crowsnest consolidated high school science 10 unit a …bchs.grasslands.ab.ca/documents/general/work...

Name: __________________________________

Science 10 – Unit A 1 Mr. R. Peebles

Crowsnest Consolidated High School

Science 10

Unit A Work booklet

Mr. R. Peebles

Name: __________________________________


Unit A—Energy and Matter in Chemical Change

WORKSHEET

1

Science Laboratory Safety Rules

1. Read all written instructions carefully before doing an activity.

2. Listen to all instructions and follow them carefully.

3. Wash your hands thoroughly after each activity and after handling chemicals.

4. Wear safety goggles, gloves, or an apron as required.

5. Think before you touch. Equipment may be hot and substances may be dangerous.

6. Smell a substance by fanning the smell toward you with your hand. Do not put your nose close to the

substance.

7. Do not taste anything in the lab.

8. Tie back loose hair and roll up loose sleeves.

9. Never pour liquids into containers held in your hand. Place a test tube in a rack before pouring

substances into it.

10. Clean up any spilled substances immediately as instructed by your teacher.

11. Never look into test tubes or containers from the top. Always look through the sides.

12. Never use cracked or broken glassware. Make sure you follow your teacher’s instructions when

getting rid of broken glass.

13. Label any container you put chemicals in.

14. Report all accidents and spills immediately to your teacher.

15. Read the WHMIS (Workplace Hazardous Materials Information System) safety symbols on any

chemical you will be using and make sure you understand all of them. See Student Reference 1 at the

back of Science 10 for more information.

Name: __________________________________



MSDS

WORKSHEET

2

MATERIAL SAFETY DATA SHEET

12% SODIUM HYPOCHLORITE

Section I: IDENTIFICATION

PRODUCT: sodium hypochlorite (12% solution)

SYNONYMS: sodium hypochlorite (12% available chlorine), Javel water, liquid bleach

CHEMICAL FORMULA: NaOClO

PRODUCT CODE NO.: 17547

Section II: HAZARDOUS INGREDIENTS

COMPOSITION: sodium hypochlorite solution 10–15 %

HAZARDS: oxidizer, corrosive

Section III: EMERGENCY OVERVIEW

Warning! Harmful if swallowed or inhaled. Causes irritation to eyes and respiratory tract. Causes

substantial but temporary eye injury.

Section IV: POTENTIAL HEALTH EFFECTS & FIRST AID MEASURES

INHALATION: Poisonous vapour. Increasing doses may cause irritation of nose and throat, coughing,

headaches, breathing difficulty, pulmonary edema, and lung injury. Remove patient to fresh air. Have

patient rest and keep warm. Seek medical attention if symptoms are severe.

INGESTION: Poisonous. Causes burns, abdominal cramps, nausea, vomiting, lowered blood pressure,

diarrhea, and shock. If patient is conscious, give 1–2 glasses of milk. Do not induce vomiting. Seek

medical attention.

EYE CONTACT: Burns, irritation. Rinse with water for at least 15 minutes. Seek medical attention.

SKIN CONTACT: Burns, irritation. Rinse with plenty of water. Wash contaminated clothing before re-

use.

Section V: PHYSICAL DATA

BOILING POINT: 101

o

C, starts decomposing to NaCl and NaClO

3

at 40

o

C

FREEZING/MELTING POINT: −25°C

VAPOUR DENSITY (AIR=1): 1.3

VAPOUR PRESSURE: 17.5 mm Hg at 20°C

SOLUBILITY IN WATER: fully miscible

SPECIAL FIRE FIGHTING PROCEDURES & PRECAUTIONS: Wear self-contained breathing

apparatus.

UNUSUAL FIRE & EXPLOSION HAZARDS: May release chlorine gas

Section VI: REACTIVITY

STABILITY: Inherently unstable; slowly decomposes liberating Cl

2

; unstable above 40°C

CONDITIONS & MATERIALS TO AVOID: Temperatures above 40

o

C, direct sunlight, acids, metals,

ammonia, oxidizable materials, urea

HAZARDOUS DECOMPOSITION PRODUCTS: Cl

2

Name: __________________________________


continued...

Section VII: EMPLOYEE PROTECTION

CONTROL MEASURES: Use with adequate ventilation.

RESPIRATORY PROTECTION: Use chlorine gas respirator.

PROTECTIVE CLOTHING: Neoprene, rubber or plastic gloves, use plastic sleeves, apron and boots if

handling large quantity.

EYE PROTECTION: Safety goggles

Section VIII: ENVIRONMENTAL PROTECTION

ENVIRONMENTAL PRECAUTIONS: Local exhaust acceptable

SPILL OR LEAK PRECAUTIONS: Wear gloves, boots, apron and goggles during clean-up.

