honors chemistry - unit 2 web viewbe able to identify and write the five basic types of equations:...

Unit 5 Packet - of 18Honors Chemistry - Unit 5Chapter 8 – Chemical EquationsQuiz on Diatomic Molecules: Vocab Assignment Due:

Problem Set Due: Test Date:

VOCABULARY Assignment Use the Two-column Notes format/strategy on page 913 (blue textbook) to study/complete your vocabulary assignment.1) chemical reaction 2) reactants 3) products4) single displacement 5) double

displacement6) decomposition

7) Synthesis (composition)

8) combustion 9) subscript

10) coefficient 11) activity seriesOBJECTIVES: Be able to balance chemical equations using coefficients. Be able to identify and write the five basic types of equations: single

displacement, double displacement, synthesis, decomposition and combustion. Be able to use correct notation in equations (such as state symbols). Be able to identify the seven diatomic molecules and use them correctly in

equations. Be able to use the activity series to write equationsSYMBOLS USED IN CHEMICAL EQUATIONS(brief descriptions and table listed below)

State symbols (after formula) s, l, g or aq (book uses cr for crystalline solid) up arrow () gas down arrow () ppt reversible rxn squiggly line above arrow = electric current or with e- as shown below above arrow = heat temp, pressure may be written above arrow catalyst may be written below or above arrow

Unit 5 Packet - of 18

CHEMICAL EQUATIONS AND REACTIONS

Chemical Equation: represents with symbols and formulas the reactants and products

Example:Reactants yields ProductsFe2O3 + 2 Al 2 Fe + Al2O3

Equations must:Represent known facts – all reactants and products must be includedContain correct formulas

Coefficients: numbers in front of compounds/elements Represents the number of moles

Subscripts : numbers in the formulas They are never changed!

Symbols used in equations are on your objective sheet !

WRITING AND BALANCING EQUATIONSDiatomic molecules: Occur in pairs in their natural state (when they are alone and not ionic, not in compounds) – Notice there are 7 of these and they make a 7 shape on the PT!!!!!

Memorize!! (quiz):


Writing & Balancing Equations

Diatomic molecules –occur in pairs in their natural state(when they are alone; not in compounds)I2, Br2, Cl2, F2, O2, N2, H2 (*Quiz*)

II BrBring ClClay FFor OOur NNew HHouseor

HHis BrBrown ClClown FFound NNo OOranges IInside

Unit 5 Packet - of 18When writing equations you must satisfy the law of conservation matter (matter can not be created or destroyed)Therefore we must have the same type and number of each atom on each side of the equation.

BALANCING EQUATIONS: 4 steps:1. Start with a word equation2. Convert to a formula equation (don’t forget the diatomic molecules!)3. Balance with coefficients:

balance each atom one at a timebalance polyatomic ions on each side of the equation as one unitbalance H and O last (they often appear in more than one compound)

4. Check; if coefficients are not the lowest possible; reduce down.

*****Remember NEVER change subscripts***** Examples:

1. water breaks down into hydrogen and oxygen

2. aluminum carbide reacts with water to produce methane gas (CH4) and aluminum hydroxide

3. Na2SO4 + LiCl Li2SO4 + NaCl

You try:

1. calcium oxide reacts with bromine to make calcium bromide and oxygen

2. Ba(NO3)2 + PbO2 BaO + Pb(NO3)4

Unit 5 Packet - of 18BALANCING CHEMICAL REACTIONS

Balance the following reactions:

1. K3PO4 + HCl KCl + H3PO4

2. Na + HNO3 NaNO3 + H2

3. S + O2 SO3

4. Ca(ClO3)2 CaCl2 + O2

5. C2H12 + O2 CO2 + H2O

6. Potassium iodide + lead (II) nitrate potassium nitrate + lead (II) iodide

7. Iron (III) oxide + carbon carbon monoxide + iron

8. Mercury (II) oxide mercury + oxygen

9. Calcium + aluminum chloride calcium chloride + aluminum

10. Mercury (I) nitrate + sodium carbonate sodium nitrate + mercury (I) carbonate

11. Potassium bromide + aluminum nitrate potassium nitrate + aluminum bromide

12. Calcium phosphate + aluminum sulfate calcium sulfate + aluminum phosphate

13. Rubidium + acetic acid rubidium acetate + hydrogen

Unit 5 Packet - of 18Equation Writing Balance and ID the following rxns :

1. Zn + H2SO4 ZnSO4 + H2

2. Na + Br2 NaBr

3. H2O H2 + O2

4. Cl2 + KI KCl + I2

5. HNO3 + LiOH H2O + LiNO3

6. C3H8 + O2 CO2 + H2O

7. Sodium + iodine sodium iodide

8. Zinc + hydrochloric acid zinc chloride and hydrogen gas

9. Potassium hydroxide heated yields potassium oxide and water

10. Magnesium and water produce magnesium hydroxide and hydrogen gas

Reaction Prediction

1. Tin (II) and copper (II) sulfate

2. Iron (III) nitrate and sodium chromate

3. Calcium and iodine

4. Magnesium and sulfuric acid

5. Calcium oxide electrolyzed

6. Carbon and oxygen

7. Sodium carbonate and hydrochloric acid

8. Iron (II) sulfide electrolyzed

9. Platinum (II) and lead (II) nitrate

10. Lithium oxide and water

11. C2H4 + O2

Unit 5 Packet - of 18WRITING CHEMICAL EQUATIONS

Write balanced equations for the following reactions after identifying the type of reaction.

