€¦ · web viewa scientist is calculating the density of water. in one trial she measures 20.0...

Unit 6: Chemical Reactions Class Packet

Name:_________________________ Period:__________**SHOW ALL WORK FOR CREDIT**

DATE TOPIC/ACTIVITY HOMEWORK

Monday 2/3 1. Review (pg. 4-12)

Tuesday 2/4 1. Demos2. Continue Review (pg. 4-12)

Wednesday 2/5 1. Types of Chemical Reactions Activity (pg. 13-15)

Thursday 2/6 1. Finish Types of Chemical Reactions Activity2. Notes on Balancing Chemical Reactions

Friday 2/7 1. Work Day (pg. 16-20) Finish Pages (16-20)

Monday 2/10LATE START

1. Types of Chemical Reactions Quiz Video Notes: Law of Conservation of Mass

Tuesday 2/11 1. LOC Activity and Notes

Wednesday 2/12 1. LOC Activity, Notes, and Worksheet (pg.21)

Thursday 2/13 1. Unit 6 Quiz

Friday 2/14 NO SCHOOL

Monday 2/17 NO SCHOOL

Tuesday 2/18 1. Predicting Products Notes2. Solubility Rules

Wednesday 2/19 1. Predicting Products Worksheet (pg. 27-30)

Thursday 2/20 1. Predicting Products Activity2. Continue Worksheets (pg. 27-30)

Friday 2/21 1. Predicting Products Quiz2. Video Notes : Endo/Exothermic Reactions

Endo/Exo Worksheet

Monday 2/24 1. Reactions Lab Day #1

Tuesday 2/25 1. Reactions Lab Day #2

Wednesday 2/26 2. Reactions Lab Day #3 Due Monday March 2nd

Thursday 2/27 Review

Friday 2/28 Unit 6 Test

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KEY IDEAS

In all chemical reactions there is a conservation of mass, energy, and charge.

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A balanced chemical equation represents conservation of atoms. The coefficients in a balanced chemical equation can be used to determine mole ratios in the reaction.

The formula mass of a substance is the sum of the atomic masses of its atoms. The molar mass (gram formula mass) of a substance equals one mole of that substance.

The percent composition by mass of each element in a compound can be calculated mathematically.

Types of chemical reactions include synthesis, decomposition, single replacement, and double replacement.

Evidence that a chemical reaction has occurred

o heat and/or light given offo gas producedo precipitate – an insoluble product formed by the reaction of two solutionso unexpected color change

Diatomic Molecules – elements that exist in pairs (H2, N2, O2, F2, Cl2, Br2, I2)

Review

1. A precise measurement is one that a. contains the correct number of significant figures

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b. is close to the true valuec. contains at least three sig figsd. has measurements close to each other

2. In order to find the volume of a liquid accurately use a(n)______while to find the mass of an object use a(n) ________

a. balance, graduated cylinder.b. Erlenmeyer flask, balance.c. graduated cylinder, balance.d. beaker, graduated cylinder.

3. If there are 2.54 cm in an inch and 10mm in a cm, how many inches are in 12,500 mm?a. 254 inb. 398 inc. 492 ind. 1250 in

4. A scientist is calculating the density of water. In one trial she measures 20.0 mL of water into a graduated cylinder, then measures the mass on a balance. She finds the mass of the graduated cylinder to be 95.45g and the mass of the cylinder and the water to be 115.41g. How should she correctly record the density?

a. 1.0 g/mLb. 0.9980 g/mLc. 1.00 g/mLd. 0.998 g/mL

5. In the same experiment as question 5, another student records their densities in g/mL for 4 different trials: #1- 0.9#2- 0.968#3- 1.0#4- 1.006

Trial___ is most accurate and Trial___ is most precise, given the theoretical density of water at 20°C is 0.9999 g/mL.