WASTE DISPOSAL: Small spills: mop up with water and run to waste. Large spills: transfer to salvage

container and consult with professional disposal company. Inform local authorities if liquid has entered

surface drains or sewers.

Section IX: REGULATORY CONTROLS

DEPT. OF TRANSPORTATION: Regulated under Transport of Dangerous Goods

DOT CLASSIFICATION: Class 8 (9.2) UN: 1791 PG: III

DOT PROPER SHIPPING NAME: Hypochlorite solutions

OTHER DOT INFORMATION: N/A

WHMIS CLASSIFICATION: C, E, F

OTHER REGULATORY REQUIREMENT: none

Section X: PRECAUTIONS: HANDLING, STORAGE, AND USAGE

Store in cool, dry place away from acids. Do not store in metal containers. Use in well-ventilated area.

Name: __________________________________



SAFETY

WHMIS and Hazardous Household Product Symbols

WORKSHEET

3

Goal Review the meanings of warning labels in the science classroom and at home.

Think About It

Throughout Canada, standard symbols are used to identify

dangerous materials

The Workplace Hazardous Materials Information

System (WHMIS) has produced symbols for such

work places as science laboratories. These are

known as WHMIS symbols.

The Hazardous Household Product Symbols

(HHPS) were developed for people buying and

using materials around the home.

Both sets of symbols provide warnings about the possible

hazards of using certain products, as well as the necessary

precautions to

take.

What to Do

Reinforce your understanding of WHMIS symbols and

HHPS symbols by

reading “Safety Symbols” on page 455 in your

SCIENCE 10 textbook

reviewing all the WHMIS symbols and HHPS

symbols

answering the questions that begin on the next

page

WHMIS HHPS

continued...

Name: __________________________________

Science 10 - Unit A 6 Mr. R. Peebles

1. Briefly explain what kind of hazard each word describes.

(a) toxic

(b) flammable

(c) explosive

(d) reactive

(e) corrosive

2. In the space provided, draw the standard WHMIS symbol for each material.

Corrosive Material

Flammable and

Combustible Material Compressed Gas

3. Choose two WHMIS symbols you did not use to answer question 2. Describe some precautions you

would take when handling a product labelled with each symbol.

WHMIS symbol Meaning Precautions

(a)

(b)

continued...

Name: __________________________________


4. Study the display your teacher has provided, showing products that many people use in their homes.

Look for symbols that are HHPS.

Read the label on each product to find out how the product is used and decide why it has an HHPS.

Complete the table below.

HHPS How product used Suggested precautions

(a)

(b)

(c)

Name: __________________________________



PRACTICE QUESTIONS

Nuclear Notation

WORKSHEET

4

Atomic Number and Mass Number

Name Mass Number

Atomic

Number

Number of

Protons

Number of

Neutrons

carbon-14 14 6 6 8

hydrogen-1 1 1

hydrogen-2 2 1

carbon-12

oxygen-18

4 2

20 10

64 29

35 45

7 7

16 16

20 21

9 10

26 30

53 74

calcium-40

119 50

26 33

208 82

silver-108

mercury-201

Name: __________________________________



PRACTICE QUESTIONS

Nuclear Notation

WORKSHEET

5

1. State the number of neutrons in each of the following isotopes.

a)

Ne

b) He

c) Ca

d) Al

2. State the number of each of the following subatomic particles in

oxygen-17.

a) protons

b) electrons

c) neutrons

3. A certain isotope has a mass number of 35. The isotope has 18

neutrons.

a) What is the atomic number of the isotope?

b) What is the atomic symbol of the isotope?

c) Use nuclear notation to represent the isotope.

22

10

4

2

40

20

27

13

Name: __________________________________



PRACTICE QUESTIONS

Bohr Models & EELR (Electron Energy Level Representations)

WORKSHEET

6

Bohr Models are diagrams used to represent the placement of electrons around the nucleus of an

atom. Electrons are arranged around the nucleus in varying ENERGY LEVELS. We will use rings

around the nucleus to represent where we may find the electrons.

To draw Bohr Models:

1. Draw a nucleus (circle) and write in the number of protons and neutrons for the specific

element. Ex. Carbon - 12

2. Count which period the element is located. The number of periods represents the number of

energy levels that element contains.

(a) ex. Carbon is in period 2 = 2 energy levels.

(b) draw dashed rings to represent the levels

3. To add in the electrons (e

-

) use the atomic number, this is equal to the number of electrons in

the element, to determine how many electrons to add.

(a) Use a dot,

● = e

-

. Carbon: atomic number = 6 = 6 electrons.

(b) One pair of electrons on each side of the level, 1

st

level 2 e

-

, 2

nd

level 8 e

-

, 3

rd

level 8 e

-

, etc.

Energy levels can only hold a max. of 8 electrons (except for the 1

st

), this referred to the

Octet Rule.

