Name:

Unit 2 Outline —Chemistry

Chapter 6DAY OUTLINE - KEY TERMS

1 Ch.5 TestAssignment: Read p.256-260

Practice Problems p.259p.260

2 6.1 Notes (slides 1 -8) 1. SynthesisAssignment: Practice Problems p. 261 2. Decomposition

p. 262 3. Single Replacement4. Double Replacement

3 6.1 Notes (slides 9-12) 5. NeutralizationAssignment: Practice Problemsp.263,p.264 6. Combustion

Classifying Chemical Reactions Wksht 7. Precipitate8. Catalyst

4 Chemical Reactions Lab (due in 2 classes)

5 Assignment: Predicting the Products Wksht6 6.1 QUIZ

6.2 NotesAssignment: Different Rates of Reactions Wksht

Complete_Chemical_Reactions_Lab7 Hand in Chemical Reactions Lab

Assignment: Ch.6 Review p.282-2&3#l,2 (odd),3-5,7Assessment 6.1 and 6.2 Wkshts

8 Chemistry Unit Review Game

9 Hand in Ch.6 packageChemistry Unit Test (Chapters 4, 5 and 6)

Chapter 6: Chemical Reactions Key TermsKey Term Definition Exa mp/Graphic

1. Synthesis

2. Decomposition

3. Single RepOacement

4. Double Replacement

5. Neutralization

6. Combustion

7. Precipitate

8. Catalyst

6.1 Types of Chemical Reactions1. Synthesis Reactions

Occur when two or more reactants (usually elements)

___________

to form a compound.General Formula:

___________________________________________

(where A and B represent elements)

.can produce ionic or covalent compounds

Ionic:

_______________________________________________

Covalent:

_________________________________________

2. Decomposition

•are the opposite of synthesis reactions•A compound

_________________________

into two or more products (often elements).General Formula:

Ionic and Covalent Compounds can DecomposeIonic:

_______________________________________________

Covalent:

_______________________________________

3. Single Replacement

When one element from a

_________________

is replaced with a separate

•Two types, based on whether the single element is a metal or a non-metalGeneral Forms:

____________________________________________

where A is a metal, or

___________________________________________

where A is a non-metal

The Two Types:

•When A is a

____________

•WhenAisa

___________

4. Double Replacement

elements

___________________

between two compounds to form two new compounds.

•Two ionic solutions react to form a precipitate (solid) and another ionic solution

•General Form:

Example:+ +

5. Neutralization (aka Acid-Base reactions)

•occur when an and a react to form a and•acids (start with ) and bases (end in

____,

or begin with

_______

General Form:

•HX + MOH —* MX + H20 (where X and M are elements)

Ex.1___________ +

___________

-

____________

+

Ex.2___________ +

___________ ____________

+

6. Combustion

•occurs when a compound or element reacts with

_________________

Always makes and

______________

(in grade 10 examples)

Aka. hydrocarbon combustionGeneral Form:

Ex.1____________ +

____________ _____________

+

Ex.2_____________ +

_____________ ______________

+

Ex.3 + -* +

Name:

Classifying Chemical Reactions

Use the following letters to classify the reactions in the questions below:

S Synthesis D = Decomposition SR = Single Replacement

DR = Double Replacement N = Neutralization

C = Combustion

1. Identify AND balance the following chemical reactions:

REACTION TYPE

a. Hg0- Hg +_02

b. Zn + H2S04- ZnSO4 + H2

c. NaOH + HC1 - NaCl + H20

d. A12(S04)3 + — Ca(OH)2 - A1(OH)3 + CaSO4

e. H2+ O2 H20

f. C3H8 + 02 - CO2 + H20

g. CaCO3 - — CaO + CO2

h. H20 + Fe - Fe203 + H2

i. Zn + CuSO4 - ZnSO4 + Cu

j.Al + 02 ) A1203

k. C4H8 + 02 - H20 + CO2

1. NaOH + H2SO4 - Na2SO4 + H20

m. HF-) H2+ F2

n. — Pb(NO3)2 + KI - Pb12 + KNO3

o. H2S04 + KOH - K2S04 + H2O

p.S8 + 02 SO3

q.C2H6+ O2 - H20 + CO2

2. Classify each reaction and write the formula of each product or products. Balancethe equation.

a. Na+N2-

b. A1F3 -

c. CuSO4 + Al

d. Cal2 + Pb(N03)2 )

e. C4H10 + 02 )

f. AgNO3 + NaBr -

g.CsI + Cl2 -)

3. Classify each of the following reactions and write balanced formula equations forthem.

a. sodium + oxygen - sodium oxide

b. aluminum chloride - aluminum + chlorine

c. cadmium + gold (III) nitrate -) cadmium nitrate + gold

d. glucose (C6H1206)+ oxygen - carbon dioxide + water

e. sulphuric acid + sodium hydroxide - sodium sulphate + water

f. sodium sulphate + calcium chloride - sodium chloride + calcium sulphate

ApplyingName Date Knowledge

______

Use with textbook pages 256-267.