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

6. Element X is located between sodium (Na) and Potassium (K) on the periodic table. Element X has aa. higher atomic number than Potassium (K)b. higher atomic mass than Potassium (K)c. higher atomic mass than Sodium (Na)

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d. lower atomic number than Sodium (Na)

7. An element has 5 protons, 5 electrons, and 6 neutrons. Its atomic number is:a. 5b. 10c. 11d. 16

8. Which of the following electron configurations describes a halogen?a. 1s22s22p63s23p63d104s24p6

b. 1s22s22p63s23p63d104s24p5

c. 1s22s22p63s23p63d104s24p4

d. 1s22s22p63s23p63d104s24p3

9. As you move from left to right on the periodic table:a. the atomic number increasesb. the atomic number decreasesc. the atomic mass decreasesd. the radioactivity increases

10. Which set of atoms has (1) electron for bonding?a. hydrogen (H) and helium (He)b. lithium (Li) and fluorine (F)c. helium (He) and neon (Ne)d. lithium (Li) and sodium (Na)

11. The correct formula for nickel (III) sulfite isa. Ni2(SO)3

b. Ni2(SO3)3

c. NiSO3

d. N2(SO3)3

12. How many electrons does chlorine need to fill its outer energy level?a. 1b. 2c. 5d. 7

13. What is the correct name of KOH?a. Monopotassium oxygen hydrideb. Potassium hydratec. Potassium (I) oxygen hydrided. Potassium hydroxide

14. What is the correct name for PO3

a. Monophosphorous trioxideb. Potassium oxidec. Phosphorous oxided. Phosphorous trioxide

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15. A covalent bond involves:a. Sharing electronsb. Exchange of electronsc. Sharing of metallic bondsd. Exchange of protons

16. In which pair of covalent molecules does the first one contains a double bond and the second contain a triple bond?

a. O2 and N2

b. CH3CH3 and CH4

c. CH4 and H2

d. Cl2 and NH2

17. The correct lewis structure for CO2 is:

18. What is the volume, in liters, of 576 grams of SO2 gas at STP?a. 101 Lb. 202 Lc. 216 Ld. 788 L

19. What is the percent composition of oxygen in KNO3?a. 0.475 %b. 47.5 %c. 15.8 %d. 23.3 %

20. Convert 1.20 x 1025 molecules of fluorine to grams.a. 380 gb. 760 gc. 1.4 x 1050 gd. 2.7 x 1050 g

Naming Review

1. lead(II) sulfide

2. P4S9

3. hydrogen fluoride

4. zinc hydroxide 6


5. sodium bromate

6. SF6

7. KNO3

8. Uranium (IV) oxide

9. PbCl2

10. ZnSO4

11. ammonium carbonate

12. chromium(III) sulfite

13. nickel(II) sulfate hexahydrate

14. sulfur trioxide

15. Rb2CrO4

16. Al2O3

17. N2O3

18. K2SO3

19. HgO

20. iron(II) nitride

21. tetraphosphorus decoxide

22. copper(I) oxide

23. aluminum hypochlorite

24. potassium peroxide

25. CuSO3

26. CO

27. MgS

28. KClO2

29. BrI

30. nitrogen trichloride

31. lead (iv) carbonate

32. potassium hydrogen sulfite

33. sodium borate

34. barium sulfite

35. SnCl2

36. copper (ii) sulfate pentahydrate

37. TiPO3

38. Cs2S

39. Li2O2

40. Mn(NO2)2

41. Mercury (i) phosphate

42. sodium hydrogen carbonate

43. copper(I) hydrogen sulfate

44. carbon tetrachloride

45. ammonium phosphate

46. SO2

47. MgSO4·9H2O

48. Co(C2H3O2)2

49. P2O3

50. FeP

Naming Review 2

1. Identify the following compounds as Ionic compound or covalent compound, write the name of the Compounds, and calculate its Molar mass.