ASSIGNMENT: On loose-leaf paper, divide the sheet into 3 columns (see example table)

Complete the table for elements 1-20 from the periodic table (leave EELR column blank)

Element Bohr Model EELR

Hydrogen

# protons =

# electrons=

# neutrons=

Will be completed at a later

time

helium# protons =

# electrons=

# neutrons

6 p

+

6 n

0

6 p

+

6 n

0

6 p

+

6 n

0

Name: __________________________________



PRACTICE QUESTIONS

Electron Dot Diagrams

WORKSHEET

7

Goal Demonstrate your understanding of energy levels, and practice drawing electron dot diagrams.

What to Do

Answer each question in the space provided.

1. Complete the following table.

Name of element Period number Group number Number of

energy levels

Number of valence

electrons

hydrogen 1

3 3

2 6

strontium

14 3

6 2

2. Complete the following table by drawing both the energy level diagram and electron dot diagram for

each element. The first row is completed as an example.

Name of element

Energy level diagram Electron dot diagram

carbon

oxygen

lithium

Name: __________________________________


Name of element

Energy level diagram Electron dot diagram

chlorine

magnesium

phosphorus

3. Draw the missing electron dot diagrams in the following table. Refer to the periodic table as necessary.

4. What feature of helium’s energy levels justifies placing its two valence electrons in a pair? (See the table

above.)

5. Draw an electron dot diagram for an atom of each of the following elements.

selenium (Se) bromine (Br) strontium (Sr) radon (Rn) francium (Fr)

6. Explain how you decided on the number and placement of the dots.

Name: __________________________________



PRACTICE QUESTIONS

Ions and Isotopes

WORKSHEET

8

What to Do

Answer each question in the space provided.

1. Complete the following table by filling in the missing information about ions.

Name of ion

Symbol Number of protons Number of electrons Ion charge

lithium ion

Li

+

3 2 1+

19 18 1+

Mg

2+

chloride ion

9 1–

O

2–

I

–

scandium ion

18 2–

Se

2–

7 10

Al

3+

10 4–

calcium ion

phosphide ion

continue…

Name: __________________________________


2. Complete the following table by drawing the EELR. The first row is completed as an example.

3. What is a common feature in all of the EELR diagrams in question 2? (Hint: think “levels”)

_______________________________________________________________________________________________

_______________________________________________________________________________________________

Ion Symbol EELR Diagram Ion Symbol EELR Diagram

Lithium

ion

Li

+

Aluminum

ion

Oxide ion

Calcium ion

Iodide ion

Chloride ion

Sodium

ion

Beryllium ion

Name: __________________________________



PRACTICE QUESTIONS

Ionic Compounds

WORKSHEET

9

Part 1: Modelling Ionic Bonds

Model the formation of of the following ionic compounds using electron dot diagrams. Write the electron dot diagram

for each element in the name. Show the transfer of electrons and the formation of the ionic compound.

1. lithium hydride

4. sodium fluoride

continue…

Name: __________________________________


5. calcium oxide

6. magnesium chloride

7. aluminium oxide

Name: __________________________________



PRACTICE QUESTIONS

Ionic Compounds

WORKSHEET

10


Element Anion

Name Symbol Name Symbol

fluorine F fluoride F

–

chloride

bromide

oxide

sulfide

nitride


Formula Total charge on

cation(s)

Total charge on

anion(s)

Correct () or

incorrect (X)

formula?

Correct formula and

name of compound

(a) LiO

(b) MgO

(c) K

2

S

(d) AlBr

3

(e) NaN

3

continue…

Name: __________________________________


3. Complete the following table to write the formula of each compound.

Name of compound Cation Anion Formula

(a) beryllium fluoride

(b) sodium nitride

(c) calcium sulfide

(d) aluminum chloride

(e) lithium oxide

(f) magnesium nitride

(g) gallium sulfide

(h) barium bromide

4. Write the chemical formula of the following. Include the state.

a) lithium hydride f) magnesium chloride

b) silver chloride g) aluminum hydride

c) sodium oxide h) barium sulfide

d) calcium phosphide i) strontium phosphide

e) sodium iodide j) potassium phosphide

continue…

Name: __________________________________


5. Write the proper chemical name of the following:

a) NaCl

(s)

f) ScCl

3(s)

b) Al

2

S

3(s)

g) AlF

3(s)

c) MgI

2(s)

h) LiBr

(s)

d) Zn

3

As

2(s)

i) Na

2

S

(s)

e) CsF

(s)

j) BaI

2(s)

6. Complete the following table to find the charge on the cation in these compounds. Decide if your answers

are reasonable before you move on to question 7.