Predicting the products1. For each of the following:

I. predict the products

II. classify the reaction as synthesis (S), decomposition (D), single replacement (SR),double replacement (DR), neutralization (N), or combustion (C)

III. write a balanced equation

(a) H10 -

(b) H,, + Cl2 -÷

(c) NaT + F2

(d) AgNO3 + Na3PO4 -

(e) Ba(OH)2 + H2S04 -

(f) P4 + Cl2-

(g) CH3OH +

(h) Sr(OH)2 + H3P04

(i) Fe12 —

(j) CuC12 + Fe -

(k) Cr2(S04)3 + K2C03

(1) C2H5OH + °2

© 2008 McGraw-Hill Ryerson Limited Section 6.1 Types of Chemica’ Reactions • MHR 109

ApplyingName Date Knowledge

(m)H2+ F2 -

(n)Ag20

(o)C12 + KI

2. For each of the following:

I. complete the word equation by predicting the products

II. classify the reaction as synthesis (S), decomposition (D), single replacement (SR),double replacement (DR), or neutralization (N)

Ill, write a balanced equation for each word equation

(a) sodium + chlorine —

(b) gallium fluoride + cesium

(c) calcium hydroxide + nitric acid —

(d) barium chloride + silver nitrate —

(e) cobalt(II) bromide —

(f) copper(II) iodide + bromine —

(g) phosphoric acid + magnesium hydroxide —

(h) zinc + iodine -

(i) beryllium chloride —

(j) iron(III) sulphate + calcium hydroxide -÷

110 MHR • Section 6.1 Types of Chemic& Reactions © 2008 McGraw-H1N Ryerson Limited

Name Date Comprehension

Use with textbook pages 2 72-277.

Different rates of reactions1. Indicate whether each of the following would increase or decrease the rate of

reaction.

(a) adding heat

______________________________________

(b) removing heat

_____________________________________

(c) adding a catalyst

(d)diluting a solution

_______________________________________

(e) removing an enzyme

(f) lowering the temperature

(g) increasing the temperature

(h) decreasing the surface area

_______________________________________

(i) increasing the concentration of a solution

U) breaking a reactant down into smaller pieces

2. Identify which situation would have a higher reaction rate.affected the rate of reaction in each situation.

Then state the factor that

Situation X Situation Y Situation Factorwith a higher affectingreaction rate the rate of

(X or Y) reaction

(a) 1 g of sugar (cubes) 1 g of sugar (grains)

116 MHR • Section 6.2 Factors Affecting the Rate of Chemical Reactions © 2008 McGraw-HW Ryerson Limited

Name

0 °C

Comprehension

1HI;1

(c) low number of particles = high number of particles = more collisionsfew collisions

.c) •%i

.,

)

(d) enzyme added no enzyme added

(e) twigs logs

(b)

Date

© 2008 McGraw-Hill Ryerson Limited Section 6.2 Factors Affecting the Rate of Chemical Reactions • MHR 117

Name: Block: Date:

Science 10 Types of Chemical Reactions Lab

Abstract:There are many varieties of chemical reactions, some of them difficult to classify. However, the majority of chemicalreactions fit into one of these six categories:

1. Synthesis (Combination): A + B —. AB(Two substances combine to form a new substance.)

2. Decomposition: AB —* A + B(The opposite of synthesis; one substance decomposes to form two new substances.)

3. Single Replacement: AB + X —* A + XB(A single change of partners results.)

4. Double Replacement: AB + XV —+ AY + XB(Similar to single replacement, but a double exchange of partners occurs.)

5. Combustion: CH +02 —÷ C02 + 1120(Organic compound plus Oxygen (burning) produces Carbon Dioxide and water)

6. Neutralization: HX + XOH —* MN + H20

(Acid + Base produces an ionic compound (salt) and water)

Purpose:1. To observe a variety of chemical reactions.2. To interpret an explain observations with balanced chemical equations.

3. To classify each reaction as one of the six main types.

Materials: See lab sheets

Procedure:1. Put on safety goggles and an apron.2. Make observations before, during, and after each reaction. Record your observations in your copy of

Table 1 in your notebook.