Formula Ionic or Covalent Name Molar Mass

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Compound ( g/mole)

1 NaCl

2 CO2

3 FeCl3

4 AlF3

5 N2O5

6 MgCO3

7 P2O5

8 N2O4

9 AgNO3

10 Cu2O

11 SO2

12 Ca3(PO4)2

13 IF5

14 P2S3

15 Ca(OH)2

16 NaHCO3

17 Na2SO3

18 SF6

19 B2H6

20 H2S

2. Identify the following compounds as Ionic compound or covalent compound, write the formula of the Compounds, and calculate its Molar mass.

NameIonic or Covalent

FormulaMolar mass

Compound (g/mole)

1 Magnesium chloride

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2 Aluminum sulfate

3 Diboron tetrabromide

4 Potassium chloride

5 Sodium fluoride

6 Sodium chlorite

7 Sulfur dioxide

8 Ammonium Chloride

9 Copper (II) oxide

10 Nitrogen tribromide

11 Calcium chloride

12 Potassium nitrate

13 Carbone monoxide

14 Silicon dioxide

15 Potassium oxide

16 Tin(IV) selenide

17sodium

phosphate18 Sulfur tetrafluoride

19 Aluminum oxide

20 Arsenic pentfluoride

Types of Reactions Intro Activity

For each type of reaction, write a short description of what you see.1. Synthesis (also called combination)

A + B AB

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2. DecompositionAB A + B OR

3. Single Replacement (also called displacement) A + BC AC + B ORA + BC BA + C OR

4. Double-Replacement

AB + CD AD + CB OR

5. Combustion

CH molecule + O2 CO2 + H2O

6.

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Match the types of reactions to the descriptions below.Match the types of reactions to the descriptions below.Match the types of reactions to the descriptions below.Match the types of reactions to the descriptions below.Match the types of reactions to the descriptions below.Match the types of reactions to the descriptions below.Match the types of reactions to the descriptions below.Match the types of reactions to the descriptions below.Match the types of reactions to the descriptions below.Match the types of reactions to the descriptions below.Match the types of reactions to the descriptions below.Match the types of reactions to the descriptions below.Match the types of reactions to the descriptions below.Match the types of reactions to the descriptions below.Match the types of reactions to the descriptions below.Match the types of reactions to the descriptions below.Match the types of reactions to the descriptions below.Match the types of reactions to the descriptions below.Match the types of reactions to the descriptions below.Match the types of reactions to the descriptions below.Match the types of reactions to the descriptions below.Match the types of reactions to the descriptions below.Match the types of reactions to the descriptions below.Match the types of reactions to the descriptions below.Match the types of reactions to the descriptions below.Match the types of reactions to the descriptions below.Match the types of reactions to the descriptions below.Match the types of reactions to the descriptions below.Match the types of reactions to the descriptions below.Match the types of reactions to the descriptions below.Match the types of reactions to the descriptions below.Match the types of reactions to the descriptions below.


7. Can two elements be used as reactant for a synthesis reaction? If yes, support your answer using the above reactions.

8. Can two compounds be used as reactants for a synthesis reaction? Support your answer using the above reactions.

9. In a single replacement reaction, do any atoms change their charge? Support your answer using the above reactions.

10. In double replacement reactions, do any of the atoms change charge? If yes, support your answer using the above reactions.

11.Based on the examples provided above, which type(s) of reactions typically involve REACTANTS that contain ions dissolved in solution (water).

12.What are the 2 products of a combustion reaction?

Determine what type of reaction is depicted in the following equations. . .

