonmetallic element Use periodic table for speciesIonic compound SOLIDIonic compound in solution AqueousIon AqueousMolecular compound Often gas or liquid, unless there are many

atoms in the formulaWater Liquid unless at high temperaturesAcid AqueousHydrocarbons Solid or liquid unless simple



Predicting Reaction Products IPredicting Reaction Products IIn each of the following practice problems:

a. Examine the reactants and circle the type of reaction that is expected.b. Predict the products of the reaction and finish the word equation.c. Check to see if your products are reasonable.

1. aluminum plus hydrochloric acid S D SR DR C

2. calcium hydroxide plus nitric acid S D SR DR C

3. carbonic acid (heated) S D SR DR C

4. carbon dioxide plus water S D SR DR C

5. magnesium plus zinc nitrate S D SR DR C

6. mercury(II) oxide (heated) S D SR DR C

7. mercury plus oxygen S D SR DR C

8. zinc chloride plus hydrogen sulfide S D SR DR C

9. oxygen plus sulfur S D SR DR C

10. silver iodide plus iron(III) sulfide S D SR DR C



Predicting Reaction Products IIPredicting Reaction Products IIIn each of the following practice problems:


1. sodium chlorate (heated) S D SR DR C

2. sodium plus chlorine S D SR DR C

3. fluorine plus potassium bromide S D SR DR C

4. copper (heated) plus steam S D SR DR C

5. sodium bromide plus silver nitrate S D SR DR C

6. calcium phosphate plus aluminum sulfate S D SR DR C

7. zinc carbonate (heated) S D SR DR C

8. mercury(I) nitrate plus ammonium chloride S D SR DR C

9. potassium plus fluorine S D SR DR C

10. potassium phosphate plus zinc nitrate S D SR DR C



Predicting Reaction Products IIIPredicting Reaction Products IIIIn each of the following practice problems:


1. lithium hydroxide (heated) S D SR DR C

2. sodium chloride (electrolyzed) S D SR DR C

3. iron(III) hydroxide plus phosphoric acid S D SR DR C

4. methane plus oxygen S D SR DR C

5. copper(II) iodide plus silver nitrate S D SR DR C

6. calcium plus aluminum chloride S D SR DR C

7. potassium hydroxide plus hydrogen sulfide solution S D SR DR C

8. sodium carbonate plus sulfuric acid S D SR DR C

9. barium carbonate (heated) S D SR DR C

10. lithium plus bromine S D SR DR C



Predicting Reaction Products IVPredicting Reaction Products IVIn each of the following practice problems:


1. ammonium phosphate plus lithium hydroxide S D SR DR C

2. hydrogen plus oxygen S D SR DR C

3. mercury plus nitric acid S D SR DR C

4. sodium oxide plus water S D SR DR C

5. calcium carbonate plus lithium chloride S D SR DR C

6. mercury(I) hydroxide plus hydrochloric acid S D SR DR C

7. potassium nitrate (heated) S D SR DR C

8. tin plus lead(II) nitrate S D SR DR C

9. mercury(I) nitrate plus sodium carbonate S D SR DR C

10. magnesium plus hydrochloric acid S D SR DR C



Predicting Reaction Products VPredicting Reaction Products VIn each of the following practice problems:


1. ammonium nitrite plus barium hydroxide S D SR DR C

2. ammonium sulfate plus calcium hydroxide S D SR DR C

3. ammonium phosphate plus aluminum chloride S D SR DR C

4. barium oxide plus water S D SR DR C

5. iron(III) hydroxide plus nitric acid S D SR DR C

6. calcium plus oxygen S D SR DR C

7. calcium plus phosphoric acid S D SR DR C

8. calcium chloride plus ammonium hydroxide S D SR DR C

9. aluminum sulfide plus hydrochloric acid S D SR DR C

10. magnesium plus sulfur S D SR DR C



Predicting Reaction Products VIPredicting Reaction Products VIIn each of the following practice problems:


1. sodium chloride plus potassium chromate S D SR DR C

2. potassium sulfide plus iron(II) nitrate S D SR DR C

3. magnesium carbonate plus phosphoric acid S D SR DR C

4. aluminum chloride (electrolyzed) S D SR DR C

5. lead(II) chlorate (heated) S D SR DR C

6. calcium carbonate plus hydrochloric acid S D SR DR C

7. iron plus sodium bromide S D SR DR C

8. ammonium acetate plus iron(II) chloride S D SR DR C

9. zinc plus sulfuric acid S D SR DR C

10. iron plus potassium iodide S D SR DR C



Predicting Reaction Products VIIPredicting Reaction Products VIIIn each of the following practice problems:


1. lead(II) hydroxide plus hydrochloric acid S D SR DR C

2. iron plus sulfur S D SR DR C

3. potassium chlorate (heated) S D SR DR C

4. potassium plus chlorine S D SR DR C

5. iron(II) carbonate plus phosphoric acid S D SR DR C

6. potassium iodide plus ammonium nitrate S D SR DR C

7. bromine plus sodium iodide S D SR DR C

8. silver sulfide plus hydrochloric acid S D SR DR C

9. magnesium nitrate plus hydrochloric acid S D SR DR C

10. ammonia plus hydrogen chloride S D SR DR C



Predicting Reaction Products VIIIPredicting Reaction Products VIIIIn each of the following practice problems:


1. zinc hydroxide plus sulfuric acid S D SR DR C

2. calcium oxide plus water S D SR DR C

3. calcium hydroxide (heated) S D SR DR C

4. fluorine plus aluminum bromide S D SR DR C

5. carbon dioxide plus water S D SR DR C

6. copper(I) hydroxide plus hydrochloric acid S D SR DR C

7. aluminum plus oxygen S D SR DR C

8. magnesium chlorate (heated) S D SR DR C

9. bromine plus calcium chloride S D SR DR C

10. magnesium oxide plus water S D SR DR C



Predicting Reaction Products AnswersPredicting Reaction Products AnswersPredicting Reaction Products IPredicting Reaction Products I1. SR aluminum + hydrochloric acid hydrogen (g) + aluminum chloride (aq)

2. DR calcium hydroxide + nitric acid calcium nitrate (aq) + water (l)

3. D carbonic acid (heated) carbon dioxide (g) + water (l)

4. S carbon dioxide + water carbonic acid (aq)

5. SR magnesium + zinc nitrate zinc (s) + magnesium nitrate (aq)

6. D mercury(II) oxide (heated) mercury (l) + oxygen (g)

7. S, C mercury + oxygen mercury (II) oxide (s)

8. DR zinc chloride + hydrogen sulfide zinc sulfide (s) + hydrochloric acid (aq)

9. S, C oxygen + sulfur sulfur dioxide (g)

10. DR silver iodide + iron(III) sulfide silver sulfide (s) + iron (III) iodide

Predicting Reaction Products IIPredicting Reaction Products II1. D sodium chlorate (heated) sodium chloride (s) + oxygen (g)

2. S sodium + chlorine sodium chloride (s)

3. SR fluorine + potassium bromide bromine (l) + potassium fluoride

4. SR copper (heated) + steam hydrogen (g) + copper (II) oxide

5. DR sodium bromide + silver nitrate silver bromide (s) + sodium nitrate (aq)

6. DR calcium phosphate + aluminum sulfate calcium sulfate (s) + aluminum phosphate (aq)

7. D zinc carbonate (heated) zinc oxide (s) + carbon dioxide (g)

8. DR mercury(I) nitrate + ammonium chloride mercury (I) chloride (s) + ammonium nitrate (aq)

9. S potassium + fluorine potassium fluoride (s)

10. DR potassium phosphate + zinc nitrate potassium nitrate (aq) + zinc phosphate (s)

Predicting Reaction Products IIIPredicting Reaction Products III1. D lithium hydroxide (heated) lithium oxide (s) + water (l)

2. D sodium chloride (electrolyzed) sodium (s) + chlorine (g)

3. DR iron(III) hydroxide + phosphoric acid iron (III) phosphate (aq) + water (l)

4. C methane + oxygen carbon dioxide (g) + water (l)

5. DR copper(II) iodide + silver nitrate silver iodide (s) + copper (II) nitrate (aq)

6. SR calcium + aluminum chloride aluminum (s) + calcium chloride (aq)

7. DR potassium hydroxide + hydrogen sulfide solution potassium sulfide (aq) + water (l)

8. DR, D sodium carbonate + sulfuric acid sodium sulfate (aq) + water (l) + carbon dioxide (g) Carbonic acid is formed first, and then it immediately decomposes to water and carbon dioxide.