Compound Charge on cation

(a) Cu

2

S

(b) Cr

2

O

3

(c) PbO

2

(d) NiCl

2

(e) CrN

(f) HgO

7. Complete the following table by adding the missing Stock system names.

Formula Ion Name

FeCl

3

Fe

3+

iron(III) chloride

FeO Fe

2+

Cu

2

S Cu

+

PbO

2

Pb

4+

continue…

Name: __________________________________


8. Complete the following table to write the chemical formula for each compound.

Name of compound Cation Anion Chemical formula

(a) copper(I) oxide

(b) lead(IV) bromide

(c) iron(III) sulfide

(d) nickel(III) fluoride

(e) manganese(IV) sulfide

9. Write the chemical formula of the following (Remember: Stock System). Include the state.

a) chromium(II) oxide f) vanadium(V) oxide

b) tin(II) iodide g) copper(I) bromide

c) copper(II) selenide h) lead(IV) oxide

d) iron(III) chloride i) chromium (III) phosphide

e) mercury(I) sulfide j) bismuth(III)selenide

10. Write the proper chemical name of the following: (Remember: Stock System).

a) MnCl

4(s)

h) SnCl

4(s)

b) CuBr

2(s)

i) Hg

2

S

(s)

c) FeO

(s)

j) Ni

2

S

3(s)

continue…

Name: __________________________________


d) CoCl

2(s)

k) FeBr

3(s)

e) Hg

3

P

2(s)

l) CuCl

2(s)

f) Fe

2

O

3(s)

m) BiF

5(s)

g) TiO

2(s)

n) SnS

2(s)

Analyze

1. Explain why you must use the Stock system to name ionic compounds containing transition metals. In

which cases do you not need to use the Stock system to name an ionic compound? Explain your answer.

2. There is something wrong with the name written beside each of the following compounds. In each case,

explain why the name is wrong, and then write the correct name.

Formula Incorrect name Explanation Correct name

(a) Ti

2

O

3

dititanium trioxide

(b) NaCl sodium(I) chloride

(c) CuCl

2

copper chloride

(d) NO

2

nitrogen(IV) oxide

Name: __________________________________



PRACTICE QUESTIONS

Polyatomic Ionic Compounds

WORKSHEET

11

1. Write the chemical formula of the following. Include the state.

a) mercury(II) borate m) calcium hydrogen carbonate

b) zinc dihydrogen phosphate n) barium chromate

c) calcium sulfite o) silver dichromate

d) iron(III) nitrate p) lead(IV) carbonate

e) chromium(III) iodate q) tin(II) oxalate

f) sodium borate r) sodium silicate

g) zinc sulfate s) barium cyanide

h) strontium acetate t) sodium silicate

i) antimony (V) iodate u) cobalt(II) nitrate

j) zinc phosphate v) hydrogen hypochlorite

k) cesium borate w) silver acetate

continue…

Name: __________________________________



a) K

3

PO

4(s)

k) Al

2

(SO

4

)

3(s)

b) PbCr

2

O

7(s)

l) CuMnO

4(s)

c) Co

3

(PO

4

)

2(s)

m) Hg(NO

3

)

2(s)

d) Fe

2

(CO

3

)

3(s)

n) Pb(CrO

4

)

2(s)

e) Sn(HSO

4

)

2(s)

o) NiCO

3(s)

f) Cu

3

PO

4(s)

p) Ag

2

SO

4(s)

g) Fe(HCO

3

)

3(s)

q) PbSO

4(s)

h) Cr

2

(CO

3

)

3(s)

r) Ni

3

(PO

4

)

2(s)

i) Sr(IO

3

)

2(s)

s) CuSO

4(s)

j) Hg(ClO

3

)

2(s)

t) Sb

2

(HPO

4

)

3

Name: __________________________________



PRACTICE QUESTIONS

Molecular Compounds

WORKSHEET

12

Part 2: Modelling Covalent Bonds

Model the formation of of the following molecular compounds using electron dot diagrams. Write the electron dot

diagram for each element in the name. Show the sharing of electrons and the formation of the molecular compound.

1. molecular hydrogen

2. water, H

2

O

3. methane, CH

4

Name: __________________________________


4. molecular oxygen

5. molecular nitrogen

6. carbon disulfide

Name: __________________________________



PRACTICE QUESTIONS

Naming Molecular Compounds

WORKSHEET

13

1. Write the chemical formula of the following:

a) sulfur hexafluoride g) dinitrogen hexabromide

b) carbon dioxide h) sulfur dioxide

c) dinitrogen monoxide i) carbon monoxide

d) arsenic tribromide j) tetraphosphorous decaoxide

e) tetranitrogen hexahydride k) dinitrogen pentachloride

f) disulfur hexafluoride l) carbon tetrachloride


a) P

2

Cl

5

g) SiS

2

b) NCl

3

h) OCl

2

c) CS

2

i) NO

2(g)

d) ClBr

2

j) P

2

O

5

e) NO

(g)

k) SF

6

f) N

2

O

4

l) PBr

5

Name: __________________________________



PRACTICE QUESTIONS

Review: Naming Ionic and Molecular Compounds

WORKSHEET

14

Complete the following table.