1. H2 + O2 ---> H2O2. N2 + H2 ---> NH3

3. S8 + O2 ---> SO3 *4. N2 + O2 ---> N2O5. HgO ---> Hg + O2

6. Zn + HCl ---> ZnCl2 + H2

7. Na + H2O ---> NaOH +H2

8. H3PO4 ---> H4P2O7 +H2O 11


9. C10H16 + Cl2 ---> C + HCl

10. Al(OH)3 + H2SO4 ---> Al2(SO4)3 + H2O11. Fe + O2 ---> Fe2O3

12. Fe2(SO4)3 + KOH ---> K2SO4 + Fe(OH)3

13. Al + FeO ---> Al2O3 + Fe 14. 14. Fe2O3 + H2 ---> Fe + H2O15. Na2CO3 + HCl ---> NaCl + CO2

16. K + Br2 ---> KBr 17. P4 + O2 ---> P2O5

18. C2H2 + O2 ---> CO2 + H2O19. K2O + H2O ---> KOH 20. H2O2 ---> H2O + O2 21. Al + O2 ---> Al2O3

22. C7H16 + O2 ---> CO2 + H2O23. Na2O2 + H2O ---> NaOH + O2

24. SiO2 + HF ---> SiF4 + H2O 25. C + H2O ---> CO + H2

26. KClO3 ---> KCl + O2

27. Al2(SO4)3 + Ca(OH)2 ---> Al(OH)3 + CaSO4

28. FeCl3 + NH4OH ---> Fe(OH)3 + NH4Cl 29. 29. Sb + O2 ---> Sb4O6

30. C3H8 + O2 ---> CO2 + H2O

Balancing Equations 1

1. _____P + _____O2 _____P2O5

2. _____C2H2(g) + _____O2(g) _____CO2(g) + _____H2O(g)

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3. _____KI + _____Pb(NO3)2 _____PbI2 + _____KNO3

4. _____H2O + _____O2 _____H2O2

5. _____S8 + _____O2 _____SO3

6. _____HNO3 + ____NaHCO3 _____ NaNO3 + _____H2O + _____CO2

7. _____Fe2O3(s) + _____H2(g) _____Fe(s) + _____H2O(l)

8. _____CO2 + _____H2O _____C6H12O6 + _____O2 (do C’s 1st, H’s 2nd, O’s last, then recheck)

9. _____Mg(s) + _____O2(g) _____MgO(s)

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10. _____C3H8 + _____ O2 _____CO2 + _____H2O

If those where pretty easy try this extra problem:

______C8H18 + _____O2 _____CO2 + _____H2O

Balancing Equations 2

Directions: Balance the equation and give the type of reaction. 1. ____ N2 + ____ H2 ____ NH3 Type:__________________________

2. ____ KClO3 ____ KCl + ____ O2 Type:__________________________

3. ____ NaCl + ____ F2 ____ NaF + ____ Cl2 Type:__________________________

4. _____ O2 + _____ C2H5 _____CO2 + _____H2O Type:__________________________

5. ____ H2SO4 + ____ Pb(NO2)4 ____ HNO2 + ____ Pb(SO4)2 Type:__________________________

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6. ____ Ag2O ____ Ag + ____O2 Type:__________________________

7. _____Ca(OH)2 + _____H3PO4 _____Ca3(PO4)2 + _____H2O Type:__________________________

8. _____ C4H8 + _____ O2 _____CO2 + _____H2O Type:__________________________

9. _____Al + _____MgCl2 _____ Mg + _____AlCl3 Type:__________________________

10. ____Al + _____O2 _____Al2O3 Type:__________________________

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Balancing Equations Review

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Activity: Law of Conservation of Mass

Objective: The purpose of this lab is to investigate the law of conservation of mass using a very simple reaction – vinegar & baking soda! Before you begin, answer the questions below.

Materials: 2 beakers labeled A & B, Erlenmeyer flask, balance, vinegar, baking soda, balloon, plastic spoon

Procedure:

Part 11. Calibrate the balance to 0.2. Label two beakers A & B.3. Fill beaker A with 20 mL of vinegar.4. Add 1 spoonful of baking soda into beaker B. 5. Place both beakers on the balance & record the starting

mass.6. Dump the baking soda into beaker A. Do not stir.7. Place both beakers on the balance & record the ending

mass.8. Calculate the amount of mass changed by subtraction.