9. D barium carbonate (heated) barium oxide (s) + carbon dioxide (g)

10. S lithium + bromine lithium bromide (s)


Part 1, Unit 2: Chemical ReactionsPredicting Reaction Products Answers, Continued

Predicting Reaction Products IVPredicting Reaction Products IV1. N.R. ammonium phosphate + lithium hydroxide no change; both products would be soluble

2. S, C hydrogen + oxygen water (l)

3. SR mercury + nitric acid hydrogen (g) + mercury (II) nitrate (aq)

4. S sodium oxide + water sodium hydroxide (aq)

5. N.R. calcium carbonate + lithium chloride no change; calcium carbonate is not soluble, so no reaction occurs.

6. DR mercury(I) hydroxide + hydrochloric acid mercury (I) chloride + water (l)

7. D potassium nitrate (heated) potassium nitrite (s) + oxygen (g)

8. SR tin + lead(II) nitrate lead (s) + tin (II) nitrate (which decomposes)

9. DR mercury(I) nitrate + sodium carbonate mercury (I) carbonate (s) + sodium nitrate (aq)

10. SR magnesium + hydrochloric acid hydrogen (g) + magnesium chloride (aq)

Predicting Reaction Products VPredicting Reaction Products V1. N.R. ammonium nitrite + barium hydroxide no change; both products would be soluble.

2. DR ammonium sulfate + calcium hydroxide calcium sulfate (s) + ammonium hydroxide (aq)

3. DR ammonium phosphate + aluminum chloride ammonium chloride (aq) + aluminum phosphate (s)

4. S barium oxide + water barium hydroxide (aq)

5. DR iron(III) hydroxide + nitric acid iron (III) nitrate + water (l)

6. S,C calcium + oxygen calcium oxide (s)

7. SR calcium + phosphoric acid hydrogen (g) + calcium phosphate (s)

8. DR calcium chloride + ammonium hydroxide calcium hydroxide (s) + ammonium chloride (aq)

9. DR aluminum sulfide + hydrochloric acid hydrogen sulfide (g) + aluminum chloride (aq)

10. S magnesium + sulfur magnesium sulfide (s)

Predicting Reaction Products VIPredicting Reaction Products VI1. N.R. sodium chloride + potassium chromate no change; both products would be soluble.

2. DR potassium sulfide + iron(II) nitrate iron (II) sulfide (s) + potassium nitrate (aq)

3. DR magnesium carbonate + phosphoric acid magnesium phosphate (aq) + water (l) + carbon dioxide (g) Carbonic acid is formed first, and then it immediately decomposes to water and carbon dioxide.

4. D aluminum chloride (electrolyzed) aluminum (s) + chlorine (g)

5. D lead(II) chlorate (heated) lead (II) chloride (s) + oxygen (g)

6. DR calcium carbonate + hydrochloric acid calcium chloride (aq) + carbonic acid (which decomposes)

7. N.R. iron + sodium bromide no change; iron is less reactive than sodium.

8. N.R. ammonium acetate + iron(II) chloride no change; both products would be soluble.

9. SR zinc + sulfuric acid hydrogen (g) + zinc sulfate (aq)

10. N.R. iron + potassium iodide no change; iron is less reactive than potassium.


Part 1, Unit 2: Chemical ReactionsPredicting Reaction Products Answers, Continued

Predicting Reaction Products VIIPredicting Reaction Products VII1. DR lead(II) hydroxide + hydrochloric acid lead (II) chloride (aq) + water (l)

2. S iron + sulfur iron (II) sulfide (s)

3. D potassium chlorate (heated) potassium chloride (s) + oxygen (g)

4. S potassium + chlorine potassium chloride (s)

5. DR iron(II) carbonate + phosphoric acid iron (II) phosphate (aq) + carbonic acid (which decomposes)

6. N.R. potassium iodide + ammonium nitrate no change; both products would be soluble.

7. SR bromine + sodium iodide iodine (s) + sodium bromide (aq)

8. DR silver sulfide + hydrochloric acid silver chloride (s) + hydrogen sulfide (g)

9. N.R. magnesium nitrate + hydrochloric acid no change; both products would be soluble.

10. S ammonia + hydrogen chloride ammonium chloride (s)

Predicting Reaction Products VIIIPredicting Reaction Products VIII1. DR zinc hydroxide + sulfuric acid zinc sulfate (aq) + water (l)

2. S calcium oxide + water calcium hydroxide (aq)

3. D calcium hydroxide (heated) calcium oxide (s) + water (l)

4. SR fluorine + aluminum bromide bromine (l) + aluminum fluoride (s)5. S carbon dioxide + water carbonic acid (aq)

6. DR copper(I) hydroxide plus hydrochloric acid water (l) + copper(1) chloride (aq)

7. S,C aluminum plus oxygen aluminum oxide (s)

8. D magnesium chlorate (heated) oxygen (g) + magnesium chloride (s)

9. N.R. bromine plus calcium chloride no change; bromine is less reactive than chlorine.

10. S magnesium oxide plus water magnesium hydroxide (s)


part 1, unit 2: chemical...

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