Chemical formula Ionic or molecular?

Name of compound

NH

4

Cl

potassium sulfide

CI

4

calcium oxide

ammonium chloride

Li

3

N

Mg(OH)

2

zinc oxide

CuNO

3

silicon dioxide

oxygen dichloride

CuCl

FeCl

2

calcium sulfide

calcium hydrogencarbonate

P

2

O

5

silicon tetrabromide

aluminium bromate

Ca(HS)

2

ammonium nitrite

AgCH

3

COO

calcium chromate

N

2

O

5

iron(III) carbonate

HgS

silver hydrogensulfate

continue…

Name: __________________________________


Chemical formula Ionic or molecular?

Name of compound

KMnO

4

Mg(OH)

2

AlPO

4

carbon disulfide

potassium sulfate

SnF

2

K

2

Cr

2

O

7

HgS

sodium tetraborate

vanadium(V) oxide

(NH

4

)

2

Cr

2

O

7

bismuth(V) phosphate

Na

2

SiO

3

Co

3

(PO

4

)

2

Name: __________________________________



PRACTICE QUESTIONS

Solubility Table

WORKSHEET

15

Goal Predict solubility using a solubility table.

What to Do

Use the following solubility table to complete the tables below.

Ions

NH

4

+

NO

3

–

ClO

3

–

ClO

4

–

CH

3

COO

–

Cl

–

Br

–

I

–

SO

4

2–

S

2–

OH

–

CO

3

2–

PO

4

3–

SO

3

2–

High

solubility

all all most most most group 1

group 2

NH

4

+

group 1

NH

4

+

Sr

2+

Ba

2+

Tl

+

group 1

NH

4

+

Low

solubility

none none

Ag

+

Hg

+

Ag

+

Pb

2+

Cu

+

Hg

+

Tl

+

Ag

+

Pb

2+

Ca

2+

Ba

2+

Sr

2+

Ra

2+

most most most


Name

Formula

Cation Anion

High or low

solubility?

sodium chloride NaCl

Na

+

Cl

–

lithium iodide

Mg(ClO

3

)

2

strontium hydroxide

BaCO

3

continue…

Name: __________________________________



Name Formula High or low

solubility?

Al(OH)

3

ammonium chloride

K

2

S

molybdenum(V) chlorate

Pb(CH

3

COO)

2

copper(II) iodide

FeCO

3

calcium sulfite

Ba

3

(PO

4

)

2 (s)

palladium(II) bromide

HgI

strontium sulfate

Name: __________________________________



Activity

Water’s Purpose in a Reaction

WORKSHEET

16

1) Purpose: To examine some of the basic principles of chemical reactions and to make

qualitative observations of chemical reactions

2) Design: Two solid substances will be mixed in order to produce a chemical reaction.

3) Materials:

a) lead (II) nitrate

b) potassium iodide

c) Cream of tartar (potassium

bitartrate)

d) Baking soda (sodium bicarbonate)

e) 10 weighing dishes

f) 4 x 30mL beakers

g) Glass stirring rod

h) Scopula

4) CAUTION: LEAD (II) NITRATE AND SODIUM IODIDE ARE STRONG OXIDIZING AGENTS

AND MAY IRRITATE OR BURN YOUR SKIN. GLOVES AND GOGGLES ARE MADITORY!

FOLLOW ALL PROCEDURES AND DISPOSAL PROCEDURES!

5) Part 1: Lead (II) nitrate and sodium iodide

a) A balanced chemical reaction for the mixing of lead (II) nitrate and sodium iodide is

provided as followed. Label each compound correctly.

(reactants) (products)

Pb(NO

3

)

2 (s)

+2 KI

(s)

PbI

2

+ 2 KNO

3

_____________ +______________ _______________ +________________

b) Are the reactants molecular or ionic substances? How do you know?

_______________________________________________________________________________________________

______________________________________________________________________________________________

c) Gather approximately 2 x 0.5 g of each reactant in labelled weighing dishes and return to

your work table. CAUTION! Record your observations of the reactants:

_______________________________________________________________________________________________

______________________________________________________________________________________________

d) Combine 0.5 g of each reactant into a separate weighing dish and mix together using a

glass stirring rod. Record your observations.

_______________________________________________________________________________________________

______________________________________________________________________________________________

e) In separate 30 mL beakers, dissolve the remaining 0.5 g of each solid in approximately 5

mL of water. Record your observations.

_______________________________________________________________________________________________

______________________________________________________________________________________________

continue…

Name: __________________________________


f) Pour the potassium iodide solution into the lead (II) nitrate solution and record your

observations.