Part 21. Label 3 test tubes, one for each of the following solutions: NaOH, CuSO4, and Na2CO3.2. Using a clean graduated cylinder for each solution, measure out 10 mL of each and place it in the

correct test tube from step 1.3. Place a 250mL beaker on the balance, THEN zero (or tare) the balance while the beaker is on it. 4. Carefully place the test tubes, KEEPING THEM UPRIGHT, that contain NaOH and CuSO4 into the

beaker. Record their combined mass in your data table.5. Pour the NaOH test tube into the test tube containing the CuSO4 allowing them to mix. Record your

observations.6. Place both test tubes (the empty NaOH and the reaction tube) back into the beaker. Record the

mass.7. Repeat steps 3-6 using Na2SO4 instead of NaOH. You will need 10mL more of the CuSO4.

Observations: Part 1:

Part 2:

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Cleanup: Clean & dry the test tubes and graduated cylinders. All solutions may be poured down the drain.Post-lab/Analysis Part Below is the chemical equation for the reaction in part 1.

1. What are the reactants?

__________________________________________________________________

2. What are the products?

__________________________________________________________________

3. Count the number of elements on each side of the equation & write the total number down below.

Reactants Products_______Hydrogen _______Hydrogen

_______ Oxygen _______ Oxygen

_______ Carbon _______ Carbon

_______ Sodium _______ Sodium

4. Is this reaction “balanced”? Explain.

5. Compare your data and observations in part 1 to part 2. What was the same? What was different?

6. Thinking only about part 2 and the post lab questions 1-4, in your own words define the “Law of Conservation of Mass”.

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7. ALL chemical reactions MUST following the law of conservation of mass. How can we explain the result from part 1?

Law of Conservation of Mass Worksheet

1. Explain a situation in which the reactants might weigh more than the products. (note: this is actually impossible!)

2. Explain a situation in which the reactants might weigh less than the products. (note: this is also impossible!)

3. Use the LAW OF CONSERVATION OF MASS to fill out the missing information in the table below. Use the example #1 as a guide.

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4. Answer the word problems below using the LAW OF CONSERVATION OF MASS.

a) Hydrogen and oxygen react chemically to form water. How much water would form if 14.8 grams of hydrogen reacted with 34.8 grams of oxygen? (H2 + O2 H2O)

b) When ammonium nitrate (NH4NO3) explodes, the products are nitrogen, oxygen, and water. When 40.0 grams of ammonium nitrate explode, 14.0 grams of nitrogen and 8.0 grams of oxygen form. How many grams of water form? (NH4NO3 N2 + O2 + H2O)

While the law is known as the Law of Conservation of Mass, it could also be called the Law of Conservation of Atoms.

5. Using the diagrams below explain why the name Law of Conversation of Atoms would be an equally valid name.

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Predicting Products Fill-In Notes

Most reactions can be classified into _____________ of ____________ types

This allows us to study these reactions and ___________________________________________________________.

1. Synthesis (aka Combination)General Form:

2(or more) reactants 1 product (compound)

3 Cases of reactants:1. Metal & nonmetal2. Nonmetal & nonmetal3. 2 simple molecular compounds (i.e. H2O and CO2)

Ex. _______________________________ ____________________

2. DecompositionGeneral Form:

1 reactant 2 or more products

The type of compound we start with determines what the product will be:a) Binary ionic metal & nonmetalb) Binary molecular 2 elements or 2 simpler comp.c) Ternary ionic comp. 2 simpler comp.

Ex._______________ ________________________________

3. Single ReplacementGeneral form:

A + BC B + AC Element + comp. different element + different comp.

Ex. _________________________________ ________________________________

4. Double ReplacementGeneral form: + - + - + - + -

AB + CD AD + CB 2 ionic comp. 2 new ionic comp.

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Ex. ________________________________ __________________________________

5. CombustionGeneral Form:

CxHy + O2 CO2 + H2O(g) (+ energy)

Ex. ________________________________ __________________________________

Predicting Product Notes

1. Synthesis (combination)

A.) Reactants are _______________ & __________________________:

Product will be a ____________________ ionic comp.

Formula MUST be written based on ionic __________________________Then remember to balance the equation!