Rx. 1: Using tongs, hold a 6 cm length of magnesium ribbon in the hottest part of the flame for a fewmm. Let the products fall into a beaker with water and bromothymol blue.

Rx.2: Clean an iron nail with a piece sandpaper or steel wool so the surface of the nail is shiny.Observe the nail in the test tube of 0.50 M Copper(II) sulphate solution. You may need to come backand make more observations later in the class.

Rx.3: Half fill a test tube with Hydrochloric Acid / Bromothymol blue solution (yellow solution). AddCalcium hydroxide drop by drop until the solution turns green. Add more Ca(OH)2drop by drop untilthe solution turns blue.

Rx.4: Put 5 drops of ethanol solution on a watch glass. Light it with a lighter.Rx.5: Fill a test tube one quarter full with Calcium chloride solution. Fill a second test tube one quarter full

with Sodium carbonate solution. Pour the Calcium chloride solution into the test tube containingSodium carbonate solution.

Rx.6: Place a few small pieces of mossy Zinc in a test tube. Add hydrochloric acid solution to the test tubeuntil the mossy Zinc is completely covered.

Rx.7: Half fill a test tube with Hydrogen peroxide solution. (Read over alil steps llirst).

Add a small amount of Manganese (IV) oxide. (Note: Mn02 acts as a catalyst in this reaction.)Test the gas evolved by placing a glowing (not burning) splint into the mouth of the test tube. (If itlights it is oxygen; if it “pops” it is hydrogen.)

Before leaving the laboratory, clean all glassware with the brushes and soap solution provided and washyour hands thoroughly with soap and water. Leave each station clean and tidy.

Observations: Table 1 - Experimental Observations.

1

2

3

4

5

6

7

Analysis: Write the word equation and formula equation for each reaction.

Rx.#1: Word Equation: magnesium + oxygen —>

Formula Equation:

________________________________________________________

Rx.#2 Word Equation: —

Formula Equation:

Rx.#3 Word Equation: —

Formula Equation:

Rx.#4 Word Equation: —

Formula Equation:

Rx.#5 Word Equation: —

Formula Equation:

Rx.#6 Word Equation:

Formula Equation:

Rx.#7 Word Equation: —

Formula Equation:

Questions:

1. A) In Reaction 1, with which element in the air did the magnesium react?

B) Why did the ribbon turn pink in the solution?

_____________________

2. In Reaction 2, changes occurred in both the nail and the solution. What does the colour of thesolution indicate is happening?

____________________________________________________

3. What evidence of chemical change did you see in Reaction 3?

4. In Reaction 5, one of the products is Sodium chloride (table salt), which, as you know, is highlysoluble in water (dissolves easily). Therefore, what would be the element that would accountfor the precipitate (white cloudy part) which formed?

_______________________________

5. How could you test the gas released in Reaction 6 to confirm its identity?

6. a. What does the glowing splint test suggest about the identity of the gas evolved inReaction 7?

b. The formula for Hydrogen peroxide is H202. Two products are formed in Reaction 7,one of them is a common gas that you know from Question 6a and the other is acommon liquid. What is the most likely identity of this common liquid.

7. In some industrial processes, solutions have impurities removed by single replacementreactions. In electrolytic Zinc process, for instance, impurities of Cadmium in the form ofCdSO4are removed from the electrolyte by the addition of Zinc dust. Write a balancedequation for this reaction.

8. A) Write the balanced equation for the electrolysis (breaking apart) of water.

B) What type of reaction is this?

Conclusion For each reaction (#1-7) name the type of reaction that occurred.

Rx. 1: Magnesium ribbon in the flame:

____________________________________________

Rx.2: Iron nail in the test tube of 0.50 M Copper(II) sulphate solution.

Rx.3: Hydrochloric acid and Calcium Hydroxide:

Rx.4: Burning Ethyl Alcohol:

___________________________

Rx.5: Calcium chloride solution and Sodium carbonate solution.

Rx.6: Mossy Zinc and hydrochloric acid.

__________________

Rx.7: Hydrogen peroxide solution with Manganese (IV) oxide.

Use

with

text

book

page

s25

6-26

7.

Typ

esof

chem

ical

reac

tions

7.W

hat

type

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ting

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oduc

eon

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synt

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s

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mbu

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n

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com

posi

tion

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ngle

repl

acem

ent

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oxid

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sca

nbe

brok

endo

wn

into

solid

carb

onan

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ygen

gas.

Wha

tty

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reac

tion

isth

is?