_______________________________________________________________________________________________

______________________________________________________________________________________________

g) Dispose of all liquids and solid waste into the appropriate containers.

DO NOT POUR WASTE DOWN THE DRAIN OR PLACE IN THE GARBAGE.

6) Part 2: Baking soda and cream of tartar

a) The following balanced reaction is provided for you: name the missing reactants and

products.

NaHCO

3(s)

+ KHC

4

H

4

O

6(s)

NaKC

4

H

4

O

6 (aq)

+ CO

2(g)

+ H

2

O

(l)

_______________+potassium bitartrate

sodium potassium tartrate + ________________+ ____________

b) Are the reactants molecular or ionic substances? How do you know?

_______________________________________________________________________________________________

______________________________________________________________________________________________

c) Based on the chemical equation, what do you expect to see when you mix the reactants

provided?

___________________________________________________________________

d) Gather approximately 2 x 0.5 g of each reactant in labelled weighing dishes and return to

your work table. Record your observations of the reactants:

_______________________________________________________________________________________________

______________________________________________________________________________________________

e) Combine 0.5 g of each reactant into a separate weighing dish and mix together using a

glass stirring rod. Record your observations.

_______________________________________________________________________________________________

______________________________________________________________________________________________

f) In separate 30 mL beakers, dissolve the remaining 0.5 g of each solid in approximately 5

mL of distilled water. Record your observations.

_______________________________________________________________________________________________

______________________________________________________________________________________________

g) Pour the sodium bicarbonate solution into the potassium bitartrate solution and record your

observations.

_______________________________________________________________________________________________

______________________________________________________________________________________________

h) For Part 2 ONLY, all waste may be thrown in the garbage and/or down the drain.

continue…

Name: __________________________________


7) Between your partner and you, devise a scientific theory for why the solid mixtures not react

until you dissolved them in water as you observed in Parts 1 and 2.

____________________________________________________________________________________________

____________________________________________________________________________________________

____________________________________________________________________________________________

____________________________________________________________________________________________

____________________________________________________________________________________________

____________________________________________________________________________________________

____________________________________________________________________________________________

8) Based on how the reaction actually occurred, copy and rewrite the chemical equations with the

appropriate states for each reactant and product as they where in the reaction.

a) Part 1: (you will need to use your solubility table to determine which product formed the

solid)

b) Part 2:

Name: __________________________________



Activity

Physical or Chemical Reactions?

WORKSHEET

17

What to Do

Classify each change in the following table as either chemical or physical. Explain your classification.

Change

Chemical or physical? Explanation

A sheet of paper is crumpled into a ball.

A sheet of paper is set on fire and burns

to ashes.

Steel wool is placed in a glass of salty

water. The steel wool rusts.

A sheet of flexible, colourless plastic is

left outside, in bright sunlight, and

becomes yellow and brittle over time.

A teaspoon of white sugar (sucrose)

dissolves in a glass of warm water.

Vinegar is poured over a teaspoon of

baking soda. The white powdered

baking soda fizzes, and bubbles form.

A red-hot nail is inserted into a large

block of ice. Steam is formed as the nail

contacts the block, and water flows

away from the nail.

Name: __________________________________



Activity

Chemical Reactions

WORKSHEET

18

1. Complete the following tables writing the complete skeleton equation for each question.

- Ensure to include:

o Proper chemical formulas (remember: Ionic vs. Molecular)

o States for each compound or element (refer to periodic table and solubility table)

Word

equation

iron + sulfur → iron(II) sulfide

Skeleton

equation

2.

Word

equation

calcium + oxygen gas → calcium oxide

Skeleton

equation

3.

Word

equation

calcium oxide + carbon dioxide

→ calcium carbonate

Skeleton

equation

4.

Word

equation

copper(II) oxide

→ copper + ox

ygen gas

Skeleton

equation

5.

Word

equation

water → hydrogen gas + oxygen gas

Skeleton

equation

continue…

Name: __________________________________


6.

Word

equation

potassium + water → potassium hydroxide + hydrogen gas

Skeleton

equation

7.

Word

equation

zinc + tin(II) chloride

→ zinc

chloride + tin

Skeleton

equation

8.

Word

equation

copper + silver nitrate → copper(II) nitrate + silver

Skeleton

equation

9.

Word

equation

potassium iodide + lead(II) nitrate → potassium nitrate + lead(II) iodide

Skeleton

equation

10.

Word

equation

sodium chloride + silver nitrate → sodium nitrate + silver chloride

Skeleton

equation

11.

Word

equation

barium chloride + potassium sulfate

→ barium sulfate + potassium chloride

Skeleton

equation

continue…

Name: __________________________________


12. Refer back to your chemical reactions, 1-11. What do the reactions in each group have in

common?