1. aluminum sulfate + calcium phosphate

2. magnesium chloride + manganese (III) nitrate

3. Hydrogen gas + oxygen gas

4. Strontium metal + copper (II) nitrate

5. copper (II) oxide + sulfuric acid

6. nitrogen gas + lithium metal

7. C4 H8 + O2

8. sodium bromide + oxygen gas

9. copper (II) nitride (heated)

10. potassium metal + water

11. C3 H8 + oxygen gas

12. ammonium sulfate + sodium chloride

13. NiO + S

Unit 5 Packet - of 18REACTION TYPES

1. Synthesis: (or composition): 2 or more substances combine to form 1 new substance

A + X AX

Ex’s:

2. Decomposition: A single substance produces 2 or more simpler substances

AX A + X

Ex’s:

Electrolysis: Ex:

Unit 5 Packet - of 183. Single Displacement (Replacement):

1 element replaces a similar element in a cmpd

A + BX AX + B

Hint: In reactions write water as HOH.

Ex’s:

4. Double Displacement (Replacement): The ions of 2 cmpds switch places to form 2 new cmpds.

AX + BY AY + BX

*often one of the new cmpds will be a ppt.

Ex’s:

Unit 5 Packet - of 185. Combustion: When a substance combines with oxygen releasing a large amount of energy in the form of light and heat.

Often combustions involve a hydrocarbon : cmpd containing C and H

CxHy + O2 CO2 + H2O

Ex.

Group Practice: ID, Write & Balance the following equations:

1. C2H4 + O2

2. Barium + Copper (II) chloride

3. O2 + Ca

4. PbCl4 + Al(NO3)3

5. CaCl2

Unit 5 Packet - of 18Activity SeriesPg 265-267

1. What is the activity series2. Where are the most active elements found in the series?3. Look at the sample Questions 8-6 on pg 266 then do the practice

questions4. Do the section review 1-2 on page 267.

Activity Series Practice (Use the series for single displacement reactions or synthesis reactions with oxygen):

I. Based on the activity series of metals and halogens, circle the element within each pair that is more likely to replace the other in a compound?

K and Na Al and Ni Bi and Cr Cl and F

Cl and I Fe and Sr I and F Au and Ag

II. Using the activity series of metals and halogens, predict whether each of the possible reactions listed below will occur. For the reactions that will occur, write the products and balance the equation:

Ni(s) + CuCl2(aq)

Zn(s) + Pb(NO3)2(aq)

Cl2(g) + KI(aq)

Cu(s) + FeSO4(aq)

Ba(s) + H2O(l)

III. Use the activity series to predict whether each of the following synthesis reactions will occur, and write the chemical equations for those predicted to occur:

Ca(s) + O2(g)

Ni(s) + O2(g)

Au(s) + O2(g)

Unit 5 Packet - of 18Unit 5 Problem Set Name: Pd:___

First and last name please!

You must show work for credit – put final answer on the blank provided include units!

Review Questions:1. Name the following:

A. FeSO4

B. BaCl2

C. CO

D. NH4NO2

2. Write the formula for the following:

A. diphosphorus trisulfide

B. cobalt (III) carbonate

C. silver sulfide

D. sulfuric acid 3. Nicotine, a component of tobacco, is 74.1 percent C, 8.6 percent H and 17.3

percent N by mass; the molar mass is about 162.5 g. What is nicotine’s empirical formula? Its molecular formula?

empirical formula

molecular formula

4. A. How many formula units are in 78.3 g of lead (II) phosphate?

B. Calculate the molarity of a 1.5 liter solution of 498.6 g of lead (II) phosphate.

Unit 5 Packet - of 185. Calculate the percent composition of aluminum dichromate.

Al

Cr

O Current Unit Material:6. Write balanced equations for the following reactions (use your notes and

reference packet to help you with these reactions!):A. Calcium metal is added to water.

B. A solution of tin (II) chloride is added to a solution of iron (III) sulfate

C. Chlorine gas is bubbled into a solution of lithium iodide.

D. C3H8 is burned in oxygen

7. How is 2Cl different from Cl2 ?

8. The poisonous gas, hydrogen sulfide, can be neutralized with a base such as NaOH producing water and sodium sulfide. A student asked to write a balanced equation for the reaction wrote the following:

Na2OH(aq) + H2S (g) Na2S (aq) + H2O (l) A. Is this equation correct?

B. Explain why or why not, and supply the correctly balanced equation if necessary.

honors chemistry - unit 2 web viewbe able to identify and write the five basic types of equations:...

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