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synt

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neut

rali

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on

Ass

essw

tent

ID

ate

_________

Use

the

foll

owin

gw

ord

equa

tion

toan

swer

ques

tion

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tass

ium

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rate

—ox

ygen

+po

tass

ium

chlo

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hat

type

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acti

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ew

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tion

?

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synt

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ent

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Whi

chof

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pres

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asi

ngle

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reac

tion

?

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+2

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O3

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2+

2Ag

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ld(H)

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ide

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ncgo

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cyan

ide

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agne

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dere

acts

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brom

ine

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ne.

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only

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and

Hi

only

B. I

and

ill

only

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II,

and

III

11.

Whi

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coef

fici

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bala

nces

the

foll

owin

geq

uati

on?

Fe

+02

Fe

203

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,i,l

C.4

,2,3

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0.4

,3,2

12.

Wha

tco

effi

cien

tis

need

edfo

rw

ater

inor

der

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eth

efo

llow

ing

equa

tion

?

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O2

+H

0

A.2

C.4

B.3

D.6

13.

Hyd

roch

lori

cac

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used

tone

utra

lize

bari

umhy

drox

ide.

Wha

tis

the

form

ula

for

the

salt

prod

uced

byth

isne

utra

liza

tion

?

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BaC

I,C.

Ba(C

l02)2

B.B

a(C

lO)

20.

Ba(C

l01),

Ass

esse

aent

61

Use

the

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acti

onto

answ

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.

2H

NO

3+

Be(

OH

)2

-B

e(N

03)2

+

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0

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Whi

chof

the

foll

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ents

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ue?

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NO

2is

anac

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e(N

03)2

isa

base

.

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isis

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reac

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IV.

The

prod

ucts

ofth

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ea

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and

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er.

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I,U

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lon

ly

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and

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18.

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ium

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hide

.W

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com

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rmed

from

this

reac

tion

?

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dS

B.C

dS

O4

C.N

aS,

0.C

dNO

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ame

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e

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chea

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ical

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tion

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KG

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-+2

KGb

+3

022.

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2S33.

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+H

NO

3—

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0+

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.__.2

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+19

02-‘

14H

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+Cu

Cu(

N0

2+

2Ag

6._._

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N0

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rO4

-Pb

CrO

4+

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3

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ctio

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pe

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nthe

sis

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mbu

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lizat

ion

0.de

com

posit

ion

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gle

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ent

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uble

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acem

ent

14.

Whi

chre

acta

nts

form

the

salt

Mg

SO

4in

ane

utra

liza

tion

reac

tion

?

A.S

O2

and

Mg0

2

B.H2S

and

MgO

H

C.H20

and

Mg(

OH

)2

0.H

,S0

4an

dM

g(O

H)

2

15.

Giv

enth

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com

plet

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onof

ach

emic

alre

actio

n:C

,H804

+02

Whi

chof

the

foll

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gar

eth

epr

oduc

tsfo

rmed

from

this

reac

tion

?

H2

II.H20

Ill.C

O2

16.A

.I

and

IIon

ly

B.

Ian

dII

Ion

ly

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and

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only

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ndIl

l

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enth

ein

com

plet

eeq

uati

onof

ach

emic

alre

actio

n:

bar

ium

chlo

rid

e+

amm

oniu

mca

rbonat

e

Whi

chof

the

foll

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gar

eth

epr

oduc

tsfo

rmed

from

this

reac

tion

?

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II.NH

Cl

[LBa

CO3

A.

Ian

dII

only

B.I

and

III

only

C.H

and

Ill

only

0.1,

11.

and

ifi

02

00

8M

cGra

w-H

ill

Rye

rson

Lim

ited

Sec

tion

6.1

Types

ofC

hem

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Rea

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ns•

MH

R11

111

2M

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on6.

11\

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08

McG

raw

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rson

Lim

ited

Ass

ess

sen

t

Use

with

text

book

page

s27

2-27

7.

Fac

tors

affe

ctin

gth

era

teof

chem

kal

rio

ctio

ns

Mat

chth

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the

left

with

the

best

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crip

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Each

Des

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may

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ncen

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nB.

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ved

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aver

age

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ergy

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ple

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fect

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?

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and

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ly

B.I

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and

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only

D.I,

II,

and

ifi

9.In

crea

sing

whi

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tratio

n

A. I

and

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ly

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nd

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only

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and

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only

D.I,

II,

and

III

10.

Whi

chof

the

foll

owin

gw

ill

low

erth

era

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reac

tion

?

A.ad

ding

anen

zym

eto

the

reac

tion

B.de

crea

sing

the

tem

pera

ture

from

40’C

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chun

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calc

ium

upin

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ved

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solu

tion

Nam

eD

ate

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atin

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