Reactions Similarities among reactions

1, 2, and 3

4 and 5

6, 7, and 8

9, 10, and 11

13. Develop a classification system for the chemical reactions you observed in this activity.

continue…

Name: __________________________________


14. Write the skeleton equations 1-11 on the following page. Using the pipe cleaners to assist

you, devise a method to ensure that the Law of Conservation of Matter (the number of

atoms in the reactants must equal the number of atoms in the products) remains true for

each equation.

Equation # Skeleton Equation

1

Fe

(s)

+ S

8 (s)

FeS

(s)

2

3

4

5

6

7

8

9

10

11

Name: __________________________________



Activity

Balancing Chemical Reactions

WORKSHEET

19

What to Do

Answer the questions in each section in the space provided.

Balancing Formation Reaction Equations

1. Balance each equation for a formation reaction.

(a) K

(s)

+ O

2(g)

K

2

O

(s)

(b) P

4(s)

+ Cl

2(g)

PCl

5(s)

(c) Cu

(s)

+ S

8(s)

CuS

(s)

(d) Mg

(s)

+ O

2(g)

MgO

(s)

(e) Fe

(s)

+ O

2(g)

Fe

2

O

3(s)

(f) P

4(s)

+ S

8(g)

P

2

S

5(s)

(g) C

(s)

+ O

2(g)

CO

(g)

(h) N

2(g)

+ O

2(g)

NO

2(g)

(i) Li

(s)

+ N

2(g)

Li

3

N

(s)

(j) S

8(s)

+ O

2(g)

SO

2(g)

2. Write a balanced chemical equation to represent each reaction described below.

(a) Solid aluminum metal reacts with oxygen gas to form solid aluminum oxide.

(b) Metallic zinc combines with elemental sulfur to form zinc sulfide.

Balancing Decomposition Reaction Equations

3. Balance each equation for a decomposition reaction.

(a) NaCl

(s)

Na

(s)

+ Cl

2(g)

(b) CaBr

2(s)

Ca

(s)

+ Br

2(l)

(c) CCl

4(l)

C

(s)

+ Cl

2(g)

(d) NCl

3

(g)

N

2(g)

+ Cl

2(g)

continue…

Name: __________________________________


(e) P

4

O

10(s)

P

4(s)

+ O

2(g)

(f) Ag

2

O

(s)

Ag

(s)

+ O

2(g)

(g) HCl

(aq)

H

2(g)

+ Cl

2(g)

(h) KI

(s)

K

(s)

+ I

2(s)

(i) AlCl

3(s)

Al

(s)

+ Cl

2(g)

(j) CuO

(s)

Cu

(s)

+ O

2(g)


(a) Rubidium oxide decomposes into its elements.

(b) Calcium chloride decomposes into its elements.

Balancing Single Replacement Reaction Equations

5. Balance each equation for a single replacement reaction.

(a) K

(s)

+ H

3

PO

4(aq)

K

3

PO

4(aq)

+ H

2(g)

(b) Fe

(s)

+ H

2

S

(aq)

Fe

2

S

3(s)

+ H

2(g)

(c) Cl

2(g)

+ MgBr

2(aq)

MgCl

2(aq)

+ Br

2(aq)

(d) Cu

(s)

+ Ag

2

CO

3(s)

CuCO

3(s)

+ Ag

(s)

(e) Br

2(g)

+ KI

(aq)

I

2(aq)

+ KBr

(aq)

(f) Mg

(s)

+ Zn

3

(PO

4

)

2(s)

Mg

3

(PO

4

)

2(s)

+ Zn

(s)

(g) K

(s)

+ Al(NO

3

)

3(aq)

Al

(s)

+ KNO

3(aq)

(h) Ca

(s)

+ H

2

O

(l)

Ca(OH)

2(s)

+ H

2(g)

(i) Na

(s)

+ H

2

SO

4(s)

Na

2

SO

4(aq)

+ H

2(g)

(j) K

(s)

+ H

2

O

(l)

KOH

(aq)

+ H

2(g)

6. Write a balanced chemical equation to represent each reaction (a & b) described below.

(a) Silver reacts with gold(III) nitrate.

continue…

Name: __________________________________


(b) Copper reacts with lead(II) sulfate.