Ex. Li + F2

Ex. Ca + O2

Ex. Al + I2

B.) Reactants are 2 nonmetals

Product will be a binary ______________________ compound.Many reactions can form more than 1 possible product

Ex. S + O2 SO2 or SO3

More importantly:3 cases where only 1 product can form

H2 + O2 H2O H2 + N2 NH3

H2 + X2 2HX (where X is any halogen)

Ex. ____H2 + ____Cl2 C.) Reactants are 2 molecular comp.

Usually the reactants combine in a 1:1 ratio, product contains all the atoms from the reactants

Ex. ____H2O + ____ CO2

Ex. ____NH3 + ____ HCl

2. DecompositionA.) if starting substance is a binary ionic comp.:

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break apart into its _____ _____________________.

Ex. ____CuCl

B) If starting with a binary molecular comp.:

Most will break apart into an element and a simpler comp.

Ex. ____H2O2

Molecular comp. that always break apart into elements: ___________, ___________, and ___________

C.) If starting with a ternary ionic comp.:It will not break apart into its elements.

Usually form 2 simple comp., one of which comes from the polyatomic ion (see chart):

Ex. ____MgSO _______________________________________

Ex. ____Na2CO3 ______________________________________

3. Combustion

A.) CxHy + O2 H2O + CO2 (complete combustion)

B.) CxHy + O2 H2O + CO +/or C +/or CO2 (incomplete combustion)

Ex. ____ CH4 + ____O2

4. Single Replacement

_______________ replace metals, ______________________ replace nonmetals

Ex. ____Mg + ____ZnBr2

Ex. ____Mg + ____NaBr

5. Double Replacement

Just remember to switch fronts or backs

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Balance new compounds’ ____________________________!

Then balance the equation.

Ex. ____CaSO4 + ____AgNO3

Predicting Products

Predict the products for the following reactions and balance the equation

Synthesis:

1) _____Mg + _____N2

2) _____H2 + _____O2

3) _____Al + _____ O2

Decomposition

4) ____ PBr3

5) ____ H2O

Single Replacement

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6) ____ Na + ____ FeBr3

7) ____ HBr + ____ Fe

8) ____ NaI + _____ F2

Double Replacement

9) ____ NaOH + ____ H2SO4

10) ____ PbSO4 + ____ AgNO3

11) ____ KMnO4 + ____ ZnCl2

Combustion

12) ____ C2H4O2 + ____ O2

13) ____ O2 + ____ C5H12O2

For the following reactions, 1) give the type, 2) predict the products, and 3) balance the reaction.

1. Type:__________________ _____NH3

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2. Type:__________________ _____K + _____AgCl

3. Type:__________________ _____Na + _____N2

4. Type:__________________ _____C2H5 + _____O2

5. Type:__________________ _____Br2 + _____HCl

6. Type:__________________ _____Al(NO3)3 + _____CaS

7. Type:__________________ _____Al + _____O2

8. Type:__________________ _____Fe2O3

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Predicting Products 2

1. Combustion: C6H12 + O2

2. Synthesis: Mg + I2

3. Double replacement: CuCl2 + H2S

4. Double replacement: NaOH + HClO4

5. Decomposition: ZnCO3 + heat

6. Single replacement: HCl + Zn

7. ________________ Na + MgCl2

8. ________________ Fe(OH)3

9. ________________ K + Cl2

10. C4H6 + O2

11. ________________ BaCl2 + K3PO4

12. ________________ Al2(CO3)3

13. ________________ Al + O2

14. ________________ Pb(NO3)2 + KOH

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15. ________________ H2SO4 + BaCl2

16. ________________ Ca + AgCl

17. ________________ H3PO4 + FeBr3

18. ________________ Li + N2

19. ________________ HCl + Mg(OH)2

20. ________________ Mg(OH)2 + heat

Endothermic vs Exothermic

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1. Endothermic or exothermic?