Balancing Double Replacement Reaction Equations

7. Balance each equation for a double replacement reaction.

(a) Na

2

SO

4(aq)

+ BaCl

2(aq)

BaSO

4(s)

+ NaCl

(aq)

(b) HNO

3(aq)

+ Ba(OH)

2(aq)

H

2

O

(l)

+ Ba(NO

3

)

2(aq)

(c) Na

2

CO

3(aq)

+ Fe(NO

3

)

3(aq)

Fe

2

(CO

3

)

3(s)

+ NaNO

3(aq)

(d) CaCl

2(aq)

+ K

3

PO

4(aq)

Ca

3

(PO

4

)

2(s)

+ KCl

(aq)

(e) Al

2

(SO

4

)

3(aq)

+ Ba(OH)

2(aq)

Al(OH)

3(s)

+ BaSO

4(s)

(f) NaOH

(aq)

+ H

2

SO

4(aq)

H

2

O

(l)

+ Na

2

SO

4(aq)

(g) Na

3

PO

4(aq)

+ Ag

2

SO

4

(s)

Na

2

SO

4(aq)

+ Ag

3

PO

4(s)

(h) Na

2

CrO

4(aq)

+ Cu(NO

3

)

2(aq)

NaNO

3(aq)

+ CuCrO

4(aq)

(i) H

3

PO

4(aq)

+ KOH

(aq)

H

2

O

(l)

+ K

3

PO

4(aq)

(j) Na

2

CO

3(aq)

+ HNO

3(aq)

H

2

CO

3(aq)

+ NaNO

3(aq)


(a) Solutions of sodium hydroxide and hydrochloric acid react.

(b) A silver nitrate solution reacts with a sodium chloride solution.

Balancing Combustion Reaction Equations

9. Balance each equation for a combustion reaction.

(a) C

2

H

6(g)

+ O

2(g)

CO

2(g)

+ H

2

O

(g)

(b) C

3

H

8(g)

+ O

2(g)

CO

2(g)

+ H

2

O

(g)

(c) C

6

H

14(g)

+ O

2(g)

CO

2(g)

+ H

2

O

(g)

(d) C

8

H

18(g)

+ O

2(g)

CO

2(g)

+ H

2

O

(g)

(e) C

2

H

2(g)

+ O

2(g)

CO

2(g)

+ H

2

O

(g)

(f) C

2

H

4(g)

+ O

2(g)

CO

2(g)

+ H

2

O

(g)

continue…

Name: __________________________________


(g) ZnS

(s)

+ O

2(g)

ZnO

(s)

+ SO

2(g)

(h) CH

3

NO

2(l)

+ O

2(g)

CO

2(g)

+ H

2

O

(g)

+ NO

2(g)

(i) NH

3(g)

+ O

2(g)

NO

2(g)

+ H

2

O

(g)

(j) C

2

H

5

SH

(g)

+ O

2(g)

CO

2(g)

+ H

2

O

(g)

+ SO

2(g)


(a) Candle wax, C

25

H

52

, is burned to produce carbon dioxide and water.

(b) Sucrose, C

12

H

22

O

11

, is burned to produce carbon dioxide and water.

Classifying and Balancing Equations

11. Classify each reaction as a formation (F), decomposition (D), single replacement (SR), double

replacement (DR), or combustion (C) reaction. Then balance each equation.

Reaction Classification

Li

(s)

+ AlCl

3(aq)

Al

(s)

+ LiCl

(aq)

NH

3(g)

N

2(g)

+ H

2(g)

K

(s)

+ Br

2(l)

KBr

(s)

C

10

H

22(l)

+ O

2(g)

CO

2(g)

+ H

2

O

(g)

NH

4

OH

(aq)

+ H

2

CO

3(aq)

H

2

O

(l)

+ (NH

4

)

2

CO

3(aq)

H

2

O

(l)

H

2(g)

+ O

2(g)

Al

(s)

+ Cl

2(g)

AlCl

3(s)

Zn

(s)

+ SnF

4(aq)

Sn

(s)

+ ZnF

2(aq)

Name: __________________________________



Activity

Mole Calculations

WORKSHEET

20

Find the molar mass of each of the following elements.

1. potassium , K

(s)

2. zirconium, Zr

(s)

3. chlorine, Cl

2(g)

4. oxygen, O

2(g)

Determine the molar mass of each of the following compounds.

5. potassium bromide, KBr

(s)

6. methane, CH

4(g)

Name: __________________________________


7. sodium sulfate, Na

2

SO

4(s)

8. aluminum nitrate, Al(NO

3

)

3 (s)

Calculate the number of moles in each of the following:

9. 1000 g of NaCl

10. 32.5 g of NaHCO

3(s)

11. 4.69 g of Na

2

CO

3(s)

12. 0.258 g of MgSO

4

7H

2

O

(s)

Name: __________________________________


13. 550 g of sodium phosphate

14. 6.2 g of carbon dioxide

15. 500 mL of water

Calculate the mass in grams of the following:

16. 0.21 mol of NaCl

(s)

17. 55.56 mol of H

2

O

(l)

Name: __________________________________


18. 0.100 mol of KHC

4

H

4

O

6(s)

19. 1.2 mol of sodium sulphate decahydrate

20. 0.15 mol of phosphorus

21. 0.025 mol of tin (II) fluoride

22. 0.400 mol of calcium sulphate dihydrate

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