2. Is energy released or absorbed? Explain how you know in terms of the graph.

3. Which numbers on page 1 could this graph represent?

4. Endothermic or exothermic?

5. Is energy released or absorbed? Explain how you know in terms of the graph.

6. Which numbers on page 1 could this graph represent?

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Dissociation EquationsI. Class Practice

a. AlF3

b. Cobalt (II) chlorate

II. Write the Balanced dissociation equations for the following compounds.

1. NaBr

2. CaCl2

3. (NH4)2SO4

4. K2SO3

5. Fe3(SO4)2

6. Li3PO4

III. Write the balanced dissociation equation for:

7. Sodium chloride

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8. Lead (IV) sulfide

9. Ammonium acetate

10.Potassium cyanide

11.Strontium oxide

12.Strontium hydroxide

Net Ionic EquationsWhen two solutions of ionic compounds are mixed, a solid may form. This type of reaction is called aprecipitation reaction, and the solid produced in the reaction is known as the precipitate. You can predict whethera precipitate will form using a list of solubility rules such as those found in the table below. When a combination ofions is described as insoluble, a precipitate forms.

There are three types of equations that are commonly written to describe a precipitationreaction. The molecular equation shows each of the substances in the reaction as compounds withphysical states written next to the chemicalformulas. The complete ionic equation shows each of the compounds as separate ions if they are water soluble. Insoluble substances are not separated and these have the symbol (s) written next to them.

Notice that there are ions that are present on both sides of the reaction arrow – that is, they do not react. These ions are known as spectator ions and they are commonly eliminated from complete ionic equation by crossing them out. The remaining equation is known as the net ionic equation.

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Write the complete ionic equation and cross out the spectator ions to give the net ionic equation

for each of the reactions below. Include physical states for each species.

Write the net ionic equation for each of the following reactions. List all spectator ions.7. A solution of aluminum bromide, AlBr3 reacts with a solution of sodium hydroxide, NaOH to form theprecipitate aluminum hydroxide, Al(OH)3.

8. Aqueous copper (II) nitrate, Cu(NO3)2 reacts with aqueous potassium carbonate, K2CO3 forming solidcopper (II) carbonate, Cu(CO3).

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9. A solution of barium chloride, BaCl2 reacts with a solution of magnesium sulfate, MgSO4 to form theprecipitate barium sulfate, BaSO4.

10. Aqueous potassium sulfide, K2S reacts with a solution of cadmium chloride, CdCl2 to form solid cadmiumsulfide, CdS.

Practice Problems on Net Ionic Equations

Show the total ionic and net ionic forms of the following equations. If all species are spectator ions, please indicate that no reaction takes place. Note! You need to make sure the original equation is balanced before proceeding! A set of solubility rules are given at the end of this document. 1. Molecular: AgNO3(aq) + KCl(aq) AgCl(s) + KNO3(aq)

Total Ionic:

Net Ionic:

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2. Molecular: Mg(NO3)2(aq) + Na2CO3(aq) MgCO3(s) + NaNO3(aq)

Total Ionic:

Net Ionic:

3.Molecular: strontium bromide(aq) + potassium sulfate(aq) strontium sulfate(s) + potassium bromide(aq)

Total Ionic:

Net Ionic:

4. Molecular: manganese(II)chloride(aq) + ammonium carbonate(aq) manganese(II)carbonate(s) + ammonium chloride(aq)

Total Ionic:

Net Ionic:

5. Molecular:chromium(III)nitrate(aq) + iron(II)sulfate(aq) chromium(III)sulfate(aq) + iron(II)nitrate(aq)

Total Ionic:

Net Ionic:

Please complete the following reactions, and show the total ionic and net ionic forms of the equation:

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6. K3PO4(aq) + Al(NO3)3(aq)

7. BeI2(aq) + Cu2SO4(aq)

8. Ni(NO3)3(aq) + KBr(aq)

9. cobalt(III)bromide + potassium sulfide

10. barium nitrate + ammonium phosphate

11. calcium hydroxide + iron(III)chloride

12. rubidium fluoride + copper(II)sulfate

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€¦ · web viewa scientist is calculating the density of water. in one trial she measures 20.0...

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